1. INORGANIC CHEMISTRY EVERYTHING IS MADE OF ELEMENTS

2. ELEMENTS 92 NATURALLY OCCURRING HYDROGEN LIGHTEST URANIUM HEAVIEST

3. BIG SIX ELEMENTS OXYGEN CARBON HYDROGEN NITROGEN CALCIUM PHOSPHORUS

4. ATOMS SMALLEST PARTICLES OF ELEMENTS PROTONS –UNCHARGED PARTICLES ELECTRONS –NEGATIVELY CHARGED PARTICLES NEUTRONS –POSITIVELY CHARGED PARTICLES

5. Protons and neutrons are in the nucleus. Electrons move around the nucleus. The Study of Atoms Figure 2.1

6. ATOMIC NUMBER NUMBER OF PROTONS IN NUCLEUS

7. ATOMIC MASS PROTONS + NEUTRONS EQUAL MASS

8. ISOTOPES OF AN ELEMENT ARE ATOMS WITH DIFFERENT NUMBERS OF NEUTRONS. ISOTOPES OF OXYGEN ARE: EACH CHEMICAL ELEMENT HAS A DIFFERENT NUMBER OF PROTONS. ISOTOPES

10. ELECTRONS ARE ARRANGED IN ELECTRON SHELLS CORRESPONDING TO DIFFERENT ENERGY LEVELS

13. OCTET RULE ATOMS ARE MOST STABLE WHEN THEIR OUTERMOST SHELLS ARE FILLED WITH 2 ELECTRONS THE FIRST FEW ELEMENTS & 8 ELECTRONS FOR THE LARGER ATOMS

17. CHEMICAL COMPOUNDS

18. CHEMICAL FORMULAS DESCRIBE COMPOSITION AND STRUCTURE OF ELEMENTS AND COMPOUNDS

19. STRUCTURAL ISOMERS SAME CHEMICAL FORMULA DIFFERENT ARRANGEMENTS

20. CHEMICAL EQUATIONS REACTANTS ON THE LEFT PRODUCTS ON THE RIGHT

21. NOBLE GASES INERT ATOMS TEND TO LOSE OR GAIN ELECTRONS TO FILL THEIR OUTER SHELLS

22. ATOMS FORM MOLECULES ATOMS COMBINE TO COMPLETE THE OUTERMOST SHELL THE NUMBER OF MISSING OR EXTRA ELECTRONS IN THIS SHELL IS THE VALENCE COMBINE IN FIXED RATIOS

23. A compound contains different kinds of atoms. The forces holding atoms in a compound are chemical bonds. How Atoms Form Molecules: Chemical Bonds

24. CHEMICAL BONDS IONIC COVALENT

25. The number of protons and electrons is equal in an atom. Ions are atoms that have gained or lost electrons and are charged. How Atoms Form Molecules: Chemical Bonds Figure 2.2a

26. Covalent bonds form when two atoms share one or more pairs of electrons. Covalent Bonds Figure 2.3a

30. POLAR COVALENT BONDS

31. Hydrogen bonds form when a hydrogen atom covalently bonded to an O or N atom in another molecule. Hydrogen Bonds Figure 2.4

32. Ionic bonds are attractions between ions of opposite charge. One atom loses electrons and another gains electrons. Ionic Bonds Figure 2.2b

33. CHEMICAL REACTIONS INVOLVE THE MAKING OR BREAKING OF BONDS BETWEEN ATOMS. A CHANGE IN CHEMICAL ENERGY OCCURS DURING A CHEMICAL REACTION. ENDERGONIC REACTIONS ABSORB ENERGY. EXERGONIC REACTIONS RELEASE ENERGY. CHEMICAL REACTIONS

34. METABOLIC CHEMICAL REACTIONS ARE REVERSIBLE USUALLY LITTLE FREE DIFFERENCE BETWEEN REACTANTS AND PRODUCTS THIS MEANS AS LONG AS EXTERNAL ENERGY IS AVAILABLE MOST REACTINS IN LIVING CELLS ARE THEORETICALLY REVERSIBLE –ALLOWS CELLS TO CONTROL RELEASE OF FREE ENERGY –ALLOWS CELLS TO RESYNTHESIZE BIOLOGICAL MOLECULES

35. THE DIRECTION OF A REVERSIBLE REACTION WILL DEPEND ON: – THE CONCENTRATIONS OF THE CHEMICALS –THEIR ENERGY RELATIONSHIPS –THEIR SOLUBILITY

36. TYPES OF CHEMICAL REACTIONS SYNTHESIS REACTIONS DECOMPOSITION REACTIONS EXCHANGE REACTIONS REVERSIBLE REACTIONS

37. Occur when atoms, ions, or molecules combine to form new, larger molecules Anabolism is the synthesis of molecules in a cell. Synthesis Reactions

38. Occur when a molecule is split into smaller molecules, ions, or atoms. Catabolism is the decomposition reactions in a cell. Decomposition Reactions

39. Are part synthesis and part decomposition. Exchange Reactions

40. Can readily go in either direction. Each direction may need special conditions. Reversible Reactions

41. REDOX REACTIONS REDOX REACTIONS: PAIRED OXIDATION AND REDUCTION REACTIONS OXIDATION: LOSS OF ELECTRONS REDUCTION: GAIN IN ELECTRONS ORGANIC MOLECULES LOSE HYDROGEN ATOMS RATHER THAN JUST ELECTRONS

42. METABOLISM ALL THE REACTIONS THAT OCCUR IN THE CELL

43. WATER THE REASON WHY LIFE CAN SURVIVE HERE ON EARTH

44. PROPERTIES OF WATER POLAR MOLECULE EXCELLENT SOLVENT COHESIVE ADHESIVE TENDS TO MAINTAIN A STABLE TEMPERATURE HIGH SPECIFIC HEAT

45. WATER IS A POLAR MOLECULE

46. EACH WATER MOLECULE FORM FOR A MAXIMUM OF FOUR HYDROGEN BONDS

47. Solvent –Polar substances dissociate, forming solutes WATER AS A SOLVENT

48. WATER AND CAPILLARY ACTION ADHESIVE AND COHESIVE QUALITIES

49. Hydrogen bonding between water molecules makes water a temperature buffer. WATER AS A TEMPERATURE BUFFER Figure 2.4b

50. HEAT OF VAPORIZATION IT TAKE 540 CALORIES TO CHANGE ONE GRAM OF LIQUID WATER INTO ONE GRAM OF WATER VAPOR

51. HEAT OF FUSION WATER LOSES 80 CALORIES PER GRAM AS IT TURNS TO ICE

52. WATER BECOMES LESS DENSE AS IT FREEZES REACHES MAXIMUM DENSITY AT 4 DEGREES C EXPANDS AGAIN AS TEMPERATURE EXPANDS THIS IS WHY LAKES AND POOLS FREEZE FROM SURFACE DOWN & ICE FLOATS

54. ALL CHEMICAL REACTIONS IN THE CELLS AND EXTRACELLULAR FLUIDS TAKE PLACE IN SOLUTION H + AND OH  PARTICIPATE IN CHEMICAL REACTIONS Water

55. An acid is a substance that dissociates into one or more H +. HCl  H + + Cl  ACIDS Figure 2.6a

56. A base is a substance that dissociates into one or more OH . NaOH  Na + + OH  BASES Figure 2.6b

57. A salt is a substance that dissociates into cations and anions, neither of which is H + or OH . NaCl  Na + + Cl  SALTS Figure 2.6c

58. DISSOLUTION OF SALTS

59. IMPORTANCE OF SALTS SOURCE OF MINERAL IONS ESSENTIAL FOR: –FLUID BALANCE –ACID-BASE BALANCE –NERVE AND MUSCLE FUNCTION –BLOOD CLOTTING –BONE FORMATION –ETC

60. The amount of H + in a solution is expressed as pH. pH =  log[H + ] Increasing [H + ], increases acidity. Increasing [OH  ] increases alkalinity. Most organisms grow best between pH 6.5 and 8.5. Acid-Base Balance

61. BUFFERS OPERATE TO MAINTAIN APPROPRIATE pH levels WEAK ACID, WEAK BASE AND THE SALT OF THE ACID AND BASE

62. SODIUM BICARBONATE- CARBONIC ACID BUFFER SYSTEM COMMON BUFFERING SYSTEM

63. Figure 2.7