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Chapter 9: Problem 38

What are the strongest attractive forces that must be overcome to (a) melt ice? (b) sublime bromine? (c) boil chloroform (CHCl \(_{3}\) )? (d) vaporize benzene \(\left(\mathrm{C}_{6} \mathrm{H}_{6}\right)\) ?

Short Answer

Expert verified
Answer: a) For ice, the strongest attractive force is hydrogen bonding. b) For bromine, it is Van der Waals (London dispersion) forces. c) For chloroform, it is dipole-dipole interactions. d) For benzene, it is also Van der Waals (London dispersion) forces.

Step by step solution

01

Identify the molecule and its structure

Ice is a solid form of water (H2O), and its structure contains polar molecules held together by hydrogen bonding.
02

Determine the strongest attractive force that must be overcome

In the case of ice, the strongest attractive force that must be overcome is hydrogen bonding between the water molecules. #b) Sublime Bromine#
03

Identify the molecule and its structure

Bromine (Br2) is a non-polar diatomic molecule.
04

Determine the strongest attractive force that must be overcome

In the case of bromine, the strongest attractive force that must be overcome is the Van der Waals (London dispersion) forces between the non-polar bromine molecules. #c) Boil Chloroform (CHCl \(_{3}\) )#
05

Identify the molecule and its structure

Chloroform (CHCl\(_{3}\)) is a polar molecule with a central carbon atom bonded to one hydrogen and three chlorine atoms.
06

Determine the strongest attractive force that must be overcome

In the case of chloroform, the strongest attractive force that must be overcome is the dipole-dipole interaction between the polar chloroform molecules. #d) Vaporize Benzene \(\left(\mathrm{C}_{6} \mathrm{H}_{6}\right)\)#
07

Identify the molecule and its structure

Benzene (C6H6) is an aromatic hydrocarbon with a planar hexagonal structure containing alternating single and double carbon bonds.
08

Determine the strongest attractive force that must be overcome

In the case of benzene, the strongest attractive force that must be overcome is the Van der Waals (London dispersion) forces between the non-polar benzene molecules.

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Most popular questions from this chapter

The density of liquid mercury at \(20^{\circ} \mathrm{C}\) is \(13.6 \mathrm{~g} / \mathrm{cm}^{3}\), its vapor pressure is \(1.2 \times 10^{-3} \mathrm{~mm} \mathrm{Hg}\). (a) What volume (in \(\mathrm{cm}^{3}\) ) is occupied by one mole of \(\mathrm{Hg}(l)\) at \(20^{\circ} \mathrm{C}\) ? (b) What volume (in \(\mathrm{cm}^{3}\) ) is occupied by one mole of \(\mathrm{Hg}(\mathrm{g})\) at \(20^{\circ} \mathrm{C}\) and the equilibrium vapor pressure? (c) The atomic radius of \(\mathrm{Hg}\) is \(0.155 \mathrm{~nm}\). Calculate the volume (in \(\mathrm{cm}^{3}\) ) of one mole of \(\mathrm{Hg}\) atoms \(\left(V=4 \pi r^{3} / 3\right)\). (d) From your answers to (a), (b), and (c), calculate the percentage of the total volume occupied by the atoms in \(\mathrm{Hg}(l)\) and \(\mathrm{Hg}(g)\) at \(20^{\circ} \mathrm{C}\) and \(1.2 \times 10^{-3} \mathrm{~mm} \mathrm{Hg}\)

Of the four general types of solids, which one(s) (a) are generally insoluble in water? (b) have very high melting points? (c) conduct electricity as solids?

In the blanks provided, answer the questions below, using LT (for is less than), GT (for is greater than), \(\mathrm{EQ}\) (for is equal to), or MI (for more information required). (a) The boiling point of \(\mathrm{C}_{3} \mathrm{H}_{7} \mathrm{OH}(\mathrm{MM}=60.0 \mathrm{~g} / \mathrm{mol})\) the boiling point of \(\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{C}=\mathrm{O}(\mathrm{MM}=58.0 \mathrm{~g} / \mathrm{mol})\). (b) The vapor pressure of \(\mathrm{X}\) is \(250 \mathrm{~mm} \mathrm{Hg}\) at \(57^{\circ} \mathrm{C}\). Given a sealed flask at \(57^{\circ} \mathrm{C}\) that contains only gas, the pressure in the flask \(245 \mathrm{~mm} \mathrm{Hg}\) (c) The melting-point curve for Y tilts to the right of a straight line. The density of \(\mathrm{Y}(l) \quad\) the density of \(\mathrm{Y}(s)\). (d) The normal boiling point of \(\mathrm{A}\) is \(85^{\circ} \mathrm{C}\), while the normal boiling point of \(\mathrm{B}\) is \(45^{\circ} \mathrm{C}\). The vapor pressure of \(\mathrm{A}\) at \(85^{\circ} \mathrm{C}\) pressure of \(\mathrm{B}\) at \(45^{\circ} \mathrm{C}\). (e) The triple point of \(A\) is \(25 \mathrm{~mm} \mathrm{Hg}\) and \(5^{\circ} \mathrm{C}\). The melting point of \(\mathrm{A}\) \(5^{\circ} \mathrm{C}\)

The vapor pressure of bromine, \(\mathrm{Br}_{2}(l)\) at \(25^{\circ} \mathrm{C}\) is \(228 \mathrm{~mm} \mathrm{Hg}\). (a) How many grams of bromine will be present as a gas if liquid bromine is poured into an evacuated 2.00-L flask at \(25^{\circ} \mathrm{C} ?\) (b) If \(2.00 \mathrm{~g}\) of bromine is used, what is the final pressure in the flask? Will there be liquid in the flask? (c) If \(2.00 \mathrm{~g}\) of bromine is put into an evacuated \(750.0\) -mL flask at \(25^{\circ} \mathrm{C}\), what is the final pressure in the flask? Will there be any liquid in the flask?

What are the strongest attractive forces that must be overcome to (a) boil silicon hydride \(\mathrm{SiH}_{4} ?\) (b) vaporize calcium chloride? (c) dissolve \(\mathrm{Cl}_{2}\) in carbon tetrachloride, \(\mathrm{CCl}_{4} ?\) (d) melt iodine?
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