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1 AP Chemistry Fall Semester Practice Exam 4 MULTIPLE CHOICE PORTION: Write the letter for the correct answer to the following questions on the provided answer sheet. Each multiple choice question is worth 2 points. 1. Which of the following represents the ground state electron configuration for the Mn +3 ion? a. 1s 2 2s 2 2p 6 3s 2 3p 6 3d 4 d. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 8 b. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 5 e. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 1 3d 3 c. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 2 2. Consider the following molecules: CCl 4, CO 2, PCl 3, PCl 5, SF 6 Which of the following does not describe any of the molecules listed above? a. linear d. tetrahedral b. octahedral e. trigonal pyramidal c. square planar 3. Which of the following molecules has the shortest bond length? a. N 2 b. O 2 c. Cl 2 d. Br 2 e. I 2 4. A student wishes to prepare 2.00 liters of a M KIO 3 solution. The proper procedure is to weigh out: a g of KIO 3 and add 2.00 kg of water. b g of KIO 3 and add water until the final homogeneous solution has a volume of 2.00 L. c g of KIO 3 and add water until the final homogeneous solution has a volume of 2.00 L. d g of KIO 3 and add 2.00 L of water. e g of KIO 3 and add 2.00 L of water. 5. Which of the following must be true for a reaction that proceeds spontaneously from initial standard state conditions? a. ΔG > 0 and K > 1 d. ΔG < 0 and K < 1 b. ΔG > 0 and K < 1 e. ΔG = 0 and K = 1 c. ΔG < 0 and K > 1 6. Which of the following has a zero dipole moment? a. HCN b. NH 3 c. SO 2 d. NO 2 e. PF 5 7. Consider the following information: 1. Difference in temperature between freezing point of solvent and freezing point of solution. 2. Molal freezing point depression constant, K f, for solvent. In addition to the information above, which of the following gives the minimum data required to determine the molecular mass of a nonionic substance by the freezing point depression technique? a. No further information is necessary. d. Mass of solute and volume of solvent. b. Mass of solute. e. Mass of solute, mass of solvent, and c. Mass of solute and mass of solvent. vapor pressure of solvent.
2 8. Consider the following reaction: N 2 (g) + 3 H 2 (g) 2 NH 3 (g) The reaction indicated above is thermodynamically spontaneous at 298K, but becomes nonspontaneous at higher temperatures. Which of the following is true at 298K? a. ΔG, ΔH, and ΔS are all positive. b. ΔG, ΔH, and ΔS are all negative. c. ΔG and ΔH are negative, but ΔS is positive. d. ΔG and ΔS are negative, but ΔH is positive. e. ΔG and ΔH are positive, but ΔS is negative. 9. For which of the following molecules are resonance structures necessary to describe the bonding satisfactorily? a. H 2 S b. SO 2 c. CO 2 d. OF 2 e. PF Pi bonding occurs in each of the following species EXCEPT: a. CO 2 b. C 2 H 4 c. CN 1 d. C 6 H 6 e. CH What is the mole fraction of ethanol, C 2 H 5 OH, in an aqueous solution in which the ethanol concentration is 4.6 m? a b c d e Questions refer to atoms of the following elements. a. lithium b. carbon c. nitrogen d. oxygen e. fluorine 12. In the ground state, have only 1 electron in each of the three p orbitals. 13. Have the smallest atomic radius. 14. Have the smallest value for first ionization energy. 15. The hybridization of the carbon atoms in C 2 H 6 can be described as: a. sp b. sp 2 c. sp 3 d. dsp 3 e. d 2 sp Of the following organic compounds, which is the LEAST soluble in water at 298K? a. CH 3 OH, methanol d. C 6 H 12 O 6, glucose b. CH 3 CH 2 CH 2 OH, 1-propanol e. CH 3 COOH, ethanoic acid c. C 6 H 14, hexane 17. How many electrons can be accommodated in all the atomic orbitals that correspond to the principal quantum number 4? a. 2 b. 8 c. 18 d. 32 e. 40
3 18. If ΔG for a certain reaction has a negative value at 298K, which of the following must be true? I. The reaction is exothermic. II. The reaction occurs spontaneously at 298K. III. The rate of the reaction is fast at 298K. a. I only d. II and III only b. II only e. I, II, and III c. I and II only 19. A linear molecule can have the general formulas AA, AB, or AB 2. Given a molecule with the general formula AB 2, which of the following would be the most useful in determining whether the molecule was bent or linear? a. Ionization energies d. Electronegativities b. Electron affinities e. Bond energies c. Dipole moments 20. How many moles of solid calcium nitrate should be added to 450. ml of 0.35 M aluminum nitrate to increase the concentration of the nitrate ion to 1.7 M? (Assume that the volume of the solution remains constant.) a mole b mole c mole d mole e mole 21. The enthalpy change for the reaction, A X is ΔH rxn. This reaction can be broken down into a series of steps as shown in the diagram: B ΔH 2 C ΔH 1 ΔH 3 A ΔH rxn X A relationship that must exist among the various enthalpy changes is: a. ΔH rxn ΔH 1 ΔH 2 ΔH 3 = 0 b. ΔH rxn + ΔH 1 + ΔH 2 + ΔH 3 = 0 c. ΔH 3 (ΔH 1 + ΔH 2 ) = ΔH rxn d. ΔH 2 (ΔH 3 + ΔH 1 ) = ΔH rxn e. ΔH rxn + ΔH 2 = ΔH 1 + ΔH The valence electron configuration of element A is 3s 2 3p 1 and that of element B is 3s 2 3p 4. What is the probable empirical formula for a compound of the two elements? a. A 2 B b. AB 2 c. A 3 B 2 d. A 2 B 3 e. AB 23. What is the molality of a 10.% C 6 H 2 O solution? a m b m c. 1.2 m d. 12 m
4 24. A certain organic compound has a vapor pressure of 132 mm Hg at 54 C. To determine the vapor pressure of 2.00 moles of the compound at 37 C, taking the heat of vaporization for the compound to be 4.33 x 10 4 J/mol, you would use: a. the Arrhenius equation d. the ideal gas law b. the Clausius-Clapeyron equation e. Raoult's law c. the combined gas laws 25. Consider the following information: Species Bond Energy (kcal/mole) F F 33 H H 103 H F 135 Calculate the value of ΔH for the following reaction: H 2 (g) + F 2 (g) 2 HF (g) a. 406 kcal/mol d. 134 kcal/mol b. 320 kcal/mol e kcal/mol c. 271 kcal/mol 26. A molecule exhibits d 2 sp 3 hybridization in its bonding structure. The most probable geometric shape of this molecule is: a. triangular bipyramidal d. linear b. T-shaped e. square planar c. octahedral Questions refer to the following entropy changes. a. The change in entropy will be positive. b. The change in entropy will be zero. c. The change in entropy will be negative. d. The change in entropy will be cannot be determined from the information given. 27. Predict the change in entropy. Cl 2 (g) 2 Cl (g) 28. Predict the change in entropy. H 2 (g) at 5.0 atm H 2 (g) at 1.0 atm 29. Predict the change in entropy. Sublimation of solid CO Predict the change in entropy. 2 H 2 (g) + O 2 (g) 2 H 2 O (g) 31. Predict the change in entropy. PCl 5 (g) PCl 3 (g) + Cl 2 (g) 32. Calculate the volume of a 36.45% solution of hydrochloric acid (density 1.50 g/ml) required to prepare 9.0 L of a 5.0 M solution. a. 0.5 L b. 1.0 L c. 2.0 L d. 2.5 L e. 3.0 L
5 33. For the isoelectronic series, S 2, Cl 1, Ar, K +1, and Sc +3, which species requires the least energy to remove an outer electron? a. S 2 b. Cl 1 c. Ar d. K +1 e. Sc +3 Questions refer to the following phase diagram that is NOT drawn to scale Pressure (atm) a. 78 C b. 57 C, 5.1 atm c. 31 C, 73 atm d. 31 C e. None of the above Temperature ( C) 34. What is the normal boiling point of the substance? 35. Which point represents the critical point? 36. Which point represents the triple point? 37. Molecules that have trigonal planar configurations include which of the following: I. BCl 3 II. CHCl 3 III. NCl 3 a. I only d. II and III only b. III only e. I, II, and III c. I and II only 38. Which of the following molecules is paramagnetic? a. C 2 b. N 2 c. O 2 d. F 2
6 39. What is the bond order of a molecule of nitrogen? a. 3 b. 2 c. 1 d Sterling silver, which contains 93% silver and 7% copper is a(n) alloy. a. interstitial b. substitutional c. p-type d. n-type 41. Consider the following data: Species ΔH f (kj/mole) NO 2 (g) 34 H 2 O (l) 286 HNO 3 (aq) 207 NO (g) 90. Calculate the value of ΔH for the following reaction: 3 NO 2 (g) + H 2 O (l) 2 HNO 3 (aq) + NO (g) a kj b. 184 kj c kj d. 184 kj 42. Types of hybridization exhibited by the C atoms in acetylene, C 2 H 2, include which of the following? I. sp II. sp 2 III. sp 3 a. I only d. I and II only b. II only e. I and III only c. III only
7 AP Chemistry Fall Semester Exam 2004 Name ESSAY PORTION: Write your answer on the provided answer sheet. This section is worth 16 points. 1. For each of the following, use appropriate chemical principles to explain the observation. a. When table salt (NaCl) and sugar (C 12 H 22 O 11 ) are dissolved in water, it is observed that both solutions have higher boiling points than pure water. b. When table salt (NaCl) and sugar (C 12 H 22 O 11 ) are dissolved in water, it is observed that the boiling point of 0.10 M NaCl (aq) is higher than that of 0.10 M C 12 H 22 O 11 (aq). c. Water droplets form on the outside of a beaker containing an ice bath. 2. Use the principles of atomic structure and/or chemical bonding to explain each of the following. In each part, your answer must include references to both substances. a. The second ionization energy of K is greater than the second ionization energy of Ca. b. The carbon-to-carbon bond energy in C 2 H 4 is greater than it is in C 2 H 6. c. The boiling point of Cl 2 is lower than the boiling point of Br Consider the following reaction: C (s) + CO 2 (g) 2 CO (g) Carbon (graphite), carbon dioxide, and carbon monoxide form an equilibrium mixture, as represented by the equation above. a. Predict the sign for the change in entropy, ΔS, for the reaction. Justify your prediction. b. In the table below are data that show the percent of CO in the equilibrium mixture at two different temperatures. Predict the sign for the change in enthalpy, ΔH, for the reaction. Justify your prediction. Temperature % CO 700 C C 94
8 AP Chemistry Fall Semester Exam 2004 ESSAY ANSWER SHEET: Name 1. a. b. c.
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11 AP Chemistry Fall Semester Exam 2004 MULTIPLE CHOICE ANSWER SHEET: Name
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