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| comparison of bond length |
- Multiple bonds are shorter than single covalent bonds.
- Double and triple covalent bonds are stronger than single covalent bonds and they are characterized by the sharing of four or six electrons between atoms, respectively.
- Double and triple bonds are comprised of sigma bonds between hybridized orbitals, and pi bonds between unhybridized p orbitals.
- Double and triple bonds offer added stability to compounds, and restrict any rotation around the bond axis.
- Bond lengths between atoms with multiple bonds are shorter than in those with single bonds.
- Bond length is defined as the distance between the nuclei of two covalently bonded atoms in a molecule.
- For a given pair of atoms such as carbon and nitrogen, triple bonds are shorter than double bond, which, in turn are shorter than single bond.