Write the formula for each of the following compounds: a....

Write the formula for each of the following compounds:
a. chromium(VI) oxide
b. disulfur dichloride
c. nickel(II) fluoride
d. potassium hydrogen phosphate
e. aluminum nitride
$\mathbf{f}$. ammonia
g. manganese(IV) sulfide
h. sodium dichromate
i. ammonium sulfite
i. carbon tetraiodide

Key Concepts

Ionic and Covalent Compound Formation

Understanding whether a compound is ionic or covalent is key to determining its formula. Ionic compounds, often formed between metals and nonmetals (including polyatomic ions), require balancing charges, while covalent compounds, typically formed between nonmetals, are denoted by combining element symbols with subscripts that indicate the number of atoms present.

Charge Neutrality

The charge neutrality principle states that the total positive charge from cations must equal the total negative charge from anions in a neutral compound. Applying this concept ensures the correct stoichiometric ratios, which are used to write accurate chemical formulas.

Oxidation States

Oxidation states denote the number of electrons lost or gained by an element in a compound, and are essential for writing formulas when elements, especially transition metals, can have multiple valence states. They help determine the correct ratio of elements necessary for charge balance in the compound.

Chemical Nomenclature

Chemical nomenclature provides a systematic set of rules for naming compounds, allowing chemists to deduce the composition and structure of a compound from its name and vice versa. This involves identifying the types of elements present, their ratios, and specific indications such as oxidation states for transition metals.

Polyatomic Ions

Polyatomic ions are groups of covalently bonded atoms that carry an overall charge and behave as a single ion in reactions. Recognizing common polyatomic ions is crucial when writing formulas, as it simplifies the process of balancing charges within ionic compounds.

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