Chemistry: Rules for Naming Compounds, Polyatomic Ions

Is there a metal present?

NO: This is type III, use prefixes (ex: Dioxygen difluoride)

YES: Then, does the metal form more than one cation?
If so, Type II: determine the charge of the cation and use a Roman numeral after the element name for the cation
If no, it is Type I. Use the element name for the cation.

Rules for naming binary compounds
1. Cation always named first and the anion is named second.
2. A monatomic cation takes its name from the name of the element. For example, Na+ is called sodium in the names of compounds containing this ion.
3. A monatomic anion is named by taking the root of the element name and adding -ide. (ex: Cl- ion is called chloride)
Rules for Type 1 Binary Compounds: Binary Ionic Compounds
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Using the principle of charge balance, determine the cation charge.
Include in the cation name a Roman numeral indicating the charge.
Type 2 Binary Ionic Compounds
Both type 1 and type 2 binary ionic compounds can involve polyatomic ions that must be memorized

Note on several series of polyatomic anions that contain an atom of a given element and different numbers of oxygen atoms: these anions are called OXYANIONS

When there are two members in a series like this, the name of the one with the smaller # of oxygen atoms ends in -ite and the name of the one with the larger # ends in -ate.

ex: sulfite SO3 2- and sulfate SO4 2-

When more than two oxyanions make up a series, hypo- (less than) and per- (more than) are used as prefixes to name the members of the series w/the fewest and the most oxygen atoms

ex: CLO – (hypochlorite)
CLO2 – (chlorite)
CLO3 – (chlorate)
CLO4 – (perchlorate)

can think of -ite being the suffix for the “sprite,” or the oxyanion with the smaller number of oxygen atoms

Ionic compounds with polyatomic ions
Binary covalent compounds are formed between two nonmetals. Although these compounds do not contain ions, they are named very similarly to binary ionic compounds:

1. The first element in the formula is named first, using the full element name.
2. The second element is named as if it were an anion
3. Prefixes are used to denote # of atoms present
4. Prefix mono- is never used for naming the first element. Ex: CO is called carbon monoxide, not monocarbon monoxide.

Binary COVALENT Compounds: Type III
Naming Acids
An acid can be viewed as a molecule with one or more H+ ions attached to an anion. (So, yes: HCL is an acid)

If the anion does not contain oxygen, the acid is named with the prefix hydro- and the suffix -ic.
example: HCL is hydrochloric acid

When the anion contains oxygen, the acidic name is formed from the root name of the anion with a suffix of -ic or -ous depending on the name of the anion.

1. If the anion name ends in -ate, the suffix -ic is added to the root name. ex: H2SO4 contains the sulfate anion (SO4 2-) and is called sulfuric acid.

2. If the anion name ends in -ite, the -ite is replaced by -ous. Ex: H2SO3 (contains sulfite -> SO3 2-), is named sulfurous acid

So basically, when naming acids and there is oxygen in the anion, use -ous if the anion name ends in -ite and -ic if the anion name ends in -ate.

Naming Acids
Hydrogen sulfate (or bisulfate)
Hydrogen sulfate (or bisulfate)
Sulfate
Sulfate
Sulfite
Sulfite
Nitrate
Nitrate
Nitrite
Nitrite
Mercury (I)
Mercury (I)
Ammonium
Ammonium
Hypochlorite
Hypochlorite
Hydrogen carbonate (or bicarbonate)
Hydrogen carbonate (or bicarbonate)
Carbonate
Carbonate
Thiocyanate
Thiocyanate
Dihydrogen phosphate
Dihydrogen phosphate
Hydrogen Phosphate
Hydrogen Phosphate
Phosphate
Phosphate
Cyanide
Cyanide
Hydroxide
Hydroxide
Chlorate
Chlorate
Chlorite
Chlorite
Acetate
Acetate
Perchlorate
Perchlorate
Permanganate
Permanganate
Dichromate
Dichromate
Chromate
Chromate
Oxalate
Oxalate
Peroxide
Peroxide
Bromate anion
Bromate anion
Hydronium
Hydronium
Iodate
Iodate
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