In graphite, each `C` atom is

Options

A. `sp^(3)`
B. sp
C. `sp^(2)`
D. None of these

Answer

To answer the question "In graphite, each C atom is...", we need to analyze the structure and bonding of carbon atoms in graphite.

### Step-by-Step Solution:

1. **Understanding Graphite Structure**:
- Graphite is a form of carbon where each carbon atom is arranged in a hexagonal lattice. This means that the carbon atoms are bonded in a two-dimensional plane.

2. **Bonding in Graphite**:
- In graphite, each carbon atom is bonded to three other carbon atoms. This results in a planar structure where the carbon atoms form a series of interconnected hexagons.

3. **Valence Electrons of Carbon**:
- Carbon has four valence electrons. In graphite, three of these electrons are used to form sigma bonds with three neighboring carbon atoms.

4. **Hybridization**:
- Since each carbon atom forms three sigma bonds, the hybridization of carbon in graphite is determined by the number of bonds formed. The remaining fourth electron is involved in delocalized π-bonding across the layers of graphite.
- The hybridization that corresponds to three sigma bonds is **sp² hybridization**.

5. **Conclusion**:
- Therefore, in graphite, each carbon atom is **sp² hybridized**.

### Final Answer:
In graphite, each C atom is **sp² hybridized**.

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