Assign oxidation numbers to each element in the following compounds. (a) NO2

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Step 1: Understand the rules for assigning oxidation numbers.

Step 2: Assign the oxidation number for oxygen (O), which is typically -2 in compounds.

Step 3: Let the oxidation number of nitrogen (N) be x.

Step 4: Set up the equation based on the compound's neutrality: x + 2(-2) = 0.

Step 5: Solve the equation for x to find the oxidation number of nitrogen.

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Oxidation Numbers

Oxidation numbers are a way to keep track of electron transfer in chemical reactions. They represent the hypothetical charge an atom would have if all bonds were ionic. The rules for assigning oxidation numbers include that the oxidation number of an element in its elemental form is zero, and for compounds, the sum of oxidation numbers must equal the overall charge of the molecule.

Rules for Assigning Oxidation Numbers

There are specific rules for assigning oxidation numbers, such as oxygen typically having an oxidation number of -2, and hydrogen usually being +1. In compounds, the more electronegative element is assigned a negative oxidation number, while the less electronegative element is assigned a positive one. These rules help in determining the oxidation states of each element in a compound.

Balancing Oxidation States

When assigning oxidation numbers, it is essential to ensure that the total oxidation states balance to equal the charge of the compound. For neutral compounds, the sum of the oxidation numbers must be zero. This balancing act is crucial for understanding redox reactions and the transfer of electrons between species.