Explain the formation of Triple bond with diagram.

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Solution

Acetylene molecule contains a triple bond between two C atoms. Each C atom is sp hybridised. The 2s orbital and one 2p orbital (for each C atom) hybridises to form two sp hybridized orbitals. These two hybrid orbitals are linear with angle of 180 $^{o}$ . sp hybrid orbital of one C atom overlaps with sp hybrid orbital of other C atom to form a C-C sigma bond. The remaining sp hybrid orbital of each C atom overlaps with 1s orbital of H to form C-H sigma bonds. Now each C atom is left with two p orbitals.
If Z is the molecular axis, then P $_{x}$ and P $_{y}$ orbitals are remaining on each C atom. P $_{x}$ orbital on one C atom overlaps with P $_{x}$ orbital on another C atom to form a pi bond. Similarly, P $_{y}$ orbital on one C atom overlaps with P $_{y}$ orbital on another C atom to form a pi bond. Thus a triple bond is formed between two C atoms. The triple bond contains one sigma and two pi bonds.

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In the context of hydrocarbons, consider the following statements,

i) Compounds with single bonds are more stable than those with double or triple bonds.

ii) During the formation of the double or triple bonds, the spatial orientation of other orbitals changes and interelectronic repulsions increase.

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