2. Matter- anything that takes up space and has mass Energy- the ability to do work Kinetic (energy in motion) Potential (stored)

3. Chemical- ATP  ADP + P i (glycolysis) Mechanical- muscles moving, producing heat, digestion Electrical- charges particles Na + /K +, Ca ++, nerve and muscle Radiant (electromagnetic)- energy that travels in waves (visible, UV, IR)  Retina, light  skin  vitamin D

4. Maintaining Homeostasis Reproduction, Development & Growth Movement

5. .. Periodic Table 112 known elements Pure substances that cannot be broken down into simpler chemical entities by ordinary chemical reactions

7. An element is composed of atoms (0.1-1 nm in diameter) Atom  cluster of small particles (proton, neutron, electron)

8. Protons (p + ) Electrons (e - ) Neutrons (n o )

9. proton neutron electron hydrogen atom helium atom carbon atom 1p, 0n, 1e-2p, 2n, 2e- 6p, 6n, 6e-

10. atomic number: number of p; #p = #e- 2 He  2e- and 2p He

11. atomic mass (atomic wt.) : sum of masses of p+n He  2p + 2n, atomic mass = 4 4 2 He He p + ne-

12. p = n = e- = Atomic number = Atomic mass = C Carbon Atom

13. O16O17O18 stable isotopes Atoms that differ in the number of neutrons 16 8 O 18 8 O 17 8 O #p #p+n O

14. Cause cancer Destroy cancerous cells Medical imaging Half-life: C-14= 5600 yrs I-131= 8 days SPECT Kidney function heart function

15. Two or more atoms held together by chemical bonds OxygenO 2 NitrogenN 2 AmmoniaNH 3 Carbon DioxideCO 2 WaterH 2 O MethaneCH 4 GlucoseC 6 H 12 O 6

16. Carbohydrates: C 6 H 12 O 6 (glucose) Lipids: C 3 H 8 O 3 (glycerol) + 3C 16 H 32 O 2 (fatty acids) Proteins: COOH-NH 2 Nucleic Acids: sugar, PO 4, N 2 containing base CHON, PS

17. Binding two or more different kinds of elements together NaCl CH 4 C 6 H 12 O 6

18. An atom that has either gained or lost electrons such that it exhibits a net charge Na + (cation) Cl - (anion)

19. Sodium (Na) Atom 11 P + 12 N o

20. Sodium (Na + ) Ion 11 P + 12 N o

21. Chlorine (Cl) Atom 17 P + 18 N o

22. Chloride (Cl - ) Ion 17 P + 18 N o

23. HydrogenH + PotassiumK + FluorideF - CalciumCa +2 MagnesiumMg +2 HydroxideOH -HydroxideOH - BicarbonateHCO 3 -BicarbonateHCO 3 - NitrateNO 3 -NitrateNO 3 - PhosphatePO 4 -3PhosphatePO 4 -3

24. Ionic Covalent Hydrogen

25. Transfer of electron 17 P + 18 N o 11 P + 12 N o

26. electron sharing O H H

27. Between Water Molecules Covalent bond Hydrogen bond

29. A  B reactant  product

30. A + B  AB

31. AB  A + B

32. AB + CD  AC + BD

33. H 2 O  H + + OH -

34. Exergonic- a spontaneous chemical reaction where there is a net release of free energy Endergonic- A nonspontaneous chemical reaction where energy is absorbed from the surroundings

35. C 6 H 12 O 6 + 6O 2  6CO 2 + 6H 2 O + energy ATP  ADP + P i + energy

36. 6CO 2 + 6H 2 O + energy  C 6 H 12 O 6 + 6O 2 ADP + P i + energy  ATP

38. ATP  ADP + P i + energy

39. ADP + P i  ATP H2OH2OH2OH2O

40. Boiling Point: 100 o C Freezing Point: 0 o C Density: 1g/cm 3 gasliquid solid

41. 1.High heat capacity-very resistant to temp change; the ocean helps control the temp of the Earth (water heats slower than land) 2.High heat of vaporization- amount of heat needed to make water boil; a lot of energy is needed to break H 2 bonds 3.High Surface tension- cohesion of water molecules (ex. water striders) 4. Polarity solvent properties - universal solvent; H 2 O + NaCl Na + + Cl -

43. HCl  H + + Cl - Proton donor, i.e., they donate H + ions HCl is a strong acid with a pH 1-2

44. Na + + OH -  NaOH NH 3 + H +  NH 4 OH - + H +  H 2 O HCO 3 - +H +  H 2 CO 3 Proton acceptor, i.e., they take up H+ ions NaOH is a strong base ~pH 12

45. Neutralization- HCl + NaOH  H 2 O + NaCl Buffer- resists dramatic changes in pH; ex. tums, rolaids…buffers stomach acid

46. Acidic0-6 Neutral7 Basic (alkaline)8-14 Type of Solution pH Value 0-14

47. Logarithmic scale blood

48. CO 2 + H 2 O ↔ H 2 CO 3 ↔ HCO 3 - + H + ↔ CO 3 2- + 2H + By-product of respiration carbonic acid bicarbonate carbonate The addition of CO 2 makes blood acidic

49. Blood too basic: H 2 CO 3 HCO 3 - + H + pH drops Blood too acidic: HCO 3 - + H + H 2 CO 3 pH rises Blood ave. pH = 7.4

50. Inquiry 1.How many neutrons in 7 N? 2.Of the following pH’s which is most acidic? 3762 3. The symbols K, Na, C, and S are: 4. Which of the following are elements? water; sugar; table salt; the atmosphere 5. Which of the following are pure substances? wine; seawater; blood; iron 14