Textbook Question
Consider the following bonds: Ca and O, C and O, K and O, Oand O, and N and O. (6.7)d. Arrange the covalent bonds in order of decreasing polarity.
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10. Chemical Bonding
Dipole Moment (Simplified)
Multiple Choice
Arrange the following molecules in order of decreasing dipole moment.
H–I H–F H–Br H–Cl
A
H–Cl >H–I > H–Br > H–F
B
H–Br >H–Cl > H–F > H–I
C
H–F >H–Cl > H–Br > H–I
D
H–I >H–Cl > H–Br > H–F
Verified step by step guidance1
Understand that the dipole moment of a molecule is determined by the difference in electronegativity between the atoms and the distance between them. The greater the difference in electronegativity, the larger the dipole moment.
Identify the electronegativities of the halogens involved: Fluorine (F) has the highest electronegativity, followed by Chlorine (Cl), Bromine (Br), and Iodine (I).
Recognize that the dipole moment is also influenced by the bond length. Generally, as the bond length increases, the dipole moment decreases if the electronegativity difference is the same.
Compare the molecules: H–F has the highest dipole moment due to the highest electronegativity difference, followed by H–Cl, H–Br, and H–I, considering both electronegativity and bond length.
Arrange the molecules in order of decreasing dipole moment: H–F > H–Cl > H–Br > H–I.
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