Rules of Naming Oxyanions

Rules of Naming Oxyanions

1. The name has a root taken from the name of the central atom ( for example, carbonate, CO3 -2 , and nitrate, NO3 -).

2. The names of the ions usually end in -ite or -ate. The -ite ending idicated the anion with the smaller number of oxygens. Thus, the NO2- ion is the nitrite ion. The -ate ending indivated the one with the higher number of oxgens. thus, NO3 ion is the nitrate ion.

3. When more than two polyatomic ions exist with the same central atom, the prefixes hypo- and per- (as in hyper-) are used to indicate the smallest and the largest number of oxygens. For example,

ClO- Hypochlorite, ClO2 -    chlorite,  ClO3 - chlorate, ClO4 - perchlorate, MnO- permanganale

4. There are some exceptions to these generalizations. The names of the hydroxide (OH-), peroxide (O2 -2), and cyanide (CN-) ions for example, have the -ide ending because they were once thought to be monoatomic ions.

5. A polyatomic anions with a charge more neative than 1- may add a hydrogen cation (H+) to give another anion. These anions are named from the parent anion by adding the word hydrogen. For example

HCO3- hydrogen carbonate, HPO4 -2 hydrogen phosphate, H2PO4 - dihydrogen phosphate, HSO4- hydrogen sulfate, HSO3- hydrogen sulfite, HS- hydrogen sulfide, HC2O4- hydrogen oxalate.

Comments 4 comments

miztical 6 years ago

the mathematical way of naming oxoaionsd

aaa 4 years ago

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paula092097 4 years ago

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LADY GAGO 2 years ago

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