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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) The intermolecular attractive force that operates between all molecules is "London dispersion forces" or "van der Waals forces". (b) The intermolecular attractive force that operates only between polar molecules is called "dipole-dipole interactions". (c) The intermolecular attractive force that operates between the hydrogen atom of a polar bond and a nearby small electronegative atom is called "hydrogen bonding".

Step by step solution

01

(a) Type of force that operates between all molecules:

The intermolecular attractive force that operates between all molecules, regardless of their polarity or type, is called "London dispersion forces" or "van der Waals forces". These forces arise due to temporary fluctuations in electron distribution around molecules, which create temporary dipoles that induce dipoles in nearby molecules.
02

(b) Type of force that operates only between polar molecules:

The intermolecular attractive force that operates only between polar molecules is called "dipole-dipole interactions". These forces occur when the positive end (partial positive charge) of one polar molecule interacts with the negative end (partial negative charge) of another polar molecule.
03

(c) Type of force that operates between the hydrogen atom of a polar bond and a nearby small electronegative atom:

The intermolecular attractive force that operates only between the hydrogen atom of a polar bond and a nearby small electronegative atom (such as fluorine, oxygen, or nitrogen) is called "hydrogen bonding". This is a special case of dipole-dipole interaction, where the hydrogen atom forms a particularly strong interaction with the nearby electronegative atom due to the significant difference in electronegativity between them.

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Most popular questions from this chapter

If 42.0 \(\mathrm{kJ}\) of heat is added to a \(32.0-\mathrm{g}\) sample of liquid methane under 1 \(\mathrm{atm}\) of pressure at a temperature of \(-170^{\circ} \mathrm{C}\) , what are the final state and temperature of the methane once the system equilibrates? Assume no heat is lost to the surroundings. The normal boiling point of methane is \(-161.5^{\circ} \mathrm{C}\) The specific heats of liquid and gaseous methane are 3.48 and \(2.22 \mathrm{J} / \mathrm{g}-\mathrm{K}\) , respectively. [ Section 11.4\(]\)

Hydrazine \(\left(\mathrm{H}_{2} \mathrm{NNH}_{2}\right),\) hydrogen peroxide \((\mathrm{HOOH}),\) and water \(\left(\mathrm{H}_{2} \mathrm{O}\right)\) all have exceptionally high surface tensions compared with other substances of comparable molecular weights. (a) Draw the Lewis structures for these three compounds. (b) What structural property do these substances have in common, and how might that account for the high surface tensions?

Which member in each pair has the greater dispersion forces? (a) \(\mathrm{H}_{2} \mathrm{O}\) or \(\mathrm{H}_{2} \mathrm{S},(\mathbf{b}) \mathrm{CO}_{2}\) or \(\mathrm{CO},(\mathbf{c}) \operatorname{siH}_{4}\) or \(\mathrm{GeH}_{4}\) .

(a) What is the significance of the critical point in a phase diagram? (b) Why does the line that separates the gas and liquid phases end at the critical point?

(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 1 atm of air? Explain.
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