Certainly! We can determine the empirical formulas for the ionic compounds formed by combining the given ions using the principle of charge balance. An empirical formula reflects the simplest whole-number ratio of cations to anions that results in a neutrally charged compound. Here’s a step-by-step construction of four such compounds:
### Step 1: Combine [tex]\( Fe^{3+} \)[/tex] with [tex]\( OH^{-} \)[/tex]
1. The charge on [tex]\( Fe^{3+} \)[/tex] is +3, and the charge on [tex]\( OH^{-} \)[/tex] is -1.
2. To balance the charges, we need three [tex]\( OH^{-} \)[/tex] ions to neutralize one [tex]\( Fe^{3+} \)[/tex] ion.
3. Therefore, the formula of the compound is [tex]\( Fe(OH)_3 \)[/tex].
### Step 2: Combine [tex]\( Fe^{3+} \)[/tex] with [tex]\( C_2H_3O_2^{-} \)[/tex]
1. The charge on [tex]\( Fe^{3+} \)[/tex] is +3, and the charge on [tex]\( C_2H_3O_2^{-} \)[/tex] is -1.
2. To balance the charges, we need three [tex]\( C_2H_3O_2^{-} \)[/tex] ions to neutralize one [tex]\( Fe^{3+} \)[/tex] ion.
3. Therefore, the formula of the compound is [tex]\( Fe(C_2H_3O_2)_3 \)[/tex].
### Step 3: Combine [tex]\( Fe^{2+} \)[/tex] with [tex]\( OH^{-} \)[/tex]
1. The charge on [tex]\( Fe^{2+} \)[/tex] is +2, and the charge on [tex]\( OH^{-} \)[/tex] is -1.
2. To balance the charges, we need two [tex]\( OH^{-} \)[/tex] ions to neutralize one [tex]\( Fe^{2+} \)[/tex] ion.
3. Therefore, the formula of the compound is [tex]\( Fe(OH)_2 \)[/tex].
### Step 4: Combine [tex]\( Fe^{2+} \)[/tex] with [tex]\( C_2H_3O_2^{-} \)[/tex]
1. The charge on [tex]\( Fe^{2+} \)[/tex] is +2, and the charge on [tex]\( C_2H_3O_2^{-} \)[/tex] is -1.
2. To balance the charges, we need two [tex]\( C_2H_3O_2^{-} \)[/tex] ions to neutralize one [tex]\( Fe^{2+} \)[/tex] ion.
3. Therefore, the formula of the compound is [tex]\( Fe(C_2H_3O_2)_2 \)[/tex].
### Formulated Compounds:
1. [tex]\( Fe(OH)_3 \)[/tex]: Formed by [tex]\( Fe^{3+} \)[/tex] and [tex]\( OH^{-} \)[/tex]
2. [tex]\( Fe(C_2H_3O_2)_3 \)[/tex]: Formed by [tex]\( Fe^{3+} \)[/tex] and [tex]\( C_2H_3O_2^{-} \)[/tex]
3. [tex]\( Fe(OH)_2 \)[/tex]: Formed by [tex]\( Fe^{2+} \)[/tex] and [tex]\( OH^{-} \)[/tex]
4. [tex]\( Fe(C_2H_3O_2)_2 \)[/tex]: Formed by [tex]\( Fe^{2+} \)[/tex] and [tex]\( C_2H_3O_2^{-} \)[/tex]
These are four possible ionic compounds with their empirical formulas based on the combination of the given ions.
