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Write the empirical formula for at least four ionic compounds that could be formed from the following ions:

[tex]Fe^{3+}, Fe^{2+}, OH^{-}, C_2H_3O_2^{-}[/tex]

Sagot :

GinnyAnsweridn
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.
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