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Chapter 10: Problem 35

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
Answer: a. \(\mathrm{OCS}\) b. \(\mathrm{SO}_{2}\) c. \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{NH}_{2}\) d. \(\mathrm{H}_{2} \mathrm{CO}\) e. \(\mathrm{CH}_{3} \mathrm{OH}\)

Step by step solution

01

Identify Intermolecular Forces

In \(\mathrm{CO}_{2}\), the molecule is nonpolar due to the linear molecular geometry, so it only has London dispersion forces. In \(\mathrm{OCS}\), the molecule is polar because of its asymmetric linear molecular geometry, so it has both dipole-dipole forces and London dispersion forces.
02

Compare Intermolecular Forces

Since \(\mathrm{OCS}\) has both dipole-dipole forces and London dispersion forces while \(\mathrm{CO}_{2}\) only has London dispersion forces, \(\mathrm{OCS}\) has stronger intermolecular forces. ###Pair B: \(\mathrm{SeO}_{2}\) and \(\mathrm{SO}_{2}\)###
03

Identify Intermolecular Forces

Both \(\mathrm{SeO}_{2}\) and \(\mathrm{SO}_{2}\) have bent molecular geometries, making them polar molecules. Therefore, they both have dipole-dipole forces and London dispersion forces.
04

Compare Intermolecular Forces

Due to the greater electronegativity of sulfur compared to selenium, the dipole-dipole forces are stronger in \(\mathrm{SO}_{2}\). Therefore, \(\mathrm{SO}_{2}\) has stronger intermolecular forces. ###Pair C: \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{NH}_{2}\) and \(\mathrm{H}_{2} \mathrm{NCH}_{2} \mathrm{CH}_{2} \mathrm{NH}_{2}\)###
05

Identify Intermolecular Forces

Both molecules contain N-H bonds, so they can engage in hydrogen bonding, dipole-dipole forces, and London dispersion forces.
06

Compare Intermolecular Forces

Both molecules have similar hydrogen bonding capabilities, so we must compare their London dispersion forces. \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{NH}_{2}\) has more carbons and hence a larger molecular weight and surface area, leading to stronger London dispersion forces. Therefore, \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{NH}_{2}\) has stronger intermolecular forces. ###Pair D: \(\mathrm{CH}_{3} \mathrm{CH}_{3}\) and \(\mathrm{H}_{2} \mathrm{CO}\)###
07

Identify Intermolecular Forces

\(\mathrm{CH}_{3} \mathrm{CH}_{3}\) (ethane) is a nonpolar molecule, so it only has London dispersion forces. \(\mathrm{H}_{2} \mathrm{CO}\) (formaldehyde) contains a polar C=O bond and has dipole-dipole forces in addition to London dispersion forces.
08

Compare Intermolecular Forces

Since \(\mathrm{H}_{2} \mathrm{CO}\) has dipole-dipole forces in addition to London dispersion forces, it has stronger intermolecular forces compared to \(\mathrm{CH}_{3} \mathrm{CH}_{3}\). ###Pair E: \(\mathrm{CH}_{3} \mathrm{OH}\) and \(\mathrm{H}_{2} \mathrm{CO}\)###
09

Identify Intermolecular Forces

\(\mathrm{CH}_{3} \mathrm{OH}\) (methanol) has an O-H bond and can form hydrogen bonds, giving it hydrogen bonding, dipole-dipole forces, and London dispersion forces. As previously mentioned, \(\mathrm{H}_{2} \mathrm{CO}\) has dipole-dipole forces and London dispersion forces.
10

Compare Intermolecular Forces

Since \(\mathrm{CH}_{3} \mathrm{OH}\) can form hydrogen bonds, which are stronger than dipole-dipole forces, methanol has stronger intermolecular forces compared to \(\mathrm{H}_{2} \mathrm{CO}\).

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Most popular questions from this chapter

What fraction of the total volume of a cubic closest packed structure is occupied by atoms? (Hint: \(V_{\text {sphere }}=\frac{4}{3} \pi r^{3}\).) What fraction of the total volume of a simple cubic structure is occupied by atoms? Compare the answers.

A topaz crystal has an interplanar spacing \((d)\) of \(1.36 \AA^{\circ}(1 \AA=\) \(\left.1 \times 10^{-10} \mathrm{~m}\right) .\) Calculate the wavelength of the \(\mathrm{X}\) ray that should be used if \(\theta=15.0^{\circ}\) (assume \(n=1\) ).

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Iodine, like most substances, exhibits only three phases: solid, liquid, and vapor. The triple point of iodine is at 90 torr and \(115^{\circ} \mathrm{C}\). Which of the following statements concerning liquid \(\mathrm{I}_{2}\) must be true? Explain your answer. a. \(\mathrm{I}_{2}(l)\) is more dense than \(\mathrm{I}_{2}(g)\). b. \(\mathrm{I}_{2}(l)\) cannot exist above \(115^{\circ} \mathrm{C}\). c. \(\mathrm{I}_{2}(l)\) cannot exist at 1 atmosphere pressure. d. \(\mathrm{I}_{2}(l)\) cannot have a vapor pressure greater than 90 torr. e. \(\mathrm{I}_{2}(l)\) cannot exist at a pressure of 10 torr.

Consider the following enthalpy changes: $$ \begin{aligned} \mathrm{F}^{-}+\mathrm{HF} \longrightarrow \mathrm{FHF}^{-} \quad \Delta H=-155 \mathrm{~kJ} / \mathrm{mol} \\ \left(\mathrm{CH}_{3}\right)_{2} \mathrm{C}=\mathrm{O}+\mathrm{HF} \longrightarrow\left(\mathrm{CH}_{3}\right)_{2} \mathrm{C}=\mathrm{O}-\mathrm{-HF} \\ \Delta H=-46 \mathrm{~kJ} / \mathrm{mol} \\ \mathrm{H}_{2} \mathrm{O}(g)+\mathrm{HOH}(g) \longrightarrow \mathrm{H}_{2} \mathrm{O}--\mathrm{HOH}(\text { in ice }) \\ \Delta H=-21 \mathrm{~kJ} / \mathrm{mol} \end{aligned} $$ How do the strengths of hydrogen bonds vary with the electronegativity of the element to which hydrogen is bonded? Where in the preceding series would you expect hydrogen bonds of the following type to fall?
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