The carbon atoms in diamond are bonded to each other by

Options

A. ionic bond
B. Coordinate bond
C. hydrogen bonds
D. covalent bonds

Explanation

To determine how carbon atoms in diamond are bonded to each other, we can follow these steps:

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

**Hint:** Think about the arrangement of atoms in diamond and how they connect to each other.

### Step 2: Identify the Type of Bonding
The bonds between the carbon atoms in diamond are formed by sharing electrons. This is characteristic of covalent bonding. In covalent bonds, atoms share pairs of electrons to achieve stability.

**Hint:** Recall the definition of covalent bonds and how they differ from ionic or hydrogen bonds.

### Step 3: Determine the Hybridization
In diamond, each carbon atom undergoes sp³ hybridization. This means that one s orbital and three p orbitals mix to form four equivalent sp³ hybrid orbitals, which are arranged tetrahedrally around each carbon atom.

**Hint:** Consider how hybridization affects the bonding and geometry of the molecule.

### Step 4: Eliminate Other Bond Types
- **Ionic Bonds:** These require a significant difference in electronegativity between two atoms, which is not the case for carbon atoms.
- **Hydrogen Bonds:** These occur between hydrogen and electronegative atoms, which is not applicable here.
- **Coordinate Bonds:** These require one atom to donate a lone pair, which carbon does not have in this context.

**Hint:** Analyze why the other bond types do not apply to carbon bonding in diamond.

### Conclusion
Based on the above reasoning, the carbon atoms in diamond are bonded to each other by **covalent bonds**.

**Final Answer:** Covalent Bonds.

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