General Chemistry I (CHEM 1113) Syllabus and Study Guide

Course Overview

Introduction to General Chemistry I (CHEM 1113)

This course provides a foundational introduction to the principles of chemistry, including atomic and molecular structure, chemical reactions, stoichiometry, and the properties of matter. It is designed for students pursuing science and health-related majors and fulfills a core science requirement.

• Course Title: CHEM 1113.02, General Chemistry I Lecture

• Instructor: Dr. John Beatty

• Class Meeting Times: Monday and Wednesday, 9:30 am to 10:50 am

• Location: CFO 204

• Prerequisites: One year of high school chemistry and a passing score on a placement exam or a grade of C or better in CHEM 1013.

Course Description and Objectives

Course Description

Chemistry 1113 covers the basic chemical principles and introduces students to the scientific method, atomic theory, chemical bonding, stoichiometry, and chemical reactions. The course includes both lecture and laboratory components (lab is a separate course).

Course Objectives

• Understand the nature of substances and how properties vary with type and amount of solute and solvent.

• Learn the fundamental steps that determine the rates of chemical reactions.

• Apply the laws of conservation of mass and energy to chemical processes.

• Understand the behavior of acids and bases in solution.

Textbook and Materials

Required Textbook

• General Chemistry (2nd edition) by Sue Bohns (available as an online homework system called OWL).

• Scientific calculator (non-graphing, non-programmable).

Other Required Materials

• Notebook for notes and homework.

• Access to Canvas for course documents and assignments.

Major Topics Covered

Key Topics and Skills

Students will develop proficiency in the following areas:

• Atomic structure and periodic trends

• Chemical bonding and molecular geometry

• Stoichiometry and chemical equations

• States of matter and intermolecular forces

• Thermochemistry and energy changes in reactions

• Acids, bases, and solution chemistry

• Redox reactions and oxidation numbers

• Gas laws and properties of gases

Representative Skills and Learning Outcomes

• State the law of conservation of mass

• Use significant figures in calculations

• Convert between temperature units

• Balance chemical equations

• Write chemical formulas and names

• Calculate percent composition from formulas

• Determine empirical and molecular formulas

• Calculate limiting reactants and percent yield

• Assign oxidation numbers

• Use molarity in concentration calculations

• Apply gas laws to solve for pressure, volume, or temperature

• Calculate heat changes using calorimetry

• Write net ionic equations for reactions in water

• Apply intermolecular force concepts

• Relate energy changes to phase transitions

Grading and Assessment

Course Grade Components

Component	Percentage
Online Homework	15%
Quizzes	10%
Three Exams	45%
Final Exam	30%

Grading Scale

Grade	Percentage
A	89.5 – 100%
B	79.5 – 89.4%
C	69.5 – 79.4%
D	59.5 – 69.4%
F	< 59.5%

Course Policies and Expectations

Attendance and Participation

• Regular attendance and active participation are required.

• Students are expected to arrive on time and be prepared for class.

• Class discussions and group activities are integral to learning.

Homework and Quizzes

• Homework assignments are completed online via the OWL system.

• Quizzes are given throughout the semester; the lowest quiz grade will be dropped.

Exams

• Three in-class exams and one comprehensive final exam.

• Make-up exams are only given with documented, valid excuses.

Scientific Method and Inquiry

Nature of Science in Chemistry

Chemistry is a science that relies on observation, experimentation, and the scientific method to understand the natural world. Students will learn to:

• Formulate and test hypotheses

• Analyze and interpret data

• Communicate scientific findings effectively

Important Equations and Concepts

Representative Equations

• Law of Conservation of Mass: $\text{Total mass of reactants} = \text{Total mass of products}$

• Ideal Gas Law: $PV = nRT$

• Molarity: $M = \frac{\text{moles of solute}}{\text{liters of solution}}$

• Percent Yield: $\text{Percent Yield} = \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \times 100\%$

• Energy Change (q): $q = m c \Delta T$

Academic Integrity and University Policies

Academic Integrity

• All assignments must be completed honestly and independently.

• Cheating, plagiarism, and other forms of academic dishonesty are strictly prohibited.

Accessibility and Support

• Students with disabilities should contact the university’s Office of Disability Services for accommodations.

• Support services are available for students experiencing academic or personal difficulties.

Additional Info

• Course includes safety training for laboratory work (if enrolled in lab).

• Canvas is used for course documents, grades, and communication.

• Students are encouraged to participate in class discussions and group activities.