[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

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.

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.

$sp^3$

$dsp^2$

$d^2sp^3$

$sp^3d^2$

sp3, 109.5°

sp3d, slightly less than 90°

sp3d2, 90°

dsp3, 120°

$sp^3$ hybridization, resulting in bond angles of $109.5^\circ$.

$sp^3d$ hybridization, resulting in bond angles of $90^\circ$ and $120^\circ$.

$sp^3d^2$ hybridization, resulting in bond angles of $90^\circ$.

$dsp^3$ hybridization, resulting in bond angles of $120^\circ$.

$sp^3$

$dsp^2$

$d^2sp^3$

$sp^3d^2$

$N{H_3}$

$NH_4^ +$

$PC{l_5}$

$SC{l_2}$

$sp^3$ hybridization with bond angles of $109.5^\circ$.

$sp^3d$ hybridization with bond angles of exactly $90^\circ$ and $120^\circ$.

$sp^3d^2$ hybridization with bond angles of $90^\circ$.

$sp^3d$ hybridization with bond angles of approximately $102^\circ$ and $173^\circ$ due to lone pair repulsion.

sp3, ns2np2

sp3d, ns2np3

sp3d2, ns2np4

dsp3, ns2np3nd1