Questions: Several tin salts are brightly colored. Give the name for each of the following ionic tin Part 1 of 4 SnBr2 (pale yellow solid): Part 2 of 4 SnCl2 (white solid): Part 3 of 4 SnBr4 (colorless solid):

Several tin salts are brightly colored. Give the name for each of the following ionic tin

Part 1 of 4
SnBr2 (pale yellow solid):

Part 2 of 4
SnCl2 (white solid):

Part 3 of 4
SnBr4 (colorless solid):

Transcript text: Several tin salts are brightly colored. Give the name for each of the following ionic tin Part 1 of 4 $\mathrm{SnBr}_{2}$ (pale yellow solid): $\square$ Part 2 of 4 $\mathrm{SnCl}_{2}$ (white solid): $\square$ Part 3 of 4 $\mathrm{SnBr}_{4}$ (colorless solid): $\square$

Solution

Solution Steps

Step 1: Identify the Cation and Anion in Each Compound

For each given compound, we need to identify the cation (tin ion) and the anion (bromide or chloride).

Step 2: Determine the Oxidation State of Tin

For $\mathrm{SnBr}_{2}$: Tin (Sn) is combined with two bromide ions (Br$^{-}$). Each bromide ion has a charge of -1, so the total negative charge is -2. Therefore, the tin ion must have a charge of +2 to balance the charges.
For $\mathrm{SnCl}_{2}$: Tin (Sn) is combined with two chloride ions (Cl$^{-}$). Each chloride ion has a charge of -1, so the total negative charge is -2. Therefore, the tin ion must have a charge of +2 to balance the charges.
For $\mathrm{SnBr}_{4}$: Tin (Sn) is combined with four bromide ions (Br$^{-}$). Each bromide ion has a charge of -1, so the total negative charge is -4. Therefore, the tin ion must have a charge of +4 to balance the charges.

Step 3: Name the Compounds

For $\mathrm{SnBr}_{2}$: The tin ion has a +2 charge, so the name is tin(II) bromide.
For $\mathrm{SnCl}_{2}$: The tin ion has a +2 charge, so the name is tin(II) chloride.
For $\mathrm{SnBr}_{4}$: The tin ion has a +4 charge, so the name is tin(IV) bromide.