CHEMISTRY II FINAL EXAM REVIEW
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1 Name Period CHEMISTRY II FINAL EXAM REVIEW Final Exam: approximately 75 multiple choice questions Ch 12: Stoichiometry Ch 5 & 6: Electron Configurations & Periodic Properties Ch 7 & 8: Bonding Ch 14: Gas Laws Ch 15, 16, 20: Solutions Ch 19: Acids & Bases Ch. 18: Kinetics & Equilibrium On the final exam day, you will need: a pencil with a good eraser a scientific calculator (know how to use it) On the final exam day, you will be given: a periodic table 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
2 Stoichiometry Know how to perform mole calculations with mole ratios Limiting reagent calculations Percent yield calculations 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: CaCO 3 + 2NaOH Ca(OH) 2 + Na 2 CO 3 4. If 56 grams of calcium metal are dropped into hydrochloric acid, how many liters of gas are made? RXN: Ca + 2HCl CaCl 2 5. When 4.7 x atoms of sodium are put into excess water, how many grams of base are made? RXN: 2Na + 2H 2 O 2NaOH +H 2 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: N 2 + 2Al 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: O 2 + 4Na 2Na 2 O
3 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: 2NaNO 3 + BaSO 4 Na 2 SO 4 + Ba(NO 3 ) 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 sec -1? 16. If red light has a wavelength of 6.5 x 10 2 nm, what is the frequency of this red light? 17. What is the energy of a wave with a frequency of 5.75 x sec -1? 18. Explain why you saw different colors during the flame test lab: 19. How many electrons can the 4 th energy level hold? What about the 3 rd energy level? 20. What is the maximum number of electrons held by the p sublevel? d f 21. What does Hund s Rule say?
4 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 (1s 2 ) 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:
5 Iron(III) to Fluorine Aluminum to Oxygen Formula: Name: Formula: Name: 37. Bond the following molecules covalently: CO 2 H 2 S CH 2 O 38. Draw all of the possible resonance structures for CO 3 2- : 39. Draw the following molecules in 3D. Determine the shape, bond angles, and polarity. CBr 4 Shape: AsCl 3 Shape: Bond Angles: Polar or nonpolar: Strongest intermolecular force: Bond Angles: polar or nonpolar: strongest intermolecular force: BF 3 Shape: H 2 S Shape: (B is ok with 6e-) Bond Angles: Bond Angles: Polar or nonpolar: Strongest intermolecular force: Polar or nonpolar: 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
6 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 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 27 o C and a volume of 120-L and the pressure becomes 750-mmHg and the temperature becomes 22 o C, what is the new volume? 51. An 95.6 L balloon has a pressure of kpa at 29 o C. 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.
7 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 grams of butane gas react with excess oxygen gas, calculate the volume of carbon dioxide gas produced at 25.0 o C and 1.04-atm pressure. RXN: 2C 4 H O 2 8CO H 2 O 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?
8 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. SO 4 2- b. Al c. N 2 O 5 d. CrO 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 K w 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?
9 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 K eq 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
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