General Chemistry I Syllabus and Study Guide

Course Overview

Introduction to General Chemistry I

This course provides a foundational understanding of chemistry, focusing on the principles and concepts essential for further study in science and health-related fields. Topics include stoichiometry, atomic structure, chemical bonding, molecular geometry, thermodynamics, kinetics, equilibrium, acids and bases, and nuclear chemistry. The course combines lectures and laboratory work to reinforce theoretical knowledge with practical skills.

Course Structure and Policies

Course Materials

• Textbook: Free electronic/online textbook available via provided links.

• Online Homework System: Required for assignments and practice exams.

• Calculator: Simple scientific calculator (TI-83 or higher not allowed on exams).

• Lab Supplies: Must be purchased from the college bookstore.

Methods of Evaluation

• Three Unit Exams: 40% of final grade

• Final Exam (cumulative): 25% of final grade

• Homework: 10% of final grade

• Lab Experiments: Top 10 highest lab scores count for 25% of final grade

Grading System

Letter Grade	Percentage Range
A	90–100%
B+	87–89%
B	80–86%
C+	77–79%
C	70–76%
D	60–69%
F	Below 60%

Attendance and Participation

• Attendance is required for both lectures and labs.

• Lab grade must be at least 64% to pass the course.

• Students must check Canvas for grades, assignments, and announcements.

Makeup Policy

• One exam makeup per semester allowed for legitimate reasons (documentation required).

• No makeups for homework; late work not accepted.

• Lab makeups only for documented emergencies.

Major Topics Covered

Matter and Measurements

Students will learn about the classification of matter, physical and chemical properties, and measurement techniques. Quantitative problem-solving is emphasized.

• Matter: Anything that has mass and occupies space.

• Measurements: Use of SI units, significant figures, and dimensional analysis.

• Example: Calculating density using $\text{Density} = \frac{\text{Mass}}{\text{Volume}}$.

Elements, Atoms, and Atomic Structure

Explores the structure of atoms, elements, and the laws governing chemical combination. Students will write electron configurations and understand atomic theory.

• Atom: The smallest unit of an element retaining its chemical properties.

• Electron Configuration: Arrangement of electrons in an atom, e.g., $1s^2 2s^2 2p^6$ for neon.

• Example: Determining the number of protons, neutrons, and electrons in an isotope.

Stoichiometry and Chemical Equations

Focuses on balancing chemical equations, using stoichiometric relationships to solve quantitative problems, and understanding mole concepts.

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

• Mole Concept: $1 \text{mol} = 6.022 \times 10^{23}$ particles.

• Example: Balancing $2H_2 + O_2 \rightarrow 2H_2O$ and calculating mass of water produced.

Chemical Bonding and Molecular Geometry

Students will learn about covalent and ionic bonds, Lewis structures, and the shapes of molecules using VSEPR theory.

• Covalent Bond: Sharing of electron pairs between atoms.

• Ionic Bond: Transfer of electrons from one atom to another.

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

• Example: Drawing the Lewis structure for $CO_2$ and predicting its linear geometry.

Thermochemistry and Kinetics

Introduces energy changes in chemical reactions and the factors affecting reaction rates.

• Thermochemistry: Study of heat changes in chemical reactions.

• Kinetics: Study of reaction rates and mechanisms.

• Example: Calculating enthalpy change using $\Delta H = \sum \Delta H_{\text{products}} - \sum \Delta H_{\text{reactants}}$.

Equilibrium, Acids and Bases, and Nuclear Chemistry

Examines chemical equilibrium, acid-base reactions, and the basics of nuclear chemistry.

• Chemical Equilibrium: State where forward and reverse reaction rates are equal.

• Acids and Bases: Definitions, pH calculations, and titration concepts.

• Nuclear Chemistry: Radioactive decay and nuclear reactions.

• Example: Calculating $K_{eq}$ for a reaction and determining pH from $[H^+]$.

Laboratory Component

Lab Techniques and Safety

Laboratory work reinforces lecture topics and teaches essential techniques such as measurement, solution preparation, and data analysis. Safety is emphasized at all times.

• Lab Reports: Must be completed individually; collaboration is not permitted.

• Lab Safety: Proper attire and adherence to safety protocols required.

• Example: Using a pipet to measure liquid volume accurately.

Academic Integrity and Success Tips

Academic Integrity

• Cheating, plagiarism, and unauthorized collaboration are strictly prohibited.

• Violations will be reported and may result in disciplinary action.

How to Succeed

• Spend at least two to three hours per week on assignments outside of class.

• Follow the weekly schedule and stay on top of assignments.

• Check Canvas and announcements regularly.

Learning Outcomes

• Balance and solve chemical equations using stoichiometric relationships.

• Write electron configurations for ground state atoms.

• Demonstrate understanding of atomic and molecular properties.

• Draw Lewis structures and determine geometry of compounds.

• Write IUPAC names for compounds and structures.

• Evaluate types of intermolecular forces in covalent and ionic substances.

Withdrawal and Refund Schedule

Date	Refund/Withdrawal Policy
September 10	100% refund
September 16	50% refund without course record
September 24	No refund, withdrawal without record
November 24	Change to Audit with Instructor Approval
After November 24	No withdrawals

Additional info: These notes are based on the syllabus for General Chemistry I and cover the main topics, policies, and expectations for students enrolled in the course. For detailed content on each chapter, refer to the course textbook and lecture materials.