The charges x and y on the following ions are
`(i) [Co(NH_(3))_(2) Cl_(4)]^(x) " " (ii) [Fe(CN)_(6)]^(y)`
(Oxidation state of Co is +3 and Fe is + 2 in their respective complexes.)

Options

A. x = + 1 , y = - 1
B. x = -1 , y = + 3
C. x = -1 , y = -4
D. x = -2 , y = -3

Explanation

To find the charges \( x \) and \( y \) on the given coordination compounds, we will analyze each complex separately using the oxidation states provided.

### Step 1: Analyze the first complex \([Co(NH_3)_2Cl_4]^x\)

1. **Identify the oxidation state of cobalt (Co)**: It is given as +3.
2. **Determine the oxidation state of the ligands**:
- Ammonia (\(NH_3\)) is a neutral ligand, so its contribution is 0.
- Chlorine (\(Cl\)) typically has an oxidation state of -1.
3. **Set up the equation**:
\[ \text{Total charge} = \text{Oxidation state of Co} + \text{Sum of oxidation states of ligands} \]
\[ x = +3 + (2 \times 0) + (4 \times -1) \]
\[ x = +3 + 0 - 4 \]
\[ x = -1 \]

### Step 2: Analyze the second complex \([Fe(CN)_6]^y\)

1. **Identify the oxidation state of iron (Fe)**: It is given as +2.
2. **Determine the oxidation state of the ligands**:
- Cyanide (\(CN\)) has an oxidation state of -1.
3. **Set up the equation**:
\[ y = \text{Oxidation state of Fe} + \text{Sum of oxidation states of ligands} \]
\[ y = +2 + (6 \times -1) \]
\[ y = +2 - 6 \]
\[ y = -4 \]

### Final Answer
Thus, the charges on the ions are:
- \( x = -1 \)
- \( y = -4 \)