PbO2 is:

(A) basic

(B) acidic

(C) neutral

(D) amphoteric

To determine the nature of lead(IV) oxide, or PbO2, we need to consider its chemical properties and how it interacts with acids and bases. The correct answer to your question is (D) amphoteric.

Understanding Amphotericity

An amphoteric substance is one that can react both as an acid and as a base, depending on the conditions and the substances it encounters. In the case of PbO2, it can react with both acids and bases, which is a key characteristic of amphoteric compounds.

Reactions with Acids

When PbO2 is treated with an acid, such as hydrochloric acid (HCl), it can react to form lead(II) chloride (PbCl2) and water. This reaction demonstrates its ability to act as a base:

• PbO2 + 4 HCl → PbCl2 + 2 H2O + Cl2

Reactions with Bases

Conversely, PbO2 can also react with strong bases, such as sodium hydroxide (NaOH), indicating its acidic behavior. In this scenario, it can form a lead(IV) hydroxide complex:

• PbO2 + 2 NaOH + 2 H2O → Na2[Pb(OH)4]

Comparative Properties

To further clarify why PbO2 is classified as amphoteric, let’s compare it with other types of oxides:

• Basic Oxides: These typically react only with acids. For example, magnesium oxide (MgO) is a basic oxide.
• Acidic Oxides: These react with bases but not with acids. An example is sulfur dioxide (SO2).
• Neutral Oxides: These do not react with either acids or bases, like carbon monoxide (CO).

Conclusion on PbO2

Given its ability to react with both acids and bases, PbO2 fits the definition of an amphoteric oxide. This property is significant in various chemical processes and applications, including its role in batteries and as a pigment in ceramics. Understanding these classifications helps in predicting the behavior of different compounds in chemical reactions.