Write the formula for each ionic compound. a. copper(II) chloride

Verified step by step guidance

1. Identify the ions involved: Copper(II) indicates Cu^{2+} and chloride indicates Cl^{-}.
2. Determine the charges: Copper(II) has a charge of +2, and chloride has a charge of -1.
3. Balance the charges: To balance the charges, you need two chloride ions to balance one copper ion.
4. Write the formula: Combine the ions in the ratio that balances the charges, which is CuCl_2.
5. Verify the formula: Ensure that the total positive charge equals the total negative charge, confirming the formula is correct.

Key Concepts

Ionic Compounds

Ionic compounds are formed when atoms transfer electrons, resulting in the formation of positively charged cations and negatively charged anions. These oppositely charged ions attract each other, creating a stable compound. The overall charge of the compound must be neutral, which is achieved by balancing the charges of the ions involved.

Nomenclature of Ionic Compounds

The nomenclature of ionic compounds involves naming the cation first, followed by the anion. For transition metals, like copper, the oxidation state is indicated in parentheses. For example, in copper(II) chloride, the 'II' indicates that copper has a +2 charge, while chloride has a -1 charge, leading to the formula CuCl2.

Charge Balance in Ionic Formulas

To write the correct formula for an ionic compound, it is essential to ensure that the total positive charge from the cations equals the total negative charge from the anions. In the case of copper(II) chloride, one copper ion (Cu²⁺) balances with two chloride ions (Cl⁻), resulting in the formula CuCl2, which reflects this charge balance.