$sp^3$

$d^2sp^3$

$dsp^2$

$sp^3d^2$

${{\rm{H}}_2}$ molecule

${\rm{C}}{{\rm{l}}_2}$molecule

Hydrogen chloride

Hydrogen bromide molecule

It is diamagnetic and inner orbital complex

It is diamagnetic and outer orbital complex

It is paramagnetic and inner orbital complex

It is paramagnetic and outer orbital complex

Lower paramagnetism, $d^2sp^3$ hybridisation

Diamagnetism, $sp^3d^2$ hybridisation

Higher paramagnetism, $sp^3d^2$ hybridisation

No change in magnetic properties, $d^2sp^3$ hybridisation

${H_2}S{O_3} > {H_2}S{O_4}\, > \,{H_2}{S_2}{O_7}$

${H_2}S{O_4}\, > \,{H_2}{S_2}{O_7} > {H_2}S{O_3}$

$\,\,{H_2}{S_2}{O_7} > {H_2}S{O_4} > {H_2}S{O_3}$

$\,\,{H_2}{S_2}{O_7} > {H_2}S{O_3}.{H_2}S{O_4}$

1 $\sigma$ and 1 $\pi$

1 $\sigma$ and 2 $\pi$

2 $\sigma$ and 1 $\pi$

3 $\sigma$ and 0 $\pi$

2 unpaired electrons, paramagnetic

4 unpaired electrons, paramagnetic

0 unpaired electrons, diamagnetic

5 unpaired electrons, paramagnetic

Due to s - s overlapping

Due to s - p overlapping

Due to p - p overlapping

Due to hybridisation

$CN^-$

$Cl^-$

$F^-$

$NH_3$

[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, 109.5°

sp3d, slightly less than 90°

sp3d2, 90°

dsp3, 120°