Ncert Exercises & Solutions

Examine the types of overlaps given below:

A.	In figure (I), the net overlap is zero.
B.	In figure (II), no overlap occurs due to different symmetry.
C.	In figure (I), the bond formation does not occur.
D.	In figure (II), bond formation occurs.

Select all the correct statements:

1.	A and B only	2.	A, B and C
3.	B and D only	4.	A and C only

Hint: Atomic orbitals must overlap in the same phase and symmetry.

Explanation:

A. In figure (I), the net overlap is zero. (Correct). The constructive overlap (+lobe with +lobe) is cancelled out by the destructive overlap (-lobe with +lobe).

B. In figure (II), no overlap occurs due to different symmetry. (Correct). The \(P_x \) and \(P_y\) orbitals are orthogonal (perpendicular), and the symmetry mismatch results in a net zero overlap.

C. In figure (I), the bond formation does not occur. (Correct). Since the net overlap is zero, no molecular orbital can be formed, and thus no bond forms.

D. In figure (II), bond formation occurs. (Incorrect). Bond formation does not occur because the net overlap is zero (no overlap due to symmetry)

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