1. Chem Fall Final Review1 Chemistry Fall Semester Review

2. Chem Fall Final Review2 Test Format 95 multiple choice95 multiple choice Each question holds the equal weightEach question holds the equal weight Scantron (pencil)Scantron (pencil) ~104 minutes~104 minutes

3. Chem Fall Final Review3 Final Schedule 1/13: Per. 61/13: Per. 6 1/14: Per. 1 and 71/14: Per. 1 and 7 1/15: Per. 2 and 31/15: Per. 2 and 3 1/16: Per. 4 and 51/16: Per. 4 and 5

4. Chem Fall Final Review4 Recommendations Study old review sheetsStudy old review sheets Study your ionsStudy your ions Know your shapes!Know your shapes! Time you math problemsTime you math problems

5. Chem Fall Final Review5 Review of the Units: Unit 1: Scientific Method and the Metric System

6. Chem Fall Final Review6 Review of the Units: Unit 2: Matter, density, chemical and physical properties, atomic theory and the mole

7. Chem Fall Final Review7 Review of the Units: Unit 3: Structure of the atom, quantum theory, atomic models and electron configurations

8. Chem Fall Final Review8 Review of the Units: Unit 3: Also, periodic law and properties

9. Chem Fall Final Review9 Review of the Units: Unit 4: Types of chemical bonds, molecular geometry and resonance

10. Chem Fall Final Review10 Review of the Units: Unit 5: Naming! Molar mass, oxidation numbers, and polyatomic ions…

11. Chem Fall Final Review11 Review of the Units: Unit 5: Also, percent composition, empirical formula and molecular formula

12. Chem Fall Final Review12 Review of the Units: Unit 6: Reactions. Clues of rxns. Balancing equations. Types of reactions.

13. Chem Fall Final Review13 Review of the Units: Unit 6: Also, predicting products

14. Chem Fall Final Review14 Review of the Units: Unit 7: Stoichiometry, Percent yield, and limiting reactants

15. Chem Fall Final Review15 Unit 1

16. Chem Fall Final Review16 Unit 1 Know the scientific method Know the scientific method

17. Chem Fall Final Review17 Unit 1 Problem, hypothesis, experiment, observations, law, theory Problem, hypothesis, experiment, observations, law, theory

18. Chem Fall Final Review18 Unit 1 Scientists solve problems by using the scientific method Scientists solve problems by using the scientific method

19. Chem Fall Final Review19 Unit 1 Hypotheses are tested with experiments. Can become theories. Hypotheses are tested with experiments. Can become theories.

20. Chem Fall Final Review20 Unit 1 Theories explain observations made over long periods of time. Theories explain observations made over long periods of time.

21. Chem Fall Final Review21 Unit 1 Laws are used to summarize observed behavior Laws are used to summarize observed behavior Law of conservation of mass Law of conservation of mass

22. Chem Fall Final Review22 Unit 1 Observations can be quantitative (data) or qualitative (descriptions) Observations can be quantitative (data) or qualitative (descriptions)

23. Chem Fall Final Review23 Unit 1 All measurements are made with accuracy and maximum precision All measurements are made with accuracy and maximum precision Significant figures Significant figures

24. Chem Fall Final Review24 Unit 1 Significant figures: all certain plus one uncertain digit Significant figures: all certain plus one uncertain digit

25. Chem Fall Final Review25 Unit 1 The metric system is based on prefixes The metric system is based on prefixes

26. Chem Fall Final Review26 Unit 1 kilo- L kilo- L hecto- hecto- deka- deka- Base (m, L, g) Base (m, L, g) deci- deci- centi- centi- milli- R milli- R

27. Chem Fall Final Review27 Unit 1 Convert 54.6 mg  g Convert 54.6 mg  g Answer: divide 54.6 by 1000 = 0.0546 g Answer: divide 54.6 by 1000 = 0.0546 g

28. Chem Fall Final Review28 Unit 1 Temperature measure average kinetic energy of a substance Temperature measure average kinetic energy of a substance Fahrenheit, Celsius, Kelvin Fahrenheit, Celsius, Kelvin

29. Chem Fall Final Review29 Unit 1 Kelvin is the “absolute” temperature scale Kelvin is the “absolute” temperature scale

30. Chem Fall Final Review30 Unit 1 K  o C: K – 273 K  o C: K – 273 o C  K: o C + 273 o C  K: o C + 273 o C  o F: ( o C x 1.80) + 32 o C  o F: ( o C x 1.80) + 32 o F  o C: ( o F – 32) / 1.80 o F  o C: ( o F – 32) / 1.80

31. Chem Fall Final Review31 Unit 1 Convert 140 K  o C Convert 140 K  o C Answer: - 133 K Answer: - 133 K

32. Chem Fall Final Review32 Unit 2

33. Chem Fall Final Review33 Unit 2 Sig fig in calculations Sig fig in calculations Lesser number in mult / div Lesser number in mult / div Line up numbers in add / subtraction Line up numbers in add / subtraction

34. Chem Fall Final Review34 Unit 2 Find the area of volume of a box: L=10.0 cm, w=2.5 cm, h=5.60 cm Find the area of volume of a box: L=10.0 cm, w=2.5 cm, h=5.60 cm Answer: 140 cm 3 Answer: 140 cm 3

35. Chem Fall Final Review35 Unit 2 Physical properties: substance stays the same Physical properties: substance stays the same Chemical: reactivity! Chemical: reactivity!

36. Chem Fall Final Review36 Unit 2 Atoms, compounds and mixtures Atoms, compounds and mixtures Atoms cannot be separated Atoms cannot be separated

37. Chem Fall Final Review37 Unit 2 Compounds can be separated by chemical means; mixtures by physical means Compounds can be separated by chemical means; mixtures by physical means

38. Chem Fall Final Review38 Unit 2 Hetero- vs. homogeneous mixtures Hetero- vs. homogeneous mixtures Heterogeneous can be separated by filtration Heterogeneous can be separated by filtration What about homo-? What about homo-?

39. Chem Fall Final Review39 Unit 2 Know about Democritus, Dalton, Thomson, Rutherford and Mendeleev Know about Democritus, Dalton, Thomson, Rutherford and Mendeleev

40. Chem Fall Final Review40 Unit 2 Dalton’s atomic theory is not entirely accepted today. (1 st atomic theory) Dalton’s atomic theory is not entirely accepted today. (1 st atomic theory) Why not? Why not?

41. Chem Fall Final Review41 Unit 2 Thomson: CRT (electron) Thomson: CRT (electron) Rutherford: Au foil (nucleus) Rutherford: Au foil (nucleus) Mendeleev: first periodic table Mendeleev: first periodic table

42. Chem Fall Final Review42 Unit 2 Modern periodic: arranged by increasing atomic number Modern periodic: arranged by increasing atomic number

43. Chem Fall Final Review43 Unit 2 Atomic # = # of p Atomic # = # of p Atomic mass = # of p + n in the nucleus Atomic mass = # of p + n in the nucleus # of electrons = atomic # (if not an ion) # of electrons = atomic # (if not an ion)

44. Chem Fall Final Review44 Unit 2 How many electrons in an atom of N with a mass # of 15? How many electrons in an atom of N with a mass # of 15? Answer: 7 Answer: 7

45. Chem Fall Final Review45 Unit 2 Isotopes: same # p, diff’t # n Isotopes: same # p, diff’t # n Isomers: same formula, diff’t shape Isomers: same formula, diff’t shape

46. Chem Fall Final Review46 Unit 2 Change g  moles Change g  moles Divide by the molar mass Divide by the molar mass Change moles  g Change moles  g Mult. by the molar mass Mult. by the molar mass

47. Chem Fall Final Review47 Unit 2 How many moles in 25.0 grams of Fe? How many moles in 25.0 grams of Fe? Answer: 0.448 mol Answer: 0.448 mol

48. Chem Fall Final Review48 Unit 2 How many moles in 25.0 grams of NaNO 3 ? How many moles in 25.0 grams of NaNO 3 ? Answer: 0.294 mol Answer: 0.294 mol

49. Chem Fall Final Review49 Unit 2 Which sample has more atoms? 10 g of Ag or 10 g of Au? Which sample has more atoms? 10 g of Ag or 10 g of Au? Answer: Ag Answer: Ag

50. Chem Fall Final Review50 Unit 3

51. Chem Fall Final Review51 Unit 3 Wave theory of light Wave theory of light C = λ ν C = λ ν E = hν E = hν Higher frequencies = higher energies Higher frequencies = higher energies

52. Chem Fall Final Review52 Unit 3 Photons are released when electrons return to their ground state Photons are released when electrons return to their ground state (red, yellow, blue) (red, yellow, blue)

53. Chem Fall Final Review53 Unit 3 Bohr: used quantum theory to describe electron orbits Bohr: used quantum theory to describe electron orbits Schrödinger: used wave mechanics to describe electron orbitals Schrödinger: used wave mechanics to describe electron orbitals

54. Chem Fall Final Review54 Unit 3 Orbitals: probability maps Orbitals: probability maps Electron configurations: based on quantum numbers Electron configurations: based on quantum numbers

55. Chem Fall Final Review55 Unit 3 Orbital shapes: s, p, d, f Orbital shapes: s, p, d, f Aufbau, Pauli, Hunds Aufbau, Pauli, Hunds Know the rules! Know the rules!

56. Chem Fall Final Review56 Unit 3 Look for the incorrect configuration Look for the incorrect configuration 3 types of configurations 3 types of configurations [Noble] [Noble]

57. Chem Fall Final Review57 Unit 3 Elements “want” to have noble gas configurations Elements “want” to have noble gas configurations How many electrons are needed by N to achieve a noble gas config? How many electrons are needed by N to achieve a noble gas config? Ans: 3 Ans: 3

58. Chem Fall Final Review58 Unit 3 Which element has the configuration of 1s 2 2s 2 2p 6 3s 2 3p 5 ? Which element has the configuration of 1s 2 2s 2 2p 6 3s 2 3p 5 ? Ans: Chlorine Ans: Chlorine

59. Chem Fall Final Review59 Unit 3 Periodic properties… Periodic properties… Electronegativity Electronegativity Ionization energy Ionization energy Atomic radii Atomic radii Ionic radii Ionic radii

60. Chem Fall Final Review60 Unit 3 Which type of elements have higher electronegativities? Which type of elements have higher electronegativities? Ans: non-metals Ans: non-metals

61. Chem Fall Final Review61 Unit 3 Know the “families” Know the “families” Grouped by similar chemical characteristics Grouped by similar chemical characteristics Due to valence electrons Due to valence electrons

62. Chem Fall Final Review62 Unit 4

63. Chem Fall Final Review63 Unit 4 Three types of bonds Three types of bonds Ionic: metals + non- metals Ionic: metals + non- metals Covalent: 2 non-metals Covalent: 2 non-metals

64. Chem Fall Final Review64 Unit 4 Shapes! Bent, linear, trigonal pyramidal… Shapes! Bent, linear, trigonal pyramidal… Shape of CO 2 Shape of CO 2 Ans: Linear Ans: Linear

65. Chem Fall Final Review65 Unit 4 Bond angles: linear, bent, tetrahedral Bond angles: linear, bent, tetrahedral

66. Chem Fall Final Review66 Unit 4 Resonance!!! Resonance!!!

67. Chem Fall Final Review67 Unit 5

68. Chem Fall Final Review68 Unit 5 Naming… Naming… Type I: (Grp. 1&2 metals + non-metal) Type I: (Grp. 1&2 metals + non-metal) Type II: Other metals + non-metal Type II: Other metals + non-metal

69. Chem Fall Final Review69 Unit 5 Oxidation states: Oxidation states: Al +3, Zn +2, Ag +1 Al +3, Zn +2, Ag +1

70. Chem Fall Final Review70 Unit 5 Naming… Naming… Type III: 2 non-metals (use prefixes—bi-, tri-, tetra-) Type III: 2 non-metals (use prefixes—bi-, tri-, tetra-)

71. Chem Fall Final Review71 Unit 5 Naming… Naming… Polyatomic ions Polyatomic ions

72. Chem Fall Final Review72 Unit 5 Name these: Name these: CO 2, NaNO 3, CuN CO 2, NaNO 3, CuN Formulas? Formulas? Iron(II)oxide, sodium oxide

73. Chem Fall Final Review73 Unit 5 Empirical formula: Empirical formula: %  g  mol  ratios  E.F. Molecular formula Molecular formula molar mass / emp. mass = ratio (n)

74. Chem Fall Final Review74 Unit 6

75. Chem Fall Final Review75 Unit 6 Balancing equations Balancing equations Reactants  products Reactants  products Number of atoms must be the same on each side of the equation Number of atoms must be the same on each side of the equation

76. Chem Fall Final Review76 Unit 6 Expect to balance several equations Expect to balance several equations

77. Chem Fall Final Review77 Unit 6 CH 4 (g) + O 2 (g)  CO 2 (g) + H 2 O (g) CH 4 (g) + O 2 (g)  CO 2 (g) + H 2 O (g) When the above equation is balanced, what is the coefficient of oxygen?

78. Chem Fall Final Review78 Unit 6 CH 4 (g) + 2 O 2 (g)  CO 2 (g) + 2 H 2 O (g) CH 4 (g) + 2 O 2 (g)  CO 2 (g) + 2 H 2 O (g) When the above equation is balanced, what is the coefficient of oxygen?

79. Chem Fall Final Review79 Unit 6 Types of reactions: synthesis, decomposition, single replacement, double replacement, combustion Types of reactions: synthesis, decomposition, single replacement, double replacement, combustion

80. Chem Fall Final Review80 Unit 6 In PPT rxns: solids form In PPT rxns: solids form Spectator ions remain dissolved Spectator ions remain dissolved

81. Chem Fall Final Review81 Unit 7

82. Chem Fall Final Review82 Unit 7 Stoichiometry Stoichiometry Balance eq.  grams to moles  ratios  moles to grams Balance eq.  grams to moles  ratios  moles to grams

83. Chem Fall Final Review83 Unit 7 CH 4 (g) + 2 O 2 (g)  CO 2 (g) + 2 H 2 O (g) CH 4 (g) + 2 O 2 (g)  CO 2 (g) + 2 H 2 O (g) If 2.0 moles of methane react with excess oxygen, how many moles of water will be produced?

84. Chem Fall Final Review84 Unit 7 CH 4 (g) + 2 O 2 (g)  CO 2 (g) + 2 H 2 O (g) CH 4 (g) + 2 O 2 (g)  CO 2 (g) + 2 H 2 O (g) Ans: 4.0 moles

85. Chem Fall Final Review85 Unit 7 Expect to perform several stoichiometric calculations Expect to perform several stoichiometric calculations

86. Chem Fall Final Review86 Unit 7 Limiting reactants Limiting reactants Have vs. need Have vs. need

87. Chem Fall Final Review87 Unit 7 Percent Yield: Percent Yield: Actual Actual ----------------- x 100% ----------------- x 100% Theoretical Theoretical

88. Chem Fall Final Review88 The End Don’t forget to write your version on your scantron Don’t forget to write your version on your scantron Good Luck! Good Luck!