5.5: Naming Ionic Compounds

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Sep 19, 2019
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- 5.4: Naming Inorganic Compounds
- 5.6: Naming Acids

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Learning Objectives

To use the rules for naming ionic compounds.

After learning a few more details about the names of individual ions, you will be one step away from knowing how to name ionic compounds. This section begins the formal study of nomenclature, the systematic naming of chemical compounds.

Naming Ions

The name of a monatomic cation is simply the name of the element followed by the word ion. Thus, Na⁺ is the sodium ion, Al³⁺ is the aluminum ion, Ca²⁺ is the calcium ion, and so forth.

We have seen that some elements lose different numbers of electrons, producing ions of different charges (Figure 3.3). Iron, for example, can form two cations, each of which, when combined with the same anion, makes a different compound with unique physical and chemical properties. Thus, we need a different name for each iron ion to distinguish Fe²⁺ from Fe³⁺. The same issue arises for other ions with more than one possible charge.

There are two ways to make this distinction. In the simpler, more modern approach, called the Stock system, an ion’s positive charge is indicated by a roman numeral in parentheses after the element name, followed by the word ion. Thus, Fe²⁺ is called the iron(II) ion, while Fe³⁺ is called the iron(III) ion. This system is used only for elements that form more than one common positive ion. We do not call the Na⁺ ion the sodium(I) ion because (I) is unnecessary. Sodium forms only a 1+ ion, so there is no ambiguity about the name sodium ion.

Table $\PageIndex{1}$ : The Modern and Common System of Cation Names
Element	Stem	Charge	Modern Name	Common Name
iron	ferr-	2+	iron(II) ion	ferrous ion
iron	ferr-	3+	iron(III) ion	ferric ion
copper	cupr-	1+	copper(I) ion	cuprous ion
copper	cupr-	2+	copper(II) ion	cupric ion
tin	stann-	2+	tin(II) ion	stannous ion
tin	stann-	4+	tin(IV) ion	stannic ion
lead	plumb-	2+	lead(II) ion	plumbous ion
lead	plumb-	4+	lead(IV) ion	plumbic ion
chromium	chrom-	2+	chromium(II) ion	chromous ion
chromium	chrom-	3+	chromium(III) ion	chromic ion
gold	aur-	1+	gold(I) ion	aurous ion
gold	aur-	3+	gold(III) ion	auric ion

The second system, called the common system, is not conventional but is still prevalent and used in the health sciences. This system recognizes that many metals have two common cations. The common system uses two suffixes (-ic and -ous) that are appended to the stem of the element name. The -ic suffix represents the greater of the two cation charges, and the -ous suffix represents the lower one. In many cases, the stem of the element name comes from the Latin name of the element. Table $\PageIndex{1}$ lists the elements that use the common system, along with their respective cation names.

Table $\PageIndex{2}$ : Some Monatomic Anions
Ion	Name
F⁻	fluoride ion
Cl⁻	chloride ion
Br⁻	bromide ion
I⁻	iodide ion
O²⁻	oxide ion
S²⁻	sulfide ion
P³⁻	phosphide ion
N³⁻	nitride ion

The name of a monatomic anion consists of the stem of the element name, the suffix -ide, and then the word ion. Thus, as we have already seen, Cl⁻ is “chlor-” + “-ide ion,” or the chloride ion. Similarly, O²⁻ is the oxide ion, Se²⁻ is the selenide ion, and so forth. Table $\PageIndex{2}$ lists the names of some common monatomic ions. The polyatomic ions have their own characteristic names, as discussed earlier.

Example $\PageIndex{1}$

Name each ion.

Ca²⁺
S²⁻
SO₃²⁻
NH₄⁺
Cu⁺

Solution

the calcium ion
the sulfide ion
the sulfite ion
the ammonium ion
the copper(I) ion or the cuprous ion

Exercise $\PageIndex{1}$

Name each ion.

Fe²⁺
Fe³⁺
SO₄²⁻
Ba²⁺
HCO₃⁻

Answer a:: iron(II) ion
Answer b:: iron(III) ion
Answer c:: sulfate ion
Answer d:: barium ion
Answer e:: hydrogen carbonate ion or bicarbonate ion

Example $\PageIndex{2}$

Write the formula for each ion.

the bromide ion
the phosphate ion
the cupric ion
the magnesium ion

Solution

Br⁻
PO₄³⁻
Cu²⁺
Mg²⁺

Exercise $\PageIndex{2}$

Write the formula for each ion.

the fluoride ion
the carbonate ion
the stannous ion
the potassium ion

Answer a:: F^-
Answer b:: CO₃²^-
Answer c:: Sn ²⁺
Answer d:: K⁺

Naming Binary Ionic Compounds with a Metal that Forms Only One Type of Cation

A binary ionic compound is a compound composed of a monatomic metal cation and a monatomic nonmetal anion. The metal cation is named first, followed by the nonmetal anion as illustrated in Figure $\PageIndex{1}$ for the compound BaCl₂. The word ion is dropped from both parts.

5.7A.PNG — Figure $\PageIndex{1}$ : Naming $BaCl_2$
Naming formula: Name of metal cation + base
name of nonmetal anion + suffix -ide. BaCl2 is named as barium chloride.

Subscripts in the formula do not affect the name.

Example $\PageIndex{3}$ : Naming Ionic Compounds

Name each ionic compound.

CaCl₂
AlF₃
KCl

Solution

Using the names of the ions, this ionic compound is named calcium chloride.
The name of this ionic compound is aluminum fluoride.
The name of this ionic compound is potassium chloride

Exercise $\PageIndex{3}$

Name each ionic compound.

AgI
MgO
Ca₃P₂

Answer a:: silver iodide
Answer b:: magnesium oxide
Answer c:: calcium phosphide

Naming Binary Ionic Compounds with a Metal That Forms More Than One Type of Cation

If you are given a formula for an ionic compound whose cation can have more than one possible charge, you must first determine the charge on the cation before identifying its correct name. For example, consider FeCl₂ and FeCl₃_. In the first compound, the iron ion has a 2+ charge because there are two Cl⁻ ions in the formula (1− charge on each chloride ion). In the second compound, the iron ion has a 3+ charge, as indicated by the three Cl⁻ ions in the formula. These are two different compounds that need two different names. By the Stock system, the names are iron(II) chloride and iron(III) chloride (Figure $\PageIndex{2}$ ).

Table $\PageIndex{3}$ : Naming the $FeCl_2$ and $FeCl_3$ Compounds in the Modern/Stock System.
Name of cation (metal) + (Roman Numeral in parenthesis) + Base name of anion (nonmetal) and -ide

If we were to use the stems and suffixes of the common system, the names would be ferrous chloride and ferric chloride, respectively (Figure $\PageIndex{3}$ ) .

Table $\PageIndex{4}$ : Naming the $FeCl_2$ and $FeCl_3$ Compounds in the Old/Common System.
"Old" base name of cation (metal) and -ic or -ous + Base name of anion (nonmetal) and -ide
-ous (for ions with lower charge)	-ic (for ions with higher charge)

Example $\PageIndex{4}$ :

Name each ionic compound.

Co₂O₃
FeCl2

Solution

Solutions to Example 5.7.4
	Explanation	Answer
a	We know that cobalt can have more than one possible charge; we just need to determine what it is. Oxide always has a 2− charge, so with three oxide ions, we have a total negative charge of 6−. This means that the two cobalt ions have to contribute 6+, which for two cobalt ions means that each one is 3+. Therefore, the proper name for this ionic compound is cobalt(III) oxide.	cobalt(III) oxide
b	Iron can also have more than one possible charge. Chloride always has a 1− charge, so with two chloride ions, we have a total negative charge of 2−. This means that the one iron ion must have a 2+ charge. Therefore, the proper name for this ionic compound is iron(II) chloride.	iron(II) chloride

Exercise $\PageIndex{4}$

Name each ionic compound.

AuCl₃
PbO₂
CuO

Answer a:: gold(III) chloride
Answer b:: lead(IV) oxide
Answer c:: copper(II) oxide

Naming Ionic Compounds with Polyatomic Ions

The process of naming ionic compounds with polyatomic ions is the same as naming binary ionic compounds. The cation is named first, followed by the anion. One example is the ammonium sulfate compound in Figure $\PageIndex{6}$ .

(NH4)2SO4 is named as ammonium sulfate. — Figure $\PageIndex{2}$ : Naming Ionic Compounds with Polyatomic Ions

Example $\PageIndex{5}$ : Naming Ionic Compounds

Write the proper name for each ionic compound.

(NH₄)₂S
AlPO₄,
Fe₃(PO₄)₂

Solution

Solutions to Example 5.7.5
Explanation	Answer
a. The ammonium ion has a 1+ charge and the sulfide ion has a 2− charge. Two ammonium ions need to balance the charge on a single sulfide ion. The compound’s name is ammonium sulfide.	ammonium sulfide
b. The ions have the same magnitude of charge, one of each (ion) is needed to balance the charges. The name of the compound is aluminum phosphate.	aluminum phosphate
c. Neither charge is an exact multiple of the other, so we have to go to the least common multiple of 6. To get 6+, three iron(II) ions are needed, and to get 6−, two phosphate ions are needed . The compound’s name is iron(II) phosphate.	iron(II) phosphate

Exercise $\PageIndex{5A}$

Write the proper name for each ionic compound.

(NH₄)₃PO₄
Co(NO₂)₃

Answer a:: ammonium phosphate
Answer b:: cobalt(III) nitrite

Figure $\PageIndex{1}$ is a synopsis of how to name simple ionic compounds.

3.7.jpg — Figure $\PageIndex{3}$ : A Guide to Naming Simple Ionic Compounds.

Exercise $\PageIndex{5B}$

Name each ionic compound.

ZnBr₂
Al₂O₃
(NH₄)₃PO₄
AuF₃
AgF

Answer a:: zinc bromide

Answer b:: aluminum oxide

Answer c:: ammonium phosphate

Answer d:: gold(III) fluoride or auric fluoride

Answer e:: silver fluoride

Summary

Ionic compounds are named by stating the cation first, followed by the anion.
Positive and negative charges must balance.
Some anions have multiple forms and are named accordingly with the use of roman numerals in parentheses.
Ternary compounds are composed of three or more elements.