On the basis of the expected charges on the monatomic ions, give the chemical formula of each of the following compounds: (a) manganese(II) telluride; (b) barium arsenide; (c) silicon nitride; (d) lithium bismuthide: (c) zirconium(IV) chloride.

Understanding oxidation states in the periodic table is a foundational skill for identifying the charges of ions when writing ionic compound formulas. Elements are organized into groups (vertical columns) where they exhibit similar chemical properties, including tendencies to lose or gain electrons, known as oxidation states.

For instance, alkali metals in group 1 have an oxidation state of +1, meaning they lose one electron when forming an ion. Alkaline earth metals in group 2 have an oxidation state of +2. Moving towards the right side of the periodic table, nonmetals like halogens in group 17 usually have an oxidation state of -1 because they tend to gain one electron. Oxygen in group 16 generally has an oxidation state of -2. The transition metals can have multiple oxidation states, which are typically indicated in parentheses within the compound name, such as manganese(II) indicating a +2 charge.

Writing chemical formulas involves pairing cations (positively charged ions) with anions (negatively charged ions) to form a neutral compound. The goal is to combine these ions in ratios that balance their charges to zero.

The skill lies in knowing the charges involved and using subscripts to indicate the number of each ion type needed to achieve neutrality. In the example of barium arsenide, we took the +2 charge from barium and the -3 charge from arsenic to determine that two arsenic ions are needed for every three barium ions, which is represented as Ba₃As₂. By understanding how to balance the charges, one can write the formula for any ionic compound.

Monatomic ions are ions composed of only one atom. The charge of a monatomic ion is determined by the loss or gain of electrons, with metals typically losing electrons to become cations, and nonmetals gaining electrons to become anions. The charges for these ions are predictable based on the group number of the periodic table.

For example, lithium (Li) is in group 1 and typically forms a +1 charged ion, noted as Li⁺. Chlorine (Cl), in group 17, forms a -1 charged ion, represented as Cl^-. It's critical for students to memorize these common charges as they are used frequently in chemical formula writing.

Binary compounds are chemical compounds composing of two different elements. The naming of binary compounds follows a specific nomenclature, especially when dealing with ionic compounds. The cation (positive ion) is named first, followed by the anion (negative ion). The anion's name is modified to end in '-ide', as seen in lithium bismuthide or manganese(II) telluride.

Understanding the nomenclature is essential for communication in chemistry, as it conveys the composition of the compound in a standard format. When multiple oxidation states are possible, such as with transition metals, the specific oxidation state is indicated in the compound's name using Roman numerals, directing the reader to the correct formula of the compound.