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Chapter 11: Problem 15

(a) Which type of intermolecular attractive force operates between all molecules? (b) Which type of intermolecular attractive force operates only between polar molecules? (c) Which type of intermolecular attractive force operates only between the hydrogen atom of a polar bond and a nearby small electronegative atom?

Short Answer

Expert verified
(a) Dispersion forces operate between all molecules. (b) Dipole-dipole forces operate only between polar molecules. (c) Hydrogen bonding operates only between the hydrogen atom of a polar bond (e.g., H-F, H-O, or H-N) and a nearby small electronegative atom (F, O, or N).

Step by step solution

01

(a) Intermolecular attractive force operates between all molecules

The type of intermolecular attractive force that operates between all molecules is called dispersion forces, also known as London dispersion forces or Van der Waals forces. These forces result from the temporary movement of electrons within a molecule, which creates a temporary dipole in the molecule. The temporary dipole can then induce nearby dipoles in neighboring molecules, leading to an attraction between the molecules.
02

(b) Intermolecular attractive force operates only between polar molecules

The type of intermolecular attractive force that operates only between polar molecules is called dipole-dipole forces. Polar molecules have a positive and a negative end, or dipole, due to a difference in electronegativity between the atoms making up the molecule. In a polar molecule, the more electronegative atom pulls electron density towards itself, creating a partial negative charge while the other atom develops a partial positive charge. Dipole-dipole forces occur when the partial positive charge of one polar molecule attracts the partial negative charge of an adjacent polar molecule.
03

(c) Intermolecular attractive force operates only between the hydrogen atom of a polar bond and a nearby small electronegative atom

The type of intermolecular attractive force that operates only between the hydrogen atom of a polar bond (e.g., H-F, H-O, or H-N) and a nearby small electronegative atom (F, O, or N) is called hydrogen bonding. Hydrogen bonding is a particularly strong type of dipole-dipole interaction that occurs specifically between a hydrogen atom bonded to an electronegative atom and an electronegative atom in a neighboring molecule. This strong interaction results from the small size of hydrogen and the highly electronegative atoms (F, O, or N), which allow for a close approach and strong attraction between the molecules.

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Most popular questions from this chapter

Ethylene glycol \(\left(\mathrm{HOCH}_{2} \mathrm{CH}_{2} \mathrm{OH}\right)\) and pentane \(\left(\mathrm{C}_{5} \mathrm{H}_{12}\right)\) are both liquids at room temperature and room pressure, and have about the same molecular weight. (a) One of these liquids is much more viscous than the other. Which one do you predict is more viscous? (b) One of these liquids has a much lower normal boiling point \(\left(36.1^{\circ} \mathrm{C}\right)\) compared to the other one \(\left(198^{\circ} \mathrm{C}\right)\). Which liquid has the lower normal boiling point? (c) One of these liquids is the major component in antifreeze in automobile engines. Which liquid would you expect to be used as antifreeze? (d) One of these liquids is used as a "blowing agent" in the manufacture of polystyrene foam because it is so volatile. Which liquid would you expect to be used as a blowing agent?

Which type of intermolecular force accounts for each of these differences? (a) Acetone, \(\left(\mathrm{CH}_{3}\right)_{2} \mathrm{CO},\) boils at $56^{\circ} \mathrm{C} ;\( dimethyl sulfoxide or DMSO, (CH \)\left._{3}\right)_{2}$ SO, boils at \(189^{\circ}\) C. (b) \(\mathrm{CCl}_{4}\) is a liquid at atmospheric pressure and room temperature, whereas \(\mathrm{CH}_{4}\) is a gas under the same conditions. \((\mathbf{c})\) \(\mathrm{H}_{2} \mathrm{O}\) boils at \(100^{\circ} \mathrm{C}\) but \(\mathrm{H}_{2} \mathrm{~S}\) boils at \(-60^{\circ} \mathrm{C}\). (d) 1 -propanol boils at \(97^{\circ} \mathrm{C}\), whereas 2 -propanol boils at \(82.6^{\circ} \mathrm{C}\).

(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.

True or false: (a) Molecules containing polar bonds must be polar molecules and have dipole-dipole forces. (b) For the halogen gases, the dispersion forces decrease while the boiling points increase as you go down the column in the periodic table. (c) In terms of the total attractive forces for a given substance, the more polar bonds there are in a molecule, the stronger the dipole-dipole interaction. \(\mathbf{d}\) ) All other factors being the same, total attractive forces between linear molecules are greater than those between molecules whose shapes are nearly spherical. (e) The more electronegative the atom, the more polarizable it is.

Indicate whether each statement is true or false: (a) The critical pressure of a substance is the pressure at which it turns into a solid at room temperature. \((\mathbf{b})\) The critical temperature of a substance is the highest temperature at which the liquid phase can form. (c) Generally speaking, the higher the critical temperature of a substance, the lower its critical pressure. (d) In general, the more intermolecular forces there are in a substance, the higher its critical temperature and pressure.
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