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

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Identify the overall charge of the ion, which is -1 for \( \text{BrO}^- \).

Assign the oxidation number of oxygen as -2, which is typical for oxygen in most compounds.

Let the oxidation number of bromine be \( x \).

Set up the equation based on the sum of oxidation numbers equaling the charge of the ion: \( x + (-2) = -1 \).

Solve the equation for \( x \) to find the oxidation number of bromine.

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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.

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02:42

Oxidation Numbers

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.

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Oxidation Number Rules

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.

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