Which type of hybridization is observed in methane (CH₄)?

Which type of hybridization is observed in methane (CH₄)?

• A. sp² hybridization
• B. sp hybridization
• C. sp³ hybridization
• D. sp²d hybridization

Answer: (C)

In methane (CH₄), the central carbon atom undergoes sp³ hybridization to form four equivalent covalent bonds with hydrogen atoms. Sp³ hybridization occurs when one s orbital mixes with three p orbitals, resulting in four sp³ hybrid orbitals that are arranged tetrahedrally around the carbon atom. This geometry allows for maximum separation between the bonding pairs of electrons, minimizing repulsion according to VSEPR (Valence Shell Electron Pair Repulsion) theory. Each of the sp³ hybrid orbitals overlaps with the 1s orbital of a hydrogen atom to form a sigma (σ) bond, resulting in a stable configuration for the methane molecule. The tetrahedral arrangement observed in CH₄ leads to bond angles of approximately 109.5 degrees, consistent with the geometry predicted by sp³ hybridization. The other types of hybridization mentioned do not apply to methane. For example, sp² hybridization involves one s orbital and two p orbitals, leading to a trigonal planar geometry with bond angles of about 120 degrees, and sp hybridization involves one s and one p orbital, resulting in a linear geometry with 180-degree bond angles. Sp²d hybridization is not relevant here as it pertains to the

In methane (CH₄), the central carbon atom undergoes sp³ hybridization to form four equivalent covalent bonds with hydrogen atoms. Sp³ hybridization occurs when one s orbital mixes with three p orbitals, resulting in four sp³ hybrid orbitals that are arranged tetrahedrally around the carbon atom. This geometry allows for maximum separation between the bonding pairs of electrons, minimizing repulsion according to VSEPR (Valence Shell Electron Pair Repulsion) theory.

Each of the sp³ hybrid orbitals overlaps with the 1s orbital of a hydrogen atom to form a sigma (σ) bond, resulting in a stable configuration for the methane molecule. The tetrahedral arrangement observed in CH₄ leads to bond angles of approximately 109.5 degrees, consistent with the geometry predicted by sp³ hybridization.

The other types of hybridization mentioned do not apply to methane. For example, sp² hybridization involves one s orbital and two p orbitals, leading to a trigonal planar geometry with bond angles of about 120 degrees, and sp hybridization involves one s and one p orbital, resulting in a linear geometry with 180-degree bond angles. Sp²d hybridization is not relevant here as it pertains to the