Anion names endings

The rule now used, without exception, is that anion names ending in ide , ite and ate , respectively, are changed to end in ido , ito and ato , respectively, when modifying the ligand name for use in additive nomenclature (Sections IR-7.1.3, and IR-9.2.2.3). This entails several changes from Refs. 11 and 22. 

When the anion name ends in -ite, name. For example. the suffix -ous is used in the acid... 

If the anion name ends in -ate, the suffix -ic is added to the root name. For example, H2SO4 contains the sulfate anion (S04 ) and is called sulfuric acid H3PO4 contains the phosphate anion (P04 ) and is called phosphoric acid and HC2H3O2 contains the acetate ion (C2H302 ) and is called acetic acid. 

When the anion contains oxygen, the acid name is formed from the root name of the central element of the anion or the anion name, with a suffix of -ic or -ous. When the anion name ends in -ate, the suffix -ic is used. 

If one and the same compound contains two (or more) cationic or anionic centers, some of these structural elements must be expressed as prefixes in the final name. Cation names ending with ium are traditionally prefixed as. ..io... and systematically as. ..iumyl... anion names ending with. ..ate or. ..ide transform into the prefix formats. ..ato... and. ..idyl..., respectively. Priorities are assigned as follows cations ... 

Heteroatomic and Other Anions. A few heteroatomic anions have names ending in -ide. These are... 

Other Polyatomic Anions. Names for other polyatomic anions consist of the root name of the central atom with the ending -ate and followed by the valence of the central atom expressed by its oxidation number. Atoms and groups attached to the central atom are treated as ligands in a complex. 

An oxoacid that forms from a polyatomic anion whose name ends in -ate has a name ending in -ic. For example, HNO3 forms by adding a proton to the nitrate polyatomic anion, so HNO3 is nitric acid. Likewise, HCIO4 is perchloric acid from the perchlorate anion. 

A The name of each of these ionic compounds is the name of the cation followed by that of the anion. Each anion name is a modified (with the ending ide ) version of the name of the element. Each cation name is the name of the metal, with the oxidation state appended in Roman numerals in parentheses if there is more than one type of cation for that metal. 

Anionic complexes always have names ending in ate. This will require a change in the name of the metal. Thus, aluminum would become aluminate, and zinc would become zincate. The only exceptions to this are some of the metals whose symbols are based on Latin or Greek names. These exceptions are ... 

A< Ba(Q02)2.Bcirium is an alkaline ecirth metal (Group IIA) and thus has a chcii e of -1-2. You should recognize chlorite as the name of a polyatomic ion. In fact, any anion name that doesn t end in -ide should scream polyatomic ion to you. As Table 6-1 shows, chlorite is ClOj , which reveals that the chlorite ion has a-1 charge. Two chlorite ions cire necessary to neutralize the -1-2 chcirge of a single barium cation, so the chemical formula is Ba(C102)2-... 

Hydrobromic acid. HBr is a binary acid it doesn t contain oxygen, so it isn t an oxy-acid. You begin by writing hydro-. Next, change the ending of the anion name, bromine, to -ic and write bromic after hydro- Write acid at the end, and you re done ... 

These compounds are all ordinciry ionic compounds, so you simply need to pair the cation name with the anion name and change the anion name s ending to -ide. 

Ligands are named first, starting with any anionic ones, and the name of the metal is followed without a space by the oxidation state in Roman numerals (or the Arabic 0, for zero-valent metal centers) in parentheses. If the complex as a whole is anionic, the metal name is made to end in -ate, which replaces endings such as -ium or -um (nickelate, chromate, tantalate) and is followed by the oxidation state. Where the chemical symbol is derived from a Latin name, the anion name is usually also Latinized cuprate, argentate, aurate, ferrate, stannate, plumbate—but mercurate is an exception. 

Traditional names are still accepted for the exceptions listed in (Table 1-4). The ending -ic of the acid name becomes -ate in the anion name, and -ous becomes -ite. 

Additive nomenclature1 is based on the combination of element names or roots of element names and/or ligand names. The simplest and oldest additive nomenclature is binary nomenclature that expresses two components, e.g. sodium chloride. The cationic or electropositive portion of the compound expressed in a binary name is the element name unchanged or a group name ending in -ium , and the anionic or electronegative portion of a compound expressed in the name ends in -ide, -ite or -ate. The proportions of cations and anions in neutral compounds are indicated by Stock numbers or simple or multiplicative prefixes (see Section 3.3.2). Additive nomenclature denotes composition. For examples see Table 1. 

FIGURE 2.11 Main-group cations and anions. A cation bears the same name as the element it is derived from an anion name has an -ide ending. 

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