Determine the oxidation number of the element as indicated
Cr in `CrO_(2)Cl_(2)`

Answer

To determine the oxidation number of chromium (Cr) in the compound \( \text{CrO}_2\text{Cl}_2 \), we can follow these steps:

### Step-by-Step Solution:

1. **Identify the Compound**: We have the compound \( \text{CrO}_2\text{Cl}_2 \).

2. **Assign Oxidation States**:
- The oxidation state of oxygen (O) is typically \(-2\).
- The oxidation state of chlorine (Cl) is typically \(-1\).

3. **Set Up the Equation**:
- Let the oxidation number of chromium (Cr) be \( x \).
- In the compound \( \text{CrO}_2\text{Cl}_2 \), there are 2 oxygen atoms and 2 chlorine atoms.
- The total contribution from the oxygen atoms is \( 2 \times (-2) = -4 \).
- The total contribution from the chlorine atoms is \( 2 \times (-1) = -2 \).

4. **Write the Charge Balance Equation**:
- Since the compound is neutral, the sum of the oxidation states must equal zero:
\[ x + (-4) + (-2) = 0 \]

5. **Simplify the Equation**:
- Combine the terms:
\[ x - 6 = 0 \]

6. **Solve for \( x \)**:
- Rearranging gives:
\[ x = +6 \]

7. **Conclusion**:
- The oxidation number of chromium (Cr) in \( \text{CrO}_2\text{Cl}_2 \) is \( +6 \).

### Final Answer:
The oxidation number of chromium in \( \text{CrO}_2\text{Cl}_2 \) is \( +6 \).