Final Exam Review Questions PDF

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Final review questions with lecture slide references....

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The final for this class won’t be written by Dr. Statler so it would probably be something that covers the general vicinity of chemistry. The questions here will mostly be pulled off of slides or test questions. I’m not sure how helpful this will be. For the most part, this is more like a practice test (sort of) rather than a practice study guide, although each question has questions related to it attached to it. Also, you should probably study topics that aren’t covered in these questions as well. The last 12 questions are questions from topics that were covered after midterm 3. Finally, the second has a “rough” outline of the equation sheet, sort of. It might not look like that specifically but it’s a rough sketch.

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Questions 1) Which of the following is accurate but not precise?

a.

b.

c.

Practice: Unit 1 - Foundations slide (know precision vs accuracy)

d.

e.

2) A concise verbal statement or mathematical equation that summarizes a broad variety of observations and experiences is called a(n) __________. a. Law b. Theory c. Hypothesis d. Experiment e. Test Practice: Unit 1 - extra practice #3-8 3) Which of the following process is a chemical change? a. Adding food coloring to water b. Freezing water in the refrigerator c. Mixing salt and pepper into yolk d. Fruit molding e. Heating of food in a microwave Practice: Unit 1 - extra practice #26 - 33 4) Which famous experiment led to the discovery of the atomic nucleus? a. Rutherford b. Millikan c. Thomsan d. Avogadro e. Dalton Practice: Unit 1 - slides, (know, relatively, what experiment each person was famous for) 5) Osmium has a density of 22.6 g/cm3. What is the mass of a block with the dimensions 1.01 x 0.233 x 0.648 cm? a. 6.75 x 10-3 b. 3.45 c. 148 d. 6.75 x 103

e. 34.5 Practice: Unit 1 - extra practice algorithmic questions #12 - 13 6) Which isotope has 36 electrons in the atom?

a.

80 Kr 36 80

b.

35 Br

c.

78 Se 34

d.

34 Cl 17

e.

36 Hg 80

Practice: Know how chemical notations work

7) Which pair of atoms constitutes a pair of isotopes of the same element?

a.

14 6 Z

14 7 Z

b.

14 6 Z

14 6 Z

c.

17 9 Z

17 8 Z

d.

19 10 Z

19 9 Z

e.

20 Z 10

21 11 Z

Practice: Know how chemical notations work 8) There are _________ molecules of methane in 0.123 mol of methane (CH4) a. 5 b. 2.46 x 102 c. 2.04 x 1025 d. 7.40 x 1022 e. 0.615 Practice: Conversions from Unit 1 9) Which group in the periodic table contains only nonmetals? a. 1A b. 6A c. 2B d. 2A e. 8A Practice: Know periods and groups are on the periodic table 10) Given the equation:

n n 2 (¿¿ f 2)❑ 1 1 − , 2❑ (¿¿ f 1 )❑ ❑ ¿ RE ¿ Δ E=¿

R E=−2.18 ×10

−18

An hydrogen atom emits light with a wavelength of 486 nm. Which electron transition corresponds with this action? Note: this is the second longest wavelength emission of visible light corresponding with the hydrogen atom in the Balmer series a. n = 4 to n = 3 b. n = 4 to n = 2 c. n = 4 to n = 1 d. n = 3 to n = 1 e. n = 3 to n = 2 Practice: Unit 2 - Ch 7 Extra practice questions #71 - 79 11) A photon that has an energy of 4.38 x 10-18 J has a wavelength that is similar to which of the following? a. Highly energized photons from a uranium bomb test b. Photons emitted by the human body c. Photons used in old radios d. Looking at a painting e. Photons used to check what’s inside luggage at airports Practice: Unit 2 - Ch 7 Extra practice questions #1 - 31 12) What is the frequency (s-1) of electromagnetic radiation with a wavelength of 0.53 m? a. 5.7 x 108 b. 1.8 x 10-9 c. 1.6 x 108 d. 1.3 x 10-33 e. 1.3 x 1033 Practice: Unit 2 - Ch 7 Extra practice questions #1 - 31 13) Which of the following people is associated with the fact that atoms can be both waves and particles? a. De Brolige b. Einstein c. Schrodinger d. Heisenberg e. Plank Practice: know, relatively, what experiment each person was famous for 14) Which one of the following represents an acceptable set of quantum numbers for an

electron in an atom? (order of n, l, ml, and ms) a. 2,2,-1,-1/2 b. 1,0,0,1/2 c. 3,3,3,1/2 d. 4,5,-5,1/2 e. 3,3,3,1 Practice: Unit 2 - Ch 7 Extra practice questions #46 - 70 15) In which of the orbitals does a phosphorus atom experience the greatest shielding? a. 2p b. 3s c. 3p d. 2s e. 1s Practice: Unit 2 - Ch 7 Extra practice questions #46 - 70 16) The 4d subshell in the ground state of atomic xeon contains _________ electrons. a. 2 b. 6 c. 8 d. 10 e. 36 Practice: Unit 2 - Ch 7 Extra practice questions #46 - 70 17) [Ar]4s23d104p3 is the electron configuration of which atom? a. As b. V c. P d. Sb e. Sn Practice: Unit 2 - Ch 8 Extra practice questions #13 - 24

18) Which of the following violates Hund’s rule?

a.

b.

c.

d.

e. Practice: Unit 2 - Ch 8 Extra practice questions #1 - 9, #87 - 91

19) Which of the following violates the Aufbau principle

a.

b.

c.

d.

e. Practice: Unit 2 - Ch 8 Extra practice questions #1 - 9, #87 - 91 20) Rank the following atoms in atomic size: Mg, Na, P, Si, Ar a. Mg > Na > P > Si > Ar b. Ar > Si > P > Na > Mg c. Si > P > Ar > Na > Mg d. Na > Mg > Si > P > Ar e. Ar > P > Si > Mg > Na Practice: Unit 2 - Ch 8 Extra practice questions #56 - 61 21) Of the following atoms, which has the largest first ionization energy? a. Br b. O c. C d. P e. I Practice: Unit 2 - Ch 8 Extra practice questions #62 - 68 22) Of the following elements, which has the most negative electron affinity? a. S

b. Cl c. Se d. Br e. I Practice: Unit 2 - Ch 8 Extra practice question algorithmic questions # 1 - 10. 23) Which of the following correctly represents the electron affinity of bromine? a. Br (g) → Br + (g) + e b. Br (g) + e - → Br - (g) c. Br2 (g) + e - → Br - (g) d. Br2 (g) + 2e - → 2Br - (g) e. Br + (g) + e - → Br (g) Practice: Unit 2 - Ch 8 Extra practice questions #92-93 24) What is the chemical formula for molybdenum(IV) hypochlorite? a. Mo(ClO3)4 b. Mo(ClO)4 c. Mo(ClO2)4 d. Mo(ClO4)4 e. MoCl4 Practice: Unit 3 - Extra practice questions #19 - 34 25) What is the correct formula of ammonium sulfide? a. NH4SO3 b. (NH4)2SO4 c. (NH4)2S d. NH3S e. N2S3 Practice: Unit 3 - Extra practice questions #19 - 34 26) The naturally occurring and stable isotopes of aluminum are 26Al and 27Al. What would be expected if someone was to place a random sample of naturally occurring stable aluminum in a mass spectrometer? a. A greater amount of 27Al b. A greater amount of 26Al c. Approximately the same amount of 26Al and 27Al d. There is no way to predict the outcome e. More information is needed to predict the outcome Practice: Understand how atomic mass works 27) What is the oxidation number of chromium in Cr2O72a. +3 b. +12 c. +7

d. +6 e. +14 Practice: Unit 8 & 9 Extra practice questions #85 - 89. 28) When the following equation is balanced, the coefficient of H3PO4 is: H3PO4 (aq) + NaOH (aq) → Na3PO4 (aq) + H2O (l) a. 1 b. 2 c. 3 d. 4 e. 0 Practice: Unit 3 Extra practice questions #76-78 29) The electron-domain geometry of a sulfur centered compound is trigonal bipyramidal. The hybridization of the center sulfur atom is: a. sp b. sp2 c. sp3 d. sp3d e. sp3d2 Practice: Bonding Models dynamic study modulos 30) The bond between the nitrogen atoms in HNNH contains a. one σ bond and one π bond b. one σ bond and two π bond c. two σ bond and one π bond d. two σ bond and two π bond e. one σ bond and zero π bond Practice: Bonding Models dynamic study modulos 31) The C-Cl-C bond angle in the CCl2O molecule (C is the central atom) is slightly: a. Greater than 90° b. Less than 109.5° c. Less than 120° d. Greater than 120° e. Greater than 109.5° Practice: Unit 4 Extra practice multiple choice questions (near the bottom) #1 - 41 32) The electron domain geometry and molecular geometry of iodine trichloride are ________ and __________, respectively. a. trigonal bipyramidal, trigonal planar b. tetrahedral, trigonal pyramidal c. trigonal bipyramidal, T-shaped d. octahedral, trigonal planar

e. t-shaped, trigonal planar Practice: Unit 4 Extra practice multiple choice questions (near the bottom) #1 - 41 33) The molecular geometry of the CHF3 molecule is ________, and this molecule is ________. a. trigonal bipyramidal, polar b. tetrahedral, nonpolar c. seesaw, polar d. trigonal planar, nonpolar e. trigonal bipyramidal, polar Practice: Unit 4 Extra practice multiple choice questions (near the bottom) #1 - 41 34) Given these electronegativity values, which covalent bond is most polar? H C N O 2.1 2.5 3.0 3.5 a. C-H b. N-H c. O-H d. O-C e. O-H Practice: Unit 4 Extra practice problems #47 - 59 35) Which of the following has the smallest bond length? a. H-F b. H-Cl c. H-Br d. H-I e. H-At Practice: Unit 4 Extra practice problems #95 - 101 36) In the reaction HNO3 (aq) + CaCO3 (s) → Ca(NO3)2 (aq) + CO2 (g) + H2O (l) which bonds release energy in the process of this reaction? a. N-O b. H-O c. C-O (in CO2) d. Ca-(NO3) e. H-(NO3) Practice: Unit 4 Extra practice problems #104 - 110 37) Rank the following compounds in decreasing melting point: RbI, MgO, NaCl, KCl a. RbI < MgO < NaCl < KCl b. RbI < NaCl < KCl < MgO c. RbI < KCl < NaCl < MgO d. MgO < NaCl < KCl < RbI

e. MgO < KCl < NaCl < RbI Practice: Unit 4 Extra practice problems #23 - 32 38) Given the following molecules, rank them in terms of bond order: NO3-, NO2+ , NH4+, NO a. NO < NH4+ < NO2+ < NO3b. NH4+ < NO2+ < NO3- < NO c. NH4+ < NO3- < NO2+ < NO d. NO < NO2+ < NO3- < NH4+ e. NO3- < NH4+ < NO2+ < NO Practice: Unit 4 Extra practice problems #64 - 81 & know how to calculate bond order 39) Rank the following in terms of increasing ionic characteristics: H-Al, H-B, H-C, H-H a. H-H < H-C < H-B < H-Al b. H-C < H-B < H-H < H-Al c. H-Al < H-H < H-B < H-C d. H-Al < H-B < H-C < H-H e. H-H < H-C < H-B < H-Al Practice: Unit 4 Extra practice problems #47 - 59 40) Determining lattice energy from the Born-Haber cycle requires the use of _______ a. The Octet Rule b. Coulomb’s Law c. Periodic Law d. Hess’s Law e. Avogadro’s Number Practice: Lattice energy trends and overview of the born-haber cycle 41) In the molecule triiodide (I3-), the center I has _______ lone pairs and _______ paired electrons. a. 0, 5 b. 2, 3 c. 1, 4 d. 1, 3 e. 3, 2 Practice: Unit 4 Extra practice problems #64 - 81 42) Which of the following molecules have a net dipole moment of zero but has polar bonds. a. Cl2 b. SnCl2 c. H2S d. CCl4 e. CH3Cl Practice: Unit 4 Extra practice multiple choice questions (near the bottom) #1 - 41

43) When a system__________ΔE is always negative. a. Absorbs heat and does work b. Gives off heat and does work c. Absorbs heat and has work done to it d. Gives off heat hnd has work done to it e. None of the above result in ΔE always being negative Practice: Unit 5 Multiple choice Q #2-5 & #20-23 & Algorithm questions #1, 16-18 44) How many kJ of heat are consumed when 5.74 of CO (g) is formed in the following reaction? CH3OH (l) → CO(g) + 2H2 (g) ΔH = 128.1 a. 23.3 b. 62.0 c. 26.3 d. 162 e. 8.3 Practice: Unit 5 Multiple Choice Q: #38-52, Algorithm question #20-25 45) Given the following reactions, CaCO3 (s) → CaO(s) + CO2 (g) ΔH = 178.1 kJ C (s) + O2 (g) → CO2 (g) ΔH = -393.5 kJ what is the enthalpy of the reaction CaCO3 (s) → CaO (s) + C (s) + O2 (g) a. 215.4 b. 571.6 c. -215.4 d. -571.6 e. 7.01 x 104 Practice: Unit 5 multiple choice #61-64 46) In an internal combustion engine, there are 8 cylinders each with a total volume of 3.2 L. During the engine cycle, each cylinder expands from ½ of its original volume to its full volume at a constant pressure of 45 atm. The work (J) is done by the 1 cylinder during the engine cycle should be _______ and has a magnitude ________. (101.3 J = 1 L·atm) a. Positive, < 100 b. Negative, > 100 c. Positive, > 100 d. Negative, < 100 e. Cannot determine Practice: Understand pressure volume problems in Unit 5 energetics slides 47) For which of the following reactions is the value of ΔH°rxn equal to the ΔH°f of the product? a. H2 (g)+ 1/2O2 (g) → H2O(l) b. H2 (g)+ O2 (g) → H2O2 (l)

c. 2C (s) + 2H2 (g) → C2H4 (g) d. 1/2N2 (g) + O2 (g) → NO2 (g) e. All of the above Practice: Unit 5 multiple choice #69-71 48) Of the following, only _________ is impossible for an ideal gas.

a. b.

c.

d.

e. Practice: Unit 6 #6-17, Algorithmic questions #5-7 49) Of the following gases, ________ will have the fastest effusion rate a. NH3 b. CH4 c. Ar d. HBr e. HCl Practice: Unit 6 #64-76, Algorithmic questions #63 50) Arrange the following gases in increasing root mean square speed at 25°C. Cl2, O2, F2, N2 a. Cl2 < F2 < O2 < N2 b. Cl2 < O2 < F2 < N2 c. N2 < F2 < Cl2 < O2 d. Cl2 < F2 < N2 < O2 e. F2 < O2 < N2 < Cl2 Practice: Unit 6 #64-76, Algorithmic questions #63 51) When gases are treated as real gases, using the van der Waals equations, the actual volume occupied by gas molecules __________the pressure exerted and the attractive forces between gas molecules __________ the pressure exerted, as compared to ideal gas.

a. decreases, increases b. increases, increases c. increases, decreases d. does not affect, decreases e. does not affect, increases Practice: Unit 6 #77-79 52) The density of chlorine gas at 1.21 atm and 34.9°C is _______ g/L. a. 0.0497 b. 0.295 c. 0.423 d. 1.70 e. 3.39 Practice: Unit 6 #31 & 33 53) The total pressure exerted by a mixture of 1.5 g H2 and 5.0 g of N2 in a 5.00 L vessel at 298 K is _________ atm a. 1.06 b. 9.08 c. 4.51 d. 32.4 e. 5.27 Practice: Unit 6 #44-56 54) Which one of the following substances exhibit dipole-dipole attraction between molecules? a. XeF4 b. AsH3 c. CO2 d. BCl3 e. Cl2 Practice: Unit 7 #28-39, #42-49, #56-63 55) Which of the following derivatives of ethane would have the highest boiling point? a. C2Br6 b. C2F6 c. C2I6 d. C2Cl6 e. C2H6 Practice: Unit 7 #28-39, #42-49, #56-63 56) What causes a meniscus to form? a. Viscosity b. The material of the container c. Cohesive and adhesive forces

d. Volume of the liquid e. Amount of hydrogen in the liquid Practice: Unit 7 #28-39, #42-49, #56-63

57) The phase change of B-C and D-E are not associated with a change in temperature because the energy from the heat is used up to a. Increase the distance between molecules b. Break intramolecular bonds c. Increase the viscosity of the molecules d. Increase the velocity of molecules e. Increase the density of the sample Practice: Unit 7 #50-52, #75-86

58) According to the phase diagram, what is the normal boiling point of this liquid (in °C)? a. -3 b. 10 c. 29 d. 38 e. 0 Practice: Unit 7 #87-91 59) What is the empirical formula for a compound that contains 27.0% S, 13.4% O, and 59.6% Cl by mass? a. SOCl b. SOCl2 c. S2OCl d. SO2Cl e. ClSO4 Practice: Dynamic Study Modulo “Mass Percent and Empirical Formulas” 60) FeS and O2 react to form Fe2O3 and SO2. If 294 grams of FeS is allowed to react with 176 grams of O2, how many grams of Fe2O3 are produced? a. 267 b. 534 c. 878 d. 251 e. 201 Practice: Unit 8 & 9 questions #20 - 27 61) Which of the following are weak electrolytes? HCl, HC2H3O2, NH3, KCl a. HCl, KCl b. HCl, HC2H3O2

c. NH3 d. NH3, HC2H3O2 e. HC2H3O2, NH3, KCl Practice: Unit 8 & 9 questions #55 - 61 63) The net ionic equation for the formation of an aqueous solution of Al(NO3)3 via mixing solid Al(OH)3 and aqueous nitric acid is __________. a. Al(OH)3 (s) + 3HNO3 (aq) → 3H3O (l) + Al(NO3)3 (aq) b. Al3+ (aq) + 3OH - (aq) + 3H+ (aq) + NO3- (aq) → 3H2O (l) + Al3+ (aq) + NO3- (aq) c. Al3+ (aq) + 3OH - (aq) + 3H+ (aq) → 3H2O (l) + Al3+ (aq) d. 3H+ + 3OH - (aq) → 3H2O (l) e. Al(OH)3 (s) + 3H+ (aq) → 3H2O (l) + Al3+ (aq) Practice: Unit 8 & 9 questions #73 - 78 64) A combination of which of the following will result in a precipitate? a. NaC2H3O2 (aq) and HCl (aq) b. NaOH (aq) and HCl (aq) c. AgNO3 (aq) and Ca(C2H3O2)2 (aq) d. KOH (aq) and Mg(NO3)2 (aq) e. NaOH (aq) and HCl (aq) Practice: Unit 8 & 9 questions #62 - 72 65) Which species of sulfur has the highest oxidation number? a. S8 b. H2S c. SO2 d. H2SO3 e. K2SO4 Practice: Unit 8 & 9 Extra practice questions #85 - 89. 66) Which of the following is an oxidation-reduction reaction? a. Cu (s) + 2AgNO3 (aq) → 2Ag (s) + Cu(NO3)2 (aq) b. HCl (aq) + NaOH (aq) → H2O (l) + NaCl (aq) c. AgNO3 (aq) + HCl (aq) → AgCl (s) + HNO 3 (aq) d. Ba(C2H3O2)2 (aq) + Na2SO4 (aq) → BaSO4 (s) + 2NaC2H3O2 (aq) e. H2CO3 (aq) + Ca(NO3)2 (aq) → 2HNO3 (aq) + CaCO3 (s) Practice: Unit 8 & 9 Extra practice questions #90 - 96 67) Pure acetic acid (HC2H3O2) is a liquid and is known as glacial acetic acid. Calculate the molarity of a solution prepared by dissolving 10.00 mL of glacial acetic acid at 25°C in sufficient water to make a 500.0 mL solution. The density of glacial acetic acid at 25°C is 1.049 g/mL. a. 1.26 x 103 b. 21.0 c. 0.0210

d. 0.350 e. 3.50 x 10-4 Practice: Unit 8 & 9 Extra practice algorithmic questions #28 - 66 68) Lead ions can be precipitated from aqueous solutions by the addition of aqueous iodide: Pb2+ (aq) + 2I- (aq) → PbI2 (s) Lead iodide is virtually insoluble in water so that the reaction appears to go to completion. How many milliliters of 3.550 M HI (aq) must be added to a solution containing 0.700 mol of Pb(NO3)2 (aq) to completely precipitate the lead? a. 2.54 x 10-3 b. 394 c. 197 d. 0.197 e. 0.394 Practice: Unit 8 & 9 Extra practice algorithmic questions #28 - 66 69) Which substance is the reducing agent in the reaction below? Pb + PbO2 + 2H2SO4 → 2PbSO4 + 2H2O a. Pb b. PbO2 c. H2SO4 d. PbSO4 e. H2O Practice: Unit 8 & 9 Extra practice questions #90 - 96 70) What is the enthalpy change (in kJ) of a chemical reaction that raises the temperature of 250.0 ml of solution having a density of 1.25 g/ml by 7.80 °C? (The specific heat of the solution is 3.74 joules/gram-K.) a. -7.43 b. 9.12 c. 8.20 d. -9.12 e. 6.51 Practice: Unit 5 multiple choice #15-18, Algorithm question #4-11 71) When a 3.88-g sample of solid ammonium nitrate is added to 60.0 mL of water in a coffeecup calorimeter, the temperature drops from 23.0°C to 18.4 °C. Calculate ΔH (in kJ/mol NH4NO3) for the solution process. Assume that the specific heat of the solution is the same as the water. NH4NO3 (s) → NH4- (aq) + NO3- (aq) a. 25.34 b. -25.34

c. 23.8 d. -23.8 e. 0.316 Practice: Unit 5 multiple choice #15-18, Algorithm question #4-11 72) When a 3.88-g sample of solid ammonium nitrate is used to create a 60.0 mL solution in a coffee-cup calorimeter, the temperature drops from 23.0 oc to 18.4 °C. Calculate ΔH (in kJ/mol NH4N03) for the solution process. Assume that the specific heat of the solution is the same as the water. NH4NO3 (s) → NH4- (aq) + NO3- (aq) a. 25.34 b. -25.34 c. 23.8 d. -23.8 e. 0.297 Practice: Unit 5 multiple choice #15-18, Algorithm question #4-11

Answers: 1. D 2. A 3. D 4. A 5. B 6. A 7. B 8. D 9. E 10. B 11. D 12. A 13. A 14. B 15. C 16. D 17. A 18. B 19. B 20. D 21. B 22. B 23. B 24. B 25. C 26. A 27. D 28. A 29. D 30. B 31. C 32. C 33. B 34. E 35. A 36. E 37. C 38. C 39. A 40. D 41. E 42. D 43. B

44. C 45. B 46. B 47. E 48. B 49. B 50. A 51. C 52. E 53. C 54. B 55. C 56. C 57. A 58. C 59. B 60. D 61. D 62. D 63. E 64. D 65. E 66. A 67. D 68. B 69. A 70. D 71. A 72. C

Spot the difference between 71 & 72 ;)...