Diamond is

Options

A. an insulator
B. a conductor
C. a semiconductor
D. none of these

Answer

To determine the electrical properties of diamond, we need to analyze its atomic structure and the presence of free electrons. Here’s a step-by-step solution:

### Step 1: Understand the Structure of Diamond
Diamond is a crystalline form of carbon where each carbon atom is tetrahedrally bonded to four other carbon atoms. This structure is very stable and rigid.

**Hint:** Remember that the bonding in diamond involves each carbon atom sharing its electrons with neighboring carbon atoms.

### Step 2: Identify the Valence Electrons
Each carbon atom has four valence electrons. In diamond, these valence electrons are involved in covalent bonding with adjacent carbon atoms.

**Hint:** Valence electrons are the outermost electrons that can participate in bonding.

### Step 3: Analyze Free Electrons
For a material to conduct electricity, it must have free electrons that can move freely through the lattice. In diamond, all four valence electrons of each carbon atom are involved in bonding and are not free to move.

**Hint:** Free electrons are essential for electrical conductivity; if all electrons are bonded, there are no free electrons available.

### Step 4: Classify Diamond Based on Conductivity
Since diamond has no free electrons available for conduction, it cannot conduct electricity. Therefore, it is classified as an insulator.

**Hint:** Insulators are materials that do not allow the flow of electric current due to the absence of free charge carriers.

### Conclusion
Based on the analysis, we conclude that diamond is an insulator.

**Final Answer:** Diamond is an insulator.

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