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Chapter 11: Problem 12

At room temperature, Si is a solid, \(\mathrm{CCl}_{4}\) is a liquid, and Ar is gas. List these substances in order of (a) increasing intermolecular energy of attraction and (b) increasing boiling point.

Short Answer

Expert verified
a) Increasing intermolecular energy of attraction: Ar < CCl4 < Si b) Increasing boiling point: Ar < CCl4 < Si

Step by step solution

01

Identify the intermolecular forces

For Si: Since it's a solid and a covalent network, it has covalent bonding. For CCl4: It is a nonpolar molecule due to the equal distribution of charge, and thus has London dispersion forces (LDF). For Ar: It is an inert noble gas, and also has London dispersion forces. Step 2: Compare the strengths of intermolecular forces
02

Compare the intermolecular forces

Covalent bonding in Si is stronger than LDFs. Therefore, Si will have a greater energy of attraction and a higher boiling point than both CCl4 and Ar. Between CCl4 and Ar, CCl4 has stronger LDFs than Ar because it has more electrons which make the LDFs stronger. So, CCl4 has a greater energy of attraction and a higher boiling point than Ar. Step 3: List the substances in order of increasing intermolecular energy of attraction
03

Arrange the substances based on intermolecular energy of attraction

From our comparison in step 2, we can list the substances in the following order: Ar < CCl4 < Si Step 4: List the substances in order of increasing boiling point
04

Arrange the substances based on boiling point

Since boiling point is directly related to the strength of intermolecular forces, we can arrange the substances in the same order as in step 3: Ar < CCl4 < Si Final Answer: a) Increasing intermolecular energy of attraction: Ar < CCl4 < Si b) Increasing boiling point: Ar < CCl4 < Si

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Most popular questions from this chapter

Acetone \(\left[\left(\mathrm{CH}_{3}\right)_{2} \mathrm{CO}\right]\) is widely used as an industrial solvent. (a) Draw the Lewis structure for the acetone molecule and predict the geometry around each carbon atom. (b) Is the acetone molecule polar or nonpolar? (c) What kinds of intermolecular attractive forces exist between acetone mol-ecules? (\boldsymbol{d} 1 Propanol ~ ( C H ~ \(_{3} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{OH}\) ) has a molecular weight that is very similar to that of acetone, yet acetone boils at \(56.5^{\circ} \mathrm{C}\) and 1 -propanol boils at \(97.2^{\circ} \mathrm{C}\) . Explain the difference.

(a) What atoms must a molecule contain to participate in hydrogen bonding with other molecules of the same kind? (b) Which of the following molecules can form hydrogen bonds with other molecules of the same kind: \(\mathrm{CH}_{3} \mathrm{F}, \mathrm{CH}_{3} \mathrm{NH}_{2}, \mathrm{CH}_{3} \mathrm{OH}, \mathrm{CH}_{3} \mathrm{B}\) ?

(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?

You are high up in the mountains and boil water to make some tea. However, when you drink your tea, it is not as hot as it should be. You try again and again, but the water is just not hot enough to make a hot cup of tea. Which is the best explanation for this result? (a) High in the mountains, it is probably very dry, and so the water is rapidly evaporating from your cup and cooling it. (b) High in the mountains, it is probably very windy, and so the water is rapidly evaporating from your cup and cooling it. (c) High in the mountains, the air pressure is significantly less than 1 atm, so the boiling point of water is much lower than at sea level. (d) High in the mountains, the air pressure is significantly less than 1 atm, so the boiling point of water is much higher than at sea level.

(a) Which is generally stronger, intermolecular interactions or intramolecular interactions? (b) Which of these kinds of interactions are broken when a liquid is converted to a gas?
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