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<title>Naming Ionic Compounds</title>
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<div class="section" id="averill_1.0-ch02_s03" condition="start-of-chunk" version="5.0" lang="en">
<h2 class="title editable block">
<span class="title-prefix">2.3</span> Naming Ionic Compounds</h2>
<div class="learning_objectives editable block" id="averill_1.0-ch02_s03_n01">
<h3 class="title">Learning Objective</h3>
<ol class="orderedlist" id="averill_1.0-ch02_s03_l01">
<li>To name ionic compounds.</li>
</ol>
</div>
<p class="para editable block" id="averill_1.0-ch02_s03_p01">The empirical and molecular formulas discussed in the preceding section are precise and highly informative, but they have some disadvantages. First, they are inconvenient for routine verbal communication. For example, saying “C-A-three-P-O-four-two” for Ca<sub class="subscript">3</sub>(PO<sub class="subscript">4</sub>)<sub class="subscript">2</sub> is much more difficult than saying “calcium phosphate.” In addition, you will see in <a class="xref" href="averill_1.0-ch02_s04#averill_1.0-ch02_s04">Section 2.4 "Naming Covalent Compounds"</a> that many compounds have the same empirical and molecular formulas but different arrangements of atoms, which result in very different chemical and physical properties. In such cases, it is necessary for the compounds to have different names that distinguish among the possible arrangements.</p>
<p class="para editable block" id="averill_1.0-ch02_s03_p02">Many compounds, particularly those that have been known for a relatively long time, have more than one name: a <em class="emphasis">common</em> name (sometimes more than one) and a <em class="emphasis">systematic</em> name, which is the name assigned by adhering to specific rules. Like the names of most elements, the common names of chemical compounds generally have historical origins, although they often appear to be unrelated to the compounds of interest. For example, the systematic name for KNO<sub class="subscript">3</sub> is potassium nitrate, but its common name is saltpeter.</p>
<p class="para editable block" id="averill_1.0-ch02_s03_p03">In this text, we use a systematic nomenclature to assign meaningful names to the millions of known substances. Unfortunately, some chemicals that are widely used in commerce and industry are still known almost exclusively by their common names; in such cases, you must be familiar with the common name as well as the systematic one. The objective of this and the next two sections is to teach you to write the formula for a simple inorganic compound from its name—and vice versa—and introduce you to some of the more frequently encountered common names.</p>
<p class="para editable block" id="averill_1.0-ch02_s03_p04">We begin with <em class="emphasis">binary ionic compounds</em>, which contain only two elements. The procedure for naming such compounds is outlined in <a class="xref" href="#averill_1.0-ch02_s03_f01">Figure 2.10 "Naming an Ionic Compound"</a> and uses the following steps:</p>
<div class="figure full editable block" id="averill_1.0-ch02_s03_f01">
<p class="title"><span class="title-prefix">Figure 2.10</span> Naming an Ionic Compound</p>
<img src="section_06/31092c38512b1a22518b627df41aca40.jpg">
</div>
<ol class="orderedlist block" id="averill_1.0-ch02_s03_l02">
<li>Place the ions in their proper order: cation and then anion.</li>
<li>
<p class="para">Name the cation.</p>
<ol class="orderedlist" id="averill_1.0-ch02_s03_l03" numeration="loweralpha">
<li>
<strong class="emphasis bold">Metals that form only one cation.</strong> As noted in <a class="xref" href="averill_1.0-ch02_s01#averill_1.0-ch02_s01">Section 2.1 "Chemical Compounds"</a>, these metals are usually in groups 1–3, 12, and 13. The name of the cation of a metal that forms only one cation is the same as the name of the metal (with the word <em class="emphasis">ion</em> added if the cation is by itself). For example, Na<sup class="superscript">+</sup> is the sodium ion, Ca<sup class="superscript">2+</sup> is the calcium ion, and Al<sup class="superscript">3+</sup> is the aluminum ion.</li>
<li>
<p class="para"><strong class="emphasis bold">Metals that form more than one cation.</strong> As shown in <a class="xref" href="#averill_1.0-ch02_s03_f02">Figure 2.11 "Metals That Form More Than One Cation and Their Locations in the Periodic Table"</a>, many metals can form more than one cation. This behavior is observed for most transition metals, many actinides, and the heaviest elements of groups 13–15. In such cases, the positive charge on the metal is indicated by a roman numeral in parentheses immediately following the name of the metal. Thus Cu<sup class="superscript">+</sup> is copper(I) (read as “copper one”), Fe<sup class="superscript">2+</sup> is iron(II), Fe<sup class="superscript">3+</sup> is iron(III), Sn<sup class="superscript">2+</sup> is tin(II), and Sn<sup class="superscript">4+</sup> is tin(IV).</p>
<p class="para" id="averill_1.0-ch02_s03_p05">An older system of nomenclature for such cations is still widely used, however. The name of the cation with the <em class="emphasis">higher</em> charge is formed from the root of the element’s Latin name with the suffix -<em class="emphasis">ic</em> attached, and the name of the cation with the <em class="emphasis">lower</em> charge has the same root with the suffix -<em class="emphasis">ous</em>. The names of Fe<sup class="superscript">3+</sup>, Fe<sup class="superscript">2+</sup>, Sn<sup class="superscript">4+</sup>, and Sn<sup class="superscript">2+</sup> are therefore ferric, ferrous, stannic, and stannous, respectively. Even though this text uses the systematic names with roman numerals, you should be able to recognize these common names because they are still often used. For example, on the label of your dentist’s fluoride rinse, the compound chemists call tin(II) fluoride is usually listed as stannous fluoride.</p>
<p class="para" id="averill_1.0-ch02_s03_p06">Some examples of metals that form more than one cation are in <a class="xref" href="#averill_1.0-ch02_s03_t01">Table 2.5 "Common Cations of Metals That Form More Than One Ion"</a> along with the names of the ions. Note that the simple Hg<sup class="superscript">+</sup> cation does not occur in chemical compounds. Instead, all compounds of mercury(I) contain a <em class="emphasis">dimeric</em> cation, Hg<sub class="subscript">2</sub><sup class="superscript">2+</sup>, in which the two Hg atoms are bonded together.</p>
<div class="table" id="averill_1.0-ch02_s03_t01" frame="all">
<p class="title"><span class="title-prefix">Table 2.5</span> Common Cations of Metals That Form More Than One Ion</p>
<table cellpadding="0" cellspacing="0">
<thead>
<tr>
<th align="center">Cation</th>
<th align="center">Systematic Name</th>
<th align="center">Common Name</th>
<th align="center">Cation</th>
<th align="center">Systematic Name</th>
<th align="center">Common Name</th>
</tr>
</thead>
<tbody>
<tr>
<td>Cr<sup class="superscript">2+</sup>
</td>
<td>chromium(II)</td>
<td>chromous</td>
<td>Cu<sup class="superscript">2+</sup>
</td>
<td>copper(II)</td>
<td>cupric</td>
</tr>
<tr>
<td>Cr<sup class="superscript">3+</sup>
</td>
<td>chromium(III)</td>
<td>chromic</td>
<td>Cu<sup class="superscript">+</sup>
</td>
<td>copper(I)</td>
<td>cuprous</td>
</tr>
<tr>
<td>Mn<sup class="superscript">2+</sup>
</td>
<td>manganese(II)</td>
<td>manganous*</td>
<td>Hg<sup class="superscript">2+</sup>
</td>
<td>mercury(II)</td>
<td>mercuric</td>
</tr>
<tr>
<td>Mn<sup class="superscript">3+</sup>
</td>
<td>manganese(III)</td>
<td>manganic*</td>
<td>Hg<sub class="subscript">2</sub><sup class="superscript">2+</sup>
</td>
<td>mercury(I)</td>
<td>mercurous<sup class="superscript">†</sup>
</td>
</tr>
<tr>
<td>Fe<sup class="superscript">2+</sup>
</td>
<td>iron(II)</td>
<td>ferrous</td>
<td>Sn<sup class="superscript">4+</sup>
</td>
<td>tin(IV)</td>
<td>stannic</td>
</tr>
<tr>
<td>Fe<sup class="superscript">3+</sup>
</td>
<td>iron(III)</td>
<td>ferric</td>
<td>Sn<sup class="superscript">2+</sup>
</td>
<td>tin(II)</td>
<td>stannous</td>
</tr>
<tr>
<td>Co<sup class="superscript">2+</sup>
</td>
<td>cobalt(II)</td>
<td>cobaltous*</td>
<td>Pb<sup class="superscript">4+</sup>
</td>
<td>lead(IV)</td>
<td>plumbic*</td>
</tr>
<tr>
<td>Co<sup class="superscript">3+</sup>
</td>
<td>cobalt(III)</td>
<td>cobaltic*</td>
<td>Pb<sup class="superscript">2+</sup>
</td>
<td>lead(II)</td>
<td>plumbous*</td>
</tr>
</tbody>
<tfoot>
<tr>
<th colspan="6">* Not widely used.</th>
</tr>
<tr>
<th colspan="6">
<sup class="superscript">†</sup>The isolated mercury(I) ion exists only as the gaseous ion.</th>
</tr>
</tfoot>
</table>
</div>
</li>
<li>
<strong class="emphasis bold">Polyatomic cations.</strong> The names of the common polyatomic cations that are relatively important in ionic compounds (such as, the ammonium ion) are in <a class="xref" href="averill_1.0-ch02_s02#averill_1.0-ch02_s02_s02_t01">Table 2.4 "Common Polyatomic Ions and Their Names"</a>.</li>
</ol>
</li>
<li>
<p class="para">Name the anion.</p>
<ol class="orderedlist" id="averill_1.0-ch02_s03_l04" numeration="loweralpha">
<li>
<strong class="emphasis bold">Monatomic anions.</strong> Monatomic anions are named by adding the suffix -<em class="emphasis">ide</em> to the root of the name of the parent element; thus, Cl<sup class="superscript">−</sup> is chloride, O<sup class="superscript">2−</sup> is oxide, P<sup class="superscript">3−</sup> is phosphide, N<sup class="superscript">3−</sup> is nitride (also called azide), and C<sup class="superscript">4−</sup> is carbide. Because the charges on these ions can be predicted from their position in the periodic table, it is <em class="emphasis">not</em> necessary to specify the charge in the name. Examples of monatomic anions are in <a class="xref" href="averill_1.0-ch02_s01#averill_1.0-ch02_s01_s03_t01">Table 2.2 "Some Common Monatomic Ions and Their Names"</a>.</li>
<li>
<p class="para"><strong class="emphasis bold">Polyatomic anions.</strong> Polyatomic anions typically have common names that you must learn; some examples are in <a class="xref" href="averill_1.0-ch02_s02#averill_1.0-ch02_s02_s02_t01">Table 2.4 "Common Polyatomic Ions and Their Names"</a>. Polyatomic anions that contain a single metal or nonmetal atom plus one or more oxygen atoms are called <em class="emphasis">oxoanions (or oxyanions)</em>. In cases where only two oxoanions are known for an element, the name of the oxoanion with more oxygen atoms ends in -<em class="emphasis">ate</em>, and the name of the oxoanion with fewer oxygen atoms ends in -<em class="emphasis">ite</em>. For example, NO<sub class="subscript">3−</sub> is nitrate and NO<sub class="subscript">2−</sub> is nitrite.</p>
<p class="para" id="averill_1.0-ch02_s03_p07">The halogens and some of the transition metals form more extensive series of oxoanions with as many as four members. In the names of these oxoanions, the prefix <em class="emphasis">per</em>- is used to identify the oxoanion with the most oxygen (so that ClO<sub class="subscript">4</sub><sup class="superscript">−</sup> is perchlorate and ClO<sub class="subscript">3</sub><sup class="superscript">−</sup> is chlorate), and the prefix <em class="emphasis">hypo</em>- is used to identify the anion with the fewest oxygen (ClO<sub class="subscript">2</sub><sup class="superscript">−</sup> is chlorite and ClO<sup class="superscript">−</sup> is hypochlorite). The relationship between the names of oxoanions and the number of oxygen atoms present is diagrammed in <a class="xref" href="#averill_1.0-ch02_s03_f03">Figure 2.12 "The Relationship between the Names of Oxoanions and the Number of Oxygen Atoms Present"</a>. Differentiating the oxoanions in such a series is no trivial matter. For example, the hypochlorite ion is the active ingredient in laundry bleach and swimming pool disinfectant, but compounds that contain the perchlorate ion can explode if they come into contact with organic substances.</p>
</li>
</ol>
</li>
<li>
<p class="para">Write the name of the compound as the name of the cation followed by the name of the anion.</p>
<p class="para" id="averill_1.0-ch02_s03_p08">It is <em class="emphasis">not</em> necessary to indicate the number of cations or anions present per formula unit in the name of an ionic compound because this information is implied by the charges on the ions. You must consider the charge of the ions when writing the formula for an ionic compound from its name, however. Because the charge on the chloride ion is −1 and the charge on the calcium ion is +2, for example, consistent with their positions in the periodic table, simple arithmetic tells you that calcium chloride must contain twice as many chloride ions as calcium ions to maintain electrical neutrality. Thus the formula is CaCl<sub class="subscript">2</sub>. Similarly, calcium phosphate must be Ca<sub class="subscript">3</sub>(PO<sub class="subscript">4</sub>)<sub class="subscript">2</sub> because the cation and the anion have charges of +2 and −3, respectively. The best way to learn how to name ionic compounds is to work through a few examples, referring to <a class="xref" href="#averill_1.0-ch02_s03_f01">Figure 2.10 "Naming an Ionic Compound"</a>, <a class="xref" href="averill_1.0-ch02_s01#averill_1.0-ch02_s01_s03_t01">Table 2.2 "Some Common Monatomic Ions and Their Names"</a>, <a class="xref" href="averill_1.0-ch02_s02#averill_1.0-ch02_s02_s02_t01">Table 2.4 "Common Polyatomic Ions and Their Names"</a>, and <a class="xref" href="#averill_1.0-ch02_s03_t01">Table 2.5 "Common Cations of Metals That Form More Than One Ion"</a> as needed.</p>
</li>
</ol>
<div class="figure large editable block" id="averill_1.0-ch02_s03_f02">
<p class="title"><span class="title-prefix">Figure 2.11</span> Metals That Form More Than One Cation and Their Locations in the Periodic Table</p>
<img src="section_06/499a3d3810e4febb228d28f9bf40dc85.jpg">
<p class="para">With only a few exceptions, these metals are usually transition metals or actinides.</p>
</div>
<div class="figure large medium-height editable block" id="averill_1.0-ch02_s03_f03">
<p class="title"><span class="title-prefix">Figure 2.12</span> The Relationship between the Names of Oxoanions and the Number of Oxygen Atoms Present</p>
<img src="section_06/20bbc08e23637b38faa0f5b0d0812d1d.jpg">
</div>
<div class="callout editable block" id="averill_1.0-ch02_s03_n02">
<h3 class="title">Note the Pattern</h3>
<p class="para" id="averill_1.0-ch02_s03_p09">Cations are always named before anions.</p>
<p class="para" id="averill_1.0-ch02_s03_p10">Most transition metals, many actinides, and the heaviest elements of groups 13–15 can form more than one cation.</p>
</div>
<div class="exercises editable block" id="averill_1.0-ch02_s03_n03">
<h3 class="title">Example 6</h3>
<p class="para" id="averill_1.0-ch02_s03_p11">Write the systematic name (and the common name if applicable) for each ionic compound.</p>
<ol class="orderedlist" id="averill_1.0-ch02_s03_l05" numeration="loweralpha">
<li>LiCl</li>
<li>MgSO<sub class="subscript">4</sub>
</li>
<li>(NH<sub class="subscript">4</sub>)<sub class="subscript">3</sub>PO<sub class="subscript">4</sub>
</li>
<li>Cu<sub class="subscript">2</sub>O</li>
</ol>
<p class="para" id="averill_1.0-ch02_s03_p12"><strong class="emphasis bold">Given: </strong>empirical formula</p>
<p class="para" id="averill_1.0-ch02_s03_p13"><strong class="emphasis bold">Asked for: </strong>name</p>
<p class="para" id="averill_1.0-ch02_s03_p14">
<strong class="emphasis bold">Strategy:</strong>
</p>
<p class="para" id="averill_1.0-ch02_s03_p15"><strong class="emphasis bold">A</strong> If only one charge is possible for the cation, give its name, consulting <a class="xref" href="averill_1.0-ch02_s01#averill_1.0-ch02_s01_s03_t01">Table 2.2 "Some Common Monatomic Ions and Their Names"</a> or <a class="xref" href="averill_1.0-ch02_s02#averill_1.0-ch02_s02_s02_t01">Table 2.4 "Common Polyatomic Ions and Their Names"</a> if necessary. If the cation can have more than one charge (<a class="xref" href="#averill_1.0-ch02_s03_t01">Table 2.5 "Common Cations of Metals That Form More Than One Ion"</a>), specify the charge using roman numerals.</p>
<p class="para" id="averill_1.0-ch02_s03_p16"><strong class="emphasis bold">B</strong> If the anion does not contain oxygen, name it according to step 3a, using <a class="xref" href="averill_1.0-ch02_s01#averill_1.0-ch02_s01_s03_t01">Table 2.2 "Some Common Monatomic Ions and Their Names"</a> and <a class="xref" href="averill_1.0-ch02_s02#averill_1.0-ch02_s02_s02_t01">Table 2.4 "Common Polyatomic Ions and Their Names"</a> if necessary. For polyatomic anions that contain oxygen, use <a class="xref" href="averill_1.0-ch02_s02#averill_1.0-ch02_s02_s02_t01">Table 2.4 "Common Polyatomic Ions and Their Names"</a> and the appropriate prefix and suffix listed in step 3b.</p>
<p class="para" id="averill_1.0-ch02_s03_p17"><strong class="emphasis bold">C</strong> Beginning with the cation, write the name of the compound.</p>
<p class="para" id="averill_1.0-ch02_s03_p18">
<strong class="emphasis bold">Solution:</strong>
</p>
<ol class="orderedlist" id="averill_1.0-ch02_s03_l06" numeration="loweralpha">
<li>
<strong class="emphasis bold">A B</strong> Lithium is in group 1, so we know that it forms only the Li<sup class="superscript">+</sup> cation, which is the lithium ion. Similarly, chlorine is in group 7, so it forms the Cl<sup class="superscript">−</sup> anion, which is the chloride ion. <strong class="emphasis bold">C</strong> Because we begin with the name of the cation, the name of this compound is lithium chloride, which is used medically as an antidepressant drug.</li>
<li>
<strong class="emphasis bold">A B</strong> The cation is the magnesium ion, and the anion, which contains oxygen, is sulfate. <strong class="emphasis bold">C</strong> Because we list the cation first, the name of this compound is magnesium sulfate. A hydrated form of magnesium sulfate (MgSO<sub class="subscript">4</sub>·7H<sub class="subscript">2</sub>O) is sold in drugstores as Epsom salts, a harsh but effective laxative.</li>
<li>
<strong class="emphasis bold">A B</strong> The cation is the ammonium ion (from <a class="xref" href="averill_1.0-ch02_s02#averill_1.0-ch02_s02_s02_t01">Table 2.4 "Common Polyatomic Ions and Their Names"</a>), and the anion is phosphate. <strong class="emphasis bold">C</strong> The compound is therefore ammonium phosphate, which is widely used as a fertilizer. It is not necessary to specify that the formula unit contains three ammonium ions because three are required to balance the negative charge on phosphate.</li>
<li>
<strong class="emphasis bold">A B</strong> The cation is a transition metal that often forms more than one cation (<a class="xref" href="#averill_1.0-ch02_s03_t01">Table 2.5 "Common Cations of Metals That Form More Than One Ion"</a>). We must therefore specify the positive charge on the cation in the name: copper(I) or, according to the older system, cuprous. The anion is oxide. <strong class="emphasis bold">C</strong> The name of this compound is copper(I) oxide or, in the older system, cuprous oxide. Copper(I) oxide is used as a red glaze on ceramics and in antifouling paints to prevent organisms from growing on the bottoms of boats.</li>
</ol>
<div class="informalfigure small">
<img src="section_06/4bf4f9d222a9d28cfed4b69a82362273.jpg">
<p class="para"><strong class="emphasis bold">Cu</strong><sub class="subscript"><strong class="emphasis bold">2</strong></sub><strong class="emphasis bold">O.</strong> The bottom of a boat is protected with a red antifouling paint containing copper(I) oxide, Cu<sub class="subscript">2</sub>O.</p>
</div>
<p class="simpara">Exercise</p>
<p class="para" id="averill_1.0-ch02_s03_p19">Write the systematic name (and the common name if applicable) for each ionic compound.</p>
<ol class="orderedlist" id="averill_1.0-ch02_s03_l07" numeration="loweralpha">
<li>CuCl<sub class="subscript">2</sub>
</li>
<li>MgCO<sub class="subscript">3</sub>
</li>
<li>FePO<sub class="subscript">4</sub>
</li>
</ol>
<p class="para" id="averill_1.0-ch02_s03_p20">
<strong class="emphasis bold">Answer:</strong>
</p>
<ol class="orderedlist" id="averill_1.0-ch02_s03_l08" numeration="loweralpha">
<li>copper(II) chloride (or cupric chloride)</li>
<li>magnesium carbonate</li>
<li>iron(III) phosphate (or ferric phosphate)</li>
</ol>
</div>
<div class="exercises editable block" id="averill_1.0-ch02_s03_n04">
<h3 class="title">Example 7</h3>
<p class="para" id="averill_1.0-ch02_s03_p21">Write the formula for each compound.</p>
<ol class="orderedlist" id="averill_1.0-ch02_s03_l09" numeration="loweralpha">
<li>calcium dihydrogen phosphate</li>
<li>aluminum sulfate</li>
<li>chromium(III) oxide</li>
</ol>
<p class="para" id="averill_1.0-ch02_s03_p22"><strong class="emphasis bold">Given: </strong>systematic name</p>
<p class="para" id="averill_1.0-ch02_s03_p23"><strong class="emphasis bold">Asked for: </strong>formula</p>
<p class="para" id="averill_1.0-ch02_s03_p24">
<strong class="emphasis bold">Strategy:</strong>
</p>
<p class="para" id="averill_1.0-ch02_s03_p25"><strong class="emphasis bold">A</strong> Identify the cation and its charge using the location of the element in the periodic table and <a class="xref" href="averill_1.0-ch02_s01#averill_1.0-ch02_s01_s03_t01">Table 2.2 "Some Common Monatomic Ions and Their Names"</a>, <a class="xref" href="averill_1.0-ch02_s01#averill_1.0-ch02_s01_s04_t01">Table 2.3 "The Physical Properties of Typical Ionic Compounds and Covalent Molecular Substances"</a>, <a class="xref" href="averill_1.0-ch02_s02#averill_1.0-ch02_s02_s02_t01">Table 2.4 "Common Polyatomic Ions and Their Names"</a>, and <a class="xref" href="#averill_1.0-ch02_s03_t01">Table 2.5 "Common Cations of Metals That Form More Than One Ion"</a>. If the cation is derived from a metal that can form cations with different charges, use the appropriate roman numeral or suffix to indicate its charge.</p>
<p class="para" id="averill_1.0-ch02_s03_p26"><strong class="emphasis bold">B</strong> Identify the anion using <a class="xref" href="averill_1.0-ch02_s01#averill_1.0-ch02_s01_s03_t01">Table 2.2 "Some Common Monatomic Ions and Their Names"</a> and <a class="xref" href="averill_1.0-ch02_s02#averill_1.0-ch02_s02_s02_t01">Table 2.4 "Common Polyatomic Ions and Their Names"</a>. Beginning with the cation, write the compound’s formula and then determine the number of cations and anions needed to achieve electrical neutrality.</p>
<p class="para" id="averill_1.0-ch02_s03_p27">
<strong class="emphasis bold">Solution:</strong>
</p>
<ol class="orderedlist" id="averill_1.0-ch02_s03_l10" numeration="loweralpha">
<li>
<strong class="emphasis bold">A</strong> Calcium is in group 2, so it forms only the Ca<sup class="superscript">2+</sup> ion. <strong class="emphasis bold">B</strong> Dihydrogen phosphate is the H<sub class="subscript">2</sub>PO<sub class="subscript">4</sub><sup class="superscript">−</sup> ion (<a class="xref" href="averill_1.0-ch02_s02#averill_1.0-ch02_s02_s02_t01">Table 2.4 "Common Polyatomic Ions and Their Names"</a>). Two H<sub class="subscript">2</sub>PO<sub class="subscript">4</sub><sup class="superscript">−</sup> ions are needed to balance the positive charge on Ca<sup class="superscript">2+</sup>, to give Ca(H<sub class="subscript">2</sub>PO<sub class="subscript">4</sub>)<sub class="subscript">2</sub>. A hydrate of calcium dihydrogen phosphate, Ca(H<sub class="subscript">2</sub>PO<sub class="subscript">4</sub>)<sub class="subscript">2</sub>·H<sub class="subscript">2</sub>O, is the active ingredient in baking powder.</li>
<li>
<strong class="emphasis bold">A</strong> Aluminum, near the top of group 13 in the periodic table, forms only one cation, Al<sup class="superscript">3+</sup> (<a class="xref" href="#averill_1.0-ch02_s03_f02">Figure 2.11 "Metals That Form More Than One Cation and Their Locations in the Periodic Table"</a>). <strong class="emphasis bold">B</strong> Sulfate is SO<sub class="subscript">4</sub><sup class="superscript">2−</sup> (<a class="xref" href="averill_1.0-ch02_s02#averill_1.0-ch02_s02_s02_t01">Table 2.4 "Common Polyatomic Ions and Their Names"</a>). To balance the electrical charges, we need two Al<sup class="superscript">3+</sup> cations and three SO<sub class="subscript">4</sub><sup class="superscript">2−</sup> anions, giving Al<sub class="subscript">2</sub>(SO<sub class="subscript">4</sub>)<sub class="subscript">3</sub>. Aluminum sulfate is used to tan leather and purify drinking water.</li>
<li>
<strong class="emphasis bold">A</strong> Because chromium is a transition metal, it can form cations with different charges. The roman numeral tells us that the positive charge in this case is +3, so the cation is Cr<sup class="superscript">3+</sup>. <strong class="emphasis bold">B</strong> Oxide is O<sup class="superscript">2−</sup>. Thus two cations (Cr<sup class="superscript">3+</sup>) and three anions (O<sup class="superscript">2−</sup>) are required to give an electrically neutral compound, Cr<sub class="subscript">2</sub>O<sub class="subscript">3</sub>. This compound is a common green pigment that has many uses, including camouflage coatings.</li>
</ol>
<div class="informalfigure small">
<img src="section_06/8e3c0dceaa6092a9332da8a7875489ad.jpg">
<p class="para"><strong class="emphasis bold">Cr</strong><sub class="subscript"><strong class="emphasis bold">2</strong></sub><strong class="emphasis bold">O</strong><sub class="subscript"><strong class="emphasis bold">3</strong></sub><strong class="emphasis bold">.</strong> Chromium(III) oxide (Cr<sub class="subscript">2</sub>O<sub class="subscript">3</sub>) is a common pigment in dark green paints, such as camouflage paint.</p>
</div>
<p class="simpara">Exercise</p>
<p class="para" id="averill_1.0-ch02_s03_p28">Write the formula for each compound.</p>
<ol class="orderedlist" id="averill_1.0-ch02_s03_l11" numeration="loweralpha">
<li>barium chloride</li>
<li>sodium carbonate</li>
<li>iron(III) hydroxide</li>
</ol>
<p class="para" id="averill_1.0-ch02_s03_p29">
<strong class="emphasis bold">Answer:</strong>
</p>
<ol class="orderedlist" id="averill_1.0-ch02_s03_l12" numeration="loweralpha">
<li>BaCl<sub class="subscript">2</sub>
</li>
<li>Na<sub class="subscript">2</sub>CO<sub class="subscript">3</sub>
</li>
<li>Fe(OH)<sub class="subscript">3</sub>
</li>
</ol>
</div>
<div class="callout editable block" id="averill_1.0-ch02_s03_n05">
<h3 class="title">Summary</h3>
<p class="para" id="averill_1.0-ch02_s03_p30">Ionic compounds are named according to systematic procedures, although common names are widely used. Systematic nomenclature enables us to write the structure of any compound from its name and vice versa. Ionic compounds are named by writing the cation first, followed by the anion. If a metal can form cations with more than one charge, the charge is indicated by roman numerals in parentheses following the name of the metal. <strong class="emphasis bold">Oxoanions</strong> are polyatomic anions that contain a single metal or nonmetal atom and one or more oxygen atoms.</p>
</div>
<div class="key_takeaways editable block" id="averill_1.0-ch02_s03_n06">
<h3 class="title">Key Takeaway</h3>
<ul class="itemizedlist" id="averill_1.0-ch02_s03_l13">
<li>There is a systematic method used to name ionic compounds.</li>
</ul>
</div>
<div class="qandaset block" id="averill_1.0-ch02_s03_qs01" defaultlabel="number">
<h3 class="title">Conceptual Problems</h3>
<ol class="qandadiv" id="averill_1.0-ch02_s03_qs01_qd01">
<li class="qandaentry" id="averill_1.0-ch02_s03_qs01_qd01_qa01">
<div class="question">
<p class="para">Name each cation.</p>
<ol class="orderedlist" numeration="loweralpha">
<li>K<sup class="superscript">+</sup>
</li>
<li>Al<sup class="superscript">3+</sup>
</li>
<li>NH<sub class="subscript">4</sub><sup class="superscript">+</sup>
</li>
<li>Mg<sup class="superscript">2+</sup>
</li>
<li>Li<sup class="superscript">+</sup>
</li>
</ol>
</div>
</li>
<li class="qandaentry" id="averill_1.0-ch02_s03_qs01_qd01_qa02">
<div class="question">
<p class="para">Name each anion.</p>
<ol class="orderedlist" numeration="loweralpha">
<li>Br<sup class="superscript">−</sup>
</li>
<li>CO<sub class="subscript">3</sub><sup class="superscript">2−</sup>
</li>
<li>S<sup class="superscript">2−</sup>
</li>
<li>NO<sub class="subscript">3</sub><sup class="superscript">−</sup>
</li>
<li>HCO<sub class="subscript">2</sub><sup class="superscript">−</sup>
</li>
<li>F<sup class="superscript">−</sup>
</li>
<li>ClO<sup class="superscript">−</sup>
</li>
<li>C<sub class="subscript">2</sub>O<sub class="subscript">4</sub><sup class="superscript">2−</sup>
</li>
</ol>
</div>
</li>
<li class="qandaentry" id="averill_1.0-ch02_s03_qs01_qd01_qa03">
<div class="question">
<p class="para">Name each anion.</p>
<ol class="orderedlist" numeration="loweralpha">
<li>PO<sub class="subscript">4</sub><sup class="superscript">3−</sup>
</li>
<li>Cl<sup class="superscript">−</sup>
</li>
<li>SO<sub class="subscript">3</sub><sup class="superscript">2−</sup>
</li>
<li>CH<sub class="subscript">3</sub>CO<sub class="subscript">2</sub><sup class="superscript">−</sup>
</li>
<li>HSO<sub class="subscript">4</sub><sup class="superscript">−</sup>
</li>
<li>ClO<sub class="subscript">4</sub><sup class="superscript">−</sup>
</li>
<li>NO<sub class="subscript">2</sub><sup class="superscript">−</sup>
</li>
<li>O<sup class="superscript">2−</sup>
</li>
</ol>
</div>
</li>
<li class="qandaentry" id="averill_1.0-ch02_s03_qs01_qd01_qa04">
<div class="question">
<p class="para">Name each anion.</p>
<ol class="orderedlist" numeration="loweralpha">
<li>SO<sub class="subscript">4</sub><sup class="superscript">2−</sup>
</li>
<li>CN<sup class="superscript">−</sup>
</li>
<li>Cr<sub class="subscript">2</sub>O<sub class="subscript">7</sub><sup class="superscript">2−</sup>
</li>
<li>N<sup class="superscript">3−</sup>
</li>
<li>OH<sup class="superscript">−</sup>
</li>
<li>I<sup class="superscript">−</sup>
</li>
<li>O<sub class="subscript">2</sub><sup class="superscript">2−</sup>
</li>
</ol>
</div>
</li>
<li class="qandaentry" id="averill_1.0-ch02_s03_qs01_qd01_qa05">
<div class="question">
<p class="para">Name each compound.</p>
<ol class="orderedlist" numeration="loweralpha">
<li>MgBr<sub class="subscript">2</sub>
</li>
<li>NH<sub class="subscript">4</sub>CN</li>
<li>CaO</li>
<li>KClO<sub class="subscript">3</sub>
</li>
<li>K<sub class="subscript">3</sub>PO<sub class="subscript">4</sub>
</li>
<li>NH<sub class="subscript">4</sub>NO<sub class="subscript">2</sub>
</li>
<li>NaN<sub class="subscript">3</sub>
</li>
</ol>
</div>
</li>
<li class="qandaentry" id="averill_1.0-ch02_s03_qs01_qd01_qa06">
<div class="question">
<p class="para">Name each compound.</p>
<ol class="orderedlist" numeration="loweralpha">
<li>NaNO<sub class="subscript">3</sub>
</li>
<li>Cu<sub class="subscript">3</sub>(PO<sub class="subscript">4</sub>)<sub class="subscript">2</sub>
</li>
<li>NaOH</li>
<li>Li<sub class="subscript">4</sub>C</li>
<li>CaF<sub class="subscript">2</sub>
</li>
<li>NH<sub class="subscript">4</sub>Br</li>
<li>MgCO<sub class="subscript">3</sub>
</li>
</ol>
</div>
</li>
<li class="qandaentry" id="averill_1.0-ch02_s03_qs01_qd01_qa07">
<div class="question">
<p class="para">Name each compound.</p>
<ol class="orderedlist" numeration="loweralpha">
<li>RbBr</li>
<li>Mn<sub class="subscript">2</sub>(SO<sub class="subscript">4</sub>)<sub class="subscript">3</sub>
</li>
<li>NaClO</li>
<li>(NH<sub class="subscript">4</sub>)<sub class="subscript">2</sub>SO<sub class="subscript">4</sub>
</li>
<li>NaBr</li>
<li>KIO<sub class="subscript">3</sub>
</li>
<li>Na<sub class="subscript">2</sub>CrO<sub class="subscript">4</sub>
</li>
</ol>
</div>
</li>
<li class="qandaentry" id="averill_1.0-ch02_s03_qs01_qd01_qa08">
<div class="question">
<p class="para">Name each compound.</p>
<ol class="orderedlist" numeration="loweralpha">
<li>NH<sub class="subscript">4</sub>ClO<sub class="subscript">4</sub>
</li>
<li>SnCl<sub class="subscript">4</sub>
</li>
<li>Fe(OH)<sub class="subscript">2</sub>
</li>
<li>Na<sub class="subscript">2</sub>O</li>
<li>MgCl<sub class="subscript">2</sub>
</li>
<li>K<sub class="subscript">2</sub>SO<sub class="subscript">4</sub>
</li>
<li>RaCl<sub class="subscript">2</sub>
</li>
</ol>
</div>
</li>
<li class="qandaentry" id="averill_1.0-ch02_s03_qs01_qd01_qa09">
<div class="question">
<p class="para">Name each compound.</p>
<ol class="orderedlist" numeration="loweralpha">
<li>KCN</li>
<li>LiOH</li>
<li>CaCl<sub class="subscript">2</sub>
</li>
<li>NiSO<sub class="subscript">4</sub>
</li>
<li>NH<sub class="subscript">4</sub>ClO<sub class="subscript">2</sub>
</li>
<li>LiClO<sub class="subscript">4</sub>
</li>
<li>La(CN)<sub class="subscript">3</sub>
</li>
</ol>
</div>
</li>
</ol>
</div>
<div class="qandaset block" id="averill_1.0-ch02_s03_qs01_ans" defaultlabel="number">
<h3 class="title">Answer</h3>
<ol class="qandadiv">
<li class="qandaentry" id="averill_1.0-ch02_s03_qs01_qd01_qa01_ans" audience="instructoronly">
<div class="answer" audience="instructoronly" d="" html="http://www.w3.org/1999/xhtml" mml="http://www.w3.org/1998/Math/MathML" xlink="http://www.w3.org/1999/xlink" xml="http://www.w3.org/XML/1998/namespace">
</div>
</li>
<li class="qandaentry" id="averill_1.0-ch02_s03_qs01_qd01_qa02_ans" audience="instructoronly">
<div class="answer" audience="instructoronly" d="" html="http://www.w3.org/1999/xhtml" mml="http://www.w3.org/1998/Math/MathML" xlink="http://www.w3.org/1999/xlink" xml="http://www.w3.org/XML/1998/namespace">
</div>
</li>
<li class="qandaentry" id="averill_1.0-ch02_s03_qs01_qd01_qa03_ans" audience="instructoronly">
<div class="answer" audience="instructoronly" d="" html="http://www.w3.org/1999/xhtml" mml="http://www.w3.org/1998/Math/MathML" xlink="http://www.w3.org/1999/xlink" xml="http://www.w3.org/XML/1998/namespace">
</div>
</li>
<li class="qandaentry" id="averill_1.0-ch02_s03_qs01_qd01_qa04_ans" audience="instructoronly">
<div class="answer" audience="instructoronly" d="" html="http://www.w3.org/1999/xhtml" mml="http://www.w3.org/1998/Math/MathML" xlink="http://www.w3.org/1999/xlink" xml="http://www.w3.org/XML/1998/namespace">
</div>
</li>
<li class="qandaentry" id="averill_1.0-ch02_s03_qs01_qd01_qa05_ans" audience="instructoronly">
<div class="answer" audience="instructoronly" d="" html="http://www.w3.org/1999/xhtml" mml="http://www.w3.org/1998/Math/MathML" xlink="http://www.w3.org/1999/xlink" xml="http://www.w3.org/XML/1998/namespace">
</div>
</li>
<li class="qandaentry" id="averill_1.0-ch02_s03_qs01_qd01_qa06_ans" audience="instructoronly">
<div class="answer" audience="instructoronly" d="" html="http://www.w3.org/1999/xhtml" mml="http://www.w3.org/1998/Math/MathML" xlink="http://www.w3.org/1999/xlink" xml="http://www.w3.org/XML/1998/namespace">
</div>
</li>
<li class="qandaentry" id="averill_1.0-ch02_s03_qs01_qd01_qa07_ans">
<div class="answer">
<p class="para">
</p>
<ol class="orderedlist" numeration="loweralpha"> <li>rubidium bromide</li>
<li>manganese(III) sulfate</li>
<li>sodium hypochlorite</li>
<li>ammonium sulfate</li>
<li>sodium bromide</li>
<li>potassium iodate</li>
<li>sodium chromate</li>
</ol>
</div>
</li>
<li class="qandaentry" id="averill_1.0-ch02_s03_qs01_qd01_qa08_ans" audience="instructoronly">
<div class="answer" audience="instructoronly" d="" html="http://www.w3.org/1999/xhtml" mml="http://www.w3.org/1998/Math/MathML" xlink="http://www.w3.org/1999/xlink" xml="http://www.w3.org/XML/1998/namespace">
</div>
</li>
<li class="qandaentry" id="averill_1.0-ch02_s03_qs01_qd01_qa09_ans" audience="instructoronly">
<div class="answer" audience="instructoronly" d="" html="http://www.w3.org/1999/xhtml" mml="http://www.w3.org/1998/Math/MathML" xlink="http://www.w3.org/1999/xlink" xml="http://www.w3.org/XML/1998/namespace">
</div>
</li>
</ol>
</div>
<div class="qandaset block" id="averill_1.0-ch02_s03_qs02" defaultlabel="number">
<h3 class="title">Numerical Problems</h3>
<ol class="qandadiv" id="averill_1.0-ch02_s03_qs02_qd01">
<li class="qandaentry" id="averill_1.0-ch02_s03_qs02_qd01_qa02">
<div class="question">
<p class="para">For each ionic compound, name the cation and the anion and give the charge on each ion.</p>
<ol class="orderedlist" numeration="loweralpha">
<li>BeO</li>
<li>Pb(OH)<sub class="subscript">2</sub>
</li>
<li>BaS</li>
<li>Na<sub class="subscript">2</sub>Cr<sub class="subscript">2</sub>O<sub class="subscript">7</sub>
</li>
<li>ZnSO<sub class="subscript">4</sub>
</li>
<li>KClO</li>
<li>NaH<sub class="subscript">2</sub>PO<sub class="subscript">4</sub>
</li>
</ol>
</div>
</li>
<li class="qandaentry" id="averill_1.0-ch02_s03_qs02_qd01_qa01">
<div class="question">
<p class="para">For each ionic compound, name the cation and the anion and give the charge on each ion.</p>
<ol class="orderedlist" numeration="loweralpha">
<li>Zn(NO<sub class="subscript">3</sub>)<sub class="subscript">2</sub>
</li>
<li>CoS</li>
<li>BeCO<sub class="subscript">3</sub>
</li>
<li>Na<sub class="subscript">2</sub>SO<sub class="subscript">4</sub>
</li>
<li>K<sub class="subscript">2</sub>C<sub class="subscript">2</sub>O<sub class="subscript">4</sub>
</li>
<li>NaCN</li>
<li>FeCl<sub class="subscript">2</sub>
</li>
</ol>
</div>
</li>
<li class="qandaentry" id="averill_1.0-ch02_s03_qs02_qd01_qa04">
<div class="question">
<p class="para">Write the formula for each compound.</p>
<ol class="orderedlist" numeration="loweralpha">
<li>magnesium carbonate</li>
<li>aluminum sulfate</li>
<li>potassium phosphate</li>
<li>lead(IV) oxide</li>
<li>silicon nitride</li>
<li>sodium hypochlorite</li>
<li>titanium(IV) chloride</li>
<li>disodium ammonium phosphate</li>
</ol>
</div>
</li>
<li class="qandaentry" id="averill_1.0-ch02_s03_qs02_qd01_qa03">
<div class="question">
<p class="para">Write the formula for each compound.</p>
<ol class="orderedlist" numeration="loweralpha">
<li>lead(II) nitrate</li>
<li>ammonium phosphate</li>
<li>silver sulfide</li>
<li>barium sulfate</li>
<li>cesium iodide</li>
<li>sodium bicarbonate</li>
<li>potassium dichromate</li>
<li>sodium hypochlorite</li>
</ol>
</div>
</li>
<li class="qandaentry" id="averill_1.0-ch02_s03_qs02_qd01_qa06">
<div class="question">
<p class="para">Write the formula for each compound.</p>
<ol class="orderedlist" numeration="loweralpha">
<li>zinc cyanide</li>
<li>silver chromate</li>
<li>lead(II) iodide</li>
<li>benzene</li>
<li>copper(II) perchlorate</li>
</ol>
</div>
</li>
<li class="qandaentry" id="averill_1.0-ch02_s03_qs02_qd01_qa05">
<div class="question">
<p class="para">Write the formula for each compound.</p>
<ol class="orderedlist" numeration="loweralpha">
<li>calcium fluoride</li>
<li>sodium nitrate</li>
<li>iron(III) oxide</li>
<li>copper(II) acetate</li>
<li>sodium nitrite</li>
</ol>
</div>
</li>
<li class="qandaentry" id="averill_1.0-ch02_s03_qs02_qd01_qa08">
<div class="question">
<p class="para">Write the formula for each compound.</p>
<ol class="orderedlist" numeration="loweralpha">
<li>sodium hydroxide</li>
<li>calcium cyanide</li>
<li>magnesium phosphate</li>
<li>sodium sulfate</li>
<li>nickel(II) bromide</li>
<li>calcium chlorite</li>
<li>titanium(IV) bromide</li>
</ol>
</div>
</li>
<li class="qandaentry" id="averill_1.0-ch02_s03_qs02_qd01_qa07">
<div class="question">
<p class="para">Write the formula for each compound.</p>
<ol class="orderedlist" numeration="loweralpha">
<li>sodium chlorite</li>
<li>potassium nitrite</li>
<li>sodium nitride (also called sodium azide)</li>
<li>calcium phosphide</li>
<li>tin(II) chloride</li>
<li>calcium hydrogen phosphate</li>
<li>iron(II) chloride dihydrate</li>
</ol>
</div>
</li>
<li class="qandaentry" id="averill_1.0-ch02_s03_qs02_qd01_qa09">
<div class="question">
<p class="para">Write the formula for each compound.</p>
<ol class="orderedlist" numeration="loweralpha">
<li>potassium carbonate</li>
<li>chromium(III) sulfite</li>
<li>cobalt(II) phosphate</li>
<li>magnesium hypochlorite</li>
<li>nickel(II) nitrate hexahydrate</li>
</ol>
</div>
</li>
</ol>
</div>
</div>
</div>
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