Name the compounds in parts a-d and write the formulas for...

Name the compounds in parts a-d and write the formulas for the compounds in parts e-h.
a. NaBr
b. $\mathrm{Rb}_{2} \mathrm{O}$
c. $\mathrm{CaS}$
d. AII $_{3}$
e. strontium fluoride
f. aluminum selenide
g. potassium nitride
h. magnesium phosphide

Key Concepts

Charge Balance and Oxidation States

Understanding the typical oxidation states of elements is crucial for balancing the charges in an ionic compound. The principles of charge balance require that the sum of the positive and negative charges in the compound equals zero, leading to the correct empirical formulas for ionic compounds.

Writing Chemical Formulas

Writing chemical formulas for ionic compounds involves determining the correct ratio of cations to anions so that the overall charge is zero. This balancing is achieved by using the charges of the ions to determine the subscripts in the formula, ensuring that the total positive and negative charges cancel each other.

Ionic Compound Nomenclature

Naming ionic compounds requires identifying the constituent ions and applying specific naming rules. The metal or cation is usually named first followed by the anion. For monatomic anions, the element's root name is modified to end in -ide, while polyatomic anions have distinct names. In cases where a metal can form more than one ion, its oxidation state is indicated in parentheses using Roman numerals.

Ionic Bonding

Ionic bonding refers to the formation of chemical compounds by the electrostatic attraction between oppositely charged ions. In these compounds, metals typically lose electrons to form positively charged cations, while nonmetals gain electrons to form negatively charged anions. The resulting lattice structure is held together by the strong ionic forces between the ions.

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