To determine the correct formula for the ionic compound tin(IV) bromide, we need to understand the oxidation states of tin and bromine involved.
1. Identify the oxidation state of tin in tin(IV) bromide
- The Roman numeral "IV" in the name indicates that tin has an oxidation state of +4.
2. Identify the oxidation state of bromine in bromide
- Bromine typically has an oxidation state of -1 in bromide ions.
3. Determine the ratio of tin to bromine needed to balance the charges
- Tin (IV) has a charge of +4.
- Each bromide ion has a charge of -1.
- To neutralize the +4 charge of one tin ion, we need four bromide ions, each with a charge of -1.
4. Write the balanced formula
- Combining one tin ion (Sn) with four bromide ions (Br) yields the compound: SnBr₄
Considering the options provided:
1. \( \text{Sn } 4 \text{ Br} \)
2. \( \text{SnB} \)
3. \( \text{SnBr}_4 \)
4. \( \text{SnBr}_2 \)
The correct formula for tin(IV) bromide is \( \text{SnBr}_4 \).
Thus, the correct answer is:
[tex]\( \text{SnBr}_4 \)[/tex] (option 3)
