
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.
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.
Ethane belongs to the simplest form of hydrocarbons with only single bonds, that is Alkane. It has:
Here is a complete understanding of its hybridisation.
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:

Four unpaired electrons → enough to form four bonds
Ground state vs excited state orbital diagram
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
Each carbon uses its 4 sp³ orbitals to form:
Result:
Geometry and bonding of ethane
| 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 |
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
Formal charge = 4 – (0 + ½×8) = 4 – 4 = 0
Hydrogen (H) – each
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.
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.
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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