Question

give in brief o2 is paramagnetic and N2 is diamagnetic​

Answer 1

O2 is paramagnetic because it has two unpaired electrons.

Explanation:

The Lewis structure of

O

2

gives a misleading impression.

It shows that all the electrons in oxygen are paired, so oxygen should be diamagnetic.

Yet oxygen is paramagnetic.

The correct explanation comes from Molecular Orbital theory.

The atomic orbitals of the

O

atoms overlap to form the σ and π orbitals of the

O

2

molecule as shown in the diagram above.

We add the 12 valence electrons according to the Aufbau principle.

The last two electrons go into separate, degenerate π orbitals, according to Hund's Rule.

Thus, oxygen has two unpaired electrons and is paramagnetic.

In N2 molecule, all electrons are paired. That means half of the electrons spin clockwise and half of the electrons spin anticlockwise. Because of their opposite spins they produce magnetic field in opposite direction thus the resultant magnetism becomes zero. When such molecules are placed in an external magnetic field they produce induced magnetic field in opposite direction and that's why they repel the magnetic field. This type of magnetism is called diamagnetism.

Answer 2

O₂ is paramagnetic because there are more unpaired electrons and N₂ is diamagnetic​ because no unpaired electrons.

Explanation :

As there are 6 electrons present in oxygen.

The number of electrons present in $O_2$ molecule = 2(8) = 16

The molecular orbital configuration of $O_2$ molecule will be,

$(\sigma_{1s})^2,(\sigma_{1s}^*)^2,(\sigma_{2s})^2,(\sigma_{2s}^*)^2,(\sigma_{2p_z})^2,[(\pi_{2p_x})^2=(\pi_{2p_y})^2],[(\pi_{2p_x}^*)^1=(\pi_{2p_y}^*)^1],(\sigma_{2p_z}^*)^0$

The number of unpaired electron in molecule are, 2. So, this is paramagnetic. That means, more the number of unpaired electrons, more paramagnetic.

As there are 6 electrons present in oxygen.

The number of electrons present in $N_2$ molecule = 2(7) = 14

The molecular orbital configuration of $N_2$ molecule will be,

$(\sigma_{1s})^2,(\sigma_{1s}^*)^2,(\sigma_{2s})^2,(\sigma_{2s}^*)^2,(\sigma_{2p_z})^2,[(\pi_{2p_x})^2=(\pi_{2p_y})^2],[(\pi_{2p_x}^*)^0=(\pi_{2p_y}^*)^0],(\sigma_{2p_z}^*)^0$

The number of unpaired electron in $N_2$ molecule are, 0. So, this is diamagnetic. That means, more the number of unpaired electrons, more paramagnetic.

Learn more about : molecular orbital configuration

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