Chapter 15 Water and Aqueous Systems 15.1 Water and Its Properties 15.2 Homogeneous Aqueous Systems 15.3 Heterogeneous Aqueous Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

What properties of water make it essential to life on Earth? CHEMISTRY & YOU What properties of water make it essential to life on Earth? Water covers about three quarters of Earth’s surface. All known life forms are made mostly of water. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Water in the Liquid State What factor causes the high surface tension, low vapor pressure, and high boiling point of water? Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Water in the Liquid State Water, H2O, is a simple molecule consisting of three atoms. The oxygen atom forms a covalent bond with each of the hydrogen atoms. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Water in the Liquid State Water, H2O, is a simple molecule consisting of three atoms. The oxygen atom forms a covalent bond with each of the hydrogen atoms. Oxygen has a greater electronegativity than hydrogen, so the oxygen atom attracts the electron pair of the covalent O—H bond to a greater extent than the hydrogen atom. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Water in the Liquid State Water, H2O, is a simple molecule consisting of three atoms. The oxygen atom forms a covalent bond with each of the hydrogen atoms. Oxygen has a greater electronegativity than hydrogen, so the oxygen atom attracts the electron pair of the covalent O—H bond to a greater extent than the hydrogen atom. Thus, the O—H bond is highly polar. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Water in the Liquid State Molecule has net polarity Polar bonds δ– δ+ The oxygen atom acquires a partial negative charge (δ–). Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Water in the Liquid State Molecule has net polarity Polar bonds δ– δ+ The oxygen atom acquires a partial negative charge (δ–). The less electronegative hydrogen atoms acquire partial positive charges (δ+). Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Water in the Liquid State How do the polarities of the two O—H bonds affect the polarity of the molecule? Molecule has net polarity Polar bonds δ– δ+ Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Water in the Liquid State How do the polarities of the two O—H bonds affect the polarity of the molecule? Molecule has net polarity Polar bonds δ– δ+ The molecule has a bent shape. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Water in the Liquid State How do the polarities of the two O—H bonds affect the polarity of the molecule? Molecule has net polarity Polar bonds δ– δ+ The molecule has a bent shape. The two O—H bond polarities do not cancel. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Water in the Liquid State How do the polarities of the two O—H bonds affect the polarity of the molecule? Molecule has net polarity Polar bonds δ– δ+ The molecule has a bent shape. The two O—H bond polarities do not cancel. The water molecule as a whole is polar. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Water in the Liquid State In general, polar molecules are attracted to one another by dipole interactions. The negative end of one molecule attracts the positive end of another molecule. δ+ δ– Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Water in the Liquid State However, in water, this attraction results in hydrogen bonding. Hydrogen bonds are attractive forces that arise when a hydrogen atom is covalently bonded to a very electronegative atom and also weakly bonded to an unshared electron pair of another electronegative atom. Liquid water Hydrogen bond Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Water in the Liquid State Many unique and important properties of water—including its high surface tension, low vapor pressure, and high boiling point—result from hydrogen bonding. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Water in the Liquid State Surface Tension Have you ever noticed that water forms nearly spherical droplets on a leaf? Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Water in the Liquid State Surface Tension The water molecules within the body of the liquid form hydrogen bonds with the other molecules that surround them on all sides. The attractive forces on each of these molecules are balanced. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Water in the Liquid State Surface Tension The water molecules within the body of the liquid form hydrogen bonds with the other molecules that surround them on all sides. The attractive forces on each of these molecules are balanced. Water molecules at the surface of the liquid experience an unbalanced attraction. As a result, water molecules at the surface tend to be drawn inward. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Water in the Liquid State Surface Tension The inward force, or pull, that tends to minimize the surface area of a liquid is called surface tension. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Water in the Liquid State Surface Tension The inward force, or pull, that tends to minimize the surface area of a liquid is called surface tension. All liquids have a surface tension, but water’s surface tension is higher than most. The surface tension of water tends to hold a drop of liquid in a spherical shape. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Water in the Liquid State Surface Tension It is possible to decrease the surface tension of water by adding a surfactant. A surfactant is any substance that interferes with the hydrogen bonding between water molecules and thereby reduces surface tension. Soaps and detergents are surfactants. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Water in the Liquid State Vapor Pressure Hydrogen bonding between water molecules also explains water’s unusually low vapor pressure. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Water in the Liquid State Vapor Pressure Hydrogen bonding between water molecules also explains water’s unusually low vapor pressure. An extensive network of hydrogen bonds holds the molecules in liquid water to one another. These hydrogen bonds must be broken before water changes from the liquid to the vapor state, so the tendency of these molecules to escape is low and evaporation is slow. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Water in the Liquid State Boiling Point Molecular compounds of low molecular mass are usually gases or liquids with low boiling points at normal atmospheric pressure. Ammonia (NH3) has a molar mass of 17.0 g/mol and boils at about –33˚C. Water has a molar mass of 18.0 g/mol, but it has a boiling point of 100˚C. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Water in the Liquid State Boiling Point The difference between the boiling points of ammonia and water is due to hydrogen bonding, which is more extensive in water than in ammonia. It takes much more heat to disrupt the attractions between water molecules than those between ammonia molecules. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Some insects are able to walk across water Some insects are able to walk across water. How do the properties of water explain their ability? Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Some insects are able to walk across water Some insects are able to walk across water. How do the properties of water explain their ability? The surface tension of water is relatively high. As long as the forces holding the surface water molecules together are stronger than the forces exerted down on the water by the insect, the insect will not sink. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Water in the Solid State How can you describe the structure of ice? Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Water in the Solid State Ice cubes float in your glass of iced tea because solid water has a lower density than liquid water. This situation is not usual for liquids. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Water in the Solid State As water begins to cool, it behaves initially like a typical liquid. It contracts slightly, and its density gradually increases. When the temperature of the water falls below 4˚C, the density of water actually starts to decrease. Density of Liquid Water and Ice Temperature (˚C) Density (g/cm3) 100 (liquid water) 0.9584 50 0.9881 25 0.9971 10 0.9997 4 1.0000 0 (liquid water) 0.9998 0 (ice) 0.9168 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Water in the Solid State Below 4˚C, water no longer behaves like a typical liquid. Ice, which forms at 0˚C, has about a 10% lower density than water at 0˚C. Ice is one of only a few solids that floats in its own liquid. Density of Liquid Water and Ice Temperature (˚C) Density (g/cm3) 100 (liquid water) 0.9584 50 0.9881 25 0.9971 10 0.9997 4 1.0000 0 (liquid water) 0.9998 0 (ice) 0.9168 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Water in the Solid State Why is ice less dense than liquid water? Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Water in the Solid State Why is ice less dense than liquid water? The structure of ice is a regular open framework of water molecules in a hexagonal arrangement. The hexagonal symmetry of a snowflake reflects the structure of the ice crystal. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Water in the Solid State The unique properties of ice are a result of hydrogen bonding. Extensive hydrogen bonding in ice holds the water molecules farther apart in a more ordered arrangement than in liquid water. Hydrogen bond Ice Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Water in the Solid State The fact that ice floats has important consequences for all organisms. The liquid water at the bottom of an otherwise frozen body of water is warmer than 0˚C, so fish and other aquatic life are better able to survive. If ice were denser than liquid water, bodies of water would tend to freeze solid during the winter months, destroying many types of organisms. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

CHEMISTRY & YOU What properties of water that result from hydrogen bonding make it essential to life on Earth? Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

CHEMISTRY & YOU What properties of water that result from hydrogen bonding make it essential to life on Earth? The low vapor pressure of water keeps the liquid water in all of Earth’s lakes and oceans from evaporating rapidly. If water did not have such a high boiling point, it would be a vapor at the usual temperatures found on Earth. The fact that ice floats allows fish and other aquatic life to survive the winter months. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

In ice, how many hydrogen bonds can be formed between one hydrogen atom of a water molecule and the oxygen in surrounding water molecules? A. 0 B. 1 C. 2 D. 3 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

In ice, how many hydrogen bonds can be formed between one hydrogen atom of a water molecule and the oxygen in surrounding water molecules? A. 0 B. 1 C. 2 D. 3 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Key Concepts Many unique and important properties of water—including its high surface tension, low vapor pressure, and high boiling point—result from hydrogen bonding. The structure of ice is a regular open framework of water molecules in a hexagonal arrangement. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Glossary Terms surface tension: an inward force that tends to minimize the surface area of a liquid; it causes the surface to behave as if it were a thin skin surfactant: any substance that interferes with the hydrogen bonding between water molecules and thereby reduces surface tension; soaps and detergents are surfactants Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Bonding and Interactions BIG IDEA Bonding and Interactions Water molecules are held together through hydrogen bonds. The hydrogen bonding interactions between water molecules account for the unique properties of water, including its high surface tension, low vapor pressure, and high boiling point. Hydrogen bonding also accounts for the fact that ice is less dense than liquid water. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

END OF 15.1 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.