Statement-I: The molecules XeF4, SiF4, SeF4 and BF4− all have two different E–F bond lengths, where E is the central atom.
Statement-II: Among O2, O2+, O2− and F2, the species O2 has the highest bond order.
Choose the correct option.

Both statements are correct
Both statements are incorrect
Statement-I correct, Statement-II incorrect
Statement-I incorrect, Statement-II correct

Question

Statement-I: The molecules XeF4, SiF4, SeF4 and BF4&minus; all have two different E&ndash;F bond lengths, where E is the central atom.
Statement-II: Among O2, O2+, O2&minus; and F2, the species O2 has the highest bond order.
Choose the correct option.

Both statements are correct
Both statements are incorrect
Statement-I correct, Statement-II incorrect
Statement-I incorrect, Statement-II correct

Shiksha Nation · Accepted Answer

Solution:
Statement-I:
XeF4 is square planar and all Xe&ndash;F bonds are equal.
SiF4 is tetrahedral and all Si&ndash;F bonds are equal.
BF4&minus; is tetrahedral and all B&ndash;F bonds are equal.
Only SeF4 shows axial and equatorial bond differences.
Therefore Statement-I is incorrect.
Statement-II:



Species
Bond Order


O2
2


O2+
2.5


O2&minus;
1.5


F2
1



Highest bond order is O2+, not O2.
Therefore Statement-II is also incorrect.
Answer:
Option (2)

Verified Answer