{"id":969,"date":"2017-12-14T21:52:57","date_gmt":"2017-12-14T21:52:57","guid":{"rendered":"https:\/\/courses.lumenlearning.com\/suny-mcc-introductorychemistry\/back-matter\/glossary\/"},"modified":"2017-12-14T21:52:57","modified_gmt":"2017-12-14T21:52:57","slug":"glossary","status":"publish","type":"back-matter","link":"https:\/\/courses.lumenlearning.com\/suny-introductory-chemistry\/back-matter\/glossary\/","title":{"raw":"Glossary","rendered":"Glossary"},"content":{"raw":"
Term<\/td>\nDefinition<\/td>\nSection of Book<\/td>\n<\/tr>
abbreviated electron configuration<\/td>\nAn electron configuration that uses one of the noble gases to represent the core of electrons up to that element<\/td>\nOrganization of Electrons in Atoms<\/td>\n<\/tr>
absolute zero<\/td>\nThe minimum possible temperature, labeled 0 K (zero kelvins)<\/td>\nOther Units: Temperature and Density<\/td>\n<\/tr>
acid<\/td>\nAn ionic compound of the\u00a0H+\u00a0cation dissolved in water<\/td>\nAcids<\/td>\n<\/tr>
acid<\/td>\nA compound that increases the amount of\u00a0H+\u00a0ions in an aqueous solution<\/td>\nNeutralization Reactions<\/td>\n<\/tr>
acid dissociation constant (K<\/em>a<\/sub>)<\/td>\nThe equilibrium constant for the dissociation of a weak acid into ions<\/td>\nSome Special Types of Equilibria<\/td>\n<\/tr>
acid salt<\/td>\nAn ionic compound whose aqueous solution is slightly acidic<\/td>\nStrong and Weak Acids and Bases and Their Salts<\/td>\n<\/tr>
activated complex<\/td>\nSee transition state<\/td>\nReaction Mechanisms<\/td>\n<\/tr>
activation energy (Ea)<\/td>\nThe minimum amount of kinetic energy molecules must possess for an effective collision to occur<\/td>\nFactors that Affect the Rate of Reactions<\/td>\n<\/tr>
active site<\/td>\nArea of enzymatic action where substrate molecules react<\/td>\nCatalysis<\/td>\n<\/tr>
activity series<\/td>\nA list of elements that will replace elements below them in single-replacement reactions<\/td>\nTypes of Chemical Reactions: Single- and Double-Displacement Reactions<\/td>\n<\/tr>
actual yield<\/td>\nThe amount that is actually produced in a chemical reaction<\/td>\nYields<\/td>\n<\/tr>
addition reaction<\/td>\nA reaction where atoms are added across a double or triple bond<\/td>\nHydrocarbons<\/td>\n<\/tr>
adhesion<\/td>\nThe tendency of a substance to interact with other substances because of intermolecular forces<\/td>\nProperties of Liquids<\/td>\n<\/tr>
adsorb<\/td>\nBind\u00a0to the surface of another substance<\/td>\nCatalysis<\/td>\n<\/tr>
alcohol<\/td>\nAn organic compound that contains an OH functional group<\/td>\nAlkyl halides and alcohols<\/td>\n<\/tr>
aldehyde<\/td>\nA compound that has a carbonyl functional group at the end of a chain of C atoms<\/td>\nOther Oxygen-Containing Functional Groups<\/td>\n<\/tr>
aliphatic hydrocarbons<\/td>\nA hydrocarbon based on chains of C atoms<\/td>\nHydrocarbons<\/td>\n<\/tr>
alkaline battery<\/td>\nA type of dry cell that contains an alkaline (i.e., basic) moist paste, rather than an acidic paste<\/td>\nApplications of Redox Reactions: Voltaic Cells<\/td>\n<\/tr>
alkane<\/td>\nAn aliphatic hydrocarbon with only single covalent bonds<\/td>\nHydrocarbons<\/td>\n<\/tr>
alkene<\/td>\nAn aliphatic hydrocarbon that contains a C\u2013C double bond<\/td>\nHydrocarbons<\/td>\n<\/tr>
alkyl halide<\/td>\nAn organic compound that contains a halogen atom<\/td>\nAlkyl halides and alcohols<\/td>\n<\/tr>
alkyne<\/td>\nAn aliphatic hydrocarbon that contains a C\u2013C triple bond<\/td>\nHydrocarbons<\/td>\n<\/tr>
alpha particle<\/td>\nA type of radioactive emission equivalent to a helium nucleus<\/td>\nRadioactivity<\/td>\n<\/tr>
amide group<\/td>\nA functional group that is the combination of the amine and carbonyl functional groups<\/td>\nOther Functional Groups<\/td>\n<\/tr>
amide bond<\/td>\nThe bond between the N atom and the C atom in an amide.<\/td>\nOther Functional Groups<\/td>\n<\/tr>
amine<\/td>\nAn organic derivative of ammonia<\/td>\nOther Functional Groups<\/td>\n<\/tr>
amorphous solid<\/td>\nA solid with no long-term structure or repetition<\/td>\nSolids<\/td>\n<\/tr>
amphiprotic<\/td>\nA substance that can act as a proton donor or a proton acceptor<\/td>\nBr\u00f8nsted-Lowry Acids and Bases<\/td>\n<\/tr>
analyte<\/td>\nThe reagent of unknown concentration<\/td>\nAcid-Base Titrations<\/td>\n<\/tr>
angular momentum quantum number (\u2113)<\/td>\nAn index that affects the energy and the spatial distribution of an electron in an atom<\/td>\nQuantum Numbers for Electrons<\/td>\n<\/tr>
anion<\/td>\nA species with an overall negative charge<\/td>\nIons and Ionic Compounds<\/td>\n<\/tr>
anode<\/td>\nThe half cell that contains the oxidation reaction<\/td>\nApplications of Redox Reactions: Voltaic Cells<\/td>\n<\/tr>
antibonding molecular orbital<\/td>\nA higher energy molecular orbital generated by destructive combination of atomic orbitals<\/td>\nMolecular Orbitals<\/td>\n<\/tr>
aromatic hydrocarbons<\/td>\nFlat ring systems, which contain continuously overlapping\u00a0p\u00a0orbitals, such as benzene<\/td>\nHydrocarbons<\/td>\n<\/tr>
Arrhenius acid<\/td>\nA compound that increases the hydrogen ion concentration in aqueous solution<\/td>\nArrhenius Acids and Bases<\/td>\n<\/tr>
Arrhenius base<\/td>\nA compound that increases the hydroxide ion concentration in aqueous solution<\/td>\nArrhenius Acids and Bases<\/td>\n<\/tr>
atmosphere (atm)<\/td>\nA unit of pressure equal to the average atmospheric pressure at sea level; defined as exactly 760 mmHg<\/td>\nPressure<\/td>\n<\/tr>
atom<\/td>\nThe smallest piece of an element that maintains the identity of that element<\/td>\nAtomic Theory<\/td>\n<\/tr>
atomic mass<\/td>\nThe sum of the number of protons and neutrons in a nucleus<\/td>\nAtomic Theory<\/td>\n<\/tr>
atomic mass<\/td>\nThe weighted average of the masses of the isotopes that compose an element<\/td>\nMasses of Atoms and Molecules<\/td>\n<\/tr>
atomic mass unit<\/td>\nOne-twelfth of the mass of a carbon-12 atom<\/td>\nMasses of Atoms and Molecules<\/td>\n<\/tr>
atomic number<\/td>\nThe number of protons in an atom<\/td>\nAtomic Theory<\/td>\n<\/tr>
atomic radius<\/td>\nAn indication of the size of an atom<\/td>\nPeriodic Trends<\/td>\n<\/tr>
atomic symbol<\/td>\nA one- or two-letter representation of the name of an element<\/td>\nAtomic Theory<\/td>\n<\/tr>
atomic theory<\/td>\nThe concept that atoms play a fundamental role in chemistry<\/td>\nAtomic Theory<\/td>\n<\/tr>
aufbau principle<\/td>\n(German for \u201cbuilding up\u201d): \u00a0electrons fill the lowest energy orbitals first.<\/td>\nOrganization of Electrons in Atoms<\/td>\n<\/tr>
autoionization constant of water (K<\/em>w<\/sub>)<\/td>\nThe product of the hydrogen ion and hydroxide ion concentrations<\/td>\nAutoionization of Water<\/td>\n<\/tr>
autoionization of water<\/td>\nWater molecules act as acids (proton donors) and bases (proton acceptors) with each other to a tiny extent in all aqueous solutions<\/td>\nAutoionization of Water<\/td>\n<\/tr>
Avogadro's law<\/td>\nA gas law that relates number of particles to volume<\/td>\nOther Gas Laws<\/td>\n<\/tr>
balanced chemical equation<\/td>\nA condition when the reactants and products of a chemical equation have the same number of atoms of all elements present<\/td>\nThe Chemical Equation<\/td>\n<\/tr>
base<\/td>\nA compound that increases the amount of\u00a0OH\u2212\u00a0ions in an aqueous solution<\/td>\nNeutralization Reactions<\/td>\n<\/tr>
basic salt<\/td>\nAn ionic compound whose aqueous solution is slightly basic<\/td>\nStrong and Weak Acids and Bases and Their Salts<\/td>\n<\/tr>
becquerel (Bq)<\/td>\nA unit of radioactivity equal to 1 decay per second<\/td>\nUnits of Radioactivity<\/td>\n<\/tr>
beta particle<\/td>\nA type of radioactive emission equivalent to an electron<\/td>\nRadioactivity<\/td>\n<\/tr>
boiling (or vaporization)<\/td>\nThe process of a liquid becoming a gas<\/td>\nPhase Transitions: Melting, Boiling and Subliming<\/td>\n<\/tr>
boiling point<\/td>\nThe characteristic temperature at which a liquid becomes a gas<\/td>\nPhase Transitions: Melting, Boiling and Subliming<\/td>\n<\/tr>
boiling point elevation<\/td>\nThe increase of a solution\u2019s boiling point because of the presence of solute<\/td>\nColligative Properties of Solutions<\/td>\n<\/tr>
boiling point elevation constant (K<\/em>b<\/sub>)<\/td>\nThe constant that relates the molality concentration of a solution and its boiling point change<\/td>\nColligative Properties of Solutions<\/td>\n<\/tr>
bond energy<\/td>\nThe approximate amount of energy needed to break a covalent bond<\/td>\nOther Aspects of Covalent Bonding<\/td>\n<\/tr>
bond order<\/td>\nA method of evaluating bond strength<\/td>\nMolecular Orbitals<\/td>\n<\/tr>
bonding electron pair<\/td>\nA pair of electrons that makes a covalent bond<\/td>\nCovalent Bonds<\/td>\n<\/tr>
bonding molecular orbital<\/td>\nThe lower energy molecular orbital generated by constructive combination of atomic orbitals<\/td>\nMolecular Orbitals<\/td>\n<\/tr>
Boyle's law<\/td>\nA gas law that relates pressure and volume at constant temperature and amount<\/td>\nGas Laws<\/td>\n<\/tr>
branched hydrocarbons<\/td>\nA carbon compound that is not a straight chain, having substituents appended to the longest chain<\/td>\nBranched Hydrocarbons<\/td>\n<\/tr>
Br\u00f8nsted-Lowry acid<\/td>\nAny species that can donate a proton to another molecule<\/td>\nBr\u00f8nsted-Lowry Acids and Bases<\/td>\n<\/tr>
Br\u00f8nsted-Lowry base<\/td>\nAny species that can accept a proton from another molecule<\/td>\nBr\u00f8nsted-Lowry Acids and Bases<\/td>\n<\/tr>
buffer<\/td>\nA solution that resists dramatic changes in pH<\/td>\nBuffers<\/td>\n<\/tr>
buffer capacity<\/td>\nThe amount of strong acid or base a buffer can counteract<\/td>\nBuffers<\/td>\n<\/tr>
burette or buret<\/td>\nA precisely calibrated volumetric delivery tube<\/td>\nAcid-Base Titrations<\/td>\n<\/tr>
calorie<\/td>\nA unit of energy measurement originally defined in terms of warming up a given quantity of water. 1 cal = 4.184 J<\/td>\nEnergy<\/td>\n<\/tr>
calorimeter<\/td>\nA container used to measure the heat of a chemical reaction<\/td>\nEnthalpy and Chemical Reactions<\/td>\n<\/tr>
calorimetry<\/td>\nThe process of measuring enthalpy changes for chemical reactions<\/td>\nEnthalpy and Chemical Reactions<\/td>\n<\/tr>
capillary action<\/td>\nThe behavior of a liquid in narrow surfaces due to differences in adhesion and cohesion<\/td>\nProperties of Liquids<\/td>\n<\/tr>
carbonyl group<\/td>\nA functional group where an O atom and a C atom are joined with a double bond<\/td>\nOther Oxygen-Containing Functional Groups<\/td>\n<\/tr>
carboxyl group<\/td>\nA functional group composed of a carbonyl group and an OH group<\/td>\nOther Oxygen-Containing Functional Groups<\/td>\n<\/tr>
carboxylate ion<\/td>\nA negatively charged ion derived from a carboxylic acid<\/td>\nOther Oxygen-Containing Functional Groups<\/td>\n<\/tr>
carboxylic acid<\/td>\nA molecule with a carboxyl group<\/td>\nOther Oxygen-Containing Functional Groups<\/td>\n<\/tr>
catalyst<\/td>\nA substance that increases the speed of a reaction<\/td>\nShifting Equilibria: Le Chatelier\u2019s Principle<\/td>\n<\/tr>
catalyst<\/td>\nA substance thaty accelerates a reaction by participating in it without being consumed<\/td>\nFactors that Affect the Rate of Reactions<\/td>\n<\/tr>
catalyst<\/td>\nA substance that lowers the activation energy of a specific reaction by providing an alternate reaction pathway<\/td>\nCatalysis<\/td>\n<\/tr>
cathode<\/td>\nThe half cell that contains the reduction reaction<\/td>\nApplications of Redox Reactions: Voltaic Cells<\/td>\n<\/tr>
cation<\/td>\nA species with an overall positive charge<\/td>\nIons and Ionic Compounds<\/td>\n<\/tr>
central atom<\/td>\nThe atom in the center of a molecule<\/td>\nCovalent Bonds<\/td>\n<\/tr>
Charles's law<\/td>\nA gas law that relates volume and temperature at constant pressure and amount<\/td>\nGas Laws<\/td>\n<\/tr>
chemical bond<\/td>\nThe connection between two atoms in a molecule<\/td>\nMolecules an Chemical Nomenclature<\/td>\n<\/tr>
chemical change<\/td>\nThe process of demonstrating a chemical property<\/td>\nSome Basic Definitions<\/td>\n<\/tr>
chemical equation<\/td>\nA concise way of representing a chemical reaction<\/td>\nThe Chemical Equation<\/td>\n<\/tr>
chemical equilibrium<\/td>\nThe point at which forward and reverse chemical reactions balance each other\u2019s progress<\/td>\nChemical Equilibrium<\/td>\n<\/tr>
chemical nomenclature<\/td>\nA very specific system for naming compounds, in which unique substances get unique names<\/td>\nMolecules an Chemical Nomenclature<\/td>\n<\/tr>
chemical property<\/td>\nA characteristic that describes how matter changes form in the presence of other matter<\/td>\nSome Basic Definitions<\/td>\n<\/tr>
chemistry<\/td>\nThe study of the interactions of matter with other matter and with energy<\/td>\nIntroduction<\/td>\n<\/tr>
coefficient<\/td>\nThe part of a number in scientific notation that is multiplied by a power of 10<\/td>\nExpressing Numbers<\/td>\n<\/tr>
coefficient<\/td>\nA number in a chemical equation indicating more than one molecule of the substance<\/td>\nThe Chemical Equation<\/td>\n<\/tr>
cohesion<\/td>\nThe tendency of a substance to interact with itself<\/td>\nProperties of Liquids<\/td>\n<\/tr>
colligative property<\/td>\nA property of solutions related to the fraction that the solute particles occupy in the solution, not their identity<\/td>\nColligative Properties of Solutions<\/td>\n<\/tr>
collision theory<\/td>\nThe theory that reactions occur when reactant molecules \u201ceffectively collide\u201d<\/td>\nFactors that Affect the Rate of Reactions<\/td>\n<\/tr>
combined gas law<\/td>\nA gas law that combines pressure, volume, and temperature<\/td>\nOther Gas Laws<\/td>\n<\/tr>
combustion reaction<\/td>\nA chemical reaction in which a reactant combines with oxygen to produce oxides of all other elements as products<\/td>\nComposition, Decomposition, and Combustion Reactions<\/td>\n<\/tr>
complete ionic equation<\/td>\nA chemical equation in which the dissolved ionic compounds are written as separated ions<\/td>\nIonic Equations: A Closer Look<\/td>\n<\/tr>
composition reaction<\/td>\nA chemical reaction in which a single substance is produced from multiple reactants<\/td>\nComposition, Decomposition, and Combustion Reactions<\/td>\n<\/tr>
compound<\/td>\nA combination of more than one element<\/td>\nSome Basic Definitions<\/td>\n<\/tr>
compressibility factor<\/td>\nA measure of the extent of deviation from ideal gas behaviour<\/td>\nReal Gases<\/td>\n<\/tr>
concentrated solution<\/td>\nA solution with a lot of solute<\/td>\nSome Definitions<\/td>\n<\/tr>
concentration<\/td>\nHow much solute is dissolved in a given amount of solvent<\/td>\nSome Definitions<\/td>\n<\/tr>
concentration (verb)<\/td>\nThe removal of solvent, which increases the concentration of the solute in the solution<\/td>\nDilutions and Concentrations<\/td>\n<\/tr>
condensation<\/td>\nThe process of a gas becoming a liquid<\/td>\nPhase Transitions: Melting, Boiling and Subliming<\/td>\n<\/tr>
condensed structure<\/td>\nA listing of the atoms bonded to each C atom in a chain<\/td>\nHydrocarbons<\/td>\n<\/tr>
conjugate acid-base pair<\/td>\nTwo species whose formulas differ by only a hydrogen ion<\/td>\nBr\u00f8nsted-Lowry Acids and Bases<\/td>\n<\/tr>
continuous spectrum<\/td>\nAn image that contains all colors of light<\/td>\nQuantum Numbers for Electrons<\/td>\n<\/tr>
conversion factor<\/td>\nA fraction that can be used to convert a quantity from one unit to another<\/td>\nConverting Units<\/td>\n<\/tr>
covalent bond<\/td>\nA chemical bond formed by two atoms sharing electrons<\/td>\nCovalent Bonds<\/td>\n<\/tr>
covalent network solids<\/td>\nA crystalline solid composed of atoms of one or more elements that are covalently bonded together in a seemingly never-ending fashion<\/td>\nSolids<\/td>\n<\/tr>
critical point<\/td>\nThe point at the highest temperature and pressure at which liquids and gases remain distinguishable<\/td>\nProperties of Liquids<\/td>\n<\/tr>
crystalline solid<\/td>\nA solid with a regular, repeating three-dimensional structure<\/td>\nSolids<\/td>\n<\/tr>
curie<\/td>\nA unit of radioactivity equal to\u00a03.7\u00d71010\u00a0decays\/s<\/td>\nUnits of Radioactivity<\/td>\n<\/tr>
d<\/em> block<\/td>\nThe columns of the periodic table in which\u00a0d<\/em>\u00a0subshells are being occupied<\/td>\nElectronic Structure and the Periodic Table<\/td>\n<\/tr>
Dalton's law of partial pressures<\/td>\nThe total pressure of a gas mixture,\u00a0Ptot, is equal to the sum of the partial pressures of the components,\u00a0Pi<\/td>\nGas Mixtures<\/td>\n<\/tr>
daughter isotope<\/td>\nThe product left over from the parent isotope in a nuclear equation<\/td>\nRadioactivity<\/td>\n<\/tr>
decomposition reaction<\/td>\nA chemical reaction in which a single substance becomes more than one substance<\/td>\nComposition, Decomposition, and Combustion Reactions<\/td>\n<\/tr>
degrees<\/td>\nThe unit of temperature scales<\/td>\nOther Units: Temperature and Density<\/td>\n<\/tr>
density<\/td>\nA physical property defined as a substance\u2019s mass divided by its volume<\/td>\nOther Units: Temperature and Density<\/td>\n<\/tr>
deposition<\/td>\nThe process of a gas becoming a solid<\/td>\nPhase Transitions: Melting, Boiling and Subliming<\/td>\n<\/tr>
derived unit<\/td>\nA unit that is a product or a quotient of a fundamental unit<\/td>\nExpressing Units<\/td>\n<\/tr>
diatomic molecule<\/td>\nA molecule with only two atoms<\/td>\nMolecules an Chemical Nomenclature<\/td>\n<\/tr>
diffusion<\/td>\nThe movement of gas molecules through one or more additional types of gas via random molecular motion<\/td>\nMolecular Effusion and Diffusion<\/td>\n<\/tr>
dilute<\/td>\nA solution with very little solute<\/td>\nSome Definitions<\/td>\n<\/tr>
dilution<\/td>\nThe addition of solvent, which decreases the concentration of the solute in the solution<\/td>\nDilutions and Concentrations<\/td>\n<\/tr>
dilution equation<\/td>\nThe mathematical formula for calculating new concentrations or volumes when a solution is diluted or concentrated<\/td>\nDilutions and Concentrations<\/td>\n<\/tr>
dipole-dipole interactions<\/td>\nAn intermolecular force caused by molecules with a permanent dipole<\/td>\nIntermolecular Forces<\/td>\n<\/tr>
dispersion force (or London dispersion force)<\/td>\nAn intermolecular force caused by the instantaneous position of an electron in a molecule<\/td>\nIntermolecular Forces<\/td>\n<\/tr>
dissociation<\/td>\nThe process of an ionic compound separating into ions when it dissolves<\/td>\nIonic Equations: A Closer Look<\/td>\n<\/tr>
double bond<\/td>\nA covalent bond composed of two pairs of bonding electrons<\/td>\nCovalent Bonds<\/td>\n<\/tr>
double-replacement reaction<\/td>\nA chemical reaction in which parts of two ionic compounds are exchanged<\/td>\nTypes of Chemical Reactions: Single- and Double-Displacement Reactions<\/td>\n<\/tr>
dry cell<\/td>\nA modern battery that does not contain large amounts of aqueous solution<\/td>\nApplications of Redox Reactions: Voltaic Cells<\/td>\n<\/tr>
dynamic equilibrium<\/td>\nWhen a process still occurs but the opposite process also occurs at the same rate so that there is no net change in the system.<\/td>\nProperties of Liquids<\/td>\n<\/tr>
effective nuclear charge (Zeff)<\/td>\nThe net nuclear charge feld by valence electrons<\/td>\nPeriodic Trends<\/td>\n<\/tr>
effusion<\/td>\nThe movement of gas molecules from one container to another via a tiny hole<\/td>\nMolecular Effusion and Diffusion<\/td>\n<\/tr>
electrodes<\/td>\nThe cathode or anode of a voltaic cell<\/td>\nApplications of Redox Reactions: Voltaic Cells<\/td>\n<\/tr>
electrolysis<\/td>\nThe process of making a nonspontaneous redox reaction occur by forcing electricity into a cell<\/td>\nElectrolysis<\/td>\n<\/tr>
electrolytic cell<\/td>\nA cell into which electricity is forced to make a nonspontaneous reaction occur<\/td>\nElectrolysis<\/td>\n<\/tr>
electromagnetic spectrum<\/td>\nThe full span of the possible wavelengths, frequencies, and energies of light<\/td>\nLight<\/td>\n<\/tr>
electron<\/td>\nA tiny subatomic particle with a negative charge<\/td>\nAtomic Theory<\/td>\n<\/tr>
electron affinity (EA)<\/td>\nThe energy change when a gas-phase atom accepts an electron<\/td>\nPeriodic Trends<\/td>\n<\/tr>
electron configuration<\/td>\nA listing of the shell and subshells labels<\/td>\nOrganization of Electrons in Atoms<\/td>\n<\/tr>
electron deficient molecules<\/td>\nA molecule with less than eight electrons in the valence shell of an atom<\/td>\nViolations of the Octet Rule<\/td>\n<\/tr>
electron group geometry<\/td>\nhow electron groups (bonds and nonbonding electron pairs) are arranged<\/td>\nMolecular Shapes and Polarity<\/td>\n<\/tr>
electron groups<\/td>\nA covalent bond of any type or a lone electron pair<\/td>\nMolecular Shapes and Polarity<\/td>\n<\/tr>
electron shell<\/td>\nA term used to describe electrons with the same principal quantum number<\/td>\nQuantum Numbers for Electrons<\/td>\n<\/tr>
electronegativity<\/td>\nA\u00a0scale for judging how much atoms of any element attract electrons<\/td>\nOther Aspects of Covalent Bonding<\/td>\n<\/tr>
electroplating<\/td>\nThe deposition of a thin layer of metal on an object for protective or decorative purposes<\/td>\nElectrolysis<\/td>\n<\/tr>
element<\/td>\nA substance that cannot be broken down into simpler chemical substances by ordinary chemical means<\/td>\nSome Basic Definitions<\/td>\n<\/tr>
elementary step<\/td>\nEach event that occurs in a chemical reaction as a result of an effective collision<\/td>\nReaction Mechanisms<\/td>\n<\/tr>
elimination reaction<\/td>\nThe removal of a functional group (either X or OH) and a H atom from an adjacent carbon<\/td>\nAlkyl halides and alcohols<\/td>\n<\/tr>
endothermic<\/td>\nA chemical reaction that has a positive change in enthalpy<\/td>\nEnthalpy and Chemical Reactions<\/td>\n<\/tr>
energy<\/td>\nThe ability to do work.\u00a0is the ability to do work<\/td>\nEnergy<\/td>\n<\/tr>
enthalpy change<\/td>\nThe heat of a process at constant pressure; denoted\u00a0\u0394H<\/td>\nEnthalpy and Chemical Reactions<\/td>\n<\/tr>
enthalpy of formation<\/td>\nThe enthalpy change for a formation reaction; denoted\u00a0\u0394Hf.\u00a0and is given the symbol \u0394Hf<\/td>\nFormation Reactions<\/td>\n<\/tr>
enthalpy of fusion<\/td>\nThe amount of energy needed to change from a solid to a liquid or from a liquid to a solid<\/td>\nPhase Transitions: Melting, Boiling and Subliming<\/td>\n<\/tr>
enthalpy of sublimation<\/td>\nThe amount of energy needed to change from a solid to a gas or from a gas to a solid<\/td>\nPhase Transitions: Melting, Boiling and Subliming<\/td>\n<\/tr>
enthalpy of vaporization<\/td>\nThe amount of energy needed to change from a liquid to a gas or from a gas to a liquid<\/td>\nPhase Transitions: Melting, Boiling and Subliming<\/td>\n<\/tr>
entropy<\/td>\nThe level of randomness (or disorder) of a system, or a measure of the energy dispersal of the molecules in the system<\/td>\nEntropy and the Second Law of Thermodynamics<\/td>\n<\/tr>
enzyme<\/td>\nProtein molecules which serve to catalyze biochemical reactions<\/td>\nCatalysis<\/td>\n<\/tr>
enzyme-substrate complex<\/td>\nThe binding of substrate to the enzymatic active site<\/td>\nCatalysis<\/td>\n<\/tr>
equilibrium constant (Keq)<\/td>\nA numerical value that relates to the ratio of products and reactants at equilibrium<\/td>\nThe Equilibrium Constant<\/td>\n<\/tr>
equivalence point<\/td>\nThe point of the reaction when all the analyte has been reacted with the titrant<\/td>\nAcid-Base Titrations<\/td>\n<\/tr>
ester group<\/td>\nA functional group made by combining a carboxylic acid with an alcohol<\/td>\nOther Oxygen-Containing Functional Groups<\/td>\n<\/tr>
ether group<\/td>\nA functional group that has an O atom attached to two organic groups<\/td>\nOther Oxygen-Containing Functional Groups<\/td>\n<\/tr>
evaporation<\/td>\nThe formation of a gas phase from a liquid at temperatures below the boiling point<\/td>\nProperties of Liquids<\/td>\n<\/tr>
exact number<\/td>\nA number from a defined relationship that technically has an infinite number of significant figures<\/td>\nConverting Units<\/td>\n<\/tr>
exothermic<\/td>\nA chemical reaction that has a negative change in enthalpy<\/td>\nEnthalpy and Chemical Reactions<\/td>\n<\/tr>
expanded valence shell molecules<\/td>\nA molecule with more than eight electrons in the valence shell of an atom<\/td>\nViolations of the Octet Rule<\/td>\n<\/tr>
experiment<\/td>\nA test of the natural universe to see if a guess (hypothesis) is correct<\/td>\nChemistry as a Science<\/td>\n<\/tr>
exponent<\/td>\nThe raised number to the right of a 10 indicating the number of factors of 10 in the original number<\/td>\nExpressing Numbers<\/td>\n<\/tr>
f<\/em> block<\/td>\nThe columns of the periodic table in which\u00a0f<\/em>\u00a0subshells are being occupied<\/td>\nElectronic Structure and the Periodic Table<\/td>\n<\/tr>
fission<\/td>\nThe breaking apart of an atomic nucleus into smaller nuclei<\/td>\nRadioactivity<\/td>\n<\/tr>
formation reaction<\/td>\nA chemical reaction that forms one mole of a substance from its constituent elements in their standard states<\/td>\nFormation Reactions<\/td>\n<\/tr>
freezing point depression<\/td>\nThe decrease of a solution\u2019s freezing point because of the presence of solute<\/td>\nColligative Properties of Solutions<\/td>\n<\/tr>
freezing point depression constant (Kf)<\/td>\nThe constant that relates the molality concentration of a solution and its freezing point change<\/td>\nColligative Properties of Solutions<\/td>\n<\/tr>
frequency<\/td>\nThe number of cycles of light that pass a given point in one second<\/td>\nLight<\/td>\n<\/tr>
frequency factor (A<\/em>)<\/td>\nA factor that takes into account the frequency of reactions and the likelihood of correct molecular orientation<\/td>\nActivation Energy and the Arrhenius Equation<\/td>\n<\/tr>
frontier molecular orbitals<\/td>\nA term which refers to the HOMO and LUMO, the most likely orbitals to be involved in chemical reactions or processes<\/td>\nMolecular Orbitals<\/td>\n<\/tr>
functional group<\/td>\nA collection of atoms or bonds with certain characteristic reactions<\/td>\nAlkyl halides and alcohols<\/td>\n<\/tr>
fundamental units<\/td>\nOne of the seven basic units of SI used in science<\/td>\nExpressing Units<\/td>\n<\/tr>
gamma ray<\/td>\nA type of radioactive emission that is a very energetic form of electromagnetic radiation<\/td>\nRadioactivity<\/td>\n<\/tr>
gas law<\/td>\nA simple mathematical formula that allows one to model, or predict, the behavior of a gas<\/td>\nGas Laws<\/td>\n<\/tr>
Gay-Lussac's law<\/td>\nA gas law that relates pressure with absolute temperature<\/td>\nOther Gas Laws<\/td>\n<\/tr>
Geiger counter<\/td>\nAn electrical device that detects radioactivity<\/td>\nUnits of Radioactivity<\/td>\n<\/tr>
Gibbs free energy (G<\/em>)<\/td>\nA measure of spontaneity which incorporates both enthalpy and entropy<\/td>\nGibbs Free Energy<\/td>\n<\/tr>
Graham's law of effusion<\/td>\nA law which relates the rate of effusion of a gas to the inverse of the square root of its molar mass<\/td>\nMolecular Effusion and Diffusion<\/td>\n<\/tr>
gray (Gy)<\/td>\nA unit of radioactive exposure qual to 100 rad<\/td>\nUnits of Radioactivity<\/td>\n<\/tr>
half cell<\/td>\nA part of a voltaic cell that contains one half reaction<\/td>\nApplications of Redox Reactions: Voltaic Cells<\/td>\n<\/tr>
half reaction<\/td>\nThe individual oxidation or reduction reaction of a redox reaction<\/td>\nBalancing Redox Reactions<\/td>\n<\/tr>
half reaction method<\/td>\nThe method of balancing redox reactions by writing and balancing the individual half reactions<\/td>\nBalancing Redox Reactions<\/td>\n<\/tr>
half-life<\/td>\nThe amount of time it takes for one-half of a radioactive isotope to decay<\/td>\nHalf-Life<\/td>\n<\/tr>
half-life<\/td>\nThe amount of time required for the concentration of a reactant to drop to one half of its initial concentration<\/td>\nConcentration-Time Relationships: Integrated Rate Laws<\/td>\n<\/tr>
heat<\/td>\nThe transfer of energy from one body to another due to a difference in temperature<\/td>\nWork and Heat<\/td>\n<\/tr>
heating curve<\/td>\nA plot of the temperature versus the amount of heat added<\/td>\nPhase Transitions: Melting, Boiling and Subliming<\/td>\n<\/tr>
Hess's law<\/td>\nWhen chemical equations are combined algebraically, their enthalpies can be combined in exactly the same way<\/td>\nHess's Law<\/td>\n<\/tr>
heterogeneous catalyst<\/td>\nA catalyst that is in a different phase from one or more of the reactants<\/td>\nCatalysis<\/td>\n<\/tr>
heterogeneous equilibrium<\/td>\nAn equilibrium in which more than one phase of reactants or products is present<\/td>\nThe Equilibrium Constant<\/td>\n<\/tr>
heterogeneous mixture<\/td>\nA non-uniform combination of more than one substance<\/td>\nSome Basic Definitions<\/td>\n<\/tr>
HOMO<\/td>\nThe highest occupied molecular orbital<\/td>\nMolecular Orbitals<\/td>\n<\/tr>
homogeneous catalyst<\/td>\nA catalyst that is present in the same phase as the reactant molecules<\/td>\nCatalysis<\/td>\n<\/tr>
homogeneous mixture<\/td>\nA uniform mixture of more than one substance that behaves as a single substance<\/td>\nSome Basic Definitions<\/td>\n<\/tr>
Hund's rule<\/td>\nOne electron is placed in each degenerate orbital before pairing electrons in the same orbital<\/td>\nOrganization of Electrons in Atoms<\/td>\n<\/tr>
hybridization<\/td>\nA mathematical mixing of atomic orbitals<\/td>\nValence Bond Theory and Hybrid Orbitals<\/td>\n<\/tr>
hydrocarbons<\/td>\nAn organic compound composed of carbon and hydrogen<\/td>\nHydrocarbons<\/td>\n<\/tr>
hydrogen bonding<\/td>\nThe very strong interaction between molecules due to H atoms being bonded to N, O, or F atoms<\/td>\nIntermolecular Forces<\/td>\n<\/tr>
hydrogenation reaction<\/td>\nThe reaction of hydrogen across a C\u2013C double or triple bond, usually in the presence of a catalyst<\/td>\nHydrocarbons<\/td>\n<\/tr>
hydronium ion<\/td>\nThe actual chemical species that represents a hydrogen ion in aqueous solution<\/td>\nArrhenius Acids and Bases<\/td>\n<\/tr>
hypothesis<\/td>\nAn educated guess about how the natural universe works<\/td>\nChemistry as a Science<\/td>\n<\/tr>
hyrolysis<\/td>\nA reaction with water<\/td>\nBr\u00f8nsted-Lowry Acids and Bases<\/td>\n<\/tr>
ICE chart<\/td>\nA table used to calculate equilibria values featuring rows of initial, change and equlibria concentration<\/td>\nCalculating Equilibrium Constant Values<\/td>\n<\/tr>
ideal gas<\/td>\nA gas that conforms exactly to the tenets of the kinetic molecular theory<\/td>\nReal Gases<\/td>\n<\/tr>
ideal gas law<\/td>\nA gas law that relates all four independent physical properties of a gas under any conditions<\/td>\nThe Ideal Gas Law and Some Applications<\/td>\n<\/tr>
indicator<\/td>\nA substance whose color change indicates the equivalence point of a titration<\/td>\nAcid-Base Titrations<\/td>\n<\/tr>
initial rate<\/td>\nThe instantaneous rate at the start of a reaction<\/td>\nReaction Rates<\/td>\n<\/tr>
initial rates method<\/td>\nA method to determine the rate law from the instantaneous reaction rate upon mixing the reactants<\/td>\nRate Laws<\/td>\n<\/tr>
instantaneous reaction rate<\/td>\nThe rate of reaction at one instant in time<\/td>\nReaction Rates<\/td>\n<\/tr>
intermediate<\/td>\nA chemical species does not appear in the overall balanced equation and is generated in one elementary step but used up in a subsequent step<\/td>\nReaction Mechanisms<\/td>\n<\/tr>
ion<\/td>\nA species with an overall electric charge<\/td>\nIons and Ionic Compounds<\/td>\n<\/tr>
ionic compound<\/td>\nA compound formed from positive and negative ions<\/td>\nIons and Ionic Compounds<\/td>\n<\/tr>
ionic formula<\/td>\nThe chemical formula for an ionic compound<\/td>\nIons and Ionic Compounds<\/td>\n<\/tr>
ionic solid<\/td>\nA crystalline solid composed of ions<\/td>\nSolids<\/td>\n<\/tr>
ionization energy (IE)<\/td>\nThe amount of energy required to remove an elec tron from an atom in the gas phase<\/td>\nPeriodic Trends<\/td>\n<\/tr>
isolated system<\/td>\nA system that does not allow a transfer of energy or matter into or out of the system<\/td>\nEnergy<\/td>\n<\/tr>
isomer<\/td>\nA molecule with the same molecular formula as another molecule but a different structure<\/td>\nHydrocarbons<\/td>\n<\/tr>
isothermal<\/td>\nA process that does not change the temperature<\/td>\nPhase Transitions: Melting, Boiling and Subliming<\/td>\n<\/tr>
isotopes<\/td>\nAtoms of the same element that have different numbers of neutrons<\/td>\nAtomic Theory<\/td>\n<\/tr>
joule<\/td>\nThe SI unit of energy<\/td>\nEnergy<\/td>\n<\/tr>
Kelvin scale<\/td>\nThe fundamental unit of temperature in SI<\/td>\nOther Units: Temperature and Density<\/td>\n<\/tr>
ketone<\/td>\nA compound where the carbonyl carbon is attached to two carbon chains<\/td>\nOther Oxygen-Containing Functional Groups<\/td>\n<\/tr>
kinetic energy<\/td>\nThe energy due to motion<\/td>\nKinetic-Molecular Theory of Gases<\/td>\n<\/tr>
kinetic-molecular theory of gases<\/td>\nA model which helps us understand gases at the molecular level and their physical properties<\/td>\nKinetic-Molecular Theory of Gases<\/td>\n<\/tr>
kinetics<\/td>\nThe study of reaction rate and the factors that can influence reaction rate<\/td>\nIntroduction to Kinetics<\/td>\n<\/tr>
law of conservation of energy<\/td>\nThe total energy of an isolated system does not increase or decrease<\/td>\nEnergy<\/td>\n<\/tr>
law of mass action<\/td>\nThe relationship of the amounts of reactants and products at equilibrium<\/td>\nThe Equilibrium Constant<\/td>\n<\/tr>
Le Chatelier\u2019s principle<\/td>\nIf an equilibrium is stressed, then the reaction shifts to reduce the stress<\/td>\nShifting Equilibria: Le Chatelier\u2019s Principle<\/td>\n<\/tr>
Lewis diagram<\/td>\nA representation of the valence electrons of an atom that uses dots around the symbol of the element<\/td>\nLewis Electron Dot Diagrams<\/td>\n<\/tr>
limiting reagent<\/td>\nThe reactant that runs out first for a given chemical reaction<\/td>\nLimiting Reagents<\/td>\n<\/tr>
line spectrum<\/td>\nAn image that contains only certain colors of light<\/td>\nQuantum Numbers for Electrons<\/td>\n<\/tr>
locant<\/td>\nThe numerical position of a substituent<\/td>\nBranched Hydrocarbons<\/td>\n<\/tr>
lock and key model<\/td>\nA simple model used to describe enzyme activity, where substrates must fit into appropriately shaped active sites<\/td>\nCatalysis<\/td>\n<\/tr>
lone electron pairs<\/td>\nA pair of electrons that does not make a covalent bond<\/td>\nCovalent Bonds<\/td>\n<\/tr>
LUMO<\/td>\nThe lowest unoccupied molecular orbital<\/td>\nMolecular Orbitals<\/td>\n<\/tr>
magnetic quantum number (ml)<\/td>\nThe index that determines the orientation of the electron\u2019s spatial distribution<\/td>\nQuantum Numbers for Electrons<\/td>\n<\/tr>
mass-mass calculation<\/td>\nA calculation in which you start with a given mass of a substance and calculate the mass of another substance involved in the chemical equation<\/td>\nMole-Mass and Mass-Mass Calculations<\/td>\n<\/tr>
matter<\/td>\nAnything that has mass and takes up space.\u00a0is anything that has mass and takes up space<\/td>\nSome Basic Definitions<\/td>\n<\/tr>
mean free path<\/td>\nThe average distance traveled by a molecule between collisions<\/td>\nMolecular Effusion and Diffusion<\/td>\n<\/tr>
melting<\/td>\nThe process of a solid becoming a liquid<\/td>\nPhase Transitions: Melting, Boiling and Subliming<\/td>\n<\/tr>
melting point<\/td>\nThe characteristic temperature at which a solid becomes a liquid<\/td>\nPhase Transitions: Melting, Boiling and Subliming<\/td>\n<\/tr>
meniscus<\/td>\nThe curved surface a liquid makes as it approaches a solid barrier<\/td>\nProperties of Liquids<\/td>\n<\/tr>
metal<\/td>\nAn element that conducts electricity and heat well and is shiny, silvery, solid, ductile, and malleable<\/td>\nSome Basic Definitions<\/td>\n<\/tr>
metallic solid<\/td>\nA solid with the characteristic properties of a metal<\/td>\nSolids<\/td>\n<\/tr>
microstate (W<\/em>)<\/td>\nA\u00a0term used\u00a0to describe different possible arrangements of molecular position and kinetic energy, at a particular thermodynamic state<\/td>\nEntropy and the Second Law of Thermodynamics<\/td>\n<\/tr>
millimeters of mercury (mmHg)<\/td>\nThe amount of pressure exerted by a column of mercury exactly 1 mm high<\/td>\nPressure<\/td>\n<\/tr>
mixture<\/td>\nA physical combination of more than one substance<\/td>\nSome Basic Definitions<\/td>\n<\/tr>
molality (m)<\/td>\nThe number of moles of solute per kilogram of solvent<\/td>\nQuantitative Units of Concentration<\/td>\n<\/tr>
molar mass<\/td>\nThe mass of 1 mol of a substance in grams<\/td>\nThe Mole<\/td>\n<\/tr>
molar volume<\/td>\nThe volume of exactly 1 mol of a gas; equal to 22.4 L at STP<\/td>\nThe Ideal Gas Law and Some Applications<\/td>\n<\/tr>
molarity (M)<\/td>\nThe number of moles of solute divided by the number of liters of solution<\/td>\nQuantitative Units of Concentration<\/td>\n<\/tr>
mole<\/td>\nThe number of things equal to the number of atoms in exactly 12 g of carbon-12; equals\u00a06.022\u00d71023\u00a0things<\/td>\nThe Mole<\/td>\n<\/tr>
mole fraction<\/td>\nThe ratio of the number of moles of a component in a mixture divided by the total number of moles in the sample<\/td>\nGas Mixtures<\/td>\n<\/tr>
mole fraction<\/td>\nThe ratio of the number of moles of a component to the total number of moles in a system<\/td>\nColligative Properties of Solutions<\/td>\n<\/tr>
molecular formula<\/td>\nA formal listing of what and how many atoms are in a molecule<\/td>\nMolecules an Chemical Nomenclature<\/td>\n<\/tr>
molecular geometry<\/td>\nhow the atoms in a molecule are arranged<\/td>\nMolecular Shapes and Polarity<\/td>\n<\/tr>
molecular mass<\/td>\nThe sum of the masses of the atoms in a molecule<\/td>\nMasses of Atoms and Molecules<\/td>\n<\/tr>
molecular orbital theory (MO theory)<\/td>\nA more sophisticated model\u00a0 of chemical bonding where new molecular orbitals are generated using a mathematical process called Linear Combination of Atomic Orbitals (LCAO)<\/td>\nMolecular Orbitals<\/td>\n<\/tr>
molecular polarity<\/td>\nThe vector sum of the individual bond dipoles<\/td>\nMolecular Shapes and Polarity<\/td>\n<\/tr>
molecular solid<\/td>\nA crystalline solid whose components are covalently bonded molecules<\/td>\nSolids<\/td>\n<\/tr>
molecularity<\/td>\nThe total number of molecules that participate in the effective collision of the elementary step<\/td>\nReaction Mechanisms<\/td>\n<\/tr>
molecule<\/td>\nThe smallest part of a substance that has the physical and chemical properties of that substance<\/td>\nMolecules an Chemical Nomenclature<\/td>\n<\/tr>
mole-mass calculation<\/td>\nA calculation in which you start with a given number of moles of a substance and calculate the mass of another substance involved in the chemical equation, or vice versa<\/td>\nMole-Mass and Mass-Mass Calculations<\/td>\n<\/tr>
mole-mole calculation<\/td>\nA stoichiometry calculation when one starts with moles of one substance and convert to moles of another substance using the balanced chemical equation<\/td>\nThe Mole in Chemical Reactions<\/td>\n<\/tr>
monomer<\/td>\nThe repeated unit of a polymer<\/td>\nPolymers<\/td>\n<\/tr>
net ionic equation<\/td>\nA chemical equation with the spectator ions removed<\/td>\nIonic Equations: A Closer Look<\/td>\n<\/tr>
neutral salt<\/td>\nAn ionic compound that does not affect the acidity of its aqueous solution<\/td>\nStrong and Weak Acids and Bases and Their Salts<\/td>\n<\/tr>
neutralization reaction<\/td>\nThe reaction of an acid with a base to produce water and a salt<\/td>\nNeutralization Reactions<\/td>\n<\/tr>
neutralization reaction<\/td>\nThe reaction of an acid and a base to produce water and a salt<\/td>\nArrhenius Acids and Bases<\/td>\n<\/tr>
neutron<\/td>\nA subatomic particle with no charge<\/td>\nAtomic Theory<\/td>\n<\/tr>
node (nodal plane)<\/td>\nAn area of zero electron density<\/td>\nMolecular Orbitals<\/td>\n<\/tr>
nomenclature<\/td>\nThe rules of naming in organic chemistry<\/td>\nBranched Hydrocarbons<\/td>\n<\/tr>
nonmetal<\/td>\nAn element that exists in various colors and phases, is brittle, and does not conduct electricity or heat well<\/td>\nSome Basic Definitions<\/td>\n<\/tr>
nonpolar covalent bond<\/td>\nThe equal sharing of electrons in a covalent bond<\/td>\nOther Aspects of Covalent Bonding<\/td>\n<\/tr>
normal boiling point<\/td>\nThe characteristic temperature at which a liquid becomes a gas when the surrounding pressure is exactly 1 atm<\/td>\nPhase Transitions: Melting, Boiling and Subliming<\/td>\n<\/tr>
nuclear energy<\/td>\nThe controlled harvesting of energy from fission reactions<\/td>\nNuclear Energy<\/td>\n<\/tr>
nuclear equation<\/td>\nA chemical equation that emphasizes changes in atomic nuclei<\/td>\nRadioactivity<\/td>\n<\/tr>
nuclear model<\/td>\nThe model of an atom that has the protons and neutrons in a central nucleus with the electrons in orbit about the nucleus<\/td>\nAtomic Theory<\/td>\n<\/tr>
nucleus<\/td>\nThe center of an atom that contains protons and neutrons<\/td>\nAtomic Theory<\/td>\n<\/tr>
odd-electron molecules<\/td>\nA molecule with an odd number of electrons in the valence shell of an atom<\/td>\nViolations of the Octet Rule<\/td>\n<\/tr>
orbital<\/td>\nThe specific set of principal, angular momentum, and magnetic quantum numbers for an electron<\/td>\nQuantum Numbers for Electrons<\/td>\n<\/tr>
osmosis<\/td>\nThe tendency of solvent molecules to pass through a semipermeable membrane due to concentration differences<\/td>\nColligative Properties of Solutions<\/td>\n<\/tr>
osmotic pressure<\/td>\nThe tendency of a solution to pass solvent through a semipermeable membrane due to concentration differences<\/td>\nColligative Properties of Solutions<\/td>\n<\/tr>
oxidation<\/td>\nThe loss of one or more electrons by an atom; an increase in oxidation number<\/td>\nOxidation-Reduction Reactions<\/td>\n<\/tr>
oxidation<\/td>\nThe loss of one or more electrons by an atom; an increase in oxidation number<\/td>\nOxidation-Reduction Reactions<\/td>\n<\/tr>
oxidation number<\/td>\nA number assigned to an atom that helps keep track of the number of electrons on the atom<\/td>\nOxidation-Reduction Reactions<\/td>\n<\/tr>
oxidation number<\/td>\nA number assigned to an atom that helps keep track of the number of electrons on the atom<\/td>\nOxidation-Reduction Reactions<\/td>\n<\/tr>
oxidation-reduction (redox) reactions<\/td>\nA chemical reaction that involves the transfer of electrons<\/td>\nOxidation-Reduction Reactions<\/td>\n<\/tr>
p block<\/td>\nThe columns of the periodic table in which\u00a0p\u00a0subshells are being occupied<\/td>\nElectronic Structure and the Periodic Table<\/td>\n<\/tr>
parent isotope<\/td>\nThe reactant in a nuclear equation<\/td>\nRadioactivity<\/td>\n<\/tr>
parts per billion (ppb)<\/td>\nRatio of mass of solute to total mass of sample times 1,000,000,000<\/td>\nQuantitative Units of Concentration<\/td>\n<\/tr>
parts per million (ppm)<\/td>\nRatio of mass of solute to total mass of sample times 1,000,000<\/td>\nQuantitative Units of Concentration<\/td>\n<\/tr>
parts per thousand (ppth)<\/td>\nRatio of mass of solute to total mass of sample times 1,000<\/td>\nQuantitative Units of Concentration<\/td>\n<\/tr>
Pauli exclusion principle<\/td>\nNo two electrons in an atom can have the same set of four quantum numbers<\/td>\nOrganization of Electrons in Atoms<\/td>\n<\/tr>
percent yield<\/td>\nActual yield divided by theoretical yield times 100% to give a percentage between 0% and 100%<\/td>\nYields<\/td>\n<\/tr>
percentage composition by mass\u00a0(or\u00a0mass percentage, % m\/m)<\/td>\nRatio of mass of solute to the total mass of a sample times 100<\/td>\nQuantitative Units of Concentration<\/td>\n<\/tr>
periodic table<\/td>\nA chart of all the elements<\/td>\nAtomic Theory<\/td>\n<\/tr>
periodic trends<\/td>\nThe variation of properties versus position on the periodic table<\/td>\nPeriodic Trends<\/td>\n<\/tr>
pH<\/td>\nThe negative logarithm of the hydrogen ion concentration<\/td>\nThe pH Scale<\/td>\n<\/tr>
pH scale<\/td>\nThe range of values from 0 to 14 that describes the acidity or basicity of a solution<\/td>\nThe pH Scale<\/td>\n<\/tr>
phase<\/td>\nAn important physical property that defines whether matter is a solid, liquid, gas or supercritical fluid<\/td>\nSome Basic Definitions<\/td>\n<\/tr>
phase diagram<\/td>\nA graphical representation of the equilibrium relationships that exist between the phases of a substance under specified pressures and temperatures<\/td>\nProperties of Liquids<\/td>\n<\/tr>
photon<\/td>\nThe name of a discrete unit of light acting as a particle<\/td>\nLight<\/td>\n<\/tr>
physical change<\/td>\nA change that occurs when a sample of matter changes one or more of its physical properties<\/td>\nSome Basic Definitions<\/td>\n<\/tr>
physical property<\/td>\nA characteristic that describes matter as it exists<\/td>\nSome Basic Definitions<\/td>\n<\/tr>
pi bond (\u03c0 bond)<\/td>\nThe sideways overlap of\u00a0p orbitals, placing electron density on opposite sides of the inter-nuclear axis - a double or triple bond<\/td>\nValence Bond Theory and Hybrid Orbitals<\/td>\n<\/tr>
Planck's constant<\/td>\nThe proportionality constant between the frequency and the energy of light: 6.626 \u00d7 10\u221234 J\u00b7s<\/td>\nLight<\/td>\n<\/tr>
pOH<\/td>\nThe negative logarithm of the hydroxide ion concentration<\/td>\nThe pH Scale<\/td>\n<\/tr>
polar covalent bond<\/td>\nA covalent bond between different atoms that attract the shared electrons by different amounts and cause an imbalance of electron distribution<\/td>\nOther Aspects of Covalent Bonding<\/td>\n<\/tr>
polarity<\/td>\nA measure of the unequal sharing of electrons which has resulted in a dipole moment<\/td>\nOther Aspects of Covalent Bonding<\/td>\n<\/tr>
polyatomic ions<\/td>\nAn ion that contains more than one atom<\/td>\nIons and Ionic Compounds<\/td>\n<\/tr>
polymer<\/td>\nA long molecule made of many repeating units<\/td>\nPolymers<\/td>\n<\/tr>
polymerization<\/td>\nThe process of making a polymer<\/td>\nPolymers<\/td>\n<\/tr>
polyprotic acid<\/td>\nAn acid capable of donating more than one H+ ion<\/td>\nSome Special Types of Equilibria<\/td>\n<\/tr>
precipitate<\/td>\nA solid that falls out of solution in a precipitation reaction<\/td>\nTypes of Chemical Reactions: Single- and Double-Displacement Reactions<\/td>\n<\/tr>
precipitation reaction<\/td>\nA chemical reaction in which two ionic compounds are dissolved in water and form a new ionic compound that does not dissolve<\/td>\nTypes of Chemical Reactions: Single- and Double-Displacement Reactions<\/td>\n<\/tr>
prefix<\/td>\nA prefix used with a unit that refers to a multiple or fraction of a fundamental unit to make a more conveniently sized unit for a specific quantity<\/td>\nExpressing Units<\/td>\n<\/tr>
pressure<\/td>\nForce per unit area<\/td>\nPressure<\/td>\n<\/tr>
primary battery<\/td>\nA battery that cannot be recharged<\/td>\nApplications of Redox Reactions: Voltaic Cells<\/td>\n<\/tr>
principal quantum number (n)<\/td>\nThe index that largely determines the energy of an electron in an atom<\/td>\nQuantum Numbers for Electrons<\/td>\n<\/tr>
product<\/td>\nA final substance in a chemical equation<\/td>\nThe Chemical Equation<\/td>\n<\/tr>
proton<\/td>\nA subatomic particle with a positive charge<\/td>\nAtomic Theory<\/td>\n<\/tr>
qualitative<\/td>\nA description of the quality of an object<\/td>\nChemistry as a Science<\/td>\n<\/tr>
quantitative<\/td>\nA description of a specific amount of something<\/td>\nChemistry as a Science<\/td>\n<\/tr>
quantization<\/td>\nWhen a quantity is restricted to having only certain values<\/td>\nQuantum Numbers for Electrons<\/td>\n<\/tr>
quantum mechanics<\/td>\nThe theory of electrons that treats them as a wave<\/td>\nQuantum Numbers for Electrons<\/td>\n<\/tr>
quantum number<\/td>\nAn index that corresponds to a property of an electron, like its energy<\/td>\nQuantum Numbers for Electrons<\/td>\n<\/tr>
rad<\/td>\nA unit of radioactive exposure equal to 0.01 J\/g of tissue<\/td>\nUnits of Radioactivity<\/td>\n<\/tr>
radioactive decay<\/td>\nThe spontaneous change of a nucleus from one element to another<\/td>\nRadioactivity<\/td>\n<\/tr>
radioactivity<\/td>\nEmanations of particles and radiation from atomic nuclei<\/td>\nRadioactivity<\/td>\n<\/tr>
Raoult's law<\/td>\nThe mathematical formula for calculating the vapor pressure of a solution<\/td>\nColligative Properties of Solutions<\/td>\n<\/tr>
rate constant (k<\/em>)<\/td>\nA proportionality constant specific to each reaction at a particular temperature<\/td>\nRate Laws<\/td>\n<\/tr>
rate-determining step<\/td>\nThe slowest step in a multistep mechanism<\/td>\nReaction Mechanisms<\/td>\n<\/tr>
rate law<\/td>\nA mathematical relationship between the reaction rate and the reactant concentrations<\/td>\nRate Laws<\/td>\n<\/tr>
reactant<\/td>\nAn initial substance in a chemical equation<\/td>\nThe Chemical Equation<\/td>\n<\/tr>
reaction mechanism<\/td>\nThe bond making and bond breaking steps which occur at the molecular level during a chemical reaction<\/td>\nReaction Mechanisms<\/td>\n<\/tr>
reaction order<\/td>\nThe sum of the concentration term exponents in a rate law equation<\/td>\nRate Laws<\/td>\n<\/tr>
reaction rate<\/td>\nThe speed of a chemical reaction<\/td>\nIntroduction to Kinetics<\/td>\n<\/tr>
real gases<\/td>\nA gas that deviates from ideal behaviour<\/td>\nReal Gases<\/td>\n<\/tr>
redox reaction<\/td>\nA chemical reaction that involves the transfer of electrons<\/td>\nOxidation-Reduction Reactions<\/td>\n<\/tr>
reduction<\/td>\nThe gain of one or more electrons by an atom; a decrease in oxidation number<\/td>\nOxidation-Reduction Reactions<\/td>\n<\/tr>
reduction<\/td>\nThe gain of one or more electrons by an atom; a decrease in oxidation number<\/td>\nOxidation-Reduction Reactions<\/td>\n<\/tr>
rem<\/td>\nA unit of radioactive exposure that includes a factor to account for the type of radioactivity<\/td>\nUnits of Radioactivity<\/td>\n<\/tr>
ribozyme<\/td>\nRibonucleic acid (RNA) molecules capable of catalyzing certain chemical reactions<\/td>\nCatalysis<\/td>\n<\/tr>
root-mean-square (rms) speed\u00a0(urms)<\/td>\nThe speed of molecules having exactly the same kinetic energy as the average kinetic energy of the sample<\/td>\nKinetic-Molecular Theory of Gases<\/td>\n<\/tr>
s block<\/td>\nThe columns of the periodic table in which\u00a0s\u00a0subshells are being occupied<\/td>\nElectronic Structure and the Periodic Table<\/td>\n<\/tr>
salt<\/td>\nAny ionic compound that is formed from a reaction between an acid and a base<\/td>\nNeutralization Reactions<\/td>\n<\/tr>
salt<\/td>\nAny ionic compound that is formed from a reaction between an acid and a base<\/td>\nArrhenius Acids and Bases<\/td>\n<\/tr>
salt bridge<\/td>\nA part of a voltaic cell that contains a solution of some ionic compound whose ions migrate to either side of the voltaic cell to maintain the charge balance<\/td>\nApplications of Redox Reactions: Voltaic Cells<\/td>\n<\/tr>
saturated hydrocarbons<\/td>\nA carbon compound with the maximum possible number of H atoms in its formula<\/td>\nHydrocarbons<\/td>\n<\/tr>
saturated solution<\/td>\nA solution with the maximum amount of solute dissolved in it<\/td>\nSome Definitions<\/td>\n<\/tr>
science<\/td>\nThe process of knowing about the natural universe through observation and experiment<\/td>\nChemistry as a Science<\/td>\n<\/tr>
scientific law<\/td>\nA specific statement that is thought to be never violated by the entire natural universe<\/td>\nChemistry as a Science<\/td>\n<\/tr>
scientific notation<\/td>\nAn expression of a number using powers of 10<\/td>\nExpressing Numbers<\/td>\n<\/tr>
screening<\/td>\nThe repelling valence electrons by core electrons<\/td>\nPeriodic Trends<\/td>\n<\/tr>
second law of thermodynamics<\/td>\nA spontaneous process will increase the entropy of the universe<\/td>\nEntropy and the Second Law of Thermodynamics<\/td>\n<\/tr>
secondary battery<\/td>\nA battery that can be recharged<\/td>\nApplications of Redox Reactions: Voltaic Cells<\/td>\n<\/tr>
semimetal<\/td>\nAn element that has properties of both metals and nonmetals<\/td>\nSome Basic Definitions<\/td>\n<\/tr>
semipermeable membrane<\/td>\nA thin membrane that will pass certain small molecules but not others<\/td>\nColligative Properties of Solutions<\/td>\n<\/tr>
SI unit<\/td>\n\u00a0International System of Units used by all scientists, literally translated from\u00a0\u201cle Syst\u00e8me International d\u2019unit\u00e9s.\u201d<\/td>\nExpressing Units<\/td>\n<\/tr>
Sievert (Sv)<\/td>\nSievert (Sv) is a related unit and is defined as 100 rem<\/td>\nUnits of Radioactivity<\/td>\n<\/tr>
sigma bond (\u03c3 bond)<\/td>\nOrbital overlap to form a bond which has cylindrical symmetry - a single bond<\/td>\nValence Bond Theory and Hybrid Orbitals<\/td>\n<\/tr>
significant figures<\/td>\nThe limit of the number of places a measurement can be properly expressed with<\/td>\nSignificant Figures<\/td>\n<\/tr>
silicones<\/td>\nA polymer based on a silicon and oxygen backbone<\/td>\nPolymers<\/td>\n<\/tr>
single bond<\/td>\nA covalent bond composed of one pair of electrons<\/td>\nCovalent Bonds<\/td>\n<\/tr>
single-replacement reaction<\/td>\nA chemical reaction in which one element is substituted for another element in a compound<\/td>\nTypes of Chemical Reactions: Single- and Double-Displacement Reactions<\/td>\n<\/tr>
solidification<\/td>\nThe process of a liquid becoming a solid<\/td>\nPhase Transitions: Melting, Boiling and Subliming<\/td>\n<\/tr>
solubility<\/td>\nThe maximum amount of a solute that can be dissolved in a given amount of a solvent<\/td>\nSome Definitions<\/td>\n<\/tr>
solubility rules<\/td>\nGeneral statements that predict which ionic compounds dissolve and which do not<\/td>\nTypes of Chemical Reactions: Single- and Double-Displacement Reactions<\/td>\n<\/tr>
solute<\/td>\nThe minor component of a solution<\/td>\nSome Definitions<\/td>\n<\/tr>
solution<\/td>\nSee homogeneous mixture<\/td>\nSome Basic Definitions<\/td>\n<\/tr>
solvent<\/td>\nThe major component of a solution<\/td>\nSome Definitions<\/td>\n<\/tr>
specific heat capacity<\/td>\nThe proportionality constant between heat, mass, and temperature change; also called specific heat<\/td>\nWork and Heat<\/td>\n<\/tr>
spectator ion<\/td>\nAn ion that does nothing in the overall course of a chemical reaction<\/td>\nIonic Equations: A Closer Look<\/td>\n<\/tr>
spin quantum number (ms)<\/td>\nThe index that indicates one of two spin states for an electron<\/td>\nQuantum Numbers for Electrons<\/td>\n<\/tr>
spontaneous process<\/td>\nA process that occurs without the influence of external forces or a change that moves a system towards equilibrium<\/td>\nSpontaneous Change<\/td>\n<\/tr>
standard molar entropy\u00a0 (So)<\/td>\nThe entropy of 1 mole of a substance in its standard state, at 1 atm of pressure<\/td>\nMeasuring Entropy and Entropy Changes<\/td>\n<\/tr>
standard notation<\/td>\nA straightforward expression of a number<\/td>\nExpressing Numbers<\/td>\n<\/tr>
standard temperature and pressure (STP)<\/td>\nA set of benchmark conditions used to compare other properties of gases; 100 kPa\u00a0for pressure and 273 K for temperature<\/td>\nThe Ideal Gas Law and Some Applications<\/td>\n<\/tr>
stoichiometry<\/td>\nThe relating of one chemical substance to another using a balanced chemical reaction<\/td>\nStoichiometry<\/td>\n<\/tr>
strong acid<\/td>\nAny acid that is 100% dissociated into ions in aqueous solution<\/td>\nStrong and Weak Acids and Bases and Their Salts<\/td>\n<\/tr>
strong base<\/td>\nAny base that is 100% dissociated into ions in aqueous solution<\/td>\nStrong and Weak Acids and Bases and Their Salts<\/td>\n<\/tr>
sublimation<\/td>\nThe process of a solid becoming a gas<\/td>\nPhase Transitions: Melting, Boiling and Subliming<\/td>\n<\/tr>
subshell<\/td>\nA term used to describe electrons in a shell that have the same angular momentum quantum number<\/td>\nQuantum Numbers for Electrons<\/td>\n<\/tr>
substance<\/td>\nMatter that has the same physical and chemical properties throughout.<\/td>\nSome Basic Definitions<\/td>\n<\/tr>
substituent<\/td>\nA branch off a main chain in a hydrocarbon<\/td>\nBranched Hydrocarbons<\/td>\n<\/tr>
substrate<\/td>\nThe reactants which are specific for a biological catalyst<\/td>\nCatalysis<\/td>\n<\/tr>
supercritical fluid<\/td>\nA phase beyond the critical point, where liquid and gas phases are no longer distinct<\/td>\nProperties of Liquids<\/td>\n<\/tr>
supersaturated solution<\/td>\nA unstable solution with more than the normal maximum amount of solute in it<\/td>\nSome Definitions<\/td>\n<\/tr>
surface tension<\/td>\nAn effect caused by an imbalance of forces on the atoms at the surface of a liquid<\/td>\nProperties of Liquids<\/td>\n<\/tr>
surrounding atoms<\/td>\nAn atom that makes covalent bonds to the central atom(s)<\/td>\nCovalent Bonds<\/td>\n<\/tr>
system<\/td>\nThe part of the universe under study<\/td>\nEnergy<\/td>\n<\/tr>
temperature<\/td>\nA measure of the average amount of kinetic energy a system contains<\/td>\nOther Units: Temperature and Density<\/td>\n<\/tr>
theoretical yield<\/td>\nAn amount that is theoretically produced as calculated using the balanced chemical reaction<\/td>\nYields<\/td>\n<\/tr>
theory<\/td>\nA general statement that explains a large number of observations<\/td>\nChemistry as a Science<\/td>\n<\/tr>
thermochemical equation<\/td>\nA chemical equation that includes an enthalpy change<\/td>\nEnthalpy and Chemical Reactions<\/td>\n<\/tr>
thiol<\/td>\nThe sulfur analog of an alcohol<\/td>\nOther Functional Groups<\/td>\n<\/tr>
third law of thermodynamics<\/td>\nAt absolute zero the entropy of a pure, perfect crystal is zero<\/td>\nMeasuring Entropy and Entropy Changes<\/td>\n<\/tr>
titrant<\/td>\nThe reagent of known concentration<\/td>\nAcid-Base Titrations<\/td>\n<\/tr>
titration<\/td>\nA chemical reaction performed quantitatively to determine the exact amount of a reagent<\/td>\nAcid-Base Titrations<\/td>\n<\/tr>
torr<\/td>\nAnother name for a millimeter of mercury<\/td>\nPressure<\/td>\n<\/tr>
tracer<\/td>\nA substance that can be used to follow the pathway of that substance through a structure<\/td>\nUses of Radioactive Isotopes<\/td>\n<\/tr>
transition state<\/td>\nThe highest energy transitional point in the elementary step<\/td>\nReaction Mechanisms<\/td>\n<\/tr>
triple bond<\/td>\nA covalent bond composed of three pairs of bonding electrons<\/td>\nCovalent Bonds<\/td>\n<\/tr>
unsaturated hydrocarbons<\/td>\nA carbon compound with less than the maximum possible number of H atoms in its formula<\/td>\nHydrocarbons<\/td>\n<\/tr>
unsaturated solution<\/td>\nA solution with less than the maximum amount of solute dissolved in it<\/td>\nSome Definitions<\/td>\n<\/tr>
valence electrons<\/td>\nThe electrons in the highest-numbered shell, plus any electrons in the last unfilled subshell. The electrons most likely involved in chemical reactions<\/td>\nElectronic Structure and the Periodic Table<\/td>\n<\/tr>
valence shell<\/td>\nThe highest-numbered shell in an atom that contains electrons<\/td>\nElectronic Structure and the Periodic Table<\/td>\n<\/tr>
valence shell electron pair repulsion theory (VSEPR)<\/td>\nThe general concept that estimates the shape of a simple molecule:\u00a0 electron pairs repel each other to get as far away from each other as possible<\/td>\nMolecular Shapes and Polarity<\/td>\n<\/tr>
van der Waal's equation<\/td>\nAn equation which compensates for deviations from ideal gas behaviour, correcting for intermolecular forces and the volume of gas molecules<\/td>\nReal Gases<\/td>\n<\/tr>
van\u2019t Hoff factor\u00a0(i)<\/td>\nThe number of particles each solute formula unit breaks apart into when it dissolves<\/td>\nColligative Properties of Ionic Solutes<\/td>\n<\/tr>
vapor<\/td>\nMaterial in the gas phase due to evaporation<\/td>\nProperties of Liquids<\/td>\n<\/tr>
vapor pressure<\/td>\nThe partial pressure exerted by evaporation of a liquid<\/td>\nGas Mixtures<\/td>\n<\/tr>
vapor pressure depression<\/td>\nThe decrease of a solution\u2019s vapor pressure because of the presence of a solute<\/td>\nColligative Properties of Solutions<\/td>\n<\/tr>
vector quantity<\/td>\nA quantity which has both a magnitude and direction<\/td>\nMolecular Shapes and Polarity<\/td>\n<\/tr>
voltaic (galvanic) cell<\/td>\nAn apparatus that allows for useful electrical work to be extracted from a redox reaction.<\/td>\nApplications of Redox Reactions: Voltaic Cells<\/td>\n<\/tr>
wavelength<\/td>\nThe distance between corresponding points in two adjacent light cycles<\/td>\nLight<\/td>\n<\/tr>
weak acid<\/td>\nAny acid that is less than 100% dissociated into ions in aqueous solution<\/td>\nStrong and Weak Acids and Bases and Their Salts<\/td>\n<\/tr>
weak base<\/td>\nAny base that is less than 100% dissociated into ions in aqueous solution<\/td>\nStrong and Weak Acids and Bases and Their Salts<\/td>\n<\/tr><\/tbody><\/table>","rendered":"\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n
Term<\/td>\nDefinition<\/td>\nSection of Book<\/td>\n<\/tr>\n
abbreviated electron configuration<\/td>\nAn electron configuration that uses one of the noble gases to represent the core of electrons up to that element<\/td>\nOrganization of Electrons in Atoms<\/td>\n<\/tr>\n
absolute zero<\/td>\nThe minimum possible temperature, labeled 0 K (zero kelvins)<\/td>\nOther Units: Temperature and Density<\/td>\n<\/tr>\n
acid<\/td>\nAn ionic compound of the\u00a0H+\u00a0cation dissolved in water<\/td>\nAcids<\/td>\n<\/tr>\n
acid<\/td>\nA compound that increases the amount of\u00a0H+\u00a0ions in an aqueous solution<\/td>\nNeutralization Reactions<\/td>\n<\/tr>\n
acid dissociation constant (K<\/em>a<\/sub>)<\/td>\nThe equilibrium constant for the dissociation of a weak acid into ions<\/td>\nSome Special Types of Equilibria<\/td>\n<\/tr>\n
acid salt<\/td>\nAn ionic compound whose aqueous solution is slightly acidic<\/td>\nStrong and Weak Acids and Bases and Their Salts<\/td>\n<\/tr>\n
activated complex<\/td>\nSee transition state<\/td>\nReaction Mechanisms<\/td>\n<\/tr>\n
activation energy (Ea)<\/td>\nThe minimum amount of kinetic energy molecules must possess for an effective collision to occur<\/td>\nFactors that Affect the Rate of Reactions<\/td>\n<\/tr>\n
active site<\/td>\nArea of enzymatic action where substrate molecules react<\/td>\nCatalysis<\/td>\n<\/tr>\n
activity series<\/td>\nA list of elements that will replace elements below them in single-replacement reactions<\/td>\nTypes of Chemical Reactions: Single- and Double-Displacement Reactions<\/td>\n<\/tr>\n
actual yield<\/td>\nThe amount that is actually produced in a chemical reaction<\/td>\nYields<\/td>\n<\/tr>\n
addition reaction<\/td>\nA reaction where atoms are added across a double or triple bond<\/td>\nHydrocarbons<\/td>\n<\/tr>\n
adhesion<\/td>\nThe tendency of a substance to interact with other substances because of intermolecular forces<\/td>\nProperties of Liquids<\/td>\n<\/tr>\n
adsorb<\/td>\nBind\u00a0to the surface of another substance<\/td>\nCatalysis<\/td>\n<\/tr>\n
alcohol<\/td>\nAn organic compound that contains an OH functional group<\/td>\nAlkyl halides and alcohols<\/td>\n<\/tr>\n
aldehyde<\/td>\nA compound that has a carbonyl functional group at the end of a chain of C atoms<\/td>\nOther Oxygen-Containing Functional Groups<\/td>\n<\/tr>\n
aliphatic hydrocarbons<\/td>\nA hydrocarbon based on chains of C atoms<\/td>\nHydrocarbons<\/td>\n<\/tr>\n
alkaline battery<\/td>\nA type of dry cell that contains an alkaline (i.e., basic) moist paste, rather than an acidic paste<\/td>\nApplications of Redox Reactions: Voltaic Cells<\/td>\n<\/tr>\n
alkane<\/td>\nAn aliphatic hydrocarbon with only single covalent bonds<\/td>\nHydrocarbons<\/td>\n<\/tr>\n
alkene<\/td>\nAn aliphatic hydrocarbon that contains a C\u2013C double bond<\/td>\nHydrocarbons<\/td>\n<\/tr>\n
alkyl halide<\/td>\nAn organic compound that contains a halogen atom<\/td>\nAlkyl halides and alcohols<\/td>\n<\/tr>\n
alkyne<\/td>\nAn aliphatic hydrocarbon that contains a C\u2013C triple bond<\/td>\nHydrocarbons<\/td>\n<\/tr>\n
alpha particle<\/td>\nA type of radioactive emission equivalent to a helium nucleus<\/td>\nRadioactivity<\/td>\n<\/tr>\n
amide group<\/td>\nA functional group that is the combination of the amine and carbonyl functional groups<\/td>\nOther Functional Groups<\/td>\n<\/tr>\n
amide bond<\/td>\nThe bond between the N atom and the C atom in an amide.<\/td>\nOther Functional Groups<\/td>\n<\/tr>\n
amine<\/td>\nAn organic derivative of ammonia<\/td>\nOther Functional Groups<\/td>\n<\/tr>\n
amorphous solid<\/td>\nA solid with no long-term structure or repetition<\/td>\nSolids<\/td>\n<\/tr>\n
amphiprotic<\/td>\nA substance that can act as a proton donor or a proton acceptor<\/td>\nBr\u00f8nsted-Lowry Acids and Bases<\/td>\n<\/tr>\n
analyte<\/td>\nThe reagent of unknown concentration<\/td>\nAcid-Base Titrations<\/td>\n<\/tr>\n
angular momentum quantum number (\u2113)<\/td>\nAn index that affects the energy and the spatial distribution of an electron in an atom<\/td>\nQuantum Numbers for Electrons<\/td>\n<\/tr>\n
anion<\/td>\nA species with an overall negative charge<\/td>\nIons and Ionic Compounds<\/td>\n<\/tr>\n
anode<\/td>\nThe half cell that contains the oxidation reaction<\/td>\nApplications of Redox Reactions: Voltaic Cells<\/td>\n<\/tr>\n
antibonding molecular orbital<\/td>\nA higher energy molecular orbital generated by destructive combination of atomic orbitals<\/td>\nMolecular Orbitals<\/td>\n<\/tr>\n
aromatic hydrocarbons<\/td>\nFlat ring systems, which contain continuously overlapping\u00a0p\u00a0orbitals, such as benzene<\/td>\nHydrocarbons<\/td>\n<\/tr>\n
Arrhenius acid<\/td>\nA compound that increases the hydrogen ion concentration in aqueous solution<\/td>\nArrhenius Acids and Bases<\/td>\n<\/tr>\n
Arrhenius base<\/td>\nA compound that increases the hydroxide ion concentration in aqueous solution<\/td>\nArrhenius Acids and Bases<\/td>\n<\/tr>\n
atmosphere (atm)<\/td>\nA unit of pressure equal to the average atmospheric pressure at sea level; defined as exactly 760 mmHg<\/td>\nPressure<\/td>\n<\/tr>\n
atom<\/td>\nThe smallest piece of an element that maintains the identity of that element<\/td>\nAtomic Theory<\/td>\n<\/tr>\n
atomic mass<\/td>\nThe sum of the number of protons and neutrons in a nucleus<\/td>\nAtomic Theory<\/td>\n<\/tr>\n
atomic mass<\/td>\nThe weighted average of the masses of the isotopes that compose an element<\/td>\nMasses of Atoms and Molecules<\/td>\n<\/tr>\n
atomic mass unit<\/td>\nOne-twelfth of the mass of a carbon-12 atom<\/td>\nMasses of Atoms and Molecules<\/td>\n<\/tr>\n
atomic number<\/td>\nThe number of protons in an atom<\/td>\nAtomic Theory<\/td>\n<\/tr>\n
atomic radius<\/td>\nAn indication of the size of an atom<\/td>\nPeriodic Trends<\/td>\n<\/tr>\n
atomic symbol<\/td>\nA one- or two-letter representation of the name of an element<\/td>\nAtomic Theory<\/td>\n<\/tr>\n
atomic theory<\/td>\nThe concept that atoms play a fundamental role in chemistry<\/td>\nAtomic Theory<\/td>\n<\/tr>\n
aufbau principle<\/td>\n(German for \u201cbuilding up\u201d): \u00a0electrons fill the lowest energy orbitals first.<\/td>\nOrganization of Electrons in Atoms<\/td>\n<\/tr>\n
autoionization constant of water (K<\/em>w<\/sub>)<\/td>\nThe product of the hydrogen ion and hydroxide ion concentrations<\/td>\nAutoionization of Water<\/td>\n<\/tr>\n
autoionization of water<\/td>\nWater molecules act as acids (proton donors) and bases (proton acceptors) with each other to a tiny extent in all aqueous solutions<\/td>\nAutoionization of Water<\/td>\n<\/tr>\n
Avogadro’s law<\/td>\nA gas law that relates number of particles to volume<\/td>\nOther Gas Laws<\/td>\n<\/tr>\n
balanced chemical equation<\/td>\nA condition when the reactants and products of a chemical equation have the same number of atoms of all elements present<\/td>\nThe Chemical Equation<\/td>\n<\/tr>\n
base<\/td>\nA compound that increases the amount of\u00a0OH\u2212\u00a0ions in an aqueous solution<\/td>\nNeutralization Reactions<\/td>\n<\/tr>\n
basic salt<\/td>\nAn ionic compound whose aqueous solution is slightly basic<\/td>\nStrong and Weak Acids and Bases and Their Salts<\/td>\n<\/tr>\n
becquerel (Bq)<\/td>\nA unit of radioactivity equal to 1 decay per second<\/td>\nUnits of Radioactivity<\/td>\n<\/tr>\n
beta particle<\/td>\nA type of radioactive emission equivalent to an electron<\/td>\nRadioactivity<\/td>\n<\/tr>\n
boiling (or vaporization)<\/td>\nThe process of a liquid becoming a gas<\/td>\nPhase Transitions: Melting, Boiling and Subliming<\/td>\n<\/tr>\n
boiling point<\/td>\nThe characteristic temperature at which a liquid becomes a gas<\/td>\nPhase Transitions: Melting, Boiling and Subliming<\/td>\n<\/tr>\n
boiling point elevation<\/td>\nThe increase of a solution\u2019s boiling point because of the presence of solute<\/td>\nColligative Properties of Solutions<\/td>\n<\/tr>\n
boiling point elevation constant (K<\/em>b<\/sub>)<\/td>\nThe constant that relates the molality concentration of a solution and its boiling point change<\/td>\nColligative Properties of Solutions<\/td>\n<\/tr>\n
bond energy<\/td>\nThe approximate amount of energy needed to break a covalent bond<\/td>\nOther Aspects of Covalent Bonding<\/td>\n<\/tr>\n
bond order<\/td>\nA method of evaluating bond strength<\/td>\nMolecular Orbitals<\/td>\n<\/tr>\n
bonding electron pair<\/td>\nA pair of electrons that makes a covalent bond<\/td>\nCovalent Bonds<\/td>\n<\/tr>\n
bonding molecular orbital<\/td>\nThe lower energy molecular orbital generated by constructive combination of atomic orbitals<\/td>\nMolecular Orbitals<\/td>\n<\/tr>\n
Boyle’s law<\/td>\nA gas law that relates pressure and volume at constant temperature and amount<\/td>\nGas Laws<\/td>\n<\/tr>\n
branched hydrocarbons<\/td>\nA carbon compound that is not a straight chain, having substituents appended to the longest chain<\/td>\nBranched Hydrocarbons<\/td>\n<\/tr>\n
Br\u00f8nsted-Lowry acid<\/td>\nAny species that can donate a proton to another molecule<\/td>\nBr\u00f8nsted-Lowry Acids and Bases<\/td>\n<\/tr>\n
Br\u00f8nsted-Lowry base<\/td>\nAny species that can accept a proton from another molecule<\/td>\nBr\u00f8nsted-Lowry Acids and Bases<\/td>\n<\/tr>\n
buffer<\/td>\nA solution that resists dramatic changes in pH<\/td>\nBuffers<\/td>\n<\/tr>\n
buffer capacity<\/td>\nThe amount of strong acid or base a buffer can counteract<\/td>\nBuffers<\/td>\n<\/tr>\n
burette or buret<\/td>\nA precisely calibrated volumetric delivery tube<\/td>\nAcid-Base Titrations<\/td>\n<\/tr>\n
calorie<\/td>\nA unit of energy measurement originally defined in terms of warming up a given quantity of water. 1 cal = 4.184 J<\/td>\nEnergy<\/td>\n<\/tr>\n
calorimeter<\/td>\nA container used to measure the heat of a chemical reaction<\/td>\nEnthalpy and Chemical Reactions<\/td>\n<\/tr>\n
calorimetry<\/td>\nThe process of measuring enthalpy changes for chemical reactions<\/td>\nEnthalpy and Chemical Reactions<\/td>\n<\/tr>\n
capillary action<\/td>\nThe behavior of a liquid in narrow surfaces due to differences in adhesion and cohesion<\/td>\nProperties of Liquids<\/td>\n<\/tr>\n
carbonyl group<\/td>\nA functional group where an O atom and a C atom are joined with a double bond<\/td>\nOther Oxygen-Containing Functional Groups<\/td>\n<\/tr>\n
carboxyl group<\/td>\nA functional group composed of a carbonyl group and an OH group<\/td>\nOther Oxygen-Containing Functional Groups<\/td>\n<\/tr>\n
carboxylate ion<\/td>\nA negatively charged ion derived from a carboxylic acid<\/td>\nOther Oxygen-Containing Functional Groups<\/td>\n<\/tr>\n
carboxylic acid<\/td>\nA molecule with a carboxyl group<\/td>\nOther Oxygen-Containing Functional Groups<\/td>\n<\/tr>\n
catalyst<\/td>\nA substance that increases the speed of a reaction<\/td>\nShifting Equilibria: Le Chatelier\u2019s Principle<\/td>\n<\/tr>\n
catalyst<\/td>\nA substance thaty accelerates a reaction by participating in it without being consumed<\/td>\nFactors that Affect the Rate of Reactions<\/td>\n<\/tr>\n
catalyst<\/td>\nA substance that lowers the activation energy of a specific reaction by providing an alternate reaction pathway<\/td>\nCatalysis<\/td>\n<\/tr>\n
cathode<\/td>\nThe half cell that contains the reduction reaction<\/td>\nApplications of Redox Reactions: Voltaic Cells<\/td>\n<\/tr>\n
cation<\/td>\nA species with an overall positive charge<\/td>\nIons and Ionic Compounds<\/td>\n<\/tr>\n
central atom<\/td>\nThe atom in the center of a molecule<\/td>\nCovalent Bonds<\/td>\n<\/tr>\n
Charles’s law<\/td>\nA gas law that relates volume and temperature at constant pressure and amount<\/td>\nGas Laws<\/td>\n<\/tr>\n
chemical bond<\/td>\nThe connection between two atoms in a molecule<\/td>\nMolecules an Chemical Nomenclature<\/td>\n<\/tr>\n
chemical change<\/td>\nThe process of demonstrating a chemical property<\/td>\nSome Basic Definitions<\/td>\n<\/tr>\n
chemical equation<\/td>\nA concise way of representing a chemical reaction<\/td>\nThe Chemical Equation<\/td>\n<\/tr>\n
chemical equilibrium<\/td>\nThe point at which forward and reverse chemical reactions balance each other\u2019s progress<\/td>\nChemical Equilibrium<\/td>\n<\/tr>\n
chemical nomenclature<\/td>\nA very specific system for naming compounds, in which unique substances get unique names<\/td>\nMolecules an Chemical Nomenclature<\/td>\n<\/tr>\n
chemical property<\/td>\nA characteristic that describes how matter changes form in the presence of other matter<\/td>\nSome Basic Definitions<\/td>\n<\/tr>\n
chemistry<\/td>\nThe study of the interactions of matter with other matter and with energy<\/td>\nIntroduction<\/td>\n<\/tr>\n
coefficient<\/td>\nThe part of a number in scientific notation that is multiplied by a power of 10<\/td>\nExpressing Numbers<\/td>\n<\/tr>\n
coefficient<\/td>\nA number in a chemical equation indicating more than one molecule of the substance<\/td>\nThe Chemical Equation<\/td>\n<\/tr>\n
cohesion<\/td>\nThe tendency of a substance to interact with itself<\/td>\nProperties of Liquids<\/td>\n<\/tr>\n
colligative property<\/td>\nA property of solutions related to the fraction that the solute particles occupy in the solution, not their identity<\/td>\nColligative Properties of Solutions<\/td>\n<\/tr>\n
collision theory<\/td>\nThe theory that reactions occur when reactant molecules \u201ceffectively collide\u201d<\/td>\nFactors that Affect the Rate of Reactions<\/td>\n<\/tr>\n
combined gas law<\/td>\nA gas law that combines pressure, volume, and temperature<\/td>\nOther Gas Laws<\/td>\n<\/tr>\n
combustion reaction<\/td>\nA chemical reaction in which a reactant combines with oxygen to produce oxides of all other elements as products<\/td>\nComposition, Decomposition, and Combustion Reactions<\/td>\n<\/tr>\n
complete ionic equation<\/td>\nA chemical equation in which the dissolved ionic compounds are written as separated ions<\/td>\nIonic Equations: A Closer Look<\/td>\n<\/tr>\n
composition reaction<\/td>\nA chemical reaction in which a single substance is produced from multiple reactants<\/td>\nComposition, Decomposition, and Combustion Reactions<\/td>\n<\/tr>\n
compound<\/td>\nA combination of more than one element<\/td>\nSome Basic Definitions<\/td>\n<\/tr>\n
compressibility factor<\/td>\nA measure of the extent of deviation from ideal gas behaviour<\/td>\nReal Gases<\/td>\n<\/tr>\n
concentrated solution<\/td>\nA solution with a lot of solute<\/td>\nSome Definitions<\/td>\n<\/tr>\n
concentration<\/td>\nHow much solute is dissolved in a given amount of solvent<\/td>\nSome Definitions<\/td>\n<\/tr>\n
concentration (verb)<\/td>\nThe removal of solvent, which increases the concentration of the solute in the solution<\/td>\nDilutions and Concentrations<\/td>\n<\/tr>\n
condensation<\/td>\nThe process of a gas becoming a liquid<\/td>\nPhase Transitions: Melting, Boiling and Subliming<\/td>\n<\/tr>\n
condensed structure<\/td>\nA listing of the atoms bonded to each C atom in a chain<\/td>\nHydrocarbons<\/td>\n<\/tr>\n
conjugate acid-base pair<\/td>\nTwo species whose formulas differ by only a hydrogen ion<\/td>\nBr\u00f8nsted-Lowry Acids and Bases<\/td>\n<\/tr>\n
continuous spectrum<\/td>\nAn image that contains all colors of light<\/td>\nQuantum Numbers for Electrons<\/td>\n<\/tr>\n
conversion factor<\/td>\nA fraction that can be used to convert a quantity from one unit to another<\/td>\nConverting Units<\/td>\n<\/tr>\n
covalent bond<\/td>\nA chemical bond formed by two atoms sharing electrons<\/td>\nCovalent Bonds<\/td>\n<\/tr>\n
covalent network solids<\/td>\nA crystalline solid composed of atoms of one or more elements that are covalently bonded together in a seemingly never-ending fashion<\/td>\nSolids<\/td>\n<\/tr>\n
critical point<\/td>\nThe point at the highest temperature and pressure at which liquids and gases remain distinguishable<\/td>\nProperties of Liquids<\/td>\n<\/tr>\n
crystalline solid<\/td>\nA solid with a regular, repeating three-dimensional structure<\/td>\nSolids<\/td>\n<\/tr>\n
curie<\/td>\nA unit of radioactivity equal to\u00a03.7\u00d71010\u00a0decays\/s<\/td>\nUnits of Radioactivity<\/td>\n<\/tr>\n
d<\/em> block<\/td>\nThe columns of the periodic table in which\u00a0d<\/em>\u00a0subshells are being occupied<\/td>\nElectronic Structure and the Periodic Table<\/td>\n<\/tr>\n
Dalton’s law of partial pressures<\/td>\nThe total pressure of a gas mixture,\u00a0Ptot, is equal to the sum of the partial pressures of the components,\u00a0Pi<\/td>\nGas Mixtures<\/td>\n<\/tr>\n
daughter isotope<\/td>\nThe product left over from the parent isotope in a nuclear equation<\/td>\nRadioactivity<\/td>\n<\/tr>\n
decomposition reaction<\/td>\nA chemical reaction in which a single substance becomes more than one substance<\/td>\nComposition, Decomposition, and Combustion Reactions<\/td>\n<\/tr>\n
degrees<\/td>\nThe unit of temperature scales<\/td>\nOther Units: Temperature and Density<\/td>\n<\/tr>\n
density<\/td>\nA physical property defined as a substance\u2019s mass divided by its volume<\/td>\nOther Units: Temperature and Density<\/td>\n<\/tr>\n
deposition<\/td>\nThe process of a gas becoming a solid<\/td>\nPhase Transitions: Melting, Boiling and Subliming<\/td>\n<\/tr>\n
derived unit<\/td>\nA unit that is a product or a quotient of a fundamental unit<\/td>\nExpressing Units<\/td>\n<\/tr>\n
diatomic molecule<\/td>\nA molecule with only two atoms<\/td>\nMolecules an Chemical Nomenclature<\/td>\n<\/tr>\n
diffusion<\/td>\nThe movement of gas molecules through one or more additional types of gas via random molecular motion<\/td>\nMolecular Effusion and Diffusion<\/td>\n<\/tr>\n
dilute<\/td>\nA solution with very little solute<\/td>\nSome Definitions<\/td>\n<\/tr>\n
dilution<\/td>\nThe addition of solvent, which decreases the concentration of the solute in the solution<\/td>\nDilutions and Concentrations<\/td>\n<\/tr>\n
dilution equation<\/td>\nThe mathematical formula for calculating new concentrations or volumes when a solution is diluted or concentrated<\/td>\nDilutions and Concentrations<\/td>\n<\/tr>\n
dipole-dipole interactions<\/td>\nAn intermolecular force caused by molecules with a permanent dipole<\/td>\nIntermolecular Forces<\/td>\n<\/tr>\n
dispersion force (or London dispersion force)<\/td>\nAn intermolecular force caused by the instantaneous position of an electron in a molecule<\/td>\nIntermolecular Forces<\/td>\n<\/tr>\n
dissociation<\/td>\nThe process of an ionic compound separating into ions when it dissolves<\/td>\nIonic Equations: A Closer Look<\/td>\n<\/tr>\n
double bond<\/td>\nA covalent bond composed of two pairs of bonding electrons<\/td>\nCovalent Bonds<\/td>\n<\/tr>\n
double-replacement reaction<\/td>\nA chemical reaction in which parts of two ionic compounds are exchanged<\/td>\nTypes of Chemical Reactions: Single- and Double-Displacement Reactions<\/td>\n<\/tr>\n
dry cell<\/td>\nA modern battery that does not contain large amounts of aqueous solution<\/td>\nApplications of Redox Reactions: Voltaic Cells<\/td>\n<\/tr>\n
dynamic equilibrium<\/td>\nWhen a process still occurs but the opposite process also occurs at the same rate so that there is no net change in the system.<\/td>\nProperties of Liquids<\/td>\n<\/tr>\n
effective nuclear charge (Zeff)<\/td>\nThe net nuclear charge feld by valence electrons<\/td>\nPeriodic Trends<\/td>\n<\/tr>\n
effusion<\/td>\nThe movement of gas molecules from one container to another via a tiny hole<\/td>\nMolecular Effusion and Diffusion<\/td>\n<\/tr>\n
electrodes<\/td>\nThe cathode or anode of a voltaic cell<\/td>\nApplications of Redox Reactions: Voltaic Cells<\/td>\n<\/tr>\n
electrolysis<\/td>\nThe process of making a nonspontaneous redox reaction occur by forcing electricity into a cell<\/td>\nElectrolysis<\/td>\n<\/tr>\n
electrolytic cell<\/td>\nA cell into which electricity is forced to make a nonspontaneous reaction occur<\/td>\nElectrolysis<\/td>\n<\/tr>\n
electromagnetic spectrum<\/td>\nThe full span of the possible wavelengths, frequencies, and energies of light<\/td>\nLight<\/td>\n<\/tr>\n
electron<\/td>\nA tiny subatomic particle with a negative charge<\/td>\nAtomic Theory<\/td>\n<\/tr>\n
electron affinity (EA)<\/td>\nThe energy change when a gas-phase atom accepts an electron<\/td>\nPeriodic Trends<\/td>\n<\/tr>\n
electron configuration<\/td>\nA listing of the shell and subshells labels<\/td>\nOrganization of Electrons in Atoms<\/td>\n<\/tr>\n
electron deficient molecules<\/td>\nA molecule with less than eight electrons in the valence shell of an atom<\/td>\nViolations of the Octet Rule<\/td>\n<\/tr>\n
electron group geometry<\/td>\nhow electron groups (bonds and nonbonding electron pairs) are arranged<\/td>\nMolecular Shapes and Polarity<\/td>\n<\/tr>\n
electron groups<\/td>\nA covalent bond of any type or a lone electron pair<\/td>\nMolecular Shapes and Polarity<\/td>\n<\/tr>\n
electron shell<\/td>\nA term used to describe electrons with the same principal quantum number<\/td>\nQuantum Numbers for Electrons<\/td>\n<\/tr>\n
electronegativity<\/td>\nA\u00a0scale for judging how much atoms of any element attract electrons<\/td>\nOther Aspects of Covalent Bonding<\/td>\n<\/tr>\n
electroplating<\/td>\nThe deposition of a thin layer of metal on an object for protective or decorative purposes<\/td>\nElectrolysis<\/td>\n<\/tr>\n
element<\/td>\nA substance that cannot be broken down into simpler chemical substances by ordinary chemical means<\/td>\nSome Basic Definitions<\/td>\n<\/tr>\n
elementary step<\/td>\nEach event that occurs in a chemical reaction as a result of an effective collision<\/td>\nReaction Mechanisms<\/td>\n<\/tr>\n
elimination reaction<\/td>\nThe removal of a functional group (either X or OH) and a H atom from an adjacent carbon<\/td>\nAlkyl halides and alcohols<\/td>\n<\/tr>\n
endothermic<\/td>\nA chemical reaction that has a positive change in enthalpy<\/td>\nEnthalpy and Chemical Reactions<\/td>\n<\/tr>\n
energy<\/td>\nThe ability to do work.\u00a0is the ability to do work<\/td>\nEnergy<\/td>\n<\/tr>\n
enthalpy change<\/td>\nThe heat of a process at constant pressure; denoted\u00a0\u0394H<\/td>\nEnthalpy and Chemical Reactions<\/td>\n<\/tr>\n
enthalpy of formation<\/td>\nThe enthalpy change for a formation reaction; denoted\u00a0\u0394Hf.\u00a0and is given the symbol \u0394Hf<\/td>\nFormation Reactions<\/td>\n<\/tr>\n
enthalpy of fusion<\/td>\nThe amount of energy needed to change from a solid to a liquid or from a liquid to a solid<\/td>\nPhase Transitions: Melting, Boiling and Subliming<\/td>\n<\/tr>\n
enthalpy of sublimation<\/td>\nThe amount of energy needed to change from a solid to a gas or from a gas to a solid<\/td>\nPhase Transitions: Melting, Boiling and Subliming<\/td>\n<\/tr>\n
enthalpy of vaporization<\/td>\nThe amount of energy needed to change from a liquid to a gas or from a gas to a liquid<\/td>\nPhase Transitions: Melting, Boiling and Subliming<\/td>\n<\/tr>\n
entropy<\/td>\nThe level of randomness (or disorder) of a system, or a measure of the energy dispersal of the molecules in the system<\/td>\nEntropy and the Second Law of Thermodynamics<\/td>\n<\/tr>\n
enzyme<\/td>\nProtein molecules which serve to catalyze biochemical reactions<\/td>\nCatalysis<\/td>\n<\/tr>\n
enzyme-substrate complex<\/td>\nThe binding of substrate to the enzymatic active site<\/td>\nCatalysis<\/td>\n<\/tr>\n
equilibrium constant (Keq)<\/td>\nA numerical value that relates to the ratio of products and reactants at equilibrium<\/td>\nThe Equilibrium Constant<\/td>\n<\/tr>\n
equivalence point<\/td>\nThe point of the reaction when all the analyte has been reacted with the titrant<\/td>\nAcid-Base Titrations<\/td>\n<\/tr>\n
ester group<\/td>\nA functional group made by combining a carboxylic acid with an alcohol<\/td>\nOther Oxygen-Containing Functional Groups<\/td>\n<\/tr>\n
ether group<\/td>\nA functional group that has an O atom attached to two organic groups<\/td>\nOther Oxygen-Containing Functional Groups<\/td>\n<\/tr>\n
evaporation<\/td>\nThe formation of a gas phase from a liquid at temperatures below the boiling point<\/td>\nProperties of Liquids<\/td>\n<\/tr>\n
exact number<\/td>\nA number from a defined relationship that technically has an infinite number of significant figures<\/td>\nConverting Units<\/td>\n<\/tr>\n
exothermic<\/td>\nA chemical reaction that has a negative change in enthalpy<\/td>\nEnthalpy and Chemical Reactions<\/td>\n<\/tr>\n
expanded valence shell molecules<\/td>\nA molecule with more than eight electrons in the valence shell of an atom<\/td>\nViolations of the Octet Rule<\/td>\n<\/tr>\n
experiment<\/td>\nA test of the natural universe to see if a guess (hypothesis) is correct<\/td>\nChemistry as a Science<\/td>\n<\/tr>\n
exponent<\/td>\nThe raised number to the right of a 10 indicating the number of factors of 10 in the original number<\/td>\nExpressing Numbers<\/td>\n<\/tr>\n
f<\/em> block<\/td>\nThe columns of the periodic table in which\u00a0f<\/em>\u00a0subshells are being occupied<\/td>\nElectronic Structure and the Periodic Table<\/td>\n<\/tr>\n
fission<\/td>\nThe breaking apart of an atomic nucleus into smaller nuclei<\/td>\nRadioactivity<\/td>\n<\/tr>\n
formation reaction<\/td>\nA chemical reaction that forms one mole of a substance from its constituent elements in their standard states<\/td>\nFormation Reactions<\/td>\n<\/tr>\n
freezing point depression<\/td>\nThe decrease of a solution\u2019s freezing point because of the presence of solute<\/td>\nColligative Properties of Solutions<\/td>\n<\/tr>\n
freezing point depression constant (Kf)<\/td>\nThe constant that relates the molality concentration of a solution and its freezing point change<\/td>\nColligative Properties of Solutions<\/td>\n<\/tr>\n
frequency<\/td>\nThe number of cycles of light that pass a given point in one second<\/td>\nLight<\/td>\n<\/tr>\n
frequency factor (A<\/em>)<\/td>\nA factor that takes into account the frequency of reactions and the likelihood of correct molecular orientation<\/td>\nActivation Energy and the Arrhenius Equation<\/td>\n<\/tr>\n
frontier molecular orbitals<\/td>\nA term which refers to the HOMO and LUMO, the most likely orbitals to be involved in chemical reactions or processes<\/td>\nMolecular Orbitals<\/td>\n<\/tr>\n
functional group<\/td>\nA collection of atoms or bonds with certain characteristic reactions<\/td>\nAlkyl halides and alcohols<\/td>\n<\/tr>\n
fundamental units<\/td>\nOne of the seven basic units of SI used in science<\/td>\nExpressing Units<\/td>\n<\/tr>\n
gamma ray<\/td>\nA type of radioactive emission that is a very energetic form of electromagnetic radiation<\/td>\nRadioactivity<\/td>\n<\/tr>\n
gas law<\/td>\nA simple mathematical formula that allows one to model, or predict, the behavior of a gas<\/td>\nGas Laws<\/td>\n<\/tr>\n
Gay-Lussac’s law<\/td>\nA gas law that relates pressure with absolute temperature<\/td>\nOther Gas Laws<\/td>\n<\/tr>\n
Geiger counter<\/td>\nAn electrical device that detects radioactivity<\/td>\nUnits of Radioactivity<\/td>\n<\/tr>\n
Gibbs free energy (G<\/em>)<\/td>\nA measure of spontaneity which incorporates both enthalpy and entropy<\/td>\nGibbs Free Energy<\/td>\n<\/tr>\n
Graham’s law of effusion<\/td>\nA law which relates the rate of effusion of a gas to the inverse of the square root of its molar mass<\/td>\nMolecular Effusion and Diffusion<\/td>\n<\/tr>\n
gray (Gy)<\/td>\nA unit of radioactive exposure qual to 100 rad<\/td>\nUnits of Radioactivity<\/td>\n<\/tr>\n
half cell<\/td>\nA part of a voltaic cell that contains one half reaction<\/td>\nApplications of Redox Reactions: Voltaic Cells<\/td>\n<\/tr>\n
half reaction<\/td>\nThe individual oxidation or reduction reaction of a redox reaction<\/td>\nBalancing Redox Reactions<\/td>\n<\/tr>\n
half reaction method<\/td>\nThe method of balancing redox reactions by writing and balancing the individual half reactions<\/td>\nBalancing Redox Reactions<\/td>\n<\/tr>\n
half-life<\/td>\nThe amount of time it takes for one-half of a radioactive isotope to decay<\/td>\nHalf-Life<\/td>\n<\/tr>\n
half-life<\/td>\nThe amount of time required for the concentration of a reactant to drop to one half of its initial concentration<\/td>\nConcentration-Time Relationships: Integrated Rate Laws<\/td>\n<\/tr>\n
heat<\/td>\nThe transfer of energy from one body to another due to a difference in temperature<\/td>\nWork and Heat<\/td>\n<\/tr>\n
heating curve<\/td>\nA plot of the temperature versus the amount of heat added<\/td>\nPhase Transitions: Melting, Boiling and Subliming<\/td>\n<\/tr>\n
Hess’s law<\/td>\nWhen chemical equations are combined algebraically, their enthalpies can be combined in exactly the same way<\/td>\nHess’s Law<\/td>\n<\/tr>\n
heterogeneous catalyst<\/td>\nA catalyst that is in a different phase from one or more of the reactants<\/td>\nCatalysis<\/td>\n<\/tr>\n
heterogeneous equilibrium<\/td>\nAn equilibrium in which more than one phase of reactants or products is present<\/td>\nThe Equilibrium Constant<\/td>\n<\/tr>\n
heterogeneous mixture<\/td>\nA non-uniform combination of more than one substance<\/td>\nSome Basic Definitions<\/td>\n<\/tr>\n
HOMO<\/td>\nThe highest occupied molecular orbital<\/td>\nMolecular Orbitals<\/td>\n<\/tr>\n
homogeneous catalyst<\/td>\nA catalyst that is present in the same phase as the reactant molecules<\/td>\nCatalysis<\/td>\n<\/tr>\n
homogeneous mixture<\/td>\nA uniform mixture of more than one substance that behaves as a single substance<\/td>\nSome Basic Definitions<\/td>\n<\/tr>\n
Hund’s rule<\/td>\nOne electron is placed in each degenerate orbital before pairing electrons in the same orbital<\/td>\nOrganization of Electrons in Atoms<\/td>\n<\/tr>\n
hybridization<\/td>\nA mathematical mixing of atomic orbitals<\/td>\nValence Bond Theory and Hybrid Orbitals<\/td>\n<\/tr>\n
hydrocarbons<\/td>\nAn organic compound composed of carbon and hydrogen<\/td>\nHydrocarbons<\/td>\n<\/tr>\n
hydrogen bonding<\/td>\nThe very strong interaction between molecules due to H atoms being bonded to N, O, or F atoms<\/td>\nIntermolecular Forces<\/td>\n<\/tr>\n
hydrogenation reaction<\/td>\nThe reaction of hydrogen across a C\u2013C double or triple bond, usually in the presence of a catalyst<\/td>\nHydrocarbons<\/td>\n<\/tr>\n
hydronium ion<\/td>\nThe actual chemical species that represents a hydrogen ion in aqueous solution<\/td>\nArrhenius Acids and Bases<\/td>\n<\/tr>\n
hypothesis<\/td>\nAn educated guess about how the natural universe works<\/td>\nChemistry as a Science<\/td>\n<\/tr>\n
hyrolysis<\/td>\nA reaction with water<\/td>\nBr\u00f8nsted-Lowry Acids and Bases<\/td>\n<\/tr>\n
ICE chart<\/td>\nA table used to calculate equilibria values featuring rows of initial, change and equlibria concentration<\/td>\nCalculating Equilibrium Constant Values<\/td>\n<\/tr>\n
ideal gas<\/td>\nA gas that conforms exactly to the tenets of the kinetic molecular theory<\/td>\nReal Gases<\/td>\n<\/tr>\n
ideal gas law<\/td>\nA gas law that relates all four independent physical properties of a gas under any conditions<\/td>\nThe Ideal Gas Law and Some Applications<\/td>\n<\/tr>\n
indicator<\/td>\nA substance whose color change indicates the equivalence point of a titration<\/td>\nAcid-Base Titrations<\/td>\n<\/tr>\n
initial rate<\/td>\nThe instantaneous rate at the start of a reaction<\/td>\nReaction Rates<\/td>\n<\/tr>\n
initial rates method<\/td>\nA method to determine the rate law from the instantaneous reaction rate upon mixing the reactants<\/td>\nRate Laws<\/td>\n<\/tr>\n
instantaneous reaction rate<\/td>\nThe rate of reaction at one instant in time<\/td>\nReaction Rates<\/td>\n<\/tr>\n
intermediate<\/td>\nA chemical species does not appear in the overall balanced equation and is generated in one elementary step but used up in a subsequent step<\/td>\nReaction Mechanisms<\/td>\n<\/tr>\n
ion<\/td>\nA species with an overall electric charge<\/td>\nIons and Ionic Compounds<\/td>\n<\/tr>\n
ionic compound<\/td>\nA compound formed from positive and negative ions<\/td>\nIons and Ionic Compounds<\/td>\n<\/tr>\n
ionic formula<\/td>\nThe chemical formula for an ionic compound<\/td>\nIons and Ionic Compounds<\/td>\n<\/tr>\n
ionic solid<\/td>\nA crystalline solid composed of ions<\/td>\nSolids<\/td>\n<\/tr>\n
ionization energy (IE)<\/td>\nThe amount of energy required to remove an elec tron from an atom in the gas phase<\/td>\nPeriodic Trends<\/td>\n<\/tr>\n
isolated system<\/td>\nA system that does not allow a transfer of energy or matter into or out of the system<\/td>\nEnergy<\/td>\n<\/tr>\n
isomer<\/td>\nA molecule with the same molecular formula as another molecule but a different structure<\/td>\nHydrocarbons<\/td>\n<\/tr>\n
isothermal<\/td>\nA process that does not change the temperature<\/td>\nPhase Transitions: Melting, Boiling and Subliming<\/td>\n<\/tr>\n
isotopes<\/td>\nAtoms of the same element that have different numbers of neutrons<\/td>\nAtomic Theory<\/td>\n<\/tr>\n
joule<\/td>\nThe SI unit of energy<\/td>\nEnergy<\/td>\n<\/tr>\n
Kelvin scale<\/td>\nThe fundamental unit of temperature in SI<\/td>\nOther Units: Temperature and Density<\/td>\n<\/tr>\n
ketone<\/td>\nA compound where the carbonyl carbon is attached to two carbon chains<\/td>\nOther Oxygen-Containing Functional Groups<\/td>\n<\/tr>\n
kinetic energy<\/td>\nThe energy due to motion<\/td>\nKinetic-Molecular Theory of Gases<\/td>\n<\/tr>\n
kinetic-molecular theory of gases<\/td>\nA model which helps us understand gases at the molecular level and their physical properties<\/td>\nKinetic-Molecular Theory of Gases<\/td>\n<\/tr>\n
kinetics<\/td>\nThe study of reaction rate and the factors that can influence reaction rate<\/td>\nIntroduction to Kinetics<\/td>\n<\/tr>\n
law of conservation of energy<\/td>\nThe total energy of an isolated system does not increase or decrease<\/td>\nEnergy<\/td>\n<\/tr>\n
law of mass action<\/td>\nThe relationship of the amounts of reactants and products at equilibrium<\/td>\nThe Equilibrium Constant<\/td>\n<\/tr>\n
Le Chatelier\u2019s principle<\/td>\nIf an equilibrium is stressed, then the reaction shifts to reduce the stress<\/td>\nShifting Equilibria: Le Chatelier\u2019s Principle<\/td>\n<\/tr>\n
Lewis diagram<\/td>\nA representation of the valence electrons of an atom that uses dots around the symbol of the element<\/td>\nLewis Electron Dot Diagrams<\/td>\n<\/tr>\n
limiting reagent<\/td>\nThe reactant that runs out first for a given chemical reaction<\/td>\nLimiting Reagents<\/td>\n<\/tr>\n
line spectrum<\/td>\nAn image that contains only certain colors of light<\/td>\nQuantum Numbers for Electrons<\/td>\n<\/tr>\n
locant<\/td>\nThe numerical position of a substituent<\/td>\nBranched Hydrocarbons<\/td>\n<\/tr>\n
lock and key model<\/td>\nA simple model used to describe enzyme activity, where substrates must fit into appropriately shaped active sites<\/td>\nCatalysis<\/td>\n<\/tr>\n
lone electron pairs<\/td>\nA pair of electrons that does not make a covalent bond<\/td>\nCovalent Bonds<\/td>\n<\/tr>\n
LUMO<\/td>\nThe lowest unoccupied molecular orbital<\/td>\nMolecular Orbitals<\/td>\n<\/tr>\n
magnetic quantum number (ml)<\/td>\nThe index that determines the orientation of the electron\u2019s spatial distribution<\/td>\nQuantum Numbers for Electrons<\/td>\n<\/tr>\n
mass-mass calculation<\/td>\nA calculation in which you start with a given mass of a substance and calculate the mass of another substance involved in the chemical equation<\/td>\nMole-Mass and Mass-Mass Calculations<\/td>\n<\/tr>\n
matter<\/td>\nAnything that has mass and takes up space.\u00a0is anything that has mass and takes up space<\/td>\nSome Basic Definitions<\/td>\n<\/tr>\n
mean free path<\/td>\nThe average distance traveled by a molecule between collisions<\/td>\nMolecular Effusion and Diffusion<\/td>\n<\/tr>\n
melting<\/td>\nThe process of a solid becoming a liquid<\/td>\nPhase Transitions: Melting, Boiling and Subliming<\/td>\n<\/tr>\n
melting point<\/td>\nThe characteristic temperature at which a solid becomes a liquid<\/td>\nPhase Transitions: Melting, Boiling and Subliming<\/td>\n<\/tr>\n
meniscus<\/td>\nThe curved surface a liquid makes as it approaches a solid barrier<\/td>\nProperties of Liquids<\/td>\n<\/tr>\n
metal<\/td>\nAn element that conducts electricity and heat well and is shiny, silvery, solid, ductile, and malleable<\/td>\nSome Basic Definitions<\/td>\n<\/tr>\n
metallic solid<\/td>\nA solid with the characteristic properties of a metal<\/td>\nSolids<\/td>\n<\/tr>\n
microstate (W<\/em>)<\/td>\nA\u00a0term used\u00a0to describe different possible arrangements of molecular position and kinetic energy, at a particular thermodynamic state<\/td>\nEntropy and the Second Law of Thermodynamics<\/td>\n<\/tr>\n
millimeters of mercury (mmHg)<\/td>\nThe amount of pressure exerted by a column of mercury exactly 1 mm high<\/td>\nPressure<\/td>\n<\/tr>\n
mixture<\/td>\nA physical combination of more than one substance<\/td>\nSome Basic Definitions<\/td>\n<\/tr>\n
molality (m)<\/td>\nThe number of moles of solute per kilogram of solvent<\/td>\nQuantitative Units of Concentration<\/td>\n<\/tr>\n
molar mass<\/td>\nThe mass of 1 mol of a substance in grams<\/td>\nThe Mole<\/td>\n<\/tr>\n
molar volume<\/td>\nThe volume of exactly 1 mol of a gas; equal to 22.4 L at STP<\/td>\nThe Ideal Gas Law and Some Applications<\/td>\n<\/tr>\n
molarity (M)<\/td>\nThe number of moles of solute divided by the number of liters of solution<\/td>\nQuantitative Units of Concentration<\/td>\n<\/tr>\n
mole<\/td>\nThe number of things equal to the number of atoms in exactly 12 g of carbon-12; equals\u00a06.022\u00d71023\u00a0things<\/td>\nThe Mole<\/td>\n<\/tr>\n
mole fraction<\/td>\nThe ratio of the number of moles of a component in a mixture divided by the total number of moles in the sample<\/td>\nGas Mixtures<\/td>\n<\/tr>\n
mole fraction<\/td>\nThe ratio of the number of moles of a component to the total number of moles in a system<\/td>\nColligative Properties of Solutions<\/td>\n<\/tr>\n
molecular formula<\/td>\nA formal listing of what and how many atoms are in a molecule<\/td>\nMolecules an Chemical Nomenclature<\/td>\n<\/tr>\n
molecular geometry<\/td>\nhow the atoms in a molecule are arranged<\/td>\nMolecular Shapes and Polarity<\/td>\n<\/tr>\n
molecular mass<\/td>\nThe sum of the masses of the atoms in a molecule<\/td>\nMasses of Atoms and Molecules<\/td>\n<\/tr>\n
molecular orbital theory (MO theory)<\/td>\nA more sophisticated model\u00a0 of chemical bonding where new molecular orbitals are generated using a mathematical process called Linear Combination of Atomic Orbitals (LCAO)<\/td>\nMolecular Orbitals<\/td>\n<\/tr>\n
molecular polarity<\/td>\nThe vector sum of the individual bond dipoles<\/td>\nMolecular Shapes and Polarity<\/td>\n<\/tr>\n
molecular solid<\/td>\nA crystalline solid whose components are covalently bonded molecules<\/td>\nSolids<\/td>\n<\/tr>\n
molecularity<\/td>\nThe total number of molecules that participate in the effective collision of the elementary step<\/td>\nReaction Mechanisms<\/td>\n<\/tr>\n
molecule<\/td>\nThe smallest part of a substance that has the physical and chemical properties of that substance<\/td>\nMolecules an Chemical Nomenclature<\/td>\n<\/tr>\n
mole-mass calculation<\/td>\nA calculation in which you start with a given number of moles of a substance and calculate the mass of another substance involved in the chemical equation, or vice versa<\/td>\nMole-Mass and Mass-Mass Calculations<\/td>\n<\/tr>\n
mole-mole calculation<\/td>\nA stoichiometry calculation when one starts with moles of one substance and convert to moles of another substance using the balanced chemical equation<\/td>\nThe Mole in Chemical Reactions<\/td>\n<\/tr>\n
monomer<\/td>\nThe repeated unit of a polymer<\/td>\nPolymers<\/td>\n<\/tr>\n
net ionic equation<\/td>\nA chemical equation with the spectator ions removed<\/td>\nIonic Equations: A Closer Look<\/td>\n<\/tr>\n
neutral salt<\/td>\nAn ionic compound that does not affect the acidity of its aqueous solution<\/td>\nStrong and Weak Acids and Bases and Their Salts<\/td>\n<\/tr>\n
neutralization reaction<\/td>\nThe reaction of an acid with a base to produce water and a salt<\/td>\nNeutralization Reactions<\/td>\n<\/tr>\n
neutralization reaction<\/td>\nThe reaction of an acid and a base to produce water and a salt<\/td>\nArrhenius Acids and Bases<\/td>\n<\/tr>\n
neutron<\/td>\nA subatomic particle with no charge<\/td>\nAtomic Theory<\/td>\n<\/tr>\n
node (nodal plane)<\/td>\nAn area of zero electron density<\/td>\nMolecular Orbitals<\/td>\n<\/tr>\n
nomenclature<\/td>\nThe rules of naming in organic chemistry<\/td>\nBranched Hydrocarbons<\/td>\n<\/tr>\n
nonmetal<\/td>\nAn element that exists in various colors and phases, is brittle, and does not conduct electricity or heat well<\/td>\nSome Basic Definitions<\/td>\n<\/tr>\n
nonpolar covalent bond<\/td>\nThe equal sharing of electrons in a covalent bond<\/td>\nOther Aspects of Covalent Bonding<\/td>\n<\/tr>\n
normal boiling point<\/td>\nThe characteristic temperature at which a liquid becomes a gas when the surrounding pressure is exactly 1 atm<\/td>\nPhase Transitions: Melting, Boiling and Subliming<\/td>\n<\/tr>\n
nuclear energy<\/td>\nThe controlled harvesting of energy from fission reactions<\/td>\nNuclear Energy<\/td>\n<\/tr>\n
nuclear equation<\/td>\nA chemical equation that emphasizes changes in atomic nuclei<\/td>\nRadioactivity<\/td>\n<\/tr>\n
nuclear model<\/td>\nThe model of an atom that has the protons and neutrons in a central nucleus with the electrons in orbit about the nucleus<\/td>\nAtomic Theory<\/td>\n<\/tr>\n
nucleus<\/td>\nThe center of an atom that contains protons and neutrons<\/td>\nAtomic Theory<\/td>\n<\/tr>\n
odd-electron molecules<\/td>\nA molecule with an odd number of electrons in the valence shell of an atom<\/td>\nViolations of the Octet Rule<\/td>\n<\/tr>\n
orbital<\/td>\nThe specific set of principal, angular momentum, and magnetic quantum numbers for an electron<\/td>\nQuantum Numbers for Electrons<\/td>\n<\/tr>\n
osmosis<\/td>\nThe tendency of solvent molecules to pass through a semipermeable membrane due to concentration differences<\/td>\nColligative Properties of Solutions<\/td>\n<\/tr>\n
osmotic pressure<\/td>\nThe tendency of a solution to pass solvent through a semipermeable membrane due to concentration differences<\/td>\nColligative Properties of Solutions<\/td>\n<\/tr>\n
oxidation<\/td>\nThe loss of one or more electrons by an atom; an increase in oxidation number<\/td>\nOxidation-Reduction Reactions<\/td>\n<\/tr>\n
oxidation<\/td>\nThe loss of one or more electrons by an atom; an increase in oxidation number<\/td>\nOxidation-Reduction Reactions<\/td>\n<\/tr>\n
oxidation number<\/td>\nA number assigned to an atom that helps keep track of the number of electrons on the atom<\/td>\nOxidation-Reduction Reactions<\/td>\n<\/tr>\n
oxidation number<\/td>\nA number assigned to an atom that helps keep track of the number of electrons on the atom<\/td>\nOxidation-Reduction Reactions<\/td>\n<\/tr>\n
oxidation-reduction (redox) reactions<\/td>\nA chemical reaction that involves the transfer of electrons<\/td>\nOxidation-Reduction Reactions<\/td>\n<\/tr>\n
p block<\/td>\nThe columns of the periodic table in which\u00a0p\u00a0subshells are being occupied<\/td>\nElectronic Structure and the Periodic Table<\/td>\n<\/tr>\n
parent isotope<\/td>\nThe reactant in a nuclear equation<\/td>\nRadioactivity<\/td>\n<\/tr>\n
parts per billion (ppb)<\/td>\nRatio of mass of solute to total mass of sample times 1,000,000,000<\/td>\nQuantitative Units of Concentration<\/td>\n<\/tr>\n
parts per million (ppm)<\/td>\nRatio of mass of solute to total mass of sample times 1,000,000<\/td>\nQuantitative Units of Concentration<\/td>\n<\/tr>\n
parts per thousand (ppth)<\/td>\nRatio of mass of solute to total mass of sample times 1,000<\/td>\nQuantitative Units of Concentration<\/td>\n<\/tr>\n
Pauli exclusion principle<\/td>\nNo two electrons in an atom can have the same set of four quantum numbers<\/td>\nOrganization of Electrons in Atoms<\/td>\n<\/tr>\n
percent yield<\/td>\nActual yield divided by theoretical yield times 100% to give a percentage between 0% and 100%<\/td>\nYields<\/td>\n<\/tr>\n
percentage composition by mass\u00a0(or\u00a0mass percentage, % m\/m)<\/td>\nRatio of mass of solute to the total mass of a sample times 100<\/td>\nQuantitative Units of Concentration<\/td>\n<\/tr>\n
periodic table<\/td>\nA chart of all the elements<\/td>\nAtomic Theory<\/td>\n<\/tr>\n
periodic trends<\/td>\nThe variation of properties versus position on the periodic table<\/td>\nPeriodic Trends<\/td>\n<\/tr>\n
pH<\/td>\nThe negative logarithm of the hydrogen ion concentration<\/td>\nThe pH Scale<\/td>\n<\/tr>\n
pH scale<\/td>\nThe range of values from 0 to 14 that describes the acidity or basicity of a solution<\/td>\nThe pH Scale<\/td>\n<\/tr>\n
phase<\/td>\nAn important physical property that defines whether matter is a solid, liquid, gas or supercritical fluid<\/td>\nSome Basic Definitions<\/td>\n<\/tr>\n
phase diagram<\/td>\nA graphical representation of the equilibrium relationships that exist between the phases of a substance under specified pressures and temperatures<\/td>\nProperties of Liquids<\/td>\n<\/tr>\n
photon<\/td>\nThe name of a discrete unit of light acting as a particle<\/td>\nLight<\/td>\n<\/tr>\n
physical change<\/td>\nA change that occurs when a sample of matter changes one or more of its physical properties<\/td>\nSome Basic Definitions<\/td>\n<\/tr>\n
physical property<\/td>\nA characteristic that describes matter as it exists<\/td>\nSome Basic Definitions<\/td>\n<\/tr>\n
pi bond (\u03c0 bond)<\/td>\nThe sideways overlap of\u00a0p orbitals, placing electron density on opposite sides of the inter-nuclear axis – a double or triple bond<\/td>\nValence Bond Theory and Hybrid Orbitals<\/td>\n<\/tr>\n
Planck’s constant<\/td>\nThe proportionality constant between the frequency and the energy of light: 6.626 \u00d7 10\u221234 J\u00b7s<\/td>\nLight<\/td>\n<\/tr>\n
pOH<\/td>\nThe negative logarithm of the hydroxide ion concentration<\/td>\nThe pH Scale<\/td>\n<\/tr>\n
polar covalent bond<\/td>\nA covalent bond between different atoms that attract the shared electrons by different amounts and cause an imbalance of electron distribution<\/td>\nOther Aspects of Covalent Bonding<\/td>\n<\/tr>\n
polarity<\/td>\nA measure of the unequal sharing of electrons which has resulted in a dipole moment<\/td>\nOther Aspects of Covalent Bonding<\/td>\n<\/tr>\n
polyatomic ions<\/td>\nAn ion that contains more than one atom<\/td>\nIons and Ionic Compounds<\/td>\n<\/tr>\n
polymer<\/td>\nA long molecule made of many repeating units<\/td>\nPolymers<\/td>\n<\/tr>\n
polymerization<\/td>\nThe process of making a polymer<\/td>\nPolymers<\/td>\n<\/tr>\n
polyprotic acid<\/td>\nAn acid capable of donating more than one H+ ion<\/td>\nSome Special Types of Equilibria<\/td>\n<\/tr>\n
precipitate<\/td>\nA solid that falls out of solution in a precipitation reaction<\/td>\nTypes of Chemical Reactions: Single- and Double-Displacement Reactions<\/td>\n<\/tr>\n
precipitation reaction<\/td>\nA chemical reaction in which two ionic compounds are dissolved in water and form a new ionic compound that does not dissolve<\/td>\nTypes of Chemical Reactions: Single- and Double-Displacement Reactions<\/td>\n<\/tr>\n
prefix<\/td>\nA prefix used with a unit that refers to a multiple or fraction of a fundamental unit to make a more conveniently sized unit for a specific quantity<\/td>\nExpressing Units<\/td>\n<\/tr>\n
pressure<\/td>\nForce per unit area<\/td>\nPressure<\/td>\n<\/tr>\n
primary battery<\/td>\nA battery that cannot be recharged<\/td>\nApplications of Redox Reactions: Voltaic Cells<\/td>\n<\/tr>\n
principal quantum number (n)<\/td>\nThe index that largely determines the energy of an electron in an atom<\/td>\nQuantum Numbers for Electrons<\/td>\n<\/tr>\n
product<\/td>\nA final substance in a chemical equation<\/td>\nThe Chemical Equation<\/td>\n<\/tr>\n
proton<\/td>\nA subatomic particle with a positive charge<\/td>\nAtomic Theory<\/td>\n<\/tr>\n
qualitative<\/td>\nA description of the quality of an object<\/td>\nChemistry as a Science<\/td>\n<\/tr>\n
quantitative<\/td>\nA description of a specific amount of something<\/td>\nChemistry as a Science<\/td>\n<\/tr>\n
quantization<\/td>\nWhen a quantity is restricted to having only certain values<\/td>\nQuantum Numbers for Electrons<\/td>\n<\/tr>\n
quantum mechanics<\/td>\nThe theory of electrons that treats them as a wave<\/td>\nQuantum Numbers for Electrons<\/td>\n<\/tr>\n
quantum number<\/td>\nAn index that corresponds to a property of an electron, like its energy<\/td>\nQuantum Numbers for Electrons<\/td>\n<\/tr>\n
rad<\/td>\nA unit of radioactive exposure equal to 0.01 J\/g of tissue<\/td>\nUnits of Radioactivity<\/td>\n<\/tr>\n
radioactive decay<\/td>\nThe spontaneous change of a nucleus from one element to another<\/td>\nRadioactivity<\/td>\n<\/tr>\n
radioactivity<\/td>\nEmanations of particles and radiation from atomic nuclei<\/td>\nRadioactivity<\/td>\n<\/tr>\n
Raoult’s law<\/td>\nThe mathematical formula for calculating the vapor pressure of a solution<\/td>\nColligative Properties of Solutions<\/td>\n<\/tr>\n
rate constant (k<\/em>)<\/td>\nA proportionality constant specific to each reaction at a particular temperature<\/td>\nRate Laws<\/td>\n<\/tr>\n
rate-determining step<\/td>\nThe slowest step in a multistep mechanism<\/td>\nReaction Mechanisms<\/td>\n<\/tr>\n
rate law<\/td>\nA mathematical relationship between the reaction rate and the reactant concentrations<\/td>\nRate Laws<\/td>\n<\/tr>\n
reactant<\/td>\nAn initial substance in a chemical equation<\/td>\nThe Chemical Equation<\/td>\n<\/tr>\n
reaction mechanism<\/td>\nThe bond making and bond breaking steps which occur at the molecular level during a chemical reaction<\/td>\nReaction Mechanisms<\/td>\n<\/tr>\n
reaction order<\/td>\nThe sum of the concentration term exponents in a rate law equation<\/td>\nRate Laws<\/td>\n<\/tr>\n
reaction rate<\/td>\nThe speed of a chemical reaction<\/td>\nIntroduction to Kinetics<\/td>\n<\/tr>\n
real gases<\/td>\nA gas that deviates from ideal behaviour<\/td>\nReal Gases<\/td>\n<\/tr>\n
redox reaction<\/td>\nA chemical reaction that involves the transfer of electrons<\/td>\nOxidation-Reduction Reactions<\/td>\n<\/tr>\n
reduction<\/td>\nThe gain of one or more electrons by an atom; a decrease in oxidation number<\/td>\nOxidation-Reduction Reactions<\/td>\n<\/tr>\n
reduction<\/td>\nThe gain of one or more electrons by an atom; a decrease in oxidation number<\/td>\nOxidation-Reduction Reactions<\/td>\n<\/tr>\n
rem<\/td>\nA unit of radioactive exposure that includes a factor to account for the type of radioactivity<\/td>\nUnits of Radioactivity<\/td>\n<\/tr>\n
ribozyme<\/td>\nRibonucleic acid (RNA) molecules capable of catalyzing certain chemical reactions<\/td>\nCatalysis<\/td>\n<\/tr>\n
root-mean-square (rms) speed\u00a0(urms)<\/td>\nThe speed of molecules having exactly the same kinetic energy as the average kinetic energy of the sample<\/td>\nKinetic-Molecular Theory of Gases<\/td>\n<\/tr>\n
s block<\/td>\nThe columns of the periodic table in which\u00a0s\u00a0subshells are being occupied<\/td>\nElectronic Structure and the Periodic Table<\/td>\n<\/tr>\n
salt<\/td>\nAny ionic compound that is formed from a reaction between an acid and a base<\/td>\nNeutralization Reactions<\/td>\n<\/tr>\n
salt<\/td>\nAny ionic compound that is formed from a reaction between an acid and a base<\/td>\nArrhenius Acids and Bases<\/td>\n<\/tr>\n
salt bridge<\/td>\nA part of a voltaic cell that contains a solution of some ionic compound whose ions migrate to either side of the voltaic cell to maintain the charge balance<\/td>\nApplications of Redox Reactions: Voltaic Cells<\/td>\n<\/tr>\n
saturated hydrocarbons<\/td>\nA carbon compound with the maximum possible number of H atoms in its formula<\/td>\nHydrocarbons<\/td>\n<\/tr>\n
saturated solution<\/td>\nA solution with the maximum amount of solute dissolved in it<\/td>\nSome Definitions<\/td>\n<\/tr>\n
science<\/td>\nThe process of knowing about the natural universe through observation and experiment<\/td>\nChemistry as a Science<\/td>\n<\/tr>\n
scientific law<\/td>\nA specific statement that is thought to be never violated by the entire natural universe<\/td>\nChemistry as a Science<\/td>\n<\/tr>\n
scientific notation<\/td>\nAn expression of a number using powers of 10<\/td>\nExpressing Numbers<\/td>\n<\/tr>\n
screening<\/td>\nThe repelling valence electrons by core electrons<\/td>\nPeriodic Trends<\/td>\n<\/tr>\n
second law of thermodynamics<\/td>\nA spontaneous process will increase the entropy of the universe<\/td>\nEntropy and the Second Law of Thermodynamics<\/td>\n<\/tr>\n
secondary battery<\/td>\nA battery that can be recharged<\/td>\nApplications of Redox Reactions: Voltaic Cells<\/td>\n<\/tr>\n
semimetal<\/td>\nAn element that has properties of both metals and nonmetals<\/td>\nSome Basic Definitions<\/td>\n<\/tr>\n
semipermeable membrane<\/td>\nA thin membrane that will pass certain small molecules but not others<\/td>\nColligative Properties of Solutions<\/td>\n<\/tr>\n
SI unit<\/td>\n\u00a0International System of Units used by all scientists, literally translated from\u00a0\u201cle Syst\u00e8me International d\u2019unit\u00e9s.\u201d<\/td>\nExpressing Units<\/td>\n<\/tr>\n
Sievert (Sv)<\/td>\nSievert (Sv) is a related unit and is defined as 100 rem<\/td>\nUnits of Radioactivity<\/td>\n<\/tr>\n
sigma bond (\u03c3 bond)<\/td>\nOrbital overlap to form a bond which has cylindrical symmetry – a single bond<\/td>\nValence Bond Theory and Hybrid Orbitals<\/td>\n<\/tr>\n
significant figures<\/td>\nThe limit of the number of places a measurement can be properly expressed with<\/td>\nSignificant Figures<\/td>\n<\/tr>\n
silicones<\/td>\nA polymer based on a silicon and oxygen backbone<\/td>\nPolymers<\/td>\n<\/tr>\n
single bond<\/td>\nA covalent bond composed of one pair of electrons<\/td>\nCovalent Bonds<\/td>\n<\/tr>\n
single-replacement reaction<\/td>\nA chemical reaction in which one element is substituted for another element in a compound<\/td>\nTypes of Chemical Reactions: Single- and Double-Displacement Reactions<\/td>\n<\/tr>\n
solidification<\/td>\nThe process of a liquid becoming a solid<\/td>\nPhase Transitions: Melting, Boiling and Subliming<\/td>\n<\/tr>\n
solubility<\/td>\nThe maximum amount of a solute that can be dissolved in a given amount of a solvent<\/td>\nSome Definitions<\/td>\n<\/tr>\n
solubility rules<\/td>\nGeneral statements that predict which ionic compounds dissolve and which do not<\/td>\nTypes of Chemical Reactions: Single- and Double-Displacement Reactions<\/td>\n<\/tr>\n
solute<\/td>\nThe minor component of a solution<\/td>\nSome Definitions<\/td>\n<\/tr>\n
solution<\/td>\nSee homogeneous mixture<\/td>\nSome Basic Definitions<\/td>\n<\/tr>\n
solvent<\/td>\nThe major component of a solution<\/td>\nSome Definitions<\/td>\n<\/tr>\n
specific heat capacity<\/td>\nThe proportionality constant between heat, mass, and temperature change; also called specific heat<\/td>\nWork and Heat<\/td>\n<\/tr>\n
spectator ion<\/td>\nAn ion that does nothing in the overall course of a chemical reaction<\/td>\nIonic Equations: A Closer Look<\/td>\n<\/tr>\n
spin quantum number (ms)<\/td>\nThe index that indicates one of two spin states for an electron<\/td>\nQuantum Numbers for Electrons<\/td>\n<\/tr>\n
spontaneous process<\/td>\nA process that occurs without the influence of external forces or a change that moves a system towards equilibrium<\/td>\nSpontaneous Change<\/td>\n<\/tr>\n
standard molar entropy\u00a0 (So)<\/td>\nThe entropy of 1 mole of a substance in its standard state, at 1 atm of pressure<\/td>\nMeasuring Entropy and Entropy Changes<\/td>\n<\/tr>\n
standard notation<\/td>\nA straightforward expression of a number<\/td>\nExpressing Numbers<\/td>\n<\/tr>\n
standard temperature and pressure (STP)<\/td>\nA set of benchmark conditions used to compare other properties of gases; 100 kPa\u00a0for pressure and 273 K for temperature<\/td>\nThe Ideal Gas Law and Some Applications<\/td>\n<\/tr>\n
stoichiometry<\/td>\nThe relating of one chemical substance to another using a balanced chemical reaction<\/td>\nStoichiometry<\/td>\n<\/tr>\n
strong acid<\/td>\nAny acid that is 100% dissociated into ions in aqueous solution<\/td>\nStrong and Weak Acids and Bases and Their Salts<\/td>\n<\/tr>\n
strong base<\/td>\nAny base that is 100% dissociated into ions in aqueous solution<\/td>\nStrong and Weak Acids and Bases and Their Salts<\/td>\n<\/tr>\n
sublimation<\/td>\nThe process of a solid becoming a gas<\/td>\nPhase Transitions: Melting, Boiling and Subliming<\/td>\n<\/tr>\n
subshell<\/td>\nA term used to describe electrons in a shell that have the same angular momentum quantum number<\/td>\nQuantum Numbers for Electrons<\/td>\n<\/tr>\n
substance<\/td>\nMatter that has the same physical and chemical properties throughout.<\/td>\nSome Basic Definitions<\/td>\n<\/tr>\n
substituent<\/td>\nA branch off a main chain in a hydrocarbon<\/td>\nBranched Hydrocarbons<\/td>\n<\/tr>\n
substrate<\/td>\nThe reactants which are specific for a biological catalyst<\/td>\nCatalysis<\/td>\n<\/tr>\n
supercritical fluid<\/td>\nA phase beyond the critical point, where liquid and gas phases are no longer distinct<\/td>\nProperties of Liquids<\/td>\n<\/tr>\n
supersaturated solution<\/td>\nA unstable solution with more than the normal maximum amount of solute in it<\/td>\nSome Definitions<\/td>\n<\/tr>\n
surface tension<\/td>\nAn effect caused by an imbalance of forces on the atoms at the surface of a liquid<\/td>\nProperties of Liquids<\/td>\n<\/tr>\n
surrounding atoms<\/td>\nAn atom that makes covalent bonds to the central atom(s)<\/td>\nCovalent Bonds<\/td>\n<\/tr>\n
system<\/td>\nThe part of the universe under study<\/td>\nEnergy<\/td>\n<\/tr>\n
temperature<\/td>\nA measure of the average amount of kinetic energy a system contains<\/td>\nOther Units: Temperature and Density<\/td>\n<\/tr>\n
theoretical yield<\/td>\nAn amount that is theoretically produced as calculated using the balanced chemical reaction<\/td>\nYields<\/td>\n<\/tr>\n
theory<\/td>\nA general statement that explains a large number of observations<\/td>\nChemistry as a Science<\/td>\n<\/tr>\n
thermochemical equation<\/td>\nA chemical equation that includes an enthalpy change<\/td>\nEnthalpy and Chemical Reactions<\/td>\n<\/tr>\n
thiol<\/td>\nThe sulfur analog of an alcohol<\/td>\nOther Functional Groups<\/td>\n<\/tr>\n
third law of thermodynamics<\/td>\nAt absolute zero the entropy of a pure, perfect crystal is zero<\/td>\nMeasuring Entropy and Entropy Changes<\/td>\n<\/tr>\n
titrant<\/td>\nThe reagent of known concentration<\/td>\nAcid-Base Titrations<\/td>\n<\/tr>\n
titration<\/td>\nA chemical reaction performed quantitatively to determine the exact amount of a reagent<\/td>\nAcid-Base Titrations<\/td>\n<\/tr>\n
torr<\/td>\nAnother name for a millimeter of mercury<\/td>\nPressure<\/td>\n<\/tr>\n
tracer<\/td>\nA substance that can be used to follow the pathway of that substance through a structure<\/td>\nUses of Radioactive Isotopes<\/td>\n<\/tr>\n
transition state<\/td>\nThe highest energy transitional point in the elementary step<\/td>\nReaction Mechanisms<\/td>\n<\/tr>\n
triple bond<\/td>\nA covalent bond composed of three pairs of bonding electrons<\/td>\nCovalent Bonds<\/td>\n<\/tr>\n
unsaturated hydrocarbons<\/td>\nA carbon compound with less than the maximum possible number of H atoms in its formula<\/td>\nHydrocarbons<\/td>\n<\/tr>\n
unsaturated solution<\/td>\nA solution with less than the maximum amount of solute dissolved in it<\/td>\nSome Definitions<\/td>\n<\/tr>\n
valence electrons<\/td>\nThe electrons in the highest-numbered shell, plus any electrons in the last unfilled subshell. The electrons most likely involved in chemical reactions<\/td>\nElectronic Structure and the Periodic Table<\/td>\n<\/tr>\n
valence shell<\/td>\nThe highest-numbered shell in an atom that contains electrons<\/td>\nElectronic Structure and the Periodic Table<\/td>\n<\/tr>\n
valence shell electron pair repulsion theory (VSEPR)<\/td>\nThe general concept that estimates the shape of a simple molecule:\u00a0 electron pairs repel each other to get as far away from each other as possible<\/td>\nMolecular Shapes and Polarity<\/td>\n<\/tr>\n
van der Waal’s equation<\/td>\nAn equation which compensates for deviations from ideal gas behaviour, correcting for intermolecular forces and the volume of gas molecules<\/td>\nReal Gases<\/td>\n<\/tr>\n
van\u2019t Hoff factor\u00a0(i)<\/td>\nThe number of particles each solute formula unit breaks apart into when it dissolves<\/td>\nColligative Properties of Ionic Solutes<\/td>\n<\/tr>\n
vapor<\/td>\nMaterial in the gas phase due to evaporation<\/td>\nProperties of Liquids<\/td>\n<\/tr>\n
vapor pressure<\/td>\nThe partial pressure exerted by evaporation of a liquid<\/td>\nGas Mixtures<\/td>\n<\/tr>\n
vapor pressure depression<\/td>\nThe decrease of a solution\u2019s vapor pressure because of the presence of a solute<\/td>\nColligative Properties of Solutions<\/td>\n<\/tr>\n
vector quantity<\/td>\nA quantity which has both a magnitude and direction<\/td>\nMolecular Shapes and Polarity<\/td>\n<\/tr>\n
voltaic (galvanic) cell<\/td>\nAn apparatus that allows for useful electrical work to be extracted from a redox reaction.<\/td>\nApplications of Redox Reactions: Voltaic Cells<\/td>\n<\/tr>\n
wavelength<\/td>\nThe distance between corresponding points in two adjacent light cycles<\/td>\nLight<\/td>\n<\/tr>\n
weak acid<\/td>\nAny acid that is less than 100% dissociated into ions in aqueous solution<\/td>\nStrong and Weak Acids and Bases and Their Salts<\/td>\n<\/tr>\n
weak base<\/td>\nAny base that is less than 100% dissociated into ions in aqueous solution<\/td>\nStrong and Weak Acids and Bases and Their Salts<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n
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