Question

In diamond, each carbon atom is bonded to four other carbon atoms forming a:

• A. Hexagonal structure
• B. Rigid three-dimensional structure
• C. Football-shaped structure
• D. Ring structure

Hint:

Diamond contains a giant three-dimensional covalent network in which every carbon atom is bonded to four other carbon atoms. This is the primary reason for its exceptional hardness.

Answer 1

The Correct Option is B

Concept: Diamond is one of the most important allotropes of carbon. The remarkable hardness and strength of diamond arise from its unique atomic arrangement. Each carbon atom uses all four of its valence electrons to form covalent bonds with four neighboring carbon atoms.

Step 1: Understand the bonding in diamond.
Every carbon atom in diamond undergoes \(sp^3\) hybridization. As a result, each carbon atom forms four strong covalent bonds directed toward the corners of a tetrahedron. \[ \text{Each carbon atom} \longrightarrow 4 \text{ covalent bonds} \] This arrangement leaves no free electrons in the structure.

Step 2: Examine the crystal structure.
The tetrahedral arrangement repeats continuously throughout the crystal. The covalent bonds extend in all directions, producing a giant interconnected network. Unlike graphite, diamond does not consist of separate layers. Instead, the entire crystal behaves as a single giant molecule.

Step 3: Relate structure to properties.
Because every carbon atom is firmly attached to four neighboring atoms by strong covalent bonds:

• Diamond is extremely hard.

• It has a very high melting point.

• It possesses great mechanical strength.

• It forms a rigid three-dimensional network.
Hence, the correct answer is: \[ \boxed{\text{Rigid three-dimensional structure}} \]