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Chapter 11: Problem 24

Propyl alcohol \(\left(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{OH}\right)\) and isopropyl alcohol \(\left[\left(\mathrm{CH}_{3}\right)_{2} \mathrm{CHOH}\right],\) whose space- filling models are shown, have boiling points of 97.2 and \(82.5^{\circ} \mathrm{C}\), respectively. Explain why the boiling point of propyl alcohol is higher, even though both have the molecular formula, \(\mathrm{C}_{3} \mathrm{H}_{8} \mathrm{O}\).

Short Answer

Expert verified
Propyl alcohol's linear structure results in stronger dispersion forces, requiring more energy to break its intermolecular forces, thus a higher boiling point.

Step by step solution

01

Understand Molecular Structures

Both propyl alcohol (1-propanol) and isopropyl alcohol (2-propanol) have the same molecular formula, \(C_3H_8O\). Propyl alcohol has a straight-chain structure (CH\(_3\)CH\(_2\)CH\(_2\)OH), while isopropyl alcohol has a branched structure (\((CH_3)_2CHOH\)). The structural difference affects how the molecules interact.
02

Explore Shape and Surface Area

The linear structure of propyl alcohol allows for greater surface area contact between molecules compared to the branched structure of isopropyl alcohol. This increased surface area in propyl alcohol results in stronger London dispersion forces, which are a type of van der Waals force.
03

Analyze Intermolecular Forces

Both alcohols can form hydrogen bonds because they contain -OH groups. However, the stronger London dispersion forces in propyl alcohol, due to its greater surface area, contribute to a higher overall intermolecular attraction.
04

Correlate Boiling Point and Intermolecular Forces

The boiling point of a substance is related to the strength of its intermolecular forces. Propyl alcohol's combination of hydrogen bonding and stronger London dispersion forces due to its linear structure means it takes more energy (higher temperature) to break these forces, resulting in a higher boiling point than isopropyl alcohol.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Intermolecular Forces
Intermolecular forces are the attractive forces that occur between neighboring molecules. They are crucial in determining the physical properties of substances, such as boiling points. Boiling a liquid involves supplying enough energy to overcome these intermolecular forces, allowing molecules to move freely and transition into a gaseous state.

The primary types of intermolecular forces include dipole-dipole interactions, hydrogen bonding, and London dispersion forces. The stronger these forces are between molecules, the higher the temperature needed to overcome them, thus leading to a higher boiling point.
Hydrogen Bonding
Hydrogen bonding is a specific, strong type of dipole-dipole interaction. It occurs when a hydrogen atom, covalently bonded to a highly electronegative atom such as oxygen, nitrogen, or fluorine, interacts with a lone pair of electrons on another electronegative atom.

Both propyl alcohol and isopropyl alcohol have -OH groups, enabling hydrogen bonding between their molecules. This bond is relatively strong and significantly affects the boiling points of substances. Despite having similar capabilities for hydrogen bonding, the boiling points differ due to other forces at play, such as London dispersion forces.
London Dispersion Forces
London dispersion forces are the weakest type of van der Waals forces. They arise from momentary differences in charge distribution within a molecule that induce temporary dipoles in nearby molecules.
  • The strength of London dispersion forces is influenced by the surface area and the shape of molecules.
  • Molecules with larger surface areas can have more significant London dispersion interactions, leading to higher boiling points.
In propyl alcohol, the larger surface area due to its linear structure allows for stronger London dispersion forces compared to the branched structure of isopropyl alcohol. This difference is a key contributor to the variation in their boiling points.
Molecular Structure
Molecular structure determines how molecules occupy space and interact with one another. The arrangement of atoms in a molecule (its geometry and shape) can significantly influence its physical properties.

Both propyl alcohol and isopropyl alcohol share the same molecular formula, but they differ in structure. This particular aspect influences the type and strength of intermolecular forces they experience, directly affecting boiling points. Understanding these differences is crucial when investigating properties like boiling point variations.
Linear Structure
A linear structure is characterized by a straight, unbranched arrangement of atoms. In the case of propyl alcohol, this straight-chain formation allows for more effective alignment and interaction between molecules.

The greater alignment capability afforded by a linear structure increases the overall surface area for interactions. This results in stronger intermolecular forces, particularly London dispersion forces, because the molecules can pack closer together. Therefore, substances with a linear structure often demonstrate higher boiling points compared to those with branched structures.
Branched Structure
A branched structure features a more compact and complex arrangement of atoms, forming side-chains extending off the main chain. Isopropyl alcohol has such a structure.
  • Branched molecules generally have a reduced surface area for intermolecular interactions as compared to their linear counterparts.
  • This reduced surface area results in weaker London dispersion forces.
Consequently, substances with branched structures tend to have lower boiling points, as observed with isopropyl alcohol compared to propyl alcohol.

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Most popular questions from this chapter

A number of salts containing the tetrahedral polyatomic anion, \(\mathrm{BF}_{4}^{-}\), are ionic liquids, whereas salts containing the somewhat larger tetrahedral ion \(\mathrm{SO}_{4}{ }^{2-}\) do not form ionic liquids. Explain this observation.

(a) What is the significance of the triple point in a phase diagram? (b) Could you measure the triple point of water by measuring the temperature in a vessel in which water vapor, liquid water, and ice are in equilibrium under \(101,32 \mathrm{kPa}\) of air? Explain.

(a) What phase change is represented by the "heat of vaporization" of a substance? (b) Is the process of vaporization endothermic or exothermic? (c) If you compare a substance's heat of vaporization to the amount of heat released during condensation, which one is generally larger (consider the numerical value only)?

The table below lists the density of substance \(\mathrm{X}\) at various temperatures and at \(101.3 \mathrm{kPa}\). The normal melting point of substance \(X\) is \(80 \mathrm{~K}\). \begin{tabular}{cc} \hline Temperature \((\mathrm{K})\) & Density \((\mathrm{mol} / \mathrm{L})\) \\ \hline 90 & 35.2 \\ 100 & 33.8 \\ 110 & 32.1 \\ 120 & 0.136 \\ 140 & 0.110 \\ 160 & 0.0893 \\ 180 & 0.0796 \\ \hline \end{tabular} (a) Over what temperature range is substance \(X\) a solid? (b) Over what temperature range is \(\mathrm{X}\) a liquid? \((\mathbf{c})\) Over what temperature range in the table is \(\mathrm{X}\) a gas? (d) Estimate the normal boiling point of \(X .\) (e) Given that \(X\) is a nonpolar molecule, suggest the kind of intermolecular forces in \(\mathrm{X}\).

(a) How does the average kinetic energy of molecules compare with the average energy of attraction between molecules in solids, liquids, and gases? (b) Why does increasing the temperature cause a solid substance to change in succession from a solid to a liquid to a gas? (c) What happens to a eas if you put it under extremelv high pressuret
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