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Home / Chemistry / Understanding the Hybridization of Acetylene

Understanding the Hybridization of Acetylene

Last Updated on Jul 12, 2025
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Have you ever wondered how atoms bond together to form different shapes and molecules? That’s where hybridisation comes in. It’s a concept in chemistry that helps us understand how atomic orbitals mix to form new orbitals for bonding. Hybridisation makes it easier to explain the structure, shape and bonding in molecules like methane, ethene, and acetylene. If you’re preparing for exams like NEET or JEE, knowing the basics of hybridisation will help you solve many bonding and structure related questions easily.

What is Acetylene?

Acetylene is a simple hydrocarbon with the formula C2H2. It has two carbon atoms, triple bonded to each other and one hydrogen atom attached to each carbon. It’s a colourless gas used in welding and as a building block in organic chemistry. Understanding its structure helps in learning about sp hybridisation.

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Hybridisation of Acetylene

In acetylene (C2H2), each carbon atom forms two bonds one with hydrogen and one with another carbon. To do this, the carbon atoms use sp hybridization. This means one s orbital and one p orbital mix to form two sp hybrid orbitals, which arrange in a straight line. The remaining two p orbitals on each carbon stay unhybridised and help form the two π bonds of the triple bond. This type of bonding gives acetylene its linear shape and strong C≡C triple bond.

Step by Step Explanation of sp Hybridisation in Acetylene

Each carbon atom in acetylene has the electron configuration 1s2 2s2 2p2. To form bonds, one 2s orbital and one 2p orbital combine to form two sp hybrid orbitals.

  • One sp orbital forms a sigma bond with hydrogen
  • The other forms a sigma bond between the two carbon atoms
  • The remaining two unhybridised p orbitals on each carbon overlap sideways to form two π bonds, completing the C≡C triple bond

Molecular Geometry of Acetylene

Because the carbon atoms are sp hybridised, the molecule takes a linear shape.

  • The bond angle between H–C≡C–H is 180°.
  • All atoms lie in a straight line, which is a key feature of sp hybridisation

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Comparison with other Hydrocarbons

Molecule

Formula

Hybridization

Bond Type

Geometry

Ethane

C₂H₆

sp³

Single bonds

Tetrahedral

Ethene

C₂H₄

sp²

Double bond (C=C)

Trigonal planar

Acetylene

C₂H₂

sp

Triple bond (C≡C)

Linear

Importance of Hydrocarbons
  • Helps understand how atoms from bonds
  • Explains the shape of molecules 
  • Tells whether a bond is single, double or triple
  • Helps identify bond angles in molecule
  • Useful for predicting how reactive a molecule is

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FAQs

There are three sigma bonds and two pi bonds in C2H2.

Yes, C2H2 is linear in shape.

No, C2H2 is a nonpolar molecule.

The molecule C2H2 has no isomers. It is a linear, symmetrical molecule with only one type of atomic arrangement possible.

The IUPAC name of C2H2 is Ethyne and the common name of C2H2 is acetylene.
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