Complete the exercises below. Write the chemical formula for each of the following compounds, and indicate the oxidation state of nitrogen in each: a. nitric oxide, b. hydrazine, c. potassium cyanide, d. sodium nitrite, e. ammonium chloride, f. lithium nitride.

A chemical formula represents the composition of a compound, indicating the types and numbers of atoms present. For example, in nitric oxide (NO), the formula shows one nitrogen atom and one oxygen atom. Understanding how to derive these formulas involves knowledge of valence electrons and the bonding behavior of elements.

The oxidation state (or oxidation number) of an element in a compound reflects its degree of oxidation or reduction, indicating how many electrons an atom has gained, lost, or shared. For nitrogen in compounds like hydrazine (N2H4) or sodium nitrite (NaNO2), determining the oxidation state requires applying rules based on the electronegativity of the other elements and the overall charge of the compound.

Compounds can be classified as ionic or covalent based on the nature of the bonds between their atoms. Ionic compounds, such as potassium cyanide (KCN), consist of metal and non-metal ions held together by electrostatic forces, while covalent compounds, like hydrazine, involve the sharing of electrons between non-metals. This distinction is crucial for predicting properties and behaviors of the compounds.