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General Inorganic CHEM 112 Spring 2010

Page history last edited by Juana Mendenhall 14 years, 1 month ago

          CHEM 112-03 ELEMENTAL INORGANIC CHEMISTRY Spring 2010                           

 Instructor: Dr. Juana Mendenhall  Email: jmendenhall@morehouse.edu

Office Location: 218 Merrill Hall Phone: 404-681-2800 x 2286

 


This course will introduce the fundamental principles that underlie all of chemistry.  Throughout the semester you will learn:

-The role and significance of elemental inorganic chemistry in general, physical, and organic chemistries.

-How to understand the basic concepts of chemistry and use them when solving chemical equations or problems.

After completing this course, students will understand and know how to:

Describe how the rate of a reaction is related to the rate of disappearance of a reactant or formation of a product; Explain how to obtain the data needed for a kinetic study from the results of a simple chemical analysis;

Establish the exact rate of a chemical reaction from the slope of a tangent line to the concentration vs. time graph; In addition to explaining how to determine the initial rate; State the meaning of reaction order; using the rate law to determine the order of a reaction;

Apply the method of initial rates to determine the rate law for a reaction;

Use the rate law and rate data to calculate a rate constant (k), or use the rate law and the rate constant to calculate rate data;

Apply the integrated rate law and establish through rate data, equations, and graphs, whether a reaction is zero order, first order, or second order;

Describe the collision theory of reactions, stating the factors that affect collision frequency and those that lead to favourable collisions;

Explain the concept of activation energy;

Show how transition-state theory extends theoretical explanations of chemical kinetics;

Use the Arrhenius equation in calculating involving rate constants, temperatures, and activation energies;

Describe a reaction mechanism, and distinguish between elementary process and net chemical reactions;

Derive the rate law from a simple mechanism with the concepts of steady-state condition and rate-determining step;

Describe the role of a catalyst and explain the difference between homogenous and heterogeneous catalysis.

Describe the condition of equilibrium in a reversible reaction and how equilibrium concentrations are established experimentally;

Write the equilibrium constant expression in terms of concentrations Kc for a reaction, and use the value of Kc and the concentrations of all species but one to determine the equilibrium concentration of that species;

Derive K values for situations where chemical equations are reversed, multiplied through by constant coefficients or added together;

Assess the relative importance of the forwards and reverse reactions from the magnitude of an equilibrium constant;

Write an equilibrium constant expression in terms of partial pressures of gases (Kp), and relate the value of Kp to the corresponding value of Kc;

Calculate a numerical value of an equilibrium constant if equilibrium conditions are given;

Predict the direction in which a reaction proceeds toward equilibrium by comparing the reaction quotient, Qc to Kc;

Use the ideal gas law and Dalton’s law of partial pressures in working with Kp expressions;

Apply Le Châtelier’s principle by making qualitative predictions of how equilibrium conditions change when an equilibrium mixture is disturbed;

Calculate the final equilibrium condition in reversible reaction from a given set of initial conditions;

Calculate the new equilibrium concentrations or partial pressures after an equilibrium system has adapted to changed conditions;

Describe the similarities and differences among the Arrhenius, Brønsted-Lowry, and Lewis theories of acids and bases;

Identify Brønsted-Lowry conjugate acids and bases; write equations of acid-base reactions;

Identify Lewis acid-base reactions and write equations for acid-base reactions that involve them;

Explain what self-ionization (for autoionization) is, and describe the nature of the proton in aqueous solution;

Calculate ion concentrations in solutions of strong electrolytes, and relate [H3O+] and [OH-] through, Kw;

Given a value of any one of [H3O+], [OH-], pH, and pOH, be able to compute values of the other three.

Identify a weak acid or base, write a chemical equation to represent its ionization, and set up its ionization constant expression;

Calculate one Ka, [H3O+], or the molarity of a weak acid, given the other two (and perform similar calculations for a weak base) and know how to simplify these calculations by making suitable approximations;

Use the relative strengths of Brønsted-Lowry acids and bases to predict the direction of acid-base reactions;

Describe the effect of common ions on the ionization of weak acids and bases, and calculate the concentrations of all species present in solutions of weak acids or bases and their common ions;

Explain why the pH of water changes markedly when a small amount of H3O+ or OH- is added, and why the pH of a buffer does not change very much with a similar addition;

Describe how buffer solutions can be prepared;

Know the limitations of the basic equations used to determine the pH of buffer solutions (Henderson-Hasselbalch equation) by understanding their derivations;

Calculate the pH of a buffer solution from concentrations of the buffer components and a value of Ka or K, and describe how to prepare a buffer that has a specific pH;

Determine the changes in pH of buffer solutions resulting from adding acids or bases;

Explain how an acid-base indicator works to determine the equivalence point in a titration;

Calculate pH values and plot the titration curve of a strong acid with a strong base, or a strong base with a strong acid;

Calculate pH values and plot the titration curve of a weak acid with a strong base or of a weak base with a strong acid;

Plot titration curves and use those curves to determine the initial pH, buffer region, and the pH of the equivalence point, as well as to select an appropriate indicator;

Write the solubility product expression Ksp for a slightly soluble ionic compound;

Calculate Ksp from the solubility of an ionic compound or solubility from the value of Ksp;

Calculate the effect of common ions on the aqueous solubilites of sparingly soluble salts;

Determine if a salt will precipitate from solutions based on the concentration of its ions;

Determine the concentration of ions remaining in solution after precipitation and predict whether precipitation will be complete;

Describe, through net ionic equations and calculations, the effect of pH on the precipitation and dissolving of certain substances;

Write equations showing the effect of complex ion formation on other equilibrium processes such as solubility equilibrium;

Describe how a voltaic cell operates, using the concepts of electrodes, salt bridges, half-cell reactions, net cell reaction, and cell diagram;

Describe the standard hydrogen electrode and explain how other standard electrode potentials are related to it;

Use tabulated standard potentials, Eº, to determine Eºcell for an oxidation-reduction reaction and predict whether the reaction is spontaneous;

Quantitatively and qualitatively predict the effect of varying conditions (concentrations and gas pressures) on the value of Ecell;

Explain the corrosion of metals in the electrochemical terms and describe methods of corrosion protection;

Describe an electrolyte cell and how it differs from a voltaic cell;

Use Faraday’s laws to relate the quantity of chemical change produced by a given amount of electric charge;

Distinguish between heat and work and use specific heat to determine temperature changes and quantities of heat;

Interconvert joules and calories and apply the first law of thermodynamics;

Know the definition of work and calculate pressure-volume work for a gas;

State the meaning of the concept of state function, demonstrated by enthalpy;

Calculate the heat of a reaction at constant volume, qv, from bomb calorimetry data;

Explain how to use a Styrofoam coffee cup calorimeter and interpret the data obtained;

Apply Hess’s Law of constant heat summation;

State the definitions of standard state and standard formation reaction, and write the standard formation reaction for any substance;

Apply Hess’s law in special case of standard formation reactions; that is, compute ∆Hºrxn from ∆Hºf ;

Explain the meaning of spontaneous change as it applies to chemical reactions;

Explain why entropy is important and how it is related to the disorder of the system;

Know the relationship between entropy, heat, and temperature;

Know the Boltzmann equation for entropy;

Explain why entropy alone is not used to predict a spontaneous change and why free energy is needed;

Qualitatively predict whether reactions are spontaneous or nonspontaneous based on their change in enthalpy or entropy values;

Determine ∆Gº from tabulated data, both tables of ∆Gºf and those of ∆Hºf and Sº;

Understand and implement the Gibbs-Helmholtz equation, to determine ∆Gº at various temperatures;

Write the thermodynamic equilibrium constant expressions Keq for reactions and relate these to Kp and Kc;

Compute the values of Keq from tabulated data and ∆Gº = -RT ln Keq;

Explain how absolute entropies are determined with the third law of thermodynamics;

Apply the fundamental expressions relating to frequency, wavelength, and velocity of electromagnetic radiation, with appropriate units;

List the various types of radiation and their approximate wavelengths;

Know how light is dispersed into a spectrum and the difference between continuous and line spectra;

Use the Rydberg equation to determine the wavelengths of lines in hydrogen’s spectrum;

Know and be able to use Planck’s equation;

Know and be able to apply Bohr’s model of the hydrogen atom: the assumptions, the picture of the atom, the energy expression, and the energy-level diagram;

Summarize de Broglie’s and Heisenberg’s ideas;

Explain the differences between Bohr’s and Schrödinger’s models of the atom;

Know and be able to apply the quantum number relationships of wave mechanics;

Know what an orbital is and sketch the appearance of s, p, and d orbitals;

Know how orbital energies are modified when more than one electron is present in an atom;

Learn the three basic principles governing electron configuration;

Apply the Aufbau principle; write electron configurations with many different methods;

Use the periodic table to describe the Aufbau process and explain the basic features of the electron configurations of the representative and transition elements, esp., the number of valence electrons in each representative group;

Use the periodic law, the periodic table, and trends in atomic properties to make predications about the physical and chemical behaviour of various elements;

State the basic assumptions of the Lewis theory and relate the Lewis symbol for an element to its position in the periodic table;

Write Lewis structures for simple ionic compounds

Define electronegativity, and use its value to assess the relative metallic/non-metallic character of an element;

Use the basic rules of Lewis theory to propose a plausible skeleton structure for a molecule and assign valance electrons to this structure;

Compute the formal charge on each atom in a Lewis structure and use formal charges to determine which of several Lewis structures is the most plausible;

Recognize situations when resonance occurs, and draw plausible resonance structures;

Draw Lewis structures for odd-electron and electron-deficient structures;

State which elements can have expanded octets, and be able to draw Lewis structures with expanded octets;

Use bond distances to help in writing Lewis structures and bond energies to compute the enthalpy change of a reaction;

Predict the electron-pair geometry and molecular shape of a molecule or ion with VSEPR theory and know that single bonds act similarly to multiple bonds to determine molecular shape;

Use electronegativities to determine if a bond is polar, and use bond polarities and molecular shape to predict whether a molecule has dipole moment;

Explain the fundamental basis of valence bond theory;

Write the hybridization schemes for the formation of hybrid orbitals, and predict the geometrical shapes of molecules in terms of pure and hybrid orbitals used in bonding;

Use the relationship between VSEPR theory and valence bond theory to predict molecular geometries and bonding schemes;

Describe multiple bonds between second period elements in terms of the overlap of orbitals;

 

 

Required Texts  

General Chemistry Principles & Modern Applications 9th ed. by Petrucci, Harwood, Herring, and Madura. Students are expected to read all the assigned chapters/articles prior to class.  

 

Reference Material

General Chemistry The Central Science by Brown, LeMay, and Bursten 6th ed.

Chemistry by Chang 5th ed.

 

Co-requisites

Concurrent enrollment in Chemistry 112R and 112L. Note that students who have previously passed Chemistry 112L (grade C or better) are still required to register for Chemistry 112R.

 

NOTE: The Department will confirm the prerequisites and co-requisites for each student in this class. If a student is found to not have the proper prerequisites and co-prerequisites, they will be immediately and involuntarily withdrawn from the course, regardless of time spent in the course or performance in the course. If you believe that you do not have the proper prerequisites and co-prerequisites, you should notify the instructor immediately.

 

Grading Scale

100-93

A+

89-92

A

85-88

A-

82-84

B+

79-82

B

75-78

B-

72-74

C+

69-72

C

65-68

C-

60-64

D+

55-59

D

50-54

D-

0-50

F

 

                                               

 

 

 

 

 

 

 

 

 

 

 

 

 

Evaluation Point Scale

 

PLTL

25

Participation

10

Homework & Quizzes

75

Exams (3)

100

Final Exam

Total Points

100

510

 

                                                                                                                                                                                                                                                                                                                                                        

                                                                                                                                                     

Class Process & Policies

Attendance

This is a student centred discussion-based course and your active participation is essential to its success.  Punctual attendance at class meetings is required, and every absence affects your class participation grade. In the event of your absence, it is your responsibility to contact the instructor and make up any missed material. Every unexcused absence will lower the final grade by 5%.  Excused absences (e.g., physical illness, death of a close family member, religious holiday observance or personal/family emergency) will not affect your final grade. However, you may be asked to supply appropriate documentation. Travel is NOT an excused absence. Please plan holiday and other travel accordingly.

 

Participation

Respectful discussion is encouraged during class. Dr. Mendenhall may also ask questions of individual students during the lecture period, and the student’s answer will be factored into credit for participation. Chemistry can be a complex subject to understand and will require you to read the textbook and ask for help. The goal of participating in lecture is to make sure that learning chemistry is simple, fun, and exciting! CHEM 112-R is used as a tutoring and support mechanism to reinforce what you have done in lecture it is mandatory that you attend.

 

Questions & Concerns

I do not assume that you have background in my individual fields. If you catch me using jargon I did not define please raise your hand and ask us to define or clarify. Our goal is for everyone in the class to be engaged and participating in dialog, not for me to show you how much vocabulary I know. If you have questions, comments, or concerns about this course or research in general please ask or contact me by email. Keep in mind that we may not respond to your email immediately. Make sure that you ask questions or schedule meetings well in advance of upcoming deadlines. It is likely that other students in the class have questions similar to yours; so ask questions about class content, scheduling, or assignments during class times or on http://drjuanamendenhall.pbworks.com/General-Inorganic-Chem-112-Spring-2010.

 

Homework, Quizzes, as Exams

A suggested homework problem sheet will be given to you during the first week of class. The suggested homework problems will be essential in assisting you with understanding what is taught in the lecture component of the class. Please take the time to do each problem set at the end of every chapter. HOMEWORK problems for each chapter(s) are due at the day of the each exam (excluding the final exam). Quizzes maybe announced or unannounced it is your responsibility to prepare for lecture by working homework problems and reading the chapter.

 

Laptop Computers and Cellular Phones

Please do not bring your laptops to class unless we specifically ask you to.  Please turn all ringers and sound alerts on cell phones off before entering class. Cell phone calculators are not permitted on exams or quizzes. Please be advised that you will not be able to use any cell phone calculator on quiz or exam.

 

Academic Honesty

All students are expected to abide by the Morehouse College Honor Code.  Unfamiliarity with the Honor Code is not an excuse. Students may collaborate on the design and implementation of research studies, as well as on the evaluation of research articles. Reports and examinations, however, must be written independently and demonstrate some independent thinking. Cell phone calculators are not permitted on exams or quizzes. Please be advised that you will not be able to use any cell phone calculator on quiz or exam. The appearance of collaboration on written laboratory reports and/or examinations will result in a report to the Honor Council. If you are not already familiar with what constitutes academic dishonesty, please consult the Honor Code online at http://www.morehouse.edu.

     

 

Students with Disabilities or Special Needs

Morehouse College is committed to equal opportunity in education for all students, including those with documented disabilities. Students with disabilities or those who suspect they have a disability must register with the Office of Disability (“ODS”) in order to receive accommodations. Students currently registered with ODS are required to present their Disability Services Accommodations Letter to faculty (Dr. Mendenhall) immediately upon receiving the accommodations. If you have any questions, contact the Office of Disability Services, 104 Sale Hale Annex, Morehouse College, 830 Westview Dr. S.W., Atlanta, GA 30314 (404)-215-3626. http://www.morehouse.edu/campus_life/counseling_serv/disability.html.

 

 

 Additional Support

Robert W. Woodruff (Main) Library

You can contact librarians, specific to your discipline area (i.e. Chemistry, Biology, Engineering), which can help you identify research materials.  The library’s website has contact information as well as FAQs on researching at Emory.  We strongly encourage you to take advantage of the resources provided here. Their website is www.acutr.edu.

 

 

 

TENATIVE CLASS SCHEDULE (subject to change)

 

 

Week   

Date

Chapter

Topic

Class Reading

1

1/11/10

14

General Information & Review

Chapter 14

2

1/18/10

14

Chemical Kinetics

Chapter 14

3

1/25/10

15

Chemical Equilibrium & Acids & Bases

Chapter 15 & 16

4

2/1/10

15

Acids & Bases

Chapter 16 & 17

5

5

2/8/10

2/10/10

17

14-17

Acids & Bases II

Exam 1

STUDY

Chapter 18

6

2/14/10

18

Solubility & Complex Ion Equilibria

Chapter 20

7

2/21/10

20

Electrochemistry

Chapter 7

8

2/28/10

7

Thermochemistry

 

9

3/1/10

 

Spring Break

Chapter 19

10

3/7/10

19

Entropy & Free Energy

STUDY

10

3/14/10

7, 18-20

Exam 2

Chapter 8

11

3/21/10

8

Atomic Structure

Chapter 8,9

12

3/28/10

9

Periodic Table & Atomic Properties

Chapter 9, 25

13

13

4/2/10

4/2/10

9 & 25

8-9, 25

Periodic Table/Atomic Properties

Exam 3

STUDY

Chapter 10

14

15

16

4/4/10

4/11/10

4/18/10

10

11

10-11

Chemical Bonding I

Chemical Bonding II

Exam 4

Chapter 11

STUDY

17

4/25/10

cumulative

FINAL EXAM

 

 

 

 


 

 

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