Chem Exam 1. September 26, Dr. Susan E. Bates. Name 9:00 OR 10:00
|
|
- Randall Wright
- 5 years ago
- Views:
Transcription
1 Chem 1711 Exam 1 September 26, 2013 Dr. Susan E. Bates Name 9:00 OR 10:00 N A = x 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 Li Na K Rb Cs Fr (223) 4 Be Mg Ca Sr Ba Ra Sc Y * La * Ac (227) 22 Ti Zr Hf Rf (261) 23 V Nb Ta Db (262) 24 Cr Mo W Sg (263) 25 Mn Tc Re Bh (262) 26 Fe Ru Os Hs (265) 27 Co Rh Ir Mt (266) 28 Ni Pd Pt (269) 29 Cu Ag Au (272) 30 Zn Cd Hg (277) 5 B Al Ga In Tl ? 6 C Si Ge Sn Pb (289) 7 N P As Sb Bi O S Se Te Po (210) 9 F Cl Br I At (210) 2 He Ne Ar Kr Xe Rn (222) 58 Ce Th Pr Pa (231) 60 Nd U Pm (147) 93 Np (237) 62 Sm Pu (242) 63 Eu Am (243) 64 Gd Cm (247) 65 Tb Bk (247) 66 Dy Cf (251) 67 Ho Es (254) 68 Er Fm (253) 69 Tm Md (256) 70 Yb No (254) 71 Lu Lr (257)
2 Chem 1711: Exam 1 Part I (46 points): Short Answer. Name 1. Give the missing IUPAC name or chemical formula for each of the following: FeBr 2 4H 2 O nickel (III) hydroxide IF 5 yttrium chlorite HC 2 H 3 O 2 (aq) dinitrogen tetroxide 2. a. Give the name of one transition metal found in the 5 th period of the periodic table. b. Give the name of one metalloid in group VA of the periodic table. c. Consider the element with 19 protons in its nucleus. This element is best described as which one of the following? halogen noble gas alkali metal alkaline earth metal 3. Consider the ion 121 Sn 2+. How many protons, neutrons & electrons are there? p n e 4. Balance the following chemical equation: IBr + NH 3 NI 3 + NH 4 Br 5. a. Consider 65 molecules of P 2 O 5. This collection of molecules contains how many phosophorus atoms? How many atoms in total are contained in this sample? b. A mol sample of P 2 O 5 contains how many molecules? c. What is the mass of 1 P 2 O 5 molecule? Circle the one best answer below amu g amu g amu g 6. a. Which of the following numbers has (unambiguously) 4 significant figures? Circle the one best answer below: x x 10 4 b. Give the answer to the following calculation with the correct number of significant figures: = molecules of NH 3 and 35 molecules of O 2 are combined and allowed to react accoring to the following equation: 4 NH 3 (g) + 5 O 2 (g) 4 NO (g) + 6 H 2 O (g) a. Identify the limiting reactant. b. What is the maximum number of water molecules that can form? c. How many molecules of the excess reactant remain unconsumed when the reaction is complete?
3 8. Perform the following unit conversions: a lb/in 2 = kg/m 2 b kj = MJ 1 lb = g; 1 in = 2.54 cm 9. A 750 g sample of a compound composed of only manganese and oxygen is analyzed and found to contain 210 g O. Determine the mass percent manganese in this compound. Part II (39 points): Multiple Choice. For each of the following questions, indicate the one best answer by bubbling in the appropriate letter on the provided Scan Tron answer sheet. 1. Calculate the average atomic mass for fictional element El given the following data: symbol isotope mass percent abundance 121 El amu El amu El amu a amu b amu c amu d amu e amu 2. Who is credited with establishing the nuclear structure of the atom? a. J.J. Thomson b. Joseph Proust c. John Dalton d. Ernest Rutherford e. Antoine Lavoisier 3. Which one of the following statements about isotopes of a particular element is not true? a. Each unique isotope has a different atomic mass. b. Each unique isotope has a different atomic number. c. Each unique isotope has a different number of neutrons. d. Each unique isotope has a different number of nucleons. e. In neutral atoms of each isotope, the number of electrons equals the number of protons. 4. The term that is related to the reproducability of a measurement is a. precision b. accuracy c. qualitative d. intensive e. physical 5. A g sample of an element contains x atoms. Identify this element. a. I b. Ag c. La d. Pd e. Rh
4 6. A 19.0 g sample of lithium is burned in air and converted completely to lithium oxide. The mass of lithium oxide formed must be a. exactly 19.0 g b. less than 19.0 g c. more than 19.0 g d. equal to 30.0 g e. there is not enough information provided to answer this question 7. Which of the following are binary molecular compounds? i. C 5 H 10 ii. HNO 2 iii. Al 2 O 3 iv. Cl 2 O 7 v. Na 3 PO 4 a. i, iii, iv b. i, ii, iv c. ii, iii, v d. i and iv e. none of these 8. Which one of the following is the greatest? a. number of nitrogen atoms in 1 mol of ntirogen in its elemental form b. number of formula units in 1 mol of ammonium phosphate c. number of ammonium ions in 1 mol of ammonium phosphate d. number of oxygen atoms in 1 mol of ammonium phosphate e. number of molecules in 1 mol of nitrogen dioxide 9. A compound has C 3 H 5 O 2 as its empirical formula. Which one of the following can not be this compound s molecular formula? a. C 3 H 5 O 2 b. C 9 H 10 O 6 c. C 12 H 20 O 8 d. C 6 H 10 O 4 e. all of these are possible 10. Consider the following reaction: I 2 (s) + 2 Na 2 S 2 O 3 (aq) Na 2 S 4 O 6 (aq) + 2 NaI (aq). Determine the mass (in g) of I 2 required to react completely with g Na 2 S 2 O 3. For I 2, molar mass = g/mol; for Na 2 S 2 O 3, molar mass = g/mol. a g b g c g d g e g 11. Calculate the density (in g/cm 3 ) of technetium if mol occupies a volume of 2.11 cm 3. a g/cm 3 b g/cm 3 c g/cm 3 d g/cm 3 e g/cm Which one of the following statements about lab measurements is correct? a. A 50-mL burette is not as precise as a 50-mL graduated cylinder. b. Extrapolation is a more reliable method of estimation than interpolation. c. In a linear graph of time vs. distance, the slope can have units of cm/s. d. Standard deviation is an indication of the accuracy of a set of measurements. e. A 25-mL pipette is precise to 4 significant figures.
5 13. Based on the observaitons you made during the Reactions and Solubility lab, which one of the following ions is generally not soluble? a. Na + b. K + c. NH 4 + d. Ag + e. NO 3 Part III (15 points): Problems. Work each of the following problems. Show all work clearly; work with units in all steps; report your answers with correct units and significant figures. No partial credit will be given if I cannot follow your work. 1. A compound is composed of potassium, chromium, and oxygen. After analysis, it is found to be % potassium and 35.35% chromium by mass. Determine the empirical formula of this compound. 2. Consider saccharin (C 7 H 5 NO 3 S) to answer a c below. a. Determine the molar mass of saccharin. Include units with your answer. b. Determine the amount (in mol) of saccharin that contains 2.8 x carbon atoms. mol c. Determine the mass (in g) of oxygen in 825 mg saccharin. g 3. Consider the following reaction: Fe 3 O 4 (s) + 4 H 2 (g) 3 Fe (s) + 4 H 2 O (l) kg Fe 3 O 4 and g H 2 are combined and allowed to react. Determine the mass (in g) of iron collected if the reaction proceeds in 88.22% yield. g
Chem 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 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 informationReporting Category 1: Matter and Energy
Name: Science Teacher: Reporting Category 1: Matter and Energy Atoms Fill in the missing information to summarize what you know about atomic structure. Name of Subatomic Particle Location within the Atom
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 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 information5 questions, 3 points each, 15 points total possible. 26 Fe Cu Ni Co Pd Ag Ru 101.
Physical Chemistry II Lab CHEM 4644 spring 2017 final exam KEY 5 questions, 3 points each, 15 points total possible h = 6.626 10-34 J s c = 3.00 10 8 m/s 1 GHz = 10 9 s -1. B= h 8π 2 I ν= 1 2 π k μ 6 P
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 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 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 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 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 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 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 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 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 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 informationReporting Category 1: Matter and Energy
Name: Science Teacher: Reporting Category 1: Matter and Energy Atoms 8.5A Fill in the missing information to summarize what you know about atomic structure. Name of Subatomic Particle Location within the
More informationSpeed of light c = m/s. x n e a x d x = 1. 2 n+1 a n π a. He Li Ne Na Ar K Ni 58.
Physical Chemistry II Test Name: KEY CHEM 464 Spring 18 Chapters 7-11 Average = 1. / 16 6 questions worth a total of 16 points Planck's constant h = 6.63 1-34 J s Speed of light c = 3. 1 8 m/s ħ = h π
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 information8/30/2010. The Components of Matter Chapter 2. Element, Atom, Compound, and Molecule. Elements, Compounds, and Mixtures
The Components of Matter Chapter 2 Element, Atom, Compound, and Molecule CHEMICAL ELEMENTS - pure substances that cannot be decomposed by ordinary means to other substances. An ATOM is the smallest particle
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 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 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 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 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 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 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 informationMANY ELECTRON ATOMS Chapter 15
MANY ELECTRON ATOMS Chapter 15 Electron-Electron Repulsions (15.5-15.9) The hydrogen atom Schrödinger equation is exactly solvable yielding the wavefunctions and orbitals of chemistry. Howev er, the Schrödinger
More informationDURATION: 2 HOUR 45 MINUTES
1 Exam 9 Our country, our future 525/1 S6 CHEMISTRY PAPER 1 DURATION: 2 HOUR 45 MINUTES For Marking guide contact and consultations: Dr. Bbosa Science 0776 802709. Answer all question in part I and six
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 information6.3 Classifying Elements with the Periodic Table
6.3 Classifying Elements with the Periodic Table The Periodic Table was developed by scientists to organize elements in such a way as to make sense of the growing information about their properties. The
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 informationAdvanced Chemistry. Mrs. Klingaman. Chapter 5: Name:
Advanced Chemistry Mrs. Klingaman Chapter 5: The Periodic Law Name: _ Mods: Chapter 5: The Periodic Law Reading Guide 5.1 History of the Periodic Table (pgs. 125-129) 1) What did Dimitri Mendeleev notice
More information