Graphite is an example of:

Options

A. ionic solid
B. covalent solid
C. metallic solid
D. none of these

Answer

**Step-by-Step Solution:**

1. **Identify the Nature of Graphite:**
- Graphite is an allotrope of carbon, which means it is a different structural form of the same element.

2. **Determine the Hybridization of Carbon in Graphite:**
- In graphite, each carbon atom is sp² hybridized. This hybridization leads to a planar structure where each carbon atom is bonded to three other carbon atoms.

3. **Understand the Structure of Graphite:**
- Graphite has a layered, sheet-like structure. The carbon atoms form hexagonal rings, and these sheets are stacked on top of one another.

4. **Analyze the Bonding in Graphite:**
- The carbon-carbon bonds within the sheets are covalent bonds, formed by the sharing of electrons. These bonds are strong and non-polar.

5. **Examine Inter-sheet Interactions:**
- The sheets in graphite are held together by weak Van der Waals forces. These forces are much weaker than covalent bonds.

6. **Evaluate Electrical Conductivity:**
- Graphite is a good conductor of electricity due to the presence of delocalized electrons within the sheets. These free electrons can move and carry charge.

7. **Consider the Types of Solids:**
- Ionic solids consist of charged ions held together by strong electrostatic forces. Graphite does not have charged particles; hence, it cannot be classified as an ionic solid.
- Metallic solids consist of metal atoms with metallic bonding. Since graphite is composed of carbon (a non-metal), it cannot be classified as a metallic solid.
- Covalent solids are characterized by atoms bonded together by covalent bonds. Since graphite has covalent bonds between carbon atoms, it fits this category.

8. **Conclusion:**
- Based on the analysis, graphite is classified as a covalent solid.

**Final Answer:**
Graphite is an example of a covalent solid.

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