Question

Assuming that s-p mixing is not allowed, the bond order and magnetic nature of diatomic molecule B2 is​

Answer 1

Answer:

A

1 and diamagnetic

In Hund's rule of maximum multiplicity, if two or more orbitals of equal energy are available, electrons will occupy them singly before filling them in pairs.

B

2

(10)=σ

1s

2

σ

1s

2

∗

σ

2s

2

σ

2s

2

∗

π

2p

x

2

Number of bonding electrons = 6

Number of Antibonding electrons = 4

Bond order =

2

(Number of bonding electrons−Number of antibonding electrons)

Bond order =

2

6−4

=1

Since there are no unpaired electrons, it is diamagnetic in nature.

Explanation:

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Answer 2

the bond order for B2 molecule is 1. Note: In the molecular orbital diagram, we can see that there are unpaired electrons in the B2 molecule. Thus, the B2 molecule is paramagnetic in nature. If there are no unpaired electrons then the molecules are diamagnetic in nature