{"id":1389,"date":"2018-08-11T03:11:34","date_gmt":"2018-08-11T03:11:34","guid":{"rendered":"https:\/\/courses.lumenlearning.com\/suny-mcc-introductorychemistry\/?post_type=chapter&#038;p=1389"},"modified":"2024-10-10T21:11:06","modified_gmt":"2024-10-10T21:11:06","slug":"nomenclature-from-che151","status":"publish","type":"chapter","link":"https:\/\/courses.lumenlearning.com\/suny-mcc-introductorychemistry\/chapter\/nomenclature-from-che151\/","title":{"raw":"5.4 Chemical Nomenclature","rendered":"5.4 Chemical Nomenclature"},"content":{"raw":"<div class=\"textbox learning-objectives\">\r\n<h3>Learning Objectives<\/h3>\r\nBy the end of this section, you will be able to:\r\n<ul>\r\n \t<li>Name and write formulas of ionic compounds, binary molecular compounds, and acids using IUPAC rules<\/li>\r\n<\/ul>\r\n<\/div>\r\n<strong>Nomenclature<\/strong>, a collection of rules for naming things, is important in science and in many other situations. This module describes an approach that is used to name simple ionic and molecular compounds, such as NaCl, CaCO<sub>3<\/sub>, and N<sub>2<\/sub>O<sub>4<\/sub>. The simplest of these are <strong>binary compounds<\/strong>, those containing only two elements, but we will also consider how to name ionic compounds containing polyatomic ions, and one specific, very important class of compounds known as acids (subsequent chapters in this text will focus on these compounds). We will limit our attention here to inorganic compounds, compounds that are composed principally of elements other than carbon, and will follow the nomenclature guidelines proposed by IUPAC.\r\n<h2>Ionic Compounds<\/h2>\r\nTo name an inorganic compound, we need to consider the answers to several questions. First, is the compound ionic or molecular? If the compound is ionic, does the metal form ions of only one type (fixed charge) or more than one type (variable charge)? Are the ions monatomic (simple) or polyatomic? If the compound is molecular, does it contain hydrogen? If so, does it also contain oxygen? From the answers we derive, we place the compound in an appropriate category and then name it accordingly.\r\n<h3>Compounds Containing Fixed Charged Metals and Simple Anions<\/h3>\r\nThe name of a binary compound containing fixed charged metals consists of the name of the cation (the name of the metal) followed by the name of the anion (the name of the nonmetallic element with its ending replaced by the suffix \u2013<em>ide<\/em>). Some examples are given in Table 1.\r\n<table id=\"fs-idp282234816\" class=\"span-all\" summary=\"The examples of ionic compounds shown in this table are N a C l sodium chloride, K B r potassium bromide, C a I subscript 2 calcium iodide, C s F cesium fluoride, L i C l lithium chloride, N a subscript 2 O sodium oxide, C d S cadmium sulfide, M g subscript 3 N subscript 2 magnesium nitride, C a subscript 3 P subscript 2 calcium phosphide, and A l subscript 4 C subscript 3 aluminum carbide.\">\r\n<thead>\r\n<tr>\r\n<th style=\"width: 675.967px; text-align: center;\" colspan=\"2\">Table 1. Names of Some Ionic Compounds<\/th>\r\n<\/tr>\r\n<\/thead>\r\n<tbody>\r\n<tr>\r\n<td style=\"width: 316.517px; text-align: center;\">NaCl, sodium chloride<\/td>\r\n<td style=\"width: 346.917px; text-align: center;\">Na<sub>2<\/sub>O, sodium oxide<\/td>\r\n<\/tr>\r\n<tr>\r\n<td style=\"width: 316.517px; text-align: center;\">KBr, potassium bromide<\/td>\r\n<td style=\"width: 346.917px; text-align: center;\">CdS, cadmium sulfide<\/td>\r\n<\/tr>\r\n<tr>\r\n<td style=\"width: 316.517px; text-align: center;\">CaI<sub>2<\/sub>, calcium iodide<\/td>\r\n<td style=\"width: 346.917px; text-align: center;\">Mg<sub>3<\/sub>N<sub>2<\/sub>, magnesium nitride<\/td>\r\n<\/tr>\r\n<tr>\r\n<td style=\"width: 316.517px; text-align: center;\">CsF, cesium fluoride<\/td>\r\n<td style=\"width: 346.917px; text-align: center;\">Ca<sub>3<\/sub>P<sub>2<\/sub>, calcium phosphide<\/td>\r\n<\/tr>\r\n<tr>\r\n<td style=\"width: 316.517px; text-align: center;\">LiCl, lithium chloride<\/td>\r\n<td style=\"width: 346.917px; text-align: center;\">Al<sub>4<\/sub>C<sub>3<\/sub>, aluminum carbide<\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\n<h3><span style=\"font-size: 16px; line-height: 1.5;\">Compounds Containing a Metal Ion with a Variable Charge<\/span><\/h3>\r\nMost of the transition metals can form two or more cations with different charges (Note: tin and lead are outside the transition metal area and have variable charges, both can be either 2+ or 4+). Compounds of these metals with nonmetals are named with the same method as compounds in the first category, except the charge of the metal ion is specified by a Roman numeral in parentheses after the name of the metal. The charge of the metal ion is determined from the formula of the compound and the charge of the anion. For example, consider binary ionic compounds of iron and chlorine. Iron typically exhibits a charge of either 2+ or 3+, and the two corresponding compound formulas are FeCl<sub>2<\/sub> and FeCl<sub>3<\/sub>. The simplest name, \u201ciron chloride,\u201d will, in this case, be ambiguous, as it does not distinguish between these two compounds. In cases like this, the charge of the metal ion is included as a Roman numeral in parentheses immediately following the metal name. These two compounds are then unambiguously named iron(II) chloride and iron(III) chloride, respectively. Other examples are provided in Table 2.\r\n<table id=\"fs-idp282283328\" class=\"span-all\" summary=\"The transition metal ionic compound examples included in this table are F e C L subscript 3 or iron three chloride, H g subscript 2 O or mercury one oxide, H g O or mercury two oxide, and C u subscript 3 ( P O subscript 4 ) subscript 2 or copper two phosphate.\">\r\n<thead>\r\n<tr>\r\n<th style=\"width: 675.967px; text-align: center;\" colspan=\"2\">Table 2. Names of Some Transition Metal Ionic Compounds<\/th>\r\n<\/tr>\r\n<tr>\r\n<th style=\"width: 421.933px; text-align: center;\">Transition Metal Ionic Compound<\/th>\r\n<th style=\"width: 241.5px; text-align: center;\">Name<\/th>\r\n<\/tr>\r\n<\/thead>\r\n<tbody>\r\n<tr>\r\n<td style=\"width: 421.933px; text-align: center;\">FeCl<sub>3<\/sub><\/td>\r\n<td style=\"width: 241.5px; text-align: center;\">iron(II) chloride<\/td>\r\n<\/tr>\r\n<tr>\r\n<td style=\"width: 421.933px; text-align: center;\">Hg<sub>2<\/sub>O<\/td>\r\n<td style=\"width: 241.5px; text-align: center;\">mercury(I) oxide<\/td>\r\n<\/tr>\r\n<tr>\r\n<td style=\"width: 421.933px; text-align: center;\">HgO<\/td>\r\n<td style=\"width: 241.5px; text-align: center;\">mercury(II) oxide<\/td>\r\n<\/tr>\r\n<tr>\r\n<td style=\"width: 421.933px; text-align: center;\">Cu<sub>3<\/sub>P<sub>2<\/sub><\/td>\r\n<td style=\"width: 241.5px; text-align: center;\">copper(II) phosphide<\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\nOut-of-date nomenclature used the suffixes \u2013<em>ic<\/em> and \u2013<em>ous<\/em> to designate metals with higher and lower charges, respectively: Iron(III) chloride, FeCl<sub>3<\/sub>, was previously called ferric chloride, and iron(II) chloride, FeCl<sub>2<\/sub>, was known as ferrous chloride. Though this naming convention has been largely abandoned by the scientific community, it remains in use by some segments of industry. For example, you may see the words <em>stannous fluoride<\/em> on a tube of toothpaste. This represents the formula SnF<sub>2<\/sub>, which is more properly named tin(II) fluoride. The other fluoride of tin is SnF<sub>4<\/sub>, which was previously called stannic fluoride but is now named tin(IV) fluoride.\r\n<h3>Compounds Containing Polyatomic Ions<\/h3>\r\nCompounds containing polyatomic ions are named similarly to those containing only monatomic ions, except there is no need to change to an \u2013<em>ide<\/em> ending, since the suffix is already present in the name of the anion. Most polyatomic ions end in <em>\u2013ate<\/em> and <em>\u2013ite<\/em>. Examples of ionic compounds containing polyatomic ions are shown in Table 3.\r\n<table id=\"fs-idp279316112\" class=\"span-all\" style=\"height: 98px; width: 658.533px;\" summary=\"The examples of polyatomic ionic compounds shown in this table are K C subscript 2 H subscript 3 O subscript 2 potassium acetate, N a H C O subscript 3 sodium bicarbonate, A l subscript 2 ( C O subscript 3 ) subscript 3 aluminum carbonate, (N H subscript 4) CL, ammonium chloride, C a S O subscript 4 calcium sulfate, and M g subscript 3 ( P O subscript 4 ) subscript 2 magnesium phosphate.\">\r\n<thead>\r\n<tr style=\"height: 14px;\">\r\n<th style=\"width: 645px; height: 14px; text-align: center;\" colspan=\"3\">Table 3. Names of Some Polyatomic Ionic Compounds<\/th>\r\n<\/tr>\r\n<\/thead>\r\n<tbody>\r\n<tr style=\"height: 14px;\">\r\n<td style=\"text-align: center; width: 318px; height: 14px;\">KC<sub>2<\/sub>H<sub>3<\/sub>O<sub>2<\/sub>, potassium acetate<\/td>\r\n<td style=\"text-align: center; width: 314.467px; height: 14px;\" colspan=\"2\">Cu<sub>2<\/sub>NO<sub>3<\/sub>, copper(I) nitrate<\/td>\r\n<\/tr>\r\n<tr style=\"height: 14px;\">\r\n<td style=\"text-align: center; width: 318px; height: 14px;\">Al<sub>2<\/sub>(CO<sub>3<\/sub>)<sub>3<\/sub>, aluminum carbonate<\/td>\r\n<td style=\"text-align: center; height: 14px; width: 314.467px;\" colspan=\"2\">Sn(OH)<sub>2<\/sub>, tin(II) hydroxide<\/td>\r\n<\/tr>\r\n<tr style=\"height: 14px;\">\r\n<td style=\"text-align: center; width: 318px; height: 14px;\">NaHCO<sub>3<\/sub>, sodium bicarbonate<\/td>\r\n<td style=\"text-align: center; height: 14px; width: 314.467px;\" colspan=\"2\">Mn(SO<sub>4<\/sub>)<sub>2<\/sub>, manganese(IV) sulfite<\/td>\r\n<\/tr>\r\n<tr style=\"height: 14px;\">\r\n<td style=\"text-align: center; width: 318px; height: 14px;\">Mg<sub>3<\/sub>(PO<sub>4<\/sub>)<sub>2<\/sub>, magnesium phosphate<\/td>\r\n<td style=\"text-align: center; height: 14px; width: 314.467px;\" colspan=\"2\">Ni(CN)<sub>2<\/sub>, nickel(II) cyanide<\/td>\r\n<\/tr>\r\n<tr style=\"height: 14px;\">\r\n<td style=\"text-align: center; width: 318px; height: 14px;\">CaSO<sub>4<\/sub>, calcium sulfate<\/td>\r\n<td style=\"text-align: center; height: 14px; width: 314.467px;\" colspan=\"2\">AuSCN, gold(I) thiocyanate<\/td>\r\n<\/tr>\r\n<tr style=\"height: 14px;\">\r\n<td style=\"text-align: center; width: 318px; height: 14px;\">(NH<sub>4<\/sub>)Cl, ammonium chloride<\/td>\r\n<td style=\"text-align: center; width: 314.467px; height: 14px;\" colspan=\"2\">Pb(ClO<sub>4<\/sub>)<sub>2<\/sub>, lead(II) perchlorate<\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\n<table id=\"fs-idp279316112\" class=\"span-all\" style=\"width: 474.533px;\" summary=\"The examples of polyatomic ionic compounds shown in this table are K C subscript 2 H subscript 3 O subscript 2 potassium acetate, N a H C O subscript 3 sodium bicarbonate, A l subscript 2 ( C O subscript 3 ) subscript 3 aluminum carbonate, (N H subscript 4) CL, ammonium chloride, C a S O subscript 4 calcium sulfate, and M g subscript 3 ( P O subscript 4 ) subscript 2 magnesium phosphate.\">\r\n<thead>\r\n<tr>\r\n<th style=\"text-align: center; width: 675.967px;\" colspan=\"3\">Table 4. Common Polyatomic Ions<\/th>\r\n<\/tr>\r\n<\/thead>\r\n<tbody>\r\n<tr>\r\n<td style=\"text-align: center; width: 226px;\">NH<sub>4<\/sub><sup>+<\/sup>, ammonium<\/td>\r\n<td style=\"text-align: center; width: 437.433px;\" colspan=\"2\">OH<sup>-<\/sup>, hydroxide<\/td>\r\n<\/tr>\r\n<tr>\r\n<td style=\"text-align: center; width: 226px;\">C<sub>2<\/sub>H<sub>3<\/sub>O<sub>2<\/sub><sup>-<\/sup>, acetate<\/td>\r\n<td style=\"text-align: center; width: 437.433px;\" colspan=\"2\">NO<sub>3<\/sub><sup>-<\/sup>, nitrate<\/td>\r\n<\/tr>\r\n<tr>\r\n<td style=\"text-align: center; width: 226px;\">CO<sub>3<\/sub><sup>2-<\/sup>, carbonate<\/td>\r\n<td style=\"text-align: center; width: 437.433px;\" colspan=\"2\">NO<sub>2<\/sub><sup>-<\/sup>, nitrite<\/td>\r\n<\/tr>\r\n<tr>\r\n<td style=\"text-align: center; width: 226px;\">HCO<sub>3<\/sub><sup>-<\/sup>, hydrogen carbonate*<\/td>\r\n<td style=\"text-align: center; width: 437.433px;\" colspan=\"2\">PO<sub>4<\/sub><sup>3-<\/sup>, phosphate<\/td>\r\n<\/tr>\r\n<tr>\r\n<td style=\"text-align: center; width: 226px;\">CN<sup>-<\/sup>, cyanide<\/td>\r\n<td style=\"text-align: center; width: 437.433px;\" colspan=\"2\">PO<sub>3<\/sub><sup>3-<\/sup>, phosphite<\/td>\r\n<\/tr>\r\n<tr>\r\n<td style=\"text-align: center; width: 226px;\">SCN<sup>-<\/sup>, thiocyanate<\/td>\r\n<td style=\"text-align: center;\" colspan=\"2\">SO<sub>4<\/sub><sup>2-<\/sup>, sulfate<\/td>\r\n<\/tr>\r\n<tr>\r\n<td style=\"text-align: center; width: 226px;\">ClO<sub>4<\/sub><sup>-<\/sup>, perchlorate<\/td>\r\n<td style=\"text-align: center;\" colspan=\"2\">SO<sub>3<\/sub><sup>2-<\/sup>. sulfite<\/td>\r\n<\/tr>\r\n<tr>\r\n<td style=\"text-align: center; width: 226px;\">ClO<sub>3<\/sub><sup>-<\/sup>, chlorate<\/td>\r\n<td style=\"text-align: center;\" colspan=\"2\"><\/td>\r\n<\/tr>\r\n<tr>\r\n<td style=\"text-align: center; width: 226px;\">ClO<sub>2<\/sub><sup>-<\/sup>, chlorite<\/td>\r\n<td style=\"text-align: center;\" colspan=\"2\">*hydrogen carbonate can also go by bicarbonate<\/td>\r\n<\/tr>\r\n<tr>\r\n<td style=\"text-align: center; width: 226px;\">ClO<sup>-<\/sup>, hypochlorite<\/td>\r\n<td style=\"text-align: center; width: 437.433px;\" colspan=\"2\"><\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\n<div class=\"textbox shaded\">\r\n<h3>Ionic Compounds in Your Cabinets<\/h3>\r\nEvery day you encounter and use a large number of ionic compounds. Some of these compounds, where they are found, and what they are used for are listed in Table 5. Look at the label or ingredients list on the various products that you use during the next few days, and see if you run into any of those in this table, or find other ionic compounds that you could now name or write as a formula.\r\n<table id=\"fs-idp268265360\" class=\"span-all\" summary=\"The everyday ionic compound examples included in this table are: N a C L sodium chloride, or ordinary table salt, K I potassium iodide which is added to iodized salt, N a F, sodium fluoride which is an ingredient in toothpaste, N a H C O subscript 3 sodium bicarbonate which is baking soda, used in cooking and as an antacid, N a subscript 2 C O subscript 3 sodium carbonate which is washing soda and is used in cleaning agents, N a O C l sodium hypochlorite which is the active ingredient in household bleach, C a C O subscript 3 calcium carbonate which is an ingredient of antacids, M g ( O H ) subscript 2, magnesium hydroxide which is also an ingredient of antacids, A l ( O H ) subscript 3 aluminum hydroxide which is also an ingredient in antacids, N a O H sodium hydroxide which is lye and is used as a drain cleaner, K subscript 3 P O subscript 4 potassium phosphate which is a food additive, M g S O subscript 4 magneisum sulfate which is added to purified water, N a subscript 2 H P O subscript 4 sodium hydrogen phosphate which is an anti-caking agent and is used in powdered products, and N a subscript 2 S O subscript 3 sodium sulfite which is a preservative.\">\r\n<thead>\r\n<tr>\r\n<th colspan=\"2\">Table 5. Everyday Ionic Compounds<\/th>\r\n<\/tr>\r\n<tr>\r\n<th>Ionic Compound<\/th>\r\n<th>Use<\/th>\r\n<\/tr>\r\n<\/thead>\r\n<tbody>\r\n<tr>\r\n<td>NaCl, sodium chloride<\/td>\r\n<td>ordinary table salt<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>KI, potassium iodide<\/td>\r\n<td>added to \u201ciodized\u201d salt for thyroid health<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>NaF, sodium fluoride<\/td>\r\n<td>ingredient in toothpaste<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>NaHCO<sub>3<\/sub>, sodium bicarbonate<\/td>\r\n<td>baking soda; used in cooking (and as antacid)<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Na<sub>2<\/sub>CO<sub>3<\/sub>, sodium carbonate<\/td>\r\n<td>washing soda; used in cleaning agents<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>NaOCl, sodium hypochlorite<\/td>\r\n<td>active ingredient in household bleach<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>CaCO<sub>3<\/sub> calcium carbonate<\/td>\r\n<td>ingredient in antacids<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Mg(OH)<sub>2<\/sub>, magnesium hydroxide<\/td>\r\n<td>ingredient in antacids<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Al(OH)<sub>3<\/sub>, aluminum hydroxide<\/td>\r\n<td>ingredient in antacids<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>NaOH, sodium hydroxide<\/td>\r\n<td>lye; used as drain cleaner<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>K<sub>3<\/sub>PO<sub>4<\/sub>, potassium phosphate<\/td>\r\n<td>food additive (many purposes)<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>MgSO<sub>4<\/sub>, magnesium sulfate<\/td>\r\n<td>added to purified water<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Na<sub>2<\/sub>HPO<sub>4<\/sub>, sodium hydrogen phosphate<\/td>\r\n<td>anti-caking agent; used in powdered products<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Na<sub>2<\/sub>SO<sub>3<\/sub>, sodium sulfite<\/td>\r\n<td>preservative<\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\n<\/div>\r\n<div class=\"textbox examples\">\r\n<h3>Example 1: <strong>Naming Ionic Compounds<\/strong><\/h3>\r\nName the following ionic compounds, which contain a metal that can have more than one ionic charge:\r\n<ol>\r\n \t<li>Li<sub>2<\/sub>S<\/li>\r\n \t<li>Li<sub>2<\/sub>SO<sub>4<\/sub><\/li>\r\n \t<li>Li<sub>2<\/sub>SO<sub>3<\/sub><\/li>\r\n \t<li>Fe<sub>2<\/sub>O<sub>3<\/sub><\/li>\r\n \t<li>CuSe<\/li>\r\n \t<li>GaN<\/li>\r\n \t<li>CrCl<sub>3<\/sub><\/li>\r\n \t<li>Ti<sub>2<\/sub>(SO<sub>4<\/sub>)<sub>3<\/sub><\/li>\r\n<\/ol>\r\n[reveal-answer q=\"143093\"]Show Answer[\/reveal-answer]\r\n[hidden-answer a=\"143093\"]\r\n<ol>\r\n \t<li>lithium sulfide<\/li>\r\n \t<li>lithium sulfate<\/li>\r\n \t<li>lithium sulfite<\/li>\r\n \t<li>iron(III) oxide<\/li>\r\n \t<li>copper(II) selenide<\/li>\r\n \t<li>gallium nitride<\/li>\r\n \t<li>chromium(III) chloride<\/li>\r\n \t<li>titanium(III) sulfate<\/li>\r\n<\/ol>\r\n[\/hidden-answer]\r\n<h4><strong>Check Your Learning<\/strong><\/h4>\r\nWrite the formulas of the following ionic compounds:\r\n<ol>\r\n \t<li>chromium(III) phosphide<\/li>\r\n \t<li>mercury(II) sulfide<\/li>\r\n \t<li>manganese(II) phosphate<\/li>\r\n \t<li>copper(I) oxide<\/li>\r\n \t<li>chromium(VI) fluoride<\/li>\r\n<\/ol>\r\n[reveal-answer q=\"560392\"]Show Answer[\/reveal-answer]\r\n[hidden-answer a=\"560392\"]\r\n<ol>\r\n \t<li>CrP<\/li>\r\n \t<li>HgS<\/li>\r\n \t<li>Mn<sub>3<\/sub>(PO<sub>4<\/sub>)<sub>2<\/sub><\/li>\r\n \t<li>Cu<sub>2<\/sub>O<\/li>\r\n \t<li>CrF<sub>6<\/sub><\/li>\r\n<\/ol>\r\n[\/hidden-answer]\r\n\r\n<\/div>\r\n<h2>Molecular (Covalent) Compounds<\/h2>\r\nThe bonding characteristics of inorganic molecular compounds are different from ionic compounds, and they are named using a different system as well. The charges of cations and anions dictate their ratios in ionic compounds, so specifying the names of the ions provides sufficient information to determine chemical formulas. However, because covalent bonding allows for significant variation in the combination ratios of the atoms in a molecule, the names for molecular compounds must explicitly identify these ratios.\r\n<h3>Compounds Composed of Two Elements<\/h3>\r\nWhen two nonmetallic elements form a molecular compound, several combination ratios are often possible. For example, carbon and oxygen can form the compounds CO and CO<sub>2<\/sub>. Since these are different substances with different properties, they cannot both have the same name (they cannot both be called carbon oxide). To deal with this situation, we use a naming method that is somewhat similar to that used for ionic compounds, but with added prefixes to specify the numbers of atoms of each element. The name of the more metallic element (the one farther to the left and\/or bottom of the periodic table) is first, followed by the name of the more nonmetallic element (the one farther to the right and\/or top) with its ending changed to the suffix \u2013<em>ide<\/em>. The numbers of atoms of each element are designated by the Greek prefixes shown in Table 5.\r\n<table id=\"fs-idp268400368\" class=\"span-all\" summary=\"This table has two columns labeled \u201cprefix\u201d and \u201cnumber\u201d. Mono is associated with one although this prefix is sometimes omitted. Di is associated with two. Tri is associated with three. Tetra is associated with four. Penta is associated with five. Hexa is associated with six. Hepta is associated with seven. Octa is associated with eight. Nona is associated with nine. Deca is associated with ten.\">\r\n<thead>\r\n<tr>\r\n<th colspan=\"5\">Table 5. Nomenclature Prefixes<\/th>\r\n<\/tr>\r\n<tr>\r\n<th>Number<\/th>\r\n<th>Prefix<\/th>\r\n<th><\/th>\r\n<th>Number<\/th>\r\n<th>Prefix<\/th>\r\n<\/tr>\r\n<\/thead>\r\n<tbody>\r\n<tr>\r\n<td>1 (sometimes omitted)<\/td>\r\n<td>mono-<\/td>\r\n<td rowspan=\"6\"><\/td>\r\n<td>6<\/td>\r\n<td>hexa-<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>2<\/td>\r\n<td>di-<\/td>\r\n<td>7<\/td>\r\n<td>hepta-<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>3<\/td>\r\n<td>tri-<\/td>\r\n<td>8<\/td>\r\n<td>octa-<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>4<\/td>\r\n<td>tetra-<\/td>\r\n<td>9<\/td>\r\n<td>nona-<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>5<\/td>\r\n<td>penta-<\/td>\r\n<td>10<\/td>\r\n<td>deca-<\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\nWhen only one atom of the first element is present, the prefix <em>mono<\/em>- is usually deleted from that part. Thus, CO is named carbon monoxide, and CO<sub>2<\/sub> is called carbon dioxide. When two vowels are adjacent, the <em>a<\/em> in the Greek prefix is usually dropped. Some other examples are shown in Table 6.\r\n<table id=\"fs-idp269568176\" class=\"span-all\" summary=\"A two column table is shown. The left column is titled \u201cCompound\u201d and the right column is titled \u201cName.\u201d From left to right, the first row reads \u201cS O subscript 2\u201d and \u201csulfur dioxide.\u201d The second row reads \u201cS O subscript 3\u201d and \u201csulfur trioxide.\u201d The third row reads \u201cN O subscript 2\u201d and \u201cnitrogen dioxide.\u201d The fourth row reads \u201cN subscript 2 O subscript 4\u201d and \u201cdinitrogen tetroxide.\u201d The fifth row reads \u201cN subscript 2 O subscript 5\u201d and \u201cdinitrogen pentoxide.\u201d The sixth row reads \u201cB C l subscript 3\u201d and \u201cboron trichloride.\u201d The seventh row reads \u201cS F subscript 6\u201d and \u201csulfur hexafluoride.\u201d The eighth row reads \u201cP F subscript 5\u201d and \u201cphosphorus pentafluoride.\u201d The ninth row reads \u201cP subscript 4 O subscript 10\u201d and \u201ctetraphosphorus decaoxide.\u201d The tenth row reads \u201cI F subscript 7\u201d and \u201ciodine heptafluoride.\u201d\">\r\n<thead>\r\n<tr>\r\n<th colspan=\"5\">Table 6. Names of Some Molecular Compounds Composed of Two Elements<\/th>\r\n<\/tr>\r\n<tr>\r\n<th>Compound<\/th>\r\n<th>Name<\/th>\r\n<th><\/th>\r\n<th>Compound<\/th>\r\n<th>Name<\/th>\r\n<\/tr>\r\n<\/thead>\r\n<tbody>\r\n<tr>\r\n<td>SO<sub>2<\/sub><\/td>\r\n<td>sulfur dioxide<\/td>\r\n<td rowspan=\"6\"><\/td>\r\n<td>BCl<sub>3<\/sub><\/td>\r\n<td>boron trichloride<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>SO<sub>3<\/sub><\/td>\r\n<td>sulfur trioxide<\/td>\r\n<td>SF<sub>6<\/sub><\/td>\r\n<td>sulfur hexafluoride<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>NO<sub>2<\/sub><\/td>\r\n<td>nitrogen dioxide<\/td>\r\n<td>PF<sub>5<\/sub><\/td>\r\n<td>phosphorus pentafluoride<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>N<sub>2<\/sub>O<sub>4<\/sub><\/td>\r\n<td>dinitrogen tetroxide<\/td>\r\n<td>P<sub>4<\/sub>O<sub>10<\/sub><\/td>\r\n<td>tetraphosphorus decaoxide<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>N<sub>2<\/sub>O<sub>5<\/sub><\/td>\r\n<td>dinitrogen pentoxide<\/td>\r\n<td>IF<sub>7<\/sub><\/td>\r\n<td>iodine heptafluoride<\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\nThere are a few common names that you will encounter as you continue your study of chemistry. For example, although NO is often called nitric oxide, its proper name is nitrogen monoxide. Similarly, N<sub>2<\/sub>O is known as nitrous oxide even though our rules would specify the name dinitrogen monoxide. (And H<sub>2<\/sub>O is usually called water, not dihydrogen monoxide.)\r\n<div class=\"textbox examples\">\r\n<h3>Example 2: <strong>Naming Covalent Compounds<\/strong><\/h3>\r\nName the following covalent compounds:\r\n<ol>\r\n \t<li>SF<sub>6<\/sub><\/li>\r\n \t<li>N<sub>2<\/sub>O<sub>3<\/sub><\/li>\r\n \t<li>Cl<sub>2<\/sub>O<sub>7<\/sub><\/li>\r\n \t<li>P<sub>4<\/sub>O<sub>6<\/sub><\/li>\r\n<\/ol>\r\n[reveal-answer q=\"1263\"]Show Answer[\/reveal-answer]\r\n[hidden-answer a=\"1263\"]Because these compounds consist solely of nonmetals, we use prefixes to designate the number of atoms of each element:\r\n<ol>\r\n \t<li>sulfur hexafluoride<\/li>\r\n \t<li>dinitrogen trioxide<\/li>\r\n \t<li>dichlorine heptoxide<\/li>\r\n \t<li>tetraphosphorus hexoxide<\/li>\r\n<\/ol>\r\n[\/hidden-answer]\r\n<h4><strong>Check Your Learning<\/strong><\/h4>\r\nWrite the formulas for the following compounds:\r\n<ol>\r\n \t<li>phosphorus pentachloride<\/li>\r\n \t<li>dinitrogen monoxide<\/li>\r\n \t<li>iodine heptafluoride<\/li>\r\n \t<li>carbon tetrachloride<\/li>\r\n<\/ol>\r\n[reveal-answer q=\"405667\"]Show Answer[\/reveal-answer]\r\n[hidden-answer a=\"405667\"]\r\n<ol>\r\n \t<li>PCl<sub>5<\/sub><\/li>\r\n \t<li>N<sub>2<\/sub>O<\/li>\r\n \t<li>IF<sub>7<\/sub><\/li>\r\n \t<li>CCl<sub>4<\/sub><\/li>\r\n<\/ol>\r\n[\/hidden-answer]\r\n\r\n<\/div>\r\n<div class=\"textbox key-takeaways\">\r\n<h3>Key Concepts and Summary<\/h3>\r\nChemists use nomenclature rules to clearly name compounds. Ionic and molecular compounds are named using somewhat-different methods. Binary ionic compounds typically consist of a metal and a nonmetal. The name of the metal is written first, followed by the name of the nonmetal with its ending changed to \u2013<em>ide<\/em>. For example, K<sub>2<\/sub>O is called potassium oxide. If the metal can form ions with different charges, a Roman numeral in parentheses follows the name of the metal to specify its charge. Thus, FeCl<sub>2<\/sub> is iron(II) chloride and FeCl<sub>3<\/sub> is iron(III) chloride.\r\n\r\nSome compounds contain polyatomic ions; the names of common polyatomic ions should be memorized. Molecular compounds can form compounds with different ratios of their elements, so prefixes are used to specify the numbers of atoms of each element in a molecule of the compound. Examples include SF<sub>6<\/sub>, sulfur hexafluoride, and N<sub>2<\/sub>O<sub>4<\/sub>, dinitrogen tetroxide.\r\n\r\n<\/div>\r\n<div class=\"textbox exercises\">\r\n<h3>Exercises<\/h3>\r\n<ol>\r\n \t<li>Name the following compounds:\r\n<ol style=\"list-style-type: lower-alpha;\">\r\n \t<li>CsCl<\/li>\r\n \t<li>BaO<\/li>\r\n \t<li>K<sub>2<\/sub>S<\/li>\r\n \t<li>BeCl<sub>2 <\/sub><\/li>\r\n \t<li>AlF<sub>3<\/sub><\/li>\r\n<\/ol>\r\n<\/li>\r\n \t<li>Name the following compounds:\r\n<ol style=\"list-style-type: lower-alpha;\">\r\n \t<li>NaF<\/li>\r\n \t<li>Rb<sub>2<\/sub>O<\/li>\r\n \t<li>BCl<sub>3 <\/sub><\/li>\r\n \t<li>P<sub>4<\/sub>O<sub>6 <\/sub><\/li>\r\n \t<li>ICl<sub>3<\/sub><\/li>\r\n<\/ol>\r\n<\/li>\r\n \t<li>Write the formulas of the following compounds:\r\n<ol style=\"list-style-type: lower-alpha;\">\r\n \t<li>rubidium bromide<\/li>\r\n \t<li>magnesium selenide<\/li>\r\n \t<li>sodium oxide<\/li>\r\n \t<li>calcium chloride<\/li>\r\n \t<li>gallium phosphide<\/li>\r\n \t<li>aluminum bromide<\/li>\r\n \t<li>ammonium sulfate<\/li>\r\n<\/ol>\r\n<\/li>\r\n \t<li>Write the formulas of the following compounds:\r\n<ol style=\"list-style-type: lower-alpha;\">\r\n \t<li>lithium carbonate<\/li>\r\n \t<li>sodium perchlorate<\/li>\r\n \t<li>barium hydroxide<\/li>\r\n \t<li>ammonium carbonate<\/li>\r\n \t<li>calcium acetate<\/li>\r\n \t<li>magnesium phosphate<\/li>\r\n \t<li>sodium sulfite<\/li>\r\n<\/ol>\r\n<\/li>\r\n \t<li>Write the formulas of the following compounds:\r\n<ol style=\"list-style-type: lower-alpha;\">\r\n \t<li>chlorine dioxide<\/li>\r\n \t<li>dinitrogen tetraoxide<\/li>\r\n \t<li>potassium phosphide<\/li>\r\n \t<li>silver(I) sulfide<\/li>\r\n \t<li>aluminum nitride<\/li>\r\n \t<li>silicon dioxide<\/li>\r\n<\/ol>\r\n<\/li>\r\n \t<li>Write the formulas of the following compounds:\r\n<ol style=\"list-style-type: lower-alpha;\">\r\n \t<li>barium chloride<\/li>\r\n \t<li>magnesium nitride<\/li>\r\n \t<li>sulfur dioxide<\/li>\r\n \t<li>nitrogen trichloride<\/li>\r\n \t<li>dinitrogen trioxide<\/li>\r\n \t<li>tin(IV) chloride<\/li>\r\n<\/ol>\r\n<\/li>\r\n \t<li>Each of the following compounds contains a metal that can exhibit more than one ionic charge. Name these compounds:\r\n<ol style=\"list-style-type: lower-alpha;\">\r\n \t<li>Cr<sub>2<\/sub>O<sub>3 <\/sub><\/li>\r\n \t<li>FeCl<sub>2 <\/sub><\/li>\r\n \t<li>CrO<sub>3 <\/sub><\/li>\r\n \t<li>TiCl<sub>4 <\/sub><\/li>\r\n \t<li>CoO<\/li>\r\n \t<li>MoS<sub>2<\/sub><\/li>\r\n<\/ol>\r\n<\/li>\r\n \t<li>Each of the following compounds contains a metal that can exhibit more than one ionic charge. Name these compounds:\r\n<ol style=\"list-style-type: lower-alpha;\">\r\n \t<li>NiCO<sub>3 <\/sub><\/li>\r\n \t<li>MoO<sub>3 <\/sub><\/li>\r\n \t<li>Co(NO<sub>3<\/sub>)<sub>2 <\/sub><\/li>\r\n \t<li>V<sub>2<\/sub>O<sub>5 <\/sub><\/li>\r\n \t<li>MnO<sub>2 <\/sub><\/li>\r\n \t<li>Fe<sub>2<\/sub>O<sub>3 <\/sub><\/li>\r\n<\/ol>\r\n<\/li>\r\n \t<li>The following ionic compounds are found in common household products. Write the formulas for each compound:\r\n<ol style=\"list-style-type: lower-alpha;\">\r\n \t<li>potassium phosphate<\/li>\r\n \t<li>copper(II) sulfate<\/li>\r\n \t<li>calcium chloride<\/li>\r\n \t<li>titanium(II) oxide<\/li>\r\n \t<li>ammonium nitrate<\/li>\r\n \t<li>sodium sulfate<\/li>\r\n<\/ol>\r\n<\/li>\r\n \t<li>The following ionic compounds are found in common household products. Name each of the compounds:\r\n<ol style=\"list-style-type: lower-alpha;\">\r\n \t<li>Ca(H<sub>2<\/sub>PO<sub>4<\/sub>)<sub>2 <\/sub><\/li>\r\n \t<li>FeSO<sub>4 <\/sub><\/li>\r\n \t<li>CaCO<sub>3 <\/sub><\/li>\r\n \t<li>MgO<\/li>\r\n \t<li>NaNO<sub>2 <\/sub><\/li>\r\n \t<li>KI<\/li>\r\n<\/ol>\r\n<\/li>\r\n<\/ol>\r\n[reveal-answer q=\"708113\"]Show Selected Answers[\/reveal-answer]\r\n[hidden-answer a=\"708113\"]\r\n\r\n1. (a) cesium chloride; (b) barium oxide; (c) potassium sulfide; (d) beryllium chloride; (e) aluminum fluoride\r\n\r\n3. (a) RbBr; (b) MgSe; (c) Na<sub>2<\/sub>O; (d) CaCl<sub>2<\/sub>; (e) GaP; (f) AlBr<sub>3<\/sub>; (g) (NH<sub>4<\/sub>)<sub>2<\/sub>SO<sub>4<\/sub>\r\n\r\n5. (a) ClO<sub>2<\/sub>; (b) N<sub>2<\/sub>O<sub>4<\/sub>; (c) K<sub>3<\/sub>P; (d) Ag<sub>2<\/sub>S; (e) AlN; (f) SiO<sub>2<\/sub>\r\n\r\n7. (a) chromium(III) oxide; (b) iron(II) chloride; (c) chromium(VI) oxide; (d) titanium(IV) chloride; (e) cobalt(II) oxide; (f) molybdenum(IV) sulfide\r\n\r\n9. (a) K<sub>3<\/sub>PO<sub>4<\/sub>; (b) CuSO<sub>4<\/sub>; (c) CaCl<sub>2<\/sub>; (d) TiO<sub>2<\/sub>; (e) NH<sub>4<\/sub>NO<sub>3<\/sub>; (f) Na<sub>2<\/sub>SO<sub>4<\/sub>\r\n\r\n[\/hidden-answer]\r\n\r\n<\/div>\r\n<h2>Glossary<\/h2>\r\n<strong>binary compound: <\/strong>compound containing two different elements.\r\n\r\n<strong>nomenclature: <\/strong>system of rules for naming objects of interest","rendered":"<div class=\"textbox learning-objectives\">\n<h3>Learning Objectives<\/h3>\n<p>By the end of this section, you will be able to:<\/p>\n<ul>\n<li>Name and write formulas of ionic compounds, binary molecular compounds, and acids using IUPAC rules<\/li>\n<\/ul>\n<\/div>\n<p><strong>Nomenclature<\/strong>, a collection of rules for naming things, is important in science and in many other situations. This module describes an approach that is used to name simple ionic and molecular compounds, such as NaCl, CaCO<sub>3<\/sub>, and N<sub>2<\/sub>O<sub>4<\/sub>. The simplest of these are <strong>binary compounds<\/strong>, those containing only two elements, but we will also consider how to name ionic compounds containing polyatomic ions, and one specific, very important class of compounds known as acids (subsequent chapters in this text will focus on these compounds). We will limit our attention here to inorganic compounds, compounds that are composed principally of elements other than carbon, and will follow the nomenclature guidelines proposed by IUPAC.<\/p>\n<h2>Ionic Compounds<\/h2>\n<p>To name an inorganic compound, we need to consider the answers to several questions. First, is the compound ionic or molecular? If the compound is ionic, does the metal form ions of only one type (fixed charge) or more than one type (variable charge)? Are the ions monatomic (simple) or polyatomic? If the compound is molecular, does it contain hydrogen? If so, does it also contain oxygen? From the answers we derive, we place the compound in an appropriate category and then name it accordingly.<\/p>\n<h3>Compounds Containing Fixed Charged Metals and Simple Anions<\/h3>\n<p>The name of a binary compound containing fixed charged metals consists of the name of the cation (the name of the metal) followed by the name of the anion (the name of the nonmetallic element with its ending replaced by the suffix \u2013<em>ide<\/em>). Some examples are given in Table 1.<\/p>\n<table id=\"fs-idp282234816\" class=\"span-all\" summary=\"The examples of ionic compounds shown in this table are N a C l sodium chloride, K B r potassium bromide, C a I subscript 2 calcium iodide, C s F cesium fluoride, L i C l lithium chloride, N a subscript 2 O sodium oxide, C d S cadmium sulfide, M g subscript 3 N subscript 2 magnesium nitride, C a subscript 3 P subscript 2 calcium phosphide, and A l subscript 4 C subscript 3 aluminum carbide.\">\n<thead>\n<tr>\n<th style=\"width: 675.967px; text-align: center;\" colspan=\"2\">Table 1. Names of Some Ionic Compounds<\/th>\n<\/tr>\n<\/thead>\n<tbody>\n<tr>\n<td style=\"width: 316.517px; text-align: center;\">NaCl, sodium chloride<\/td>\n<td style=\"width: 346.917px; text-align: center;\">Na<sub>2<\/sub>O, sodium oxide<\/td>\n<\/tr>\n<tr>\n<td style=\"width: 316.517px; text-align: center;\">KBr, potassium bromide<\/td>\n<td style=\"width: 346.917px; text-align: center;\">CdS, cadmium sulfide<\/td>\n<\/tr>\n<tr>\n<td style=\"width: 316.517px; text-align: center;\">CaI<sub>2<\/sub>, calcium iodide<\/td>\n<td style=\"width: 346.917px; text-align: center;\">Mg<sub>3<\/sub>N<sub>2<\/sub>, magnesium nitride<\/td>\n<\/tr>\n<tr>\n<td style=\"width: 316.517px; text-align: center;\">CsF, cesium fluoride<\/td>\n<td style=\"width: 346.917px; text-align: center;\">Ca<sub>3<\/sub>P<sub>2<\/sub>, calcium phosphide<\/td>\n<\/tr>\n<tr>\n<td style=\"width: 316.517px; text-align: center;\">LiCl, lithium chloride<\/td>\n<td style=\"width: 346.917px; text-align: center;\">Al<sub>4<\/sub>C<sub>3<\/sub>, aluminum carbide<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<h3><span style=\"font-size: 16px; line-height: 1.5;\">Compounds Containing a Metal Ion with a Variable Charge<\/span><\/h3>\n<p>Most of the transition metals can form two or more cations with different charges (Note: tin and lead are outside the transition metal area and have variable charges, both can be either 2+ or 4+). Compounds of these metals with nonmetals are named with the same method as compounds in the first category, except the charge of the metal ion is specified by a Roman numeral in parentheses after the name of the metal. The charge of the metal ion is determined from the formula of the compound and the charge of the anion. For example, consider binary ionic compounds of iron and chlorine. Iron typically exhibits a charge of either 2+ or 3+, and the two corresponding compound formulas are FeCl<sub>2<\/sub> and FeCl<sub>3<\/sub>. The simplest name, \u201ciron chloride,\u201d will, in this case, be ambiguous, as it does not distinguish between these two compounds. In cases like this, the charge of the metal ion is included as a Roman numeral in parentheses immediately following the metal name. These two compounds are then unambiguously named iron(II) chloride and iron(III) chloride, respectively. Other examples are provided in Table 2.<\/p>\n<table id=\"fs-idp282283328\" class=\"span-all\" summary=\"The transition metal ionic compound examples included in this table are F e C L subscript 3 or iron three chloride, H g subscript 2 O or mercury one oxide, H g O or mercury two oxide, and C u subscript 3 ( P O subscript 4 ) subscript 2 or copper two phosphate.\">\n<thead>\n<tr>\n<th style=\"width: 675.967px; text-align: center;\" colspan=\"2\">Table 2. Names of Some Transition Metal Ionic Compounds<\/th>\n<\/tr>\n<tr>\n<th style=\"width: 421.933px; text-align: center;\">Transition Metal Ionic Compound<\/th>\n<th style=\"width: 241.5px; text-align: center;\">Name<\/th>\n<\/tr>\n<\/thead>\n<tbody>\n<tr>\n<td style=\"width: 421.933px; text-align: center;\">FeCl<sub>3<\/sub><\/td>\n<td style=\"width: 241.5px; text-align: center;\">iron(II) chloride<\/td>\n<\/tr>\n<tr>\n<td style=\"width: 421.933px; text-align: center;\">Hg<sub>2<\/sub>O<\/td>\n<td style=\"width: 241.5px; text-align: center;\">mercury(I) oxide<\/td>\n<\/tr>\n<tr>\n<td style=\"width: 421.933px; text-align: center;\">HgO<\/td>\n<td style=\"width: 241.5px; text-align: center;\">mercury(II) oxide<\/td>\n<\/tr>\n<tr>\n<td style=\"width: 421.933px; text-align: center;\">Cu<sub>3<\/sub>P<sub>2<\/sub><\/td>\n<td style=\"width: 241.5px; text-align: center;\">copper(II) phosphide<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<p>Out-of-date nomenclature used the suffixes \u2013<em>ic<\/em> and \u2013<em>ous<\/em> to designate metals with higher and lower charges, respectively: Iron(III) chloride, FeCl<sub>3<\/sub>, was previously called ferric chloride, and iron(II) chloride, FeCl<sub>2<\/sub>, was known as ferrous chloride. Though this naming convention has been largely abandoned by the scientific community, it remains in use by some segments of industry. For example, you may see the words <em>stannous fluoride<\/em> on a tube of toothpaste. This represents the formula SnF<sub>2<\/sub>, which is more properly named tin(II) fluoride. The other fluoride of tin is SnF<sub>4<\/sub>, which was previously called stannic fluoride but is now named tin(IV) fluoride.<\/p>\n<h3>Compounds Containing Polyatomic Ions<\/h3>\n<p>Compounds containing polyatomic ions are named similarly to those containing only monatomic ions, except there is no need to change to an \u2013<em>ide<\/em> ending, since the suffix is already present in the name of the anion. Most polyatomic ions end in <em>\u2013ate<\/em> and <em>\u2013ite<\/em>. Examples of ionic compounds containing polyatomic ions are shown in Table 3.<\/p>\n<table id=\"fs-idp279316112\" class=\"span-all\" style=\"height: 98px; width: 658.533px;\" summary=\"The examples of polyatomic ionic compounds shown in this table are K C subscript 2 H subscript 3 O subscript 2 potassium acetate, N a H C O subscript 3 sodium bicarbonate, A l subscript 2 ( C O subscript 3 ) subscript 3 aluminum carbonate, (N H subscript 4) CL, ammonium chloride, C a S O subscript 4 calcium sulfate, and M g subscript 3 ( P O subscript 4 ) subscript 2 magnesium phosphate.\">\n<thead>\n<tr style=\"height: 14px;\">\n<th style=\"width: 645px; height: 14px; text-align: center;\" colspan=\"3\">Table 3. Names of Some Polyatomic Ionic Compounds<\/th>\n<\/tr>\n<\/thead>\n<tbody>\n<tr style=\"height: 14px;\">\n<td style=\"text-align: center; width: 318px; height: 14px;\">KC<sub>2<\/sub>H<sub>3<\/sub>O<sub>2<\/sub>, potassium acetate<\/td>\n<td style=\"text-align: center; width: 314.467px; height: 14px;\" colspan=\"2\">Cu<sub>2<\/sub>NO<sub>3<\/sub>, copper(I) nitrate<\/td>\n<\/tr>\n<tr style=\"height: 14px;\">\n<td style=\"text-align: center; width: 318px; height: 14px;\">Al<sub>2<\/sub>(CO<sub>3<\/sub>)<sub>3<\/sub>, aluminum carbonate<\/td>\n<td style=\"text-align: center; height: 14px; width: 314.467px;\" colspan=\"2\">Sn(OH)<sub>2<\/sub>, tin(II) hydroxide<\/td>\n<\/tr>\n<tr style=\"height: 14px;\">\n<td style=\"text-align: center; width: 318px; height: 14px;\">NaHCO<sub>3<\/sub>, sodium bicarbonate<\/td>\n<td style=\"text-align: center; height: 14px; width: 314.467px;\" colspan=\"2\">Mn(SO<sub>4<\/sub>)<sub>2<\/sub>, manganese(IV) sulfite<\/td>\n<\/tr>\n<tr style=\"height: 14px;\">\n<td style=\"text-align: center; width: 318px; height: 14px;\">Mg<sub>3<\/sub>(PO<sub>4<\/sub>)<sub>2<\/sub>, magnesium phosphate<\/td>\n<td style=\"text-align: center; height: 14px; width: 314.467px;\" colspan=\"2\">Ni(CN)<sub>2<\/sub>, nickel(II) cyanide<\/td>\n<\/tr>\n<tr style=\"height: 14px;\">\n<td style=\"text-align: center; width: 318px; height: 14px;\">CaSO<sub>4<\/sub>, calcium sulfate<\/td>\n<td style=\"text-align: center; height: 14px; width: 314.467px;\" colspan=\"2\">AuSCN, gold(I) thiocyanate<\/td>\n<\/tr>\n<tr style=\"height: 14px;\">\n<td style=\"text-align: center; width: 318px; height: 14px;\">(NH<sub>4<\/sub>)Cl, ammonium chloride<\/td>\n<td style=\"text-align: center; width: 314.467px; height: 14px;\" colspan=\"2\">Pb(ClO<sub>4<\/sub>)<sub>2<\/sub>, lead(II) perchlorate<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<table id=\"fs-idp279316112\" class=\"span-all\" style=\"width: 474.533px;\" summary=\"The examples of polyatomic ionic compounds shown in this table are K C subscript 2 H subscript 3 O subscript 2 potassium acetate, N a H C O subscript 3 sodium bicarbonate, A l subscript 2 ( C O subscript 3 ) subscript 3 aluminum carbonate, (N H subscript 4) CL, ammonium chloride, C a S O subscript 4 calcium sulfate, and M g subscript 3 ( P O subscript 4 ) subscript 2 magnesium phosphate.\">\n<thead>\n<tr>\n<th style=\"text-align: center; width: 675.967px;\" colspan=\"3\">Table 4. Common Polyatomic Ions<\/th>\n<\/tr>\n<\/thead>\n<tbody>\n<tr>\n<td style=\"text-align: center; width: 226px;\">NH<sub>4<\/sub><sup>+<\/sup>, ammonium<\/td>\n<td style=\"text-align: center; width: 437.433px;\" colspan=\"2\">OH<sup>&#8211;<\/sup>, hydroxide<\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center; width: 226px;\">C<sub>2<\/sub>H<sub>3<\/sub>O<sub>2<\/sub><sup>&#8211;<\/sup>, acetate<\/td>\n<td style=\"text-align: center; width: 437.433px;\" colspan=\"2\">NO<sub>3<\/sub><sup>&#8211;<\/sup>, nitrate<\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center; width: 226px;\">CO<sub>3<\/sub><sup>2-<\/sup>, carbonate<\/td>\n<td style=\"text-align: center; width: 437.433px;\" colspan=\"2\">NO<sub>2<\/sub><sup>&#8211;<\/sup>, nitrite<\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center; width: 226px;\">HCO<sub>3<\/sub><sup>&#8211;<\/sup>, hydrogen carbonate*<\/td>\n<td style=\"text-align: center; width: 437.433px;\" colspan=\"2\">PO<sub>4<\/sub><sup>3-<\/sup>, phosphate<\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center; width: 226px;\">CN<sup>&#8211;<\/sup>, cyanide<\/td>\n<td style=\"text-align: center; width: 437.433px;\" colspan=\"2\">PO<sub>3<\/sub><sup>3-<\/sup>, phosphite<\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center; width: 226px;\">SCN<sup>&#8211;<\/sup>, thiocyanate<\/td>\n<td style=\"text-align: center;\" colspan=\"2\">SO<sub>4<\/sub><sup>2-<\/sup>, sulfate<\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center; width: 226px;\">ClO<sub>4<\/sub><sup>&#8211;<\/sup>, perchlorate<\/td>\n<td style=\"text-align: center;\" colspan=\"2\">SO<sub>3<\/sub><sup>2-<\/sup>. sulfite<\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center; width: 226px;\">ClO<sub>3<\/sub><sup>&#8211;<\/sup>, chlorate<\/td>\n<td style=\"text-align: center;\" colspan=\"2\"><\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center; width: 226px;\">ClO<sub>2<\/sub><sup>&#8211;<\/sup>, chlorite<\/td>\n<td style=\"text-align: center;\" colspan=\"2\">*hydrogen carbonate can also go by bicarbonate<\/td>\n<\/tr>\n<tr>\n<td style=\"text-align: center; width: 226px;\">ClO<sup>&#8211;<\/sup>, hypochlorite<\/td>\n<td style=\"text-align: center; width: 437.433px;\" colspan=\"2\"><\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<div class=\"textbox shaded\">\n<h3>Ionic Compounds in Your Cabinets<\/h3>\n<p>Every day you encounter and use a large number of ionic compounds. Some of these compounds, where they are found, and what they are used for are listed in Table 5. Look at the label or ingredients list on the various products that you use during the next few days, and see if you run into any of those in this table, or find other ionic compounds that you could now name or write as a formula.<\/p>\n<table id=\"fs-idp268265360\" class=\"span-all\" summary=\"The everyday ionic compound examples included in this table are: N a C L sodium chloride, or ordinary table salt, K I potassium iodide which is added to iodized salt, N a F, sodium fluoride which is an ingredient in toothpaste, N a H C O subscript 3 sodium bicarbonate which is baking soda, used in cooking and as an antacid, N a subscript 2 C O subscript 3 sodium carbonate which is washing soda and is used in cleaning agents, N a O C l sodium hypochlorite which is the active ingredient in household bleach, C a C O subscript 3 calcium carbonate which is an ingredient of antacids, M g ( O H ) subscript 2, magnesium hydroxide which is also an ingredient of antacids, A l ( O H ) subscript 3 aluminum hydroxide which is also an ingredient in antacids, N a O H sodium hydroxide which is lye and is used as a drain cleaner, K subscript 3 P O subscript 4 potassium phosphate which is a food additive, M g S O subscript 4 magneisum sulfate which is added to purified water, N a subscript 2 H P O subscript 4 sodium hydrogen phosphate which is an anti-caking agent and is used in powdered products, and N a subscript 2 S O subscript 3 sodium sulfite which is a preservative.\">\n<thead>\n<tr>\n<th colspan=\"2\">Table 5. Everyday Ionic Compounds<\/th>\n<\/tr>\n<tr>\n<th>Ionic Compound<\/th>\n<th>Use<\/th>\n<\/tr>\n<\/thead>\n<tbody>\n<tr>\n<td>NaCl, sodium chloride<\/td>\n<td>ordinary table salt<\/td>\n<\/tr>\n<tr>\n<td>KI, potassium iodide<\/td>\n<td>added to \u201ciodized\u201d salt for thyroid health<\/td>\n<\/tr>\n<tr>\n<td>NaF, sodium fluoride<\/td>\n<td>ingredient in toothpaste<\/td>\n<\/tr>\n<tr>\n<td>NaHCO<sub>3<\/sub>, sodium bicarbonate<\/td>\n<td>baking soda; used in cooking (and as antacid)<\/td>\n<\/tr>\n<tr>\n<td>Na<sub>2<\/sub>CO<sub>3<\/sub>, sodium carbonate<\/td>\n<td>washing soda; used in cleaning agents<\/td>\n<\/tr>\n<tr>\n<td>NaOCl, sodium hypochlorite<\/td>\n<td>active ingredient in household bleach<\/td>\n<\/tr>\n<tr>\n<td>CaCO<sub>3<\/sub> calcium carbonate<\/td>\n<td>ingredient in antacids<\/td>\n<\/tr>\n<tr>\n<td>Mg(OH)<sub>2<\/sub>, magnesium hydroxide<\/td>\n<td>ingredient in antacids<\/td>\n<\/tr>\n<tr>\n<td>Al(OH)<sub>3<\/sub>, aluminum hydroxide<\/td>\n<td>ingredient in antacids<\/td>\n<\/tr>\n<tr>\n<td>NaOH, sodium hydroxide<\/td>\n<td>lye; used as drain cleaner<\/td>\n<\/tr>\n<tr>\n<td>K<sub>3<\/sub>PO<sub>4<\/sub>, potassium phosphate<\/td>\n<td>food additive (many purposes)<\/td>\n<\/tr>\n<tr>\n<td>MgSO<sub>4<\/sub>, magnesium sulfate<\/td>\n<td>added to purified water<\/td>\n<\/tr>\n<tr>\n<td>Na<sub>2<\/sub>HPO<sub>4<\/sub>, sodium hydrogen phosphate<\/td>\n<td>anti-caking agent; used in powdered products<\/td>\n<\/tr>\n<tr>\n<td>Na<sub>2<\/sub>SO<sub>3<\/sub>, sodium sulfite<\/td>\n<td>preservative<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<\/div>\n<div class=\"textbox examples\">\n<h3>Example 1: <strong>Naming Ionic Compounds<\/strong><\/h3>\n<p>Name the following ionic compounds, which contain a metal that can have more than one ionic charge:<\/p>\n<ol>\n<li>Li<sub>2<\/sub>S<\/li>\n<li>Li<sub>2<\/sub>SO<sub>4<\/sub><\/li>\n<li>Li<sub>2<\/sub>SO<sub>3<\/sub><\/li>\n<li>Fe<sub>2<\/sub>O<sub>3<\/sub><\/li>\n<li>CuSe<\/li>\n<li>GaN<\/li>\n<li>CrCl<sub>3<\/sub><\/li>\n<li>Ti<sub>2<\/sub>(SO<sub>4<\/sub>)<sub>3<\/sub><\/li>\n<\/ol>\n<div class=\"qa-wrapper\" style=\"display: block\"><span class=\"show-answer collapsed\" style=\"cursor: pointer\" data-target=\"q143093\">Show Answer<\/span><\/p>\n<div id=\"q143093\" class=\"hidden-answer\" style=\"display: none\">\n<ol>\n<li>lithium sulfide<\/li>\n<li>lithium sulfate<\/li>\n<li>lithium sulfite<\/li>\n<li>iron(III) oxide<\/li>\n<li>copper(II) selenide<\/li>\n<li>gallium nitride<\/li>\n<li>chromium(III) chloride<\/li>\n<li>titanium(III) sulfate<\/li>\n<\/ol>\n<\/div>\n<\/div>\n<h4><strong>Check Your Learning<\/strong><\/h4>\n<p>Write the formulas of the following ionic compounds:<\/p>\n<ol>\n<li>chromium(III) phosphide<\/li>\n<li>mercury(II) sulfide<\/li>\n<li>manganese(II) phosphate<\/li>\n<li>copper(I) oxide<\/li>\n<li>chromium(VI) fluoride<\/li>\n<\/ol>\n<div class=\"qa-wrapper\" style=\"display: block\"><span class=\"show-answer collapsed\" style=\"cursor: pointer\" data-target=\"q560392\">Show Answer<\/span><\/p>\n<div id=\"q560392\" class=\"hidden-answer\" style=\"display: none\">\n<ol>\n<li>CrP<\/li>\n<li>HgS<\/li>\n<li>Mn<sub>3<\/sub>(PO<sub>4<\/sub>)<sub>2<\/sub><\/li>\n<li>Cu<sub>2<\/sub>O<\/li>\n<li>CrF<sub>6<\/sub><\/li>\n<\/ol>\n<\/div>\n<\/div>\n<\/div>\n<h2>Molecular (Covalent) Compounds<\/h2>\n<p>The bonding characteristics of inorganic molecular compounds are different from ionic compounds, and they are named using a different system as well. The charges of cations and anions dictate their ratios in ionic compounds, so specifying the names of the ions provides sufficient information to determine chemical formulas. However, because covalent bonding allows for significant variation in the combination ratios of the atoms in a molecule, the names for molecular compounds must explicitly identify these ratios.<\/p>\n<h3>Compounds Composed of Two Elements<\/h3>\n<p>When two nonmetallic elements form a molecular compound, several combination ratios are often possible. For example, carbon and oxygen can form the compounds CO and CO<sub>2<\/sub>. Since these are different substances with different properties, they cannot both have the same name (they cannot both be called carbon oxide). To deal with this situation, we use a naming method that is somewhat similar to that used for ionic compounds, but with added prefixes to specify the numbers of atoms of each element. The name of the more metallic element (the one farther to the left and\/or bottom of the periodic table) is first, followed by the name of the more nonmetallic element (the one farther to the right and\/or top) with its ending changed to the suffix \u2013<em>ide<\/em>. The numbers of atoms of each element are designated by the Greek prefixes shown in Table 5.<\/p>\n<table id=\"fs-idp268400368\" class=\"span-all\" summary=\"This table has two columns labeled \u201cprefix\u201d and \u201cnumber\u201d. Mono is associated with one although this prefix is sometimes omitted. Di is associated with two. Tri is associated with three. Tetra is associated with four. Penta is associated with five. Hexa is associated with six. Hepta is associated with seven. Octa is associated with eight. Nona is associated with nine. Deca is associated with ten.\">\n<thead>\n<tr>\n<th colspan=\"5\">Table 5. Nomenclature Prefixes<\/th>\n<\/tr>\n<tr>\n<th>Number<\/th>\n<th>Prefix<\/th>\n<th><\/th>\n<th>Number<\/th>\n<th>Prefix<\/th>\n<\/tr>\n<\/thead>\n<tbody>\n<tr>\n<td>1 (sometimes omitted)<\/td>\n<td>mono-<\/td>\n<td rowspan=\"6\"><\/td>\n<td>6<\/td>\n<td>hexa-<\/td>\n<\/tr>\n<tr>\n<td>2<\/td>\n<td>di-<\/td>\n<td>7<\/td>\n<td>hepta-<\/td>\n<\/tr>\n<tr>\n<td>3<\/td>\n<td>tri-<\/td>\n<td>8<\/td>\n<td>octa-<\/td>\n<\/tr>\n<tr>\n<td>4<\/td>\n<td>tetra-<\/td>\n<td>9<\/td>\n<td>nona-<\/td>\n<\/tr>\n<tr>\n<td>5<\/td>\n<td>penta-<\/td>\n<td>10<\/td>\n<td>deca-<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<p>When only one atom of the first element is present, the prefix <em>mono<\/em>&#8211; is usually deleted from that part. Thus, CO is named carbon monoxide, and CO<sub>2<\/sub> is called carbon dioxide. When two vowels are adjacent, the <em>a<\/em> in the Greek prefix is usually dropped. Some other examples are shown in Table 6.<\/p>\n<table id=\"fs-idp269568176\" class=\"span-all\" summary=\"A two column table is shown. The left column is titled \u201cCompound\u201d and the right column is titled \u201cName.\u201d From left to right, the first row reads \u201cS O subscript 2\u201d and \u201csulfur dioxide.\u201d The second row reads \u201cS O subscript 3\u201d and \u201csulfur trioxide.\u201d The third row reads \u201cN O subscript 2\u201d and \u201cnitrogen dioxide.\u201d The fourth row reads \u201cN subscript 2 O subscript 4\u201d and \u201cdinitrogen tetroxide.\u201d The fifth row reads \u201cN subscript 2 O subscript 5\u201d and \u201cdinitrogen pentoxide.\u201d The sixth row reads \u201cB C l subscript 3\u201d and \u201cboron trichloride.\u201d The seventh row reads \u201cS F subscript 6\u201d and \u201csulfur hexafluoride.\u201d The eighth row reads \u201cP F subscript 5\u201d and \u201cphosphorus pentafluoride.\u201d The ninth row reads \u201cP subscript 4 O subscript 10\u201d and \u201ctetraphosphorus decaoxide.\u201d The tenth row reads \u201cI F subscript 7\u201d and \u201ciodine heptafluoride.\u201d\">\n<thead>\n<tr>\n<th colspan=\"5\">Table 6. Names of Some Molecular Compounds Composed of Two Elements<\/th>\n<\/tr>\n<tr>\n<th>Compound<\/th>\n<th>Name<\/th>\n<th><\/th>\n<th>Compound<\/th>\n<th>Name<\/th>\n<\/tr>\n<\/thead>\n<tbody>\n<tr>\n<td>SO<sub>2<\/sub><\/td>\n<td>sulfur dioxide<\/td>\n<td rowspan=\"6\"><\/td>\n<td>BCl<sub>3<\/sub><\/td>\n<td>boron trichloride<\/td>\n<\/tr>\n<tr>\n<td>SO<sub>3<\/sub><\/td>\n<td>sulfur trioxide<\/td>\n<td>SF<sub>6<\/sub><\/td>\n<td>sulfur hexafluoride<\/td>\n<\/tr>\n<tr>\n<td>NO<sub>2<\/sub><\/td>\n<td>nitrogen dioxide<\/td>\n<td>PF<sub>5<\/sub><\/td>\n<td>phosphorus pentafluoride<\/td>\n<\/tr>\n<tr>\n<td>N<sub>2<\/sub>O<sub>4<\/sub><\/td>\n<td>dinitrogen tetroxide<\/td>\n<td>P<sub>4<\/sub>O<sub>10<\/sub><\/td>\n<td>tetraphosphorus decaoxide<\/td>\n<\/tr>\n<tr>\n<td>N<sub>2<\/sub>O<sub>5<\/sub><\/td>\n<td>dinitrogen pentoxide<\/td>\n<td>IF<sub>7<\/sub><\/td>\n<td>iodine heptafluoride<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<p>There are a few common names that you will encounter as you continue your study of chemistry. For example, although NO is often called nitric oxide, its proper name is nitrogen monoxide. Similarly, N<sub>2<\/sub>O is known as nitrous oxide even though our rules would specify the name dinitrogen monoxide. (And H<sub>2<\/sub>O is usually called water, not dihydrogen monoxide.)<\/p>\n<div class=\"textbox examples\">\n<h3>Example 2: <strong>Naming Covalent Compounds<\/strong><\/h3>\n<p>Name the following covalent compounds:<\/p>\n<ol>\n<li>SF<sub>6<\/sub><\/li>\n<li>N<sub>2<\/sub>O<sub>3<\/sub><\/li>\n<li>Cl<sub>2<\/sub>O<sub>7<\/sub><\/li>\n<li>P<sub>4<\/sub>O<sub>6<\/sub><\/li>\n<\/ol>\n<div class=\"qa-wrapper\" style=\"display: block\"><span class=\"show-answer collapsed\" style=\"cursor: pointer\" data-target=\"q1263\">Show Answer<\/span><\/p>\n<div id=\"q1263\" class=\"hidden-answer\" style=\"display: none\">Because these compounds consist solely of nonmetals, we use prefixes to designate the number of atoms of each element:<\/p>\n<ol>\n<li>sulfur hexafluoride<\/li>\n<li>dinitrogen trioxide<\/li>\n<li>dichlorine heptoxide<\/li>\n<li>tetraphosphorus hexoxide<\/li>\n<\/ol>\n<\/div>\n<\/div>\n<h4><strong>Check Your Learning<\/strong><\/h4>\n<p>Write the formulas for the following compounds:<\/p>\n<ol>\n<li>phosphorus pentachloride<\/li>\n<li>dinitrogen monoxide<\/li>\n<li>iodine heptafluoride<\/li>\n<li>carbon tetrachloride<\/li>\n<\/ol>\n<div class=\"qa-wrapper\" style=\"display: block\"><span class=\"show-answer collapsed\" style=\"cursor: pointer\" data-target=\"q405667\">Show Answer<\/span><\/p>\n<div id=\"q405667\" class=\"hidden-answer\" style=\"display: none\">\n<ol>\n<li>PCl<sub>5<\/sub><\/li>\n<li>N<sub>2<\/sub>O<\/li>\n<li>IF<sub>7<\/sub><\/li>\n<li>CCl<sub>4<\/sub><\/li>\n<\/ol>\n<\/div>\n<\/div>\n<\/div>\n<div class=\"textbox key-takeaways\">\n<h3>Key Concepts and Summary<\/h3>\n<p>Chemists use nomenclature rules to clearly name compounds. Ionic and molecular compounds are named using somewhat-different methods. Binary ionic compounds typically consist of a metal and a nonmetal. The name of the metal is written first, followed by the name of the nonmetal with its ending changed to \u2013<em>ide<\/em>. For example, K<sub>2<\/sub>O is called potassium oxide. If the metal can form ions with different charges, a Roman numeral in parentheses follows the name of the metal to specify its charge. Thus, FeCl<sub>2<\/sub> is iron(II) chloride and FeCl<sub>3<\/sub> is iron(III) chloride.<\/p>\n<p>Some compounds contain polyatomic ions; the names of common polyatomic ions should be memorized. Molecular compounds can form compounds with different ratios of their elements, so prefixes are used to specify the numbers of atoms of each element in a molecule of the compound. Examples include SF<sub>6<\/sub>, sulfur hexafluoride, and N<sub>2<\/sub>O<sub>4<\/sub>, dinitrogen tetroxide.<\/p>\n<\/div>\n<div class=\"textbox exercises\">\n<h3>Exercises<\/h3>\n<ol>\n<li>Name the following compounds:\n<ol style=\"list-style-type: lower-alpha;\">\n<li>CsCl<\/li>\n<li>BaO<\/li>\n<li>K<sub>2<\/sub>S<\/li>\n<li>BeCl<sub>2 <\/sub><\/li>\n<li>AlF<sub>3<\/sub><\/li>\n<\/ol>\n<\/li>\n<li>Name the following compounds:\n<ol style=\"list-style-type: lower-alpha;\">\n<li>NaF<\/li>\n<li>Rb<sub>2<\/sub>O<\/li>\n<li>BCl<sub>3 <\/sub><\/li>\n<li>P<sub>4<\/sub>O<sub>6 <\/sub><\/li>\n<li>ICl<sub>3<\/sub><\/li>\n<\/ol>\n<\/li>\n<li>Write the formulas of the following compounds:\n<ol style=\"list-style-type: lower-alpha;\">\n<li>rubidium bromide<\/li>\n<li>magnesium selenide<\/li>\n<li>sodium oxide<\/li>\n<li>calcium chloride<\/li>\n<li>gallium phosphide<\/li>\n<li>aluminum bromide<\/li>\n<li>ammonium sulfate<\/li>\n<\/ol>\n<\/li>\n<li>Write the formulas of the following compounds:\n<ol style=\"list-style-type: lower-alpha;\">\n<li>lithium carbonate<\/li>\n<li>sodium perchlorate<\/li>\n<li>barium hydroxide<\/li>\n<li>ammonium carbonate<\/li>\n<li>calcium acetate<\/li>\n<li>magnesium phosphate<\/li>\n<li>sodium sulfite<\/li>\n<\/ol>\n<\/li>\n<li>Write the formulas of the following compounds:\n<ol style=\"list-style-type: lower-alpha;\">\n<li>chlorine dioxide<\/li>\n<li>dinitrogen tetraoxide<\/li>\n<li>potassium phosphide<\/li>\n<li>silver(I) sulfide<\/li>\n<li>aluminum nitride<\/li>\n<li>silicon dioxide<\/li>\n<\/ol>\n<\/li>\n<li>Write the formulas of the following compounds:\n<ol style=\"list-style-type: lower-alpha;\">\n<li>barium chloride<\/li>\n<li>magnesium nitride<\/li>\n<li>sulfur dioxide<\/li>\n<li>nitrogen trichloride<\/li>\n<li>dinitrogen trioxide<\/li>\n<li>tin(IV) chloride<\/li>\n<\/ol>\n<\/li>\n<li>Each of the following compounds contains a metal that can exhibit more than one ionic charge. Name these compounds:\n<ol style=\"list-style-type: lower-alpha;\">\n<li>Cr<sub>2<\/sub>O<sub>3 <\/sub><\/li>\n<li>FeCl<sub>2 <\/sub><\/li>\n<li>CrO<sub>3 <\/sub><\/li>\n<li>TiCl<sub>4 <\/sub><\/li>\n<li>CoO<\/li>\n<li>MoS<sub>2<\/sub><\/li>\n<\/ol>\n<\/li>\n<li>Each of the following compounds contains a metal that can exhibit more than one ionic charge. Name these compounds:\n<ol style=\"list-style-type: lower-alpha;\">\n<li>NiCO<sub>3 <\/sub><\/li>\n<li>MoO<sub>3 <\/sub><\/li>\n<li>Co(NO<sub>3<\/sub>)<sub>2 <\/sub><\/li>\n<li>V<sub>2<\/sub>O<sub>5 <\/sub><\/li>\n<li>MnO<sub>2 <\/sub><\/li>\n<li>Fe<sub>2<\/sub>O<sub>3 <\/sub><\/li>\n<\/ol>\n<\/li>\n<li>The following ionic compounds are found in common household products. Write the formulas for each compound:\n<ol style=\"list-style-type: lower-alpha;\">\n<li>potassium phosphate<\/li>\n<li>copper(II) sulfate<\/li>\n<li>calcium chloride<\/li>\n<li>titanium(II) oxide<\/li>\n<li>ammonium nitrate<\/li>\n<li>sodium sulfate<\/li>\n<\/ol>\n<\/li>\n<li>The following ionic compounds are found in common household products. Name each of the compounds:\n<ol style=\"list-style-type: lower-alpha;\">\n<li>Ca(H<sub>2<\/sub>PO<sub>4<\/sub>)<sub>2 <\/sub><\/li>\n<li>FeSO<sub>4 <\/sub><\/li>\n<li>CaCO<sub>3 <\/sub><\/li>\n<li>MgO<\/li>\n<li>NaNO<sub>2 <\/sub><\/li>\n<li>KI<\/li>\n<\/ol>\n<\/li>\n<\/ol>\n<div class=\"qa-wrapper\" style=\"display: block\"><span class=\"show-answer collapsed\" style=\"cursor: pointer\" data-target=\"q708113\">Show Selected Answers<\/span><\/p>\n<div id=\"q708113\" class=\"hidden-answer\" style=\"display: none\">\n<p>1. (a) cesium chloride; (b) barium oxide; (c) potassium sulfide; (d) beryllium chloride; (e) aluminum fluoride<\/p>\n<p>3. (a) RbBr; (b) MgSe; (c) Na<sub>2<\/sub>O; (d) CaCl<sub>2<\/sub>; (e) GaP; (f) AlBr<sub>3<\/sub>; (g) (NH<sub>4<\/sub>)<sub>2<\/sub>SO<sub>4<\/sub><\/p>\n<p>5. (a) ClO<sub>2<\/sub>; (b) N<sub>2<\/sub>O<sub>4<\/sub>; (c) K<sub>3<\/sub>P; (d) Ag<sub>2<\/sub>S; (e) AlN; (f) SiO<sub>2<\/sub><\/p>\n<p>7. (a) chromium(III) oxide; (b) iron(II) chloride; (c) chromium(VI) oxide; (d) titanium(IV) chloride; (e) cobalt(II) oxide; (f) molybdenum(IV) sulfide<\/p>\n<p>9. (a) K<sub>3<\/sub>PO<sub>4<\/sub>; (b) CuSO<sub>4<\/sub>; (c) CaCl<sub>2<\/sub>; (d) TiO<sub>2<\/sub>; (e) NH<sub>4<\/sub>NO<sub>3<\/sub>; (f) Na<sub>2<\/sub>SO<sub>4<\/sub><\/p>\n<\/div>\n<\/div>\n<\/div>\n<h2>Glossary<\/h2>\n<p><strong>binary compound: <\/strong>compound containing two different elements.<\/p>\n<p><strong>nomenclature: <\/strong>system of rules for naming objects of interest<\/p>\n","protected":false},"author":6181,"menu_order":4,"template":"","meta":{"_candela_citation":"[]","CANDELA_OUTCOMES_GUID":"","pb_show_title":"on","pb_short_title":"","pb_subtitle":"","pb_authors":[],"pb_section_license":""},"chapter-type":[],"contributor":[],"license":[],"class_list":["post-1389","chapter","type-chapter","status-publish","hentry"],"part":1128,"_links":{"self":[{"href":"https:\/\/courses.lumenlearning.com\/suny-mcc-introductorychemistry\/wp-json\/pressbooks\/v2\/chapters\/1389","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/courses.lumenlearning.com\/suny-mcc-introductorychemistry\/wp-json\/pressbooks\/v2\/chapters"}],"about":[{"href":"https:\/\/courses.lumenlearning.com\/suny-mcc-introductorychemistry\/wp-json\/wp\/v2\/types\/chapter"}],"author":[{"embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/suny-mcc-introductorychemistry\/wp-json\/wp\/v2\/users\/6181"}],"version-history":[{"count":13,"href":"https:\/\/courses.lumenlearning.com\/suny-mcc-introductorychemistry\/wp-json\/pressbooks\/v2\/chapters\/1389\/revisions"}],"predecessor-version":[{"id":1973,"href":"https:\/\/courses.lumenlearning.com\/suny-mcc-introductorychemistry\/wp-json\/pressbooks\/v2\/chapters\/1389\/revisions\/1973"}],"part":[{"href":"https:\/\/courses.lumenlearning.com\/suny-mcc-introductorychemistry\/wp-json\/pressbooks\/v2\/parts\/1128"}],"metadata":[{"href":"https:\/\/courses.lumenlearning.com\/suny-mcc-introductorychemistry\/wp-json\/pressbooks\/v2\/chapters\/1389\/metadata\/"}],"wp:attachment":[{"href":"https:\/\/courses.lumenlearning.com\/suny-mcc-introductorychemistry\/wp-json\/wp\/v2\/media?parent=1389"}],"wp:term":[{"taxonomy":"chapter-type","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/suny-mcc-introductorychemistry\/wp-json\/pressbooks\/v2\/chapter-type?post=1389"},{"taxonomy":"contributor","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/suny-mcc-introductorychemistry\/wp-json\/wp\/v2\/contributor?post=1389"},{"taxonomy":"license","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/suny-mcc-introductorychemistry\/wp-json\/wp\/v2\/license?post=1389"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}