Oxidation Numbers in PbO2

The video tutorial explains how to determine the oxidation numbers in lead(IV) oxide (PbO2). It begins by stating that the sum of oxidation numbers in a compound is zero and that oxygen typically has an oxidation number of -2. With two oxygen atoms, the total is -4, requiring lead to have an oxidation number of +4 to balance it out. This is why the compound is called lead(IV) oxide. The tutorial also demonstrates an algebraic method to verify this calculation, confirming that lead's oxidation number is indeed +4. The video concludes with a summary of the findings.

What is the typical oxidation number of oxygen in compounds?

• +1

• 0

• -2

• +2

In PbO2, what is the total oxidation number contributed by the two oxygen atoms?

• -2

• -4

• +4

• +2

What must be the oxidation number of lead in PbO2 to balance the compound to zero?

• +2

• +3

• +1

• +4

Why is PbO2 referred to as lead(IV) oxide?

• Because oxygen has an oxidation number of +4

• Because the compound has four oxygen atoms

• Because lead has an oxidation number of +4

• Because lead has an oxidation number of +2

In the algebraic method, what equation is set up to find the oxidation number of lead in PbO2?

• x - 4 = 0

• x + 4 = 0

• x - 2 = 0

• x + 2(-2) = 0

What is the final oxidation number of lead in PbO2 using the algebraic method?

• +2

• +3

• +4

• +1