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What is the formula for tin(IV) sulfide?

A. SnS
B. [tex]SnS_4[/tex]
C. [tex]SnS_2[/tex]
D. [tex]Sn_4S[/tex]

Sagot :

GinnyAnsweridn
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]
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