Name ______________________________

Period _______

CHEMISTRY II FINAL EXAM REVIEW

Final Exam: approximately 75 multiple choice questions

x Ch 12: Stoichiometry

x Ch 5 & 6: Electron Configurations & Periodic Properties

x Ch 7 & 8: Bonding

x Ch 14: Gas Laws

x Ch 15, 16, 20: Solutions

x Ch 19: Acids & Bases

x Ch. 18: Kinetics & Equilibrium

On the final exam day, you will need:

x a pencil with a good eraser

x a scientific calculator (know how to use it)

On the final exam day, you will be given:

x a periodic table

x an electronegativity table

Study Tips: 1) Complete the review packet.

2) Find all old tests and quizzes. Read them, study them, and correct mistakes.

3) Read and highlight important topics in your notes.

4) Come see me before the day of the exam if you have a lot of questions

Stoichiometry Know how to perform mole calculations with mole ratios

Limiting reagent calculations

Percent yield calculations

x Know vocabulary: precipitate, salt, metallic oxide, nonmetallic oxide, etc

2. What is “stoichiometry”? ________________________________________________________________

3. If 55.6 grams of calcium carbonate react in excess sodium hydroxide, how many grams of base are made?

RXN: CaCO3 + 2NaOH o Ca(OH)2 + Na2CO3

4. If 56 grams of calcium metal are dropped into hydrochloric acid, how many liters of gas are made?

RXN: Ca + 2HCl o CaCl2

5. When 4.7 x 1011

atoms of sodium are put into excess water, how many grams of base are made?

RXN: 2Na + 2H2O o 2NaOH +H2

6. What is the difference between the limiting reagent and the excess reagent?

_____________________________________________________________________________________

7. What is the limiting reagent when 0.3 grams of nitrogen gas are reacted with 1.2 grams of aluminum?

RXN: N2 + 2Al o 2AlN

8. Find the limiting reagent and the mass of product made when 34 g of oxygen gas react with 27 g

of sodium metal.

RXN: O2 + 4Na o 2Na2O

9. What is the percent yield when 120 grams of sodium nitrate react with barium sulfate to form 3.4 grams

of sodium sulfate?

RXN: 2NaNO3 + BaSO4 o Na2SO4 + Ba(NO3)2

10. Define the following terms:

Limiting Reagent: ___________________________________________________________________

Excess Reagent: ___________________________________________________________________

Actual Yield: ___________________________________________________________________

Theoretical Yield: ___________________________________________________________________

Waves and Electrons

11.What is frequency? _______________________________________________________________________

12. What are the units for frequency? _____________ or _____________

13. What is wavelength? _____________________________ What are the units? ______________

14. What is the frequency of a wave with a wavelength of 3.2 x 10-6

m?

15. What is the wavelength of a wavelength of a wave with a frequency of 3.1 x 1015

sec-1

?

16. If red light has a wavelength of 6.5 x 102 nm, what is the frequency of this red light?

17. What is the energy of a wave with a frequency of 5.75 x 1014

sec-1

?

18. Explain why you saw different colors during the flame test lab: ___________________________________

_________________________________________________________________________________________

19. How many electrons can the 4th

energy level hold? ________ What about the 3rd

energy level? ________

20. What is the maximum number of electrons held by the “p” sublevel? ______       “d” ______ “f” ______

21. What does Hund’s Rule say? _______________________________________________________________

22. What is the Aufbau Principle? ______________________________________________________________

23. What is the Pauli Exclusion Principle? _______________________________________________________

24. Draw the electron configurations (arrows) for the following atoms:

Na Cu

25. Write the electron notation (1s2) for the following atoms:

F Se

26. Use the noble gas shortcut to write the electron notation for the following atoms:

W No

27. List 3 elements that “borrow” with their electrons: _______________, ______________, ______________

28. Define ionization energy

29. Define electronegativity

30. Describe the trend down a column for atomic radius Across a row:

31. Where on the periodic table would you find the elements with the lowest ionization energy?

32. Where on the periodic table would you find the elements with the highest electronegativity?

33. Which elements tend to lose electrons? Gain electrons?

Bonding and Naming Compounds 34. Determine the number of valence electrons in the following atoms:

Mg _______ N _______ Br _______ Ti _______ Cr ________ Al ________ Ag ________

35. Draw the electron dot structure for each of the following:

Aluminum _________ Sulfur _________ Krypton _________ Nitrogen _________

36. Show the ionic bonding for the following:

Sodium to Nitrogen Formula: ____________

Name: ____________________________

Iron(III) to Fluorine Formula: ____________

Name: ____________________________

Aluminum to Oxygen Formula: ____________

Name: ____________________________

37. Bond the following molecules covalently:

CO2 H2S CH2O

38. Draw all of the possible resonance structures for CO32-

:

39. Draw the following molecules in 3D. Determine the shape, bond angles, and polarity.

CBr4 Shape: ________________ AsCl3 Shape: _________________

Bond Angles: __________ Bond Angles: __________

Polar or nonpolar: _______ polar or nonpolar: _____

Strongest intermolecular force: __________ strongest intermolecular force: _________

BF3 Shape: ________________ H2S Shape: _________________ (B is ok with 6e-)

Bond Angles: __________ Bond Angles: __________

Polar or nonpolar: ______ Polar or nonpolar: _____

Strongest intermolecular force: ________ Strongest intermolecular force: _____

40. Describe the three different types of intermolecular forces

41. List the three types of intermolecular forces in order of increasing strength:

Gases and the Gas Laws Know properties of solids, liquids, and gases and the arrangement and movement of atoms

Know Boyle’s, Charles’, Gay-Lussac’s, Combined, and the Ideal Gas Law

Be able to convert pressures and temperatures (memorize conversions)

Be able to perform gas stoichiometry problems

Dalton’s Law of Partial Pressures

42. Describe how solids, liquids, and gases are different at the molecular level.

43. Name the following phase changes:

a. solid to liquid ______________________ b. gas to liquid ______________________

c. liquid to gas ______________________

44. Convert the following pressures and temperatures:

a. 9ºC = _________K b. 309 K = __________ ºC c. 34 atm = ___________ mmHg

d. 2.29 atm = __________kpa

45. What Boyle’s Law say? ________________________________________________________________

What does Charles’s Law say? __________________________________________________________ 

What does Gay-Lussac’s Law say? ______________________________________________________

46. What is the equation for the ideal gas law?

47. If a 4.3 L balloon has a pressure of 1.8 atm, and the volume reduces to 3900 mL, what will the

new pressure be?

48. If a gas cylinder is kept at 24ºC and has a pressure of 768mmHg, what is the new temperature

when the pressure increases to 1.34 atm?

49. If a helium tank is at 25ºC and has a volume of 55 L, what is the new volume if the temperature

increases to 51ºC?

50. If the pressure is 102-kPa at 27oC and a volume of 120-L and the pressure becomes 750-mmHg and the

temperature becomes 22oC , what is the new volume?

51. An 95.6 L balloon has a pressure of 104.1 kPa at 29 oC. What volume will this balloon occupy after

undergoing STP conditions?

52. Find the moles of gas present at 30ºC at 912 mmHg and a volume of 25 liters.

53. How much pressure is there when 2.3 grams of nitrogen gas are at 25ºC and take up 56 liters of space?

54. A gas has a total pressure of 1.8 atm. If gas A has a pressure of 380 mmHg, gas B has a pressure of 0.75

atm, what is the pressure of gas C?

What is the percent composition of each gas from #54?

55. When 250.0-grams of butane gas react with excess oxygen gas, calculate the volume of carbon

dioxide gas produced at 25.0o C and 1.04-atm pressure.

RXN: 2C4H10 + 13 O2 o 8CO2 + 10 H2O

Solutions Know how to perform molarity and dilution calculations

Net ionic equations

Be able to perform solution stoichiometry problems

Know how to determine oxidation numbers and write redox reactions

56. Define the following terms:

Solute: ________________________________________________________________________________

Solvent: _______________________________________________________________________________

57. Calculate the molarity when 4.5 moles of salt are added to 200 mL of water.

58. How many moles are present in a 500 mL of a 0.02 M solution?

59. Define unsaturated, saturated, and supersaturated solutions: ______________________________________ ______________________________________________________________________________________

60. I want to make 400 mL of a 2.5 M solution. How much of a 6 M stock solution should I use?

61. Aluminum sulfate reacts with strontium nitrate.

Molecular Equation: ____________________________________________________________________

Ionic Equation: ________________________________________________________________________

Net Ionic Equation: _____________________________________________________________________

62. Determine the oxidation number of the element underlined in the compounds below:

a. SO42-

b. Al c. N2O5 d. CrO42-

63. Write out the following for the reaction between Aluminum and silver acetate

Oxidation rxn:

Reduction rxn:

Redox rxn:

Acid-Base Chemistry and pH Know properties of acids and bases.

Know how to use Kw to switch between [H+] and [OH

-]

Know how to use logarithms to find pH and pOH

Know the relationship between pH and pOH

Understand and be familiar with the pH scale

64. List 3 characteristics of acids: __________________________________________________________

65. List 3 characteristics of bases: ___________________________________________________________

66. If [H+] = 1.3 x 10

-8, what is [OH

-]? _________________ Is this acidic, basic, or neutral? _____________

67. If [H+] = 3.4 x 10

-3, what is pH? _________________ Is this acidic, basic, or neutral? _____________

68. If [OH-] = 2.9 x 10

-11, what is pOH? ________________ Is this acidic, basic, or neutral? _____________

69. Blood has a pH of 7.2. What is [H+]? _______________ Is this acidic, basic, or neutral? _____________

70. If pH = 5.4, what is pOH? _______________ Is this acidic, basic, or neutral? _____________

71. If pOH is 7.8, what is [H+]? _______________ Is this acidic, basic, or neutral? _____________

72. If [OH-] = 5.6 x10

-7, what is pH? _______________ Is this acidic, basic, or neutral? _____________

73. What is the molarity of HBr if 25.0mL is neutralized by 30.0mL of 1.5M KOH?

Kinetics & Equilibrium

74. List and explain 4 factors affecting the rate of a reaction

a.

b.

c.

d.

75. State LeChatelier’s Principle

76. Write the equilibrium constant expression for any reaction

77. Calculate the Keq of the reaction in which 0.50 moles of nitrogen reacts with 0.50moles of oxygen to form

0.020moles of nitrogen monoxide

78. Does the above reaction favor the reactants or products. Explain