<Tr> <Td> C * </Td> <Td> ↑ ↓ </Td> <Td> ↑ </Td> <Td> ↑ </Td> <Td> ↑ </Td> <Td> ↑ </Td> </Tr> <Tr> <Td> 1s </Td> <Td> sp </Td> <Td> sp </Td> <Td> 2p </Td> <Td> 2p </Td> </Tr> <P> resulting in two sp orbitals and two remaining p orbitals . The chemical bonding in acetylene (ethyne) (C H) consists of sp--sp overlap between the two carbon atoms forming a σ bond and two additional π bonds formed by p--p overlap . Each carbon also bonds to hydrogen in a σ s--sp overlap at 180 ° angles . </P> <P> Hybridisation helps to explain molecule shape, since the angles between bonds are (approximately) equal to the angles between hybrid orbitals, as explained above for the tetrahedral geometry of methane . As another example, the three sp hybrid orbitals are at angles of 120 ° to each other, so this hybridisation favours trigonal planar molecular geometry with bond angles of 120 ° . Other examples are given in the table below . </P>

What is the bond angle of sp hybridization