NAME



NAME _______________________ CHEMISTRY FINAL REVIEW

DATE _______________________

DIRECTIONS: Go through the review and try to answer as many questions as you can without having to look anything up. Circle/highlight the questions you couldn’t answer right away. This will identify areas that you need to concentrate on for the final. Go through your notes and worksheets to help you answer the rest of the questions.

UNIT 1 - MEASUREMENTS

1. What are significant figures?

2. How do you know how many sig figs should be in a measurement?

3. Count the number of sig figs in the following measurements.

a. 2390 d. 120

b. 0.00987 e. 4,900

c. 0.03056 f. 300

4. Express the following values in 4 sig figs.

a. 56 d. 0.087

b. 87,566 e. 1,999,999

c. 8.09449 f. 0.0063821

UNIT 2 – MATTER

5. What is matter?

6. What are the two forms of matter? Define.

7. What are the two types of mixtures? Define.

8. Give examples of the two types of mixtures.

9. What are the two types of Pure Substances? Define.

10. Give examples of the two types of Pure Substances.

11. What is an atom?

12. What is a molecule?

13. What is a chemical property? Give two examples.

14. What is a physical property? Give two examples.

15. What is density?

16. What is the density of a liquid that has a mass of 50.340 g and a volume of 300.00 mL?

17. What is an intensive physical property? Give two examples.

18. What is an extensive physical property? Give two examples.

UNIT 3 – THE ATOM

19. What are the three subatomic particles that make up an atom?

20. Where are the three subatomic particles located in an atom?

21. What are the charges of the three subatomic particles?

22. What are the masses of the three subatomic particles?

23. What is the atomic number of an atom?

24. List the atomic number for the following elements.

a. Manganese d. Barium

b. Silver e. Uranium

c. Carbon f. Rutherfordium

25. What is the mass number of an atom?

26. List the number of protons and neutrons for the following atoms.

a. Germanium – 73 d. Oxygen – 17

b. Bromine – 80 e. Nickel – 58

c. Calcium – 40 f. Mercury – 200

27. What is an ion?

28. How does an atom become an ion?

29. What are the two types of ions and how are they different?

30. List the number of electrons in the following ions.

a. Fe+3 d. K+1

b. S-2 e. I -1

c. As-3 f. Pb+4

UNIT 4 – THE ELECTRON

31. What is Quantum Mechanics?

32. What are the letters that designate the 4 Quantum Numbers?

33. What does each Quantum Number tell you?

34. What is Pauli’s Exclusion Principle?

35. What is Electron Configuration?

36. Write out the full Electron Configuration of the following elements.

a. Chromium

b. Lead

c. Europium

37. Write the shortcut Electron Configuration for the following elements.

a. Molybdenum

b. Sulfur

c. Iridium

38. What are Orbital Diagrams?

39. Draw the Orbital Diagrams for the following elements.

a. Titanium

b. Tungsten

c. Rubidium

40. What is a Valence Energy Level?

41. What are Valence Electrons?

42. Determine the Valence Energy Level and the number of Valence Electrons for the following elements.

a. Calcium d. Cadmium

b. Silicon e. Neon

c. Bismuth f. Carbon

43. What are Electron Dot Diagrams?

44. Draw the Electron Dot Diagrams for the following elements.

a. Manganese

b. Berkelium

c. Sodium

d. Nickel

e. Iodine

f. Aluminum

45. What makes an atom stable? What (general) rule tells us this?

46. How does the type of element determine the charge something will take?

47. Determine the charge that the following elements will take to become stable.

a. Li d. Ca

b. N e. F

c. Si f. Al

UNIT 5 – THE PERIODIC TABLE

48. What is the purpose of the Periodic Table?

49. What are the 3 types of elements?

50. Where on the PT are these elements located?

51. What are the vertical columns on the PT called?

52. What are the horizontal rows on the PT called?

53. What is a family?

54. List the 5 metallic families and their location on the PT.

55. List the 2 nonmetallic families on the PT.

56. What is a trend on the PT? Why is it useful?

57. What is Electronegativity?

58. What is the trend of EN on the PT?

59. What is Ionization Energy?

60. What is the trend of IE on the PT?

61. What is atomic radius?

62. What is the trend of atomic radius on the PT?

63. How is ionic radius different from atomic radius? Be specific.

UNIT 6 – FORMULAS AND NAMES

64. What is an ionic compound?

65. What is a molecular compound?

66. How do you determine the formula of a compound?

67. Which ion is written in the formula first?

68. What is a polyatomic ion?

69. List the prefixes for numbers 1-10.

1 – 6 –

2 – 7 –

3 – 8 –

4 – 9 –

5 – 10 –

70. Determine the formula of the following compounds. (Remember, you must first determine if the compound is molecular or ionic!)

a. Magnesium Chloride l. Hydrogen Nitrite

b. Iron (III) Sulfide m. Beryllium Chloride

c. Barium Nitrate n. Manganese (V) Selenide

d. Dihydrogen Monoxide o. Lead (IV) Sulfite

e. Sodium Sulfate p. Tetracarbon Hexaiodide

f. Aluminum Fluoride q. Silver Carbonate

g. Lithium Permanganate r. Pentasulfur Octafluoride

h. Ammonium Bromide s. Chromium (III) Acetate

i. Rubidium Oxide t. Hydrogen Monobromide

j. Copper (II) Phosphate u. Vanadium (I) Nitride

k. Calcium Chloride v. Gallium Oxide

71. Write the name of the following compounds. (Remember, you must first determine if the compound is molecular or ionic.)

a. SrCl2 l. CdO

b. NiS m. K3PO3

c. PBr5 n. NaF

d. Ba(NO3)2 o. CrSe

e. Mg3(PO4)2 p. FeCO3

f. BI3 q. Al(NO2)3

g. Zr(C2H3O2)2 r. SrO

h. H2S s. PtBr2

i. K2Se t. Be3N2

j. CaF2 u. ZnI2

k. NH4Cl v. PbS2

UNIT 7 – REACTIONS & EQUATIONS

72. What is a reaction? What actually occurs in a reaction?

73. What are the two parts in a reaction?

74. What is the name of the written form of a reaction?

75. Why do chemical equations need to be balanced? What law dictates this?

76. What is the name of the number that is used to balance chemical equations?

77. What are the five types of reactions?

78. Label the type of reaction and then balance the following chemical equations.

a. ________ Al + O2 → Al2O3

b. ________ CaBr2 + H3PO4 ( HBr + Ca3(PO4)2

c. ________ C4H8 + O2 ( CO2 + H2O

d. ________ KNO3 + FeCl3 ( KCl + Fe(NO3)3

e. ________ MgS + LiHCO3 ( Li2S + Mg(HCO3)2

f. ________ KMnO4 + SrSO4 ( K2SO4 + Sr(MnO4)2

g. ________ Ca + F2 ( CaF2

h. ________ KHCO3 → H2O + CO2 + K2CO3

i. ________ GaBr3 + F2 → GaF3 + Br2

j. ________ CuSO4 + Fe(C2H3O2)3 → Cu(C2H3O2)2 + Fe2(SO4)3

k. ________ H2SO4 + FeCl2 → HCl + FeSO4

l. _________ KOH + AgNO3 → AgOH + KNO3

m. _________ SrCO3 + H3PO4 → H2CO3 + Sr3(PO4)2

n. _________ C3H6 + O2 → H2O + CO2

UNIT 8 – THE MOLE

79. What does the word “mole” mean?

80. What is Avogadro’s number?

81. What is molar mass? (*This is also called formula mass.)

82. What is a conversion factor?

83. Determine the number of moles that is equal to the following masses given. (Remember, to first find the molar mass of the compound and “dump” the unit you don’t want anymore!) *For extra names help – try to name the following compounds in the margin.

a. 100g of BaCl2

b. 35g of (NH4)3PO4

c. 750g of MgS

d. 0.821g of BF3

e. 11.6g of Na2CO3

f. 68g of Al2(SO4)3

g. 275g of NaCl

h. 147g of HBr

84. Determine the mass that is equal to the following number of moles given. (Remember, to first find the molar mass of the compound and “dump” the unit you don’t want anymore!) *For extra names help – try to name the following compounds in the margin.

a. 2.16 moles of SrF2

b. 0.91 moles of C6H12O6

c. 4.33 moles of CuS

d. 10 moles of AlI3

e. 1.67 moles of KNO3

f. 5.00 moles of Fe(MnO4)3

g. 0.075 moles of LiOH

h. 8.55 moles of HgCl2

85. Convert the following quantities to volume.

a. 0.0750 moles Ar

b. 8.317 g SO2

c. 3.86 x 1022 molecules H2O

86. What is percent composition?

87. Determine the percent composition of each element in the following compounds.

a. (NH4)3PO4

b. NiCl2

c. BaCl2 · 3 H2O

88. What is a hydrate?

89. Determine the percent composition of water in the following hydrates.

a. K3PO4 · 6 H2O

b. Mg(ClO3)2 · 4 H2O

c. Na2SO4 · 2 H2O

90. What is the purpose of heating a hydrate?

91. What is an empirical formula?

92. Determine the empirical formula of the unknown compound from the percent composition given.

a. 62.6 % Tin and 37.4% Chlorine

b. 15.27% Magnesium, 44.53% Chlorine, and 40.20% Oxygen

c. A sample of an unknown compound was determined to have 15.875 g of Silver, 2.063 g of Nitrogen, and 7.063 g of Oxygen.

93. What is a molecular formula?

94. Determine the molecular formulas of the unknown compound based on the information given.

a. An unknown compound with a molar mass of 166.22 g has a percent composition of 47.05% Potassium, 14.45% Carbon, and 38.50% Oxygen.

b. An unknown compound was experimentally determined to contain 45.293g Carbon, 7.622 g Hydrogen, and 60.345g Oxygen. The molar mass of the compound is 180.18g.

UNIT 9 – STOICHIOMETRY

95. What does stoichiometry allow you to calculate?

96. What is molar ratio?

97. Determine the number of moles of ALL the other reactants and products in the following chemical reactions using the number of moles of the one substance given in the equation. (These are 1-step problems!)

a. 1.5 moles of HBr 3 CaBr2 + 2 H3PO4 ( 6 HBr + Ca3(PO4)2

b. 2.2 moles CO2 C4H8 + 6 O2 ( 4 CO2 + 4 H2O

c. 0.75 moles of Al 4 Al + 3 O2 ( 2 Al2O3

d. 3.9 moles of FeCl3 3 KNO3 + FeCl3 ( 3 KCl + Fe(NO3)3

98. Determine the masses of ALL the other reactants and products in the following chemical reactions using the mass of the one substance given in the equation. (These are tricky problems! Think about why you were given two amounts of reactants.)

a. 200.0 g C3H6 and 200.0 g of O2 2 C3H6 + 9 O2 → 6 H2O + 6 CO2

b. 45.9 g CuSO4 and 67.3 g of Fe(C2H3O2)3

3 CuSO4 + 2 Fe(C2H3O2)3 → 3 Cu(C2H3O2)2 + Fe2(SO4)3

c. 0.82 g GaBr3 and 1.0 g of F2 2 GaBr3 + 3 F2 → 2 GaF3 + 3 Br2

d. 25 g KHCO3 2 KHCO3 → H2O + CO2 + K2CO3

UNIT 10 – BONDING

1. What is a bond?

2. What are the 3 main categories of bonds? What is the difference?

3. What are the 2 types of covalent bonds? What is the difference?

4. What is a double bond? Triple bond?

5. What is the VSEPR Theory? Explain.

6. What are the 5 basic shapes formed by molecules with only bonds surrounding the center atom? (No unbonded electrons)

7. What are the shapes formed when there are unbonded pairs of electrons around the center atom?

8. Determine the shape formed by the following molecules.

a. SeF6

b. ClF3

c. AsF5

d. NH3

e. BF3

f. H2O

g. SiBr4

9. What is resonance?

UNIT 11 – GASES

Henry’s Law – The amount of a gas that can dissolve in a liquid varies directly with the partial pressure of the gas. So if pressure increases, so does solubility.

10. What does Boyle’s Law state? Its formula? What 2 factors must be held constant for this law to be true?

11. What does Charles’ Law state? Its formula? What 2 factors must be held constant for this law to be true?

12. What does the Combined Gas Law state? Its formula? What factor must be held constant for this law to be true?

13. What is the Ideal Gas Law? Its formula?

14. What is R? What is its value?

15. What unit does temperature have to be measured in to solve any gas law problem?

16. How do you convert degrees Celsius into the unit from #15?

17. Solve the following problems using the best Gas Law. Remember that standard temperature is 0(C and standard pressure is 1 atm, 101 kPa, 760 mm Hg or 760 torr.

a. Oxygen gas kept at 45.00(C has a pressure of 105.0 kPa. The pressure is decreased to 90.00 kPa. What temperature will allow this to happen?

b. What was the original pressure of Sulfur gas at 35.00(C and 590.0 cm3 when it is now in a 500.0 cm3 container with a pressure of 680.0 mm Hg and at 25.00(C?

c. What was the original volume of Hydrogen gas at 15(C if it is now at 23(C and

in a 2.0 L container?

d. What is the original pressure of a gas in a 1.10 L container if its new volume is

1.35 L with a pressure of 1.05 atm?

e. What is the new volume of Chlorine gas at STP when it was in a 2.5 L container

with a pressure of 720 torr at 33(C?

UNIT 12 – SOLIDS & LIQUIDS

18. Explain the difference between solids, liquids and gases in terms of molecular spacing?

19. Explain the difference between solids, liquids and gases in terms of Kinetic Energy and IMF?

20. What is Heat of Fusion? Heat of Vaporization?

21. Why does the temperature of a substance remain the same during a phase change?

22. What is a crystal?

23. What is a unit cell?

24. What is evaporation? How does evaporation occur?

UNIT 13 – IMF

25. What is IMF?

26. What is the importance of the IMF?

27. What are the three types of IMF?

28. Which is the strongest form of IMF? Why?

29. Which is the weakest form of IMF? Why?

30. What is a dipole?

31. What is a momentary dipole?

UNIT 14 – SOLUTIONS

32. What is a solution?

33. What are the 2 parts to a solution?

34. What is the difference between the 2 parts in #33?

35. What is solubility?

36. What are the three descriptions of solutions with respect to solubility?

37. How do you know if a solution is saturated?

38. What types of substances dissolve in each other?

39. What is a solution with water as the solvent?

40. What is molarity? What is the formula for molarity?

41. What is the molarity of a 5.0 L solution that contains 2.0 moles of K2CO3?

42. How many moles of solute are there in 0.500 L of a 1.28 M NaNO3 solution?

43. How many liters of solution will contain 1.5 moles of CaCl2 if the solution is 6.0 M CaCl2?

UNIT 15 – ACIDS & BASES

44. What is an acid?

45. What is a base?

46. What are the properties of acids? Bases?

47. What is a neutral substance?

48. What is the difference between weak acids and bases and strong acids and bases?

49. List the strong acids.

50. List the strong bases.

51. What is a conjugate acid/base pair?

52. What is a neutralization reaction? What are the products?

53. If the pH of a solution is 3.55, what is the pOH, [H3O+1], and [OH-1] of the solution?

54. What is the Keq (or Ka) expression for HC2H3O2?

UNIT 16 – REACTION RATES

Some reactions occur in several steps. Each step may occur at a different rate. The reaction can only go as fast as its slowest step. This step is called the “rate-determining step”.

55. What is the rate of reaction?

56. How does a reaction occur?

57. What is an activated complex?

58. What can increase the rate of reaction?

59. What is used to slow down the rate of reaction?

60. How does a catalyst speed up a reaction?

61. What is equilibrium?

62. State Le Chatelier’s Principle.

63. What factors affect equilibrium?

64. What is the equilibrium expression for the following reaction? 2 Mg + O2 ( 2 MgO

65. Fill in the following table for the following reaction.

CH4 (g) + 2 O2 (g) + 35 kcal ↔ CO2 (g) + 2 H2O (l)

|If… |Equilibrium Shift |[CH4] |[O2] |[CO2] |[H2O] |

|Then… | | | | | |

|[O2] ↑ | | | | | |

|[CH4] ↑ | | | | | |

|[CO2] ↑ | | | | | |

|[H2O] ↓ | | | | | |

|Pressure ↓ | | | | | |

|Temp ↓ | | | | | |

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