8. Relax and do well.
|
|
- Maximillian Morris
- 5 years ago
- Views:
Transcription
1 CHEM and 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 table, some useful equations, a table of standard heats of formation and a solubility table. All work should be done in this booklet. 2. PRINT your name, TA's name and your lab section number now in the space at the top of this sheet. DO NOT SEPARATE THESE PAGES. 3. Answer all questions that you can and whenever called for show your work clearly. Your method of solving problems should pattern the approach used in lecture. You do not have to show your work for the multiple choice or short answer questions. 4. No credit will be awarded if your work is not shown in problems 3, 4a, 4b, 4c, and Point values are shown next to the problem number. 6. Budget your time for each of the questions. Some problems may have a low point value yet be very challenging. If you do not recognize the solution to a question quickly, skip it, and return to the question after completing the easier problems. 7. Look through the exam before beginning; plan your work; then begin. 8. Relax and do well. Page 2 Page 3 Page 4 Page 5 TOTAL SCORES (26) (20) (27) (27) (00)
2 CHEM 34 EXAM III PAGE 2 (2). Write the chemical formula(s) of the product(s) and balance the following reactions. Identify all products phases as either (g)as, (l)iquid, (s)olid or (aq)ueous a) Pb(NO 3 ) 2 (aq) + Na 2 S(aq) PbS(s) + 2NaNO 3 (aq) b) C 5 H 2 (aq) + 6O 2 (g) 5CO 2 (g) + 6H 2 O(l) c) 2NaOH(aq) + H 2 SO 4 (aq) Na 2 SO 4 (aq) + 2H 2 O(l) d) Ba(OH) 2 8H 2 O(s) + NH 4 SCN(s) Ba(SCN) 2 (aq) + 0H 2 O(l) + 2NH 3 (g) (4) 2. Write the ionic and net ionic chemical equations for c). c) Ionic equation: 2Na + (aq) + 2OH (aq) + 2H + (aq) + SO 4 2 (aq) 2Na + (aq) + SO4 2 (aq) + 2H2 O(l) Net Ionic equation: 2Na + (aq) + 2OH (aq) + 2H + (aq) + SO 4 2 (aq) 2Na + (aq) + SO4 2 (aq) + 2H2 O(l) 2OH (aq) + 2H + (aq) 2H 2 O(l) OH (aq) + H + (aq) H 2 O(l) calorimeter containing 75.0 g of water at 24.5 C. The heat capacity of the calorimeter is 0.5 J C -. Determine the final temperature of the system. Note: The specific heat of aluminum is J g - C -. q Al, hot = ( q water + q calorimeter ) mass Al S.H. Al T Al, hot = ( mass water S.H. water T water + HC calorimeter T calorimeter ) 225 g J g - C - (T f C) = ( 75.0 g 4.84 J g - C - (T f 24.5 C) J C - (T f 24.5 C)) J C - (T f C) = ( 33.8 J C - (T f 24.5 C) J C - (T f 24.5 C)) J C - (T f C) = ( J C - (T f 24.5 C)) J C - (T f ) 9845 J = ( J C - (T f ) 7945 J)) J C - (T f ) = J J (T f ) = J C- = 52.8 C
3 CHEM 34 EXAM III PAGE 3 (20) 4. A hydrogen atom emits a photon of light with a wavelength of.875 x 0 6 m. a) Calculate the frequency of this photon. c x 0 8 m s x 0 6 m =.60 x 0 4 Hz (cps or s - ) b) Calculate the energy of the photon. E = h x 0-34 J s).60 x 0 4 s - =.06 x 0-9 J c) Determine the initial energy level of the electron if the final energy level the electron has is n = 3. E = 2.8 x 0 8 J n 2 f n 2 i In the above equation E is.06 x 0-9 J. We must add the negative sign because the photon is emitted by the atom as the electron falls from a higher energy level to a lower energy level..06 x 0-9 J = 2.8 x 0 8 J 3 2 f.06 x 0-9 J 2.8 x 0 8 = = J 3 2 f n 2 i n 2 i = 9 n 2 i n 2 = = i n 2 = 6.0 and n = 4 d) Draw and label an energy level diagram for the hydrogen atom and show the transition for the electron as determined in c.
4 CHEM 34 EXAM III PAGE 4 (0) 5. Calculate H for the following reaction, SiO 2 (s) + 4HF(g) SiF 4 (g) + 2H 2 O(g) H rxn = H f (products) - H f (reactants) H rxn = H f(sif 4 ) + 2 H f (H 2 O) ( H f(sio 2 ) + 2 H f(hf)) H rxn = 90.9 kj kj ( 64.9 kj kj) H rxn = 95. kj (2) 6. Write the electron configuration and indicate the number of unpaired electrons for each of the following in their ground state, i. Cr 6 unpaired electrons s 2 2s 2 2p 6 3s 2 3p 6 4s 3d 5 or [Ar]4s 3d 5 ii. I 0 unpaired electrons s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 0 4p 6 5s 2 4d 0 5p 6 or [Kr]5s 2 4d 0 5p 6 iii. Es 5 unpaired electrons s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 0 4p 6 5s 2 4d 0 5p 6 6s 2 4f 4 5d 0 5p 6 7s 2 5f 0 6d or [Rn]7s 2 5f 0 6d (5) 7. Draw the orbital diagram for the valence electrons for phosphorus in its ground state The electron configuration for phosphorus is s 2 2s 2 2p 6 3s 2 3p 3. There are five valence electron in phosphorus. 3s 3p
5 CHEM 34 EXAM III PAGE 5 Multiple Choice: (27 points) Print the letter (A, B, C, D) which corresponds to the answer selected. 8. A 9. B 0. D. B 2. A 3. C 4. C 5. B 6. D ONLY THE ANSWERS IN THE AREA ABOVE WILL BE GRADED. Select the most correct answer for each question. Each question is worth 3 points. 8. Which of these species has a standard enthalpy of formation equal to zero? A) F 2 (g) B) F(g) C) HF(aq) D) F (aq) 9. Which electron configuration is not allowed for either a neutral atom or an ion in its ground state? A) s 2 2s 2 2p 3 B) s 2 2s 2p 6 C) s 2 2s 2 2p 6 3s 2 3p 6 3d 3 D) s 2 2s 2 2p 6 3s 2 3p 6 4s 3d 0 0. Which principal quantum number transition in a hydrogen atom will release the greatest amount of energy? A) 3 B) 6 4 C) 3 5 D) 4 2. Which element in its ground state has the greatest number of unpaired electrons? A) V (atomic number 23) B) Fe (atomic number 26) C) In (atomic number 49) D) As (atomic number 33) 2. In a bomb calorimeter, reactions are carried out at A) constant volume B) constant pressure C) constant temperature D) atm pressure and 0 C 3. Which is a possible set of quantum numbers for a valence electron in phosphorus? n l m l m s A) 2 0 +/2 B) C) 3 - +/2 D) 3 2 -/2
6 CHEM 34 EXAM III PAGE 6 4. Carbon reacts with oxygen according to this equation 2C(s) + O 2 (g) 2CO(g) H = 220 kj I. The reaction is exothermic II. H f of CO is 220 kj III. The combustion of 0.5 mol of carbon produces 55 kj of heat energy A) I only B) I and II C) I and III D) I, II and III 5. Given the reactions Reaction H (kj mol - ) Mg(s) + 2HCl(aq) MgCl 2 (aq) + H 2 (g) 467 MgO(s) + 2HCl(aq) MgCl 2 (aq) + H 2 O(l) 5 and the H f for H 2 O(l) is 286 kj mol, -, the H f for MgO is, A) 904 kj B) 602 kj C) 36 kj D) 30.0 kj 6. Which of the following processes/reactions is not exothermic? A) CH 4 (g) + 2O 2 (g) CO 2 (g) + 2H 2 O(g) B) 2H 2 (g) + O 2 (g) 2H 2 O(g) C) H 2 O(g) H 2 O(l) D) SO 2 (s) SO 2 (l)
7 CHEM 34 EXAM III PAGE IA H Li 6.94 IIA 4 Be Na Mg IIIA IVA VA VIA VIIA B C N O F 9 0 Ne IIIB IVB VB VIB VIIB VIII IB IIB 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 (98) Cs Ba La Periodic Table of the Elements Hf Al Si P S Cl VIIIA 2 Ta W Re 75 Os Ir Pt Au Hg 80 Tl Pb Bi Po At Rn (209) (20) Fr Ra Ac (223) (26) (262) (263) He Ar (222) Lanthanides Actinides Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu (45) Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr (244) (243) (247) (247) (25) (252) (257) (258) (259) (260) Useful Information E n = 2.8 x 0 8 J n 2 r n = x 0 8 n 2 cm h = x 0 34 J s E = 2.8 x 0 8 J n 2 f n 2 λ = c E = hν c = 3.00 x 0 i ν 8 m s J Specific heat of H 2 O(s) = 2.09 g C Specific heat of H J 2O(l) = 4.84 g C J Specific heat of H 2 O(g) =.84 g C Heat of fusion of H 2O(s) = 6.0 kj mol Heat of vaporization of H 2 O(l) = kj mol R = L. atm mol. K or R = 8.34 J mol. H = E + nrt K q(heat flow) = mass specific heat T q reaction = (q calorimeter + q solution ) q reaction = (q calorimeter + q water ) H rxn = Σ n H f (products) - Σ m H f (reactants)
8 CHEM 34 EXAM III PAGE 8 Table of Standard Heats of Formation Substance H f Substance H f and State (kj/ mol) and State (kj/ mol) C(s) (graphite) 0 HNO 3 (aq) C(s) (diamond) 2 HNO 3 (l) HCl(g) CH 4 (g) 75 HBr(g) CH 3 OH(g) -20 HI(g) 26.5 CH 3 OH(l) -239 I 2 (g) H 2 CO(g) -6 O 2 (g) 0 CCl 4 (l) O(g) 249 HCOOH(g) -363 O 3 (g) 43 HCN(g) 35. CS 2 (g) 7.4 N 2 (g) 0 CS 2 (l) 89.7 NH 3 (g) -46 C 2 H 2(g) 227 NH 3 (aq) -80 C 2 H 4 (g) 52 NH 4 + (aq) -32 CH 3 CHO(g) -66 N 2 H 3 CH 3 (l) 54 C 2 H 5 OH(l) -278 N 2 H 4 (l) 50.6 C 2 H 5 O 2 N(g) -533 NO(g) C 2 H 6 (g) NO 2 (g) 33.8 C 3 H 6 (g) 20.9 N 2 O(g) 82.0 C 3 H 8 (g) -04 N 2 O 4 (g) 9.6 C 4 H 0 (g) -26 N 2 O 4 (l) 20 CH 2 = CHCN(l) 52 CH 3 COOH(l) -484 S 2 Cl 2 (g) -8 C 6 H 2 O 6 (s) -275 SO 2 (g) TiO 2 (s) -945 H 2 S(g) Cl 2 (g) 0 SOCl 2 (g) -23 Cl 2 (aq) -23 Cl - (aq) -67 SiCl 4 (g) -657 SiO 2 (s) SiF 4 (g) HF(g) -273 H(g) 27 TiO 2 (s) H + (aq) 0 TiCl 4 (g) -763 OH - (aq) -230 H 2 O(l) -286 ZnO(s) -348 H 2 O(g) -242 ZnS(s) -206
9 CHEM 34 EXAM III PAGE 9 Solubility Table Ion Solubility Exceptions NO 3 soluble none ClO 4 soluble none Cl soluble except Ag +, Hg 2+ 2, *Pb 2+ I soluble except Ag +, Hg 2+ 2, Pb 2+ SO 2 4 soluble except Ca 2+, Ba 2+, Sr 2+, Hg 2+, Pb 2+, Ag + CO 3 2 insoluble except Group IA and NH 4 + PO 3 4 insoluble + except Group IA and NH 4 - OH insoluble except Group IA, *Ca 2+, Ba 2+, Sr 2+ S 2 insoluble except Group IA, IIA and NH + 4 Na + soluble none NH + 4 soluble none K + soluble none *slightly soluble
8. 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 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 1314.03 Exam II John II. Gelder October 23, 1997 Name TA's Name Lab Section INSTRUCTIONS: 1. This examination consists of a total of 9 different pages. The last four pages include a periodic table,
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 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 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 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 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 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 information8. Relax and do well.
CHEM 1314.03 Exam II KEY ohn II. Gelder October 23, 1997 Name TA's Name Lab Section INSTRUCTIONS: 1. This examination consists of a total of 9 different pages. The last four pages include a periodic table,
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 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 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 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 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 informationINSTRUCTIONS: 7. Relax and do well.
EM 1314 Name Exam III TA Name John III. Gelder November 16, 1992 Lab Section INSTRUTIONS: 1. This examination consists of a total of 7 different pages. The last page includes a periodic table and some
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 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 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 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 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 information8. Relax and do well.
CHEM 1515.001 Name Exam II John II. Gelder TA's Name March 8, 2001 Lab Section INSTRUCTIONS: 1. This examination consists of a total of 8 different pages. The last three pages include a periodic table,
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 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 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 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 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 information8. Relax and do well.
CHEM 55.00-006 Exam I John I. Gelder February 5, 2002 Name TA's Name Section INSTRUCTIONS:. This examination consists of a total of 8 different pages. The last three pages include a periodic table, a table
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 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 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 1 Second Lecture Exam Fall Abbasi Khajo Kruft Levine Mathias Mathias/Ortiz Metlitsky Rahi Sanchez-Delgado Vasserman
Page 1 of 9 Chemistry 1 Second Lecture Exam Fall 2011 Name Circle the name of your recitation/lab instructor(s) Abbasi Khajo Kruft Levine Mathias Mathias/Ortiz Metlitsky Rahi Sanchez-Delgado Vasserman
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 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 information8. Relax and do well.
EM 1515.001-009 Exam II John II. Gelder March 5, 2003 Name TA's Name Section INSTRUTIONS: 1. This examination consists of a total of 9 different pages. The last four pages include a periodic table; useful
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 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 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 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 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.
EM 1515.001 Exam III John III. Gelder November 7, 2001 Name TA's Name Lab Section INSTRUTIONS: 1. This examination consists of a total of 9 different pages. The last three pages include a periodic table,
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 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 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 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 information8. Relax and do well.
CHEM 1515 Name Exam III TA's Name John III. Gelder April 7, 1993 Lab Section INSTRUCTIONS: 1. This examination consists of a total of 8 different pages. The last 2 pages include important mathematical
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 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 informationORBITAL DIAGRAM - A graphical representation of the quantum number "map" of electrons around an atom.
178 (MAGNETIC) SPIN QUANTUM NUMBER: "spin down" or "spin up" - An ORBITAL (region with fixed "n", "l" and "ml" values) can hold TWO electrons. ORBITAL DIAGRAM - A graphical representation of the quantum
More informationThe exam must be written in ink. No calculators of any sort allowed. You have 2 hours to complete the exam. Periodic table 7 0
Email: The exam must be written in ink. No calculators of any sort allowed. You have 2 hours to complete the exam. CEM 610B Exam 3 Spring 2002 Instructor: Dr. Brian Pagenkopf Page Points 2 6 3 7 4 9 5
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 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 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 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 Come to the PASS workshop with your mock exam complete. During the workshop you can work with other students to review your work.
It is most beneficial to you to write this mock midterm UNDER EXAM CONDITIONS. This means: Complete the midterm in 1.5 hours. Work on your own. Keep your notes and textbook closed. Attempt every question.
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 informationAtomic Emission Spectra. and. Flame Tests. Burlingame High School Chemistry
Atomic Structure Atomic Emission Spectra and Flame Tests Flame Tests Sodium potassium lithium When electrons are excited they bump up to a higher energy level. As they bounce back down they release energy
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(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 informationCMSC 313 Lecture 17 Postulates & Theorems of Boolean Algebra Semiconductors CMOS Logic Gates
CMSC 313 Lecture 17 Postulates & Theorems of Boolean Algebra Semiconductors CMOS Logic Gates UMBC, CMSC313, Richard Chang Last Time Overview of second half of this course Logic gates &
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 1515.002 Name Exam I John I. Gelder TA's Name February 4, 1998 Lab Section INSTRUCTIONS: 1. This examination consists of a total of 9 different pages. The last three pages include a periodic table,
More information-"l" also contributes ENERGY. Higher values for "l" mean the electron has higher energy.
175 - Giving the four parameters will uniquely identify an electron around an atom. No two electrons in the same atom can share all four. These parameters are called QUANTUM NUMBERS. PRINCIPAL QUANTUM
More informationORBITAL DIAGRAM - A graphical representation of the quantum number "map" of electrons around an atom.
160 ORBITAL DIAGRAM - A graphical representation of the quantum number "map" of electrons around an atom. 4p 3d 4s 3p 3s 2p 2s 1s Each blank represents an ORBITAL, and can hold two electrons. The 4s subshell
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 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 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 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 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 information30 Zn(s) 45 Rh. Pd(s) Ag(s) Cd(s) In(s) Sn(s) white. 77 Ir. Pt(s) Au. Hg(l) Tl. 109 Mt. 111 Uuu. 112 Uub. 110 Uun. 65 Tb. 62 Sm. 64 Gd. 63 Eu.
Enthalpy changes: experimentally it is much easier to measure heat flow at const pressure - this is enthalpy q p = )H : also nearly all chemical reactions are done at constant pressure. Enthalpy (heat)
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 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 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 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 information- Why are phase labels required? Because phase changes either absorb or release energy. ... what does this mean?
157 SINCE the enthalpy change does NOT depend on path, this means that we can use standard values for enthalpy to predict the heat change in reactions that we have not tested in a calorimeter. THERMOCHEMICAL
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 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 informationHalogens HALOGENS. Parts 2A and 2B. Chem : Feb. 19, 20 and March 3. Compare the properties and reactivity of the halogens and halides
Chem. 125-126: Feb. 19, 20 and March 3 Experiment 3 Session 2 (Three hour lab) Complete Experiment 3 Parts 2B and 3 Complete team report Complete discussion presentation Parts 2A and 2B Compare the properties
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 informationGrade 11 Science Practice Test
Grade 11 Science Practice Test Nebraska Department of Education 2012 Directions: On the following pages of your test booklet are multiple-choice questions for Session 1 of the Grade 11 Nebraska State Accountability
More informationChemistry 121 FINAL EXAM
Page 1 of 11 Name: (Print) Surname Given Names Student Number: The Irving K. Barber School of Arts and Sciences Chemistry 121 FINAL EXAM Drs. P. Knoess, K. Perry and E. Neeland FRIDAY, Dec. 9, 2005 9:00
More information-"l" also contributes ENERGY. Higher values for "l" mean the electron has higher energy.
170 - Giving the four parameters will uniquely identify an electron around an atom. No two electrons in the same atom can share all four. These parameters are called QUANTUM NUMBERS. PRINCIPAL QUANTUM
More informationCircle ONLY the LETTER of your answer.
hemistry 1304 Name (please print) Exam 5 (105 points) May 3, 2017 n my honor, I have neither given nor received unauthorized aid on this exam. Signed Date ircle NLY the LETTER of your answer. 1. (3 points)
More information8. Relax and do well.
CHEM 1515.001-009 Exam III John III. Gelder April 2, 2003 Name TA's Name Section INSTRUCTIONS: 1. This examination consists of a total of 10 different pages. The last three pages include a periodic table;
More informationCHEMICAL COMPOUNDS MOLECULAR COMPOUNDS
48 CHEMICAL COMPOUNDS - Dalton's theory does not mention this, but there is more than one way for atoms to come together to make chemical compounds! - There are TWO common kinds of chemical compound, classified
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 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 informationCHEMICAL COMPOUNDS MOLECULAR COMPOUNDS
48 CHEMICAL COMPOUNDS - Dalton's theory does not mention this, but there is more than one way for atoms to come together to make chemical compounds! - There are TWO common kinds of chemical compound, classified
More informationExperiment Three. Lab two: Parts 2B and 3. Halogens used in Parts 2 and 3. Lab one: Parts 1 and 2A. Halogens (Family VIIA) used in Parts 2 and 3
Experiment Three Lab one: Parts 1 and 2A Lab two: Parts 2B and 3 1 1A 1 H 1s 1 2 IIA 3 Li 2s 1 1 1 Na 3s 1 1 9 K 4s 1 3 7 Rb 5s 1 5 5 Cs 6s 1 8 7 Fr 7s 1 4 Be 2s 2 1 2 Mg 3s 2 3 IIIB 4 IVB 5 VB 6 VIB 7
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 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 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 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 information- Atomic line spectra are UNIQUE to each element. They're like atomic "fingerprints".
- Atomic line spectra are UNIQUE to each element. They're like atomic "fingerprints". - Problem was that the current model of the atom completely failed to explain why atoms emitted these lines. An orbit
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 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 informationCLEARLY SHOW ALL WORK AND REASONING.
Name (print clearly) Seat number Quiz 4 (100 points) Chemistry 1303.002 October 17, 2018 1. (25points) Using the information below, find the enthalpy of formation ( H f ) for gaseous hydrogen chloride.
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 information