Assign oxidation numbers to each element in the following compounds. (b) CuSO4

Verified step by step guidance

1. Identify the oxidation number of oxygen in compounds, which is typically -2.
2. Recognize that the oxidation number of sulfur in sulfate (SO₄²⁻) is usually +6.
3. Calculate the total oxidation number for the four oxygen atoms in sulfate: 4 * (-2) = -8.
4. Set up the equation for the sulfate ion: x (oxidation number of sulfur) + (-8) = -2 (overall charge of sulfate), and solve for x.
5. Determine the oxidation number of copper (Cu) by knowing that the compound is neutral, so the sum of oxidation numbers in CuSO₄ must equal zero. Use the known oxidation numbers to find the oxidation state of copper.

Key Concepts

Oxidation Numbers

Oxidation numbers are a way to keep track of electrons in chemical compounds. They indicate the degree of oxidation of an atom in a molecule, helping to determine how electrons are transferred during chemical reactions. The oxidation number of an element can be positive, negative, or zero, depending on its electron gain or loss relative to its elemental state.

Rules for Assigning Oxidation Numbers

There are specific rules for assigning oxidation numbers, such as: the oxidation number of an atom in its elemental form is zero; for monoatomic ions, it equals the charge of the ion; in compounds, hydrogen typically has an oxidation number of +1, while oxygen usually has -2. These rules help systematically determine the oxidation states of elements in various compounds.

Copper(II) Sulfate (CuSO4)

Copper(II) sulfate, or CuSO4, is a compound where copper has an oxidation state of +2. The sulfate ion (SO4) has a charge of -2, which is balanced by the +2 charge from copper. Understanding the structure and oxidation states in CuSO4 is essential for correctly assigning oxidation numbers to each element in the compound.