Introductory Chemistry I (CHM 101) - Syllabus and Course Structure Study Guide

Course Overview

This study guide summarizes the structure, objectives, and assessment methods for the Introductory Chemistry I (CHM 101) course at Northern Virginia Community College, Manassas Campus. The course is designed for non-science majors and covers foundational concepts in general, inorganic, organic, and biological chemistry, with an emphasis on both theoretical and experimental aspects.

Course Description and Purpose

• Course Title: Hybrid CHM-101 (4 credits)

• Format: Hybrid (in-person lectures and online assignments)

• Purpose: To provide a general background in chemistry, preparing students for further study or to fulfill general education requirements.

• Target Audience: Non-science majors and students needing a chemistry foundation.

Course Objectives

Upon successful completion of this course, students should be able to:

• Define and apply basic chemistry terminology.

• Balance simple chemical equations.

• Apply principles of the scientific method and measurement.

• Use chemical symbols, formulas, and nomenclature correctly.

• Perform simple stoichiometric calculations.

• Explain atomic structure and predict periodic trends.

• Solve basic gas law problems.

• Determine bonding types, molecular shapes, and polarity.

• Calculate solution concentration and pH.

• Relate concentration and temperature to reaction rates.

• Discuss the effects of air and water pollution on the environment.

Course Structure and Schedule

The course is organized by chapters, each focusing on a core topic in introductory chemistry. The schedule includes in-person meetings, online readings, video quizzes, homework, and exams. Students are expected to engage in both individual and group assignments.

Sample Weekly Structure

• In-Class Activities: Lectures, discussions, and group work.

• Online Assignments: Chapter readings, video quizzes, homework, and discussion board participation.

• Assessment: Online quizzes, exams, research project, and laboratory work.

Assessment and Grading

Student performance is evaluated through a combination of attendance, homework, quizzes, exams, laboratory reports, and a research project. The grading breakdown is as follows:

Assessment	Percentage
Attendance	1%
Homework & Discussion Board	6%
Pre-lecture Assignments (Video Quizzes)	3%
Online Quizzes	15%
Exams	25%
Comprehensive Final Exam	20%
Research Project	5%
Lab	25%

Grading Scale:

Grade	Percentage Range
A	90.0–100.0
B	80.0–89.9
C	70.0–79.9
D	60.0–69.9
F	59.9 and below

Course Topics by Chapter

• Chapter 1: The Chemical World

• Chapter 2: Measurement and Problem Solving

• Chapter 3: Matter and Energy

• Chapter 4: Atoms and Elements

• Chapter 5: Molecules and Compounds

• Chapter 6: Chemical Composition

• Chapter 7: Chemical Reactions

• Chapter 8: Quantities in Chemical Reactions

• Chapter 9: Electrons in Atoms and the Periodic Table

• Chapter 10: Chemical Bonding

• Chapter 11: Gases

Additional topics include solutions, acids and bases, chemical equilibrium, oxidation and reduction, and radioactivity, as indicated by the comprehensive final exam covering all chapters.

Course Policies and Expectations

• Attendance: Mandatory for in-person sessions; excessive absences may result in course failure.

• Participation: Active participation in discussions and group work is required.

• Assignments: Must be submitted on time; late work incurs penalties.

• Technology: Students must have access to a computer with internet, webcam, and basic office software.

• Exams: No make-up exams; final exam is comprehensive and mandatory.

Study and Success Tips

• Read textbook chapters and review PowerPoints before class meetings.

• Complete all practice problems and assignments on Canvas.

• Participate actively in group discussions and online forums.

• Prepare for quizzes and exams by reviewing key concepts and practicing calculations.

• Contact the instructor for clarification or help as needed.

Key Definitions and Concepts

• Stoichiometry: The calculation of reactants and products in chemical reactions.

• Atomic Structure: The arrangement of protons, neutrons, and electrons in an atom.

• Chemical Bonding: The interactions that hold atoms together in compounds (ionic, covalent, metallic bonds).

• Gas Laws: Mathematical relationships describing the behavior of gases (e.g., Boyle's Law, Charles's Law).

• Solution Concentration: The amount of solute dissolved in a given quantity of solvent, often expressed as molarity ($M = \frac{\text{moles of solute}}{\text{liters of solution}}$).

• pH: A measure of the acidity or basicity of a solution ($pH = -\log_{10}[H^+]$).

Example: Balancing a Chemical Equation

To balance the reaction of hydrogen and oxygen forming water:

$2H_2 + O_2 \rightarrow 2H_2O$

This equation shows that two molecules of hydrogen gas react with one molecule of oxygen gas to produce two molecules of water.

Example: Calculating Molarity

If 0.5 moles of NaCl are dissolved in 1.0 L of water, the molarity is:

$M = \frac{0.5\ \text{mol}}{1.0\ \text{L}} = 0.5\ M$

Additional Info

• Students are encouraged to use the Canvas platform regularly for updates and assignment submissions.

• Laboratory sessions are an integral part of the course and contribute significantly to the final grade.