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: Charges:
Sn has $+4$ and each oxide ion has $-2$.

Step 2: Balance:
To cancel $+4$ we need two oxide ions: $(+4) + 2(-2) = 0$.
So one Sn atom pairs with two O atoms: $\text{SnO}_2$. Option D, $\text{SnO}$, is the tin(II) oxide with only one oxygen.

Final Answer:
The formula is $\text{SnO}_2$, option (B). \[ \boxed{\text{SnO}_2} \]