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General Chemistry I for Majors (CHEM-1204) Syllabus and Study Guide

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Course Overview

Introduction to General Chemistry I

This course is the first part of a two-semester sequence designed for science and engineering majors. It covers fundamental laws, theories, and problem-solving skills in chemistry, including atomic and molecular structure, properties of matter, stoichiometry, chemical reactions, thermodynamics, and more. The course prepares students for advanced study in chemistry and related fields.

  • Course Code: CHEM-1204

  • Credits: 4

  • Format: Web-Enhanced

  • Instructor: Dr. Uttar Kumar Shrestha

Course Description

Scope and Content

The course provides a foundation in algebra-based chemistry, emphasizing the following topics:

  • Chemical reactions

  • Gases and kinetic-molecular theory

  • Nuclear chemistry

  • Quantum theory and atomic structure

  • Electron configuration and chemical periodicity

  • Stoichiometry

  • Valence bond theory and molecular orbital theory

  • Inorganic nomenclature

  • Thermochemistry

Students are expected to have completed introductory chemistry and appropriate mathematics prerequisites.

Objectives

General Education Objectives (GEO)

Upon completion, students will be able to:

  • Communicate effectively using oral, written, and electronic methods.

  • Demonstrate analytical and problem-solving skills in chemistry.

  • Apply scientific reasoning to laboratory and theoretical problems.

ACTS Course Objectives (ACO)

Students will explain, describe, and apply knowledge of:

  • Chemical reactions

  • Gases and kinetic-molecular theory

  • Nuclear chemistry

  • Quantum theory and atomic structure

  • Electron configuration and chemical periodicity

  • Stoichiometry

  • Valence bond theory and molecular orbital theory

  • Inorganic nomenclature

  • Thermochemistry

Course Learning Objectives (CLO)

  • Describe the classifications of matter and distinguish between chemical properties and physical properties.

  • Apply knowledge of stoichiometry to determine quantity of matter in moles and grams.

  • Identify the gas laws that govern physical and chemical behavior of gases.

  • Identify the first law of thermodynamics and calculate the heat absorbed or evolved during chemical change.

Required and Recommended Materials

Textbook

  • Tro's Chemistry: A Molecular Approach (Author: Nivaldo J. Tro, Edition: 6, Publisher: Pearson)

Additional Required Material

  • Scientific calculator (with common scientific functions)

  • Pencil (#2)

Recommended Material

  • Lab safety glasses (provided if needed)

Course Activities

Instructional Methods

Learning activities include lectures, video clips, exams, practice problems, in-class discussion, peer review/feedback, and lab work.

Self-Assessment Activities

  • Online homework assignments via Pearson Link

  • Assignments are due before each chapter exam

  • Students are responsible for reading instructions and submitting work on time

Assignment Schedule

Chapter #

Available

Due

1

08/20/2025, 6:00 AM

08/31/2025, 11:59 PM

2

08/28/2025, 6:00 AM

09/14/2025, 11:59 PM

3

09/09/2025, 6:00 AM

09/21/2025, 11:59 PM

4

09/16/2025, 6:00 AM

09/21/2025, 11:59 PM

5

09/22/2025, 6:00 AM

09/28/2025, 11:59 PM

6

09/26/2025, 6:00 AM

10/05/2025, 11:59 PM

7

10/02/2025, 6:00 AM

10/12/2025, 11:59 PM

8

10/13/2025, 6:00 AM

10/19/2025, 11:59 PM

9

10/18/2025, 6:00 AM

10/26/2025, 11:59 PM

10

10/28/2025, 6:00 AM

11/09/2025, 11:59 PM

11

11/10/2025, 6:00 AM

11/23/2025, 11:59 PM

21

11/02/2025, 6:00 AM

12/09/2025, 11:59 PM

Exams

  • Three exams (each 15% of grade)

  • Comprehensive final exam (20% of grade)

  • Strict exam policies: no cell phones, no early/late exams except for approved absences

Quizzes

  • 8 online quizzes via D2L (each 7% of total grade)

  • Each quiz: 10 questions, 30 minutes

  • Quizzes must be completed in one sitting

Lab Work

  • 10 lab experiments required

  • Lab reports must be submitted on time

  • Lab safety glasses required

  • Lab safety rules strictly enforced

  • If you fail the lab portion, you will automatically fail the course

Lab Safety

  • No open-toed shoes, sandals, or flip-flops

  • Long hair must be tied back

  • No loose-fitting clothing

  • Details discussed during first lab session

  • You MUST wear shoes that cover your entire foot

Grading Policy

Grade Breakdown

Activities

%

Exams (3 x 15%)

45%

Comprehensive Final

20%

Lab Reports (10 reports, lowest one dropped)

14%

Key Chemistry Concepts Covered

Chemical Reactions

Chemical reactions involve the transformation of substances through the breaking and forming of chemical bonds. Students will learn to balance chemical equations and predict products.

  • Example: Combustion of methane:

Stoichiometry

Stoichiometry is the quantitative study of reactants and products in chemical reactions. It involves calculations based on the mole concept and balanced equations.

  • Key Formula:

  • Example: Calculating the amount of product formed from a given amount of reactant.

Gas Laws

Gas laws describe the behavior of gases in terms of pressure, volume, temperature, and amount.

  • Key Formula: (Ideal Gas Law)

  • Example: Determining the volume of a gas at standard temperature and pressure.

Thermochemistry

Thermochemistry studies the energy changes that occur during chemical reactions, focusing on heat transfer and the first law of thermodynamics.

  • Key Formula:

  • First Law of Thermodynamics:

Atomic Structure and Quantum Theory

Atomic structure explores the arrangement of electrons, protons, and neutrons in atoms. Quantum theory explains the behavior of electrons in atoms using principles such as quantization of energy levels.

  • Key Concept: Electrons occupy discrete energy levels described by quantum numbers.

Periodic Table and Chemical Periodicity

The periodic table organizes elements by increasing atomic number and recurring chemical properties. Chemical periodicity refers to trends such as electronegativity, ionization energy, and atomic radius.

  • Example: Alkali metals are highly reactive due to their single valence electron.

Nomenclature

Nomenclature is the systematic naming of chemical compounds according to IUPAC rules.

  • Example: NaCl is named sodium chloride.

Bonding Theories

Valence bond theory and molecular orbital theory explain how atoms bond to form molecules, describing the sharing or transfer of electrons.

  • Key Concept: Covalent bonds involve sharing of electron pairs between atoms.

Nuclear Chemistry

Nuclear chemistry studies the changes in atomic nuclei, including radioactive decay and nuclear reactions.

  • Example: (beta decay)

Additional info:

  • Students are expected to follow all safety and academic honesty policies.

  • Lab work is essential and failure in lab results in failure of the course.

  • Reference for lab reports must be in ACS (American Chemical Society) style.

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