Write the chemical formulas for the following compounds: (a) aluminum hydroxide (b) potassium sulfate (c) copper(I) oxide (d) zinc nitrate (e) mercury(II) bromide

Verified step by step guidance

1. Identify the oxidation state of copper in copper(I) oxide, which is +1.
2. Recognize that the oxide ion has a charge of -2.
3. Determine the ratio of copper ions to oxide ions needed to balance the charges. Since copper has a +1 charge and oxide has a -2 charge, two copper ions are needed for every oxide ion.
4. Write the chemical formula by placing the number of each ion as subscripts: Cu_2O.
5. Ensure the formula is simplified and correctly represents the compound, which is Cu_2O for copper(I) oxide.

Key Concepts

Oxidation States

Oxidation states indicate the degree of oxidation of an atom in a compound. In copper(I) oxide, copper has an oxidation state of +1, meaning it has lost one electron. Understanding oxidation states is crucial for determining the correct chemical formula of compounds, especially for transition metals that can exhibit multiple oxidation states.

Ionic Compounds

Ionic compounds are formed when metals react with nonmetals, resulting in the transfer of electrons. In the case of copper(I) oxide, copper (a metal) combines with oxygen (a nonmetal) to form an ionic bond. The resulting compound consists of copper ions and oxide ions, which together create a neutral compound.

Chemical Nomenclature

Chemical nomenclature is the system of naming chemical compounds based on their composition and structure. For copper(I) oxide, the name reflects the oxidation state of copper and the presence of oxygen. Proper nomenclature helps in accurately writing the chemical formula, which in this case is Cu2O, indicating two copper ions for every oxide ion.