2. Properties of Water 2.2

3. Why Water? -Water regulates the temperature of plants and transports nutrients through them.

4. Water Water Water Polar Molecule: has uneven distribution of electrons giving it a positive and a negative end Partially due to the size differences between oxygen and hydrogen. Oxygen will take on a slight negative charge and hydrogen will take on a slight positive charge

5. “The Universal Solvent” Water’s polar nature makes it very effective in dissolving other substances, including ionic compounds into ions

6. Forms Hydrogen Bonds Holds 2 H 2 O molecules together Results in Cohesion=attractive force between like particles ex: surface tension Can result in Adhesion=attraction on unlike substances Ex: capillarity-ability for water molecules to move against gravity (think blood or plants)

7. Surface Tension Why do they “float”?

8. Specific Heat Water needs to lose or gain high amounts of energy to break bonds and change phases How could this be helpful to organisms? Keeps cells at even temperatures during environmental changes!!!

10. Solutions and Suspensions Solution: all components evenly distributed EX: Saltwater Salt is the SOLUTE Water is the SOLVENT Suspension: mixture of water and non dissolved particles EX: Blood (water and cells), Fog, Muddy Water, Paint, Flour in water

11. Acids, Bases, and Buffers Acid: makes H+ ions in solution pH- below 7 The lower the number, the stronger the acid fruit juice, acetic acid (vinegar), HCl, battery acid Base: makes OH- ions in solution pH- above 7 The higher the number, the stronger the base Seawater, ammonia, bleach, oven cleaner, lye Buffers: weak acids/bases that can react with strong acids/bases to prevent major pH changes

12. Acids and Bases Review pH Scale: indicates the concentration of H + ions in solution 0  14 0-6.9 = ACID 7 = Neutral 7.1-14 = BASE