Question

According to molecular orbital theory stability of the species b2+, b2-, b2is of the order :

Answer 1

Explanation:

Place the species B2+ , B2, and B2− in order of increasing bond length and increasing bond energy. Concept introduction: The electronic configuration for multi-electron diatomic is written using the molecular orbitals, derived from the H+2 molecular ion. As the bond order increases, the stability also increase

Answer 2

Concept:

The stability of the species is directly proportional to the bond order. As the bond order increases, the stability of the species also increases.

Given:

B₂⁺, B₂, B₂⁻

Find:

According to molecular orbital theory stability of the species B₂⁺, B₂, B₂⁻ is of the order?

Solution:

According to molecular orbital theory,  the bond order can be calculated as:

Bond order = $\frac{number of electrons in(bonding molecular orbital - antibonding molecular orbital}{2}$

In the MOT diagram of B₂⁺,

• The number of electrons in bonding molecular orbital = 0
• The number of electrons in antibonding molecular orbital = 0
• Bond order =$\frac{0-0}{2}$  = 0

In the MOT diagram of B₂⁻,

• The number of electrons in bonding molecular orbital = 3
• The number of electrons in antibonding molecular orbital = 0
• Bond order = $\frac{3-0}{2}$ = $\frac{3}{2}$ = 1.5

In the MOT diagram of B₂,

• The number of electrons in bonding molecular orbital = 2
• The number of electrons in antibonding molecular orbital = 0
• Bond order = $\frac{2-0}{2}$ = $\frac{2}{2}$ = 1

The increasing order of bond order is B₂⁺ < B₂ < B₂⁻.

Hence, the stability in the increasing order for given species is B₂⁺ < B₂ < B₂⁻.

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