Statement (a): 2P3/2 is the ground state term symbol of F
The term symbol is used to describe the electronic state of an atom or molecule. It consists of a combination of letters and numbers that represent the total angular momentum, total spin, and orbital angular momentum of the system. The term symbol is derived from the electron configuration of the atom or molecule.

In the case of fluorine (F), the electron configuration is 1s2 2s2 2p5. The ground state of fluorine has one unpaired electron in the 2p orbital. The total angular momentum (L) for this electron is 1, and the total spin (S) is 1/2. Therefore, the term symbol for the ground state of fluorine is 2P3/2.

Statement (b): PbO is more stable than PbO2
Lead (Pb) can exhibit a +2 or +4 oxidation state. PbO and PbO2 are two common oxides of lead.

PbO has Pb in the +2 oxidation state, while PbO2 has Pb in the +4 oxidation state. Generally, lower oxidation states are more stable than higher oxidation states for most elements. This is because lower oxidation states require less energy to achieve.

In the case of lead, the +2 oxidation state is more stable than the +4 oxidation state. Therefore, PbO is more stable than PbO2.

Statement (c): The power of NH3 to split the metal d-orbitals is higher than H2O
Ammonia (NH3) and water (H2O) are both commonly used as ligands in coordination compounds. Ligands can donate electron pairs to a metal center, forming coordination bonds.

Ammonia has a lone pair of electrons on the nitrogen atom, which can be donated to a metal center. This lone pair can interact with the metal d-orbitals, causing them to split into different energy levels. This splitting is known as ligand field splitting.

Water also has a lone pair of electrons on the oxygen atom, but the electronegativity of oxygen is higher than that of nitrogen. This means that the oxygen atom in water is less willing to donate its lone pair to the metal center compared to the nitrogen atom in ammonia.

Therefore, the power of NH3 to split the metal d-orbitals is higher than H2O.

Statement (d): The central atom of N(SiH3)3 is sp3 hybridized
The central atom in N(SiH3)3 is nitrogen (N). Nitrogen has five valence electrons and can form three sigma bonds with the three SiH3 groups in the molecule.

In order to accommodate these three sigma bonds, as well as the lone pair of electrons on nitrogen, the nitrogen atom undergoes sp3 hybridization. This results in four sp3 hybrid orbitals, three of which are used to form sigma bonds with the SiH3 groups and one of which contains the lone pair of electrons.

Therefore, the central atom of N(SiH3)3 is sp3 hybridized.