COLLEGE OF ENGINEERING TEST 1 TRIMESTER 2 ACADEMIC YEAR 2010/11
|
|
- Bethany Craig
- 5 years ago
- Views:
Transcription
1 COLLEGE OF ENGINEERING TEST 1 TRIMESTER 2 ACADEMIC YEAR 2010/11 PROGRAM : FOUNDATION IN ENGINEERING COURSE : CHEMISTRY I COURSE CODE : CHEF 114 DATE : 10 th December 2010 DURATION : 1.5 HOUR NAME : STUDENT ID: SECTION: LECTURER : Instructions For Candidates : 1. Answer ALL the questions. 2. Please mark the answers for Section A in the answer sheet. Write the answers for Section B in the space provided. 3. All calculations in Section B must be shown clearly in order to get full marks. 4. No reference books, papers and mobile phones are allowed into the examination hall. 5. Answer Sheet for MCQ (Section A) and the Periodic Table of the elements are provided. DO NOT OPEN THIS QUESTION PAPER UNTIL YOU ARE INSTRUCTED TO DO SO This question paper has 10 pages including this page. Attendance List CHEF114 Test 1 (10 Dec 2010) Seat No: NAME : STUDENT ID: SECTION: LECTURER : SIGNATURE: 1
2 SECTION A Multiple Choice Questions. There is ONE best response to each question. Read all responses, choose the best one and write it on your answer booklet. Blacken the circle on the answer sheet on page 9 corresponding to this answer. Answer ALL questions. (1 mark for each question) 1. An unused flashbulb contains magnesium and oxygen. After it has been used, the contents are changed to magnesium oxide but the total mass does not change. This observation can best be explained by the A. Law of Definite Proportion. B. Law of Multiple Proportions. C. Law of Conservation of Mass. D. Avogadro s Law. E. Ideal Gas Law. 2. In Rutherford s gold foil experiment, when alpha particles are used to bombard the gold foil, most of the alpha particles pass through undeflected. This result indicates that most of the volume of a gold atom consists of A. deuterons. B. neutrons. C. protons. D. empty space. E. dense space. 3. The atomic number of an element equals to A. its atomic mass divided by two. B. the number of protons. C. the number of neutrons. D. the number of protons plus neutrons. E. the charge of the element. 2
3 4. Which of the following statements are true about a sample of sulfur (S) and a sample of oxygen gas (O 2 ) if the two samples are of equal mass? I. The number of electrons in the two samples is about the same. II. The number of protons in the two samples is about the same. III. The number of atoms in the two samples is about the same. IV. There are roughly twice as many sulfur atoms as oxygen atoms. V. There are roughly twice as many oxygen atoms as sulfur atoms. A. I, II, III B. I, II, and V C. II, III, IV D. III, IV, V E. II, III, V 5. Which one of the following does NOT represent 1.00 mol of the indicated substance? A C atoms D g Zn B g Fe E Fe atoms C g C 6. Which of the following equations does NOT represent a redox reaction? A. 2Al + 6HCl 3H 2 + 2AlCl 3 B. 2H 2 O 2H 2 + O 2 C. 2NaCl + Pb(NO 3 ) 2 PbCl 2 + 2NaNO 3 D. 2NaI + Br 2 2NaBr + I 2 E. Cu(NO 3 ) 2 + Zn Zn(NO 3 ) 2 + Cu 3
4 7. A 50.0 ml sample of M ammonium nitrate (NH 4 NO 3 ) is diluted with water to a total volume of ml. What is the ammonium nitrate concentration in the resulting solution? A M B M C M D M E M 8. How does the volume of 1mol of an ideal gas change if the temperature and the pressure are both decreased by a factor of four? A. decreases by four times B. decreases by sixteen times C. increases by four times D. increases by sixteen times E. remains unchanged 9. A flask contains O 2 at 25 C and 1.00 atm. Which of the statements is TRUE? A. All O 2 molecules are moving at the same speed. B. An increase in temperature will cause the average kinetic energy to increase. C. If the average speed doubles, the average kinetic energy decreases by a factor of 4. D. The average kinetic energy depends only on the pressure. E. none of the above. 10. Which of the following gases effuses at the slowest rate? A. Ar B. SF 6 C. F 2 D. Xe E. CH 4 4
5 SECTION B Answer ALL the questions in this section. Show your calculations clearly. All work should be done within the space provided in this question booklet. Question 1 (a) The element oxygen has three (3) naturally occurring isotopes with 8, 9 and 10 neutrons in the nucleus, respectively. (i) (ii) Write the full chemical symbols for these three isotopes. State one (1) similarity and one (1) difference between these isotopes. [3 marks] [2 marks] Answer: (i) ; ; Note to examiner: 1 point each for correct full chemical symbols, give ½ point if the element is correct but incomplete mass number or atomic number. No point given if the symbol, mass number or atomic number is wrong. (ii) Possible answers are shown in the table below. Similarities Differences All isotopes are atoms of the same elements. All isotopes have the same atomic number (or the same number of protons). All isotopes will have the same electron arrangements. Each isotope has different number of neutrons. Each isotope has different mass number. Each isotope has different atomic mass. 5
6 (b) Fill in the table below with the correct chemical formulas: [5 marks] Name Nitrogen trifluoride Copper(I) cyanide Chemical formula NF 3 CuCN Iodic acid HIO 3 Silver chromate Nickel(II) nitrate hexahydrate Ag 2 CrO 4 Ni(NO 3 ) 2 6H 2 O Question 2 Ethyl acetate, CH 3 CO 2 C 2 H 5, is the solvent in many fingernail polish removers. It is prepared by the reaction of ethanol, C 2 H 5 OH, with acetic acid, CH 3 CO 2 H; the other product is water. A small amount of sulfuric acid, H 2 SO 4 is used to accelerate the reaction, but the sulfuric acid is not consumed and does not appear in the balanced equation. Suppose you are given 10.0 ml each of acetic acid and ethanol: [Given: The densities of acetic acid, ethanol and ethyl acetate are g/ml, g/ml and g/ml, respectively. The molar masses of acetic acid, ethanol and ethyl acetate are g/mol, 46.07g/mol, and g/mol, respectively]. C 2 H 5 OH + CH 3 CO 2 H CH 3 CO 2 C 2 H 5 + H 2 O (a) (b) (c) Which is the limiting reactant in this reaction? [5 marks] How many ml of ethyl acetate can be prepared using this reaction? [3 marks] Which is the excess reactant in this reaction? How many moles of the excess reactant remains at the end of this reaction? [2 marks] 6
7 Answer: (a) Density = Mass / volume (½) Mass = density x volume 1 mol C 2 H 5 OH C 2 H 5 OH: g/ml x 10 ml = g x = mol (½) g C 2 H 5 OH 1 mol CH 3 CO 2 H CH 3 CO 2 H: g/ml x 10 ml = g x = mol (½) g CH 3 CO 2 H All the coefficients are 1 in the balanced equation. Mol of C 2 H 5 OH < mol of CH 3 CO 2 H, Then, (½) Ethanol (C 2 H 5 OH) is limiting reactant. (b) mol C 2 H 5 OH x 1 mol CH 3 CO 2 C 2 H 5 x g CH 3 CO 2 C 2 H 5 (½) 1 mol C 2 H 5 OH 1 mol CH 3 CO 2 C 2 H 5 = 15.1 g CH 3 CO 2 C 2 H 5 Volume = Mass/density = 15.1 g x (½) 1 ml CH 3 CO 2 C 2 H g CH 3 CO 2 C 2 H 5 = 16.8 ml CH 3 CO 2 C 2 H 5 (c) Excess reactant is acetic acid (CH 3 CO 2 H) mol CH 3 CO 2 H mol CH 3 CO 2 H = mol CH 3 CO 2 H excess Question 3 (a) Combining Boyle s Law, Charles Law and Avogadro s Law gives the ideal gas equation. Derived the ideal gas equation using the above three laws. [5 marks] 7
8 (b) Acetylene, C 2 H 2, is an important fuel in welding. It is produced in the laboratory when calcium carbide, CaC 2, reacts with water: CaC 2 (s) + 2H 2 O(l) C 2 H 2 (g) + Ca(OH) 2 (s) Ans: 3 (a) A sample of acetylene, C 2 H 2 was collected over water at 23 o C. The total gas pressure was 748 mmhg and the volume was 543 ml. At 23 o C, the vapour pressure of water is 21 mmhg. What mass of acetylene in g was collected? [5 marks] Boyle s Law: PV = constant (½) Charles Law: V/T = constant (½) Avogadro s Law: n/v = constant (½) From these three equations V α 1/P ; V α T and V α n Therefore V α nt/p (½) Rearranging : PV/T α n (1) (½) Or PV/T = nr (R is the Gas constant) (½) PV = nrt (1) 3 (b) The total pressure is the sum of the partial pressures due to C2H2(g) and H2O(g): Ptotal = 748 mmhg = PH2O + PC2H2 = (21 mmhg) + PC2H2 PC2H2 = (748 21) = 727 mmhg. (½) Changing to atm unit; = 727mmHg / 760mmHg = atm. (½) Using the ideal gas law, PV = nrt, the number of moles of C2H2 formed is: n = PV (½) RT = (0.957atm) (0.543L) (1) ( Latm/K.mol) (( )K) = mol (1) The molar mass of C2H2 is g/mol. This amount therefore corresponds to a mass of, mass = number of moles molar mass = mol g/mol (½) = g (1) 8
9 Name : Section : Student ID : Lecturer : Answer Sheet for Multiple Choice Questions (Section A). Please use 2B pencil to fill the circle completely. Example : B D E TABLE OF CONSTANTS Avogadro's number = x /mol Gas constant, R = L.atm/ K.mol 1 atm = 760 mmhg = 760 torr = 101,325 Pa Gas constant, R = J/ K.mol 1 J = 1 kg. m 2 / s 2 1 L.atm = J Specific heat of water = J/g. C 9
10 10 PERIODIC TABLE 1 1A 18 8A 1 H A 13 3A 14 4A 15 5A 16 6A 17 7A 2 He Li Be B C N O F Ne Na Mg B 4 4B 5 5B 6 6B 7 7B B 9B 10B 11 1B 12 2B 13 Al Si P S Cl Ar K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po (209) 85 At (210) 86 Rn (222) 87 Fr (223) 88 Ra (226) 89 Ac (227) 104 Rf (261) 105 Db (262) 106 Sg (266) 107 Bh (264) 108 Hs (269) 109 Mt (268) 110 Ds (269) 58 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)
Last 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 108 (Spring-2008) Exam. 3 (105 pts)
CHEM 08 (Spring-008) Exam. (05 pts) Name: --------------------------------------------------------------------------, CLID # -------------------------------- LAST NAME, First (Circle the alphabet segment
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 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 informationRadiometric Dating (tap anywhere)
Radiometric Dating (tap anywhere) Protons Neutrons Electrons Elements on the periodic table are STABLE Elements can have radioactive versions of itself called ISOTOPES!! Page 1 in your ESRT has your list!
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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 informationChemistry 431 Practice Final Exam Fall Hours
Chemistry 431 Practice Final Exam Fall 2018 3 Hours R =8.3144 J mol 1 K 1 R=.0821 L atm mol 1 K 1 R=.08314 L bar mol 1 K 1 k=1.381 10 23 J molecule 1 K 1 h=6.626 10 34 Js N A = 6.022 10 23 molecules mol
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 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 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 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. 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 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 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 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 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 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 informationCHEM 10113, Quiz 5 October 26, 2011
CHEM 10113, Quiz 5 October 26, 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 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 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 informationHANDOUT SET GENERAL CHEMISTRY II
HANDOUT SET GENERAL CHEMISTRY II Periodic Table of the Elements 1 2 3 4 5 6 7 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 IA VIIIA 1 2 H He 1.00794 IIA IIIA IVA VA VIA VIIA 4.00262 3 Li 6.941 11 Na 22.9898
More informationK. 27 Co. 28 Ni. 29 Cu Rb. 46 Pd. 45 Rh. 47 Ag Cs Ir. 78 Pt.
1 IA 1 H Hydrogen 1.01 Atomic number Element symbol Element name Atomic mass VIIIA 1 H 1.01 IIA IIIA IVA VA VIA VIIA 2 He 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
More informationB. Characteristics of Gases assume volume and shape of container very compressible mix evenly and completely lower density than liquids and solids
Chapter 5: Gases Laws for gases are simpler than for liquids and solids. The behavior of gases is predictable. 5.1 Substances that exist as gases Air - 78 % N2; 21 % O2; 1 % other (including CO2 which
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 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 informationUsing the Periodic Table
MATH SKILLS TRANSPARENCY WORKSHEET Using the Periodic Table 6 Use with Chapter 6, Section 6.2 1. Identify the number of valence electrons in each of the following elements. a. Ne e. O b. K f. Cl c. B g.
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 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 informationChem 1711 Exam 1. Dr. Susan E. Bates. Name 9:00 OR 10:00
Chem 1711 Exam 1 September 25, 2014 Dr. Susan E. Bates ID#: 2014171 Name 9:00 OR 10:00 Please do not remove this page. The periodic table, constants, and equations you may need are on the last page of
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 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 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 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 informationGuide to the Extended Step-Pyramid Periodic Table
Guide to the Extended Step-Pyramid Periodic Table William B. Jensen Department of Chemistry University of Cincinnati Cincinnati, OH 452201-0172 The extended step-pyramid table recognizes that elements
More informationHANDOUT SET GENERAL CHEMISTRY I
HANDOUT SET GENERAL CHEMISTRY I Periodic Table of the Elements 1 2 3 4 5 6 7 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 IA VIIIA 1 2 H He 1.00794 IIA IIIA IVA VA VIA VIIA 4.00262 3 Li 6.941 11 Na 22.9898
More informationCHM 101 PRACTICE TEST 1 Page 1 of 4
CHM 101 PRACTICE TEST 1 Page 1 of 4 Please show calculations (stuffed equations) on all mathematical problems!! On the actual test, "naked answers, with no work shown, will receive no credit even if correct.
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 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 informationChapter 12 The Atom & Periodic Table- part 2
Chapter 12 The Atom & Periodic Table- part 2 Electrons found outside the nucleus; negatively charged Protons found in the nucleus; positive charge equal in magnitude to the electron s negative charge Neutrons
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 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 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 informationPLEASE PRINT YOUR NAME IN BLOCK LETTERS. Practice Exam 3. Last 4 Digits of USC ID:
Chemistry 105 B Practice Exam 3 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 1 18 2 14 3
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 126 Final Examination, Prof. Hanson, May, Section B or D (circle one) Seat Coordinate Name
Chemistry 126 Final Examination, Prof. Hanson, May, 2004 Section B or D (circle one) Seat Coordinate Name DO NOT OPEN THIS EXAM UNTIL INSTRUCTED TO DO SO Each asterisk () is 5 points. There are 40 s, for
More information9/20/2017. Elements are Pure Substances that cannot be broken down into simpler substances by chemical change (contain Only One Type of Atom)
CAPTER 6: TE PERIODIC TABLE Elements are Pure Substances that cannot be broken down into simpler substances by chemical change (contain Only One Type of Atom) The Periodic Table (Mendeleev) In 1872, Dmitri
More informationDO NOW: Retrieve your projects. We will be reviewing them again today. Textbook pg 23, answer questions 1-3. Use the section 1.2 to help you.
DO NOW: Retrieve your projects. We will be reviewing them again today. Textbook pg, answer questions. Use the section. to help you. Chapter test is FRIDAY. The Periodic Table of Elements 8 Uuo Uus Uuh
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 information7. Relax and do well.
CHEM 1014 Exam III John III. Gelder November 18, 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 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 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 informationCHEM 108 (Spring-2008)
CHEM 108 (Spring-2008) Final Exam (106 pts) Name: --------------------------------------------------------------------------, CLID # -------------------------------- LAST NAME, First (Circle the alphabet
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 informationModified from: Larry Scheffler Lincoln High School IB Chemistry 1-2.1
Modified from: Larry Scheffler Lincoln High School IB Chemistry 1-2.1 The development of the periodic table brought a system of order to what was otherwise an collection of thousands of pieces of information.
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 information1 Genesis 1:1. Chapter 10 Matter. Lesson. Genesis 1:1 In the beginning God created the heavens and the earth. (NKJV)
1 Genesis 1:1 Genesis 1:1 In the beginning God created the heavens and the earth. (NKJV) 1 Vocabulary Saturated having all the solute that can be dissolved at that temperature Neutron a particle with no
More informationWhat is the periodic table?
The periodic table of the elements represents one of the greatest discoveries in the history of science that certain elements, the basic chemical substances from which all matter is made, resemble each
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 informationWhy all the repeating Why all the repeating Why all the repeating Why all the repeating
Why all the repeating Why all the repeating Why all the repeating Why all the repeating Patterns What Patterns have you observed in your life? Where to Get Help If you don t understand concepts in chapter
More informationSecondary Support Pack. be introduced to some of the different elements within the periodic table;
Secondary Support Pack INTRODUCTION The periodic table of the elements is central to chemistry as we know it today and the study of it is a key part of every student s chemical education. By playing the
More informationA little history. When and How? Sir William Ramsey. ü 12/5/13. ü 1. Who put together the first useable Periodic Table?
ü // A little history Johahann Dobereiner (80-89) o Triads John Newlands (8-898) o Law of Octaves Who put together the first useable ic Table? Mendeleev you remember him right? When and How? You know it
More informationElement Cube Project (x2)
Element Cube Project (x2) Background: As a class, we will construct a three dimensional periodic table by each student selecting two elements in which you will need to create an element cube. Helpful Links
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 informationChemistry 171 Exam 1. January 13, Name. Periodic Table of the Elements
Chemistry 171 Exam 1 January 13, 2011 Name N A = 6.022 x 10 23 1 kg = 2.2046 lb 1 in = 2.54 cm 1 L = 1.057 qt 1 gal = 4 qt ( o F -32 0 F) x (5 0 C/9 0 F) = 0 C Periodic Table of the Elements I A II A III
More information