The oxidation state of Cr in `CrO_(5)` is

Options

A. `+6`
B. `+10`
C. `+5`
D. `+4`

Answer

To find the oxidation state of chromium (Cr) in `CrO_(5)`, we can follow these steps:

### Step-by-Step Solution:

1. **Identify the oxidation state of oxygen**:
- Oxygen typically has an oxidation state of -2.

2. **Calculate the total contribution of oxygen in `CrO_(5)`**:
- Since there are 5 oxygen atoms, the total contribution from oxygen is:
\[ 5 \times (-2) = -10 \]

3. **Set up the equation for the oxidation state of chromium**:
- Let the oxidation state of chromium be \( x \).
- The sum of the oxidation states in a neutral compound must equal zero. Therefore, we can write the equation:
\[ x + (-10) = 0 \]

4. **Solve for \( x \)**:
- Rearranging the equation gives:
\[ x = +10 \]

5. **Determine the maximum oxidation state of chromium**:
- The maximum oxidation state of chromium is +6. Since the calculated oxidation state of +10 exceeds this, it indicates that there are peroxy linkages present in the compound.

6. **Calculate the number of peroxy linkages**:
- The difference between the calculated oxidation state and the maximum oxidation state is:
\[ 10 - 6 = 4 \]
- Since each peroxy linkage reduces the oxidation state by 1, we divide this difference by 2:
\[ \text{Number of peroxy linkages} = \frac{4}{2} = 2 \]

7. **Conclusion**:
- Therefore, the oxidation state of chromium in `CrO_(5)` is +6, considering the presence of 2 peroxy linkages.

### Final Answer:
The oxidation state of Cr in `CrO_(5)` is +6.