what is the hybridisation of carbon in CH4 ? give its shape and bond angle
Answers
Answer:
Hybridization of CH4 (Methane)
Name of the Molecule Methane
Molecular Formula CH4
Hybridization Type sp3
Bond Angle 109.5o
Geometry Tetrahedral
Explanation:
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
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.