INSTRUCTIONAL METHODOLOGY

This course consists of a lecture section only.

This course covers the fundamental facts; laws, principles, theories and concepts of chemistry necessary for further work in science or science related subjects.

Course Objectives

1. Determine the rate of a reaction and its dependence on concentration, time, and temperature. 

2. Apply the method of initial rates to find the rate-law expression for a reaction and calculate k, the rate constant. 

3. Use the integrated rate-law expression for a reaction (the relationship between concentration and time). 

4. Describe the collision theory of reaction rates, transition state theory, and the role of activation energy in determining the rate of a reaction. 

5. Use Arrhenius equation to relate the activation energy for a reaction to changes in the rate constant with changes in temperature. 

6. Understand reaction mechanisms and how they lead to rate laws. 

7. Determine whether equilibrium has been established and calculate equilibrium concentrations. 

8. Derive the reaction quotient and explain the relationship between the reaction quotient and the equilibrium constant. 

9. Use LeChatelier’s Principle to predict the effects of concentration, pressure, and temperature change on equilibrium mixtures. 

10. Recognize strong electrolytes and calculate concentration of their ions. 

11. Calculate pH and pOH. 

12. Calculation involving ionization constants for weak monoprotic acids and bases and the concentrations of ions in dilute solutions. 

13. Use acid-base equilibrium concepts to salts of acids and bases. 

14. Understand the common ion effect and calculate the concentrations of all species in solutions containing common ions. 

15. Understand solubility product expressions and use Ksp in chemical calculations including effect of common-ions 

16. Use Ksp to calculate separation of ions by fractional precipitation and explain how simultaneous equilibria can be used to control solubility. 

17. Understand calculations with the thermodynamics functions, enthalpy, entropy, and free energy. 

18. Use of ΔG to predict if reaction is spontaneous at various temperatures and calculate K values 

19. Understand how to balance oxidation-reduction reactions. 

20. Write half-reactions and overall cell reactions for electrolytic processes. 

21. Understand the difference between Voltaic (galvanic) and electrolytic electrochemical cells. 

22. Determine standard and non-standard cell potentials. 

23. Understand interpretation, application, and calculations with Nernst equation. 

24. Understand the relationship of G, Ecell, and Keq 

25. Use Faraday’s Law of Electrolysis to calculate amounts of products formed, amount of current passes, time elapsed, and oxidation number. 

26. Understand the construction of simple Voltaic cells from half-cells and a salt bridge; identify the components; calculate the emf for the cell; and write half-reactions and overall cell reactions for a voltaic cell. 

27. Understand the coordination compounds and identify the ligands and their donor atoms. 

28. Determine the coordination number and the oxidation state of the metal and the charge on any complex ion. 

29. Nomenclature of coordination compounds, structures and isomers. 

30. Understand different types of isomers 

31. Understand the difference between nuclear reactions and chemical reactions. 

32. Understand the relationship between neutron-proton ratio, nuclear stability, and band of stability. 

33. Understand the common types of radiations emitted when nuclei undergo radioactive decay. 

34. Know how to calculate concentrations, half-lives, rate constants, time elapsed for first-order radioactive decay. 

35. Classify nuclear reactions as a fission or fusion. Calculate the energy released by a nuclear fission or fusion reaction. 

36. Understand how to write balanced equations for nuclear transmutations. 

37. Understand how to name alkanes, cycloalkanes, alkenes, alkynes, aromatic hydrocarbons, alcohols, ethers, amines, aldehydes, ketones, carboxylic acids, esters and amides 

38. Understand hybridization 

39. Understand simple organic reactions like substitution, addition, elimination, free-radical and polymerization. 

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COURSE EVALUATION/GRADING SCHEME

Chemistry 1312 (General Chemistry II) consists of eight units.  For each unit there will be a unit exam given in the testing center at the Riverside Campus.  Dates for each exam will be announced in lecture class well in advance.

                                    Units                                      Exams

                                    Unit I                                      Unit I Exam

                                    Unit II                                     Unit II Exam

                                    Unit III                                                Unit III Exam

                                    Unit IV                                                 Unit IV Exam

                                    Unit V                                     Unit V Exam

                                    Unit VI                                                 Unit VI Exam

                                    Unit VII                                  Unit VII Exam

                                    Unit VIII                                 Unit VIII Exam

Each exam may be retaken once.  Retests are to be taken at the Riverside Campus testing center.  All retests must be completed prior to the date on which the next regularly scheduled exam is given.  If a student chooses to retest, the final grade on the unit exam will be counted.

In addition to the credit earned on eight exams, 200 points of homework problems will be assigned during the course of the semester.  Homework assignments will be written on the board during the lecture periods, and must be handed in at the beginning of the next lecture meeting in order to receive credit.  Homework assignments handed in late will not be accepted for credit.

GRADING:   The total number of points available in this course is 1000

                                    8 Exams x 100 points  =  800 points

                                    Homework                  =  200 points

                                           Total           1000 points

The final grade will be assigned according to the percentage of points attained, that is 90% corresponds to a grade of A, 80% corresponds to a grade of B, 70% corresponds to a grade of C, 60% corresponds to a grade of D, and less than 60% corresponds to a grade of F.

                                                                   900  -  1000                A

                                                 800  -   899                 B

                                                 700  -   799                 C

                                                 600  -   699                 D

                                                     0  -   599                 F

General Education Student Learning Outcomes

Upon completion of this course, students will demonstrate competence in:

• Critical Thinking

Gathering, analyzing, synthesizing, evaluating and applying information.

• Interpersonal Skills

Interacting collaboratively to achieve common goals.

• Quantitative and Empirical Reasoning

Applying mathematical, logical and scientific principles and methods.

• Technology Skills

Using appropriate technology to retrieve, manage, analyze, and present information.

·       Written, Oral and Visual Communication
Communicating effectively, adapting to purpose, structure, audience, and medium.

Concealed Handgun Policy

·       The Austin Community College District concealed handgun policy ensures compliance with Section 411.2031 of the Texas Government Code (also known as the Campus Carry Law), while maintaining ACC’s commitment to provide a safe environment for its students, faculty, staff, and visitors.

·       Beginning August 1, 2017, individuals who are licensed to carry (LTC) may do so on campus premises except in locations and at activities prohibited by state or federal law, or the college’s concealed handgun policy.

·       It is the responsibility of license holders to conceal their handguns at all times. Persons who see a handgun on campus are asked to contact the ACC Police Department by dialing 222 from a campus phone or 512-223-7999.

COURSE POLICIES

Attendance/Class Participation Regular and punctual class and laboratory attendance is expected of all students. If attendance or compliance with other course policies is unsatisfactory, the instructor may withdraw students from the class.

Withdrawal Policy It is the responsibility of each student to ensure that his or her name is removed from the roll should he or she decides to withdraw from the class. The instructor does, however, reserve the right to drop a student should he or she feel it is necessary. If a student decides to withdraw, he or she should also verify that the withdrawal is submitted before the Final Withdrawal Date. The student is also strongly encouraged to retain their copy of the withdrawal form for their records. Students who enroll for the third or subsequent time in a course taken since Fall, 2002, may be charged a higher tuition rate, for that course. State law permits students to withdraw from no more than six courses during their entire undergraduate career at Texas public colleges or universities. With certain exceptions, all course withdrawals automatically count towards this limit. Details regarding this policy can be found in the ACC college catalog.

Incompletes An instructor may award a grade of “I” (Incomplete) if a student was unable to complete all of the objectives for the passing grade in a course due to medical/emergency reasons.  Students must have successfully completed at least 60% of the course materials to get an incomplete. An incomplete grade cannot be carried beyond the established date in the following semester. The completion date is determined by the instructor but may not be later than the final deadline for withdrawal in the subsequent semester.

Statement on Scholastic Dishonesty A student attending ACC assumes responsibility for conduct compatible with the mission of the college as an educational institution. Students have the responsibility to submit coursework that is the result of their own thought, research, or self-expression. Students must follow all instructions given by faculty or designated college representatives when taking examinations, placement assessments, tests, quizzes, and evaluations. Actions constituting scholastic dishonesty include, but are not limited to, plagiarism, cheating, fabrication, collusion, and falsifying documents. Penalties for scholastic dishonesty will depend upon the nature of the violation and may range from lowering a grade on one assignment to an “F” in the course and/or expulsion from the college.

See the Student Standards of Conduct and Disciplinary Process.

Student Rights and Responsibilities Students at the college have the rights accorded by the U.S. Constitution to freedom of speech, peaceful assembly, petition, and association. These rights carry with them the responsibility to accord the same rights to others in the college community and not to interfere with or disrupt the educational process. Opportunity for students to examine and question pertinent data and assumptions of a given discipline, guided by the evidence of scholarly research, is appropriate in a learning environment. This concept is accompanied by an equally demanding concept of responsibility on the part of the student. As willing partners in learning, students must comply with college rules and procedures.

Statement on Students with Disabilities Each ACC campus offers support services for students with documented disabilities. Students with disabilities who need classroom, academic or other accommodations must request them through the office of Student Accessibility Services (SAS). Students are encouraged to request accommodations when they register for courses or at least three weeks before the start of the semester, otherwise the provision of accommodations may be delayed. Students who have received approval for accommodations from SAS for this course must provide the instructor with the ‘Notice of Approved Accommodations’ from SAS before accommodations will be provided. Arrangements for academic accommodations can only be made after the instructor receives the ‘Notice of Approved Accommodations’ from the student. Students with approved accommodations are encouraged to submit the ‘Notice of Approved Accommodations’ to the instructor at the beginning of the semester because a reasonable amount of time may be needed to prepare and arrange for the accommodations. Additional information: about Student Accessibility Services.

Safety Statement Austin Community College is committed to providing a safe and healthy environment for study and work. You are expected to learn and comply with ACC environmental, health and safety procedures and agree to follow ACC safety policies. Additional information on these can be found at http://www.austincc.edu/offices/environmental-health-safety-and-insurance. Because some health and safety circumstances are beyond our control, we ask that you become familiar with the Emergency Procedures poster and Campus Safety Plan map in each classroom.

Additional information about emergency procedures and how to sign up for ACC Emergency Alerts to be notified in the event of a serious emergency can be found at.

Please note, you are expected to conduct yourself professionally with respect and courtesy to all. Anyone who thoughtlessly or intentionally jeopardizes the health or safety of another individual will be immediately dismissed from the day’s activity, may be withdrawn from the class, and/or barred from attending future activities.

Use of ACC EmailAll College e-mail communication to students will be sent solely to the student’s ACCmail account, with the expectation that such communications will be read in a timely fashion. ACC will send important information and will notify you of any college related emergencies using this account. Students should only expect to receive email communication from their instructor using this account. Likewise, students should use their ACCmail account when communicating with instructors and staff. Instructions for activating an ACCmail account.

Testing Center Policy Under certain circumstances, an instructor may have students take an examination in a testing center. Students using the Academic Testing Center must govern themselves according to the Student Guide. Use of ACC Testing Centers and should read the entire guide before going to take the exam. To request an exam, one must have:

·       ACC Photo ID

·       Course Abbreviation (e.g., CHEM)

·       Course Number (e.g.,1305)

·       Course Synonym (e.g., 10123)

·       Course Section (e.g., 005)

·       Instructor's Name

Do NOT bring cell phones to the Testing Center. Having your cell phone in the testing room, regardless of whether it is on or off, will revoke your testing privileges for the remainder of the semester. ACC Testing Center policies.

Student And Instructional Services ACC strives to provide exemplary support to its students and offers a broad variety of opportunities and services. Information on these services and support systems is available here. Links to many student services and other information can be found at Current Students. ACC Learning Labs provide free tutoring services to all ACC students currently enrolled in the course to be tutored. The tutor schedule for each Learning Lab may be found here.

For help setting up your ACCeID, ACC Gmail, or ACC Blackboard, see a Learning Lab Technician at any ACC Learning Lab.

COURSE OUTLINE/CALENDAR

Week 1                       Unit 1                                     Unit 1

Week 2                       Unit 1                                     Test 1 Review

Week 3                       Unit 2                                     Unit 2

Week 4                       Unit 2                                     Unit 2

Week 5                       Test 2 Review                                    Unit 3

Week 6                       Unit 3                                     Unit 3

Week 7                       Unit 3                                     Test 3 Review

Week 8                       Unit 4                                     Unit 4

Week 9                       Test 4 Review                                    Unit 5

Week 10                     Unit 5                                     Unit 5

Week 11                     Test 5 Review                                    Unit 6

Week 12                     Unit 6                                     Test 6 Review

Week 13                     Unit 7                                     Unit 7

Week 14                     Unit 7                                     Unit 7

Week 15                     Test 7 Review                                    Unit 8

Week 16                     Unit 8                                     Test Unit 8

Please note that schedule changes may occur during the semester.  Any changes will be announced in the class.

Chemistry 1312

General Chemistry II

Reading List

Textbook: Chemistry:The Central Science, 13th Edition, by Brown, Lemay and Bursten

Unit I              Chemical Kinetics

Sections           14.1 – 14.7

Unit II             Chemical Equilibrium I

Sections           15.1 – 15.7, 16.1 – 16.3

Unit III            Chemical Equilibrium II

Sections           16.4 – 16.11, 17.1 – 17.7

Unit IV            Coordination Chemistry

Sections           23.1 – 23.5

Unit V             Thermochemistry

Sections           5.1 – 5.7, 20.1 – 20.4

Unit VI            Electrochemistry        

Sections           20.1 – 20.7

Unit VII          Organic Chemistry

Sections           24.1 – 24.4

Unit VIII         Nuclear Chemistry     

Sections           21.1 – 22.9

 GENERAL CHEM-II (1312) 

Course Objectives 

Kinetics 

Reaction rates 

Rate law 

Integrated rate equations and half-life 

Collision theory 

Activation energy, 

Transition state, Arrhenius equation 

Catalysis 

Reaction mechanisms, rate-limiting step 

Chemical Equilibrium 

Dynamic equilibrium; homogeneous versus heterogeneous equilibria 

Equilibrium constant and related calculations 

Kp and Keq 

Factors affecting equilibrium and Keq: 

Reaction quotient 

Effect of Catalysts on equilibrium 

Relative stabilities of reactants and products 

LeChatelier's principle 

Predict direction of reversible reactions 

Chemical Applications 

Arrhenius, Brønsted, and Lewis acid-base definitions 

Ionization of pure water and Kw 

Effect of structure on acidity 

pH calculations with strong and weak acids and bases, 

Ka, Kb and relation to pH, pKa & pKb 

Common ion effect 

acidic and basic salts Hydrolysis of salts 

Common polyprotic acids and pH 

Buffers and buffer calculations, Henderson-Hasselbalch equation 

Titration curves 

Ksp, molar solubilities, precipitates 

Predict if ppt will occur in a solution 

Solubilities and pH and common-ion effect on solubility 

Thermodynamics 

Second and Third laws of thermodynamics 

Entropy, spontaneity, standard entropy 

Gibbs free energy 

Gibbs free energy, standard free energies of formation 

Predict spontaneity of reactions 

Relationship between G and K 

Electrochemistry 

Oxidation-reduction reactions 

Half-reactions 

Voltaic cells 

Standard cell potentials 

Predict redox reaction in combination of half-cells 

Nernst equation 

Concentration cells 

Relation of G, Ecell and Keq 

Electrolytic cells 

Faraday's law of Electrolysis 

Quantitative electrolysis 

Organic Chemistry 

Introduction to organic chemistry 

Nomenclature of alkanes, cycloalkanes, alkenes, alkynes, aromatic hydrocarbons, alcohols, ethers, amines, aldehydes, ketones, carboxylic acids, esters and amides 

Hybridization 

Types of Organic reactions 

Coordination Compounds 

Coordination compounds 

Ligands, coordination numbers 

Nomenclature 

Structural isomers and stereoisomers 

Nuclear Chemistry 

 Radiation, nuclear decay reactions 

 Modes of decay 

 Nuclear stability and n/p ratio 

 Write equation for nuclear reaction 

 Energies of nuclear reactions and nuclear binding energies 

 Kinetics of nuclear decay 

 Radioisotopic dating 

 Transmutation reactions 

 Nuclear fission and fusion, and applications in nuclear power plants 

Upon successful completion of this course, students will be able to the following: 

1. Determine the rate of a reaction and its dependence on concentration, time, and temperature. 

2. Apply the method of initial rates to find the rate-law expression for a reaction and calculate k, the rate constant. 

3. Use the integrated rate-law expression for a reaction (the relationship between concentration and time). 

4. Describe the collision theory of reaction rates, transition state theory, and the role of activation energy in determining the rate of a reaction. 

5. Use Arrhenius equation to relate the activation energy for a reaction to changes in the rate constant with changes in temperature. 

6. Understand reaction mechanisms and how they lead to rate laws. 

7. Determine whether equilibrium has been established and calculate equilibrium concentrations. 

8. Derive the reaction quotient and explain the relationship between the reaction quotient and the equilibrium constant. 

9. Use LeChatelier’s Principle to predict the effects of concentration, pressure, and temperature change on equilibrium mixtures. 

10. Recognize strong electrolytes and calculate concentration of their ions. 

11. Calculate pH and pOH. 

12. Calculation involving ionization constants for weak monoprotic acids and bases and the concentrations of ions in dilute solutions. 

13. Use acid-base equilibrium concepts to salts of acids and bases. 

14. Understand the common ion effect and calculate the concentrations of all species in solutions containing common ions. 

15. Understand solubility product expressions and use Ksp in chemical calculations including effect of common-ions 

16. Use Ksp to calculate separation of ions by fractional precipitation and explain how simultaneous equilibria can be used to control solubility. 

17. Understand calculations with the thermodynamics functions, enthalpy, entropy, and free energy. 

18. Use of ΔG to predict if reaction is spontaneous at various temperatures and calculate K values 

19. Understand how to balance oxidation-reduction reactions. 

20. Write half-reactions and overall cell reactions for electrolytic processes. 

21. Understand the difference between Voltaic (galvanic) and electrolytic electrochemical cells. 

22. Determine standard and non-standard cell potentials. 

23. Understand interpretation, application, and calculations with Nernst equation. 

24. Understand the relationship of G, Ecell, and Keq 

25. Use Faraday’s Law of Electrolysis to calculate amounts of products formed, amount of current passes, time elapsed, and oxidation number. 

26. Understand the construction of simple Voltaic cells from half-cells and a salt bridge; identify the components; calculate the emf for the cell; and write half-reactions and overall cell reactions for a voltaic cell. 

27. Understand the coordination compounds and identify the ligands and their donor atoms. 

28. Determine the coordination number and the oxidation state of the metal and the charge on any complex ion. 

29. Nomenclature of coordination compounds, structures and isomers. 

30. Understand different types of isomers 

31. Understand the difference between nuclear reactions and chemical reactions. 

32. Understand the relationship between neutron-proton ratio, nuclear stability, and band of stability. 

33. Understand the common types of radiations emitted when nuclei undergo radioactive decay. 

34. Know how to calculate concentrations, half-lives, rate constants, time elapsed for first-order radioactive decay. 

35. Classify nuclear reactions as a fission or fusion. Calculate the energy released by a nuclear fission or fusion reaction. 

36. Understand how to write balanced equations for nuclear transmutations. 

37. Understand how to name alkanes, cycloalkanes, alkenes, alkynes, aromatic hydrocarbons, alcohols, ethers, amines, aldehydes, ketones, carboxylic acids, esters and amides 

38. Understand hybridization 

39. Understand simple organic reactions like substitution, addition, elimination, free-radical and polymerization. 

Assessment: 

The expected learning outcomes will be assessed through the use of homework, assignments and/or quizzes, regular exams and the final exam. 

1. Determine the rate of a reaction and its dependence on concentration, time, and temperature. 

2. Apply the method of initial rates to find the rate-law expression for a reaction and calculate k, the rate constant. 

3. Use the integrated rate-law expression for a reaction (the relationship between concentration and time). 

4. Describe the collision theory of reaction rates, transition state theory, and the role of activation energy in determining the rate of a reaction. 

5. Use Arrhenius equation to relate the activation energy for a reaction to changes in the rate constant with changes in temperature. 

6. Understand reaction mechanisms and how they lead to rate laws. 

7. Determine whether equilibrium has been established and calculate equilibrium concentrations. 

8. Derive the reaction quotient and explain the relationship between the reaction quotient and the equilibrium constant. 

9. Use LeChatelier‟s Principle to predict the effects of concentration, pressure, and temperature change on equilibrium mixtures. 

10. Recognize strong electrolytes and calculate concentration of their ions. 

11. Calculate pH and pOH. 

12. Calculation involving ionization constants for weak monoprotic acids and bases and the concentrations of ions in dilute solutions. 

13. Use acid-base equilibrium concepts to salts of acids and bases. 

14. Understand the common ion effect and calculate the concentrations of all species in solutions containing common ions. 

15. Understand solubility product expressions and use Ksp in chemical calculations including effect of common-ions 

16. Use Ksp to calculate separation of ions by fractional precipitation and explain how simultaneous equilibria can be used to control solubility. 

17. Understand calculations with the thermodynamics functions, enthalpy, entropy, and free energy. 

18. Use of ΔG to predict if reaction is spontaneous at various temperatures and calculate K values 

19. Understand how to balance oxidation-reduction reactions. 

20. Write half-reactions and overall cell reactions for electrolytic processes. 

21. Understand the difference between Voltaic (galvanic) and electrolytic electrochemical cells. 

22. Determine standard and non-standard cell potentials. 

23. Understand interpretation, application, and calculations with Nernst equation. 

24. cell, and Keq 

25. Use Faraday‟s Law of Electrolysis to calculate amounts of products formed, amount of current passes, time elapsed, and oxidation number. 

26. Understand the construction of simple Voltaic cells from half-cells and a salt bridge; identify the components; calculate the emf for the cell; and write half-reactions and overall cell reactions for a voltaic cell. 

27. Understand the coordination compounds and identify the ligands and their donor atoms. 

28. Determine the coordination number and the oxidation state of the metal and the charge on any complex ion. 

29. Nomenclature of coordination compounds, structures and isomers. 

30. Understand different types of isomers 

31. Understand the difference between nuclear reactions and chemical reactions. 

32. Understand the relationship between neutron-proton ratio, nuclear stability, and band of stability. 

33. Understand the common types of radiations emitted when nuclei undergo radioactive decay. 

34. Know how to calculate concentrations, half-lives, rate constants, time elapsed for first-order radioactive decay. 

35. Classify nuclear reactions as a fission or fusion. Calculate the energy released by a nuclear fission or fusion reaction. 

36. Understand how to write balanced equations for nuclear transmutations. 

37. Understand how to name alkanes, cycloalkanes, alkenes, alkynes, aromatic hydrocarbons, alcohols, ethers, amines, aldehydes, ketones, carboxylic acids, esters and amides 

38. Understand hybridization 

39. Understand simple organic reactions like substitution, addition, elimination, free-radical and polymerization.