General Chemistry I (A): Syllabus, Course Structure, and Key Topics

Study Guide - Smart Notes

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

Course Overview

Introduction to General Chemistry I

This course is a multi-section lecture and discussion sequence in general chemistry, designed for college students. It covers foundational chemical principles, problem-solving skills, and scientific reasoning, preparing students for further study in chemistry and related disciplines.

Course Code: Chemistry 101
Credits: 3 (Lecture & Discussion)
Prerequisites: Satisfactory performance on the Loyola math placement test, completion of Math 117 with a grade of C- or better, or equivalent. A student missing a prerequisite may be withdrawn at any time.
Class Times: Multiple sections; refer to schedule for specific times and locations.

Course Materials

Required and Optional Resources

Textbook: Chemistry: The Central Science, Brown LeMay, et al., 14th edition or earlier.
Online Resources: Sakai (course management), Model Kit, Brown LeMay Textbook Solutions Manual.
Scientific Calculator: Non-programmable, non-graphing, e.g., TI-30X.
Additional Packet: Available at Cognella.

Course Policies

Intellectual Property and Cell Phone Policy

Copyright: Course materials may not be shared outside the course without instructor's written permission.
Cell Phone Policy: Recording of lectures is forbidden. Use of electronic devices during exams or lectures is strictly prohibited.

Course Learning Outcomes

Skills and Knowledge Developed

Students will build a conceptual understanding of chemical principles, develop scientific reasoning, and apply mathematical skills to chemistry problems. The course emphasizes the following outcomes:

Differentiation of Matter: Distinguish types of matter based on chemical and physical properties (e.g., volume, reactivity, states such as liquids, metals vs. nonmetals, ionic vs. covalent).
Multiple Perspectives: Describe aspects of matter at macroscopic, particle, and symbolic levels.
Quantitative Relationships: Use chemical characteristics, periodicity, molecular structure, chemical bonding, chemical reactions, and stoichiometry to solve problems.
Solving Quantitative Problems: Combine multiple concepts within chemical systems.
Application: Apply chemical topics to explain natural phenomena and categorize problem types.

Course Schedule and Topics

Weekly Breakdown of Topics

The following table outlines the major topics, chapters, and approximate pages covered each week. This schedule provides a roadmap for the semester, including exam dates and breaks.

Week / Day	Topic	Chapter	Approx. Pages
8/29 – 9/2	Intro, Measurements, Reporting Accuracy, Periodic Table Overview, Atomic Model	1	2–24
9/5	LABOR DAY (No class)	-	-
9/7 – 9/9	Molecular Representation, Molecular Formula, Empirical Formula, Stoichiometry, Composition, Limiting Reactant, Theoretical vs. Actual Yield	2	25–49
9/12 – 9/16	Aqueous Reactions, Net Ionic Reactions, Precipitation Activity, Acid/Base Review	4	122–126, 126–128
9/26	EXAM 1	-	-
9/28 – 10/3	Redox Reactions, Molarity, Concentration, Titration	4	137–146, 146–150
10/10 – 10/14	Stoichiometric Analysis, Enthalpy, Calorimetry, Hess’s Law	5	151–164, 164–172
10/24	EXAM 2	-	-
10/26 – 10/31	Light & Matter, Hydrogen Atom Model	6	185–192
11/2 – 11/7	Periodic Table, Electron Configuration, Principles & Trends	7	218–234
11/14	EXAM 3	5–9	-
11/23	Bond Order, Resonance, Hybridization, Polarity	8	262–276
12/15	COMMON FINAL	1–10	-

Additional info: Some topics and chapters inferred from context and standard chemistry curricula.

Key Concepts and Definitions

Fundamental Chemistry Terms

Atom: The smallest unit of an element, consisting of protons, neutrons, and electrons.
Molecule: A group of atoms bonded together, representing the smallest fundamental unit of a chemical compound.
Stoichiometry: The calculation of reactants and products in chemical reactions.
Empirical Formula: The simplest whole-number ratio of atoms in a compound.
Limiting Reactant: The reactant that is completely consumed in a reaction, limiting the amount of product formed.
Periodic Table: A tabular arrangement of elements by increasing atomic number, showing recurring chemical properties.
Electron Configuration: The distribution of electrons in an atom's orbitals.
Bond Order: The number of chemical bonds between a pair of atoms.
Hybridization: The concept of mixing atomic orbitals to form new hybrid orbitals suitable for bonding.

Important Equations and Formulas

Chemistry Equations

Empirical Formula Calculation:
Molarity:
Ideal Gas Law:
Enthalpy Change (Hess's Law):

Course Support and Communication

Instructor and Supplemental Instruction

Section Instructor: Dr. William Greene Johnson, Ph.D. (wgene@luc.edu)
Office Hours: Cudahy Science Hall, Room 322; Wednesday 2:00–3:30 PM or by appointment.
Supplemental Instructor (SI): Jacqui Wittman (jwittman@luc.edu)

Additional Policies

Accommodations and Academic Integrity

Accommodations: Provided for students with documented disabilities or religious observances.
Academic Integrity: Students are expected to adhere to university policies regarding honesty and conduct.

Summary Table: Major Chemistry Topics

Topic	Description	Example/Application
Atomic Structure	Composition and arrangement of subatomic particles in atoms	Electron configuration of Na (Sodium): 1s2 2s2 2p6 3s1
Stoichiometry	Quantitative relationships in chemical reactions	Calculating the limiting reactant in a reaction between H2 and O2
Bonding & Molecular Structure	Types of chemical bonds and molecular geometry	Predicting the shape of H2O using VSEPR theory
Thermochemistry	Energy changes in chemical reactions	Using calorimetry to determine enthalpy change
Periodic Trends	Patterns in element properties across the periodic table	Comparing ionization energies of Li, Na, and K

Additional info: Table entries inferred from standard general chemistry curriculum.