Multiple Choice
Which of the following best describes polar attractions in the context of intermolecular forces?
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13. Liquids, Solids & Intermolecular Forces
Intermolecular Forces
Multiple Choice
Which of the following best explains why I_2 is a solid at room temperature?
A
I_2 molecules experience strong London dispersion forces due to their large number of electrons.
B
I_2 molecules are held together by ionic bonds.
C
I_2 molecules form hydrogen bonds with each other.
D
I_2 molecules have strong dipole-dipole interactions because they are highly polar.
Verified step by step guidance1
Step 1: Understand the nature of the I_2 molecule. Iodine (I_2) is a diatomic molecule composed of two identical iodine atoms bonded covalently, making it a nonpolar molecule overall.
Step 2: Recall the types of intermolecular forces. The main intermolecular forces include London dispersion forces, dipole-dipole interactions, and hydrogen bonding. Since I_2 is nonpolar, dipole-dipole and hydrogen bonding are unlikely.
Step 3: Consider London dispersion forces. These forces arise from temporary fluctuations in electron distribution, creating instantaneous dipoles that induce attraction between molecules. Larger molecules with more electrons have stronger London dispersion forces.
Step 4: Apply this to I_2. Because iodine atoms are large and have many electrons, the London dispersion forces between I_2 molecules are relatively strong compared to smaller nonpolar molecules.
Step 5: Conclude why I_2 is solid at room temperature. The strong London dispersion forces between I_2 molecules provide enough attraction to hold the molecules in a solid state at room temperature, unlike weaker forces in smaller molecules.
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