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Sp hybridization is used to describe the bonding in the ethylene (acetylene) molecule. When a bond is formed between carbon atoms, two sp orbitals overlap to form a single σ-bond, and the remaining four non-hybrid p-orbitals overlap to form two π-bonds, resulting in a triple bond consisting of one σ-bond and two π-bonds. The π-bond electron distribution creates a cylindrical electron density around the bond axis. When a bond is formed between a carbon atom and a hydrogen atom, the sp orbital and s-orbital overlap again to form σ-bonds (simple bonds are formed).
