Hybridisation

The electrons rearrange themselves again after 1 electron is promoted in a process called hybridisation. This reorganises the electrons into hybrid orbitals

• 1 electron from 2s orbital is promoted to empty 2p orbital • atom is now in excited state • hybridisation of 1 s-orbital and 3 p-orbital • 4 sp3 hybrids orbitals are available for bonding • ie. methane CH4

After sp3 hybridisation

• 4 sigma bonds • Therefore, 4 single bonds are formed • ie. methane CH4

• 1 electron from 2s orbital is promoted to empty 2p orbital • atom is now in excited state • hybridisation of 1 s-orbital and 2 p-orbital. 1 p-orbital doesnt take part in hybridisation • 3 sp2 hybrids orbital and 1 p-orbital are available for bondings • ie, ethene

After sp2 hybridisation

• 3 sigma bonds (single bonds) & 1 pi bond • 1 sigma bond and 1 pi bond forms 1 double bond • therefore, 3 single bonds with 1 empty p-orbital • or 2 single bond and 1 double bond are formed • ie, ethene C2H4

• 1 electron from 2s orbital is promoted to empty 2p orbital • cabon atom is now in excited state • hybridisation of 1 s-orbital and 1 p-orbital. 2 p-orbital doesnt take part in hybridisation • 2 sp1 hybrids orbital and 2 p-orbital are available for bonding • ie,ethyene C2H2

After sp1hybridisation

• 2 sigma bonds (single bonds) & 2 pi bond • 1 sigma bond and 2 pi bond forms 1 triple bond • therefore, 2 single bonds with 2 empty p-orbital • or 1 single bond and 1 triple bond are formed • ie, ethyene C2H2