General Chemistry I (CHEM 1201) - Course Syllabus and Study Guide

General Chemistry I (CHEM 1201) - Syllabus Overview

Course Information

• Instructor: Dr. Sarah Harris

• Time and Location: MWF 10:00 AM – 10:50 AM, WESTERMAN HALL 001

• Credits: 3

• Co-requisite: CHEM 1201L (General Chemistry I Lab)

• Textbook (Required): MasteringChemistry with Pearson eText for Chemistry: The Central Science (15th ed.)

• Optional Textbook: Chemistry: The Central Science (15th ed.), Brown, LeMay, et al.

• Canvas Course Site: Students registered in this course must use the CHEM 1200-B Canvas site.

General Education Requirements

This course fulfills the Foundation Understanding the Natural World, and the Skills and Perspectives Scientific Method.

Assessment of Foundations, Skills & Perspectives

• Natural World (Learning Goal): Apply contemporary scientific models to describe the natural world, with assessment through performance in chemistry-related questions.

• Scientific Method: Students must demonstrate the ability to understand and apply the techniques of scientific inquiry, including observation, hypothesis testing, and data analysis.

Course Content and Structure

Course Topics (in order presented)

• Introduction: Matter, Energy, and Measurement (Chapter 1)

• Atoms, Molecules, and Ions (Chapter 2)

• Chemical Reactions and Reaction Stoichiometry (Chapter 3)

• Reactions in Aqueous Solution (Chapter 4)

• Thermochemistry (Chapter 5)

• Gases (Chapter 10)

• Electronic Structure of Atoms (Chapter 6)

• Periodic Properties of the Elements (Chapter 7)

• Basic Concepts of Chemical Bonding (Chapter 8)

• Molecular Geometry and Bonding Theories (Chapter 9)

• Liquids and Intermolecular Forces (Chapter 11)

Learning Goals

The fundamental aims or goals for this course are to be exposed to chemical and physical properties of the world we live in, chemical techniques used to apply these concepts, and scientific methods as they reveal them often in the public.

Objectives

• Classify the different states of matter

• Report measurements and sources of error and uncertainty

• Describe structure and bonding of atoms and ions

• Interpret atomic structure using quantum numbers and the periodic table

• Write and balance chemical equations

• Determine amounts in chemical formulas and reactions

• Complete calculations with accurate balancing, stoichiometry, and phasing

• Evaluate thermochemistry through enthalpy calculations

• Describe the kinetic molecular theory and use it to distinguish between real and ideal gas law models

Course Methods and Assessment

Teaching Methods

• Lectures, videos, demonstrations, discussion, practice problems, and group work

• Weekly reading and video assignments

• In-class and online homework and quizzes

• Three midterm exams and a cumulative final exam

Grading Breakdown

Component	Points
Homework	350
Quizzes	100
Midterms	300 (3 × 100)
Final Exam	250
Total	1000 points

Grading Scale:

• A ≥ 950 pts

• A- ≥ 900 pts

• B+ ≥ 860 pts

• B ≥ 800 pts

• B- ≥ 760 pts

• C+ ≥ 730 pts

• C ≥ 700 pts

• D ≥ 600 pts

Homework and Assignments

• Assigned on MasteringChemistry (online platform)

• Due at the end of the week, must be completed individually

• Practice problems and end-of-chapter exercises are recommended for additional study

Quizzes and Exams

• Quizzes: 5 scheduled, lowest score dropped

• Midterms: 3 scheduled during class

• Final Exam: Cumulative, scheduled for Dec 12, 2025, 3:30 pm – 5:20 pm

• No calculators allowed unless specified

Policies

• Attendance is expected; participation is your responsibility

• Missed exams require documentation and may be excused for valid reasons

• Late homework is penalized unless excused

• Academic honesty is required; plagiarism or cheating will result in disciplinary action

Key Concepts and Skills to Master

States of Matter and Measurement

• Matter: Anything that has mass and occupies space. Classified as solid, liquid, or gas.

• Measurement: Quantitative description of properties such as mass, volume, and temperature. SI units are standard.

• Uncertainty: All measurements have some degree of uncertainty, often reported as significant figures.

Atomic Structure and Periodicity

• Atoms: The basic unit of matter, composed of protons, neutrons, and electrons.

• Atomic Number (Z): Number of protons in the nucleus.

• Mass Number (A): Total number of protons and neutrons.

• Isotopes: Atoms of the same element with different numbers of neutrons.

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

• Quantum Numbers: Describe the energy, shape, and orientation of atomic orbitals.

Chemical Bonding and Molecular Structure

• Ionic Bonds: Formed by transfer of electrons from metals to nonmetals.

• Covalent Bonds: Formed by sharing of electrons between nonmetals.

• Lewis Structures: Diagrams showing bonding between atoms and lone pairs of electrons.

• VSEPR Theory: Predicts molecular geometry based on electron pair repulsion.

• Hybridization: Mixing of atomic orbitals to form new hybrid orbitals for bonding.

Chemical Reactions and Stoichiometry

• Chemical Equation: Represents a chemical reaction using symbols and formulas.

• Balancing Equations: Ensures the same number of atoms of each element on both sides.

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

• Mole Concept: 1 mole = $6.022 \times 10^{23}$ particles (Avogadro's number).

• Molar Mass: Mass of one mole of a substance, in grams per mole (g/mol).

Thermochemistry

• Energy: Capacity to do work or transfer heat.

• First Law of Thermodynamics: Energy cannot be created or destroyed, only transformed.

• Enthalpy ($\Delta H$): Heat content of a system at constant pressure.

• Calorimetry: Measurement of heat flow in a chemical reaction.

• Hess's Law: The total enthalpy change is the sum of enthalpy changes for individual steps.

Gases and Gas Laws

• Ideal Gas Law: $PV = nRT$

• Boyle's Law: $P_1V_1 = P_2V_2$ (at constant T and n)

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

• Avogadro's Law: $\frac{V_1}{n_1} = \frac{V_2}{n_2}$ (at constant P and T)

• Kinetic Molecular Theory: Explains the behavior of gases in terms of particle motion.

Intermolecular Forces

• Types: London dispersion forces, dipole-dipole interactions, hydrogen bonding.

• Effect: Influence boiling/melting points, solubility, and physical properties of substances.

Important Dates and Deadlines

Assessment	Date
Quiz #1	September 5, 2025
Midterm #1	September 24, 2025
Quiz #2	October 1, 2025
Quiz #3	October 10, 2025
Midterm #2	October 24, 2025
Quiz #4	October 29, 2025
Quiz #5	November 21, 2025
Midterm #3	December 1, 2025
Final Exam	December 12, 2025, 3:30 pm – 5:20 pm

Additional Info

• Students are expected to check Canvas regularly for updates and assignments.

• MasteringChemistry access is required for homework.

• Practice problems from the textbook are highly recommended for exam preparation.