In which of the following compounds carbon is in highest oxidation state ?

Options

A. `CH_(3)Cl`
B. `C Cl_(4)`
C. `CHCl_(3)`
D. `CH_(2)Cl_(2)`

Explanation

To determine the compound in which carbon is in the highest oxidation state, we will calculate the oxidation state of carbon in each of the given compounds. Let's analyze each compound step by step.

### Step 1: Analyze CH₃Cl
1. Let the oxidation state of carbon be \( X \).
2. The oxidation state of hydrogen is \( +1 \) and chlorine is \( -1 \).
3. The equation for the oxidation state can be set up as follows:
\[ X + (3 \times +1) + (-1) = 0 \]
\[ X + 3 - 1 = 0 \]
\[ X + 2 = 0 \implies X = -2 \]

### Step 2: Analyze CCl₄
1. Let the oxidation state of carbon be \( X \).
2. The oxidation state of chlorine is \( -1 \).
3. The equation for the oxidation state can be set up as follows:
\[ X + (4 \times -1) = 0 \]
\[ X - 4 = 0 \implies X = +4 \]

### Step 3: Analyze CHCl₃
1. Let the oxidation state of carbon be \( X \).
2. The oxidation state of hydrogen is \( +1 \) and chlorine is \( -1 \).
3. The equation for the oxidation state can be set up as follows:
\[ X + (1 \times +1) + (3 \times -1) = 0 \]
\[ X + 1 - 3 = 0 \]
\[ X - 2 = 0 \implies X = +2 \]

### Step 4: Analyze CH₂Cl₂
1. Let the oxidation state of carbon be \( X \).
2. The oxidation state of hydrogen is \( +1 \) and chlorine is \( -1 \).
3. The equation for the oxidation state can be set up as follows:
\[ X + (2 \times +1) + (2 \times -1) = 0 \]
\[ X + 2 - 2 = 0 \]
\[ X + 0 = 0 \implies X = 0 \]

### Summary of Results
- In CH₃Cl, the oxidation state of carbon is \( -2 \).
- In CCl₄, the oxidation state of carbon is \( +4 \).
- In CHCl₃, the oxidation state of carbon is \( +2 \).
- In CH₂Cl₂, the oxidation state of carbon is \( 0 \).

### Conclusion
The highest oxidation state of carbon among the given compounds is in **CCl₄**, where carbon has an oxidation state of **+4**.

### Final Answer
The compound in which carbon is in the highest oxidation state is **CCl₄**.

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