Multiple Choice
Which of the following correctly describes the direction of bond polarity in a molecule of HCl?
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11. Bonding & Molecular Structure
Dipole Moment
Multiple Choice
Which of the following statements correctly describes the permanent electric dipole moment of a water (H2O) molecule?
A
It is 1.0 × 10^{-30} C·m, indicating that water is a polar molecule.
B
It is 6.2 × 10^{-30} C·m, indicating that water is a nonpolar molecule.
C
It is 0 C·m, indicating that water is a nonpolar molecule.
D
It is 6.2 × 10^{-30} C·m, indicating that water is a polar molecule.
Verified step by step guidance1
Understand that the permanent electric dipole moment of a molecule arises from the uneven distribution of electron density, which depends on both the molecular geometry and the difference in electronegativity between atoms.
Recall that water (H\_2O) has a bent molecular shape due to the two lone pairs on oxygen, which causes an asymmetrical distribution of charge.
Recognize that the O-H bonds are polar because oxygen is more electronegative than hydrogen, creating partial negative and positive charges respectively.
Combine the bond dipoles vectorially considering the bent shape; this results in a net dipole moment that is not zero, indicating water is a polar molecule.
Note that the experimentally measured dipole moment of water is approximately 6.2 \(\times\) 10^{-30} C\(\cdot\) m, confirming its polarity.
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