What is the formula ? lead (IV) Oxide
The Correct Answer and Explanation is:
The correct chemical formula for lead (IV) oxide is PbO₂.
Explanation
Lead (IV) oxide is a chemical compound composed of the metal lead and oxygen. To write its formula correctly, we must understand the oxidation state of lead and the charges involved in forming an electrically neutral compound.
The Roman numeral IV in “lead (IV) oxide” indicates that the lead ion has a +4 charge. This is important because lead can exhibit more than one oxidation state — the most common being +2 and +4. The oxidation state tells us how many electrons an atom has lost, and it determines how the atom will bond with other elements.
Oxygen, in most of its compounds, has a -2 charge (as the oxide ion, O²⁻). To balance the +4 charge of one lead (IV) ion, we need two oxide ions, each with a -2 charge:
- Lead (IV) ion: Pb⁴⁺
- Oxide ion: O²⁻
To make a neutral compound, the total positive and negative charges must cancel each other:
- Pb⁴⁺ (one ion contributes +4)
- 2 × O²⁻ (two ions contribute -4)
Thus, the total charge is:
+4 + (-4) = 0, which is neutral.
So, combining one lead (IV) ion and two oxide ions gives the formula PbO₂.
Lead (IV) oxide is a brown or dark red crystalline solid and is used as an oxidizing agent in various chemical reactions. It is also found in the positive plate of lead-acid batteries, where it plays an essential role in energy storage and discharge.
Understanding how to write the formula of such compounds helps in identifying how elements bond and form stable structures. It is a fundamental skill in both inorganic chemistry and real-world applications like battery chemistry and industrial catalysis.
