Chemistry MCQs for NEET — Practice Questions with Answers

The correct answer is o1: octahedral. In the solid state, PCl5 exists as an ionic compound with [PCl4]+ cation and [PCl6]- anion. The [PCl6]- anion has an octahedral geometry, with the central P atom surrounded by six Cl atoms arranged at the vertices of an octahedron.

Xenon has 8 valence electrons, out of which 2 are shared with F-atoms leaving behind 3 lone pairs.

Polarizability $\propto$ atomic radii of the gas molecule.

Hence, (1).

                     s bond pair            Lone pair            Hybridisation             Shape

HgCl₂                   2                          0                         sp                     Linear

SnCl₂                   2                          1                         sp₂                   v-shape

F₂O                      2                          2                         sp₃                   v-shape

As the number of lone pair of electrons on central atom increases the bond angle decreases.

${\mathrm{NH}}_4^{+}>{\mathrm{NH}}_3 >{\mathrm{NH}}_2^{-}$

NH2-, NH3, and NH4+ have H-N-H bond angles of 105, 107 and 109 repectively

Smaller is the size of ion, higher is the lattice energy.

For a T-shaped molecule like MX3, the central atom M has 3 bonding pairs and 2 non-bonding pairs of electrons. The presence of 2 non-bonding electron pairs gives the molecule a T-shaped geometry, as the bonding pairs occupy more space and push the non-bonding pairs towards the corners.

In PCl₃, the hybridised state of P is sp³ while in PCl₅, the hybridised state of P is sp³d

NH₃ - 107 ,

NF₃ ,102,

PH₃ - 93,

PF₃- 97

H₂O- 104.5