Maximum oxidation state is present in

Options

A. `CrO_(2)Cl_(2)` and `MnO_(4)^(ө)`
B. `MnO_(2)`
C. `[Fe(CN)_(6)]^(3-)` and `[Co(CN)_(6)]^(3-)`
D. `MnO`

Explanation

To determine which compound has the maximum oxidation state, we will analyze the oxidation states of chromium (Cr), manganese (Mn), and chlorine (Cl) in the given compounds: CrO2, Cl2, and MnO4^-.

### Step-by-Step Solution:

1. **Analyze CrO2**:
- Let the oxidation state of Cr be \( x \).
- The oxidation state of oxygen (O) is \(-2\).
- The compound is neutral, so we can set up the equation:
\[ x + 2(-2) = 0 \]
- Simplifying gives:
\[ x - 4 = 0 \implies x = +4 \]

2. **Analyze Cl2**:
- In elemental form, the oxidation state of Cl in Cl2 is \( 0 \).

3. **Analyze MnO4^-**:
- Let the oxidation state of Mn be \( x \).
- The oxidation state of oxygen is \(-2\) and there are 4 oxygens, so:
\[ x + 4(-2) = -1 \]
- Simplifying gives:
\[ x - 8 = -1 \implies x = +7 \]

4. **Compare the oxidation states**:
- From the calculations:
- Cr in CrO2: +4
- Cl in Cl2: 0
- Mn in MnO4^-: +7

5. **Conclusion**:
- The maximum oxidation state among the given compounds is +7, which is present in MnO4^-.

### Final Answer:
The maximum oxidation state is present in **MnO4^-**.