PASSAGE-I : Diamond and graphite are two allotropic forms of carbon which are crystalline in nature. They differ physically but chemically they are similar. Diamond is the hardest crystalline form of carbon. In diamond each carbon atom is linked to four other carbon atoms by covalent bonds. In graphite, each carbon atom is linked to three other carbon atoms by covalent bond. Graphite is relatively soft and greasy. It is a good conductor or electricity.
Which of the folowing types of forces bind together the carbon atoms in diamond?

Options

A. Ionic
B. Covalent
C. Polar
D. van der Waals'

Answer

To answer the question regarding the type of forces that bind together the carbon atoms in diamond, we can follow these steps:

### Step-by-Step Solution:

1. **Identify the Allotropic Form**: Recognize that diamond is an allotropic form of carbon. Allotropes are different physical forms of the same element, which in this case is carbon.

2. **Understand the Structure of Diamond**: In diamond, each carbon atom is bonded to four other carbon atoms. This forms a three-dimensional (3D) crystalline structure.

3. **Determine the Type of Bonding**: The bonds between the carbon atoms in diamond are formed by the sharing of electrons.

4. **Define the Type of Bond**: Since the bonds are formed by the sharing of electrons, they are classified as covalent bonds.

5. **Conclude the Answer**: Therefore, the forces that bind the carbon atoms in diamond are covalent bonds.

### Final Answer:
The carbon atoms in diamond are bound together by **covalent bonds**.

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