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Chapter 10: Problem 37

Predict which substance in each of the following pairs would have the greater intermolecular forces. a. \(\mathrm{CO}_{2}\) or \(\mathrm{OCS}\) b. \(\mathrm{SeO}_{2}\) or \(\mathrm{SO}_{2}\) c. \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{NH}_{2}\) or \(\mathrm{H}_{2} \mathrm{NCH}_{2} \mathrm{CH}_{2} \mathrm{NH}_{2}\) d. \(\mathrm{CH}_{3} \mathrm{CH}_{3}\) or \(\mathrm{H}_{2} \mathrm{CO}\) e. \(\mathrm{CH}_{3} \mathrm{OH}\) or \(\mathrm{H}_{2} \mathrm{CO}\)

Short Answer

Expert verified
a. OCS b. SeO₂ c. H₂NCH₂CH₂NH₂ d. H₂CO e. CH₃OH

Step by step solution

01

a. CO₂ or OCS

First we have to identify the molecular structure and polarity of each molecule: CO₂: linear, non-polar molecule OCS: linear, polar molecule Since OCS is polar, it will have stronger dipole-dipole forces compared to CO₂, which only has weak London dispersion forces. Therefore, OCS has greater intermolecular forces.
02

b. SeO₂ or SO₂

Both molecules have bent structures and are polar molecules which have dipole-dipole forces. The difference is the size and polarizability of the central atom: Se: larger and more polarizable than S SeO₂ will have stronger London dispersion forces due to its larger size and polarizability. Since both have dipole-dipole forces, but SeO₂ also has stronger London dispersion forces, SeO₂ has greater intermolecular forces.
03

c. CH₃CH₂CH₂NH₂ or H₂NCH₂CH₂NH₂

Both of these molecules can form hydrogen bonds because they have N-H bonds. Hydrogen bonding is stronger than dipole-dipole and London dispersion forces. So, we need to analyze the strength of the hydrogen bonds: CH₃CH₂CH₂NH₂: has one NH₂ group for hydrogen bonding H₂NCH₂CH₂NH₂: has two NH₂ groups for hydrogen bonding H₂NCH₂CH₂NH₂ can form more hydrogen bonds, thus it has greater intermolecular forces.
04

d. CH₃CH₃ or H₂CO

We need to classify the types of intermolecular forces for each molecule: CH₃CH₃: non-polar molecule, London dispersion forces H₂CO: polar molecule, dipole-dipole forces H₂CO has stronger dipole-dipole forces compared to CH₃CH₃, which only has weak London dispersion forces. Therefore, H₂CO has greater intermolecular forces.
05

e. CH₃OH or H₂CO

We need to analyze the types of intermolecular forces for each molecule: CH₃OH: has an OH group, hydrogen bonding forces H₂CO: polar molecule, dipole-dipole forces CH₃OH has stronger hydrogen bonding forces, which are stronger than the dipole-dipole forces in H₂CO. Consequently, CH₃OH has greater intermolecular forces.

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Most popular questions from this chapter

Cake mixes and other packaged foods that require cooking often contain special directions for use at high elevations. Typically these directions indicate that the food should be cooked longer above \(5000 \mathrm{ft}\). Explain why it takes longer to cook something at higher elevations.

Consider a sealed container half-filled with water. Which statement best describes what occurs in the container? a. Water evaporates until the air is saturated with water vapor; at this point, no more water evaporates. b. Water evaporates until the air is overly saturated (supersaturated) with water, and most of this water recondenses; this cycle continues until a certain amount of water vapor is present, and then the cycle ceases. c. Water does not evaporate because the container is sealed. d. Water evaporates, and then water evaporates and recondenses simultaneously and continuously. e. Water evaporates until it is eventually all in vapor form. Explain each choice. Justify your choice, and for choices you did not pick, explain what is wrong with them.

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