2. Water Chemistry and its Impact on Life Processes By Mrs.Gilani

3. Essential Questions What are the 7 properties of water? Why is water essential to life?

8. Water  More than 60% of the human body is made from water.  Water covers more than 70% of the Earth’s surface.  It is the only substance on Earth that occurs naturally in 3 phases; solid, liquid, and gas.

9. Properties of Water  Cohesion  Adhesion  High Specific Heat  High Heat of Vaporization  Less Dense as a Solid  Universal solvent

10. Polar and Nonpolar  Covalent bonds can be polar or nonpolar depending on the molecule’s electronegativity.  Electronegativity is a measure of an atom's attraction for electrons in the covalent bond. The atom with the higher electronegativity will attract the shared electrons stronger than the other atom can. For the electrons to be nonpolar covalent, both of the electrons have the same tendency to attract the bonding pair of electrons.

11. Water  Water is a polar molecule.  Due to the fact that Oxygen is bigger and has a stronger positive charge in its nucleus than the hydrogen atom, the O doesn’t share the electrons equally with the H atoms.  The unequal sharing causes one side of the water molecule to have a slightly negative charge, and the other to have a slightly positive charge.  This creates an electrically polar structure.

14. Water  A water molecule (H 2 O), is made up of three atoms --- one oxygen and two hydrogen. H H O

15. Water is Polar  In each water molecule, the oxygen atom attracts more than its "fair share" of electrons  The oxygen end “acts” negative  The hydrogen end “acts” positive  Causes the water to be POLAR

16. Hydrogen Bonds Exist Between Water Molecules  One hydrogen bond is weak, but many hydrogen bonds are strong

17. Interaction Between Water Molecules Negative Oxygen end of one water molecule is attracted to the Positive Hydrogen end of another water molecule to form a HYDROGEN BOND

18. Cohesion  Attraction between particles of the same substance ( why water is attracted to itself)  As a result of hydrogen bonding, water molecules stick together.  Results in Surface tension (a measure of the strength of water’s surface)  Produces a surface film on water that allows insects to walk on the surface of water

19. Cohesion … Helps insects walk across water

20. Adhesion  Attraction between two different substances.  Water will make hydrogen bonds with other surfaces such as glass, soil, plant tissues, and cotton.  Capillary action-water molecules will “tow” each other along when in a thin glass tube.  Example: transpiration process which plants and trees remove water from the soil, and paper towels soak up water.

22. Adhesion Causes Capillary Action Which gives water the ability to “climb” structures

23. Adhesion Also Causes Water to … Form spheres & hold onto plant leaves Attach to a silken spider web

25. High Specific Heat  Why does the ocean water stay warm much longer?  It is due to the fact of water’s high specific heat.  It takes a lot of energy to increase its temperature.  It takes all summer and a blazing sun to increase the ocean’s temperature by just a few degrees.

26. High Specific Heat  Water’s ability to resist temperature change is one of the factors that keep the temperatures in our oceans fairly stable.  This is also the reason that humans are able to keep a normal constant body temperature of 98.6 degrees Fahrenheit.

27. Water is Less Dense as a Solid  Ice is less dense as a solid than as a liquid (ice floats)  Liquid water has hydrogen bonds that are constantly being broken and reformed.  Frozen water forms a crystal-like lattice whereby molecules are set at fixed distances.

28. Water is Less Dense as a Solid Which is ice and which is water?Which is ice and which is water?

29. Water is Less Dense as a Solid WaterIce

30. High Heat of Vaporization  Amount of energy to convert 1g of a substance from a liquid to a gas  In order for water to evaporate, hydrogen bonds must be broken.  As water evaporates, it removes a lot of heat with it (cooling effect).

31.  Water vapor forms a kind of global ‘‘blanket” which helps to keep the Earth warm.  Heat radiated from the sun warmed surface of the earth is absorbed and held absorbed and held by the vapor. by the vapor.

32. Universal Solvent  Water’s polarity causes it to act as a universal solvent.  It can dissolve many kinds of substances.

33. Homeostasis  Ability to maintain a steady state despite changing conditions  Water is important to this process because: a. Makes a good insulator b. Resists temperature change c. Universal solvent d. Coolant e. Ice protects against temperature extremes (insulates frozen lakes)

34. Solutions  In a solution, all the components are distributed evenly.  In salt water solution, table salt is the solute.  Water is the solvent, the substances in which the solute dissolves.

35. Solution

36. Mixture  A mixture is a material composed of 2 or more elements or compounds that are physically mixed together but not chemically combined.

37. Compound  A compound of 2 or more different atoms.  A chemical formula describes a compound.  Ex. H 2 O; 2 Hydrogen & 1 Oxygen

38. Acids, Bases, and pH Scales  A compound that releases hydrogen ions (H+) is called an Acid.  A compound that releases hydroxide ions (OH-) is called a Base.

39. The pH Scale  Indicates the concentration of H + ions  Ranges from 0 – 14  pH of 7 is neutral  pH 0 up to 7 is acid … H +  pH above 7 – 14 is basic… OH -  Each pH unit represents a factor of 10X change in concentration  pH 3 is 10 x 10 x 10 (1000) stronger than a pH of 6

40. Acids  Strong Acids have a pH of 1-3  Produce lots of H + ions

41. Buffers  Weak acids or bases that react with strong acids or bases to prevent sharp, sudden changes in pH (neutralization).  Produced naturally by the body to maintain homeostasis Weak Acid Weak Base

42.  H+ ion concentration and pH relate inversely. OH- ion concentration and pH relate directly.

44.  Most H+ ions: pH = 4; or pH = 5.  Most H+ ions: pH = 4; or pH = 5.  Most OH- ions: pH = 10; or pH = 13.  Most OH- ions: pH = 10; or pH = 13.  Least H+ ions: pH = 12; or pH = 13.  Least H+ ions: pH = 12; or pH = 13.  Least OH- ions: pH = 8; or pH = 9.