Which of the following species are paramagnetic in nature?

Question

Q. Which of the followoing species are paramagnetic in nature?

Answer 1

The molecular orbital configuration of F

₂ (18 electrons) is:

Answer 2

(σ 1 s)

²

(σ* 1 s)

²

(σ 2 s)

²

(σ* 2 s)

²

(σ 2 pz)

²

(π 2 px)

²

(π 2 py)

²

(π* 2 px)

²

(π* 2 p_{y})

².

Answer 3

Since, there is no unpaired electron, F₂ is diamagnetic in nature.

Answer 4

The molecular orbital configuration of B

₂ (10 electrons) is:

Answer 5

(σ 1 s)

²

(σ* 1 s)

²

(σ 2 s)

²

(σ* 2 s)

²

(π 2 px)¹ (π 2 py)¹

Answer 6

There are two unpaired electrons, so B₂ is paramagnetic.

Answer 7

The molecular orbital configuration of NO (13 electrons) is:

Answer 8

(σ 1 s)

²

(σ* 1 s)

²

(σ 2 s)

²

(σ* 2 s)

²

(π 2 px)

²

(π 2 py)

² (σ2pz)¹

Answer 9

There is one unpaired electron, so NO is paramagnetic.

Answer 10

The molecular orbital configuration of OF (17 electrons) is:

Answer 11

(σ 1 s)

²

(σ* 1 s)

²

(σ 2 s)

²

(σ* 2 s)

²

(σ 2 pz)

²

(π 2 px)

²

(π 2 p_{zy})

²

(π* 2 px)

²

(π* 2 py)

¹.

Answer 12

There is one unpaired electron, so OF is paramagnetic.

Which of the following species are paramagnetic in nature?

The molecular orbital configuration of F₂ (18 electrons) is:

(σ1s)² (σ*1s)² (σ2s)² (σ*2s)² (σ2pz)² (π2px​)² (π2py​)² (π*2px​)² (π*2py)².

Since, there is no unpaired electron, F₂ is diamagnetic in nature.

The molecular orbital configuration of B₂ (10 electrons) is:

(σ1s)² (σ*1s)² (σ2s)² (σ*2s)² (π2px​)¹ (π2py​)¹

There are two unpaired electrons, so B₂ is paramagnetic.

The molecular orbital configuration of NO (13 electrons) is:

(σ1s)² (σ*1s)² (σ2s)² (σ*2s)² (π2px​)² (π2py​)² (σ2pz)¹

There is one unpaired electron, so NO is paramagnetic.

The molecular orbital configuration of OF (17 electrons) is:

(σ1s)² (σ*1s)² (σ2s)² (σ*2s)² (σ2pz)² (π2px​)² (π2pzy)² (π*2px​)² (π*2py​)¹.

There is one unpaired electron, so OF is paramagnetic.

$The molecular orbital configuration of F$ ₂ (18 electrons) is:

$(σ 1 s)$ ² $(σ* 1 s)$ ² $(σ 2 s)$ ² $(σ* 2 s)$ ² $(σ 2 pz)$ ² $(π 2 px)$ ² $(π 2 py)$ ² $(π* 2 px)$ ² $(π* 2 p_{y})$ ².

$The molecular orbital configuration of B$ ₂ (10 electrons) is:

$(σ 1 s)$ ² $(σ* 1 s)$ ² $(σ 2 s)$ ² $(σ* 2 s)$ ² $(π 2 px)¹ (π 2 py)¹$

$The molecular orbital configuration of NO (13 electrons) is:$

$(σ 1 s)$ ² $(σ* 1 s)$ ² $(σ 2 s)$ ² $(σ* 2 s)$ ² $(π 2 px)$ ² $(π 2 py)$ ² (σ2pz)¹

$The molecular orbital configuration of OF (17 electrons) is:$

$(σ 1 s)$ ² $(σ* 1 s)$ ² $(σ 2 s)$ ² $(σ* 2 s)$ ² $(σ 2 pz)$ ² $(π 2 px)$ ² $(π 2 p_{zy})$ ² $(π* 2 px)$ ² $(π* 2 py)$ ¹.