1. The Chemistry of Life Properties of Water

2. The Water Molecule Neutral Charge –All Molecules Are Neutral

3. The Water Molecule PolarityPolarity –A water molecule is polar because there is an uneven distribution of electrons between the oxygen and hydrogen atoms. (+) (—)

4. Hydrogen Bonds Polar water molecules act like magnets and attract each otherPolar water molecules act like magnets and attract each other Hydrogen BondsHydrogen Bonds –The attraction of the Hydrogen end (+) of one molecule for the Oxygen end (-) of another water molecule. –They are the strongest bonds that can form between molecules

5. Hydrogen Bonds

6. Cohesion The attraction between molecules of the same substance (e.g. water). Allows some insects and spiders to walk on water.

7. Adhesion Attraction between molecules of different substancesAttraction between molecules of different substances Responsible for Capillary forces in plantsResponsible for Capillary forces in plants

8. Solutions & Suspensions Water is usually part of a mixture.Water is usually part of a mixture. There are two types of mixtures:There are two types of mixtures: –Solutions –Suspensions

9. Solution Ionic compounds disperse as ions in waterIonic compounds disperse as ions in water Evenly distributedEvenly distributed SOLUTESOLUTE –Substance that is being dissolved SOLVENTSOLVENT –Substance into which the solute dissolves

10. Solution

11. Suspensions Substances that don’t dissolve but separate into tiny pieces.Substances that don’t dissolve but separate into tiny pieces. Water keeps the pieces suspended so they don’t settle out.Water keeps the pieces suspended so they don’t settle out.

12. Acids, Bases & pH 1 water molecule in 550 million naturally dissociates into a Hydrogen Ion and a Hydroxide Ion1 water molecule in 550 million naturally dissociates into a Hydrogen Ion and a Hydroxide Ion Hydrogen Ion Hydroxide Ion Acid Base Acid Base H 2 O  H + + OH -

13. The pH Scale Indicates the concentration of H + ions Ranges from 0 – 14 pH of 7 is neutral pH 0 – 6.99 is acid … H + pH 7.01 – 14 is basic… OH - Each pH unit represents a factor of 10 change in concentration

14. Acids Strong Acid = pH 1-3 H + ions

15. Bases Strong Base = pH 11 – 14 OH - ions

16. Buffers Weak acids or bases that react with strong acids or bases to prevent sharp, sudden changes in pH.Weak acids or bases that react with strong acids or bases to prevent sharp, sudden changes in pH. Weak Acid Weak Base