Find the set of compound in which one compound has zero dipole moment and other has non-zero dipole moment?
Source: https://www.lazynewton.com/questions/chemistry/chemical-bonding-and-molecular-structure/find-set-compound-compound-dipole-moment-nonzero-dipole-moment-062107
Quick Answer
Option D
BF3, SO2
— To determine if a molecule has a zero or non-zero dipole moment, we need to consider both the polarity of individual…Step-by-step solution
1AnswerD·
To determine if a molecule has a zero or non-zero dipole moment, we need to consider both the polarity of individual bonds and the molecular geometry. If the vector sum of all bond dipoles is zero, the molecule has a zero dipole moment (nonpolar). If the vector sum is non-zero, the molecule has a non-zero dipole moment (polar).
Option Analysis:
- A) CO₂, BF₃
- CO₂: Linear geometry. C=O bonds are polar, but the two bond dipoles are equal in magnitude and opposite in direction, canceling each other out. Dipole moment = 0.
- BF₃: Trigonal planar geometry. B-F bonds are polar, but due to the symmetrical arrangement, the three bond dipoles cancel each other out. Dipole moment = 0.
- Both compounds have zero dipole moment. This option is incorrect.
- B) PF₃, SO₂
- PF₃: Pyramidal geometry (due to one lone pair on P). P-F bonds are polar. The lone pair contributes to the overall dipole moment, and the bond dipoles do not cancel out. Dipole moment ≠ 0.
- SO₂: Bent geometry (due to one lone pair on S). S=O bonds are polar. The lone pair contributes to the overall dipole moment, and the bond dipoles do not cancel out. Dipole moment ≠ 0.
- Both compounds have non-zero dipole moment. This option is incorrect.
- C) BeCl₂, SF₆
- BeCl₂: Linear geometry. Be-Cl bonds are polar, but the two bond dipoles are equal in magnitude and opposite in direction, canceling each other out. Dipole moment = 0.
- SF₆: Octahedral geometry. S-F bonds are polar, but due to the highly symmetrical arrangement, the six bond dipoles cancel each other out. Dipole moment = 0.
- Both compounds have zero dipole moment. This option is incorrect.
- D) BF₃, SO₂
- BF₃: Trigonal planar geometry. B-F bonds are polar, but due to the symmetrical arrangement, the three bond dipoles cancel each other out. Dipole moment = 0.
- SO₂: Bent geometry (due to one lone pair on S). S=O bonds are polar. The lone pair contributes to the overall dipole moment, and the bond dipoles do not cancel out. Dipole moment ≠ 0.
- One compound (BF₃) has zero dipole moment, and the other (SO₂) has a non-zero dipole moment. This option is correct.
Correct Answer: (D)
BF3, SO2