2006 Academic Challenge
|
|
- Bruce Blaise Brooks
- 6 years ago
- Views:
Transcription
1 2006 Academic Challenge CHEMISTRY TEST - STATE FINALS This Test Consists of 40 Questions Chemistry Test Production Team Don DeCoste, University of Illinois at Urbana - Champaign Author/Team Coordinator Gretchen Adams, University of Illinois at Urbana - Champaign Author Nancy Carter Dopke, Mercer University Reviewer Don Wayman, WYSE Coordinator of Test Production GENERAL DIRECTIONS Please read the following instructions carefully. This is a timed test; any instructions from the test supervisor should be followed promptly. The test supervisor will give instructions for filling in any necessary information on the answer sheet. Be sure you understand and correctly follow these instructions. You are to indicate your answer to each question by marking an oval that corresponds to the correct answer for that question. Only one oval should be marked to answer each question. Multiple ovals will automatically be graded as an incorrect answer. Be sure ovals are marked as. Not as,,, etc. If you wish to change an answer, erase your first mark completely before marking your new choice. You are advised to use your time effectively and to work as rapidly as you can without losing accuracy. Do not waste your time on questions that are too difficult for you. Go on to the other questions and come back to the difficult ones later if you can. *** TIME: 40 MINUTES *** DO NOT OPEN TEST BOOKLET UNTIL YOU ARE TOLD TO DO SO! 2006 Worldwide Youth in Science and Engineering WYSE, Worldwide Youth in Science and Engineering and the WYSE Design are service marks of and this work is Copyright 2006 Board of Trustees of the University of Illinois at Urbana - Champaign. All rights reserved
2 Periodic Table of the Elements *Lanthanides **Actinides 1A 2A 3A 4A 5A 6A 7A 8A 19 K Ca Rb Sr Cs Ba Li Be Na Mg H Fr (223) 88 Ra Sc Ti V Cr Mn Fe Co Ni Cu Zn Y Zr Nb Mo Tc (98) 44 Ru Rh Pd Ag Cd La* Hf Ta W Re Os Ir Pt Au Hg Unq 105 Unp 106 Unh 107 Uns 108 Uno 109 Une 89 Ac** (227) 31 Ga In Tl B Al Ge Sn Pb C Si As Sb Bi N P Se Te Po (209) 8 O S Br I At (210) 9 F Cl He Kr Xe Rn (222) 10 Ne Ar Ce Pr Nd Pm (145) 62 Sm Eu Gd Tb Dy Ho Er Tm Yb Lu Th Pa (231) 92 U Np (237) 94 Pu (244) 95 Am (243) 96 Cm (247) 97 Bk (247) 98 Cf (251) 99 Es (252) 100 Fm (257) 101 Md (258) 102 No (259) 103 Lr (260)
3 The information on this page may be useful in completing this exam. ph = -log[h + ] poh = -log[oh - ] K w = 1 x PV = nrt (R = L atm mol -1 K -1 ) (R = J mol -1 K -1 ) K = C ΔG = ΔH TΔS N A = x atoms mol -1 Assume gases behave ideally unless specifically told otherwise. Assume solutions are aqueous and at 25 C unless specifically told otherwise. STANDARD REDUCTION POTENTIALS (298 K) ε (V) Cl 2 + 2e - 2Cl Br 2 + 2e - 2Br Ag + + e - Ag 0.80 I 2 + 2e - 2I Cu e - Cu H + + 2e - H Al e - Al Mg e - Mg Na + + e - Na K + + e - K Faraday s constant (F) = 96,485 C/mol
4 WYSE Academic Challenge Chemistry Test (State Finals) A 20.0-g sample of a gaseous hydrocarbon (a compound consisting of only carbon and hydrogen) is placed in a balloon at 1.00 atm and 25 C. The volume of the balloon is 16.3 L. The 20.0-g sample of this compound contains 16.0 g carbon. Determine the molecular formula for this compound. a) CH 3 b) CH 4 c) C 3 H 8 d) C 3 H 9 e) C 2 H 6 2. Consider the reaction as represented by the following unbalanced chemical equation N 2 + H 2 NH 3 In which of the following cases is nitrogen the limiting reactant? a) Reacting 60.0 g of N 2 with 10.0 g of H 2. b) Reacting 2.0 moles of N 2 with 5.0 moles of H 2. c) Reacting g of N 2 with 60.0 g of H 2. d) Reacting 3.0 moles of N 2 with 3.0 moles of H 2. e) Nitrogen is not limiting in any of the cases above. 3. Which of the following has the highest ionization energy? a) Mg b) Mg + c) Mg 2+ d) Mg 3+ e) all the same 4. Which of the following is the most ideal gas at room conditions? a) CO b) H 2 O c) HF d) NH 3 e) N 2 5. The electron configuration 1s 2 2s 2 2p 6 3s 2 3p 6 is the correct electron configuration for the most stable form of which ion? a) The calcium ion. b) The argon ion. c) The magnesium ion. d) The fluoride ion. e) The oxide ion. 6. Consider a steel container filled with 40.0 g of helium gas (He) and 40.0 g of argon gas (Ar). What is the ratio of pressures that each gas exerts (answers are for He:Ar)? a) 1:1 b) 10:1 c) 1:10 d) 9:1 e) Need more information.
5 Chemistry 2 7. The unit cell in this two-dimensional crystal contains Xs and Os. X X X X O O O O X X X X O O O O X X X X O O O O a) 1,4 b) 2,1 c) 1,2 d) 4,1 e) 1,1 8. Consider a reaction represented by the following balanced equation 2A + 3B C + 4D You find that it requires equal masses of A and B so that there are no reactants left over. Which of the following is true? a) The molar mass of A must be greater than molar mass of B. b) The molar mass of A must be less than molar mass of B. c) The molar mass of A must be the same as molar mass of B. d) More information is needed to answer this question. e) None of the above choices (a-d) are true. 9. You carry out the reaction represented by the following balanced equation N 2 (g) + 3H 2 (g) 2NH 3 (g) You add an equal number of moles of nitrogen and hydrogen gases in a balloon. The volume of the balloon is 1.00 L before any reaction occurs. Determine the volume of the balloon after the reaction is complete. a) L b) L c) 1.00 L d) 1.50 L e) 3.00 L 10. Which of the following are isomers? a) dimethyl ether and ethanol b) propanol and propanal c) ethanol and propanol d) propanone and propanol e) dimethyl ether and methanol 11. Calculate the density of neon gas (Ne) at 1.00 atm and 25.0 C. a) g/l b) 9.84 g/l c) 20.2 g/l d) 22.4 g/l e) None of these.
6 Chemistry Which of the following is the most polar bond? a) C-H b) N-O c) C-O d) O-O e) O-S 13. Consider the reaction between 50.0 ml of M NaOH and 75.0 ml of M HCl. Which of the following statements is true? a) After the reaction, the concentration of Na + is greater than the concentration of OH -. b) The NaOH was the limiting reactant. c) After the reaction, the concentration of Na + is equal to the concentration of Cl -. d) After the reaction, the concentration of Na + is still M because Na + is a spectator ion. e) None of these are correct. 14. Which of the following has the lowest boiling point? a) H 2 O b) C 2 H 6 c) NH 3 d) CH 3 OH e) CH Which of the following molecules is non-polar even though it has polar bonds? a) Cl 2 O b) NH 3 c) CO d) N 2 e) BF Consider separate gram samples of each of the following: NH 3, N 2 O, N 2 H 4, HCN, HNO 3. Which of the samples has the largest mass of nitrogen? a) NH 3 b) N 2 O c) HCN d) N 2 H 4 e) HNO Which of the following gives the correct orders for increasing (from smallest to largest) atomic radius and ionization energy, respectively? a) S, O, F and F, O, S b) F, S, O and O, S, F c) S, F, O and S, F, O d) F, O, S and S, O, F e) none of these 18. You are asked to determine the perimeter of the cover of your textbook. You measure the length as cm and the width as cm. How many significant figures should you report for the perimeter? a) 1 b) 2 c) 3 d) 4 e) Which of the following correctly ranks the atoms from the least electronegative to the most electronegative? a) Li, B, C, N, Na b) K, Na, S, Cl, F c) Fr, N, P, O, F d) Be, Mg, Ca, Sr, Cs e) At least two of the above (a-d) correctly ranks the atoms from the least electronegative to the most electronegative.
7 20. Arrange the following 0.10 M aqueous solutions from lowest to highest ph. Chemistry 4 Kb for NH 3 = 1.8 x 10-5 Ka for HC 2 H 3 O 2 = 1.8 x 10-5 Ka for HF = 7.2 x 10-4 NaOH, HCl, NaCl, NaC 2 H 3 O 2, NH 4 F, NH 3 a) HCl, NH 4 F, NaCl, NaC 2 H 3 O 2, NaOH, NH 3 b) HCl, NaCl, NH 4 F, NH 3, NaC 2 H 3 O 2, NaOH c) HCl, NH 4 F, NaCl, NaC 2 H 3 O 2, NH 3, NaOH d) HCl, NaCl, NH 4 F, NaC 2 H 3 O 2, NH 3, NaOH e) HCl, NaCl, NaC 2 H 3 O 2, NH 3, NH 4 F, NaOH 21. What is the percent oxygen by mass in sodium sulfate? a) 38.1% b) 45.1% c) 49.6% d) 53.8% e) none of these 22. Determine the [C 6 H 6 O 6 2- ] for ml of a M solution of H 2 C 6 H 6 O 6 (Ka 1 = 7.9 x 10-5, Ka 2 = 1.6 x ). a) 4.0 x 10-3 M b) 1.3 x 10-3 M c) 7.9 x 10-5 M d) 1.6 x M e) none of these 23. The vinegar you buy in the grocery store is 0.83 M acetic acid (HC 2 H 3 O 2, Ka = 1.8 x 10-5 ). What concentration of HF (Ka = 7.2 x 10-4 ) has the same ph as vinegar? a) 1.5 x 10-5 M b) 3.9 x 10-3 M c) M d) 0.83 M e) 33 M 24. True or false: The species Cl - is not a good base in aqueous solution. a) True. This is because Cl - is the conjugate base of a weak acid. b) False. The species Cl - is a good base in aqueous solution because it is the conjugate base of a strong acid. c) True. This is because Cl - is a good proton donor. d) False. The species Cl - is a good base in aqueous solution because of its high electronegativity. e) True. This is because water has a stronger attraction for protons than does Cl -.
8 25. Which of the following will raise the ph of a weak acid HA in aqueous solution? I. Addition of water. II. Addition of NaA (s) III. Addition of NaCl (s). IV. Addition of HNO 3. V. Addition of KOH. a) IV only b) II, V c) I, III, V d) I, II, V e) II, III, V Chemistry You add an excess of solid PbCl 2 to water (K sp for PbCl 2 = 1.6 x 10-5 ). Calculate the concentration of Cl - at equilibrium. a) M b) M c) M d) M e) none of these 27. Which of the following has the lowest vapor pressure at a given temperature? a) CH 3 OCH 3 b) CH 3 CH 2 OH c) CH 3 CH 2 CH 3 d) CH 3 CH 2 CH 2 CH 3 e) H 2 O 28. For which of the following is ΔS expected to be negative? a) Table salt dissolves in water. b) N 2 (g) + 3H 2 (g) 2NH 3 (g) c) 2KClO 3 (s) 2KCl(s) + 3O 2 (g) d) Water evaporates. e) ΔS can never be negative. 29. At constant pressure what does a large negative value of ΔG for a reaction indicate? a) The reaction lies further on the product side and occurs more quickly than a reaction with a lower value of ΔG. b) The reaction lies further on the reactant side and occurs more quickly than a reaction with a lower value of ΔG. c) The reaction lies further on the product side but we know nothing of the rates of reaction. d) The reaction lies further on the reactant side but we know nothing of the rates of reaction. e) The reaction lies further on the reactant side and occurs more slowly than a reaction with a lower value of ΔG.
9 Chemistry The experimental rate law for the decomposition of nitrous oxide (N 2 O) to N 2 and O 2 is rate = k[n 2 O] 2. Two mechanisms are proposed: I. N 2 O N 2 + O N 2 O + O N 2 + O 2 II. 2N 2 O N 4 O 2 N 4 O 2 2N 2 + O 2 Which of the following could be a correct mechanism? a) Mechanism I with the first step as the rate-determining step. b) Mechanism I with the second step as the rate-determining step as long as the first step is a fast equilibrium step. c) Mechanism II with the second step as the rate-determining step if the first step is a fast equilibrium step. d) None of the choices (a-c) could be correct. e) At least two of the above choices (a-c) could be correct. 31. The name of the compound PbO 2 is a) lead(ii) oxide b) lead dioxide c) lead oxide d) lead(iv) oxide e) lead oxalate 32. Which of the following is the strongest oxidizing agent? a) Cl 2 b) K c) Cl - d) K + e) H Electrolysis of a molten salt with the formula MCl, using a current of 3.86 amp for 16.2 min, deposits 1.52 g of metal. Identify the metal. a) Li b) Na c) K d) Rb e) Ca 34. You have a system at equilibrium governed by the equation PCl 5 (g) PCl 3 (g) + Cl 2 (g), for which ΔH = -89kJ. How many of the following will shift equilibrium to the right? I. Add more PCl 5 II. Decrease the pressure by increasing the volume III. Remove Cl 2 IV. Decrease the temperature. a) 0 b) 1 c) 2 d) 3 e) A compound is composed of element X and hydrogen. Analysis shows the compound to be 80% X by mass, with three times as many hydrogen atoms as X atoms per molecule. Which element is element X? a) C b) He c) F d) S e) none of these
10 Chemistry Consider the combustion of methane (as represented by the following equation). This is the reaction that occurs for a Bunsen burner, which is a source of heat for chemical reactions in the laboratory. CH 4 (g) + 2O 2 (g) CO 2 (g) + 2H 2 O(g) For the system at chemical equilibrium, which of the following explains what happens if the temperature is raised? a) The equilibrium position is shifted to the right and the value for K increases. b) The equilibrium position is shifted to the left and the value for K decreases. c) The equilibrium position is shifted to the right and the value for K decreases. d) The equilibrium position is shifted to the left and the value for K increases. e) The equilibrium position is shifted but the value for K stays constant. 37. Calculate the solubility of Ag 2 CrO 4. The K sp for Ag 2 CrO 4 is 9.0 x a) 9.0 x M b) 2.1 x 10-4 M c) 6.5 x 10-5 M d) 3.0 x 10-6 M e) 1.3 x 10-4 M 38. Which of the following is a not a chemical change? a) Adding an acid to a base. b) Adding water to sodium. c) A phase change. d) The oxidation of iron. e) All of the above are chemical changes. 39. Arrange the following forms of electromagnetic radiation from shortest to longest wavelength. a) ultraviolet, infrared, microwaves, blue (visible), red (visible) b) red (visible), blue (visible), microwaves, infrared, ultraviolet c) microwaves, infrared, red (visible), blue (visible), ultraviolet d) ultraviolet, blue (visible), red (visible), infrared, microwaves e) microwaves, ultraviolet, infrared, red (visible), blue (visible) 40. Which organic functional group is represented in the generic formula R-OH? a) amine b) secondary alcohol c) aldehyde d) primary alcohol e) ketone
Lab Day and Time: Instructions. 1. Do not open the exam until you are told to start.
Name: Lab Day and Time: Instructions 1. Do not open the exam until you are told to start. 2. This exam is closed note and closed book. You are not allowed to use any outside material while taking this
More informationM09/4/CHEMI/SPM/ENG/TZ1/XX+ CHEMISTRY. Monday 18 May 2009 (afternoon) 45 minutes INSTRUCTIONS TO CANDIDATES
M09/4/CHEMI/SPM/ENG/TZ1/XX+ 22096110 CHEMISTRY standard level Paper 1 Monday 18 May 2009 (afternoon) 45 minutes INSTRUCTIONS TO CANDIDATES Do not open this examination paper until instructed to do so.
More informationInstructions. 1. Do not open the exam until you are told to start.
Name: Lab Day and Time: Instructions 1. Do not open the exam until you are told to start. 2. This exam is closed note and closed book. You are not allowed to use any outside material while taking this
More information8. Relax and do well.
CHEM 15 Exam II John II. Gelder March 4, 1999 Name TA's Name Lab Section INSTRUCTIONS: 1. This examination consists of a total of 7 different pages. The last two pages includes a periodic table, a solubility
More informationLab Day and Time: Instructions. 1. Do not open the exam until you are told to start.
Name: Lab Day and Time: Instructions 1. Do not open the exam until you are told to start. 2. This exam is closed note and closed book. You are not allowed to use any outside material while taking this
More informationLab Day and Time: Instructions. 1. Do not open the exam until you are told to start.
Name: Lab Day and Time: Instructions 1. Do not open the exam until you are told to start. 2. This exam is closed note and closed book. You are not allowed to use any outside material while taking this
More informationChemistry Standard level Paper 1
M15/4/CHEMI/SPM/ENG/TZ1/XX Chemistry Standard level Paper 1 Thursday 14 May 2015 (afternoon) 45 minutes Instructions to candidates Do not open this examination paper until instructed to do so. Answer all
More informationM11/4/CHEMI/SPM/ENG/TZ2/XX CHEMISTRY STANDARD LEVEL PAPER 1. Monday 9 May 2011 (afternoon) 45 minutes INSTRUCTIONS TO CANDIDATES
M11/4/CHEMI/SPM/ENG/TZ/XX 116116 CHEMISTRY STANDARD LEVEL PAPER 1 Monday 9 May 011 (afternoon) 45 minutes INSTRUCTIONS TO CANDIDATES Do not open this examination paper until instructed to do so. Answer
More information8. Relax and do well.
CHEM 1515 Exam II John II. Gelder October 14, 1993 Name TA's Name Lab Section INSTRUCTIONS: 1. This examination consists of a total of 8 different pages. The last two pages include a periodic table, a
More information2008 Academic Challenge
2008 Academic Challenge CHEMISTRY TEST - REGIONAL - - This Test Consists of 40 Questions - - Chemistry Test Production Team Don DeCoste, University of Illinois at Urbana - Champaign Author/Team Leader
More informationChapter 3: Stoichiometry
Chapter 3: Stoichiometry Chem 6A Michael J. Sailor, UC San Diego 1 Announcements: Thursday (Sep 29) quiz: Bring student ID or we cannot accept your quiz! No notes, no calculators Covers chapters 1 and
More informationM10/4/CHEMI/SPM/ENG/TZ2/XX+ CHEMISTRY. Wednesday 12 May 2010 (afternoon) 45 minutes INSTRUCTIONS TO CANDIDATES
M10/4/CHEMI/SPM/ENG/TZ/XX+ 106116 CHEMISTRY standard level Paper 1 Wednesday 1 May 010 (afternoon) 45 minutes INSTRUCTIONS TO CANDIDATES Do not open this examination paper until instructed to do so. Answer
More information8. Relax and do well.
CHEM 1215 Exam III John III. Gelder November 11, 1998 Name TA's Name Lab Section INSTRUCTIONS: 1. This examination consists of a total of 7 different pages. The last page includes a periodic table and
More informationCHEM 107 (Spring-2005) Exam 3 (100 pts)
CHEM 107 (Spring-2005) Exam 3 (100 pts) Name: ------------------------------------------------------------------------, Clid # ------------------------------ LAST NAME, First (Circle the alphabet segment
More informationChemistry 2 Exam Roane State Academic Festival. Name (print neatly) School
Name (print neatly) School There are fifteen question on this exam. Each question is weighted equally. n the answer sheet, write your name in the space provided and your answers in the blanks provided.
More informationLast 4 Digits of USC ID:
Chemistry 05 B Practice Exam Dr. Jessica Parr First Letter of last Name PLEASE PRINT YOUR NAME IN BLOCK LETTERS Name: Last 4 Digits of USC ID: Lab TA s Name: Question Points Score Grader 8 2 4 3 9 4 0
More information2008 Academic Challenge
2008 Academic Challenge CHEMISTRY TEST - SECTIONAL - - This Test Consists of 40 Questions - - Chemistry Test Production Team Don DeCoste, University of Illinois at Urbana - Champaign Author/Team Leader
More informationLab Day and Time: Instructions. 1. Do not open the exam until you are told to start. Page # Points possible Points awarded
Name: Lab Day and Time: Instructions 1. Do not open the exam until you are told to start. 2. This exam is closed note and closed book. You are not allowed to use any outside material while taking this
More informationINSTRUCTIONS: Exam III. November 10, 1999 Lab Section
CHEM 1215 Exam III John III. Gelder November 10, 1999 Name TA's Name Lab Section INSTRUCTIONS: 1. This examination consists of a total of 7 different pages. The last page includes a periodic table and
More informationPERIODIC TABLE OF THE ELEMENTS
Useful Constants and equations: K = o C + 273 Avogadro's number = 6.022 x 10 23 d = density = mass/volume R H = 2.178 x 10-18 J c = E = h = hc/ h = 6.626 x 10-34 J s c = 2.998 x 10 8 m/s E n = -R H Z 2
More informationCHEM 167 FINAL EXAM MONDAY, MAY 2 9:45 11:45 A.M GILMAN HALL
PROF. JOHN VERKADE SPRING 2005 THIS EXAM CONSISTS OF 12 QUESTIONS ON 9 PAGES CHEM 167 HOUR EXAM IV APRIL 20, 2005 SEAT NO. NAME RECIT. INSTR. RECIT. SECT. GRADING PAGE Page 2 Page 3 Page 4 Page 5 Page
More information02/05/09 Last 4 Digits of USC ID: Dr. Jessica Parr
Chemistry 05 B First Letter of PLEASE PRINT YOUR NAME IN BLOCK LETTERS Exam last Name Name: 02/05/09 Last 4 Digits of USC ID: Dr. Jessica Parr Lab TA s Name: Question Points Score Grader 2 2 9 3 9 4 2
More informationChem 102H Exam 2 - Spring 2005
Name I.D. # Chem 102H Exam 2 - Spring 2005 PHYSICAL CNSTANTS/CNVERSIN FACTRS Speed of light = 3.00! 10 8 m/s Planck!s const. = 6.63! 10-34 J s Avagadro!s Number = 6.02! 10 23 Electron charge = 1.602! 10-19
More informationOregon State University, Summer 2009 Chemistry 121 Midterm Exam 2, July 3rd, 10 am
Oregon State University, Summer 2009 Chemistry 121 Midterm Exam 2, July 3rd, 10 am DO NOT OPEN THIS EXAM UNTIL INSTRUCTED. CALCULATORS ARE NOT TO BE SHARED. Instructions : You should have with you several
More informationCHEM 108 (Spring-2008) Exam. 3 (105 pts)
CHEM 08 (Spring-008) Exam. (05 pts) Name: --------------------------------------------------------------------------, CLID # -------------------------------- LAST NAME, First (Circle the alphabet segment
More informationSolutions and Ions. Pure Substances
Class #4 Solutions and Ions CHEM 107 L.S. Brown Texas A&M University Pure Substances Pure substance: described completely by a single chemical formula Fixed composition 1 Mixtures Combination of 2 or more
More informationMarks for each question are as indicated in [] brackets.
Name Student Number CHEMISTRY 140 FINAL EXAM December 10, 2002 Numerical answers must be given with appropriate units and significant figures. Please place all answers in the space provided for the question.
More informationAdvanced Placement. Chemistry. Integrated Rates
Advanced Placement Chemistry Integrated Rates 204 47.90 9.22 78.49 (26) 50.94 92.9 80.95 (262) 52.00 93.94 83.85 (263) 54.938 (98) 86.2 (262) 55.85 0. 90.2 (265) 58.93 02.9 92.2 (266) H Li Na K Rb Cs Fr
More informationBROOKLYN COLLEGE Department of Chemistry. Chemistry 1 Second Lecture Exam Nov. 27, Name Page 1 of 5
BROOKLYN COLLEGE Department of Chemistry Chemistry 1 Second Lecture Exam Nov. 27, 2002 Name Page 1 of 5 Circle the name of your lab instructor Kobrak, Zhou, Girotto, Hussey, Du Before you begin the exam,
More informationCircle the letters only. NO ANSWERS in the Columns!
Chemistry 1304.001 Name (please print) Exam 5 (100 points) April 18, 2018 On my honor, I have neither given nor received unauthorized aid on this exam. Signed Date Circle the letters only. NO ANSWERS in
More information(C) Pavel Sedach and Prep101 1
(C) Pavel Sedach and Prep101 1 (C) Pavel Sedach and Prep101 1 (C) Pavel Sedach and Prep101 2 (C) Pavel Sedach and Prep101 2 (C) Pavel Sedach and Prep101 3 (C) Pavel Sedach and Prep101 3 (C) Pavel Sedach
More informationIf anything confuses you or is not clear, raise your hand and ask!
CHM 1045 Dr. Light s Section December 10, 2002 FINAL EXAM Name (please print) Recitation Section Meeting Time This exam consists of six pages. Make sure you have one of each. Print your name at the top
More informationChemistry 185 Exam #2 - A November 5, Lab Day and Time: Instructions. 1. Do not open the exam until you are told to start.
Name: Lab Day and Time: Instructions 1. Do not open the exam until you are told to start. 2. This exam is closed note and closed book. You are not allowed to use any outside material while taking this
More informationCHEM 107 (Spring-2004) Exam 2 (100 pts)
CHEM 107 (Spring-2004) Exam 2 (100 pts) Name: ------------------------------------------------------------------------, SSN -------------------------------- LAST NAME, First (Circle the alphabet segment
More information7. Relax and do well.
CHEM 1215 Exam II John II. Gelder October 7, 1998 Name TA's Name Lab Section INSTRUCTIONS: 1. This examination consists of a total of 5 different pages. The last page includes a periodic table and a solubility
More informationCLASS TEST GRADE 11. PHYSICAL SCIENCES: CHEMISTRY Test 4: Matter and materials 1
CLASS TEST GRADE PHYSICAL SCIENCES: CHEMISTRY Test 4: Matter and materials MARKS: 45 TIME: hour INSTRUCTIONS AND INFORMATION. Answer ALL the questions. 2. You may use non-programmable calculators. 3. You
More informationM10/4/CHEMI/SPM/ENG/TZ1/XX+ CHEMISTRY. Wednesday 12 May 2010 (afternoon) 45 minutes INSTRUCTIONS TO CANDIDATES
M10/4/EMI/SPM/ENG/TZ1/XX+ 22106110 EMISTRY standard level Paper 1 Wednesday 12 May 2010 (afternoon) 45 minutes INSTRUTIONS TO ANDIDATES Do not open this examination paper until instructed to do so. Answer
More information7. Relax and do well.
CHEM 1215 Exam II John II. Gelder October 7, 1998 Name TA's Name Lab Section INSTRUCTIONS: 1. This examination consists of a total of 5 different pages. The last page includes a periodic table and a solubility
More informationCircle the letters only. NO ANSWERS in the Columns! (3 points each)
Chemistry 1304.001 Name (please print) Exam 4 (100 points) April 12, 2017 On my honor, I have neither given nor received unauthorized aid on this exam. Signed Date Circle the letters only. NO ANSWERS in
More information8. Relax and do well.
CHEM 1225 Exam III John III. Gelder April 8, 1999 Name TA's Name Lab Section INSTRUCTIONS: 1. This examination consists of a total of 7 different pages. The last two pages includes a periodic table and
More informationK. 27 Co. 28 Ni. 29 Cu Rb. 46 Pd. 45 Rh. 47 Ag Cs Ir. 78 Pt.
1 IA 1 ydrogen 1.01 Atomic number Element symbol Element name Atomic mass VIIIA 1 1.01 IIA IIIA IVA VA VIA VIIA 2 e 4.00 Metalloids 3 Li 6.94 4 Be 9.01 5 B 10.81 6 C 12.01 7 N 14.01 8 O 16.00 9 F 19.00
More informationFall 2011 CHEM Test 4, Form A
Fall 2011 CHEM 1110.40413 Test 4, Form A Part I. Multiple Choice: Clearly circle the best answer. (60 pts) Name: 1. The common constituent in all acid solutions is A) H 2 SO 4 B) H 2 C) H + D) OH 2. Which
More information8. Relax and do well.
CHEM 1314 Name Exam IV TA Name John IV. Gelder December 14, 1992 Lab Section INSTRUCTIONS: 1. This examination consists of a total of 9 different pages. The last three pages includes a periodic table and
More information8. Relax and do well.
CHEM 1014 Exam I John I. Gelder September 16, 1999 Name TA's Name Lab Section Please sign your name below to give permission to post your course scores on homework, laboratories and exams. If you do not
More informationPart 2. Multiple choice (use answer card). 90 pts. total. 3 pts. each.
1 Exam I CHEM 1303.001 Name (print legibly) Seat no. On my honor, I have neither given nor received unauthorized aid on this exam. Signed Date Part 1. Nomenclature. 10 pts. total. 2 pts. each. Fill in
More informationPOLYTECHNIC OF NAMIBIA
POLYTECHNIC OF NAMIBIA DEPARTMENT OF HEALTH SCIENCES BACHELOR OF ENVIRONMENTAL HEALTH SCIENCES HEALTH SCIENCE CHEMISTRY (HSC 511S) NQF level 5 SECOND OPPORTUNITY EXAMINATION November 2014 TIME: MARKS:
More informationCh. 9 NOTES ~ Chemical Bonding NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics.
Ch. 9 NOTES ~ Chemical Bonding NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics. I. Review: Comparison of ionic and molecular compounds Molecular compounds Ionic
More information8. Relax and do well.
CHEM 1314.03 Exam I John I. Gelder September 25, 1997 Name TA's Name Lab Section Please sign your name below to give permission to post, by the last 4 digits of your student I.D. number, your course scores
More informationM14/4/CHEMI/SPM/ENG/TZ1/XX CHEMISTRY. Monday 19 May 2014 (afternoon) 45 minutes INSTRUCTIONS TO CANDIDATES
M14/4/CEMI/SPM/ENG/TZ1/XX 22146110 CEMISTRY standard level Paper 1 Monday 19 May 2014 (afternoon) 45 minutes INSTRUCTIONS TO CANDIDATES Do not open this examination paper until instructed to do so. Answer
More informationUNIVERSITY OF CALGARY FACULTY OF SCIENCE MIDTERM EXAMINATION CHEMISTRY 353 READ ALL THE INSTRUCTIONS CAREFULLY
WEDNESDAY MARCH 9th, 2016 UNIVERSITY OF CALGARY FACULTY OF SCIENCE MIDTERM EXAMINATION CHEMISTRY 353 Version 1 Time: 2 Hours READ ALL THE INSTRUCTIONS CAREFULLY PLEASE WRITE YOUR NAME, STUDENT I.D. NUMBER
More information7. Relax and do well.
CHEM 1215 Exam II John II. Gelder October 13, 1999 Name TA's Name Lab Section INSTRUCTIONS: 1. This examination consists of a total of 5 different pages. The last page includes a periodic table and a solubility
More information8. Relax and do well.
CHEM 1225 Exam I John I. Gelder February 4, 1999 Name KEY TA's Name Lab Section Please sign your name below to give permission to post your course scores on homework, laboratories and exams. If you do
More informationCHEM 171 EXAMINATION 1. October 9, Dr. Kimberly M. Broekemeier. NAME: Key
CHEM 171 EXAMINATION 1 October 9, 008 Dr. Kimberly M. Broekemeier NAME: Key I A II A III B IV B V B VI B VII B VIII I B II B III A IV A V A VI A VII A inert gase s 1 H 1.008 Li.941 11 Na.98 19 K 9.10 7
More informationINSTRUCTIONS: CHEM Exam I. September 13, 1994 Lab Section
CHEM 1314.05 Exam I John I. Gelder September 13, 1994 Name TA's Name Lab Section Please sign your name below to give permission to post, by the last 4 digits of your student I.D. number, your course scores
More informationTRU Chemistry Contest Chemistry 12 May 21, 2003 Time: 90 minutes
TRU Chemistry Contest Chemistry 12 May 21, 2003 Time: 90 minutes Last Name First name School Teacher Please follow the instructions below. We will send your teacher a report on your performance. Top performers
More information2008 Academic Challenge
2008 Academic Challenge CHEMISTRY TEST - STATE FINALS - - This Test Consists of 40 Questions - - Chemistry Test Production Team Don DeCoste, University of Illinois at Urbana Champaign Author/Team Leader
More informationK. 27 Co. 28 Ni. 29 Cu Rb. 46 Pd. 45 Rh. 47 Ag Cs Ir. 78 Pt.
1 IA 1 ydrogen 1.01 Atomic number Element symbol Element name Atomic mass VIIIA 1 1.01 IIA IIIA IVA VA VIA VIIA 2 e 4.00 Metalloids 3 Li 6.94 4 Be 9.01 5 B 10.81 6 C 12.01 7 N 14.01 8 O 16.00 9 F 19.00
More informationChem 51, Spring 2015 Exam 8 (Chp 8) Use your Scantron to answer Questions There is only one answer for each Question. Questions are 2 pt each.
Chem 51, Spring 2015 Exam 8 (Chp 8) Name 120 pt Use your Scantron to answer Questions 1-32. There is only one answer for each Question. Questions are 2 pt each. CHP 8.1 Solutions are Mixtures 1. A saturated
More information2005 Academic Challenge
2005 Academic Challenge CHEMISTRY TEST - STATE FINALS Chemistry Test Production Team Don DeCoste, University of Illinois at Urbana - Champaign Author/Team Coordinator Gretchen Adams, University of Illinois
More information8. Relax and do well.
CHEM 1314.05 Exam II John II. Gelder October 18, 1994 Name TA's Name Lab Section INSTRUCTIONS: 1. This examination consists of a total of 9 different pages. The last three pages include a periodic table,
More informationCHEM 10123/10125, Exam 2
CHEM 10123/10125, Exam 2 March 7, 2012 (50 minutes) Name (please print) Please box your answers, and remember that significant figures, phases (for chemical equations), and units do count! 1. (13 points)
More informationChemistry Standard level Paper 1
Chemistry Standard level Paper 1 Thursday 12 May 2016 (morning) 45 minutes Instructions to candidates Do not open this examination paper until instructed to do so. Answer all the questions. For each question,
More informationChemistry 112, Fall 2006, Section 1 (Garman and Heuck) Final Exam A (100 points) 19 Dec 2006
Chemistry 112, Fall 2006, Section 1 (Garman and Heuck) (100 points) 19 Dec 2006 Name: YOU MUST: Put your name and student ID on the bubble sheet correctly. Put the exam version on the bubble sheet on the
More informationFaculty of Natural and Agricultural Sciences Chemistry Department. Semester Test 1. Analytical Chemistry CMY 283. Time: 120 min Marks: 100 Pages: 6
Faculty of Natural and Agricultural Sciences Chemistry Department Semester Test 1 Analytical Chemistry CMY 283 Date: 5 September 2016 Lecturers : Prof P Forbes, Dr Laurens, Mr SA Nsibande Time: 120 min
More informationChemistry 1 First Lecture Exam Fall Abbasi Khajo Levine Mathias Mathias/Ortiz Metlitsky Rahi Sanchez-Delgado Vasserman
Chemistry 1 First Lecture Exam Fall 2011 Page 1 of 9 NAME Circle the name of your recitation/lab instructor(s) Abbasi Khajo Levine Mathias Mathias/Ortiz Metlitsky Rahi Sanchez-Delgado Vasserman Before
More informationChem Exam 1. September 26, Dr. Susan E. Bates. Name 9:00 OR 10:00
Chem 1711 Exam 1 September 26, 2013 Dr. Susan E. Bates Name 9:00 OR 10:00 N A = 6.022 x 10 23 mol 1 I A II A III B IV B V B VI B VII B VIII I B II B III A IV A V A VI A VII A inert gases 1 H 1.008 3 Li
More informationFINAL EXAM April 26, 2004
CM 1045 (11:15 am Lecture) Dr. Light FINAL EXAM April 26, 2004 Name (please print) Check your recitation section: Sec. 21 5:30-6:20 pm (Popovic) Sec. 24 3:30-4:20 pm (Giunta) Sec. 22 6:30-7:20 pm (Popovic)
More informationThe Periodic Table. Periodic Properties. Can you explain this graph? Valence Electrons. Valence Electrons. Paramagnetism
Periodic Properties Atomic & Ionic Radius Energy Electron Affinity We want to understand the variations in these properties in terms of electron configurations. The Periodic Table Elements in a column
More information610B Final Exam Cover Page
1 st Letter of Last Name NAME: 610B Final Exam Cover Page No notes or calculators of any sort allowed. You have 3 hours to complete the exam. CHEM 610B, 50995 Final Exam Fall 2003 Instructor: Dr. Brian
More informationAtoms and the Periodic Table
Atoms and the Periodic Table Parts of the Atom Proton Found in the nucleus Number of protons defines the element Charge +1, mass 1 Parts of the Atom Neutron Found in the nucleus Stabilizes the nucleus
More informationThe Periodic Table of Elements
The Periodic Table of Elements 8 Uuo Uus Uuh (9) Uup (88) Uuq (89) Uut (8) Uub (8) Rg () 0 Ds (9) 09 Mt (8) 08 Hs (9) 0 h () 0 Sg () 0 Db () 0 Rf () 0 Lr () 88 Ra () 8 Fr () 8 Rn () 8 At (0) 8 Po (09)
More informationLab Day and Time: Instructions. 1. Do not open the exam until you are told to start.
Name: Lab Day and Time: Instructions 1. Do not open the exam until you are told to start. 2. This exam is closed note and closed book. You are not allowed to use any outside material while taking this
More informationFaculty of Natural and Agricultural Sciences Chemistry Department. Semester Test 1 MEMO. Analytical Chemistry CMY 283
Faculty of Natural and Agricultural Sciences Chemistry Department Semester Test 1 MEMO Analytical Chemistry CMY 283 Date: 5 September 2016 Lecturers : Prof P Forbes, Dr Laurens, Mr SA Nsibande Time: 90
More information8. Relax and do well.
CHEM 1314 3;30 pm Theory Exam III John III. Gelder November 13, 2002 Name TA's Name Lab Section INSTRUCTIONS: 1. This examination consists of a total of 8 different pages. The last page include a periodic
More informationNAME: FIRST EXAMINATION
1 Chemistry 64 Winter 1994 NAME: FIRST EXAMINATION THIS EXAMINATION IS WORTH 100 POINTS AND CONTAINS 4 (FOUR) QUESTIONS THEY ARE NOT EQUALLY WEIGHTED! YOU SHOULD ATTEMPT ALL QUESTIONS AND ALLOCATE YOUR
More informationNAME: SECOND EXAMINATION
1 Chemistry 64 Winter 1994 NAME: SECOND EXAMINATION THIS EXAMINATION IS WORTH 100 POINTS AND CONTAINS 4 (FOUR) QUESTIONS THEY ARE NOT EQUALLY WEIGHTED! YOU SHOULD ATTEMPT ALL QUESTIONS AND ALLOCATE YOUR
More informationCHEM 172 EXAMINATION 1. January 15, 2009
CHEM 17 EXAMINATION 1 January 15, 009 Dr. Kimberly M. Broekemeier NAME: Circle lecture time: 9:00 11:00 Constants: c = 3.00 X 10 8 m/s h = 6.63 X 10-34 J x s J = kg x m /s Rydberg Constant = 1.096776 x
More informationPHYSICAL SCIENCES GRADE : 10
PHYSICAL SCIENCES GRADE : 0 TIME : hour TOTAL : 75 INSTRUCTIONS AND INFORMATION. Write your full name on your answer book in the appropriate place. 2. The question paper consists of SEVEN questions. Answer
More informationCHEM 130 Exp. 8: Molecular Models
CHEM 130 Exp. 8: Molecular Models In this lab, we will learn and practice predicting molecular structures from molecular formulas. The Periodic Table of the Elements IA 1 H IIA IIIA IVA VA VIA VIIA 3 5
More informationCHEM 108 (Spring-2008)
CHEM 108 (Spring-2008) Final Exam (106 pts) Name: --------------------------------------------------------------------------, CLID # -------------------------------- LAST NAME, First (Circle the alphabet
More informationAtomic Structure & Interatomic Bonding
Atomic Structure & Interatomic Bonding Chapter Outline Review of Atomic Structure Atomic Bonding Atomic Structure Atoms are the smallest structural units of all solids, liquids & gases. Atom: The smallest
More information(please print) (1) (18) H IIA IIIA IVA VA VIA VIIA He (2) (13) (14) (15) (16) (17)
CHEM 10113, Quiz 3 September 28, 2011 Name (please print) All equations must be balanced and show phases for full credit. Significant figures count, show charges as appropriate, and please box your answers!
More informationCHEM 108 (Fall-2003) Exam Final (100 pts)
CHEM 108 (Fall-2003) Exam Final (100 pts) Name: -------------------------------------------------------------------------------, SSN -------------------------------- LAST NAME, First (Circle the alphabet
More informationChem GENERAL CHEMISTRY I MIDTERM EXAMINATION
Concordia University CHEM 205 Fall 2009, B LAST NAME: FIRST NAME: STUDENT ID: Chem 205 - GENERAL CHEMISTRY I MIDTERM EXAMINATION PLEASE READ THIS BOX WHILE WAITING TO START INSTRUCTIONS: Calculators are
More informationChem 401 Unit 2 Exam Spr 2018 (Acids/ Bases/ General Equilibria /Acid-Base Equilibria)
Name: Date: Exam #: _ Chem 401 Unit 2 Exam Spr 2018 (Acids/ Bases/ General Equilibria /Acid-Base Equilibria) Multiple Choice Identify the letter of the choice that best completes the statement or answers
More informationChemistry Standard level Paper 1
M17/4/EMI/SPM/ENG/TZ1/XX hemistry Standard level Paper 1 Thursday 11 May 2017 (afternoon) 45 minutes Instructions to candidates Do not open this examination paper until instructed to do so. Answer all
More informationThe Periodic Table of the Elements
The Periodic Table of the Elements All matter is composed of elements. All of the elements are composed of atoms. An atom is the smallest part of an element which still retains the properties of that element.
More informationInstructions. 1. Do not open the exam until you are told to start.
Name: Lab Day and Time: Instructions 1. Do not open the exam until you are told to start. 2. This exam is closed note and closed book. You are not allowed to use any outside material while taking this
More informationOur country, our future 525/1 S6 CHEMISTRY PAPER 1 DURATION: 2 HOUR 45 MINUTES
1 Our country, our future 525/1 S6 CHEMISTRY Exam 10 PAPER 1 DURATION: 2 HOUR 45 MINUTES For Marking guide contact and consultations: Dr. Bbosa Science 0776 802709, Instructions - This paper consists of
More informationScholarship 2006 Chemistry
For Supervisor s S 9 3 1 0 2 Scholarship 2006 Chemistry 2.00 pm Saturday 25 November 2006 Time allowed: Three hours Total Marks: 48 Check that the National Student Number (NSN) on your admission slip is
More information8. Relax and do well.
EM 1515.001-006 Exam II John II. Gelder March 5, 2002 Name TA's Name Section INSTRUTIONS: 1. This examination consists of a total of 8 different pages. The last three pages include a periodic table, a
More informationChem 112, Fall 05 Exam 2a
Name: YOU MUST: Put your name and student ID on the bubble sheet correctly. Put all your answers on the bubble sheet. Please sign the statement on the last page of the exam. Please make sure your exam
More informationUNIVERSITY OF CALGARY FACULTY OF SCIENCE MIDTERM EXAMINATION CHEMISTRY 353 READ ALL THE INSTRUCTIONS CAREFULLY
TUESDAY MARCH 3rd, 2015 UNIVERSITY OF CALGARY FACULTY OF SCIENCE MIDTERM EXAMINATION CHEMISTRY 353 Version 1 Time: 2 Hours READ ALL THE INSTRUCTIONS CAREFULLY PLEASE WRITE YOUR NAME, STUDENT I.D. NUMBER
More informationEssential Chemistry for Biology
1 Chapter 2 Essential Chemistry for Biology Biology and Society: More Precious than Gold A drought is a period of abnormally dry weather that changes the environment and one of the most devastating disasters.
More informationMade the FIRST periodic table
Made the FIRST periodic table 1869 Mendeleev organized the periodic table based on the similar properties and relativities of certain elements Later, Henri Moseley organized the elements by increasing
More informationM09/4/CHEMI/HPM/ENG/TZ2/XX+ CHEMISTRY. Monday 18 May 2009 (afternoon) 1 hour INSTRUCTIONS TO CANDIDATES
M09/4/CEMI/PM/ENG/TZ/XX+ 096113 CEMISTRY igher level Paper 1 Monday 18 May 009 (afternoon) 1 hour INSTRUCTIONS TO CANDIDATES Do not open this examination paper until instructed to do so. Answer all the
More information8. Relax and do well.
CHEM 34.02 and 34.03 Name Exam III John III. Gelder TA's Name November 5, 2000 Lab Section INSTRUCTIONS:. This examination consists of a total of 9 different pages. The last three pages include a periodic
More informationChem October 31, Dr. Susan E. Bates
Chem 1711 Exam 2 ID#: 2013171 October 31, 2013 Dr. Susan E. Bates Name 9:00 OR 10:00 PV = nrt 1 atm = 760 mmhg = 101.3 kpa u = (3RT/M m ) 1/2 R = 0.08206 L atm K 1 mol 1 OR 8.314 J K 1 mol 1 22.4 L/mol
More informationSCIENCE 1206 UNIT 2 CHEMISTRY. September 2017 November 2017
SCIENCE 1206 UNIT 2 CHEMISTRY September 2017 November 2017 UNIT OUTLINE 1. Review of Grade 9 Terms & the Periodic Table Bohr diagrams Evidence for chemical reactions Chemical Tests 2. Naming & writing
More informationNucleus. Electron Cloud
Atomic Structure I. Picture of an Atom Nucleus Electron Cloud II. Subatomic particles Particle Symbol Charge Relative Mass (amu) protons p + +1 1.0073 neutrons n 0 1.0087 electrons e - -1 0.00054858 Compare
More information