Hybridization of CH5
Hybridization is a concept in chemistry that describes the mixing of atomic orbitals to form new hybrid orbitals. In the case of CH5, the central carbon atom is bonded to five hydrogen atoms. Let's explore the hybridization of CH5 in detail:

Hybridization Scheme:
- In CH5, the carbon atom is sp3 hybridized.
- The carbon atom has 4 valence electrons, which are distributed in the 2s and 2p orbitals.
- The hybridization of the carbon atom involves the promotion of one of the 2s electrons to the 2p orbital, resulting in four sp3 hybrid orbitals.
- These sp3 hybrid orbitals then overlap with the 1s orbitals of the five hydrogen atoms to form a total of five sigma bonds.

Geometry and Shape:
- The hybridization of CH5 results in a tetrahedral geometry around the carbon atom.
- The bond angles in CH5 are approximately 109.5 degrees, as expected for a tetrahedral arrangement.

Electron Configuration:
- Each of the five sigma bonds in CH5 is formed by the overlap of a sp3 hybrid orbital from carbon with a 1s orbital from hydrogen.
- The electron configuration of CH5 can be represented as [H-C-H-H-H].
In conclusion, the hybridization of CH5 involves the formation of sp3 hybrid orbitals on the central carbon atom, allowing for the formation of five sigma bonds with the hydrogen atoms. This results in a tetrahedral geometry for the molecule with bond angles of approximately 109.5 degrees.