Chemistry Program

STEM Institute

Chemistry 102 Syllabus

General Chemistry II

B R O O K D A L E C O M M U N I T Y C O L L E G E

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Code: CHEM-102 Title: General Chemistry II

Institute: STEM Department: Chemistry

Course Description: A continuation of CHEM 101, the student will investigate the areas of

kinetics, equilibrium, nuclear reactions, thermochemistry, electrochemistry, carbon chemistry and transition metal and organic chemistry using a problem solving approach to bring about understanding.

Prerequisites: grade of “C” or higher in CHEM 101 and in MATH 151.

Corequisites:

Prerequisites or Corequisites:

Credits: 5 Lecture Hours: 4 Lab/Studio Hours: 3

REQUIRED TEXTBOOK/MATERIALS:

Textbook: Book information is available in WebAdvisor through Search for Classes and College Bookstore.Laboratory Manual: Information available in WebAdvisory through Search for Classes and College Bookstore.Safety Goggles: New Jersey state law requires that all students wear appropriate splash and

impact proof safety goggles while performing laboratory experiments. They are available at the College Store

Laboratory Coat

ADDITIONAL TIME REQUIREMENTS:

Students must attend their regularly scheduled weekly laboratory class.

COURSE LEARNING OUTCOMES: Upon completion of this course, students will be able to:

Utilize critical thinking skills to learn fundamental chemical concepts from inorganic chemistry.

Use the scientific method to perform chemistry-based problem-solving. Reinforcement of

chemical concepts will be made as hands-on skills are developed in the laboratory program.

Determine the speeds at which reactions take place.

Calculate the pH at different points of a titration

Determine the enthalpy and entropy of a reaction

Name organic compounds

Write nuclear reactions

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GRADING STANDARD:

A = 92 – 100% A- = 89 - 91% B+ = 86 - 88% B = 82 - 85% B- = 79 - 81% C+ = 76 - 78% C = 70 - 75% D = 65 - 69% F = <65%

COURSE CONTENT:

Unit 1: Chemical Kinetics and Chemical Equilibrium

Unit 2: Acids and Bases and Acid-Base Equlibrium & Solubility Equilibrium

Unit 3: Thermochemistry, Entropy, Free Energy, and Electrochemistry

Unit 4: Organic Chemistry and Nuclear Chemistry

DEPARTMENT POLICIES:

1. Students must attend their regularly scheduled weekly laboratory section. Students arenot allowed to attend any other lab section for any reason.

2. Students must pass (65% or better) both the lecture and the laboratory portion of thecourse in the same semester or they will fail the course.

COLLEGE POLICIES: For information regarding:

Brookdale’s Academic Integrity Code

Student Conduct Code

Student Grade Appeal Process

Please refer to the BCC STUDENT HANDBOOK AND BCC CATALOG.

NOTIFICATION FOR STUDENTS WITH DISABILITIES: Brookdale Community College offers reasonable accommodations and/or services to persons with disabilities. Students with disabilities who wish to self-identify must contact the Disabilities Services Office at 732-224-2730 (voice) or 732-842-4211 (TTY) to provide appropriate documentation of the disability, and request specific accommodations or services. If a student qualifies, reasonable accommodations and/or services, which are appropriate for the college level and are recommended in the documentation, can be approved.

ADDITIONAL SUPPORT/LABS:

Learning assistants are available for help both for lab and lecture. The times of availability are posted at the learning assistants’ office.

WEBSITE: https://www.brookdalecc.edu/stem-institute/chemistry/

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Unit : #I of IV

Number of Chapters: 13,14

Name of Unit: Chemical Kinetics & Chemical Equilibrium

LEARNING OBJECTIVES RECOMMENDED PRACTICE EXERCISES

1. Represent reactions with rate expressions Read: 13.1

Do exercise: 13.27, 13.33

2. Classify the order of a reaction Read: 13.2

Do exercise: 13.33

3. Calculate the rate law of a reaction given data Read: 13.2

Do exercises: 13.21, 13.23,

13.29, 13.31,

13.35, 13.39

4. Correlate reactant concentrations or pressures Read: 13.3

with time Do exercises: 13.43, 13.45

5. Identify graphs of first and second order reactions Read: 13.3

Do exercise: 13.243, 13.45

6. Calculate activation energy both graphically and Read: 13.4

mathematically Do exercise: 13.59, 13.61

13.63

7. Classify the molecularity of a reaction and prove Read 13.6

if a given reaction mechanisms is plausible Do exercise: 13.73, 13.38,

13.81

8. Compare the three types of catalysis Read: 13.5

Do exercises: 13.18

9. Distinguish between one directional and Read: 14.1

equilibrium reactions. Write the equilibrium Do exercise: 14.2

constant expression for a reaction.

10. Write equilibrium constant Read: 14.1, 14.5

expressions for homogeneous and heterogeneous Do exercise: 14.13, 14.15

equilibrium reactions. Convert between Kp and Kc 14.17, 14.25

14.27 14.63,

14.64

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11. Identify the relationship between multiple .

equilibria reactions and each corresponding K

12. Predict the direction of an equilibrium reaction Read: 14.3

and calculate equilibrium concentrations Do exercise: 14.7, 14.29

14.42, 14.43

14.45, 14.47

13. Identify the factors that affect equilibrium and Read: 14.5

understand how each factor affects it. Do exercises: 14.8, 14.9

14.35, 14.36

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Unit : #II of IV

Number of Chapters: 15, 16, alternate text

Name of Chapters: Solutions of Acids and Bases, Reactions Between Acids and Bases

LEARNING OBJECTIVES RECOMMENDED PRACTICE EXERCISES

1. Identify conjugate acid-base pairs for Read: 15.1

Bronsted acids and bases. Do exercise: 15.25, 15.26

15.27

2. Explore the acid-base properties of water Read: 15.2

using the ion-product constant, Kw Do exercise: 15.33

3. Calculate pH and pOH Read: 15.2

Do exercise: 15.3, 15.4

15.37, 15.39,

15.130

4. Differentiate between strong and weak Read: 15.3, 15.4

acids and bases. Write dissociation reactions Do exercise: 15.32,

5. Write ionization constant expressions for weak Read: 15.5, alternate text

acids. Calculate pH of weak acids and percent Do exercise: 15.44, 15.46

ionization 15.48, 15.50

6. Write ionization constant expressions for weak Read: 15.6, alternate text

bases. Calculate pH of weak bases and percent Do exercise: 15.54, 15.56

ionization

7. Identify the relationship between the ionization Read: 15.7, 15.8

constants of acids and their conjugate bases. Do exercise: 15.51, 15.55

Calcluate pH for diprotic & polyprotic acids 15.61, 15.65

8. Determine the relationship between molecular Read: 15.8

structure and the strength of acids Do exercise: 15.100, 15.101

9. Determine the acid-base properties of salt Read: 15.6

solutions through the use of hydrolysis reactions Do exercise: 15.78, 15.69

10. Identify Lewis acids and bases Read: 15.9

Do exercise: 15.20, 15.107

15.109

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11. Differentiate between homogeneous and Read: 14.5, 16.2

heterogeneous equilibrium. Utilize the common Do exercise: 14.85

ion effect to calculate pH of weak acids and bases 16.29, 16.31

12. Identify, calculate pH of, and describe how to Read: 16.3

prepare buffer solutions Do exercise: 16.5, 16.43

16.45, 16.68

13. Calculate pH during acid-base titrations Read: 16.1, 16.2, 16.4, 16.5

Do exercise: 16.4, 16.14

16.27, 16.49

16.99

14. Understand how indicators function and Read: 16.6

select appropriate indicators for a given titration Do exercise: 16.10, 16.51

15. Write solubility products for slightly soluble salts. Read: 14.6

Calculate solubility and molar solubility. Predict Do exercise: 14.65, 14.69

if a precipitate will form under given conditions. 14.71, 14.72

14.79

16. Separate ions by fractional precipitation Read: 14.7

Do exercise: 14.83

17. Correlate the common ion effect with solubility Read: 14.7

Do exercise: 14.75, 14.77

14.78

18. Calculate pH from solubility Read: 16.9

Do exercise: 16.96

19. Calculate solubility of complex ions Read: 16.8

Do exercise:

20. Predict which ions may be present in a Read: 14.7

solution using qualitative analysis Do exercise: 14.80

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Unit: #III of IV

Number of Chapters: 5, 17, 18

Name of Chapters: Thermochemistry, Chemical Thermodynamics, Electrochemistry

LEARNING OBJECTIVES RECOMMENDED PRACTICE EXERCISES

1. Identify forms of energy. Read: 5.1

Describe what is exchanged in the 3 systems. Do exercise: 5.2, 5.4

2. Identify state functions. Demonstrate the First Read: 5.2, 5.4, 17.1, 17,2

Law of Thermodynamics. Calculate work done. Do exercise: 5.14, 17.7

17.29, 17.41

3. Correlate enthalpy and internal energy. Calculate Read: 5.2

the enthalpy of a reaction. Utilize thermochemical Do exercise 5.32, 5.37

equations to calculate the change in enthalpy. 5.87, 17.27

4. Calculate heats of reaction in constant-volume or Read: 5.3

constant-pressure calorimetry Do exercise: 5.57, 5.62

5. Calculate the standard enthalpy of reaction using Read: 5.4

the direct and indirect methods Do exercise: 5.27, 5.35

5.42, 5.68

5.67, 5.69

5.72. 5.77

5.86

6. Describe the heat of solution and dilution process

7. Distinguish between spontaneous and Read: 17.4

nonspontaneous processes. Do exercise: 17.15, 17.17

8. Define entropy and standard entropy. Determine the Read: 17.3

the higher entropy in a pair of substances. Determine Do exercise: 17.49

if the change in entropy of a system is + or -.

9. Correlate the second law of thermodynamics with Read: 17.3

the change in entropy of the universe. Calculate Do exercise: 17.11, 17.53

the change in entropy of system & surroundings.

Define The Third Law of Thermodynamics.

10. Calculate Gibbs free energy and standard free- Read: 17.4

energy changes for reactions and phase changes Do exercise: 17.57, 17.71

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11. Calculate the change in free energy in equilibrium Read: 17.5

reactions Do exercise: 17.91

12. Balance Redox Equations Read: 18.2

Do exercise: 18.31, 18.37

13. Identify the parts of electrochemical cells. Write Read: 18.3

half-cell reactions. Write cell diagrams. Do exercise: 18.39

14. Calculate standard cell potentials from standard Read: 18.4

reduction potentials (Table 19.1). Know how to Do exercise: 18.43

use that table in calculations.

15. Derive cell potential equations from ∆G and K. Read: 18.4

Calculate spontaneity of a reaction. Do exercise: 18.55, 18.60

16. Calculate cell potential using non-standard Read: 18.6

conditions/different concentrations Do exercise: 18.61, 18.69

17. Identify properties of types of batteries Read: 18.7

Do exercise: 18.71

18. Define corrosion and its prevention methods Read: 18.9

Do exercise: 18.88, 18.89

19. Define electrolysis and perform calculations Read: 18.8

involving electrolysis Do exercise: 18.81, 18.83

18.100

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Unit: # IV of IV

Number of Chapters: 21 & 22

Name of Chapters: Nuclear Chemistry, Organic Chemistry and Biochemistry

LEARNING OBJECTIVES RECOMMENDED PRACTICE EXERCISE S

1. Write balanced nuclear equations Read: 21.1

Do exercise: 21.25

2. Calculate nuclear binding energy. Determine Read: 21.1, 21.4

if a given isotope is stable or radioactive. Do exercise: 21.37, 21.41

21.49

3. Describe natural radioactivity and how Read: 21.2

radioactive dating is performed Do exercise: 21.35, 21.43

21.45

4. Describe the process of nuclear transmutation Read: 21.3

5. Describe the process of nuclear fission and its Read: 21.5

use in the development of the atomic bomb Do exercise:

and in reactors 23.55

6. Describe the process of nuclear fusion and its use Read: 21.5

in the hydrogen bomb and in reactors Do exercise: 21.16

7. Identify uses of isotopes Read: 21.6

Do exercise:

8. Determine the biological effects of radiation doses Read 21.6

9. Learn classes of organic compounds Read: 22.1-22.3

Do exercise: 22.3, 22.7

10. Name and draw aliphatic hydrocarbons. Read: 22.1, 22.3

Study aliphatic hydrocarbon reactions. Do exercise: 22.6, 22.17

Identify structural, optical, and geometric

isomers.

11. Name and draw aromatic hydrocarbons. Read: 22.2

Study aromatic hydrocarbon properties and Do exercise: 22.41

reactions.

12. Identify properties of the functional groups Read: 22.3

Do exercise: 22.45, 22.47

22.78