Statement I: The number of species among BF₄⁻, SiF₄, XeF₄ and SF₄, that have unequal E − F bond lengths is two. Here, E is the central atom. Statement II: Among O₂, O₂²⁻, F₂ and O₂⁺, O₂ has the highest bond order.

Given below are two statements: The number of species among BF₄⁻, SiF₄, XeF₄ and SF₄, that have unequal E − F bond lengths is two. Here, E is the central atom. Statement II: Among O₂, O₂²⁻, F₂ and O₂⁺, O₂ has the highest bond order.

Q. Given below are two statements:

Statement I: The number of species among BF₄⁻, SiF₄, XeF₄ and SF₄, that have unequal E − F bond lengths is two. Here, E is the central atom.

Statement II: Among O₂, O₂²⁻, F₂ and O₂⁺, O₂ has the highest bond order.

In the light of the above statements, choose the correct answer from the options given below.

(A) Both Statement I and Statement II are false

(B) Statement I is true but Statement II is false

(D) Both Statement I and Statement II are true

Correct Answer: (A)

Explanation

For Statement I, equality or inequality of E − F bond lengths depends on the molecular geometry and symmetry.

BF₄⁻ has a tetrahedral geometry, therefore all B − F bond lengths are equal. SiF₄ is also tetrahedral and all Si − F bonds are identical. XeF₄ has a square planar geometry and due to its symmetric structure, all Xe − F bonds are equal.

SF₄ has a see-saw geometry with two axial and two equatorial S − F bonds, which are unequal.

Hence, only one species shows unequal E − F bond lengths.

Therefore, Statement I is false.

For Statement II, bond order values based on molecular orbital theory are:

O₂ = 2
O₂²⁻ = 1
F₂ = 1
O₂⁺ = 2.5

Since O₂⁺ has the highest bond order, O₂ does not have the maximum bond order.

Thus, Statement II is also false.

Hence, both Statement I and Statement II are false.

Explanation

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