COURSE SYLLABUS
GPC - Dunwoody
CRN# 31864
CHEM 1151-206 SURVEY OF CHEMISTRY I
Spring 2014
Class Time:
TR
Instructor:
Prof. Myung-Hoon Kim
Office: NE-2222
Phone: (770)274-5059
E-Mail: mkim@gpc.edu
Tutoring/Advisement Hrs: M W 1:00-4:00pm, T R 2:30-4:00pm, R* 10:00-11:00am (*at LTC)
facstaff.gpc.edu/~mkim (→ Class Materials → CHEM 1151)
Website:
1:00-2:15 pm
12/18/13
Lecture Room: NE-1260
Objective:
This course is designed to provide the foundation for understanding of the basic principles of chemistry
and its application to living systems.
Description:
This course is the first course of a two semester sequence in college chemistry for allied health sciences
majors and non-science majors. It is the normal choice for nursing, dental hygiene, and other career health
sciences. It is not for pre-medicine, pre-dentistry, pre-pharmacy, or physical therapy. It does not meet the
requirements of science and engineering majors. This is a pre-requisite for BIOL 1611, Human Anatomy and
Physiology I.
Prerequisite:
Exit or exemption from Learning Support Mathematics and exit or exemption from Learning Support
Reading or ENSL 0090 with a C or better. The student must be prepared to supply evidence in the form of a
grade report or a transcript that this prerequisite has been met. CHEM 1151L (laboratory) is a co-requisite.
Required Text & Materials:
The required text is Introduction to General, Organic & Biochemistry - Structure of Life (4th
edition K. C. Timberlake, Prentice Hall, 2013). Georgia Perimeter College Edition of Vol. I (for CHEM
1151) is also available. “MasteringChemistry” (an online homework system; www.masteringchemistry.com)
is required - Course ID: CHEM1151S206S2014.
Attendance:
Students are expected to attend all class meetings. In the event of absence it is the students'
responsibility to obtain assignments and information covered during the absence. A grade of W will be
assigned if the student officially withdraws by mid-point. After mid-point withdrawal will result in a F
grade unless a hardship waiver is granted by the department head. It is the student's responsibility to complete
withdrawal through the registrar's office in the event that becomes necessary. Withdrawal from lecture
automatically requires withdrawal from the lab and vice versa. A roll sheet will be circulated at the
beginning of class. A student who arrives late should stop by at the end of class and sign it. Topics of a
missed class, due to school closing from inclement weather (tune to WSB, AM 750 kHz, or Channel 2), will
be automatically assigned as a take-home project.
Tests:
There will be four class tests and a final exam. The final exam is required. There are no make-up
tests. The final course grade is obtained by averaging the three highest class exams, the Online Homework
and the final. If one of the class exams is missed, that exam becomes the dropped exam. The grading scale
is the standard scale with 90-100 = A (Excellent), 80-89 = B(Good), 70-79 = C(Fair), etc.
Three of Best Hour Exams:
MasteringChemistry:
Final Exam:
Total
300 pts
75 pts
125 pts
500 pts
(a) Each Hour Test has 25-30 Multiple Choices and 1-2 Big Write-Out Questions.
(b) Bring #2 pencils and the ParSCORE (red) Forms.
Classroom Conduct:
Students are expected to act with respect for the professor and other classmates. Arriving late for class
can be disruptive. In the event of a late arrival it is important to enter and take a seat quietly. Talking to others in
the class during lecture/discussion prevents others from hearing the proceedings. Leaving class during session is
very disruptive and should occur only in an emergency. Food and drink are not allowed in the classroom.
Student’s Responsibility:
Students must develop a fundamental understanding of chemical concepts as well as skill in solving
problems, and the best way to do this is to rewrite class notes and work through examples and the exercise
problems doing homework. The amount of time needed to be successful in this class may vary with
background, interest, motivation, study skills, and ability. To be successful, expect a minimum of twice of
the class time/wk outside of class to study and do homework. Concepts in chemistry build on one another,
so it is important not to fall behind. Note that the student is responsible for information in the book that
may not necessarily be covered in the lecture. The laboratory grade is separate and requires additional time.
Expect 3 to 6 hours at home to prepare for a lab sessions, analyze data, find results, and prepare lab reports.
Careful attention and good use of class time can reduce the time required outside of class. Remember that
you earn a grade.
CHEMISTRY 1151 SCHEDULE
Wk
1
2
3
4
5
6
7
8
9
10
11
12
13
14
15
16
17
T
R
Jan. 14
21
28
Feb. 4
11
18
16
23
30
6
13
20
(25) 26
Mar. 4 6*
(11 13)
18
25
Apr. 1
8
15
22
May 29
6
20
27
3
10
17
24
1
(8)
Chapter
1
1, 2
2
3
3, 4
4
5
5, 6
6
7
7, 8
8
9
9
10
10
- Dates may be subject to change. -
Test #
Date
I
II
III
IV
Final
Topics & Reading Assignment of the Week
Intro, Measurements
Measurements, Energy & Matter
Energy & Matter
Atoms and Elements
Atoms and Elements, Nuclear Chemistry
Nuclear Chemistry
(Study Day) Compounds and Their Bonds
Chemical Reactions & Quantities, (* Mid-point)
- Spring Break Quantitative Relationship
Gases
Solutions
Reaction Rates
Chemical Equilibrium
Acids & Bases
Acids & Bases
Comprehensive Exam, MasteringChemistry Due
Other Information:
(1) The course home pages provide some lecture materials, sample exams from the past,
other useful information.
(2) An effective way of studying is to form a study group with classmates that meets regularly.
(3) Extra points: 10 pts for a good attendance.
CHEMISTRY 1151 COURSE CONTENTS
Chapter 1
MEASUREMENTS
1. Units of Measurement
4. Significant Figures in Calculations
7. Problem Solving
2. Scientific Notation 3. Measured Numbers and Significant Figures
5. Prefixes & Equalities 6. Writing Conversion Factors Conversi
8. Density
Chapter 2
ENERGY and MATTER
1. Energy
2. Temperature
3. Specific Heat
5. Classification of Matter
6. States and Properties of Matter
4. Energy and Nutrition
7. Changes of State
- First Exam covers Chap. 1 & 2
Chapter 3
ATOMS and ELEMENTS
1. Elements and Symbols
2. The Periodic Table 3. The Atomic
4. Atom and Mass Number
5. Isotopes and Atomic Mass
6.Electron Energy Levels
7. The Electronic Configurations
8. Periodic Trends - Atomic Size & Ionization Energy
Chapter 4
NUCLEAR CHEMISTRY
1. Natural Radioactivity
2. Nuclear Reaction
3. Radiation Measurement
4. Half-Life of Radioisotope
5. Medical Application Using Radioactivity
6. Nuclear Fusion and Fusion.
- Second Exam covers Chap. 3 & 4
Chapter 5
COMPOUNDS AND THEIR BONDS
1. Octet Rule and Ions
2. Ionic Compounds
3. Naming and Writing Ionic Formulas
4. Polyatomic Ions
5. Covalent Compounds
6. Naming and Writing Covalent Formulas
7.Electronegativity and Bond Polarity 8. Shapes and Polarity of Molecules
9. Attractive Forces in Compounds
Chapter 6
CHEMICAL REACTIONS and Quantities
1. Equations for Chemical Reactions
2. Types of Reactions
3. Oxidation-Reduction Reactions
4. The Mole
5. Molar Mass 6. Mole Relationships in Chemical Reactions
7. Mass Calculations for Reactions
8. Percent Yields and Limiting Reactants
9. Energy Changes in chemical Reactions
- Third Exam covers Chap. 5 & 6
Chapter 7
GASES
1. Properties of Gases
2. Gas Pressure
3. Pressure & Volume (Boyle’s Law)
4. Temperature & Volume (Charles’s Law)
5. Temperature & Pressure (Gay-Lussac’s Law)
6. The Combined Gas Law
7. Volume & Moles (Avogadro’s Law)
8. Ther Ideal Gas Law
9. Partial Pressure (Dalton's Law)
Chapter 8
SOLUTIONS
1. Solutions
2. Electrolytes & Nonelectrolytes
3. Solubiliy
4. Solution Concentrations
5. Dilution of Solutions & Solution Reactions
6. Properties of Solutions
- Fourth Exam covers Chap. 7 & 8
Chapter 9
REACTION RATES AND CHEMICAL EQUILIBRA
1. Rates of Reactions
2. Chemical Equibrium
3. Equilibrium Constants
4. Using Equilibrium Constants 5. Changing Equilibrium Conditions: Le Chatlier’s Principle
Chapter 10
ACIDS and BASES
1. Acids and Bases
2. Strengths of Acids and Bases
4. The pH Scale
5. Reaction of Acids and Bases
6. Buffers: The Henderson-Hasselbalch Equation
3. Ionization of Water
- Final Exam is comprehensive covering Chap. 1 – 9
Expected Educational Results:
Upon successful completion of this course, students should be able to:
1. Relate law, hypothesis, theory, and the scientific method.
2. Convert decimal values to exponential notation: Use scientific notation in calculations
3. Use significant figures in calculation.
4. Demonstrate proficiency in the metric system and be able to convert metric and British units.
5. Use density relationships.
6. Convert temperatures among the different scales.
7. Name common elements from symbols, and write symbols for names.
8. Write complete symbols for atoms.
9. Distinguish between element, compound, and mixture.
10. Demonstrate understanding of atomic structure - protons, neutrons, and electrons.
11. Write out electron configurations for first 56 elements.
12. Relate intermolecular forces to physical properties such as boiling point.
13. Name compound from formula and write formula from name.
14. Write Lewis electron-dot structures for atoms and ions.
15. Identify ionic and covalent bonds.
16. Use electronegativity to determine bond polarity.
17. Predict molecular geometries, and relate polarity and molecular geometry.
18. Balance chemical equations.
19. Classify chemical reactions.
20. Calculate formula weight (from formula) and molar mass of an element or compound.
21. Convert moles of substance to grams and vice versa.
22. Use empirical gas laws and ideal gas laws.
23. Identify colligative properties.
24. Distinguish between colloids and solutions.
25. Define radiation and half-life.
26. Relate quantities in a chemical equation (stoichiometry), and find a limiting reactant.
27. Calculate molarity from mass and volume, and carry out dilution calculations.
28. Carry out solution stoichiometry calculations.
29. Classify strong and weak acids and bases.
30. Write complete and net ionic equations; Write neutralization equations.
31. Carry out calculations involving heat of reaction.
32. Distinguish between exothermic and endothermic.
33. Define electrolyte.
34. Apply periodic trends to atomic radius, ionization energy, and electronegativity.
35. Outline unique properties of water.
36. Determine osmolarity.
37. Define Ka and pKa and relate to acid strength.
38. Define Arrhenius and Bronsted-Lowry acids and bases.
39. Calculate [H3O+] and [OH-] given appropriate information.
40. Calculate pH or pOH of a solution.
41. Identify buffer solutions and describe how buffers work.
42. Identify factors that effect rates of reaction.
43. Define activation energy and catalyst.
44. Write equilibrium expression and determine K.
45.-Use LeChatelier’s Principle.
46. Write a nuclear reaction and deduce a product or reactant.