What is a molecular dipole moment?
A. A separation of charge characterizing a nonpolar covalent bond
B. A separation of charge forming a positive and a negative end of a molecule
C. The arrangement of charges around an atom in a nonpolar molecule
D. A net cancellation of charge separation due to symmetry of the molecule
I think it's D
And, you are totally wrong. Try again.
Nonpolar molecules have zero dipole moment.
I disagree also.
The correct answer is B. A molecular dipole moment refers to a separation of charge within a molecule, resulting in a positive end and a negative end. This separation occurs due to differences in electronegativity between the atoms involved in the covalent bond. To determine whether a molecule has a molecular dipole moment, you can follow these steps:
1. Identify the type of bond present in the molecule. Typically, molecular dipole moments are observed in polar covalent bonds, where there is a significant difference in electronegativity between the atoms involved.
2. Determine the polarity of each bond. Look up the electronegativity values of the two atoms forming the bond. If there is a significant difference in electronegativity, then the bond is polar, and there will be a separation of charge.
3. Consider the molecule's geometry. To have a molecular dipole moment, the molecule should have an asymmetrical shape. If the molecule is symmetrical, the dipole moments will cancel each other out, resulting in no net dipole moment.
4. If the molecule has polar bonds and an asymmetrical shape, you can conclude that it has a molecular dipole moment.
In this question, option B states that a molecular dipole moment involves a separation of charge forming a positive and a negative end of a molecule, which accurately describes the concept. On the other hand, option D refers to a net cancellation of charge separation due to symmetry of the molecule, which is incorrect. Therefore, the correct answer is B.