2. Water- A Necessity to Life Chapter 3 – Campbell Reece Tamara Lookabaugh Moore High School AP Biology Lecture

3. Structure of Water Where are the electrons? What kind of bond is this molecule making? What kind of bonding does is make with other water molecules? H H Oxygen

4. Water is the solvent of life Polarity makes H 2 O a good solvent –polar H 2 O molecules surround + & – ions –solvents dissolve solutes creating solutions

5. How does H 2 O get to top of trees? Transpiration built on cohesion & adhesion

6. Water Polar~ opposite ends, opposite charges Cohesion~ H+ bonds holding molecules together Adhesion~ H+ bonds holding molecules to another substance Surface tension~ measurement of the difficulty to break or stretch the surface of a liquid Specific heat~ amount of heat absorbed or lost to change temperature by 1oC Heat of vaporization~ quantity of heat required to convert 1g from liquid to gas states Density……….

7. Density Less dense as solid than liquid Due to hydrogen bonding Crystalline lattice keeps molecules at a distance

8. Acid/Base & pH Dissociation of water into a hydrogen ion and a hydroxide ion Acid: increases the hydrogen concentration of a solution Base: reduces the hydrogen ion concentration of a solution pH: “power of hydrogen” Buffers: substances that minimize H+ and OH- concentrations (accepts or donates H+ ions)

9. Do you dissolve in water? Hydrophilic –substances have attraction to H 2 O –polar or non-polar?

10. Or don’t you? Hydrophobic –substances that don’t have an attraction to H 2 O –polar or non-polar? fat (triglycerol)

11. Water as a Floating Solid is Unique Most (all?) substances are more dense when they are solid, but Not water… Ice floats! –H bonds form a crystal that actually expands –Think about how water freezes –What does it look like in an ice tray?

12. Ice floats

13. Why is “ice floats” important? Oceans & lakes don’t freeze solid –surface ice insulates water below allowing life to survive the winter –if ice sank…ponds, lakes & even oceans would freeze solid –in summer, only upper few inches would thaw –seasonal turnover of lakes cycles nutrients in autumn

14. Specific heat H 2 O resists changes in temperature –high specific heat –takes a lot to heat it up –takes a lot to cool it down H 2 O moderates temperatures on Earth

15. Specific heat & climate

16. Heat of vaporization Evaporative cooling Organisms rely on heat of vaporization to remove body heat

17. Ionization of water & pH Water ionizes –H + splits off from H 2 O, leaving OH – if [H + ] = [ - OH], water is neutral if [H + ] > [ - OH], water is acidic if [H + ] < [ - OH], water is basic pH scale –how acid or basic solution is –1  7  14 H 2 O  H + + OH –

18. pH Scale 10 –1 H + Ion Concentration Examples of Solutions Stomach acid, Lemon juice 1 pH 10 0 Hydrochloric acid0 10 –2 2 10 –3 Vinegar, cola, beer 3 10 –4 Tomatoes 4 10 –5 Black coffee, Rainwater 5 10 –6 Urine, Saliva 6 10 –7 Pure water, Blood 7 10 –8 Seawater 8 10 –9 Baking soda 9 10 –10 Great Salt Lake 10 10 –11 Household ammonia 11 10 –12 Household bleach 12 10 –13 Oven cleaner 13 10 –14 Sodium hydroxide14

19. 10 0 1 2 3 4 5 6 7 8 9 3 Amount of base added Buffering range 452 pH Buffers & cellular regulation pH of cells must be kept ~7 –pH affects shape of molecules –shape of molecules affect function –pH affects cellular function Control pH by buffers –reservoir of H + donate H+ when [H + ] falls absorb H+ when [H + ] rises