Identify the formula for lead(IV) oxide.

Lead(IV) oxide is represented by the formula PbO2. The nomenclature indicates that lead (Pb) is in the +4 oxidation state, which is designated by the Roman numeral IV. The oxide ion (O) has a -2 charge.

To achieve charge neutrality in the compound, one lead ion with a +4 charge will combine with two oxide ions, each with a -2 charge. This results in the formula PbO2, as the two negative charges from the oxide ions balance the single positive charge from the lead ion, leading to a neutral compound.

The other options do not fit this description: PbO denotes lead(II) oxide, where lead has a +2 charge; Pb2O4 suggests a more complex ratio that suggests two lead ions for every four oxide ions, which would reduce to PbO2 but isn't the correct way to express lead(IV) oxide; PbO3 refers to a hypothetical compound that does not align with common nomenclature or known behavior of lead and oxygen in straightforward binary compounds.

Thus, PbO2 accurately reflects the required oxidation states and the proper stoichiometry for lead(IV) oxide.