Question

What is the formula of Tin (IV) oxide?

• A. \(\text{Sn}_2\text{O}_3\)
• B. \(\text{SnO}_2\)
• C. \(\text{SnO}_4\)
• D. \(\text{SnO}\)

Hint:

The roman number gives the charge on tin, and oxygen is 2-.

Answer 1

The Correct Option is B

Step 1: Understanding the Concept:
The roman numeral in a name tells the oxidation state of the metal. Tin(IV) means \(\text{Sn}^{4+}\). Oxide is \(\text{O}^{2-}\).

Step 2: Key Formula or Approach:
The compound must be neutral, so the total positive charge equals the total negative charge. Use the criss-cross of charges.

Step 3: Detailed Explanation:
\(\text{Sn}^{4+}\) and \(\text{O}^{2-}\): criss-cross gives \(\text{Sn}_2\text{O}_4\), which reduces to \(\text{SnO}_2\).
Check: \(+4 + 2(-2) = 0\).
\(\text{Sn}_2\text{O}_3\) would need \(\text{Sn}^{3+}\), which is not the tin(IV) state. \(\text{SnO}_4\) would need \(\text{Sn}^{8+}\). \(\text{SnO}\) is tin(II) oxide.

Final Answer:
Tin(IV) oxide is \(\text{SnO}_2\), option (B). \[ \boxed{\text{SnO}_2} \]