Question

Choose the paramagnetic species from below. Ca O2⁻ Cd2⁺ Zn Nb3⁺

Answer 1

When; all electrons are paired in the compound are element then that is diamagnetic, while Para magnetism requires unpaired electrons.

Ca:

The electronic configuration of Ca is as follows:

Ca: 20

1s²2s²2p⁶3s²3p⁶4s².

There is no unpaired electron thus it is diamagnetic.

O ^2-

The electronic configuration of O is as follows:

O : 8

1s²2s²2p⁴

And O^2- :10

1s²2s²2p⁶

There is no unpaired electron thus it is diamagnetic.

The electronic configuration of Cd is as follows:

Cd:48

1s²2s²2p⁶3s²3p⁶3d¹⁰4s²4p⁶4d¹⁰5s².

Cd2+

the electron configuration of Cd2+ is

1s²2s²2p⁶3s²3p⁶3d¹⁰4s²4p⁶4d¹⁰5s⁰.

There is no unpaired electron thus it is diamagnetic.

Zn:

The electronic configuration of Zn is as follows:

Zn : 30

1s²2s²2p⁶3s²3p⁶3d¹⁰4s²

There is no unpaired electron thus it is diamagnetic.

Nb:41

1s²2s²2p⁶3s²3p⁶3d¹⁰4s²4p⁶4d⁴5s¹.

Nb3+

the electron configuration of Nb3 + is

1s²2s²2p⁶3s²3p⁶3d¹⁰4s²4p⁶4d²5s⁰ .

There is two unpaired electron thus it is Para magnetic.