Dipole Moments in Molecules
Explore the concept of dipole moments, polarity, and their effects on molecular properties through various question types.
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Dipole Moments in Molecules
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Read each question carefully and answer to the best of your ability. Show all your work for calculations.
1. Which of the following best describes a dipole moment?
The net result of all bond dipoles in a molecule.
The amount of energy required to break a bond.
The measure of an atom's ability to attract electrons.
The total number of valence electrons in a molecule.
2. A molecule is considered polar if it has a net dipole moment. Which of the following molecules is likely to be polar?
CO2 (linear)
CH4 (tetrahedral)
H2O (bent)
Cl2 (linear)
1. A nonpolar molecule can have polar bonds.
True
False
2. The larger the difference in electronegativity between two atoms, the smaller the bond dipole moment.
True
False
1. A molecule with a symmetrical geometry and identical peripheral atoms will typically have a net dipole moment of .
2. The unit for dipole moment is the .
1. Explain how molecular geometry can influence whether a molecule is polar, even if it contains polar bonds.
2. Describe one physical property of a substance that is affected by the presence of dipole moments in its molecules.
Match each term on the left with its definition or characteristic on the right.
1. Electronegativity
a. The separation of charge within a bond
2. Nonpolar molecule
b. A molecule with no net dipole moment
3. Bond dipole
c. The ability of an atom to attract electrons in a bond