Explain Sp3 Hybridization in Methane

Methane is a saturated hydrocarbon that belongs to the alkane family. The molecule has one carbon atom in the centre and four free electrons bonded with the hydrogen atoms. The chemical formula of methane is ‘CH₄‘. Moreover, each carbon atom undertakes sp³ hybridisation only; since the other two hybridisations are not compatible with giving the free electrons their tetravalency property.

Sp³ Hybridisation in Methane

Hybridisation is the process where two or more orbitals of the same shell merge with each other and form new orbitals of the same energy in the shell. The sp³ hybridisation in methane can be referred to as the process where methane undertakes the process of successful hybridisation.

Carbon’s atom has overall four bonds, one ‘2s’ and three ‘2p’, which end up giving methane 75% ‘p’ characteristics. This result is obtained in only sp³ hybridisation. Moreover, these bonds are not completed in the initial stage. Furthermore, after the carbon molecule gets hybridised, it also bonds with the other four hydrogen molecules. Carbon’s ‘s’ orbitals merge with hydrogen’s ‘p’ orbitals at each bond, resulting in the formation of methane molecules.

Why does methane undertake hybridisation?

This occurs as a result of an imbalance in the activity levels of electrons of the carbon atom of methane. The s and p orbitals are combined to create hybrid orbitals to balance these energy levels. This also allows it to maintain electrons and remain appropriately stable in its orbitals. It places the carbon atom’s molecule in a hybrid posture and allows it to integrate, much like allowing two orbitals to share the same physical space.

How is methane hybridised?

Since the alternative two types of hybridisation, sp, and sp², do not allow carbon to generate four sigma bonds, it only produces sp³ hybridisation as in the development of CH₄.

Moreover, the hybridisation in methane also leaves no unhybridised orbitals. Also, hybridisation is the key factor on which the shape of methane molecules depends.

What is the shape of Sp3 Hybridisation in methane?

Likewise to any other sp³ hybridised molecules, methane also forms the tetrahedral shape. In this shape, each hybrid orbital of a carbon atom is placed at 109.5 degrees from the carbon axis. They repel each other, though they adjust themselves and settle at different corners (four) of a tetrahedron. This also reduces the strain among orbitals. Moreover, all sides of the tetrahedron would seem like equilateral triangles. Lastly, the shape does not get altered regardless of the carbon-hydrogen bond forming. Due to its shape, methane’s hybridisation can also be referred to as ‘Tetrahedral hybridisation’.

Conclusion

We learned different aspects of sp³ Hybridisation in methane from all the above. We concluded that the carbon molecule of methane undertakes sp³ hybridisation likewise any other carbon atom. In which three ‘2p’ orbitals overlap with one ‘2s’ orbital. As a result, four new orbitals form, which have the same energy. This hybridisation helps carbon to get four free electrons that bond with hydrogen and form methane. Due to repulsion between orbitals, they settle as far away as possible (at corners), resulting in the tetrahedral molecule shape. 

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