CHEM 1611 – General Chemistry I (Course Structure, Policies, and Study Guide)

Course Overview

Introduction to General Chemistry I

CHEM 1611 is a foundational college-level course in chemistry, designed to introduce students to the essential principles and concepts of chemical science. The course covers atomic structure, molecular composition, chemical reactions, stoichiometry, gas laws, thermodynamics, and kinetics, providing a basis for further study in chemistry and related STEM disciplines.

• Course Number: 161-01

• Credits: 3

• Lecture Days: Wednesday & Friday

• Lecture Time: 12:15 pm – 1:30 pm

• Instructor: Dr. Peyahandi Thilini De Silva

Required Materials

Textbook and Tools

• Textbook: OpenStax Chemistry, 2nd edition (freely downloadable PDF).

• Scientific Calculator: Standard, non-programmable, non-storage type.

• Electronic Device: For accessing PDFs and lecture notes.

Scope of the Course

Fundamental Concepts in Chemistry

This course introduces the basic principles of chemistry, including the structure of atoms and molecules, chemical reactions, solution preparation, stoichiometry, gas laws, and thermodynamics. Emphasis is placed on the application of chemistry in everyday life and other STEM fields.

• Atomic and molecular structure

• Chemical reactions and stoichiometry

• Gas laws and thermodynamics

• Kinetics and equilibrium

Student Learning Objectives

Key Outcomes

• Understand the structure of atoms and molecules.

• Learn solution preparation and stoichiometry.

• Apply gas laws and thermodynamics to chemical systems.

• Relate chemistry concepts to real-world applications.

Course Topics and Schedule

Weekly Breakdown

The following table outlines the topics covered each week, along with quiz and exam dates.

Date of Lecture	Topic	Quiz Due
08.27	Chapter 1: Essential Concepts	Quiz 1 (09.06)
08.29	Chapter 2: Atoms, Molecules, Ions	Quiz 2 (09.13)
09.04	3.1-3.4 (Quantum and electronic structure)	Quiz 3 (09.20)
09.11	3.5-4.2 (Periodic table, molecular & ionic compounds)	Quiz 4 (09.26)
09.17	4.3-4.6 (Dot structures, shapes, polarity)	Quiz 5 (10.03)
09.25	Unit Exam 1
10.02	5.4-6.0 (Theory), 6.1-6.2 (empirical & molecular formulas, molarity)	Quiz 6 (10.10)
10.09	7.1-7.3 (Reactions & Stoichiometry)	Quiz 7 (10.17)
10.16	7.4-7.5 (Stoichiometry & yields)	Quiz 8 (10.24)
10.23	Unit Exam 2
10.30	Chapter 8: Gas Laws	Quiz 9 (11.07)
11.06	Chapter 10: Thermochemistry	Quiz 10 (11.14)
11.12	Chapter 12: Thermodynamics	Quiz 11 (11.21)
11.19	Ch. 13 Equilibrium	Quiz 13 (11.28)
11.26	No Class
12.03	Chapter 17: Basic Kinetics	Quiz 14 (12.12)
12.05	Final Exam (cumulative)	10.30 AM - 12.30 PM

Grading Policy

Grade Components and Scale

Grades are determined by online quizzes, unit exams, and a final exam. The breakdown is as follows:

Component	Percentage
Online Quizzes (12)	4% each × 12 = 48%
Unit Exams (In Class), 3	12% each × 3 = 36%
Final Exam (In Class)	16%
Total	100%

Percentage Range	Letter Grade	Percentage Range	Letter Grade
90-100%	A	70-74%	C-
87-89%	A-	65-69%	D+
84-86%	B+	60-64%	D
80-83%	B	55-59%	D-
77-79%	B-	Below 55%	F
74-76%	C+

Course Policies

Attendance and Conduct

• Students must attend and be on time for all scheduled classes.

• Active participation and asking questions are strongly encouraged.

• Chronic absences or tardiness will not be tolerated.

• Traffic is not an acceptable excuse for lateness.

Assignments and Exams

• Quizzes and assignments must be submitted through Blackboard.

• No extensions or make-up quizzes will be granted under any circumstances.

• If a class is cancelled on the day of an exam, it will be rescheduled for the next class meeting.

• Missed exams require written documentation to be considered for a make-up.

• If multiple exams are missed, the final exam grade may be used to replace the missed exam(s).

Key Chemistry Concepts (by Chapter)

Chapter 1: Essential Concepts

• Matter: Anything that has mass and occupies space.

• Elements and Compounds: Elements are pure substances consisting of one type of atom; compounds are substances composed of two or more elements chemically combined.

• Mixtures: Physical combinations of substances that can be separated by physical means.

• States of Matter: Solid, liquid, gas.

Chapter 2: Atoms, Molecules, Ions

• Atom: The smallest unit of an element, consisting of protons, neutrons, and electrons.

• Molecule: Two or more atoms bonded together.

• Ion: An atom or molecule with a net electric charge due to loss or gain of electrons.

• Example: $\text{Na}^+$, $\text{Cl}^-$, $\text{H}_2\text{O}$

Chapter 3: Quantum and Electronic Structure

• Quantum Theory: Describes the behavior of electrons in atoms.

• Electron Configuration: The arrangement of electrons in an atom.

• Example Equation: $n = 1, 2, 3, ...$ (principal quantum number)

Chapter 4: Periodic Table, Molecular & Ionic Compounds

• Periodic Table: Organizes elements by increasing atomic number and recurring chemical properties.

• Molecular Compounds: Composed of molecules formed by nonmetals.

• Ionic Compounds: Composed of positive and negative ions.

Chapter 5-6: Chemical Bonding and Solution Preparation

• Dot Structures: Lewis structures representing valence electrons.

• Polarity: Distribution of electrical charge over atoms in a molecule.

• Molarity Equation: $M = \frac{\text{moles of solute}}{\text{liters of solution}}$

Chapter 7: Chemical Reactions & Stoichiometry

• Stoichiometry: Calculation of reactants and products in chemical reactions.

• Yield: The amount of product formed in a reaction.

• Example Equation: $\text{C}_6\text{H}_{12}\text{O}_6 + 6\text{O}_2 \rightarrow 6\text{CO}_2 + 6\text{H}_2\text{O}$

Chapter 8: Gas Laws

• Ideal Gas Law: $PV = nRT$

• Boyle's Law: $P_1V_1 = P_2V_2$ (at constant temperature)

• Charles's Law: $\frac{V_1}{T_1} = \frac{V_2}{T_2}$ (at constant pressure)

Chapter 10-12: Thermochemistry & Thermodynamics

• Thermochemistry: Study of energy changes in chemical reactions.

• First Law of Thermodynamics: $\Delta E = q + w$ (change in internal energy equals heat plus work)

• Enthalpy: $\Delta H = \Delta E + P\Delta V$

Chapter 13: Equilibrium

• Chemical Equilibrium: State where forward and reverse reactions occur at equal rates.

• Equilibrium Constant: $K = \frac{[\text{products}]}{[\text{reactants}]}$

Chapter 17: Basic Kinetics

• Kinetics: Study of reaction rates and mechanisms.

• Rate Law Example: $\text{Rate} = k[\text{A}]^m[\text{B}]^n$

Additional University Policies

Academic Integrity and Conduct

• Students must adhere to the CCSU Code of Academic Integrity.

• Plagiarism and cheating are strictly prohibited.

Equity, Inclusion, and Accommodations

• CSCU is committed to providing an inclusive and equitable learning environment.

• Accommodations are available for students with documented disabilities.

• Contact the Office of Equity and Inclusion or Student Disability Services for support.

Student Wellness

• Resources are available for student health and wellness.

Additional info: This guide summarizes the course structure, policies, and key chemistry concepts for CHEM 1611. For detailed content, refer to the OpenStax Chemistry textbook and weekly lecture materials.