NEET Chemistry Chemical Bonding and Molecular Structure Valence Bond Theory MCQs

[Ni(CN)4]2- is square planar and diamagnetic

[NiCl4]2- is tetrahedral and paramagnetic

[Ni(CN)4]2- is dsp2 hybridized

[Ni(CN)4]2- is paramagnetic

sp3, ns2np2

sp3d, ns2np3

sp3d2, ns2np4

dsp3, ns2np3nd1

Benzene (C6H6)

Carbon dioxide (CO2)

Sulfur dioxide (SO2)

Sulfur trioxide (SO3)

H2O is a strong field ligand, resulting in d2sp3 hybridization with no unpaired electrons.

H2O is a weak field ligand, resulting in sp3d2 hybridization with four unpaired electrons in the 3d orbitals of Fe2+.

H2O is a strong field ligand, resulting in sp3d2 hybridization with two unpaired electrons in the 3d orbitals of Fe2+.

H2O is a weak field ligand, resulting in dsp2 hybridization with two unpaired electrons in the 3d orbitals of Fe2+.

sp3, 109.5°

sp3d, slightly less than 90°

sp3d2, 90°

dsp3, 120°

Xe undergoes sp3 hybridization, with the two lone pairs occupying opposite corners of a tetrahedron.

Xe undergoes sp3d hybridization, with the two lone pairs occupying equatorial positions.

Xe undergoes sp3d2 hybridization, with the two lone pairs occupying axial positions to minimize repulsion, leading to a square planar arrangement of the four Xe-F bonds.

Xe undergoes dsp2 hybridization, similar to transition metal complexes.

It explains the formation of covalent bonds in terms of overlapping atomic orbitals.

It accurately predicts the magnetic properties of all complexes.

The strength of a bond is proportional to the extent of overlap of the atomic orbitals.

It introduces the concept of hybridization to explain the geometry of molecules.

$sp^3$

$sp^3d$

$sp^3d^2$

$sp^2$

Axial overlapping

Lateral overlapping

Linear overlapping

None of the above

0

1

2

3