Assign oxidation numbers to each element in the following compounds. (e) OsO4

Verified step by step guidance

1. Identify the oxidation number of oxygen, which is typically -2 in compounds.
2. Let the oxidation number of osmium (Os) be x.
3. Write the equation for the sum of oxidation numbers in the compound: x + 4(-2) = 0, since the compound is neutral.
4. Simplify the equation: x - 8 = 0.
5. Solve for x to find the oxidation number of osmium.

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 reactions. The rules for assigning oxidation numbers include that the oxidation number of an element in its elemental form is zero, and for monoatomic ions, it equals the charge of the ion.

Rules for Assigning Oxidation Numbers

There are specific rules for assigning oxidation numbers, such as hydrogen typically having an oxidation number of +1, oxygen usually being -2, and the sum of oxidation numbers in a neutral compound equaling zero. In polyatomic ions, the sum of oxidation numbers equals the charge of the ion. Understanding these rules is essential for accurately determining oxidation states in compounds.

Oxidation and Reduction Reactions

Oxidation and reduction (redox) reactions involve the transfer of electrons between substances. Oxidation refers to the loss of electrons (increase in oxidation number), while reduction refers to the gain of electrons (decrease in oxidation number). Recognizing the oxidation states of elements in compounds like OsO4 is crucial for identifying which species are oxidized and reduced in a reaction.