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What are the three main intermolecular forces? Which one describes the intermolecular forces in water? Draw a picture of three water molecules showing this intermolecular force. Draw a picture of sodium azide dissolved in water and explain the attractions involved. In terms of enthalpy and entropy, why does sodium azide dissolve spontaneously in water?

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D. 1. Silver chloride is not soluble in water. What are the relative strengths of the intermolecular forces between Ag and Ciions and water molecules as compared to the intermolecular forces between water molecules and the forces that hold the silver chloride as a solid? a. The ionic attractions are stronger than the polar covalent bonds between the H' and O ions of the b. The ionic attractions are weaker than the intermolecular forces between the Ag' and Cr ions and water c. The ionic attractions are stronger than the intermolecular forces between the Ag' and Cr ions and water d. The ionic attractions are the same as the intermolecular forces between the Ag and CI ions and water water molecules. molecules. molecules molecules 2. The value of AHsotn for a water soluble compound is +34 kJ moÄ¾1. Which value for this compound would be numerically larger, its lattice energy or its hydration energy? Select the single best answer. step. b. The lattice energy, because it is the endothermic step c. The hydration energy, because it is the exothermic step. d. The lattice energy, because it is the exothermic step. 3, which of the following are reasons why the value of ì¨,on for a gas such as CO2, dissolving in water, is negative? a. When a gas dissolves in a liquid, there is no endothermic step as with the lattice energy of a solid. b. When a gas dissolves in a liquid, there is only an exothermic step as with the lattice energy of a solid. c. The only enthalpy change is the one associated with hydration, and this is always positive. d. The only enthalpy change is the one associated with hydration, and this is always negative. e. When a gas dissolves in a liquid the lattice energy is always higher than the hydration energy, making the net enthalpy always negative. 4. Why is ammonia so much more soluble in water than is nitrogen? a. The triple bond in nitrogen prevents it from dissolving in water. b. Nitrogen has only London forces, while both water and ammonia form hydrogen bonds. c. The molar mass of nitrogen is much larger than the molar mass of ammonia, which reduces its solubility. d. Diatomic molecules are never soluble in water s which agueous solution, if either, is likely to have the highÏr boiling point 50 m Nal or en-Na e au

1. What kind of intermolecular force is responsible for the higher boiling point of pentane (C5 H12) with respect to methane (CH4 )?

2. What kind of intermolecular force is considered responsible for the higher boiling point of water with respect to hydrogen sulfide (H2 S)?

3. What kind of intermolecular force exists between sodium ions and water molecules in a water solution of sodium chloride?

4.Why are colligative properties useful for the determination of molecular weights of substances?

Acetone, CH₃COCH₃, is a common laboratory solvent. It is usually contaminated with water, however.

Why does acetone absorb water so readily?

Draw molecular structures showing how water and acetone can interact.

What intermolecular force(s) is(are) involved in the interaction?

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