The Water Molecule. Like all molecules, a water molecule is neutral. Water is polar. Why are water molecules polar?

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1 Properties of Water

2 The Water Molecule Like all molecules, a water molecule is neutral. Water is polar Why are water molecules polar?

3 Polarity oxygen atom 8 protons in its nucleus has a much stronger attraction for electrons than does the hydrogen atom with a single proton. greater probability of finding the shared electrons near the oxygen atom than near the hydrogen atom.

4 As a result: oxygen end of the molecule has a slight negative charge 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.

5 (-) Water Molecule (+) (+)

6 Hydrogen Bonds Because of their partial positive and negative charges polar molecules can attract each other.

7 attraction between hydrogen atoms on one molecule oxygen atom on another water molecule not as strong as covalent or ionic bonds.

8 One water molecule may be involved up to four hydrogen bonds at a time. responsible for many of its special properties.

9 Hydrogen bonds form between water molecules.

10 Cohesion attraction between molecules of the same substance. water is extremely cohesive because of hydrogen bonding

11 cohesion causes molecules on the surface of water to be drawn inward why drops of water form beads on a smooth surface. explains why some insects and spiders can walk on a pond's surface.

12 Adhesion an attraction between molecules of different substances. Example: The surface of water in a graduated cylinder dips in the center adhesion between water molecules and glass molecules is stronger than cohesion between water molecules.

13 Adhesion between water and glass causes water to rise in a narrow tube against the force of gravity. This effect is called capillary action.

14 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.

15 Solutions and Suspensions Mixture a material composed of two or more elements or compounds physically mixed not chemically combined.

16 Two types of mixtures can be made with water solutions suspensions

17 Solutions All the components evenly distributed Example: salt water solution Solute - table salt the substance that is dissolved. Solvent Water the substance in which the solute dissolves.

18 When a crystal of table salt is placed in warm water, sodium and chloride ions are attracted to the polar water molecules. Cl - Cl - Na + Na + Water Water

19 Ions break away from the crystal and are surrounded by water molecules. Cl - Na + Cl - Na + Water Water

20 The ions gradually become dispersed in the water, forming a solution. Cl - Na + Cl - Na + Water Water

21 Water's polarity gives it the ability to dissolve both ionic compounds salt polar molecules sugar Water is the greatest solvent on Earth.

22 Suspensions Some materials do not dissolve when placed in water separate into pieces so small that they do not settle out.

23 The movement of water molecules keeps the small particles suspended. Suspensions mixtures of water and non-dissolved material.

24 Some of the most important biological fluids are both solutions and suspensions. Blood mostly water Contains:» many dissolved compounds.» cells and other un-dissolved particles remain in suspension in the blood.

25 Acids, Bases, and ph What are acidic solutions? What are basic solutions?

26 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.

27 The ph scale scale to indicate the concentration of H + ions in solution. ranges from 0 to 14.

28 The ph Scale At a ph of 7 concentration of H + ions and OH - ions is equal. Pure water has a ph of 7. Sea water Human blood Pure water Milk Normal rainfall

29 The ph Scale ph below 7 Acidic they have more H + ions than OH - ions. The lower the ph, the greater the acidity. Acid rain Tomato juice Stomach acids Lemon juice

30 The ph Scale ph above 7 basic have more OH - ions than H + ions. Oven cleaner Bleach Ammonia solution Soap The higher the ph, the more basic the solution.

31 Acids any compound that forms H + ions in solution. contain higher concentrations of H + ions than pure water have ph values below 7.

32 Strong acids tend to have ph values that range from 1 to 3. Example: hydrochloric acid produced by the stomach

33 Bases compound that produces hydroxide ions (OH - ions) in solution. Basic same as alkaline contain lower concentrations of H + ions than pure water have ph values above 7.

34 Strong bases tend to have ph values ranging from 11 to 14. Lye NaOH Caustic soda Used in making soap, oven cleaner drain cleaners etc.

35 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.

36 Controlling ph is important for maintaining homeostasis. One of the ways that the body controls ph is through dissolved compounds called buffers. Buffers weak acids or bases can react with strong acids or bases prevent sharp, sudden changes in ph.

38 1. A molecule in which the charges are unevenly distributed is called a A. polar molecule. B. cohesive molecule. C. hydrogen molecule. D. covalent molecule.

39 2. A dissolved substance is called a A. solvent. B. solution. C. solute. D. Suspension.

40 3. A compound that produces hydroxide ions in solution is called a(an) A. base. B. buffer. C. acid. D. salt.

41 4. 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.

42 5. 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.

43 END OF SECTION

2-2 Properties of Water. Copyright Pearson Prentice Hall

2-2 Properties of Water. Copyright Pearson Prentice Hall 2-2 Properties of Water Water Water is the most important molecule on earth. Because of its unique shape and chemical behavior it easily bonds with other molecules, and itself. Water: Covalent Bond Water