Graphite is a good conductor of electricity because it contains

Options

A. bonded electrons
B. mobile electrons
C. strong C-C bonds
D. strong C=C bonds.

Explanation

**Step-by-Step Solution:**

1. **Understanding the Structure of Graphite:**
- Graphite consists of carbon atoms arranged in layers. Each carbon atom is bonded to three other carbon atoms, forming a two-dimensional hexagonal lattice.

2. **Identifying the Bonding:**
- In graphite, the carbon atoms are connected by strong carbon-carbon single bonds (sigma bonds). Each carbon atom forms three sigma bonds with neighboring carbon atoms.

3. **Valence Electrons of Carbon:**
- The electronic configuration of carbon is 1s² 2s² 2p², indicating that carbon has four valence electrons. In graphite, three of these electrons are used to form sigma bonds with adjacent carbon atoms.

4. **Free Electrons:**
- The fourth valence electron of each carbon atom is not involved in bonding and remains free. This free electron can move easily within the structure, contributing to electrical conductivity.

5. **Hybridization:**
- The carbon atoms in graphite undergo sp² hybridization. This means that one s orbital and two p orbitals mix to form three sp² hybrid orbitals, which are used to form sigma bonds. The remaining p orbital remains unhybridized and is involved in the formation of delocalized π bonds across the layers.

6. **Conclusion:**
- The presence of these free-moving electrons (mobile electrons) is what makes graphite a good conductor of electricity.

**Final Answer:**
Graphite is a good conductor of electricity because it contains mobile electrons.

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