Chemistry 112 Name Exam I Form A Section January 29,

Save this PDF as:
 WORD  PNG  TXT  JPG

Size: px
Start display at page:

Download "Chemistry 112 Name Exam I Form A Section January 29,"

Transcription

1 Chemistry 112 Name Exam I Form A Section January 29, IMPORTANT: On the scantron (answer sheet), you MUST clearly fill your name, your student number, section number, and test form (white cover = test form A; yellow cover = test form B). Use a #2 pencil. There are 25 questions on this exam. Check that you have done all of the problems and filled in the first 25 bubbles on the scantron.your score will be reported in percent (max 100%). Exam policy Hints Calculators with text-programmable memory are not allowed. Relevant data and formulas, including the periodic table, are attached at the end of this exam. Your grade will be based only on what is on the scantron form. The answer key will be posted on the web after the exam (on the Exam Schedule page). You must turn in your cover sheet with your scantron answer form. As you read the question, underline or circle key words to highlight them for yourself. Avoid errors from "mis-reading" the question. Pay attention to units and magnitudes (decimal places) of numbers obtained from calculations. There is no penalty for guessing.

2

3 CHEMISTRY 112 EXAM 1 January 29, 2013 FORM A 1. Consider the following reaction: A + B C Rate = k[b] 2 Which of the following will NOT increase the reaction rate? A. Increasing the concentration of A B. Increasing the concentration of B C. Raising the reaction temperature D. Adding a suitable catalyst E. All of the above changes will result in an increase in reaction rate 2. A possible mechanism for the reaction of hydrogen bromide with oxygen is: HBr (g) + O 2 (g) HOOBr (g) step 1 HOOBr (g) + HBr (g) 2 HOBr (g) step 2 HOBr (g) + HBr (g) H 2 O (g) + Br 2 (g) step 3 Which of the following is an intermediate in this reaction? A. HOOBr only B. HBr and O 2 only C. HOBr only D. HOOBr and HBr only E. Br 2, HOBr and HOOBr only 3. Which one of the following statements about rate constant k is FALSE? A. k is dependent on the concentration of the reactants. B. k increases with increasing temperature. C. k decreases with increasing activation energy. D. k can be increased by adding a catalyst. E. The reaction rate is directly proportional to k.

4 4. For the reaction below, = 2.5 x 10 2 atm/s, where ΔP(H 2 ) is the change in pressure of hydrogen. What is the rate of loss of C 6 H 14 (defined as ) for this reaction for the same time period? C 6 H 14 (g) C 6 H 6 (g) + 4 H 2 (g) A. 2.5 x 10 2 atm/s B x 10 3 atm/s C. 2.5 x 10 2 atm/s D atm/s E. 2.6 x 10 3 atm/s 5. For the following nuclear reaction, what is the value of x? A. 1 B. 3 C. 5 D. 7 E Given the initial rate data shown in the table below, what is the rate law of the following reaction? A. Rate = k[a][b] 2 Experiment [A] (M) [B] (M) Initial Rate (M/s) x x x 10 4 B. Rate = k[a] 2 [B] C. Rate = k[a] 2 D. Rate = k[b] 2 E. Rate = k[b]

5 7. Which points on the reaction profile below represent intermediates? A. C and E only B. B, D and F only C. A and G only D. B, C, D, E and F only E. D only 8. Consider the reaction below: Br 2 (aq) + HCOOH (aq) 2 Br (aq) + 2 H + (aq) + CO 2 (g) Why does the instantaneous reaction rate for this chemical reaction decrease with time? (Assume temperature is constant.) A. The activation energy increases. B. CO 2 gas is escaping into the atmosphere. C. The concentration of Br 2 decreases. D. The HCOOH is a catalyst. E. ΔE for the reaction increases.

6 9. What type of particle or radiation is emitted when a F-20 nucleus decays to Ne-20? A. alpha B. beta C. neutron D. positron E. proton 10. The first-order reaction A B in which A molecules (black circles) are converted to B molecules (white circles) in a 2.0 L container is shown below at two points in time. What is the concentration of A molecules after 40 seconds? A. 8.0 molecules/l B. 4.0 molecules/l C. 2.0 molecules/l D. 12 molecules/l E. 6.0 molecules/l t = 0 s t = 20 s Go on to the next page

7 11. A reaction has the following rate law: Rate = k[a][b] 2 In experiment 1, the concentrations of A and B are both 0.10 M. In experiment 2, the concentrations of A and B are both 0.30 M. If the temperature stays constant, what is the value of the ratio? A. 3.0 B. 6.0 C. 9.0 D. 18 E What does a catalyst do? A. It lowers the overall enthalpy of the reaction. B. It lowers the activation energy of the forward reaction only. C. It raises the activation energy of the reverse reaction only. D. It lowers the activation energy of both the forward and reverse reactions. E. It raises the energy of the reactant molecules Why does the rate of a reaction increase with increasing temperature? A. The reactant molecules collide less frequently. B. The reactant molecules collide with greater energy. C. The activation energy is lowered. D. The reactant molecules collide with the right orientation. E. The concentration of the reactant molecules increases. Go on to the next page

8 14. What is the nuclear binding energy per nucleon, in joules, for a 25 Mg nucleus? (nuclear mass amu) [Use the following data: proton (mass) = amu; neutron (mass) = amu] A J/nucleon B x J/nucleon C x J/nucleon D J/nucleon E x J/nucleon 15. Iodine-131, t 1/2 = 8.0 days, is used in the diagnosis and treatment of thyroid gland diseases. If a laboratory sample of iodine-131 initially emits 9.95 x β particles per day, how long will it take for the activity to drop to 6.22 x β particles per day? A. 2.0 days B. 16 days C. 32 days D. 128 days E. 64 days Go on to the next page

9 16. The decomposition of NO 2 was studied at 656 K and the data was plotted below: (M 1 ) The y-intercept of the plot is 9.20 M 1, and the slope of the line is M 1 sec 1. For a different experiment at the same temperature and an initial NO 2 concentration of M, how long would it take to decompose half of the NO 2? A sec B sec C sec D sec E sec 17. The only stable isotope of aluminum is 27 Al. What type of radioactive decay would 23 Al be expected to undergo? A. proton emission B. neutron emission C. beta decay D. positron emission E. alpha decay Go on to the next page

10 18. The temperature dependence of the rate constant for a second order reaction is plotted below: The y-intercept of the plot is 23.2, and the slope of the line is 1.61 x 10 4 K. Based on this data, what would the rate constant be at 500 K? A x 10 4 M -1 s 1 B x 10 2 M -1 s 1 C x 10 1 M -1 s 1 D M 1 s 1 E x 10 3 M 1 s Potassium-40 undergoes positron emission to form argon-40 with a half-life of 1.2 x 10 9 years. If a sample of rock from an asteroid contains 82% argon with the remaining portion being potassium, what is the age of the rock? (Assume that all of the argon in the sample is the result of potassium decay.) A. 3.4 x 10 8 years B. 2.1 x 10 9 years C. 8.3 x 10 8 years D. 1.5 x 10 6 years E. 3.0 x 10 9 years Go on to the next page

11 20. What is the balanced nuclear equation represented by the following diagram? A. B. C. D. E. Go on to the next page

12 21. For the overall reaction 2 N 2 O 5 (g) 4 NO 2 (g) + O 2 (g) the following mechanism is proposed: N 2 O 5 (g) NO 2 (g) + NO 3 (g) (fast equilibrium) NO 2 (g) + NO 3 (g) NO 2 (g) + NO (g) + O 2 (g) (slow) NO 3 (g) + NO (g) 2 NO 2 (g) (fast) Which statement is true about the rate law that is consistent with this mechanism? A. The rate law is first order in N 2 O 5. B. The rate law is second order in NO 2 and first order in NO 3. C. The rate law is first order in NO 2 and NO 3 and second order in N 2 O 5. D. The rate law is second order in N 2 O 5. E. None of these choices is consistent with the rate law. 22. The isomerization of methyl isocyanide, CH 3 NC CH 3 CN, follows first-order kinetics. The halflives were found to be 161 min at 199 C and 12.5 min at 230 C. What is the activation energy for this reaction? A x 10 3 kj/mol B kj/mol C kj/mol D. 124 kj/mol E. 163 kj/mol Go on to the next page

13 23. Suppose a certain biologically important reaction is quite slow at physiological temperature (37 o C) in the absence of a catalyst. Assuming that the collision factor A remains the same, by how much must an enzyme lower the activation energy of the reaction to achieve a million-fold increase (1 x 10 6 ) in the reaction rate? A. 10 kj/mol B. 36 kj/mol C. 51 kj/mol D. 74 kj/mol E. 82 kj/mol 24. The rate constant k for the reaction 3A 4B is 6.00 x 10 3 M 1 min 1. How long will it take for the concentration of A to drop from 0.75 M to 0.25 M? A. 2.2 x 10 3 min B. 5.5 x 10 3 min C. 180 min D. 440 min E. 5.0 x 10 2 min Go on to the last page

14 25. During a medical PET scan a patient is injected with a tracing compound that contains an 18 F isotope, which decays through positron emission. When the emitted positron encounters an electron both are completely destroyed through a matter-antimatter reaction, producing two photons that propagate in opposite directions. If the energy of each photon is x J, what is the mass of the positron? A x 10 4 amu B x 10 4 amu C x 10 3 amu D amu E amu END OF TEST

15 CHEM 112 SPRING 2013 EXAM 1 FORM - A SCRAP PAPER

16 CHEM 112 SPRING 2013 EXAM 1 FORM - A SCRAP PAPER

17 1. Standard Electrode Potentials Half-reaction E o 1/2(V) F 2 (g) + 2e 2F (aq) H 2 O 2 (aq) + 2H + (aq) + 2e 2H 2 O() Cl 2 (g) + 2e 2Cl (aq) O 2 (g) + 4H + (aq) + 4e 2H 2 O() Br 2 () + 2e 2Br (aq) Ag + (aq) + e Ag(s) Fe 3+ (aq) + e Fe 2+ (aq) O 2 (g) + 2H + (aq) + 2e H 2 O 2 (aq) I 2 (s) + 2e 2I (aq) Cu + (aq) + e Cu(s) Cu 2+ (aq) + 2e Cu(s) Sn 4+ (aq) + 2e Sn 2+ (aq) Cu 2+ (aq) + e Cu + (aq) H + (aq) + 2e H 2 (g) 0.00 Pb 2+ (aq) + 2e Pb(s) 0.13 Sn 2+ (aq) + 2e Sn(s) 0.14 Co +2 (aq) + 2e Co(s) 0.28 Ni 2+( aq) + 2e Ni(s) 0.28 Cd 2+ (aq) + 2e Cd(s) 0.40 Fe 2+ (aq) + 2e Fe(s) 0.44 Cr 3+ (aq) + 3e Cr(s) 0.74 Zn 2+ (aq) + 2e Zn(s) H 2 O() + 2e H 2 (g) + 2OH (aq) 0.83 SO 2 4 (aq) + H 2 O() + 2e SO 2 3 (aq) + 2OH (aq) 0.93 Mn 2+ (aq) + 2e Mn(s) 1.18 Al 3+ (aq) + 3e Al(s) 1.66 Mg 2+ (aq) + 2e Mg(s) 2.37 Na + (aq) + e Na(s) 2.71 Ca 2+ (aq) + 2e Ca(s) 2.76 Li + (aq) + e Li(s) Constants R = J mol 1 K 1 R = L-atm mol 1 K 1 F = 96,500 coulombs/mol electrons h = x J-s mass 1 0 n = amu mass 1 1 p = amu 1 g = 6.02 x amu 1 amp = 1 coul sec 1 Avogadro s no. = x mol 1 c = x 10 8 m sec 1 1 J = kg m 2 sec 2 = C-V 3. Equations G = H T S = nfe Chem 112 Data Sheet G o = RT log K = RT ln K G = G o + RT ln Q G = G o RT log Q E o = n log K (at 25 o C) E = E o log Q (at 25 o C) n [ X ] ph = pk a + log [ HX ] K a x K b = K w = [H + ] [OH ] pk w = ph + poh = pk a + pk b K p = K c (RT) Δn K w = 1 x at 25 C ln k = ln k k 1 2 E a RT E a = R a k = Ae ( ) RT + ln A ln[a] = ln[a] o kt 1 [A] 1 [A] o t 1/2 = 0.693/k t 1/2 = 1/k[A] o 1 1 T 2 T kt 1 log ln N t = N o o N t = N 0.301t t = kt t = kt k = t 4. MO Theory E Diagrams Rate = kn E = mc t 1 2 E = hν c = λν 6. Crystal Field Splitting for octahedral complexes E d x2 y2, d z2 d xy, d yz, d xz Δ o Name

18 PERIODIC TABLE of the ELEMENTS MAIN GROUPS MAIN GROUPS 1A 1 8A 18 1 H A 2 3A 13 4A 14 5A 15 6A 16 7A 17 2 He Li Be TRANSITION METALS 5 B C N O F Ne Na Mg B 3 4B 4 5B 5 6B 6 7B 7 8B 8 8B 9 8B 10 1B 11 2B 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 [98] 44 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 [265] 109 Mt [268] 110 [269] 111 [272] 112 [277] 114 [285] 116 [289] 118 [293] * LANTHANOIDS 58 Ce Pr Nd Pm [145] 62 Sm Eu Gd Tb Dy Ho Er Tm Yb Lu ** ACTINOIDS 90 Th Pa 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 [262]

Chemistry 112 Name Exam I Form A Section February 3,

Chemistry 112 Name Exam I Form A Section February 3, Chemistry 112 Name Exam I Form A Section February 3, 2015 email IMPORTANT: On the scantron (answer sheet), you MUST clearly fill your name, your student number, section number, and test form (white cover

More information

Last 4 Digits of USC ID:

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 information

Atoms and the Periodic Table

Atoms 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 information

PERIODIC TABLE OF THE ELEMENTS

PERIODIC 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

Chemistry Standard level Paper 1

Chemistry 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 information

INSTRUCTIONS: Exam III. November 10, 1999 Lab Section

INSTRUCTIONS: 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

Using the Periodic Table

Using 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 information

Marks for each question are as indicated in [] brackets.

Marks 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 information

Made the FIRST periodic table

Made 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 information

8. Relax and do well.

8. 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 information

The Periodic Table of Elements

The 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 information

Circle the letters only. NO ANSWERS in the Columns! (3 points each)

Circle 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 information

Chapter 3: Stoichiometry

Chapter 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 information

8. Relax and do well.

8. 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 information

Chapter 12 The Atom & Periodic Table- part 2

Chapter 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 information

Modified from: Larry Scheffler Lincoln High School IB Chemistry 1-2.1

Modified 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 information

Chemistry 126 Final Examination, Prof. Hanson, May, Section B or D (circle one) Seat Coordinate Name

Chemistry 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 information

Circle the letters only. NO ANSWERS in the Columns!

Circle the letters only. NO ANSWERS in the Columns! Chemistry 1304.001 Name (please print) Exam 5 (100 points) April 18, 2018 On my honor, I have neither given nor received unauthorized aid on this exam. Signed Date Circle the letters only. NO ANSWERS in

More information

30 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.

30 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 information

Chemistry 12 Name Exam I Form A Section February 7, 2001 Student No.

Chemistry 12 Name Exam I Form A Section February 7, 2001 Student No. Chemistry 12 Name Exam I Form A Section February 7, 2001 Student No. IMPRTANT: n the scantron (answer sheet), you MUST clearly fill your name, your student number, section number, and test form (white

More information

Fall 2011 CHEM Test 4, Form A

Fall 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 information

Ch. 9 NOTES ~ Chemical Bonding NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics.

Ch. 9 NOTES ~ Chemical Bonding NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics. Ch. 9 NOTES ~ Chemical Bonding NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics. I. Review: Comparison of ionic and molecular compounds Molecular compounds Ionic

More information

Atomic Structure & Interatomic Bonding

Atomic Structure & Interatomic Bonding Atomic Structure & Interatomic Bonding Chapter Outline Review of Atomic Structure Atomic Bonding Atomic Structure Atoms are the smallest structural units of all solids, liquids & gases. Atom: The smallest

More information

CHEM 130 Exp. 8: Molecular Models

CHEM 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 information

Chemistry Standard level Paper 1

Chemistry 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 information

7. Relax and do well.

7. 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 information

CHEM 108 (Fall-2003) Exam Final (100 pts)

CHEM 108 (Fall-2003) Exam Final (100 pts) CHEM 108 (Fall-2003) Exam Final (100 pts) Name: -------------------------------------------------------------------------------, SSN -------------------------------- LAST NAME, First (Circle the alphabet

More information

Grade 11 Science Practice Test

Grade 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 information

Element Cube Project (x2)

Element 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 information

Chemistry Standard level Paper 1

Chemistry 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 information

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 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 information

SCIENCE 1206 UNIT 2 CHEMISTRY. September 2017 November 2017

SCIENCE 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

NAME: SECOND EXAMINATION

NAME: SECOND EXAMINATION 1 Chemistry 64 Winter 1994 NAME: SECOND EXAMINATION THIS EXAMINATION IS WORTH 100 POINTS AND CONTAINS 4 (FOUR) QUESTIONS THEY ARE NOT EQUALLY WEIGHTED! YOU SHOULD ATTEMPT ALL QUESTIONS AND ALLOCATE YOUR

More information

9/20/2017. Elements are Pure Substances that cannot be broken down into simpler substances by chemical change (contain Only One Type of Atom)

9/20/2017. 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 information

UNIVERSITY OF CALGARY FACULTY OF SCIENCE MIDTERM EXAMINATION CHEMISTRY 353 READ ALL THE INSTRUCTIONS CAREFULLY

UNIVERSITY OF CALGARY FACULTY OF SCIENCE MIDTERM EXAMINATION CHEMISTRY 353 READ ALL THE INSTRUCTIONS CAREFULLY WEDNESDAY MARCH 9th, 2016 UNIVERSITY OF CALGARY FACULTY OF SCIENCE MIDTERM EXAMINATION CHEMISTRY 353 Version 1 Time: 2 Hours READ ALL THE INSTRUCTIONS CAREFULLY PLEASE WRITE YOUR NAME, STUDENT I.D. NUMBER

More information

What is the periodic table?

What 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 information

6.3 Classifying Elements with the Periodic Table

6.3 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 information

Chemistry 112 Name Practice Exam 1C Section

Chemistry 112 Name Practice Exam 1C Section Chemistry 112 Name Practice Exam 1C Section email IMPORTANT: On the scantron (answer sheet), you MUST clearly fill your name, your student number, section number, and test form (white cover = test form

More information

Chemistry 1 Second Lecture Exam Fall Abbasi Khajo Kruft Levine Mathias Mathias/Ortiz Metlitsky Rahi Sanchez-Delgado Vasserman

Chemistry 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 information

CHEMISTRY 102 Fall 2014 HOUR EXAM I Page 1

CHEMISTRY 102 Fall 2014 HOUR EXAM I Page 1 OUR EXAM I Page 1 1. Draw the Lewis structure for ICl5. ow many of the following four statements (I-IV) is/are true regarding ICl5? I. The central atom in ICl5 has one lone pair of electrons. II. Some

More information

Reporting Category 1: Matter and Energy

Reporting 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 information

Atomic Emission Spectra. and. Flame Tests. Burlingame High School Chemistry

Atomic 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 information

A little history. When and How? Sir William Ramsey. ü 12/5/13. ü 1. Who put together the first useable Periodic Table?

A 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 information

single-layer transition metal dichalcogenides MC2

single-layer transition metal dichalcogenides MC2 single-layer transition metal dichalcogenides MC2 Period 1 1 H 18 He 2 Group 1 2 Li Be Group 13 14 15 16 17 18 B C N O F Ne 3 4 Na K Mg Ca Group 3 4 5 6 7 8 9 10 11 12 Sc Ti V Cr Mn Fe Co Ni Cu Zn Al Ga

More information

8/30/2010. The Components of Matter Chapter 2. Element, Atom, Compound, and Molecule. Elements, Compounds, and Mixtures

8/30/2010. 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 information

ORBITAL DIAGRAM - A graphical representation of the quantum number "map" of electrons around an atom.

ORBITAL 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 information

SCIENCE SAC Making a World of Difference. University Interscholastic League

SCIENCE SAC Making a World of Difference. University Interscholastic League SCIENCE SAC 2013 GENERAL DIRECTIONS: DO NOT OPEN EXAM UNTIL TOLD TO DO SO. Ninety minutes should be ample time to complete this contest, but since it is not a race, contestants may take up to two hours.

More information

Circle ONLY the LETTER of your answer.

Circle 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 information

VIIIA H PREDICTING CHARGE

VIIIA H PREDICTING CHARGE 58 IA PREDICTING CHARGE VIIIA H IIA IIIA IVA VA VIA VIIA You can reliably determine the charge using our method for Groups IA, IIA, IIIB, Aluminum, and the Group VA, VIA, and VIIA NONMETALS Li Be B C N

More information

1 Electrons and Chemical Bonding

1 Electrons and Chemical Bonding CHAPTER 13 1 Electrons and Chemical Bonding SECTION Chemical Bonding BEFORE YOU READ After you read this section, you should be able to answer these questions: What is chemical bonding? What are valence

More information

Spin Cut-off Parameter of Nuclear Level Density and Effective Moment of Inertia

Spin Cut-off Parameter of Nuclear Level Density and Effective Moment of Inertia Commun. Theor. Phys. (Beijing, China) 43 (005) pp. 709 718 c International Academic Publishers Vol. 43, No. 4, April 15, 005 Spin Cut-off Parameter of Nuclear Level Density and Effective Moment of Inertia

More information

Example: Helium has an atomic number of 2. Every helium atom has two protons in its nucleus.

Example: Helium has an atomic number of 2. Every helium atom has two protons in its nucleus. 59 Atomic terms - ATOMIC NUMBER: The number of protons in the atomic nucleus. Each ELEMENT has the SAME NUMBER OF PROTONS in every nucleus. In neutral atoms, the number of ELECTRONS is also equal to the

More information

Chem 6 Sample exam 2 (150 points total) NAME:

Chem 6 Sample exam 2 (150 points total) NAME: hem 6 Sample exam 2 (150 points total) @ This is a closed book exam to which the onor Principle applies. @ The last page contains equations and physical constants; you can detach it for easy reference.

More information

-"l" also contributes ENERGY. Higher values for "l" mean the electron has higher energy.

-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 information

... but using electron configurations to describe how aluminum bromide forms is a bit cumbersome! Can we simplify the picture a bit?

... but using electron configurations to describe how aluminum bromide forms is a bit cumbersome! Can we simplify the picture a bit? 193... but using electron configurations to describe how aluminum bromide forms is a bit cumbersome! Can we simplify the picture a bit? LEWIS NOTATION / ELECTRON-DOT NOTATION - Lewis notation represents

More information

Electrons. Unit H Chapter 6

Electrons. Unit H Chapter 6 Electrons Unit H Chapter 6 1 Electrons were discovered by 1. Dalton 2. Lavoisier 3. Proust 4. Mendeleev 6. Rutherford 7. Bohr 8. Schrodinger 9. Dirac 5. Thomson 2 Electrons were discovered by 1. Dalton

More information

D) g. 2. In which pair do the particles have approximately the same mass?

D) g. 2. In which pair do the particles have approximately the same mass? 1. A student constructs a model for comparing the masses of subatomic particles. The student selects a small, metal sphere with a mass of gram to represent an electron. A sphere with which mass would be

More information

Review. 8th grade science STAAR. Name Class. Underline your strong TEKS and circle your weak TEKS: 8.5A Atoms. 7.5C Energy Flow Through Ecosystems

Review. 8th grade science STAAR. Name Class. Underline your strong TEKS and circle your weak TEKS: 8.5A Atoms. 7.5C Energy Flow Through Ecosystems 8th grade science STAAR Review Name Class Underline your strong TEKS and circle your weak TEKS: 8.5A Atoms 7.5C Energy Flow Through Ecosystems 8.5B Reactivity 8.5C Periodic Table 8.5D Chemical Formulas

More information

Putting it together... - In the early 20th century, there was a debate on the structure of the atom. Thin gold foil

Putting it together... - In the early 20th century, there was a debate on the structure of the atom. Thin gold foil 36 Putting it together... - In the early 20th century, there was a debate on the structure of the atom. RUTHERFORD EXPERIMENT Where do the particles go? Radioactive material A few bounce back A few particles

More information

NAME: 3rd (final) EXAM

NAME: 3rd (final) EXAM 1 Chem 64 Winter 2003 AME: 3rd (final) EXAM THIS EXAM IS WORTH 100 POITS AD COTAIS 9 QUESTIOS THEY ARE OT EQUALLY WEIGHTED! YOU SHOULD ATTEMPT ALL QUESTIOS AD ALLOCATE YOUR TIME ACCORDIGLY IF YOU DO'T

More information

Earth Materials I Crystal Structures

Earth Materials I Crystal Structures Earth Materials I Crystal Structures Isotopes same atomic number, different numbers of neutrons, different atomic mass. Ta ble 1-1. Su mmar y of quantu m num bers Name Symbol Values Principal n 1, 2,

More information

EXAMPLES. He VIA VIIA Li Be B C N O F Ne

EXAMPLES. He VIA VIIA Li Be B C N O F Ne 59 IA EXAMPLES VIIIA H IIA IIIA IVA VA He VIA VIIA Li Be B C N O F Ne Na Mg IIIB IVB VB Al Si P VIB VIIB VIIIB IB IIB 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

More information

Lewis dot structures for molecules

Lewis dot structures for molecules 1 Lewis dot structures for molecules In the dot structure of a molecule, - SHARED valence electrons are shown with dashes - one per pair. - UNSHARED valence electrons ("lone pairs") are represented by

More information

Atomic terms. Example: Helium has an atomic number of 2. Every helium atom has two protons in its nucleus.

Atomic terms. Example: Helium has an atomic number of 2. Every helium atom has two protons in its nucleus. Atomic terms - ATOMIC NUMBER: The number of protons in the atomic nucleus. Each ELEMENT has the SAME NUMBER OF PROTONS in every nucleus. In neutral atoms, the number of ELECTRONS is also equal to the atomic

More information

[ ]:543.4(075.8) 35.20: ,..,..,.., : /... ;. 2-. ISBN , - [ ]:543.4(075.8) 35.20:34.

[ ]:543.4(075.8) 35.20: ,..,..,.., : /... ;. 2-. ISBN , - [ ]:543.4(075.8) 35.20:34. .. - 2-2009 [661.87.+661.88]:543.4(075.8) 35.20:34.2373-60..,..,..,..,.. -60 : /... ;. 2-. : -, 2008. 134. ISBN 5-98298-299-7 -., -,,. - «,, -, -», - 550800,, 240600 «-», -. [661.87.+661.88]:543.4(075.8)

More information

Periodic Table. - Mendeleev was able to predict the properties of previously unknown elements using his "periodic law" Modern periodic table

Periodic Table. - Mendeleev was able to predict the properties of previously unknown elements using his periodic law Modern periodic table 74 Periodic Table - Mendeleev (1869): --- When atoms are arranged in order of their atomic weight, some of their chemical and physical properties repeat at regular intervals (periods) --- Some of the physical

More information

Thermochemistry. Chapter 6. Chemistry E1a

Thermochemistry. Chapter 6. Chemistry E1a Thermochemistry Chapter 6 Chemistry E1a Energy: What is it? How is it transformed? What is energy? What are the SI units for energy? Give examples of some energy What types of energy are we going to be

More information

Halogens HALOGENS. Parts 2A and 2B. Chem : Feb. 19, 20 and March 3. Compare the properties and reactivity of the halogens and halides

Halogens 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 information

Experiment 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 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 information

Practice Final Exam CH 201

Practice Final Exam CH 201 Practice Final Exam CH 201 Name: (please print) Student I D : Instructions - Read Carefully 1. Please show your work, and put your final answers in the spaces provided. 2. Point values for each question

More information

Practice Questions for Exam 2 CH 1020 Spring 2017

Practice Questions for Exam 2 CH 1020 Spring 2017 Practice Questions for Exam 2 CH 1020 Spring 2017 1. Pick all of the statements which are true about a reaction mechanism?. A rate law can be written from the molecularity of the slowest elementary step..

More information

Chemistry Higher level Paper 1

Chemistry Higher level Paper 1 hemistry igher level Paper 1 Thursday 11 May 2017 (afternoon) 1 hour Instructions to candidates Do not open this examination paper until instructed to do so. Answer all the questions. For each question,

More information

Name Section Signature TA ID #

Name Section Signature TA ID # FIRST LETTER OF YOUR LAST NAME CHEMISTRY 118 EXAM II March 8, 014 Name Section Signature TA ID # PLEASE READ THE FOLLOWING INSTRUCTIONS Do NOT begin the exam until asked to do so. There are 8 numbered

More information

Chemistry 51 Exam #3. Name KEY November 20, 2001

Chemistry 51 Exam #3. Name KEY November 20, 2001 Chemistry 51 Exam #3 Name KEY November 20, 2001 This exam has nine (9) questions. Please check before beginning to make sure no questions are missing. All scratch work must be done on the attached blank

More information

Periodic Table. Modern periodic table

Periodic Table. Modern periodic table 41 Periodic Table - Mendeleev (1869): --- When atoms are arranged in order of their atomic weight, some of their chemical and physical properties repeat at regular intervals (periods) --- Some of the physical

More information

Teacher Workbooks. Science and Nature Series. Atomic Structure, Electron Configuration, Classifying Matter and Nuclear Chemistry, Vol.

Teacher Workbooks. Science and Nature Series. Atomic Structure, Electron Configuration, Classifying Matter and Nuclear Chemistry, Vol. Teacher Workbooks Science and Nature Series Atomic Structure, Electron Configuration, Classifying Matter and Nuclear Chemistry, Vol. 1 Copyright 23 Teachnology Publishing Company A Division of Teachnology,

More information

Presenter Copy. Advanced Placement. Chemistry. Rates and Mechanisms

Presenter Copy. Advanced Placement. Chemistry. Rates and Mechanisms Advanced Placement Presenter Copy Chemistry Rates and Mechanisms 2014 47.90 91.22 178.49 (261) 50.94 92.91 180.95 (262) 52.00 93.94 183.85 (263) 54.938 (98) 186.21 (262) 55.85 101.1 190.2 (265) 58.93 102.91

More information

(FIRST) IONIZATION ENERGY

(FIRST) IONIZATION ENERGY 181 (FIRST) IONIZATION ENERGY - The amount of energy required to remove a single electron from the outer shell of an atom. - Relates to reactivity for metals. The easier it is to remove an electron, the

More information

Review A Z. a particle. proton. neutron. electron e -1. positron. e +1. Mass Number Atomic Number. Element Symbol

Review A Z. a particle. proton. neutron. electron e -1. positron. e +1. Mass Number Atomic Number. Element Symbol Nuclear Chemistry 1 Review Atomic number (Z) = number of protons in nucleus Mass number (A) = number of protons + number of neutrons = atomic number (Z) + number of neutrons Mass Number Atomic Number A

More information

KEY CHEMISTRY 2C. Section B FINAL EXAM

KEY CHEMISTRY 2C. Section B FINAL EXAM thelifecurve.com KEY Last Name First Name Lab Sec. # ; TA: ; Lab day/time: Dr. Toupadakis Spring 2013 CHEMISTRY 2C Section B Instructions: FINAL EXAM CLOSED BOOK EXAM! No books, notes, or additional scrap

More information

- Some properties of elements can be related to their positions on the periodic table.

- Some properties of elements can be related to their positions on the periodic table. 179 PERIODIC TRENDS - Some properties of elements can be related to their positions on the periodic table. ATOMIC RADIUS - The distance between the nucleus of the atoms and the outermost shell of the electron

More information

PROOF/ÉPREUVE ISO INTERNATIONAL STANDARD. Space environment (natural and artificial) Galactic cosmic ray model

PROOF/ÉPREUVE ISO INTERNATIONAL STANDARD. Space environment (natural and artificial) Galactic cosmic ray model INTERNATIONAL STANDARD ISO 15390 First edition 2004-##-## Space environment (natural and artificial) Galactic cosmic ray model Environnement spatial (naturel et artificiel) Modèle de rayonnement cosmique

More information

1 Arranging the Elements

1 Arranging the Elements CHAPTER 12 1 Arranging the Elements SECTION The Periodic Table BEFORE YOU READ After you read this section, you should be able to answer these questions: How are elements arranged on the periodic table?

More information

8. Relax and do well.

8. 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 information

AP Chem Chapter 14 Study Questions

AP Chem Chapter 14 Study Questions Class: Date: AP Chem Chapter 14 Study Questions 1. A burning splint will burn more vigorously in pure oxygen than in air because a. oxygen is a reactant in combustion and concentration of oxygen is higher

More information

- When atoms share electrons, the electrons might not be EVENLY shared. Shared electrons may spend more time around one atomic nucleus than the other.

- When atoms share electrons, the electrons might not be EVENLY shared. Shared electrons may spend more time around one atomic nucleus than the other. 228 POLARITY - When atoms share electrons, the electrons might not be EVENLY shared. Shared electrons may spend more time around one atomic nucleus than the other. - When electrons are shared UNEVENLY,

More information

1.02 Elements, Symbols and Periodic Table

1.02 Elements, Symbols and Periodic Table .0 Elements, Symbols and Periodic Table Dr. Fred O. Garces Chemistry Miramar College.0 Elements, Symbols and the Periodic Table January 0 The Elements: Building block of Matter The periodic table of the

More information

Stoichiometry. Mole Concept. Balancing Chemical Equations

Stoichiometry. Mole Concept. Balancing Chemical Equations Stoichiometry The story so far The structure of an atom protons, neutrons & electrons Electron structure & the Periodic Table Shapes of electron orbitals (Quantum Numbers) Essential and toxic elements

More information

Body-centred-cubic (BCC) lattice model of nuclear structure

Body-centred-cubic (BCC) lattice model of nuclear structure Body-centred-cubic (BCC) lattice model of nuclear structure Gamal A. Nasser Faculty of science, Mansoura University, Egypt. E-mail: chem.gamal@hotmail.com. Abstract: This model is development of solid

More information

The 18 Electron Rule. References: Gray: chapter 5 OGN: chapter 18

The 18 Electron Rule. References: Gray: chapter 5 OGN: chapter 18 The 18 Electron Rule References: Gray: chapter 5 OGN: chapter 18 Element Groups Alkali metals nert or Noble gases Alkali earths alogens e Li Na Be Mg Transition metals B Al Si N P O S F l Ne Ar K Rb s

More information

- Some properties of elements can be related to their positions on the periodic table.

- Some properties of elements can be related to their positions on the periodic table. 179 PERIODIC TRENDS - Some properties of elements can be related to their positions on the periodic table. ATOMIC RADIUS - The distance between the nucleus of the atoms and the outermost shell of the electron

More information

E4 Acids, Bases, and Salts

E4 Acids, Bases, and Salts E4 Acids, Bases, and Salts Session One of two session lab Complete Parts 1 and 2 in lab. If time allows, start or complete Part 3. Acids and Bases Q. Are acid-base properties of substances predictable

More information

Half Yearly Exam 2015

Half Yearly Exam 2015 GOZO COLLEGE Secondary School KULLEĠĠ TA GĦAWDEX Skola Sekondarja Half Yearly Exam 015 Year 9 Track 3 CHEMISTRY Time: 1½ hours Name: Class: Useful Data: Atomic numbers and relative atomic masses are given

More information

8. Relax and do well.

8. 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 information

Chemistry 1 Final Exam Dec Circle one: Abassi Castillo Ciskowska Jarzecki Kahanda Shakya

Chemistry 1 Final Exam Dec Circle one: Abassi Castillo Ciskowska Jarzecki Kahanda Shakya Chemistry 1 Final Exam Dec. 2005 Name Circle one: Abassi Castillo Ciskowska Jarzecki Kahanda Shakya Write your name on this page and on the next page. For questions 33 45 you must show work. The exam adds

More information

NJCTL.org 2015 AP Physics 2 Nuclear Physics

NJCTL.org 2015 AP Physics 2 Nuclear Physics AP Physics 2 Questions 1. What particles make up the nucleus? What is the general term for them? What are those particles composed of? 2. What is the definition of the atomic number? What is its symbol?

More information

4.06 Periodic Table and Periodic Trends

4.06 Periodic Table and Periodic Trends 4.06 Periodic Table and Periodic Trends Dr. Fred Omega Garces Chemistry 100, Miramar College 1 4.06 Periodic Table and Periodic Trend The Periodic Table and the Elements What is the periodic table? What

More information

VIIIA He IIA IIIA IVA VA VIA VIIA. Li Be B C N O F Ne. Na Mg VIB VIIB VIIIB IB IIB S. K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br

VIIIA He IIA IIIA IVA VA VIA VIIA. Li Be B C N O F Ne. Na Mg VIB VIIB VIIIB IB IIB S. K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br 188 THE FIRST TWO PERIODIC TRENDS IN A NUTSHELL LARGER IONIZATION ENERGY SMALLER RADIUS IA H IIA IIIA IVA VA VIA VIIA VIIIA He Li Be B C N O F Ne Na Mg IIIB IVB VB Al Si P VIB VIIB VIIIB IB IIB S Cl Ar

More information

Principles of Chemistry I 3150: EXAM I Thursday, 5:10PM EXAM FOR PRACTICE USE FALL 2017

Principles of Chemistry I 3150: EXAM I Thursday, 5:10PM EXAM FOR PRACTICE USE FALL 2017 Name Bubble on your scan sheet the Test Number and Test Form below: Principles of Chemistry I 3150:151-800 EXAM I Thursday, 5:10PM EXAM FOR PRACTICE USE FALL 2017 TEST 6, FORM A September 29, 2016 200+

More information

Chemistry 112 Name Exam III Form A Section April 2,

Chemistry 112 Name Exam III Form A Section April 2, Chemistry 112 Name Exam III Form A Section April 2, 2013 email IMPORTANT: On the scantron (answer sheet), you MUST clearly fill your name, your student number, section number, and test form (white cover

More information