In outer most shell of silicon 4 electrons are present and all formed bond with CH3 hence bond pair is 4 and lone pair is zero, basically hybridisation is sp3 and structure is tetrahedral.

Tetrahedral, sp3

Explanation:
The structure and hybridization of Si(CH) can be determined by following the rules of VSEPR theory and the concept of hybridization.

1. VSEPR Theory: According to VSEPR (Valence Shell Electron Pair Repulsion) theory, the electron pairs (both bonding and non-bonding) around the central atom repel each other and try to get as far away from each other as possible. This leads to the formation of specific molecular geometries.

2. Hybridization: Hybridization is the concept of combining atomic orbitals to form hybrid orbitals that are suitable for bonding. It helps to explain the molecular geometries and the types of bonds formed in a molecule.

Now, let's analyze the given molecule:

1. Silicon (Si): Silicon is the central atom in this molecule.

2. Carbon (C): Carbon is bonded to silicon and has one hydrogen atom attached to it.

Based on the VSEPR theory and the number of electron pairs around the central atom, we can determine the molecular geometry and hybridization of Si(CH).

- The central silicon atom has four regions of electron density (two sigma bonds with carbon and two lone pairs of electrons).
- According to VSEPR theory, a molecule with four regions of electron density adopts a tetrahedral geometry.
- To accommodate the tetrahedral geometry, the central silicon atom undergoes sp3 hybridization, where one 3s orbital and three 3p orbitals hybridize to form four sp3 hybrid orbitals.
- The sp3 hybrid orbitals are arranged in a tetrahedral arrangement around the silicon atom, with the carbon and hydrogen atoms occupying the corners of the tetrahedron.

Therefore, the correct answer is option D: Tetrahedral, sp3.