Diamond is an example of

Options

A. metallic crystal
B. molecular crystal
C. ionic crystal
D. covalent crystal

Answer

**Step-by-Step Solution:**

1. **Understanding the Structure of Diamond:**
- Diamond is a form of carbon where the carbon atoms are arranged in a specific way. Each carbon atom is bonded to four other carbon atoms.

**Hint:** Think about how carbon atoms are connected in diamond. What type of bond do they form?

2. **Identifying the Type of Bonding:**
- The bonds between the carbon atoms in diamond are covalent bonds. This means that the atoms share electrons to achieve stability.

**Hint:** Recall the definition of covalent bonding. What does it mean for atoms to share electrons?

3. **Recognizing the Crystal Structure:**
- Diamond forms a giant three-dimensional (3D) network. This structure is characteristic of covalent crystals, where a large number of atoms are bonded together in a continuous network.

**Hint:** Consider how the arrangement of atoms in diamond differs from other types of crystals. What makes it unique?

4. **Eliminating Other Options:**
- The other options provided are:
- A) Metallic crystal
- B) Molecular crystal
- C) Ionic crystal
- Diamond does not exhibit properties of metallic bonding (where electrons are delocalized), molecular bonding (which involves discrete molecules), or ionic bonding (which involves the transfer of electrons between atoms).

**Hint:** Think about the characteristics of metallic, molecular, and ionic crystals. How do they differ from covalent crystals?

5. **Conclusion:**
- Based on the structure and bonding of diamond, we conclude that diamond is an example of a covalent crystal.

**Final Answer:** D) Diamond is an example of a covalent crystal.