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Difficulty: MediumTetrahedral Carbon, Bonding, and Hybridization

Match each carbon species or bond descriptor on the left with its corresponding hybridization state, geometric configuration, or orbital overlap mode on the right.

  • Central carbon in methane (CH4\text{CH}_4)sp3sp^3 hybridized with tetrahedral geometry (109.5∘109.5^\circ)
  • Carbon-carbon double bond π\pi componentSideways overlap of unhybridized pp orbitals
  • Central carbon in carbon dioxide (CO2\text{CO}_2)spsp hybridized with linear geometry (180∘180^\circ)
  • Carbon atom in ethene (C2H4\text{C}_2\text{H}_4)sp2sp^2 hybridized with trigonal planar geometry (120∘120^\circ)

Answer

The central carbon in methane matches sp3sp^3 hybridization with tetrahedral geometry (109.5∘109.5^\circ); the π\pi bond component matches sideways overlap of unhybridized pp orbitals; the central carbon in carbon dioxide matches spsp hybridization with linear geometry (180∘180^\circ); and the carbon in ethene matches sp2sp^2 hybridization with trigonal planar geometry (120∘120^\circ).
Each carbon atom's hybridization and spatial arrangement depend directly on its steric number (number of σ\sigma bonds). Methane features four σ\sigma bonds (sp3sp^3, 109.5∘109.5^\circ tetrahedral). Ethene features three σ\sigma bonds per carbon (sp2sp^2, 120∘120^\circ trigonal planar). Carbon dioxide features two σ\sigma bonds (spsp, 180∘180^\circ linear). Π\Pi bonds are characterized by the sideways overlap of unhybridized 2p2p atomic orbitals.

Step-by-Step Solution

1
Determine the steric number and geometry of the carbon in methane (CH4\text{CH}_4).
Four single σ\sigma bonds give a steric number of 4, which dictates sp3sp^3 hybridization and a tetrahedral angle of 109.5∘109.5^\circ.
Mixing one ss and three pp orbitals forms four equivalent sp3sp^3 hybrid orbitals pointing to tetrahedral corners.
2
Identify how a carbon-carbon π\pi bond is formed.
It forms via lateral/sideways overlap of parallel, unhybridized pp orbitals above and below the internuclear axis.
Head-on overlap forms σ\sigma bonds, whereas parallel side-by-side overlap creates π\pi electron clouds.
3
Analyze the steric environment around the carbon in carbon dioxide (CO2\text{CO}_2).
The carbon forms two σ\sigma bonds (one to each oxygen atom) and two π\pi bonds, yielding a steric number of 2, corresponding to spsp hybridization and 180∘180^\circ linear geometry.
Two hybrid orbitals position themselves as far apart as possible at 180∘180^\circ.
4
Determine the hybridization and bond angles of carbon in ethene (C2H4\text{C}_2\text{H}_4).
Each carbon atom forms three σ\sigma bonds (steric number 3), requiring sp2sp^2 hybridization with a trigonal planar shape and 120∘120^\circ bond angles.
Three hybrid orbitals lie in a single plane separated by 120∘120^\circ.

Key Concept

Carbon Hybridization, Geometry, and Orbital Overlap
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Topics

Tetrahedral Carbon, Bonding, and Hybridization

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