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Chapter 9: 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. \(\operatorname{SeO}_{2}\) or \(\mathrm{SO}_{2}\) \(\mathbf{c .} \cdot \mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{NH}_{2}\) 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
The substances with greater intermolecular forces in each pair are: a. OCS b. SeO2 c. H2NCH2CH2NH2 d. H2CO e. CH3OH

Step by step solution

01

Pair a: CO2 or OCS

The structure of CO2 (carbon dioxide) is linear with a symmetrical distribution of electron density around the carbon atom, making it a nonpolar molecule. The only intermolecular force present in CO2 is London dispersion forces. OCS (carbonyl sulfide) is also linear, but it is polar because of the asymmetrical distribution of electron density around the central atom. In addition to London dispersion forces, OCS has dipole-dipole interactions. Thus, OCS has greater intermolecular forces than CO2.
02

Pair b: SeO2 or SO2

SeO2 (selenium dioxide) and SO2 (sulfur dioxide) are both bent molecules. Both have polar bonds and are polar molecules. However, selenium has a greater atomic size and more electrons than sulfur. This leads to larger London dispersion forces in SeO2 than in SO2. Since both molecules have dipole-dipole interactions and dispersion forces, but SeO2 has greater dispersion forces, SeO2 has greater overall intermolecular forces.
03

Pair c: CH3CH2CH2NH2 or H2NCH2CH2NH2

CH3CH2CH2NH2 (propylamine) has covalent bonds between carbon and hydrogen atoms, and a polar bond between nitrogen and hydrogen. There is no hydrogen bond within the molecule. H2NCH2CH2NH2 (ethylenediamine) also has covalent bonds between carbon and hydrogen atoms, and polar bonds between nitrogen and hydrogen. However, ethylenediamine can form hydrogen bonds with other molecules through its two nitrogen atoms. Therefore, H2NCH2CH2NH2 has greater intermolecular forces due to the presence of hydrogen bonding.
04

Pair d: CH3CH3 or H2CO

CH3CH3 (ethane) is a nonpolar hydrocarbon molecule, which means it only has London dispersion forces as its intermolecular forces. H2CO (formaldehyde) is a polar molecule due to the presence of a polar carbon-oxygen bond and a trigonal planar molecular geometry. Since it is polar, H2CO has both dispersion forces and dipole-dipole interactions. Consequently, H2CO has greater intermolecular forces than CH3CH3.
05

Pair e: CH3OH or H2CO

CH3OH (methanol) is a polar molecule with a polar bond between oxygen and hydrogen atoms. It can form hydrogen bonds with other molecules due to the presence of a hydrogen atom bonded to an oxygen atom. H2CO (formaldehyde), as discussed previously, is a polar molecule with dipole-dipole forces and London dispersion forces. However, it cannot form hydrogen bonds. Hence, CH3OH has greater intermolecular forces than H2CO due to the presence of hydrogen bonding. In summary, the substances with greater intermolecular forces in each pair are: a. OCS b. SeO2 c. H2NCH2CH2NH2 d. H2CO e. CH3OH

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Most popular questions from this chapter

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