Inorganic ChemistryAttached in next pages are the Syllabi and tests for

1) CHEM 281 Inorganic Chemistry: introduction and the lab component.

2) CHEM 281 Advanced Inorganic Chemistry: Advanced study of inorganic concpets and the lab component.

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CHEM 281 Syllabus

Louisiana Tech University: Chemistry 281 - Section 001, Winter 2013-14, TR 10:00 AM - 11:15 PM CTH 227

Labs W 2:00-06:15 PM CTH 303 Instructor:  Dr. Upali Siriwardane Office:  311 Carson Taylor Phone:  257-4941

Office hours:  MWF 8:00 am - 10:00 am;           E-mail:  Upali@latech.edu         Tu,Th  8:30-9:30 a.m. 1:00 - 2:00 pm  Course Homepage:  Blackboard: http://moodle.latech.edu/ and Follow menu to CHEM 281(001) Winter 12

Course objective: This is the first inorganic chemistry course designed primarily for chemistry, science and engineering majors who have an interest in the inorganic materials as it will be applied to future work in their professional careers. It attempts to give the student a general appreciation of the field of inorganic chemistry  with  a working knowledge  of  certain  of   its  more  important  phases as  summarized  in course syllabus and course calendar.

Text :   Chemistry: The Molecular Science REQUIRED TEXT: Inorganic Chemistry By Peter Atkins, Tina Overton,Jon Rourke, Mark Weller, Fraser Armstrong,  5th Edition 2010.OPTIONAL SUGGESTED TEXTS FOR READING: Inorganic Chemistry, Huheey and Keiter 1993, 4th Edition.Basic Inorganic Chemistry, Cotton, Wilkinson and Gaus 1995, 3rd Edition.Inorganic Chemistry, Bowser 1993.Inorganic Chemistry, Poterfield 1993, 2nd Edition.Advanced Inorganic Chemistry, Cotton and Wilkinson 1988, 5th Edition.Supplements:  A full copy of slides, my class lectures, homework, exam review guides and sample questions and answers are available online: Blackboard: http://moodle.latech.edu/ and Follow menu to CHEM 281(001)

Course Evaluation:  The final course grade will be based on a score of 1000 pts. (NO CURVE).

1. Three in class Exams: 40% (@ (400/3) pts. each) 400 pts.(40%)

2. Comprehensive Final Exam: Replace the one lowest of the three exams)

3. 15 in Class Quizzes: 10% (@10 pts. each) 100 pts.(10%)

4. Group Activity Assignments: 20% (@ 25 pts. each) 200 pts.(20%)

5. 6 Lab experiments & Reports 30% (@ 50 pts. each) 300 pts.(30%) Course Total 1000 pts.(100%)Bonus points: (50 maximum make-up pts.)

1. Bonus assignment: 50 pts. 50 pts. Bonus Total 50 pts.

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Class attendance:

You should attend all classes regularly and punctually. Attending classes just to take tests on test days does not reflect the complete learning/participation/experience provided in this course. The points you earned for the  about 15 in-class quizzes and about 10 group activity assignments reflect your class attendance/participation/experience. Failure to attend classes without proper excuses will lead to losing points for the in-class quizzes you missed and that may lead to a lower grade for you in this course. 

Grading Policy:

Grading Scale:     A = 100 - 90%    B = 89 - 80%    C = 79 - 70%    D = 69 - 60%     F = below 60%

Grades will be posted on Blackboard:  

Grades  will  be  posted  under  Course   Information   for  CHEM 281  on  Moodle.  Graded  group activity can be picked up in class or from the 311 Carson Taylor Hall.  

 Exams:  There will be three hourly exams during the class and an optional comprehensive final exam.   Contact me before an exam at 257-4941 if you will miss an exam due to a University allowed absence.    Only University allowed absences will  be eligible for making up an exam, turning in group activity assignments and lab reports late without penalty or dropping a quiz [bring dated proof within a week of the missed day(s)]. 

Hourly Exams:  January 5, 2013 Test 1   (Chps. 1&,2), January 31, 2014 Test 2   (Chps. 3 &4), February 28 , 2014, Test 3 ; (Chps. 5 & 6), Comprehensive Final Make Up Exam:  February 20, 2014 (10:00-12:15 AM, CTH 122).

NOTE:   For all exams you must bring the following: 1) The text book in case instructor allows using the tables in the book and 2) a Calculator.

Quizzes:   There will be 10-15 in-class quizzes -- about one per lecture – worth 10 points each. Each quiz will consist of 3 simple questions pertaining to the material we have covered on or before that day.  Quiz sheets with the date will be available at the beginning of each class to be used.  Why a quiz every class?  1) this requires you to come to class where you will learn more than on your own; 2) this assures me that you will be paying attention in class instead of talking to your neighbor, reading the newspaper, etc.; 3) how well you do on the quiz lets me know how well you are learning.

 Homework Assignments :   There will be about 10 Homework Assignments to be completed as the materials are introduced in the class.  Students can work study groups.  NOTE: Each student in   the  group  must   turn  in   their  own hand-written copy of   the  assignment  with   their  name printed in the upper right hand corner.   Your Homework Assignments handed in late (without justification) will lose 10% of the points per day past the due date.   The due date on the Homework Assignments means that the assignment is due in class on that day at the end of 

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class 11:15 AM.   Blank assignments  sheets  are available  on the webpage under homework: http://www.chem.latech.edu/~upali/chem281/Group-HW.html

Non-graded text book homework: There will also be nongraded text book homework problems assigned.     It   is  very important  that   you   do   the   non-graded   text   book   problems   because questions based on these will also appear on the exams.  If after attempting on your own, using solution manual and with your study group you have any trouble with the graded or non-graded homework problems, you should see me immediately!  

 Class Discussion:     I  will  be asking questions  in class   from.   You will  be  able to  discuss  the question with other students for a short period of time and answer as a group so tries to sit together.  

 Bonus Essay Assignment:   There will be one essay assignment.   It will be a 5-10 page typed essay with at  least 5 references (original articles-not web links) or equivalent assignment on some chemistry topic and it will be worth 40 points.  I will give you the topic during the first 3 weeks of classes.  It can be handed in anytime before/or on February 14, 2012 1 by 11:15 AM.

Helpful Hints for Learning Inorganic Chemistry:

1. Survey the assigned material for overall concepts before lecture-meaning SKIM READ THE BOOK!2. Go back and read the same material for comprehension focusing on unclear areas.3. Work problems within the chapter during this second reading.4. Go to lecture and take notes.5. Reread any remaining unclear areas.6. Work problems, work problems, work problems within and at the end of the chapter.

Work additional problems again and again until you fully comprehend the concept.

7. If you are still unclear about a concept, ask me but NOT on the day of the exam or the day before the exam (by then it will be too late for you to truly absorb the material).

Outside Class Assistance:  

If you can't meet with me during my office hours, then please contact me by e-mail or make an appointment with me.  A couple of days before the exams, I will hand out a study guide (which will also be posted on the internet at the beginning of the quarter) and will have a review/help session during class time. If you get a message on your returned group activity assignments or exams or by e-mail that says to COME SEE ME IMMEDIATELY, do so immediately so that we can get you on track for a good grade in this course.  

Class Rules:  

No talking while I am lecturing.  Turn cell phones off before entering class.  You are expected to pay attention to my lecture in order to learn the material presented and to complete group activity assignments on time.  If you fail to do so, you will lose points for group activity and all 

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available   BONUS   points.    Instructor only decides who are worthy of bonus points.   Any academic  misconduct,  whether  premeditated  or  unpremeditated   (as defined  in  the  Code of Student Conduct), will be reported to the Office of the Dean of Students for appropriate actions. 

Chapter Sections & Titles Pages Chapter Sections & Titles PagesTest 1Chapter 1. Atomic structure                                                       3 The origin of the elements                                                       31.1 The nucleosynthesis of light elements                                51.2 The nucleosynthesis of heavy elements                             61.3 The classification of the elements                                       8 The structures of hydrogenic atoms                                 101.4 Spectroscopic information                                                 101.5 Some principles of quantum mechanics                          111.6 Atomic orbitals                                                                     12 Many-electron atoms                                                           181.7 Penetration and shielding                                                 181.8 The building-up principle                                                   201.9 Atomic  arameters                                                              23Chapter 2. Molecular structure and bonding                     35 Lewis structures                                                                  352.1 The octet rule                                                                     352.2 Structure and bond properties                                       402.3 The VSEPR model                                                              45 Valence-bond theory                                                          482.4 The hydrogen molecule                                                   482.5 Homonuclear diatomic molecules                                  492.6 Polyatomic molecules                                                       49 Molecular orbital theory                                                   522.7 An introduction to the theory                                         522.8 Homonuclear diatomic molecules                                  552.9 Heteronuclear diatomic molecules                               582.10 Bond properties    60Test 2Chapter 3.The structures of simple solids                        71 The description of the structures of solids                 723.1 Unit cells and the description of crystal structures   723.2 The close packing of spheres                                         743.3 Holes in close-packed structures                                  76 The structures of metals and alloys                           773.4 Polytypism                                                                        773.5 Non-close-packed structures                                        783.6 Polymorphism of metals                                               793.7 Atomic radii of metals                                                   803.8 Alloys page                                                                      80 Ionic solids                                                                         833.9 Characteristic structures of ionic solids                     843.10 The rationalization of structures                              89

 Chapter 4. Acids and bases                               111 Brønsted acidity                                              1114.1 Proton transfer equilibria in water             1124.2 Solvent levelling                                            1154.3 Characteristics of Brønsted acids               1184.4 Simple oxoacids                                             1194.5 Anhydrous oxides                                          1224.6 Polyoxo compound formation                      123 Lewis acidity                                                       1254.7 Examples of Lewis acids and bases              1254.8 Group characteristics of Lewis acids            126Reactions and properties ofLewis acids and bases                                           1304.9 The fundamental types of reaction               1304.10 Hard and soft acids and bases                     132 Test 3Chapter 5. Oxidation and reduction                 141 Reduction potentials                                      1425.1 Redox half-reactions                                       1425.2 Standard potentials                                         1415.3 Trend in Standard potentials                          1445.4 The electrochemical series                             146Chapter 6. Physical techniques in inorganic chemistry                                             169 Diffraction methods                                    1696.1 X-ray diffraction                                               169 Absorption spectroscopy                             1736.3 Ultraviolet—visible spectroscopy                 1736.4 Infrared and Raman spectroscopy                 175Resonance techniques                                         1776.5 Nuclear magnetic resonance                         1776.6 Electron paramagnetic resonance                 181 Chemical analysis                                     1876.10 Atomic absorption spectroscopy                 1876,11 Elemental analysis                                       1886.12 Thermal methods                                         189 Magnetometry                                           190

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Laboratory component:

Seven laboratory experiments are selected from following categories depending on student interest. Specific instructions will be given during the lab on Wendesday 2:00-6:15 pm.

1. Glassblowing  Students make a test tube, connect two straight glass tubes,  bend glass to get U trap and make a T-joint

2. FTIR Spectroscopy Experiments:  Student prepares samples of metal carbonyl compounds and obtain their IR spectra, Rus gas samples (NH3 and HCL) and solid KBr samples. Learn about FT-IR techniques and software.

3. NMR Spectroscopy Experiment:  Student learn how to run NMR spectrometer: sample preparation, locking shimming, data collection. They will interpret the 1H and 13C data they obtain on organic and organometallic samples.

4. UV-VIS Spectroscopy Experiments:  Students run UV spectra of Ni (en)32+ and other organometallic compounds and learn the rage of their  absorptions   and intensities.

5. X-ray Diffraction Experiments:  Students prepare X-ray powder samples and learn how to run the -2 powder diffractometer and identify peak positions and search match with PDF data base.Vacuum line Synthesis and Inert atmosphere handlingStudents are exposed to handling air sensitive compounds using vacuum line and dry box.

6. Synthesis of Organometallic Compounds  Students are given the procedure Synthesize of CpFe(CO)2C(O)Ph from [CpFe(CO)2]2 , Na/Hg amalgam and benzoyl chloride.

7. High Pressure Synthesis  8. Thermal Analysis Experiments:  

Thermal Analysis of metals and hydrates of CuSO4.5H2O. They use Both DTA (tin)  and TGA (CuSO4.5H2O )to analyze their samples

9. Atomic Absorption Experiments:  Students prepare sample of  Pb and using a calibration determine the concentration of the sample.

10. GC Analysis  Students run a gas samples containing CH4 and CO2 and they learn to identify gases in the stream O2, N2 and the CH4 and CO2.

11. GC/MS Analysis Students are shown the operation of GC/MS and given the spectra of CpFe(CO)2C(O)Ph and other compounds. They assign the molecular ion fragments to Mass Spectral peaks.

12. Electrochemistry  They conduct as cyclic voltametic analysis of CpFe(CO)2C(O)Ph and other compounds (ferrocene).

Important Dates During the Winter 2011-12 Quarter:November    30 Classes begin December 20 Christmas holiday Begin at the end of classesJanuary   4 Christmas holiday Ends classes start 8:00 a.m.

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January   4 Classes resume, 8:00 a.m.January    16  ML King Jr., holiday January  17  Classes resume, 8:00 a.m.February              3                 Last day to drop courses or resign with "W" gradesFebruary    17 Mardi Gras holiday begins at the end of classesJanuary    23 Mardi Gras holiday Ends classes start 8:00 a.mFebruary 28 Last day of classesFebruary 29 Grades for graduating students due on BOSSMarch  2 Grades “live” on Student BOSSMarch  3 Commencement Day Changes on this syllabus:

Schedules on this syllabus are not contractual and may be changed by the instructor when it becomes necessary to do so as determined by the instructor.  However, any changes that are deemed necessary to be made will be communicated orally to the students during lecture.  Therefore, it is a requirement that students attend class on time or make themselves responsible for informing themselves of any changes made by the instructor during lectures.  

Last revised: November 30, 2011, Copyright © 2012, Louisiana Tech University, Department of Chemistry. All rights reserved.

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Louisiana Tech University Test 1. CHEM 281 (001). Winter 2011. Name:___________________

1. Explain how the nucleosynthesis of lighter and heavier chemical elements took place in the Universe.

2. Using the equations: E =  -2.178 x 10-18 J [1/n2f - 1/n2i] J,  = hc/E,Calculate the wavelength of light that can excite the electron in a ground state hydrogen atom to n = 7 energy level.

3. Calculate the nuclear binding energy per nucleon (MeV per nucleon)  of 208 Pb.  Mass defect (m) = Mass of Nuclide - mass of  (p + n +e ) amu

Proton mass: 1.00728 amu

Neutron mass: 1.00867 amu

Electron mass: 5.486 X 10-4 amu

931.5 MeV = 1 amu

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4. Describe the two components of components of wave function, y

5. Construct a quantum number tree for the principal quantum number n = 3.

6. Calculate the number of total, radial and angular nodes in 4d orbital# total nodes: _______

# radial nodes: _______

#angular nodes: _______

7. Which radial electron density function correspond to a 3s electron

8. How is Zeff the nuclear charge felt

by an electron in a multielectron atom is calculated?

9. Describe the following applied in obtaining an electronic configuration:a) The Building Up (Auf Bau) Principle:

b) Pauli Exclusion Principle:

c) Hunds Rule:

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10. Describe the trend of the following atomic properties in the periodic table:a) Atomic radii

b) Ionic radii

c) First ionization energies

d) Electron affinities

11. Describe following materials in terms of electrons:

a) diamagnetic;

b) paramagnetic;

c) ferromagnetic;

12. Give electronic configurations in the core format of the following:a) N :b) Ca:c) Fe :d) Fe2+ :

13. Determine the number of unpaired electrons in atoms a) O :b) Cr :c) Fe3+ :

14. Which atom has higher first ionization energy, N or O? Give a brief reason.

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15. Describe the difference between following types of radii:a) Covalent Radii: 

b) Van der Waals Radii:

c) Metallic Radii:. 

d) Ionic Radii: 

16. Using Octet Rule and Lewis dot symbols of elements describe why these three types of bonding is found in chemical substances:a) Covalent bonding

b) Ionic bonding

c) Metallic bonding

17. Draw a Lewis structure for PCl3 assuming P is the central atom.

18. Draw a Lewis structure for [POCl2]- ion assuming P is the central atom

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19. Draw the resonance structures of SO2 and calculate the partial bond order between S and O atoms.

20. How electronegativity difference between two atoms is is used to distinguish following types of bonding?a) Non-polar covalent

b) Polar covalent

c) Ionic

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Louisiana Tech University : Test 2.CHEM 281 (01) Winter 2011. Chapters 2 and 3. Name:_______________

1. Draw Lewis structures and predict the hybridization on the central atom:a) SiCl4

b) BF3

c) SF6

d) [Fe(H2O)6]+3

2. Would you expect Be2 to exist? Use a molecular orbital energy diagram to explain your reasoning.

3. What are there any differences in molecular orbital diagrams of B2, C2, N2, O2 and F2?

4. Draw a molecular orbital diagram for O2 determine the bond order and magnetic properties. 

5. Assuming that it has similar molecular orbital energies to those of carbon monoxide, deduce the bond order of the NO+ ion. (show your work)

6. Assuming that it has similar molecular orbital energies to those of carbonmonoxide, deduce the bond order of the NO- ion. (show your work)

7. Predict the intermolecular forces in following

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a) N2

b) CO2

c) CCl4

d) H2O

e) HCl

8. What  is  a  crystalline  material,  describe  the bonding and packing  in C(s)-diamond and how  it   is different from NaCl(s)? 

9. What is the coordination number of a metal atom in a face centered cube(FCC) ? 

10. Draw a simple cubic (SC) unit cell and label axes (a,b, c )and angles ()? 

11. Give the general unit cell dimensions for following crystal systems:

a)  Triclinic:      a=    b=   c=    b)  Tetragonal:  a=    b =  c=    c) Hexagonal:  a=    b=   c=   

12. What are seven crystal systems? a)  b)  c)  d)e)f)g)

13. Which would you expect to contain ionic bonds, MgCl2 or SC12? Explain your reasoning. 

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14. Draw pictures of:a)  AAAAA.. lose packing to show how a simple cubic (SC) unit cells are created.

b) Draw pictures of ABABABAB.. lose packing to show how a body centered cubic (BCC) unit cells are created.

15. How do you calculate the packing efficiency (52%) of cubic (SC) of a metal?

16. Calculate the number of atoms in a cubic unit cell of a metal:a) Simple cubic (SC):

b) Body-centered cubic (BCC)

c) Cubic closest-packed (CCP-FCC)

17. Give coordination number for both anion and cation of the following ionic lattices.a. CsCl Structure:

b. Rock Salt Structure: 

c. Fluorite Structure:

d. Sphalrite Structure:

Show  how many ions are per unit cell and show how it agrees with the formula of the pervoskite structure material, (1-2-3:Y-Ba-Cu)

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Louisiana Tech University CHEM 281. TEST 3. Chapters 4 & 5. Winter 2011-2012. Your Name: __________________ ID #:________

1. Arrange in the following ions in order of increasing acidity: [Al(OH2)6]2+, [Fe(OH2)6]3+, [Fe(OH2)6]2+. Give your reasoning.

2. Figure out the driving force for following reactions.a) Ca(OH)2  + H2SO4   --->  CaSO4  +  2H2O     b) Na2CO3 + 2HCl    --->  CO2(g) + H2O + 2NaClc) Mg + 2HCl     --->  MgCl2 + H2

a) __________________________________________b) __________________________________________c) __________________________________________

3. Identify the conjugate acid/base pairs in following reactions.a) CO3

2- + H2O  HCO3- + OH-

b) NH3 + HClO4   NH4+ + ClO4

-

    Acid1        Base2     Con-base1    Con-acid2

a) ______ ______ ______ ____________________b) ______ ______ __________________________

4. For each of the following processes, identify the Lewis acids and bases involved and characterize the process as complex formation or acid–base displacement. a) SO3 + H2O → HSO4

-   + H+

b) CH3[B12]   +   Hg2+ →  [B12]+    + CH3Hg+   (B12 designates the cobalt  macrocycle vitamin B12)

c) KCl + SnCl2         → K+    + [SnCl3]–   

d) AsF3 (g) + SbF5 (l) → [AsF2]+[SbF6]– (s)5. Explain the reaction sequence given below in terms of hard and soft Lewis acid-base behavior:

NaBr NaCNAuNO3 ---->  AuBr ----> [Au(CN)2]-

6. Explain why Na+ prefers F- to I- where as Cu+ prefers I- to F-.

7. Explain the role of Al2Cl6 as a Lewis acid catalyst in Friedel Craft Acylation of benzene. (show the steps in the reaction).

8. Explain the Lewis acidity trend observed in the following series: SiI4 > SiBr4 > SiCl4 > SiF4

9. For the redox reaction answer the following:          2Cr + 6HCl(aq)  2CrCl3 (aq) + 3H2(g)

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OHR:RHR:Oxidizing agent:Reducing agent:

10. Answer the following for  the redox  reaction that takes place in basic solution:           Al(s) + MnO4

-(aq) ----- MnO2(s) + Al(OH)4-(aq) (basic solution)

               OHR:              

 RHR:

Number of electrons transferred:              

 Net ionic equation:

Spectator ions:

Molecular equation:

11. Using the E0 values given in the table calculate the Eocell for reactions:          Fe(s) + Cu2+(aq)    Fe2+(aq) + Cu(s) 

identify following:a) Eocell;        b)  two half reactions;  

b) anode; c) cathode; d) direction of electron flow through the external wire.

Use Ellingham diagram given for following reactions:12. According to the Ellingham diagram, under what conditions might C 

be expected to reduce FeO to Fe?

13. According to the Ellingham diagram, under what conditions might aluminum be expected to reduce MgO?

14.  According to Ellinham diagram what temperature C expected to reduce CaO to Ca?

15. According to Ellinham diagram explain why a potential difference need to be applied  reduce Al2O3 to Al in it had to be accomplished at 1000ºC?

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Table of Selected Standard Potentials at 25°CCouple E° / VF2(g) + 2e- ® 2F-(aq) +3.05Ce4+(aq) + e- ® Ce3+(aq) +1.76MnO4

-(aq) + 8H+ + 5e- ® Mn2+(aq) + 4H2O(l) +1.51Cl2(g) + 2e- ® 2Cl-(aq) +1.36O2(g) + 4H+ + 2e- ® 2H2O(aq) +1.23[IrCl6]2-(aq) + e- ® [IrCl6]3-(aq) +0.87Fe3+(aq) + e- ® Fe2+(aq) +0.77[PtCl4]2-(aq) + 2e- ® Pt(s) + 4Cl-(aq) +0.76I3

-(aq) + 2e- ® 3I-(aq) +0.54[Fe(CN)6]3-(aq) + e- ® [Fe(CN)6]4-(aq) +0.36Cu2+(aq) + 2e- ® Cu(s) 0.34AgCl(s) + e- ® Ag(s) + Cl-(aq) +0.222H+(aq) + 2e- ® H2(g) 0AgI(s) + e- ® Ag(s) + I-(aq) -0.15Ni2+(aq) + 2e- ® Ni(s) -0.23Fe2+(aq) + 2e- ® Fe(s) -0.44Zn2+(aq) + 2e- ® Zn(s) -0.76Al3+(aq) + 3e- ® Al(s) -1.68Ca2+(aq) + 2e- ® Ca(s) -2.87Li+(aq) + e- ® Li(s) -3.04

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