Name each of the following compounds: a. CuI c. CoI2 b. CuI2...

Name each of the following compounds:
a. CuI
c. $\mathrm{CoI}_{2}$
b. $\mathrm{CuI}_{2}$
d. $\mathrm{Na}_{2} \mathrm{CO}_{3}$
e. $\mathrm{NaHCO}_{3}$
f. $\mathrm{S}_{4} \mathrm{~N}_{4}$
g. $\mathrm{SF}_{6}$
h. $\mathrm{NaOCl}$
i. $\mathrm{BaCrO}_{4}$
j. $\mathrm{NH}_{4} \mathrm{NO}_{3}$

Key Concepts

Ionic Compound Nomenclature

Ionic compounds are formed from the electrostatic attraction between cations and anions. The naming starts with the cation, followed by the anion. For metals with a fixed oxidation state, no additional oxidation number is needed, while transition metals (which can have variable oxidation states) are accompanied by their oxidation state in Roman numerals.

Transition Metal Nomenclature

Transition metals can have multiple oxidation states, so when they form compounds these oxidation states must be specified. This is done by placing a Roman numeral in parentheses immediately after the metal’s name to indicate its oxidation state in that particular compound.

Polyatomic Ions

Polyatomic ions are groups of atoms that act as a single charged entity. Common examples include carbonate (CO3^2-), bicarbonate (HCO3^-), chromate (CrO4^2-), nitrate (NO3^-), and ammonium (NH4^+). Their names must be memorized and incorporated into compound names correctly.

Binary Compound Naming

Binary compounds consist of two different elements. When naming them, the name of the first element (often a metal) is given first, followed by the name of the second element (often a nonmetal) with an -ide suffix. This systematic approach helps in consistently naming a wide variety of compounds.

Molecular (Covalent) Compound Nomenclature

Covalent compounds typically exist between nonmetals and are named using specific prefixes (mono-, di-, tri-, etc.) to indicate the number of atoms present. However, certain molecular compounds also have traditional names or structural formulas that deviate from these rules.

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