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Understanding Hybridisation of C₂H₆: Ethane

Understanding Hybridisation of C₂H₆: Ethane

Ethane (C₂H₆), after methane, is the second simplest alkane. Ethane is a type of saturated hydrocarbon with a Tetrahedral structure and a single bond between its two carbon atoms. It’s a common example of sp³ hybridisation in organic chemistry.

Let us understand how hybridisation happens in C₂H₆. Read on to learn how it leads to its bonding and molecular shape.

What is the Hybridisation of C₂H₆?

Ethane consists of two carbon atoms and six hydrogen atoms. Each carbon atom is bonded to three hydrogen atoms and one other carbon atom, which makes four sigma bonds. In order to form these bonds and satisfy the octet rule, carbon undergoes sp³ hybridisation.

Breakdown of C₂H₆ Hybridisation

Ethane belongs to the simplest form of hydrocarbons with only single bonds, that is Alkane. It has:

  • 2 carbon atoms
  • 6 hydrogen atoms
  • 1 C–C bond and 6 C–H bonds

Here is a complete understanding of its hybridisation.

Electronic Configuration of Carbon

The atomic number of carbon is 6.

The ground state of carbon :

1s² 2s² 2p²

Only two unpaired electrons → insufficient to form four bonds

Excited state configuration:

formula

Four unpaired electrons → enough to form four bonds

Hybridization Of Ethane

 Ground state vs excited state orbital diagram

Formation of Hybrid Orbitals

sp³ hybridisation occurs when 1 s orbital and 3 p orbitals mix.
The result:
→ 4 sp³ hybrid orbitals per carbon atom
→ There is no unhybridized orbital left

Bond Formation in Ethane

Each carbon uses its 4 sp³ orbitals to form:

  • 3 σ bond with hydrogen
  • 1 σ bond with the other carbon

Result:

  • 6 C–H σ bonds (each carbon has 3)
  • 1 C–C σ bond
  • Hybridisation type: sp³
  • Bond angle: 109.5°
  • Geometry: Tetrahedral
 Hybridization Of Ethane

 Geometry and bonding of ethane

Details At A Glance

Property Details
Molecule Ethane (C₂H₆)
Hybridisation sp³
Geometry Tetrahedral
Bond angle ~109.5°
Bonding 7 σ bonds (6 C–H, 1 C–C)
Unhybridized Orbitals 0 (all are used in hybridisation)
Carbon valency satisfied? Yes, by forming 4 bonds on each carbon atom

Formal Charge in C₂H₆

To determine if the Lewis structure of C₂H₆ is stable, we calculate the formal charge on each atom using the formula:

Formal charge = Valence electrons – (Lone pair electrons + ½ × Bonding electrons)

Step-by-step for each atom:

Carbon (C) – each

  • Valence electrons: 4
  • Lone pairs: 0
  • Bonding electrons: 8
    (2 electrons from one single bond with another C, 6 from one single bond with H)

Formal charge = 4 – (0 + ½×8) = 4 – 4 = 0

Hydrogen (H) – each

  • Valence electrons: 1
  • Lone pairs: 0
  • Bonding electrons: 2
    (1 single bond with carbon)

Formal charge = 1 – (0 + ½×2) = 1 – 1 = 0

Thus, all atoms in C₂H₆ carry zero formal charge, confirming that the Lewis structure is stable and correct.

Summing Up

Each carbon in C₂H₆ forms 4 bonds: 1 with another carbon and 3 with hydrogen (4 σ). sp³ hybridisation leads to a tetrahedral shape and ~109.5° bond angles. Ethane is a saturated molecule and is nonpolar since hybridisation changes its overall symmetry.

Frequently Asked Questions

Q1. Why does carbon undergo hybridisation in C₂H₆?

To form 4 covalent bonds, carbon promotes an electron and mixes orbitals to form hybrid orbitals.

Q2. How many σ and π bonds are present in C₂H₆?

There are 7 σ bonds and 0 π bonds in total.

Q3. What is the shape of ethane?

Due to sp³ hybridisation on each carbon atom, both carbons have a tetrahedral geometry.

Q4. Is C₂H₆ polar or nonpolar?

Ethane is nonpolar, as there is equal sharing of electrons, and it has symmetrical geometry.

Q5. What are some uses of alkane in our lives?

Alkane is mainly used in feedstock petrochemicals. Alkane is also used in the production of ethylene, and even in refrigeration.

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