Multiple Choice
Arrange the following molecules in order of decreasing dipole moment.
H–I H–F H–Br H–Cl
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10. Chemical Bonding
Dipole Moment (Simplified)
2:47 minutesProblem 69
Textbook Question
For each of the following bonds, indicate the positive end with 𝛿⁺ and the negative end with 𝛿⁻ . Draw an arrow to show the dipole for each.a. N and F
Verified step by step guidance1
Identify the electronegativity values of nitrogen (N) and fluorine (F) from the periodic table.
Compare the electronegativity values: the atom with the higher electronegativity will attract the shared electrons more strongly.
Determine the direction of the dipole: the arrow points towards the more electronegative atom, which is fluorine (F) in this case.
Label the nitrogen (N) atom with 𝛿⁺ (partial positive charge) because it is less electronegative.
Label the fluorine (F) atom with 𝛿⁻ (partial negative charge) because it is more electronegative.
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Video duration:
2mKey Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Electronegativity
Electronegativity is a measure of an atom's ability to attract and hold onto electrons in a chemical bond. In the context of the bond between nitrogen (N) and fluorine (F), fluorine is more electronegative than nitrogen, meaning it pulls the shared electrons closer to itself, creating a dipole moment.
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Dipole Moment
A dipole moment occurs in a polar bond where there is an uneven distribution of electron density. It is represented by an arrow pointing from the positive end (𝛿⁺) to the negative end (𝛿⁻) of the bond. In the N-F bond, the dipole moment indicates that fluorine has a partial negative charge due to its higher electronegativity.
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Polar vs. Nonpolar Bonds
Bonds can be classified as polar or nonpolar based on the difference in electronegativity between the two atoms involved. A polar bond, like that between N and F, has a significant difference in electronegativity, resulting in a dipole moment. In contrast, nonpolar bonds occur when atoms share electrons equally, leading to no dipole moment.
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