chem2 - Chemistry 1315 Name DO NOT TURN THIS PAGE UNTIL...

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Unformatted text preview: Chemistry 1315 Name: DO NOT TURN THIS PAGE UNTIL DIRECTED TO DO SO EXAM 4 Lab Instructor: SPRING 2005 ID Number: 1. These tests are machine graded; therefore, be sure to use a No. 1 or 2 pencil for marking the answer sheets. Completely blacken the answer circle. If you change an answer, erase completely the previous mark. 2. Write the letter code of your lab instructor (see table at bottom of this page) in the first box of the section marked "NAME". Then in the next box (do not skip a box), write your last name. Skip a space and then fill in your first name and middle initial. Example: If Joe B. Doe has Mamar Baizid, Section 17, for a lab instructor, then his answer sheet would look like: EXAMPLE: 1st Box T.A. code (see below) NAME (Last,First, M.I.) A D O E J O E B O B If your whole name does not fit, put as much as will fit. Then blacken the corresponding letters below each space on the answer sheet. 3. Fill in your ID number in the space provided, beginning with space "A". (There will be an extra box.) Then blacken the circles corresponding to the numbers below each space. 4. In the "special code" section, indicate in column K the test form you have: Mark in Column K Test Color Answer Sheet Color Swipe 1 Blue Blue 2 Gold Black 3 Pink Red 4 Tan Brown Make sure that you mark your test color in column K, and that the colored mark above your name on the answer sheet is the same as your test color. 5. In the "Special Codes" section, indicate your lecture instructor in column P. Please fill in the appropriate circle. Instructor Section Time Day Alguindigue 001 10:30-11:45 TR West 002 11:30-12:20 MWF Richter-Addo 003 8:30-9:20 MWF Thus, if Joe Doe's lecturer is Alguindigue, Sec. 001, and his test is GOLD, his "Special Codes" section would look like: SPECIAL CODES K L M N O P 2 0 1 2 3 0 1 2 3 4 0 1 2 3 0 1 2 3 0 1 2 3 1 0 1 2 3 4 4 4 4 4 The time limit on this test is 150 MINUTES. 5 5 5 5 5 READ THE TEST CAREFULLY. 5 Do not turn this page until directed to do so. 6 6 6 6 6 6 Use this booklet for scratch paper. 7 7 7 7 7 Mark your answers in this booklet, as well7as on the answer sheet, so that you can check your score with the 8 8 8 8 8 8 key after the test. 11. Each Unit Score will be calculated from the number of9correct answers. There is no penalty for guessing. 9 9 9 9 9 12. Students will be held responsible for any corrections made during the test. 13. Students who arrive more than ten minutes late, or arrive after another student has left, will not be allowed to take the examination. 6. 7. 8. 9. 10. Instructor Code Mamar Baizid A Kostyantyn Bobyk B Vishakha Devroy C Alla Dubrovska D Guinevere Giffin E Randy Hine F Bo Jin G G. Krishnamoorthy H Carolina Salazar I Section(s) Exam Room 17, 24 DH 103 22 DH 122 25 NH A102 12, 36 DH 103 29, 31 DH 122 27, 32, 40 DH 200 16, 42 DH 206 15 DH 200 20, 35 DH 218 Instructor Yi Shao Jeremy Stephens Leonid Sukharnikov Ting Sun Kim Swinehart Hui Tang Valeriya Vorozhko Hanhui Xu Hua Yang Code J K L M N O P Q R Section(s) 21, 26 11, 19 30, 37 14, 28 23 33 34, 38 13, 41 18, 39 Exam Room NH A 102 DH 128 DH 211 DH 200 DH 211 DH 206 DH 211 DH 200 DH 128 PHYSICAL AND CHEMICAL CONSTANTS Atomic mass unit Avogadro's number Boltzmann's constant Electon rest mass Electronic charge Faraday's constant Gas constant Neutron rest mass Pi Plank's constant Proton rest mass Speed of light (vacuum) Volume of a cylinder 1 amu = 1.6605402 x 10-27 kg 6.0221367 x 102 3 amu = 1 g N = 6.0221367 x 102 3 /mol k = 1.38066 x 10-23 J/K me = 5.485799 x 10-4 amu = 9.1093897 x 10-28 g e = 1.60217733 x 10-19 C F = N e = 9.6485309 x 104 C/mol R = N k = 8.3145 J/Kmol = 0.0821 Latm/Kmol mn = 1.00866 amu = 1.67495 x 10-24 g = 3.1415926536 h = 6.626 x 10-34 Js mp = 1.0072765 amu = 1.672623 x 10-24 g c = 3.00 x 108 m/s V=hr2 (h = height, r = radius) 1 lb. = 16 oz. = 453.6 g 1 in. = 2.54 cm 1 gallon = 3.7852 liter 1 mile = 5280 ft 1 meter = 6.214 x 10-4 mile (Mass numbers given in parentheses represent the mass number of the most stable isotope.) ______________________________________________________________ Unit 5 - Molecular Structure & Bonding ______________________________________________________________ 1. Which one of the following best describes the correct molecular geometry of the iodine trifluoride (IF3)? A. T-shaped D. octahedral B. square pyramidal E. trigonal bipyramidal C. see-saw 2. Which one of the Lewis structures shown below is drawn CORRECTLY? A. H O H H C C C H H O H H O H H C C O C H H H B. H O H H C S C H H O H H O H H H C C O C H H C. O H H C C C H H H H D. E. 3. Which one of the bonds shown below has the bond polarity (indicated with an arrow) drawn CORRECTLY? A. Cl H B. Se O C. I Cl D. O Pb E. Br Ge 4. Which one of the following correctly ranks the indicated elements from the most electronegative to the least electronegative? A. N > Br > As > Ga > K D. N > Br > Ga > As > K B. N > As > Br > Ga > K E. Br > N > As > K > Ga C. K > Ga > As > Br > N 5. Which one of the bonds shown below is expected to be the longest, i.e., to have the greatest bond distance? A. C C B. C N C. C O D. C S E. C I 6. Which one of the bonds shown below would be expected to have the lowest (smallest) bond energy? A. I--F B. I--O C. I--I D. I--N E. I--Cl 7. Which one of the resonance structures of the peroxysulfate anion (S2O82) shown below is drawn INCORRECTLY? A. 2O O O S O O S O O O B. 2O O O S O O S O O O C. 2O O O S O O S O O O D. 2O O O S O O S O O O E. 2O O O S O O S O O O Page 1, v1 8. The Lewis structure of histidine, a naturally-occurring amino acid, is shown below. What is the correct hybridization of the atoms labeled X, Y, and Z in the structure of histidine? X H H O H N C C O H H C H H Z C H C C C H N C H C C H H C Y A. B. C. D. E. X = sp2, Y = sp2, Z = sp3 X = sp3, Y = sp2, Z = sp3 X = sp2, Y = sp, Z = sp3 X = sp2, Y = sp3, Z = sp2 X = sp3, Y = sp2, Z = sp2 9. How many (sigma) and (pi) bonds are there in the structure shown below? H C H C H H N H H C C C C C C H H H H H A. B. C. D. E. 19 , 4 19 , 5 18 , 3 20 , 4 18 , 4 10. Which one of the following best describes the correct molecular geometry of the methanide ion (CH3)? A. B. C. D. E. tetrahedral trigonal bipyramidal trigonal planar trigonal pyramidal V-shaped (bent) ______________________________________________________________ Unit 6 - Properties of Gases ______________________________________________________________ 11. A sealed rigid container is filled with 40 g of helium (He) and 40 g of nitrogen (N2). At 30C the container has a pressure of 6.1 atm. What is the partial pressure of helium? A. 3.0 atm B. 0.7 atm C. 0.5 atm D. 1.5 atm E. 5.4 atm 12. How many liters would 5.0 moles of O2 occupy given a pressure of 15 atm, and a temperature of 50C? A. 1.4 L B. 1.8 L C. 8.8 L D. 10.2 L E. 20.5 L 13. 31.6 g of an unknown gas in a tank with a volume of 2.8 L at 30C has a pressure of 4 atm. What is the molecular weight of the gas in g/mol? A. 70 B. 14 C. 35 D. 28 E. 7 Page 2, v1 14. The left hand side of an open-ended manometer is attached to a sample of gas. The height of the Hg on the left side is 80.3 cm, while the height of the Hg on the right side is 85.0 cm. The atmospheric pressure is 0.95 atm. What is the pressure of the gas in Torr? A. 727 Torr B. 717 Torr C. 769 Torr D. 722 Torr E. 675 Torr 15. Which of the following statements about ideal gases is correct? A. B. C. D. E. Most deviations from ideal behavior occur at 25C and 1 atm The elastic nature of molecular collisions prevents loss of energy The molar volume of a gas is proportional to molecular weight At constant volume increased temperature results in decreased pressure None of the above are correct 16. A sample of H2 in a balloon with a volume of 2.5 L at 22.5C had a pressure of 2 atm. The gas was then warmed to 37.0C, which decreased the pressure by a factor of 2. What is the new volume? A. 1.3 L B. 3.7 L C. 4.2 L D. 5.2 L E. 6.1 L 17. The rate of effusion of chlorine (Cl2) from a solid container is 6 mol/min, while the rate of effusion of an unknown gas is 9.45 mol/min. Given the gases below, which is most likely for the unknown gas? A. CH4 B. Ne C. O2 D. F 2 E. N2 18. For a sample of Cl2 gas at 273 K, if the pressure is increased by a factor of 2, and the volume is decreased by a factor of 10, what is the new temperature? A. 250 K B. 55 K C. 300 K D. 355 K E. 273 K 19. Consider the following reaction H2 + Cl 2 2 HCl At 0C and 1 atm, what volume of Cl2 is required to react with 50 g of H2 gas? A. 560 L B. 1120 L C. 420 L D. 840 L E. 280 L 20. 25.0 g of ethylene is burned in oxygen giving carbon dioxide and water according to the following unbalanced equation. What volume of CO2 gas is produced at 1 atm and 25.0C? C2H4 (g) + O2(g) CO2(g) + H2O(g) A. 79.8 L B. 43.4 L C. 39.9 L D. 21.7 L E. 19.9 L ______________________________________________________________ Unit 7 - Properties of Liquids, Solids, & Solutions ______________________________________________________________ 21. Which of the following is an example of an ionic solid? A. Ca (NO3)2 B. C6H6 C. CO2 D. Au E. SO2 Page 3, v1 22. On the basis of the following diagram, choose the point that represents sublimation. A. A B. B C. C D. D E. E 23. If the boiling point of water is increased from 100C to 115C, which of the following must be true? A. B. C. D. E. The volume of water is greater than 1 L The pressure must be greater than 1 atm Water is boiling at high altitude Water is boiling at its critical point The boiling point of water cannot be greater than 100C 24. The melting point of H2O is higher than that of H2S as a result of which of the following? A. B. C. D. E. Dipole-dipole interactions Ion-dipole interactions Hydrogen bonds Ion-induced dipole interactions London dispersion forces 25. Given the following packing of chloride (AA), and assuming a positively charged group 1 metal ion could fit into the hole in the center, what coordination number would it have? How many atoms of Cl- would be in the unit cell? A. 4, 2 B. 6, 1 C. 8, 2 D. 10, 3 E. 12, 3 26. In the following reaction BaCl2 + NaOH Ba (OH)2 + NaCl A. B. C. D. E. No reaction will occur since BaCl2 is insoluble No reaction will occur since NaOH is insoluble Reaction will result in precipitation of Ba(OH)2 Ba2+ and OH are spectator ions NaCl will precipitate Page 4, v1 27. Which of the following would not be soluble in water? A. MgSO4 B. CH3OH C. Na3PO 4 D. C6H6 E. KClO4 28. Which of the following is a strong electrolyte? A. H2SO 4 B. HCOOH C. CH3OH D. CH 3COOH E. Cl2 29. The triple point is defined as the pressure and temperature where A. B. C. D. E. a molecule cannot exist as a liquid. solid is converted to vapor. the vapor pressure of solid and liquid are equal. solid, liquid and vapor are in equilibrium. only solid can exist 30. Which of the following will form a network solid? A. NaCl B. C C. Ag D. CO 2 E. CuFe ______________________________________________________________ Unit 8 - Organic Chemistry ______________________________________________________________ 31. Which one of the structures shown below contains a chiral center? A. H OH O HO C C C H H H H O H O H H H C C C C O C C H H H H H B. H O H HO C C C OH H H H O O H H H H C C O C C C C H H H H H C. H H O HO C C C OH H H D. E. 32. The reaction shown below is an example of which one of the following reaction types. H H H H H + Br2 H AlBr3 H H H H Br + H +[AlBr 4]H A. addition D. substitution B. condensation E. elimination C. reduction Page 5, v1 33. Which one of the structures shown below is that of 3ethyl2,2,6trimethyl1heptanol? A. CH2 CH3 CH3 CH3 CH2CHCH2CH C CH2 OH CH3 CH3 B. CH3 CH2 CH3 CH3 CHCH2CH2CH C CH2 OH CH3 CH3 CH3 CH3 CH3 CHCH2CH2CH C CH3 CH3 CH2 OH C. D. CH3 CH3 CH3 CH2CHCH2CH C CH2 OH CH3 CH2 CH3 E. CH3 CH3 CH3 CHCH2CH2CH C CH2 OH CH3 CH2 CH3 34. The structure of aspartame, which is used as an artificial sweetener (in foods flavored with Nutra Sweet) is shown below. What functional groups does aspartame contain? P H 2N CH CH2 C O S OH O C O CH C O CH3 CH2 H C H C C R C C H C H H H N Q A. B. C. D. E. P = amine P = amide P = amine P = amine P = amide Q = carboxylic acid R = benzene ring S = carboxylic acid Q = ester R = cyclohexane S = carboxylic acid Q = ester R = benzene ring S = carboxylic acid Q = ester R = benzene ring S = aldehyde Q = aldehyde R = benzene ring S = ketone Page 6, v1 35. Which one of the following combinations of monomers was most likely used to form the polymer shown below H O O NCH 2CH2 N C CH2 C H A. O O HO C CH2 CH2 C OH O O HO C CH2 C OH and H2NCH 2NH 2 B. and H2NCH 2CH 2NH2 C. HO CH2 CH2 CH2 OH and H2NCH 2CH 2NH2 H2NCH 2NH 2 D. HO CH CH CH CH OH 2 2 2 2 E. O O HO C CH2 C OH and and H2NCH 2CH 2OH 36. Which one of the names listed below is the correct IUPAC name for the following compound? CH3 CH3 CH Cl CH2 CH3 C CHCH2CH Br Cl CH2 CH3 A. B. C. D. E. 1bromo4, 4dichloro1, 3diethyl5methylhexane 3bromo6, 6dichloro5ethyl7methyloctane 6bromo3, 3dichloro4ethyl2methyloctane 2methyl3, 3dichloro4ethyl6bromoctane 3bromo6, 6dichloro5ethyl6isopropylhexane 37. Which one of the structures shown below is that of the major organic product from the following reaction? CH3 CH2CH 2CH2 Br + CH 3 O Na ? A. CH3 CH2CH 2CH2 OH B. OCH3 CH3 CHCH2CH2Br C. CH3O CH2 CH2CH 2CH2 Br D. CH3 CH2CH 2CH2 OCH3 E. CH3 CH2CH 2CHOCH3 Br 38. Compounds that are nonsuperimposable mirror images of one another are described as which one of the following terms? A. isoelectronic D. isotopes B. enantiomers E. diastereomers C. isomers Page 7, v1 39. The reaction shown below is best described as being a(n): H H C C H H C C C OH C C H H H H H C C O H C C C OH C C H H CrO3 H2SO 4 A. oxidation D. substitution B. addition E. polymerization C. reduction 40. The reaction (shown below) used in soap making, in which a triglyceride is hydrolyzed in the presence of aqueous potassium hydroxide to form glycerol and three moles of potassium carboxylate, is called which one of the following terms? O R C O CH2 O R C O CH O R C O CH2 a triglyceride KOH H2O O R C O K O R C O K O R C O K potassium carboxylate HO CH2 + HO CH HO CH2 glycerol A. esterification D. saponification B. isomerization E. racemization C. trihydroxylation Page 8, v1 CHEM 1315 Exam4 Spring, 2005 (Blue) Unit 1 1. 2. 3. 4. 5. 6. 7. 8. 9. A B D A E C C D A Unit 2 11. E 12. C 13. A 14. C 15. B 16. D 17. E 18. B 19. A 20. B Unit 3 21. A 22. E 23. B 24. C 25. B 26. C 27. D 28. A 29. D 30. B Unit 4 31. A 32. D 33. E 34. C 35. B 36. C 37. D 38. B 39. A 40. D 10. D ...
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This note was uploaded on 05/24/2008 for the course CHEM 1315 taught by Professor Clifford during the Spring '08 term at The University of Oklahoma.

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