The oxidation state of chromium in `Cr(CO)_(6)` is

Options

A. 0
B. `+2`
C. `-2`
D. `+6`

Explanation

To determine the oxidation state of chromium in the complex Cr(CO)₆, we can follow these steps:

### Step 1: Identify the components of the complex
The complex Cr(CO)₆ consists of chromium (Cr) and six carbon monoxide (CO) ligands.

### Step 2: Determine the nature of the ligands
Carbon monoxide (CO) is a neutral ligand, meaning it does not carry any charge. Therefore, each CO contributes 0 to the overall charge of the complex.

### Step 3: Analyze the overall charge of the complex
The question states that there is no overall charge on the complex Cr(CO)₆. This means that the total charge of the chromium and the ligands must equal zero.

### Step 4: Set up the equation for oxidation state
Let the oxidation state of chromium be represented as x. Since there are six neutral CO ligands, their contribution to the charge is 0. Therefore, we can set up the equation:

\[ x + (6 \times 0) = 0 \]

### Step 5: Solve for the oxidation state
From the equation, we have:

\[ x = 0 \]

Thus, the oxidation state of chromium in Cr(CO)₆ is 0.

### Conclusion
The oxidation state of chromium in Cr(CO)₆ is 0.

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