General Chemistry I (CHM 109) – Syllabus and Study Guide

Study Guide - Smart Notes

Tailored notes based on your materials, expanded with key definitions, examples, and context.

Course Overview

This course provides a foundational introduction to chemistry for science majors. It covers essential topics such as atomic structure, chemical bonding, stoichiometry, phases of matter, chemical energetics, molecular geometry, and introductory laboratory techniques. The course is designed to help students develop a conceptual understanding of chemistry and its applications in the real world.

Course Structure and Logistics

Course Title: General Chemistry I (CHM 109)
Schedule: MWF 9:00 – 9:50 AM
Location: 001 St. Albert Hall
Semester: Fall, 2025
Prerequisites: High school chemistry, placement in college-level math

Course Description

This course introduces the basic principles of chemistry, including the structure of atoms and molecules, chemical bonding, stoichiometry, states of matter, and the energetics of chemical reactions. Emphasis is placed on developing problem-solving skills and understanding the scientific method as applied to chemical phenomena.

Instructional Objectives

Knowledge:
- Understand and use the vocabulary of chemistry and chemical measurement.
- Comprehend the fundamental concepts of atomic structure, periodic trends, chemical bonding, molecular structure, and chemical reactions.
- Classify and compare the states of matter and their properties.
- Apply mathematical and conceptual skills to solve problems in stoichiometry, thermodynamics, and chemical reactivity.
Skills:
- Apply concepts in laboratory experiments and analyze data.
- Develop proficiency in the safe and proper use of laboratory equipment and techniques.
- Interpret and analyze data from experiments and draw logical conclusions.
Dispositions:
- Develop a scientific approach to problem-solving and critical thinking.
- Appreciate the relevance of chemistry in everyday life and other scientific disciplines.

Grading Policy

Your final grade will be determined by a combination of exams, quizzes, laboratory work, and participation. The grading scale and breakdown are as follows:

Percent	Letter Grade
93–100	A
90–92	A-
87–89	B+
83–86	B
80–82	B-
77–79	C+
73–76	C
70–72	C-
67–69	D+
60–66	D
<60	F

To continue to CHM 110, you must pass CHM 109 with a grade of C or better.

Grade Components

Item	Points	Percent of Final Grade
In-class Exams	600	37.5%
Final Exam	300	18.75%
Checkpoints	300	18.75%
Laboratory	400	25%
Active Learning/Asix	100	6.25%
Total	1600	100%

Major Topics Covered (Tentative Schedule)

Introduction to Chemistry & Lab Safety
Measurement and Units
Atomic Structure
Electronic Structure of Atoms
Periodic Table and Periodicity
Chemical Bonding (Ionic and Covalent)
Molecular Geometry and Polarity
Stoichiometry
Chemical Reactions and Equations
Thermochemistry
States of Matter (Gases, Liquids, Solids)
Solutions and Concentrations
Acids and Bases (Introductory)
Laboratory Techniques and Data Analysis

Key Definitions and Concepts

Atom: The smallest unit of an element that retains the properties of that element.
Molecule: Two or more atoms chemically bonded together.
Stoichiometry: The calculation of reactants and products in chemical reactions.
Periodic Table: A tabular arrangement of elements by increasing atomic number, showing periodic trends.
Chemical Bond: The force holding atoms together in molecules or compounds; includes ionic, covalent, and metallic bonds.
Thermochemistry: The study of energy changes during chemical reactions.
Solution: A homogeneous mixture of two or more substances.

Important Formulas and Equations

Ideal Gas Law:
Density:
Mole Concept:
Percent Composition:
Energy Change (q):

Laboratory Component

Weekly laboratory sessions reinforce lecture concepts through hands-on experiments.
Students must maintain a laboratory notebook and follow all safety protocols.
Lab work is a significant portion of the final grade (25%).

Required Materials

Textbook: OpenStax Chemistry (free online resource)
Online Homework: Asix Chemistry (registration required)
Scientific Calculator: Capable of exponents, roots, logarithms, and trigonometric functions
Laboratory Notebook: With duplicate pages
Portable Device: For in-class activities and online assignments

Attendance and Policies

Regular attendance is strongly correlated with success in the course.
Late assignments may incur penalties unless due to documented emergencies.
Academic integrity and university policies must be followed at all times.
Accommodations are available for students with documented disabilities.

Example Application

Example: Calculating the number of moles in 18 grams of water (H2O):

Molar mass of H2O = 2(1.01) + 16.00 = 18.02 g/mol
Number of moles =

Additional Info:

This guide is based on the course syllabus and is intended to provide a structured overview for exam preparation and ongoing study.
For detailed explanations of each topic, refer to the assigned textbook and lecture materials.