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Hybridization of CH4 (Methane)

In order to understand the hybridization of CH4 (methane), we have to take a look at the atomic orbitals which are of different shape and energy that take part in the process. The type of hybridization involved with CH4 is sp3. We will discuss in detail how this hybridization occurs below.

Name of the Molecule Methane
Molecular Formula CH4
Hybridization Type sp3
Bond Angle 109.5o
Geometry Tetrahedral

What is the Hybridization of Methane?

When we talk about CH4 it is basically a combination of 1 carbon and 4 hydrogen atoms. However, to form this compound the central atom carbon which has 4 valence electrons obtain more electrons from 4 hydrogen atoms to complete its octet. When the electrons are shared between carbon and hydrogen there is a formation of a covalent bond or bonds to be more accurate.

Hybridization Of CH4

Now coming to the hybridization of methane, the central atom carbon is sp3 hybridized. This is because one 2s orbital and three 2p orbitals in the valence shell of carbon combine to form four sp3 hybrid orbitals which are of equal energy and shape. Further, four H atoms also use these four sp3 hybrid orbitals of carbon to form C-H sigma bonds which ultimately leads to the formation of the methane molecule.

Important Points To Remember

  • Each sp3 hybrid orbital of carbon overlaps 1s-orbital of hydrogen to C-H sigma bonds.
  • The hybridization involves the mixing of 1 s orbital and 3 p orbitals and there are no lone pairs.
  • The sp3 hybrid orbitals are of equal energy and shape. They contain one unpaired electron each.

CH4 Molecular Geometry And Bond Angles

We have already discussed the bond formation and hybridization process above. Determining CH4 molecular geometry should be easier. In methane, the four hybrid orbitals are located in such a manner so as to decrease the force of repulsion between them. Nonetheless, the four orbitals do repel each other and get placed at the corners of a tetrahedron. CH4 has a tetrahedral shape. The sp3 hybrid orbitals have a bond angle of 109.5o.

Read More About Hybridization of Other Chemical Compounds

Chemical Bonding

Frequently Asked Questions – FAQs

Q1

What is the hybridization and geometry of CH4?

Methane molecule is sp3 hybridized and has a perfect tetrahedral geometry.
Q2

What is the bond angle of methane molecules?

The bond angle of ammonia is 109.5Β°.
Q3

Explain the hybridization of a methane molecule.

The hybridization of methane molecules occurs by mixing one orbital with three p orbitals. Each orbital consists of one unpaired electron. The s and three p orbitals of carbon overlap with the 1s orbitals of hydrogen to form bonds. Thus methane is sp3 hybridized.
Q4

What is meant by perfect geometry?

The molecule is said to have a perfect geometry if the central atom has no lone pairs and all the side atoms are the same.
Q5

Does methane have a perfect geometry?

Yes, methane has a perfect geometry.
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