Hybridization and shape of N(SiH3)3:

Hybridization is the process of combining atomic orbitals to form hybrid orbitals that have different properties from the original atomic orbitals. The shape of a molecule is determined by the arrangement of its atoms and the hybridization of its orbitals.

The molecule N(SiH3)3 contains one nitrogen atom and three silicon atoms bonded to it. The nitrogen atom has one unpaired electron in its 2p orbital, which can be used to form three sigma bonds with the silicon atoms. The hybridization of the nitrogen atom is therefore determined by the number of sigma bonds it forms.

Option B is the correct answer because the hybridization of the nitrogen atom in N(SiH3)3 is sp2, and the shape of the molecule is planar.

Explanation:

1. Hybridization of the Nitrogen atom:

The nitrogen atom in N(SiH3)3 forms three sigma bonds with the silicon atoms, which requires three orbitals. Therefore, the nitrogen atom undergoes sp2 hybridization, in which one 2s orbital and two 2p orbitals combine to form three sp2 hybrid orbitals.

2. Shape of the Molecule:

The shape of the molecule is determined by the arrangement of its atoms and the hybridization of its orbitals. In N(SiH3)3, the three sp2 hybrid orbitals on the nitrogen atom are arranged in a trigonal planar geometry, with bond angles of 120 degrees. The three Si-H bonds are also arranged in a trigonal planar geometry around each silicon atom. Therefore, the shape of the molecule is planar.

Conclusion:

In summary, the correct answer for the hybridization and shape of N(SiH3)3 is sp2 and planar, respectively. The nitrogen atom undergoes sp2 hybridization to form three sp2 hybrid orbitals, which are arranged in a trigonal planar geometry around the nitrogen atom. The three silicon atoms are also arranged in a trigonal planar geometry around the nitrogen atom, resulting in a planar shape for the molecule.