NEETChemistryChemical Bonding and Molecular Structure
Given below are two statements: one is labelled as Assertion (A) and the other is labelled as Reason (R). Assertion (A): The molecule of CO ₂ has a higher dipole moment than SO ₂ . Reason (R): CO ₂ has a linear symmetrical structure, while SO ₂ has a bent structure due to the presence of a lone pair of electrons on the sulphur atom. In the light of the above statements, choose the most appropriate answer from the opt
Options
- ABoth (A) and (R) are correct and (R) is the correct explanation of (A)
- BBoth (A) and (R) are correct but (R) is not the correct explanation of (A)
- C(A) is correct but (R) is not correct
- D(A) is not correct but (R) is correct
Correct answer
D. (A) is not correct but (R) is correct
Step-by-step solution
In CO ₂ , the central carbon atom is sp hybridized and has no lone pairs, resulting in a linear symmetrical geometry. The two C = O bond dipoles are equal and opposite, cancelling each other out exactly. Thus, the net dipole moment of CO ₂ is zero. In SO ₂ , the central sulphur atom is sp^2 hybridized and possesses one lone pair of electrons. This gives the molecule a bent (V-shaped) structure. The S = O bond dipoles do not cancel each other, resulting in a non-zero net dipole moment. Therefore, SO ₂ has a higher d