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Bonds - 1. Sigma Bonds
Sigma bonds
  • Formed by combining atomic orbitals or hybrid atomic orbitals
  • Located within the plane of the molecule
  • Circularly symmetric about the bond axis
  • Head-on overlap (hybrid orbitals maximize overlap)
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Bonds - 1. Sigma Bonds

Sigma Bonds
  • Sigma bonds are bonding molecular orbitals formed by combining atomic orbitals or hybrid atomic orbitals.
  • They form single bonds within the plane of the molecule.
  • Sigma bonds are circularly symmetric about the bond axis.
Sigma bonds look the same no matter how much they are rotated around the bond axis, which is the line that forms the bond between the two atoms.
Let's learn how to visualize the circular symmetry of electron density of a sigma bond.
  • Draw the nuclei of two atoms contained within electron spheres.
  • Connect them with a bond axis and combine them.
  • Indicate that when the two orbitals overlap, their electron density takes on an elliptical shape (like a symmetrical watermelon or football).
Then re-draw them as follows:
  • Draw the two atoms enclosed in a three-dimensional ellipsoid shape.
  • Next, slice through the center of the bond axis with a rectangular plane.
  • Carve out the ellipsoid shape.
  • Indicate that the cross-sectional plane is circular.
Key points
  • Sigma bonds comprise a circular cross-sectional plane.
  • All single bonds are sigma bonds.