Determine the oxidation number for the indicated element in each of the following substances: d. Br in HBrO

Verified step by step guidance

1. Identify the oxidation number of hydrogen (H), which is typically +1.
2. Identify the oxidation number of oxygen (O), which is typically -2.
3. Let the oxidation number of bromine (Br) be x.
4. Set up the equation based on the sum of oxidation numbers in the compound HBrO, which must equal zero: (+1) + x + (-2) = 0.
5. Solve the equation for x to find the oxidation number of Br.

Key Concepts

Oxidation Number

The oxidation number, or oxidation state, is a theoretical charge assigned to an atom in a compound, reflecting its degree of oxidation or reduction. It helps in understanding electron transfer in redox reactions. Oxidation numbers can be positive, negative, or zero, and are determined based on a set of rules, such as the charge of ions and the typical states of elements in compounds.

Rules for Assigning Oxidation Numbers

There are specific rules for assigning oxidation numbers, including that the oxidation number of an element in its elemental form is zero, and for monoatomic ions, it equals the charge of the ion. In compounds, hydrogen typically has an oxidation number of +1, oxygen usually has -2, and the sum of oxidation numbers in a neutral compound must equal zero. These rules are essential for determining the oxidation state of elements in various compounds.

Structure of HBrO

HBrO, or hypobromous acid, consists of hydrogen (H), bromine (Br), and oxygen (O). In this compound, hydrogen is bonded to oxygen, which is further bonded to bromine. Understanding the molecular structure is crucial for determining the oxidation state of bromine, as it involves analyzing the contributions of hydrogen and oxygen to the overall charge and applying the rules for oxidation numbers accordingly.