Carbon is in the lowest oxidation state in

Options

A. `CH_(4)`
B. `C Cl_(4)`
C. `CF_(4)`
D. `CO_(2)`

Explanation

To determine the lowest oxidation state of carbon in the given compounds, we will analyze each compound one by one. The oxidation state of an element in a compound can be calculated using the following formula:

\[ \text{Sum of oxidation states} = 0 \] (for neutral compounds)

Let's analyze each compound:

1. **CH₄ (Methane)**:
- Let the oxidation state of carbon be \( x \).
- Hydrogen has an oxidation state of +1.
- The equation will be:
\[ x + 4(+1) = 0 \]
\[ x + 4 = 0 \]
\[ x = -4 \]

2. **CCl₄ (Carbon Tetrachloride)**:
- Let the oxidation state of carbon be \( x \).
- Chlorine has an oxidation state of -1.
- The equation will be:
\[ x + 4(-1) = 0 \]
\[ x - 4 = 0 \]
\[ x = +4 \]

3. **CF₄ (Carbon Tetrafluoride)**:
- Let the oxidation state of carbon be \( x \).
- Fluorine has an oxidation state of -1.
- The equation will be:
\[ x + 4(-1) = 0 \]
\[ x - 4 = 0 \]
\[ x = +4 \]

4. **CO₂ (Carbon Dioxide)**:
- Let the oxidation state of carbon be \( x \).
- Oxygen has an oxidation state of -2.
- The equation will be:
\[ x + 2(-2) = 0 \]
\[ x - 4 = 0 \]
\[ x = +4 \]

Now, let's summarize the oxidation states calculated:
- CH₄: -4
- CCl₄: +4
- CF₄: +4
- CO₂: +4

From the calculations, we can see that the lowest oxidation state of carbon is in **CH₄**, where it is -4.

**Final Answer**: Carbon is in the lowest oxidation state in **CH₄**.