To determine the correct formula for tin(IV) sulfide, follow these steps:
1. Identify the oxidation states:
- Tin(IV) means tin has an oxidation state of +4.
- Sulfide is derived from sulfur, which typically has an oxidation state of -2.
2. Balance the charges:
- Tin (Sn) has a +4 charge.
- Each sulfide ion (S) has a -2 charge.
3. Determine the ratio of ions to balance the overall charge:
- To balance the +4 charge of tin, we need enough sulfide ions to neutralize the charge. Since each sulfide ion has a -2 charge, we need two sulfide ions to balance the +4 charge of one tin ion:
[tex]\[ +4 + (-2) \times 2 = 0 \][/tex]
4. Write the chemical formula:
- Since we need one tin ion (Sn) and two sulfide ions (S) to balance the charges, the formula for tin(IV) sulfide is [tex]\( SnS_2 \)[/tex].
Thus, the correct answer is:
C. [tex]\( SnS_2 \)[/tex]
