2. Basic Chemistry Water Chemistry

3. Atoms – 1 X 10 -11 Each atom is made up of a ‘nucleus’ and ‘orbits’ or ‘shells’ outside the nucleus Nucleus: Protons = + charged Neutrons = neutral/ no charge Orbits: Electrons = - charged Periodic Table: A chart of elements that have been discovered

4. What makes each atom different, i.e. a unique element??? Atomic number The number of protons in nucleus Electrons (-) will always equal protons (+) Atomic mass –The number of protons + neutrons in the nucleus

5. Molecules = atoms bonded together = chemical bonds = represents ENERGY wATERwATER METHANEMETHANE

6. Ionic Bonds – between atoms that want to give and take electrons! “Happy” atoms = outer e- shells filled! 1. 2 e- fill first shell 1s What atom is this? 2. 8 e- fill second shell 1s 2s 2p What atom is this? 3. 8 e- fill third shell ? Q: Na and Cl … what would make them

7. Covalent Bonds = electrons shared CARBON Most common atom involved in covalent bonding ½ filled outer shell (4 e-) CH 4 Methane gas

8. Compounds NaCl – Sodium Chloride - inorganic - ionic bonding - a salt C 6 H 12 O 6 - Glucose - organic - covalent bonding - a sugar

9. Water Molecule: 2 Hydrogen and 1 Oxygen atom bonded

10. H 2 0 - WATER Oxygen side is slightly negative (-) charged Hydrogen side is slightly positively charged (+) Positive ends Negative end HH O “a polar-covalent molecule”

11. CAUSE and EFFECT - Because of the ‘polarity’ of water molecules, they attract each other like magnets In this way, water molecules “stick together” – cohesion + - - + + +

12. Proof of the Cohesive nature of H 2 O … -Certain insects can “walk on water” -Cohesion between molecules of water creates a strong surface tension - benefits insects like the water strider

13. Adhesion - the tendency of two DIFFERENT substances sticking together Examples: 1. water molecules “sticking” to glass 2. capillary action

14. Capillary Action - example of adhesion - water molecules adhere to the inside of tubules that fill the stems of plants - water molecules are “drawn up” from the soil toward the top of the tree by the pull of adhesion

15. Perspective: the size of “A” water molecule –A molecule of water is so small that there are millions of molecules in a single drop of water. –About 60 million water molecules could be stretched side by side across a penny.

16. Water is the ONLY compound that commonly exists in all 3 phases (solid, liquid, gas) on earth there would be no life on earth without water.

17. WATER … the Universal Solvent In a SOLUTION, - the solvent is the substance that does the dissolving ( usually a liquid) - the solute is the substance that is dissolved (usually a solid) - so many substances are soluble in water that it is therefore called the … “universal solvent”

18. WATER … in living cells - is the SOLVENT of our cells’ cytoplasm - dissolves the SOLUTES: carbs, lipids, proteins

19. 3 types of environments living cells encounter ISOTONIC environment Equal amounts of solvent and solute molecules inside and outside of cells HYPERTONIC environment –Greater % of solute molecules in sol’n outside the cell to inside HYPOTONIC –Less % of solute molecules in the sol’n outside the cell to inside

20. In Solutions … … water molecules disassociate into 1. H + ions and 2. OH- ions

21. THE pH Scale - a scale that measures the concentration of H+ ions in the solution compared to OH- ions 1.An acidic solution (pH range 0 – 6.9) - a high concentration of H+ ions - ( Infer: a low concentration of OH- ions ) Sulfuric acid H 2 SO 4 Citric Acid HC 6 H 7 O 7

22. 2. An alkaline solution - pH range 7.1 – 14 (also known as ‘bases’) - a low concentration of H+ ions compared to OH - ions Sodium Hydroxide NaOH Calcium carbonate CaCO 3 Sodium Bicarbonate NaHCO 3

23. The pH scale ranges from 0 to 14 The pH of pure water is 7 = equal amounts of H+ and OH- ions

24. Water Chemistry Terms A. Hydrolysis - a chemical reaction where water molecules are used to break up a large compound into smaller ones B. Dehydration Synthesis - a chemical reaction where water molecules are taken away from smaller molecules in order to form a larger compound.

25. Water Chemistry Terms C. Hydrophobic -substances that will not dissolve in water - Ex. fats, oils, soaps … “non-polar ” substances D. Hydrophilic - substances that will dissolve in water -Ex. sugar, salt, tea, protein powder - “polar” substances - “LIKE DISSOLVES LIKE”

26. Water’s Uniqueness A. For most substances, their solid form is more dense than the liquid form B. But for water the solid form is less dense than the liquid form. Proof: Ice floats on water!

27. WHY is ice less dense than water/steam? water as a solid -the molecules “line up” -geometrically organized molecules water as a liquid or gas - molecules are random, in constant motion -very close together

28. Pond Temperatures

29. VII. Water: Public Health Issues A. Open Sewers - Before the invention of sewer systems, human and animal waste was collected in open water ways. - How many of the earth’s 6 billion people still live with these open sewers?

30. ANALYZE: Open Sewer Consequences -breeds disease – why? -contaminates drinking water – how? -Hurricane Katrina “undid” the sanitation system … how?