1. Slide 1 of 44 Copyright Pearson Prentice Hall Biology

2. Slide 2 of 44 Copyright Pearson Prentice Hall 2-2 Properties of Water

3. Slide 3 of 44 Copyright Pearson Prentice Hall The Water Molecule Like all molecules, a water molecule is neutral.

4. 2-2 Properties of Water Slide 4 of 44 Copyright Pearson Prentice Hall The Water Molecule Why are water molecules polar?

5. 2-2 Properties of Water Slide 5 of 44 Copyright Pearson Prentice Hall The Water Molecule Polarity However an oxygen atom, with 8 protons in its nucleus, has a much stronger attraction for electrons than does the hydrogen atom with a single proton. Thus, there is a greater probability of finding the shared electrons near the oxygen atom than near the hydrogen atom.

6. 2-2 Properties of Water Slide 6 of 44 Copyright Pearson Prentice Hall The Water Molecule As a result, the oxygen end of the molecule has a slight negative charge and the hydrogen end has a slight positive charge. A water molecule is polar because there is an uneven distribution of electrons between the oxygen and hydrogen atoms.

7. 2-2 Properties of Water Slide 7 of 44 Copyright Pearson Prentice Hall The Water Molecule Water Molecule

8. 2-2 Properties of Water Slide 8 of 44 Copyright Pearson Prentice Hall The Water Molecule Hydrogen Bonds Because of their partial positive and negative charges, polar molecules can attract each other.

9. 2-2 Properties of Water Slide 9 of 44 Copyright Pearson Prentice Hall The Water Molecule The attraction between the hydrogen atoms on one molecule and the oxygen atom on another water molecule is an example of a hydrogen bond. Hydrogen bonds are not as strong as covalent or ionic bonds.

10. 2-2 Properties of Water Slide 10 of 44 Copyright Pearson Prentice Hall The Water Molecule A single water molecule may be involved in as many as four hydrogen bonds at a time. Water’s ability to form multiple hydrogen bonds is responsible for many of its special properties.

11. 2-2 Properties of Water Slide 11 of 44 Copyright Pearson Prentice Hall The Water Molecule Hydrogen bonds form between water molecules.

12. 2-2 Properties of Water Slide 12 of 44 Copyright Pearson Prentice Hall The Water Molecule Cohesion is an attraction between molecules of the same substance. Because of hydrogen bonding, water is extremely cohesive.

13. 2-2 Properties of Water Slide 13 of 44 Copyright Pearson Prentice Hall The Water Molecule Water's cohesion causes molecules on the surface of water to be drawn inward, which is why drops of water form beads on a smooth surface. Cohesion also explains why some insects and spiders can walk on a pond's surface.

14. 2-2 Properties of Water Slide 14 of 44 Copyright Pearson Prentice Hall The Water Molecule Adhesion is an attraction between molecules of different substances. The surface of water in a graduated cylinder dips in the center because adhesion between water molecules and glass molecules is stronger than cohesion between water molecules.

15. 2-2 Properties of Water Slide 15 of 44 Copyright Pearson Prentice Hall The Water Molecule Adhesion between water and glass causes water to rise in a narrow tube against the force of gravity. This effect is called capillary action.

16. 2-2 Properties of Water Slide 16 of 44 Copyright Pearson Prentice Hall The Water Molecule Capillary action is one of the forces that draw water out of the roots of a plant and up into its stems and leaves. Cohesion holds the column of water together as it rises.

17. 2-2 Properties of Water Slide 17 of 44 Copyright Pearson Prentice Hall Solutions and Suspensions A mixture is a material composed of two or more elements or compounds that are physically mixed but not chemically combined.

18. 2-2 Properties of Water Slide 18 of 44 Copyright Pearson Prentice Hall Solutions and Suspensions Two types of mixtures can be made with water solutions suspensions

19. 2-2 Properties of Water Slide 19 of 44 Copyright Pearson Prentice Hall Solutions and Suspensions Solutions All the components of a solution are evenly distributed throughout the solution. In a salt–water solution, table salt is the solute—the substance that is dissolved. Water is the solvent—the substance in which the solute dissolves.

20. 2-2 Properties of Water Slide 20 of 44 Copyright Pearson Prentice Hall Solutions and Suspensions When a crystal of table salt is placed in warm water, sodium and chloride ions are attracted to the polar water molecules. Na + Cl - Water

21. 2-2 Properties of Water Slide 21 of 44 Copyright Pearson Prentice Hall Solutions and Suspensions Ions break away from the crystal and are surrounded by water molecules. Na + Cl - Water

22. 2-2 Properties of Water Slide 22 of 44 Copyright Pearson Prentice Hall Solutions and Suspensions The ions gradually become dispersed in the water, forming a solution. Na + Cl - Water

23. 2-2 Properties of Water Slide 23 of 44 Copyright Pearson Prentice Hall Solutions and Suspensions Water's polarity gives it the ability to dissolve both ionic compounds and other polar molecules, such as sugar. Water is the greatest solvent on Earth.

24. 2-2 Properties of Water Slide 24 of 44 Copyright Pearson Prentice Hall Solutions and Suspensions Suspensions Some materials do not dissolve when placed in water but separate into pieces so small that they do not settle out.

25. 2-2 Properties of Water Slide 25 of 44 Copyright Pearson Prentice Hall Solutions and Suspensions The movement of water molecules keeps the small particles suspended. Such mixtures of water and nondissolved material are known as suspensions.

26. 2-2 Properties of Water Slide 26 of 44 Copyright Pearson Prentice Hall Solutions and Suspensions Some of the most important biological fluids are both solutions and suspensions. The blood that circulates through your body is mostly water, which contains many dissolved compounds. Blood also contains cells and other undissolved particles that remain in suspension as the blood moves through the body.

27. 2-2 Properties of Water Slide 27 of 44 Copyright Pearson Prentice Hall Acids, Bases, and pH What are acidic solutions? What are basic solutions?

28. 2-2 Properties of Water Slide 28 of 44 Copyright Pearson Prentice Hall Acids, Bases, and pH A water molecule can react to form hydrogen and hydroxide ions. Water is neutral because the number of positive hydrogen ions (H + ) produced is equal to the number of negative hydroxide ions (OH - ) produced.

29. 2-2 Properties of Water Slide 29 of 44 Copyright Pearson Prentice Hall Acids, Bases, and pH The pH scale Chemists devised a measurement system called the pH scale to indicate the concentration of H + ions in solution. The pH scale ranges from 0 to 14.

30. 2-2 Properties of Water Slide 30 of 44 Copyright Pearson Prentice Hall Acids, Bases, and pH At a pH of 7, the concentration of H + ions and OH - ions is equal. Pure water has a pH of 7. The pH Scale Human blood Milk Sea water Normal rainfall Pure water

31. 2-2 Properties of Water Slide 31 of 44 Copyright Pearson Prentice Hall Acids, Bases, and pH Solutions with a pH below 7 are called acidic because they have more H + ions than OH - ions. The lower the pH, the greater the acidity. Acid rain Tomato juice Lemon juice Stomach acids The pH Scale

32. 2-2 Properties of Water Slide 32 of 44 Copyright Pearson Prentice Hall Acids, Bases, and pH Solutions with a pH above 7 are called basic because they have more OH - ions than H + ions. The higher the pH, the more basic the solution. The pH Scale Soap Bleach Oven cleaner Ammonia solution

33. 2-2 Properties of Water Slide 33 of 44 Copyright Pearson Prentice Hall Acids, Bases, and pH Acids An acid is any compound that forms H + ions in solution. Acidic solutions contain higher concentrations of H + ions than pure water and have pH values below 7.

34. 2-2 Properties of Water Slide 34 of 44 Copyright Pearson Prentice Hall Acids, Bases, and pH Strong acids tend to have pH values that range from 1 to 3. The hydrochloric acid produced by the stomach to help digest food is a strong acid.

35. 2-2 Properties of Water Slide 35 of 44 Copyright Pearson Prentice Hall Acids, Bases, and pH Bases A base is a compound that produces hydroxide ions (OH - ions) in solution. Basic, or alkaline, solutions contain lower concentrations of H + ions than pure water and have pH values above 7.

36. 2-2 Properties of Water Slide 36 of 44 Copyright Pearson Prentice Hall Acids, Bases, and pH Strong bases, such as lye, tend to have pH values ranging from 11 to 14.

37. 2-2 Properties of Water Slide 37 of 44 Copyright Pearson Prentice Hall Acids, Bases, and pH Buffers The pH of the fluids within most cells in the human body must generally be kept between 6.5 and 7.5. If the pH is lower or higher, it will affect the chemical reactions that take place within the cells.

38. 2-2 Properties of Water Slide 38 of 44 Copyright Pearson Prentice Hall Acids, Bases, and pH Controlling pH is important for maintaining homeostasis. One of the ways that the body controls pH is through dissolved compounds called buffers. Buffers are weak acids or bases that can react with strong acids or bases to prevent sharp, sudden changes in pH.

39. - or - Continue to: Click to Launch: Slide 39 of 44 Copyright Pearson Prentice Hall 2-2

40. Slide 40 of 44 Copyright Pearson Prentice Hall 2-2 A molecule in which the charges are unevenly distributed is called a a.polar molecule. b.cohesive molecule. c.hydrogen molecule. d.covalent molecule.

41. Slide 41 of 44 Copyright Pearson Prentice Hall 2-2 A dissolved substance is called a a.solvent. b.solution. c.solute. d.suspension.

42. Slide 42 of 44 Copyright Pearson Prentice Hall 2-2 A compound that produces hydroxide ions in solution is called a(an) a.base. b.buffer. c.acid. d.salt.

43. Slide 43 of 44 Copyright Pearson Prentice Hall 2-2 Hydrogen bonds between water molecules result from a.adhesion between water molecules. b.magnetic attractions between water molecules. c.uneven electron distribution in each water molecule. d.ionic bonds in the water molecule.

44. Slide 44 of 44 Copyright Pearson Prentice Hall 2-2 On a pH scale, a value of 2 means that the solution has a.equal concentrations of H + and OH - ions. b.the same concentration of H + ions as pure water. c.higher concentration of H + than in pure water. d.lower concentration of H + than in pure water.

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