Assign oxidation numbers to each element in the following ions. (e) BrO-

Verified step by step guidance

1. Identify the overall charge of the ion, which is -1 for \( \text{BrO}^- \).
2. Assign the oxidation number of oxygen as -2, which is typical for oxygen in most compounds.
3. Let the oxidation number of bromine be \( x \).
4. Set up the equation based on the sum of oxidation numbers equaling the charge of the ion: \( x + (-2) = -1 \).
5. Solve the equation for \( x \) to find the oxidation number of bromine.

Key Concepts

Oxidation Numbers

Oxidation numbers are a way to keep track of electrons in chemical compounds, indicating the degree of oxidation of an atom. They are assigned based on a set of rules, such as the oxidation number of an element in its elemental form is zero, and the sum of oxidation numbers in a neutral compound is zero, while in a polyatomic ion, it equals the ion's charge.

Rules for Assigning Oxidation Numbers

There are specific rules for assigning oxidation numbers, including that oxygen typically has an oxidation number of -2, hydrogen is +1 when bonded to non-metals, and halogens usually have an oxidation number of -1 unless they are bonded to oxygen or other halogens. These rules help in determining the oxidation states of elements in compounds.

Polyatomic Ions

Polyatomic ions are charged species composed of two or more atoms covalently bonded, which together carry a net charge. In the case of the bromate ion (BrO-), understanding its structure and charge is essential for correctly assigning oxidation numbers to its constituent elements, in this case, bromine and oxygen.