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Difficulty: EasyTetrahedral Carbon, Bonding, and Hybridization

Which of the following describes the type of orbital overlap that forms the carbon-carbon (C−C\text{C}-\text{C}) single bond in an ethane (C2H6C_2H_6) molecule?

  1. Head-on overlap of two sp3sp^3 hybrid orbitalsAnswer
  2. B
    Sideways overlap of two unhybridized pp orbitals
  3. C
    Head-on overlap of two sp2sp^2 hybrid orbitals
  4. D
    Sideways overlap of two sp3sp^3 hybrid orbitals

Answer

Head-on overlap of two sp3sp^3 hybrid orbitals
The carbon atoms in ethane (C2H6C_2H_6) are each bonded to four other atoms, giving them a tetrahedral arrangement and sp3sp^3 hybridization. The carbon-carbon single bond is a sigma (σ\sigma) bond formed by the direct head-on overlap of one sp3sp^3 hybrid orbital from each carbon atom.

Step-by-Step Solution

1
Determine the hybridization state of carbon atoms in ethane (C2H6C_2H_6)
Each carbon atom forms 4 single sigma (σ\sigma) bonds, corresponding to sp3sp^3 hybridization with tetrahedral geometry.
Saturated hydrocarbons (alkanes) undergo sp3sp^3 hybridization to accommodate four equivalent single bonds.
2
Identify the mode of overlap for the carbon-carbon single bond
The single bond between the two carbon atoms is a sigma (σ\sigma) bond.
Sigma bonds are always formed by direct end-to-end (head-on) overlap of atomic or hybrid orbitals along the bond axis.

Key Concept

Orbital overlap and hybridization in tetrahedral carbon (sp3sp^3 sigma bonding)
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Topics

Tetrahedral Carbon, Bonding, and Hybridization

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