{"id":1609,"date":"2015-04-22T16:36:22","date_gmt":"2015-04-22T16:36:22","guid":{"rendered":"https:\/\/courses.candelalearning.com\/oschemtemp\/?post_type=chapter&#038;p=1609"},"modified":"2016-08-09T18:00:20","modified_gmt":"2016-08-09T18:00:20","slug":"chemical-nomenclature-1-formula-not-parsing","status":"publish","type":"chapter","link":"https:\/\/courses.lumenlearning.com\/suny-buffstate-chemistryformajorsxmaster\/chapter\/chemical-nomenclature-1-formula-not-parsing\/","title":{"raw":"Chemical Nomenclature","rendered":"Chemical Nomenclature"},"content":{"raw":"<div class=\"bcc-box bcc-highlight\">\r\n<h3>LEARNING OBJECTIVE<\/h3>\r\nBy the end of this section, you will be able to:\r\n<ul>\r\n \t<li>Derive names for common types of inorganic compounds using a systematic approach<\/li>\r\n<\/ul>\r\n<\/div>\r\n<p id=\"fs-idp268117168\"><strong><span data-type=\"term\">Nomenclature<\/span><\/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><span data-type=\"term\">binary compounds<\/span><\/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 <span class=\"no-emphasis\" data-type=\"term\">acids<\/span> (subsequent chapters in this text will focus on these compounds in great detail). 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. The rules for organic compounds, in which carbon is the principle element, will be treated in a later chapter on organic chemistry.<\/p>\r\n\r\n<section id=\"fs-idp268266480\" data-depth=\"1\">\r\n<h2 data-type=\"title\">Ionic Compounds<\/h2>\r\n<p id=\"fs-idp268131792\">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 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>\r\n\r\n<section id=\"fs-idm335792\" data-depth=\"2\">\r\n<h3 data-type=\"title\">Compounds Containing Only Monatomic Ions<\/h3>\r\n<p id=\"fs-idp279143120\">The name of a binary compound containing monatomic ions 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 data-effect=\"italics\">ide<\/em>). Some examples are given in Table 1.<\/p>\r\n\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 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>NaCl, sodium chloride<\/td>\r\n<td>Na<sub>2<\/sub>O, sodium oxide<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>KBr, potassium bromide<\/td>\r\n<td>CdS, cadmium sulfide<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>CaI<sub>2<\/sub>, calcium iodide<\/td>\r\n<td>Mg<sub>3<\/sub>N<sub>2<\/sub>, magnesium nitride<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>CsF, cesium fluoride<\/td>\r\n<td>Ca<sub>3<\/sub>P<sub>2<\/sub>, calcium phosphide<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>LiCl, lithium chloride<\/td>\r\n<td>Al<sub>4<\/sub>C<sub>3<\/sub>, aluminum carbide<\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\n<\/section><section id=\"fs-idp279293712\" data-depth=\"2\">\r\n<h3 data-type=\"title\">Compounds Containing Polyatomic Ions<\/h3>\r\n<p id=\"fs-idp282236928\">Compounds containing polyatomic ions are named similarly to those containing only monatomic ions, except there is no need to change to an \u2013<em data-effect=\"italics\">ide<\/em> ending, since the suffix is already present in the name of the anion. Examples are shown in\u00a0Table 2.<\/p>\r\n\r\n<table id=\"fs-idp279316112\" class=\"span-all\" 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 colspan=\"3\">Table 2. Names of Some Polyatomic Ionic Compounds<\/th>\r\n<\/tr>\r\n<\/thead>\r\n<tbody>\r\n<tr>\r\n<td>KC<sub>2<\/sub>H<sub>3<\/sub>O<sub>2<\/sub>, potassium acetate<\/td>\r\n<td>(NH<sub>4<\/sub>)Cl, ammonium chloride<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>NaHCO<sub>3<\/sub>, sodium bicarbonate<\/td>\r\n<td>CaSO<sub>4<\/sub>, calcium sulfate<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Al<sub>2<\/sub>(CO<sub>3<\/sub>)<sub>3<\/sub>, aluminum carbonate<\/td>\r\n<td>Mg<sub>3<\/sub>(PO<sub>4<\/sub>)<sub>2<\/sub>, magnesium phosphate<\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\n<div id=\"fs-idm337456\" class=\"chemistry everyday-life\" data-type=\"note\">\r\n<div data-type=\"title\"><\/div>\r\n<div class=\"textbox shaded\" data-type=\"title\">\r\n<h3 style=\"text-align: left;\" data-type=\"title\">Ionic Compounds in Your Cabinets<\/h3>\r\n<p id=\"fs-idm70496\">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 3. 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>\r\n\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 3. 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>\r\n<\/section><section id=\"fs-idp282353488\" data-depth=\"2\">\r\n<h3 data-type=\"title\">Compounds Containing a Metal Ion with a Variable Charge<\/h3>\r\n<p id=\"fs-idp282354128\">Most of the transition metals can form two or more cations with different charges. 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+ (see <a href=\".\/chapter\/molecular-and-ionic-compounds-2\/\" target=\"_blank\">Molecular and Ionic Compounds<\/a>), 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\u00a0Table 4.<\/p>\r\n\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 colspan=\"2\">Table 4. Names of Some Transition Metal Ionic Compounds<\/th>\r\n<\/tr>\r\n<tr>\r\n<th>Transition Metal Ionic Compound<\/th>\r\n<th>Name<\/th>\r\n<\/tr>\r\n<\/thead>\r\n<tbody>\r\n<tr>\r\n<td>FeCl<sub>3<\/sub><\/td>\r\n<td>iron(II) chloride<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Hg<sub>2<\/sub>O<\/td>\r\n<td>mercury(I) oxide<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>HgO<\/td>\r\n<td>mercury(II) oxide<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Cu<sub>3<\/sub>(PO<sub>4<\/sub>)<sub>2<\/sub><\/td>\r\n<td>copper(II) phosphate<\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\n<p id=\"fs-idp268391888\">Out-of-date nomenclature used the suffixes \u2013<em data-effect=\"italics\">ic<\/em> and \u2013<em data-effect=\"italics\">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 data-effect=\"italics\">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>\r\n\r\n<div id=\"fs-idm194224\" data-type=\"example\">\r\n<div class=\"textbox shaded\">\r\n<h3>Example 1<\/h3>\r\n<h4 id=\"fs-idm193552\"><strong><span data-type=\"title\">Naming Ionic Compounds<\/span><\/strong><\/h4>\r\nName the following ionic compounds, which contain a metal that can have more than one ionic charge:\r\n<p id=\"fs-idm193056\">(a) Fe<sub>2<\/sub>S<sub>3<\/sub><\/p>\r\n<p id=\"fs-idm341872\">(b) CuSe<\/p>\r\n<p id=\"fs-idm341488\">(c) GaN<\/p>\r\n<p id=\"fs-idm341104\">(d) CrCl<sub>3<\/sub><\/p>\r\n<p id=\"fs-idp156278112\">(e) Ti<sub>2<\/sub>(SO<sub>4<\/sub>)<sub>3<\/sub><\/p>\r\n\r\n<h4 id=\"fs-idp282326320\"><strong><span data-type=\"title\">Solution<\/span><\/strong><\/h4>\r\nThe anions in these compounds have a fixed negative charge (S<sup>2-<\/sup>, Se<sup>2- <\/sup>, N<sup>3-<\/sup>, Cl<sup>-<\/sup>, and [latex]{\\text{SO}}_{4}{}^{2-}[\/latex]), and the compounds must be neutral. Because the total number of positive charges in each compound must equal the total number of negative charges, the positive ions must be Fe<sup>3+<\/sup>, Cu<sup>2+<\/sup>, Ga<sup>3+<\/sup>, Cr<sup>4+<\/sup>, and Ti<sup>3+<\/sup>. These charges are used in the names of the metal ions:\r\n<p id=\"fs-idm104688\">(a) iron(III) sulfide<\/p>\r\n<p id=\"fs-idm104272\">(b) copper(II) selenide<\/p>\r\n<p id=\"fs-idp283457040\">(c) gallium(III) nitride<\/p>\r\n<p id=\"fs-idp283457424\">(d) chromium(III) chloride<\/p>\r\n<p id=\"fs-idp283457808\">(e) titanium(III) sulfate<\/p>\r\n\r\n<h4 id=\"fs-idp283458192\"><strong><span data-type=\"title\">Check Your Learning<\/span><\/strong><\/h4>\r\nWrite the formulas of the following ionic compounds:\r\n<p id=\"fs-idp283458864\">(a) chromium(III) phosphide<\/p>\r\n<p id=\"fs-idp283459248\">(b) mercury(II) sulfide<\/p>\r\n<p id=\"fs-idp268146864\">(c) manganese(II) phosphate<\/p>\r\n<p id=\"fs-idp268147248\">(d) copper(I) oxide<\/p>\r\n<p id=\"fs-idp268147664\">(e) chromium(VI) fluoride<\/p>\r\n\r\n<div id=\"fs-idp268148048\" data-type=\"note\">\r\n<div data-type=\"title\"><\/div>\r\n<div style=\"text-align: right;\" data-type=\"title\"><strong>Answer<\/strong>:\u00a0(a) CrP; (b) HgS; (c) Mn<sub>3<\/sub>(PO<sub>4<\/sub>)<sub>2<\/sub>; (d) Cu<sub>2<\/sub>O; (e) CrF<sub>6<\/sub><\/div>\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<div id=\"fs-idm8768\" class=\"chemistry everyday-life\" data-type=\"note\">\r\n<div class=\"textbox shaded\" data-type=\"title\">\r\n<h3 data-type=\"title\">Erin Brokovich and Chromium Contamination<\/h3>\r\n<p id=\"fs-idm7968\">In the early 1990s, legal file clerk Erin Brockovich (Figure 1) discovered a high rate of serious illnesses in the small town of Hinckley, California. Her investigation eventually linked the illnesses to groundwater contaminated by Cr(VI) used by Pacific Gas &amp; Electric (PG&amp;E) to fight corrosion in a nearby natural gas pipeline. As dramatized in the film <em data-effect=\"italics\">Erin Brokovich<\/em> (for which Julia Roberts won an Oscar), Erin and lawyer Edward Masry sued PG&amp;E for contaminating the water near Hinckley in 1993. The settlement they won in 1996\u2014$333 million\u2014was the largest amount ever awarded for a direct-action lawsuit in the US at that time.<\/p>\r\n\r\n\r\n[caption id=\"\" align=\"alignnone\" width=\"881\"]<img src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/887\/2015\/04\/23211107\/CNX_Chem_02_07_ErinBrocko1.jpg\" alt=\"Figure A shows a photo of Erin Brockovich. Figure B shows a 3-D ball-and-stick model of chromate. Chromate has a chromium atom at its center that forms bonds with four oxygen atoms each. Two of the oxygen atoms form single bonds with the chromium atom while the other two form double bonds each. The structure of dichromate consists of two chromate ions that are bonded and share one of their oxygen atoms to which each chromate atom has a single bond.\" width=\"881\" height=\"328\" data-media-type=\"image\/jpeg\" \/> Figure 1. (a) Erin Brockovich found that Cr(IV), used by PG&amp;E, had contaminated the Hinckley, California, water supply. (b) The Cr(VI) ion is often present in water as the polyatomic ions chromate, CrO<sub>4<\/sub><sup>2\u2212<\/sup> (left), and dichromate, Cr<sub>2<\/sub>O<sub>7<\/sub><sup>2\u2212<\/sup> (right).[\/caption]\r\n<p id=\"fs-idp279149248\">Chromium compounds are widely used in industry, such as for chrome plating, in dye-making, as preservatives, and to prevent corrosion in cooling tower water, as occurred near Hinckley. In the environment, chromium exists primarily in either the Cr(III) or Cr(VI) forms. Cr(III), an ingredient of many vitamin and nutritional supplements, forms compounds that are not very soluble in water, and it has low toxicity. But Cr(VI) is much more toxic and forms compounds that are reasonably soluble in water. Exposure to small amounts of Cr(VI) can lead to damage of the respiratory, gastrointestinal, and immune systems, as well as the kidneys, liver, blood, and skin.<\/p>\r\n<p id=\"fs-idp279150320\">Despite cleanup efforts, Cr(VI) groundwater contamination remains a problem in Hinckley and other locations across the globe. A 2010 study by the Environmental Working Group found that of 35 US cities tested, 31 had higher levels of Cr(VI) in their tap water than the public health goal of 0.02 parts per billion set by the California Environmental Protection Agency.<\/p>\r\n\r\n<\/div>\r\n<\/div>\r\n<\/section><\/section><section id=\"fs-idp279151472\" data-depth=\"1\">\r\n<h2 data-type=\"title\">Molecular (Covalent) Compounds<\/h2>\r\n<p id=\"fs-idp268164784\">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>\r\n\r\n<section id=\"fs-idp268165696\" data-depth=\"2\">\r\n<h3 data-type=\"title\">Compounds Composed of Two Elements<\/h3>\r\n<p id=\"fs-idp268166336\">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 data-effect=\"italics\">ide<\/em>. The numbers of atoms of each element are designated by the Greek prefixes shown in Table 5.<\/p>\r\n\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\n<p id=\"fs-idm325632\">When only one atom of the first element is present, the prefix <em data-effect=\"italics\">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 data-effect=\"italics\">a<\/em> in the Greek prefix is usually dropped. Some other examples are shown in Table 6.<\/p>\r\n\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\n<p id=\"fs-idm207744\">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.) You should commit to memory the common names of compounds as you encounter them.<\/p>\r\n\r\n<div id=\"fs-idm206240\" data-type=\"example\">\r\n<div class=\"textbox shaded\">\r\n<h3>Example 2<\/h3>\r\n<h4><strong>Naming Covalent Compounds<\/strong><\/h4>\r\n<p id=\"fs-idm205600\">Name the following covalent compounds:<\/p>\r\n<p id=\"fs-idm205216\">(a) SF<sub>6<\/sub><\/p>\r\n<p id=\"fs-idp268178064\">(b) N<sub>2<\/sub>O<sub>3<\/sub><\/p>\r\n<p id=\"fs-idp268179088\">(c) Cl<sub>2<\/sub>O<sub>7<\/sub><\/p>\r\n<p id=\"fs-idp268180112\">(d) P<sub>4<\/sub>O<sub>6<\/sub><\/p>\r\n\r\n<h4 id=\"fs-idp268181136\"><strong><span data-type=\"title\">Solution<\/span><\/strong><\/h4>\r\nBecause these compounds consist solely of nonmetals, we use prefixes to designate the number of atoms of each element:\r\n<p id=\"fs-idm335200\">(a) sulfur hexafluoride<\/p>\r\n<p id=\"fs-idm334784\">(b) dinitrogen trioxide<\/p>\r\n<p id=\"fs-idm334368\">(c) dichlorine heptoxide<\/p>\r\n<p id=\"fs-idm333984\">(d) tetraphosphorus hexoxide<\/p>\r\n\r\n<h4 id=\"fs-idm333600\"><strong><span data-type=\"title\">Check Your Learning<\/span><\/strong><\/h4>\r\nWrite the formulas for the following compounds:\r\n<p id=\"fs-idm332928\">(a) phosphorus pentachloride<\/p>\r\n<p id=\"fs-idm332544\">(b) dinitrogen monoxide<\/p>\r\n<p id=\"fs-idp283400752\">(c) iodine heptafluoride<\/p>\r\n<p id=\"fs-idp283401136\">(d) carbon tetrachloride<\/p>\r\n\r\n<div id=\"fs-idp283401520\" data-type=\"note\">\r\n<div data-type=\"title\"><\/div>\r\n<div style=\"text-align: right;\" data-type=\"title\"><strong>Answer<\/strong>:\u00a0(a) PCl<sub>5<\/sub>; (b) N<sub>2<\/sub>O; (c) IF<sub>7<\/sub>; (d) CCl<sub>4<\/sub><\/div>\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<div id=\"fs-idp283404080\" class=\"chemistry link-to-learning textbox\" data-type=\"note\">\r\n<p id=\"fs-idp268192304\">The <a href=\"http:\/\/chemsite.lsrhs.net\/FlashMedia\/html\/compoundsAll.html\" target=\"_blank\">Chemiste\u00a0website<\/a> provides practice with naming chemical compounds and writing chemical formulas. You can choose binary, polyatomic, and variable charge ionic compounds, as well as molecular compounds.<\/p>\r\n\r\n<\/div>\r\n<\/section><section id=\"fs-idp268193776\" data-depth=\"2\">\r\n<h3 data-type=\"title\">Binary Acids<\/h3>\r\n<p id=\"fs-idp282238096\">Some compounds containing hydrogen are members of an important class of substances known as acids. The chemistry of these compounds is explored in more detail in later chapters of this text, but for now, it will suffice to note that many acids release hydrogen ions, H<sup>+<\/sup>, when dissolved in water. To denote this distinct chemical property, a mixture of water with an acid is given a name derived from the compound\u2019s name. If the compound is a <strong><span data-type=\"term\">binary acid<\/span><\/strong> (comprised of hydrogen and one other nonmetallic element):<\/p>\r\n\r\n<ol id=\"fs-idp282239904\" data-number-style=\"arabic\">\r\n \t<li>The word \u201chydrogen\u201d is changed to the prefix <em data-effect=\"italics\">hydro-<\/em><\/li>\r\n \t<li>The other nonmetallic element name is modified by adding the suffix -<em data-effect=\"italics\">ic<\/em><\/li>\r\n \t<li>The word \u201cacid\u201d is added as a second word<\/li>\r\n<\/ol>\r\n<p id=\"fs-idm109568\">For example, when the gas HCl (hydrogen chloride) is dissolved in water, the solution is called <em data-effect=\"italics\">hydrochloric acid<\/em>. Several other examples of this nomenclature are shown in Table 7.<\/p>\r\n\r\n<table id=\"fs-idp272649888\" class=\"span-all\" summary=\"The names of simple acids included in this table are: H F gas, which is hydrogen fluoride, H C l gas which is hydrogen chloride, H B r gas which is hydrogen bromide, H I gas which is hydrogen iodide, H subscript 2 S gas which is hydrogen sulfide, H F aqueous which is hydrofluoric acid, H C l aqueous which is hydrochloric acid, H B r aqueous which is hydrobromic acid, H I aqueous which is hydroiodic acid, and H subscript 2 S aqueous which is hydrosulfuric acid.\">\r\n<thead>\r\n<tr>\r\n<th colspan=\"2\">Table 7. Names of Some Simple Acids<\/th>\r\n<\/tr>\r\n<tr>\r\n<th>Name of Gas<\/th>\r\n<th>Name of Acid<\/th>\r\n<\/tr>\r\n<\/thead>\r\n<tbody>\r\n<tr>\r\n<td>HF(<em data-effect=\"italics\">g<\/em>), hydrogen fluoride<\/td>\r\n<td>HF(<em data-effect=\"italics\">aq<\/em>), hydrofluoric acid<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>HCl(<em data-effect=\"italics\">g<\/em>), hydrogen chloride<\/td>\r\n<td>HCl(<em data-effect=\"italics\">aq<\/em>), hydrochloric acid<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>HBr(<em data-effect=\"italics\">g<\/em>), hydrogen bromide<\/td>\r\n<td>HBr(<em data-effect=\"italics\">aq<\/em>), hydrobromic acid<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>HI(<em data-effect=\"italics\">g<\/em>), hydrogen iodide<\/td>\r\n<td>HI(<em data-effect=\"italics\">aq<\/em>), hydroiodic acid<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>H<sub>2<\/sub>S(<em data-effect=\"italics\">g<\/em>), hydrogen sulfide<\/td>\r\n<td>H<sub>2<\/sub>S(<em data-effect=\"italics\">aq<\/em>), hydrosulfuric acid<\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\n<\/section><section id=\"fs-idp268349296\" data-depth=\"2\">\r\n<h3 data-type=\"title\">Oxyacids<\/h3>\r\n<p id=\"fs-idp279162704\">Many compounds containing three or more elements (such as organic compounds or coordination compounds) are subject to specialized nomenclature rules that you will learn later. However, we will briefly discuss the important compounds known as <strong><span data-type=\"term\">oxyacids<\/span><\/strong>, compounds that contain hydrogen, oxygen, and at least one other element, and are bonded in such a way as to impart acidic properties to the compound (you will learn the details of this in a later chapter). Typical oxyacids consist of hydrogen combined with a polyatomic, oxygen-containing ion. To name oxyacids:<\/p>\r\n\r\n<ol id=\"fs-idp279164064\" data-number-style=\"arabic\">\r\n \t<li>Omit \u201chydrogen\u201d<\/li>\r\n \t<li>Start with the root name of the anion<\/li>\r\n \t<li>Replace \u2013<em data-effect=\"italics\">ate<\/em> with \u2013<em data-effect=\"italics\">ic<\/em>, or \u2013<em data-effect=\"italics\">ite<\/em> with \u2013<em data-effect=\"italics\">ous<\/em><\/li>\r\n \t<li>Add \u201cacid\u201d<\/li>\r\n<\/ol>\r\n<p id=\"fs-idp282461232\">For example, consider H<sub>2<\/sub>CO<sub>3<\/sub> (which you might be tempted to call \u201chydrogen carbonate\u201d). To name this correctly, \u201chydrogen\u201d is omitted; the \u2013<em data-effect=\"italics\">ate<\/em> of carbonate is replace with \u2013<em data-effect=\"italics\">ic<\/em>; and acid is added\u2014so its name is carbonic acid. Other examples are given in Table 8. There are some exceptions to the general naming method (e.g., H<sub>2<\/sub>SO<sub>4<\/sub> is called sulfuric acid, not sulfic acid, and H<sub>2<\/sub>SO<sub>3<\/sub> is sulfurous, not sulfous, acid).<\/p>\r\n\r\n<table id=\"fs-idp268340336\" class=\"span-all\" summary=\"This table has three columns labeled \u201cformula\u201d, \u201canion name\u201d, and \u201cacid name\u201d. H C subscript 2 H subscript 3 O subscript 2 is named acetate or acetic acid. H N O subscript 3 is named nitrate or nitric acid. H N O subscript 2 is named nitrite or nitrous acid, H C l O subscript 4 is named perchlorate or perchloric acid. H subscript 2 C O subscript 3 is named carbonate or carbonic acid. H subscript 2 S O subscript 4 is named sulfate or sulfuric acid. H subscript 2 S O subscript 3 is named sulfite or sulfurous acid. H subscript 3 P O subscript 4 is named phosphate or phosphoric acid.\">\r\n<thead>\r\n<tr>\r\n<th colspan=\"3\">Table 8. Names of Common Oxyacids<\/th>\r\n<\/tr>\r\n<tr>\r\n<th>Formula<\/th>\r\n<th>Anion Name<\/th>\r\n<th>Acid Name<\/th>\r\n<\/tr>\r\n<\/thead>\r\n<tbody>\r\n<tr>\r\n<td>HC<sub>2<\/sub>H<sub>3<\/sub>O<sub>2<\/sub><\/td>\r\n<td>acetate<\/td>\r\n<td>acetic acid<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>HNO<sub>3<\/sub><\/td>\r\n<td>nitrate<\/td>\r\n<td>nitric acid<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>HNO<sub>2<\/sub><\/td>\r\n<td>nitrite<\/td>\r\n<td>nitrous acid<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>HClO<sub>4<\/sub><\/td>\r\n<td>perchlorate<\/td>\r\n<td>perchloric acid<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>H<sub>2<\/sub>CO<sub>3<\/sub><\/td>\r\n<td>carbonate<\/td>\r\n<td>carbonic acid<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>H<sub>2<\/sub>SO<sub>4<\/sub><\/td>\r\n<td>sulfate<\/td>\r\n<td>sulfuric acid<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>H<sub>2<\/sub>SO<sub>3<\/sub><\/td>\r\n<td>sulfite<\/td>\r\n<td>sulfurous acid<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>H<sub>3<\/sub>PO<sub>4<\/sub><\/td>\r\n<td>phosphate<\/td>\r\n<td>phosphoric acid<\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\n<section id=\"fs-idm40478192\" class=\"summary\" data-depth=\"1\">\r\n<div id=\"post-355\" class=\"post-355 chapter type-chapter status-publish hentry type-1\">\r\n<div class=\"entry-content\">\r\n<div class=\"im_section\">\r\n<div class=\"im_section\">\r\n<div id=\"mclean-ch03_s01_s02_n01\" class=\"im_key_takeaways im_editable im_block\">\r\n<div class=\"bcc-box bcc-success\">\r\n<h2>Key Concepts and Summary<\/h2>\r\n<section>\r\n<div data-type=\"note\">\r\n<p id=\"fs-idp236281408\">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 data-effect=\"italics\">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. 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. Acids are an important class of compounds containing hydrogen and having special nomenclature rules. Binary acids are named using the prefix <em data-effect=\"italics\">hydro-<\/em>, changing the \u2013<em data-effect=\"italics\">ide<\/em> suffix to \u2013<em data-effect=\"italics\">ic<\/em>, and adding \u201cacid;\u201d HCl is hydrochloric acid. Oxyacids are named by changing the ending of the anion to \u2013<em data-effect=\"italics\">ic<\/em>, and adding \u201cacid;\u201d H<sub>2<\/sub>CO<sub>3<\/sub> is carbonic acid.<\/p>\r\n\r\n<\/div>\r\n<\/section><\/div>\r\n<div class=\"bcc-box bcc-info\">\r\n<h3>Chemistry End of Chapter Exercises<\/h3>\r\n<div id=\"fs-idp282297472\" data-type=\"exercise\">\r\n<div id=\"fs-idp282297728\" data-type=\"problem\">\r\n<ol>\r\n \t<li id=\"fs-idp282297984\">Name the following compounds:\r\n<ol>\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 \u00a0<\/sub><\/li>\r\n \t<li>HBr<\/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>\r\n \t<li>NaF<\/li>\r\n \t<li>Rb<sub>2<\/sub>O<\/li>\r\n \t<li>BCl<sub>3 \u00a0<\/sub><\/li>\r\n \t<li>H<sub>2<\/sub>Se<\/li>\r\n \t<li>P<sub>4<\/sub>O<sub>6 \u00a0<\/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>\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>hydrogen fluoride<\/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>\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>sulfuric acid<\/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>\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>\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>\r\n \t<li>Cr<sub>2<\/sub>O<sub>3 \u00a0<\/sub><\/li>\r\n \t<li>FeCl<sub>2 \u00a0<\/sub><\/li>\r\n \t<li>CrO<sub>3 \u00a0<\/sub><\/li>\r\n \t<li>TiCl<sub>4 \u00a0<\/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>\r\n \t<li>NiCO<sub>3 \u00a0<\/sub><\/li>\r\n \t<li>MoO<sub>3 \u00a0<\/sub><\/li>\r\n \t<li>Co(NO<sub>3<\/sub>)<sub>2 \u00a0<\/sub><\/li>\r\n \t<li>V<sub>2<\/sub>O<sub>5 \u00a0<\/sub><\/li>\r\n \t<li>MnO<sub>2\u00a0<\/sub><\/li>\r\n \t<li>Fe<sub>2<\/sub>O<sub>3\u00a0<\/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>\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 dioxide<\/li>\r\n \t<li>ammonium nitrate<\/li>\r\n \t<li>sodium bisulfate (the common name for sodium hydrogen 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>\r\n \t<li>Ca(H<sub>2<\/sub>PO<sub>4<\/sub>)<sub>2\u00a0<\/sub><\/li>\r\n \t<li>FeSO<sub>4\u00a0<\/sub><\/li>\r\n \t<li>CaCO<sub>3\u00a0<\/sub><\/li>\r\n \t<li>MgO<\/li>\r\n \t<li>NaNO<sub>2 \u00a0<\/sub><\/li>\r\n \t<li>KI<\/li>\r\n<\/ol>\r\n<\/li>\r\n \t<li>What are the IUPAC names of the following compounds?\r\n<ol>\r\n \t<li>manganese dioxide<\/li>\r\n \t<li>mercurous chloride (Hg<sub>2<\/sub>Cl<sub>2<\/sub>)<\/li>\r\n \t<li>ferric nitrate [Fe(NO<sub>3<\/sub>)<sub>3<\/sub>]<\/li>\r\n \t<li>titanium tetrachloride<\/li>\r\n \t<li>cupric bromide (CuBr<sub>2<\/sub>)<\/li>\r\n<\/ol>\r\n<\/li>\r\n<\/ol>\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<div id=\"post-355\" class=\"post-355 chapter type-chapter status-publish hentry type-1\">\r\n<div class=\"entry-content\">\r\n<div class=\"im_section\">\r\n<div class=\"im_section\">\r\n<div id=\"mclean-ch03_s01_s02_n01\" class=\"im_key_takeaways im_editable im_block\">\r\n<div class=\"bcc-box bcc-info\">\r\n<h4>Selected Answers<\/h4>\r\n1.\u00a0(a) cesium chloride; (b) barium oxide; (c) potassium sulfide; (d) beryllium chloride; (e) hydrogen bromide; (f) aluminum fluoride\r\n\r\n3.\u00a0(a) RbBr; (b) MgSe; (c) Na<sub>2<\/sub>O; (d) CaCl<sub>2<\/sub>; (e) HF; (f) GaP; (g) AlBr<sub>3<\/sub>; (h) (NH<sub>4<\/sub>)<sub>2<\/sub>SO<sub>4<\/sub>\r\n\r\n5.\u00a0(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.\u00a0(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.\u00a0(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) NaHSO<sub>4<\/sub>\r\n\r\n11. (a) manganese(IV) oxide; (b) mercury(I) chloride; (c) iron(III) nitrate; (d) titanium(IV) chloride; (e) copper(II) bromide\r\n\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<\/section>\r\n<div class=\"bcc-box bcc-success\"><section id=\"glossary\">\r\n<h3>Glossary<\/h3>\r\n<div data-type=\"definition\">\r\n<div id=\"fs-idm8143856\" data-type=\"definition\">\r\n<p data-type=\"definition\"><strong><span data-type=\"term\">binary acid\r\n<\/span><\/strong>compound that contains hydrogen and one other element, bonded in a way that imparts acidic properties to the compound (ability to release H<sup>+<\/sup> ions when dissolved in water)<\/p>\r\n<p data-type=\"definition\"><strong><span data-type=\"term\">binary compound\r\n<\/span><\/strong>compound containing two different elements.<\/p>\r\n<p data-type=\"definition\"><strong><span data-type=\"term\">nomenclature\r\n<\/span><\/strong>system of rules for naming objects of interest<\/p>\r\n\r\n<div id=\"fs-idp282228224\" data-type=\"definition\">\r\n\r\n<strong><span data-type=\"term\">oxyacid\r\n<\/span><\/strong>compound that contains hydrogen, oxygen, and one other element, bonded in a way that imparts acidic properties to the compound (ability to release H<sup>+<\/sup> ions when dissolved in water)\r\n\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<\/section><\/div>\r\n<\/section><\/section>","rendered":"<div class=\"bcc-box bcc-highlight\">\n<h3>LEARNING OBJECTIVE<\/h3>\n<p>By the end of this section, you will be able to:<\/p>\n<ul>\n<li>Derive names for common types of inorganic compounds using a systematic approach<\/li>\n<\/ul>\n<\/div>\n<p id=\"fs-idp268117168\"><strong><span data-type=\"term\">Nomenclature<\/span><\/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><span data-type=\"term\">binary compounds<\/span><\/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 <span class=\"no-emphasis\" data-type=\"term\">acids<\/span> (subsequent chapters in this text will focus on these compounds in great detail). 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. The rules for organic compounds, in which carbon is the principle element, will be treated in a later chapter on organic chemistry.<\/p>\n<section id=\"fs-idp268266480\" data-depth=\"1\">\n<h2 data-type=\"title\">Ionic Compounds<\/h2>\n<p id=\"fs-idp268131792\">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 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<section id=\"fs-idm335792\" data-depth=\"2\">\n<h3 data-type=\"title\">Compounds Containing Only Monatomic Ions<\/h3>\n<p id=\"fs-idp279143120\">The name of a binary compound containing monatomic ions 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 data-effect=\"italics\">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 colspan=\"2\">Table 1. Names of Some Ionic Compounds<\/th>\n<\/tr>\n<\/thead>\n<tbody>\n<tr>\n<td>NaCl, sodium chloride<\/td>\n<td>Na<sub>2<\/sub>O, sodium oxide<\/td>\n<\/tr>\n<tr>\n<td>KBr, potassium bromide<\/td>\n<td>CdS, cadmium sulfide<\/td>\n<\/tr>\n<tr>\n<td>CaI<sub>2<\/sub>, calcium iodide<\/td>\n<td>Mg<sub>3<\/sub>N<sub>2<\/sub>, magnesium nitride<\/td>\n<\/tr>\n<tr>\n<td>CsF, cesium fluoride<\/td>\n<td>Ca<sub>3<\/sub>P<sub>2<\/sub>, calcium phosphide<\/td>\n<\/tr>\n<tr>\n<td>LiCl, lithium chloride<\/td>\n<td>Al<sub>4<\/sub>C<sub>3<\/sub>, aluminum carbide<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<\/section>\n<section id=\"fs-idp279293712\" data-depth=\"2\">\n<h3 data-type=\"title\">Compounds Containing Polyatomic Ions<\/h3>\n<p id=\"fs-idp282236928\">Compounds containing polyatomic ions are named similarly to those containing only monatomic ions, except there is no need to change to an \u2013<em data-effect=\"italics\">ide<\/em> ending, since the suffix is already present in the name of the anion. Examples are shown in\u00a0Table 2.<\/p>\n<table id=\"fs-idp279316112\" class=\"span-all\" 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 colspan=\"3\">Table 2. Names of Some Polyatomic Ionic Compounds<\/th>\n<\/tr>\n<\/thead>\n<tbody>\n<tr>\n<td>KC<sub>2<\/sub>H<sub>3<\/sub>O<sub>2<\/sub>, potassium acetate<\/td>\n<td>(NH<sub>4<\/sub>)Cl, ammonium chloride<\/td>\n<\/tr>\n<tr>\n<td>NaHCO<sub>3<\/sub>, sodium bicarbonate<\/td>\n<td>CaSO<sub>4<\/sub>, calcium sulfate<\/td>\n<\/tr>\n<tr>\n<td>Al<sub>2<\/sub>(CO<sub>3<\/sub>)<sub>3<\/sub>, aluminum carbonate<\/td>\n<td>Mg<sub>3<\/sub>(PO<sub>4<\/sub>)<sub>2<\/sub>, magnesium phosphate<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<div id=\"fs-idm337456\" class=\"chemistry everyday-life\" data-type=\"note\">\n<div data-type=\"title\"><\/div>\n<div class=\"textbox shaded\" data-type=\"title\">\n<h3 style=\"text-align: left;\" data-type=\"title\">Ionic Compounds in Your Cabinets<\/h3>\n<p id=\"fs-idm70496\">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 3. 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 3. 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>\n<\/section>\n<section id=\"fs-idp282353488\" data-depth=\"2\">\n<h3 data-type=\"title\">Compounds Containing a Metal Ion with a Variable Charge<\/h3>\n<p id=\"fs-idp282354128\">Most of the transition metals can form two or more cations with different charges. 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+ (see <a href=\".\/chapter\/molecular-and-ionic-compounds-2\/\" target=\"_blank\">Molecular and Ionic Compounds<\/a>), 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\u00a0Table 4.<\/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 colspan=\"2\">Table 4. Names of Some Transition Metal Ionic Compounds<\/th>\n<\/tr>\n<tr>\n<th>Transition Metal Ionic Compound<\/th>\n<th>Name<\/th>\n<\/tr>\n<\/thead>\n<tbody>\n<tr>\n<td>FeCl<sub>3<\/sub><\/td>\n<td>iron(II) chloride<\/td>\n<\/tr>\n<tr>\n<td>Hg<sub>2<\/sub>O<\/td>\n<td>mercury(I) oxide<\/td>\n<\/tr>\n<tr>\n<td>HgO<\/td>\n<td>mercury(II) oxide<\/td>\n<\/tr>\n<tr>\n<td>Cu<sub>3<\/sub>(PO<sub>4<\/sub>)<sub>2<\/sub><\/td>\n<td>copper(II) phosphate<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<p id=\"fs-idp268391888\">Out-of-date nomenclature used the suffixes \u2013<em data-effect=\"italics\">ic<\/em> and \u2013<em data-effect=\"italics\">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 data-effect=\"italics\">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<div id=\"fs-idm194224\" data-type=\"example\">\n<div class=\"textbox shaded\">\n<h3>Example 1<\/h3>\n<h4 id=\"fs-idm193552\"><strong><span data-type=\"title\">Naming Ionic Compounds<\/span><\/strong><\/h4>\n<p>Name the following ionic compounds, which contain a metal that can have more than one ionic charge:<\/p>\n<p id=\"fs-idm193056\">(a) Fe<sub>2<\/sub>S<sub>3<\/sub><\/p>\n<p id=\"fs-idm341872\">(b) CuSe<\/p>\n<p id=\"fs-idm341488\">(c) GaN<\/p>\n<p id=\"fs-idm341104\">(d) CrCl<sub>3<\/sub><\/p>\n<p id=\"fs-idp156278112\">(e) Ti<sub>2<\/sub>(SO<sub>4<\/sub>)<sub>3<\/sub><\/p>\n<h4 id=\"fs-idp282326320\"><strong><span data-type=\"title\">Solution<\/span><\/strong><\/h4>\n<p>The anions in these compounds have a fixed negative charge (S<sup>2-<\/sup>, Se<sup>2- <\/sup>, N<sup>3-<\/sup>, Cl<sup>&#8211;<\/sup>, and [latex]{\\text{SO}}_{4}{}^{2-}[\/latex]), and the compounds must be neutral. Because the total number of positive charges in each compound must equal the total number of negative charges, the positive ions must be Fe<sup>3+<\/sup>, Cu<sup>2+<\/sup>, Ga<sup>3+<\/sup>, Cr<sup>4+<\/sup>, and Ti<sup>3+<\/sup>. These charges are used in the names of the metal ions:<\/p>\n<p id=\"fs-idm104688\">(a) iron(III) sulfide<\/p>\n<p id=\"fs-idm104272\">(b) copper(II) selenide<\/p>\n<p id=\"fs-idp283457040\">(c) gallium(III) nitride<\/p>\n<p id=\"fs-idp283457424\">(d) chromium(III) chloride<\/p>\n<p id=\"fs-idp283457808\">(e) titanium(III) sulfate<\/p>\n<h4 id=\"fs-idp283458192\"><strong><span data-type=\"title\">Check Your Learning<\/span><\/strong><\/h4>\n<p>Write the formulas of the following ionic compounds:<\/p>\n<p id=\"fs-idp283458864\">(a) chromium(III) phosphide<\/p>\n<p id=\"fs-idp283459248\">(b) mercury(II) sulfide<\/p>\n<p id=\"fs-idp268146864\">(c) manganese(II) phosphate<\/p>\n<p id=\"fs-idp268147248\">(d) copper(I) oxide<\/p>\n<p id=\"fs-idp268147664\">(e) chromium(VI) fluoride<\/p>\n<div id=\"fs-idp268148048\" data-type=\"note\">\n<div data-type=\"title\"><\/div>\n<div style=\"text-align: right;\" data-type=\"title\"><strong>Answer<\/strong>:\u00a0(a) CrP; (b) HgS; (c) Mn<sub>3<\/sub>(PO<sub>4<\/sub>)<sub>2<\/sub>; (d) Cu<sub>2<\/sub>O; (e) CrF<sub>6<\/sub><\/div>\n<\/div>\n<\/div>\n<\/div>\n<div id=\"fs-idm8768\" class=\"chemistry everyday-life\" data-type=\"note\">\n<div class=\"textbox shaded\" data-type=\"title\">\n<h3 data-type=\"title\">Erin Brokovich and Chromium Contamination<\/h3>\n<p id=\"fs-idm7968\">In the early 1990s, legal file clerk Erin Brockovich (Figure 1) discovered a high rate of serious illnesses in the small town of Hinckley, California. Her investigation eventually linked the illnesses to groundwater contaminated by Cr(VI) used by Pacific Gas &amp; Electric (PG&amp;E) to fight corrosion in a nearby natural gas pipeline. As dramatized in the film <em data-effect=\"italics\">Erin Brokovich<\/em> (for which Julia Roberts won an Oscar), Erin and lawyer Edward Masry sued PG&amp;E for contaminating the water near Hinckley in 1993. The settlement they won in 1996\u2014$333 million\u2014was the largest amount ever awarded for a direct-action lawsuit in the US at that time.<\/p>\n<div style=\"width: 891px\" class=\"wp-caption alignnone\"><img loading=\"lazy\" decoding=\"async\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/887\/2015\/04\/23211107\/CNX_Chem_02_07_ErinBrocko1.jpg\" alt=\"Figure A shows a photo of Erin Brockovich. Figure B shows a 3-D ball-and-stick model of chromate. Chromate has a chromium atom at its center that forms bonds with four oxygen atoms each. Two of the oxygen atoms form single bonds with the chromium atom while the other two form double bonds each. The structure of dichromate consists of two chromate ions that are bonded and share one of their oxygen atoms to which each chromate atom has a single bond.\" width=\"881\" height=\"328\" data-media-type=\"image\/jpeg\" \/><\/p>\n<p class=\"wp-caption-text\">Figure 1. (a) Erin Brockovich found that Cr(IV), used by PG&amp;E, had contaminated the Hinckley, California, water supply. (b) The Cr(VI) ion is often present in water as the polyatomic ions chromate, CrO<sub>4<\/sub><sup>2\u2212<\/sup> (left), and dichromate, Cr<sub>2<\/sub>O<sub>7<\/sub><sup>2\u2212<\/sup> (right).<\/p>\n<\/div>\n<p id=\"fs-idp279149248\">Chromium compounds are widely used in industry, such as for chrome plating, in dye-making, as preservatives, and to prevent corrosion in cooling tower water, as occurred near Hinckley. In the environment, chromium exists primarily in either the Cr(III) or Cr(VI) forms. Cr(III), an ingredient of many vitamin and nutritional supplements, forms compounds that are not very soluble in water, and it has low toxicity. But Cr(VI) is much more toxic and forms compounds that are reasonably soluble in water. Exposure to small amounts of Cr(VI) can lead to damage of the respiratory, gastrointestinal, and immune systems, as well as the kidneys, liver, blood, and skin.<\/p>\n<p id=\"fs-idp279150320\">Despite cleanup efforts, Cr(VI) groundwater contamination remains a problem in Hinckley and other locations across the globe. A 2010 study by the Environmental Working Group found that of 35 US cities tested, 31 had higher levels of Cr(VI) in their tap water than the public health goal of 0.02 parts per billion set by the California Environmental Protection Agency.<\/p>\n<\/div>\n<\/div>\n<\/section>\n<\/section>\n<section id=\"fs-idp279151472\" data-depth=\"1\">\n<h2 data-type=\"title\">Molecular (Covalent) Compounds<\/h2>\n<p id=\"fs-idp268164784\">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<section id=\"fs-idp268165696\" data-depth=\"2\">\n<h3 data-type=\"title\">Compounds Composed of Two Elements<\/h3>\n<p id=\"fs-idp268166336\">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 data-effect=\"italics\">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 id=\"fs-idm325632\">When only one atom of the first element is present, the prefix <em data-effect=\"italics\">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 data-effect=\"italics\">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 id=\"fs-idm207744\">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.) You should commit to memory the common names of compounds as you encounter them.<\/p>\n<div id=\"fs-idm206240\" data-type=\"example\">\n<div class=\"textbox shaded\">\n<h3>Example 2<\/h3>\n<h4><strong>Naming Covalent Compounds<\/strong><\/h4>\n<p id=\"fs-idm205600\">Name the following covalent compounds:<\/p>\n<p id=\"fs-idm205216\">(a) SF<sub>6<\/sub><\/p>\n<p id=\"fs-idp268178064\">(b) N<sub>2<\/sub>O<sub>3<\/sub><\/p>\n<p id=\"fs-idp268179088\">(c) Cl<sub>2<\/sub>O<sub>7<\/sub><\/p>\n<p id=\"fs-idp268180112\">(d) P<sub>4<\/sub>O<sub>6<\/sub><\/p>\n<h4 id=\"fs-idp268181136\"><strong><span data-type=\"title\">Solution<\/span><\/strong><\/h4>\n<p>Because these compounds consist solely of nonmetals, we use prefixes to designate the number of atoms of each element:<\/p>\n<p id=\"fs-idm335200\">(a) sulfur hexafluoride<\/p>\n<p id=\"fs-idm334784\">(b) dinitrogen trioxide<\/p>\n<p id=\"fs-idm334368\">(c) dichlorine heptoxide<\/p>\n<p id=\"fs-idm333984\">(d) tetraphosphorus hexoxide<\/p>\n<h4 id=\"fs-idm333600\"><strong><span data-type=\"title\">Check Your Learning<\/span><\/strong><\/h4>\n<p>Write the formulas for the following compounds:<\/p>\n<p id=\"fs-idm332928\">(a) phosphorus pentachloride<\/p>\n<p id=\"fs-idm332544\">(b) dinitrogen monoxide<\/p>\n<p id=\"fs-idp283400752\">(c) iodine heptafluoride<\/p>\n<p id=\"fs-idp283401136\">(d) carbon tetrachloride<\/p>\n<div id=\"fs-idp283401520\" data-type=\"note\">\n<div data-type=\"title\"><\/div>\n<div style=\"text-align: right;\" data-type=\"title\"><strong>Answer<\/strong>:\u00a0(a) PCl<sub>5<\/sub>; (b) N<sub>2<\/sub>O; (c) IF<sub>7<\/sub>; (d) CCl<sub>4<\/sub><\/div>\n<\/div>\n<\/div>\n<\/div>\n<div id=\"fs-idp283404080\" class=\"chemistry link-to-learning textbox\" data-type=\"note\">\n<p id=\"fs-idp268192304\">The <a href=\"http:\/\/chemsite.lsrhs.net\/FlashMedia\/html\/compoundsAll.html\" target=\"_blank\">Chemiste\u00a0website<\/a> provides practice with naming chemical compounds and writing chemical formulas. You can choose binary, polyatomic, and variable charge ionic compounds, as well as molecular compounds.<\/p>\n<\/div>\n<\/section>\n<section id=\"fs-idp268193776\" data-depth=\"2\">\n<h3 data-type=\"title\">Binary Acids<\/h3>\n<p id=\"fs-idp282238096\">Some compounds containing hydrogen are members of an important class of substances known as acids. The chemistry of these compounds is explored in more detail in later chapters of this text, but for now, it will suffice to note that many acids release hydrogen ions, H<sup>+<\/sup>, when dissolved in water. To denote this distinct chemical property, a mixture of water with an acid is given a name derived from the compound\u2019s name. If the compound is a <strong><span data-type=\"term\">binary acid<\/span><\/strong> (comprised of hydrogen and one other nonmetallic element):<\/p>\n<ol id=\"fs-idp282239904\" data-number-style=\"arabic\">\n<li>The word \u201chydrogen\u201d is changed to the prefix <em data-effect=\"italics\">hydro-<\/em><\/li>\n<li>The other nonmetallic element name is modified by adding the suffix &#8211;<em data-effect=\"italics\">ic<\/em><\/li>\n<li>The word \u201cacid\u201d is added as a second word<\/li>\n<\/ol>\n<p id=\"fs-idm109568\">For example, when the gas HCl (hydrogen chloride) is dissolved in water, the solution is called <em data-effect=\"italics\">hydrochloric acid<\/em>. Several other examples of this nomenclature are shown in Table 7.<\/p>\n<table id=\"fs-idp272649888\" class=\"span-all\" summary=\"The names of simple acids included in this table are: H F gas, which is hydrogen fluoride, H C l gas which is hydrogen chloride, H B r gas which is hydrogen bromide, H I gas which is hydrogen iodide, H subscript 2 S gas which is hydrogen sulfide, H F aqueous which is hydrofluoric acid, H C l aqueous which is hydrochloric acid, H B r aqueous which is hydrobromic acid, H I aqueous which is hydroiodic acid, and H subscript 2 S aqueous which is hydrosulfuric acid.\">\n<thead>\n<tr>\n<th colspan=\"2\">Table 7. Names of Some Simple Acids<\/th>\n<\/tr>\n<tr>\n<th>Name of Gas<\/th>\n<th>Name of Acid<\/th>\n<\/tr>\n<\/thead>\n<tbody>\n<tr>\n<td>HF(<em data-effect=\"italics\">g<\/em>), hydrogen fluoride<\/td>\n<td>HF(<em data-effect=\"italics\">aq<\/em>), hydrofluoric acid<\/td>\n<\/tr>\n<tr>\n<td>HCl(<em data-effect=\"italics\">g<\/em>), hydrogen chloride<\/td>\n<td>HCl(<em data-effect=\"italics\">aq<\/em>), hydrochloric acid<\/td>\n<\/tr>\n<tr>\n<td>HBr(<em data-effect=\"italics\">g<\/em>), hydrogen bromide<\/td>\n<td>HBr(<em data-effect=\"italics\">aq<\/em>), hydrobromic acid<\/td>\n<\/tr>\n<tr>\n<td>HI(<em data-effect=\"italics\">g<\/em>), hydrogen iodide<\/td>\n<td>HI(<em data-effect=\"italics\">aq<\/em>), hydroiodic acid<\/td>\n<\/tr>\n<tr>\n<td>H<sub>2<\/sub>S(<em data-effect=\"italics\">g<\/em>), hydrogen sulfide<\/td>\n<td>H<sub>2<\/sub>S(<em data-effect=\"italics\">aq<\/em>), hydrosulfuric acid<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<\/section>\n<section id=\"fs-idp268349296\" data-depth=\"2\">\n<h3 data-type=\"title\">Oxyacids<\/h3>\n<p id=\"fs-idp279162704\">Many compounds containing three or more elements (such as organic compounds or coordination compounds) are subject to specialized nomenclature rules that you will learn later. However, we will briefly discuss the important compounds known as <strong><span data-type=\"term\">oxyacids<\/span><\/strong>, compounds that contain hydrogen, oxygen, and at least one other element, and are bonded in such a way as to impart acidic properties to the compound (you will learn the details of this in a later chapter). Typical oxyacids consist of hydrogen combined with a polyatomic, oxygen-containing ion. To name oxyacids:<\/p>\n<ol id=\"fs-idp279164064\" data-number-style=\"arabic\">\n<li>Omit \u201chydrogen\u201d<\/li>\n<li>Start with the root name of the anion<\/li>\n<li>Replace \u2013<em data-effect=\"italics\">ate<\/em> with \u2013<em data-effect=\"italics\">ic<\/em>, or \u2013<em data-effect=\"italics\">ite<\/em> with \u2013<em data-effect=\"italics\">ous<\/em><\/li>\n<li>Add \u201cacid\u201d<\/li>\n<\/ol>\n<p id=\"fs-idp282461232\">For example, consider H<sub>2<\/sub>CO<sub>3<\/sub> (which you might be tempted to call \u201chydrogen carbonate\u201d). To name this correctly, \u201chydrogen\u201d is omitted; the \u2013<em data-effect=\"italics\">ate<\/em> of carbonate is replace with \u2013<em data-effect=\"italics\">ic<\/em>; and acid is added\u2014so its name is carbonic acid. Other examples are given in Table 8. There are some exceptions to the general naming method (e.g., H<sub>2<\/sub>SO<sub>4<\/sub> is called sulfuric acid, not sulfic acid, and H<sub>2<\/sub>SO<sub>3<\/sub> is sulfurous, not sulfous, acid).<\/p>\n<table id=\"fs-idp268340336\" class=\"span-all\" summary=\"This table has three columns labeled \u201cformula\u201d, \u201canion name\u201d, and \u201cacid name\u201d. H C subscript 2 H subscript 3 O subscript 2 is named acetate or acetic acid. H N O subscript 3 is named nitrate or nitric acid. H N O subscript 2 is named nitrite or nitrous acid, H C l O subscript 4 is named perchlorate or perchloric acid. H subscript 2 C O subscript 3 is named carbonate or carbonic acid. H subscript 2 S O subscript 4 is named sulfate or sulfuric acid. H subscript 2 S O subscript 3 is named sulfite or sulfurous acid. H subscript 3 P O subscript 4 is named phosphate or phosphoric acid.\">\n<thead>\n<tr>\n<th colspan=\"3\">Table 8. Names of Common Oxyacids<\/th>\n<\/tr>\n<tr>\n<th>Formula<\/th>\n<th>Anion Name<\/th>\n<th>Acid Name<\/th>\n<\/tr>\n<\/thead>\n<tbody>\n<tr>\n<td>HC<sub>2<\/sub>H<sub>3<\/sub>O<sub>2<\/sub><\/td>\n<td>acetate<\/td>\n<td>acetic acid<\/td>\n<\/tr>\n<tr>\n<td>HNO<sub>3<\/sub><\/td>\n<td>nitrate<\/td>\n<td>nitric acid<\/td>\n<\/tr>\n<tr>\n<td>HNO<sub>2<\/sub><\/td>\n<td>nitrite<\/td>\n<td>nitrous acid<\/td>\n<\/tr>\n<tr>\n<td>HClO<sub>4<\/sub><\/td>\n<td>perchlorate<\/td>\n<td>perchloric acid<\/td>\n<\/tr>\n<tr>\n<td>H<sub>2<\/sub>CO<sub>3<\/sub><\/td>\n<td>carbonate<\/td>\n<td>carbonic acid<\/td>\n<\/tr>\n<tr>\n<td>H<sub>2<\/sub>SO<sub>4<\/sub><\/td>\n<td>sulfate<\/td>\n<td>sulfuric acid<\/td>\n<\/tr>\n<tr>\n<td>H<sub>2<\/sub>SO<sub>3<\/sub><\/td>\n<td>sulfite<\/td>\n<td>sulfurous acid<\/td>\n<\/tr>\n<tr>\n<td>H<sub>3<\/sub>PO<sub>4<\/sub><\/td>\n<td>phosphate<\/td>\n<td>phosphoric acid<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<section id=\"fs-idm40478192\" class=\"summary\" data-depth=\"1\">\n<div id=\"post-355\" class=\"post-355 chapter type-chapter status-publish hentry type-1\">\n<div class=\"entry-content\">\n<div class=\"im_section\">\n<div class=\"im_section\">\n<div id=\"mclean-ch03_s01_s02_n01\" class=\"im_key_takeaways im_editable im_block\">\n<div class=\"bcc-box bcc-success\">\n<h2>Key Concepts and Summary<\/h2>\n<section>\n<div data-type=\"note\">\n<p id=\"fs-idp236281408\">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 data-effect=\"italics\">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. 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. Acids are an important class of compounds containing hydrogen and having special nomenclature rules. Binary acids are named using the prefix <em data-effect=\"italics\">hydro-<\/em>, changing the \u2013<em data-effect=\"italics\">ide<\/em> suffix to \u2013<em data-effect=\"italics\">ic<\/em>, and adding \u201cacid;\u201d HCl is hydrochloric acid. Oxyacids are named by changing the ending of the anion to \u2013<em data-effect=\"italics\">ic<\/em>, and adding \u201cacid;\u201d H<sub>2<\/sub>CO<sub>3<\/sub> is carbonic acid.<\/p>\n<\/div>\n<\/section>\n<\/div>\n<div class=\"bcc-box bcc-info\">\n<h3>Chemistry End of Chapter Exercises<\/h3>\n<div id=\"fs-idp282297472\" data-type=\"exercise\">\n<div id=\"fs-idp282297728\" data-type=\"problem\">\n<ol>\n<li id=\"fs-idp282297984\">Name the following compounds:\n<ol>\n<li>CsCl<\/li>\n<li>BaO<\/li>\n<li>K<sub>2<\/sub>S<\/li>\n<li>BeCl<sub>2 \u00a0<\/sub><\/li>\n<li>HBr<\/li>\n<li>AlF<sub>3<\/sub><\/li>\n<\/ol>\n<\/li>\n<li>Name the following compounds:\n<ol>\n<li>NaF<\/li>\n<li>Rb<sub>2<\/sub>O<\/li>\n<li>BCl<sub>3 \u00a0<\/sub><\/li>\n<li>H<sub>2<\/sub>Se<\/li>\n<li>P<sub>4<\/sub>O<sub>6 \u00a0<\/sub><\/li>\n<li>ICl<sub>3<\/sub><\/li>\n<\/ol>\n<\/li>\n<li>Write the formulas of the following compounds:\n<ol>\n<li>rubidium bromide<\/li>\n<li>magnesium selenide<\/li>\n<li>sodium oxide<\/li>\n<li>calcium chloride<\/li>\n<li>hydrogen fluoride<\/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>\n<li>lithium carbonate<\/li>\n<li>sodium perchlorate<\/li>\n<li>barium hydroxide<\/li>\n<li>ammonium carbonate<\/li>\n<li>sulfuric acid<\/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>\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>\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>\n<li>Cr<sub>2<\/sub>O<sub>3 \u00a0<\/sub><\/li>\n<li>FeCl<sub>2 \u00a0<\/sub><\/li>\n<li>CrO<sub>3 \u00a0<\/sub><\/li>\n<li>TiCl<sub>4 \u00a0<\/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>\n<li>NiCO<sub>3 \u00a0<\/sub><\/li>\n<li>MoO<sub>3 \u00a0<\/sub><\/li>\n<li>Co(NO<sub>3<\/sub>)<sub>2 \u00a0<\/sub><\/li>\n<li>V<sub>2<\/sub>O<sub>5 \u00a0<\/sub><\/li>\n<li>MnO<sub>2\u00a0<\/sub><\/li>\n<li>Fe<sub>2<\/sub>O<sub>3\u00a0<\/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>\n<li>potassium phosphate<\/li>\n<li>copper(II) sulfate<\/li>\n<li>calcium chloride<\/li>\n<li>titanium dioxide<\/li>\n<li>ammonium nitrate<\/li>\n<li>sodium bisulfate (the common name for sodium hydrogen 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>\n<li>Ca(H<sub>2<\/sub>PO<sub>4<\/sub>)<sub>2\u00a0<\/sub><\/li>\n<li>FeSO<sub>4\u00a0<\/sub><\/li>\n<li>CaCO<sub>3\u00a0<\/sub><\/li>\n<li>MgO<\/li>\n<li>NaNO<sub>2 \u00a0<\/sub><\/li>\n<li>KI<\/li>\n<\/ol>\n<\/li>\n<li>What are the IUPAC names of the following compounds?\n<ol>\n<li>manganese dioxide<\/li>\n<li>mercurous chloride (Hg<sub>2<\/sub>Cl<sub>2<\/sub>)<\/li>\n<li>ferric nitrate [Fe(NO<sub>3<\/sub>)<sub>3<\/sub>]<\/li>\n<li>titanium tetrachloride<\/li>\n<li>cupric bromide (CuBr<sub>2<\/sub>)<\/li>\n<\/ol>\n<\/li>\n<\/ol>\n<\/div>\n<\/div>\n<\/div>\n<\/div>\n<\/div>\n<\/div>\n<\/div>\n<\/div>\n<div id=\"post-355\" class=\"post-355 chapter type-chapter status-publish hentry type-1\">\n<div class=\"entry-content\">\n<div class=\"im_section\">\n<div class=\"im_section\">\n<div id=\"mclean-ch03_s01_s02_n01\" class=\"im_key_takeaways im_editable im_block\">\n<div class=\"bcc-box bcc-info\">\n<h4>Selected Answers<\/h4>\n<p>1.\u00a0(a) cesium chloride; (b) barium oxide; (c) potassium sulfide; (d) beryllium chloride; (e) hydrogen bromide; (f) aluminum fluoride<\/p>\n<p>3.\u00a0(a) RbBr; (b) MgSe; (c) Na<sub>2<\/sub>O; (d) CaCl<sub>2<\/sub>; (e) HF; (f) GaP; (g) AlBr<sub>3<\/sub>; (h) (NH<sub>4<\/sub>)<sub>2<\/sub>SO<sub>4<\/sub><\/p>\n<p>5.\u00a0(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.\u00a0(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.\u00a0(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) NaHSO<sub>4<\/sub><\/p>\n<p>11. (a) manganese(IV) oxide; (b) mercury(I) chloride; (c) iron(III) nitrate; (d) titanium(IV) chloride; (e) copper(II) bromide<\/p>\n<\/div>\n<\/div>\n<\/div>\n<\/div>\n<\/div>\n<\/div>\n<\/section>\n<div class=\"bcc-box bcc-success\">\n<section id=\"glossary\">\n<h3>Glossary<\/h3>\n<div data-type=\"definition\">\n<div id=\"fs-idm8143856\" data-type=\"definition\">\n<p data-type=\"definition\"><strong><span data-type=\"term\">binary acid<br \/>\n<\/span><\/strong>compound that contains hydrogen and one other element, bonded in a way that imparts acidic properties to the compound (ability to release H<sup>+<\/sup> ions when dissolved in water)<\/p>\n<p data-type=\"definition\"><strong><span data-type=\"term\">binary compound<br \/>\n<\/span><\/strong>compound containing two different elements.<\/p>\n<p data-type=\"definition\"><strong><span data-type=\"term\">nomenclature<br \/>\n<\/span><\/strong>system of rules for naming objects of interest<\/p>\n<div id=\"fs-idp282228224\" data-type=\"definition\">\n<p><strong><span data-type=\"term\">oxyacid<br \/>\n<\/span><\/strong>compound that contains hydrogen, oxygen, and one other element, bonded in a way that imparts acidic properties to the compound (ability to release H<sup>+<\/sup> ions when dissolved in water)<\/p>\n<\/div>\n<\/div>\n<\/div>\n<\/section>\n<\/div>\n<\/section>\n<\/section>\n\n\t\t\t <section class=\"citations-section\" role=\"contentinfo\">\n\t\t\t <h3>Candela Citations<\/h3>\n\t\t\t\t\t <div>\n\t\t\t\t\t\t <div id=\"citation-list-1609\">\n\t\t\t\t\t\t\t <div class=\"licensing\"><div class=\"license-attribution-dropdown-subheading\">CC licensed content, Shared previously<\/div><ul class=\"citation-list\"><li>Chemistry. <strong>Provided by<\/strong>: OpenStax College. <strong>Located at<\/strong>: <a target=\"_blank\" href=\"http:\/\/openstaxcollege.org\">http:\/\/openstaxcollege.org<\/a>. <strong>License<\/strong>: <em><a target=\"_blank\" rel=\"license\" href=\"https:\/\/creativecommons.org\/licenses\/by\/4.0\/\">CC BY: Attribution<\/a><\/em>. <strong>License Terms<\/strong>: Download for free at https:\/\/openstaxcollege.org\/textbooks\/chemistry\/get<\/li><\/ul><\/div>\n\t\t\t\t\t\t <\/div>\n\t\t\t\t\t <\/div>\n\t\t\t <\/section>","protected":false},"author":17,"menu_order":14,"template":"","meta":{"_candela_citation":"[{\"type\":\"cc\",\"description\":\"Chemistry\",\"author\":\"\",\"organization\":\"OpenStax College\",\"url\":\"http:\/\/openstaxcollege.org\",\"project\":\"\",\"license\":\"cc-by\",\"license_terms\":\"Download for free at https:\/\/openstaxcollege.org\/textbooks\/chemistry\/get\"}]","CANDELA_OUTCOMES_GUID":"","pb_show_title":"on","pb_short_title":"","pb_subtitle":"","pb_authors":[],"pb_section_license":""},"chapter-type":[],"contributor":[],"license":[],"class_list":["post-1609","chapter","type-chapter","status-publish","hentry"],"part":3034,"_links":{"self":[{"href":"https:\/\/courses.lumenlearning.com\/suny-buffstate-chemistryformajorsxmaster\/wp-json\/pressbooks\/v2\/chapters\/1609","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/courses.lumenlearning.com\/suny-buffstate-chemistryformajorsxmaster\/wp-json\/pressbooks\/v2\/chapters"}],"about":[{"href":"https:\/\/courses.lumenlearning.com\/suny-buffstate-chemistryformajorsxmaster\/wp-json\/wp\/v2\/types\/chapter"}],"author":[{"embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/suny-buffstate-chemistryformajorsxmaster\/wp-json\/wp\/v2\/users\/17"}],"version-history":[{"count":9,"href":"https:\/\/courses.lumenlearning.com\/suny-buffstate-chemistryformajorsxmaster\/wp-json\/pressbooks\/v2\/chapters\/1609\/revisions"}],"predecessor-version":[{"id":5503,"href":"https:\/\/courses.lumenlearning.com\/suny-buffstate-chemistryformajorsxmaster\/wp-json\/pressbooks\/v2\/chapters\/1609\/revisions\/5503"}],"part":[{"href":"https:\/\/courses.lumenlearning.com\/suny-buffstate-chemistryformajorsxmaster\/wp-json\/pressbooks\/v2\/parts\/3034"}],"metadata":[{"href":"https:\/\/courses.lumenlearning.com\/suny-buffstate-chemistryformajorsxmaster\/wp-json\/pressbooks\/v2\/chapters\/1609\/metadata\/"}],"wp:attachment":[{"href":"https:\/\/courses.lumenlearning.com\/suny-buffstate-chemistryformajorsxmaster\/wp-json\/wp\/v2\/media?parent=1609"}],"wp:term":[{"taxonomy":"chapter-type","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/suny-buffstate-chemistryformajorsxmaster\/wp-json\/pressbooks\/v2\/chapter-type?post=1609"},{"taxonomy":"contributor","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/suny-buffstate-chemistryformajorsxmaster\/wp-json\/wp\/v2\/contributor?post=1609"},{"taxonomy":"license","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/suny-buffstate-chemistryformajorsxmaster\/wp-json\/wp\/v2\/license?post=1609"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}