CHEM-105 Principles of General Chemistry I: Syllabus and Study Guide

Course Overview

Introduction to General Chemistry I

General Chemistry I is the first semester course designed for students majoring in chemistry, life sciences, and related fields. It covers foundational chemical principles, laboratory skills, and problem-solving techniques essential for further study in chemistry and related disciplines.

• Credits: 4 (includes three hours lecture, three hours laboratory per week)

• Prerequisites: Completion of high school chemistry and MATH-099, or consent of department chair

• Textbook: Chemistry: The Central Science by Brown, LeMay, Bursten (15th Edition)

• Online Access: Mastering Chemistry platform

• Lab Manual: CHEM-105 LAB MANUAL (July 2023)

• Calculator: Non-programmable, non-graphing scientific calculator

Course Objectives

Learning Outcomes

Upon successful completion, students will be able to:

1. Solve scientific problems using the metric system and proper mathematical methods, with non-programmable calculators.

2. Describe the nature of matter and atomic theory and its relevance to chemical phenomena.

3. Apply nomenclature and formulas in writing balanced chemical equations and solving stoichiometric problems.

4. Analyze chemical reactions both qualitatively and quantitatively, including thermochemistry.

5. Explain physical laws governing chemical behavior and apply them to problem-solving.

6. Interpret periodic trends and electron configuration of elements.

7. Predict and formulate bonding in atoms and molecular geometry of compounds.

8. Perform laboratory experiments to reinforce concepts and develop technical skills.

9. Communicate scientific information using oral, written, and visual modes.

Course Schedule

Lecture Topics and Laboratory Experiments

The course is organized into weekly topics and corresponding laboratory experiments. Below is a summary table:

Week of	Lecture Topics	Laboratory Experiments
Sep. 02	Welcome and Chapter 1 (Introduction)	Lab Safety Briefing, Washing Glassware, Safety Quiz
Sep. 08	Chapter 2 (Atoms, Molecules, & Ions)	Density Experiment #1
Sep. 15	Chapter 2 (continued)	Avogadro's Number Experiment #5
Sep. 22	Chapter 3 (Chemical Reactions & Stoichiometry)	Chemical Reactions Experiment #4
Sep. 29	Chapter 4 (Reactions in Aqueous Solutions)	Spectrophotometric Determination of Copper Experiment #2
Oct. 06	Chapter 4 (continued)	Solution Conductivity and pH Experiment #3
Oct. 13	Chapter 5 (Thermochemistry)	Calorimetry Experiment #13
Oct. 20	Chapter 6 (Electronic Structure of Atoms)	Limiting Reactant Experiment #8
Oct. 27	Chapter 6 (continued)	Bright Light Spectra Experiment #11
Nov. 03	Chapter 7 (Periodic Properties of Elements)	Titrations Experiment #7
Nov. 10	Chapter 7 (continued)	Heat, Temperature, and Absolute Zero Experiment #9
Nov. 17	Chapter 8 (Chemical Bonding)	Molar Mass of Gas Experiment #12
Nov. 24	Chapter 9 (Molecular Geometry & Bonding Theories)	Classroom Assignment Presentations
Dec. 01	Chapter 10 (Gases)	No Laboratory Class (Thanksgiving Holiday)
Dec. 08	Review	Molecular Geometry – Dry Lab
Dec. 15	Final ACS Comprehensive Exam	No Laboratory Class (Final Exam Week)

Additional info: Deadlines for classroom assignments and lab report submissions are specified in the schedule. Lab reports are due at the start of the next lab following completion.

Key Topics Covered

Atomic Structure and Periodicity

This topic introduces the fundamental building blocks of matter: atoms, molecules, and ions. Students learn about atomic theory, electron configuration, and periodic trends.

• Atomic Theory: The concept that all matter is composed of atoms.

• Electron Configuration: Arrangement of electrons in an atom's orbitals.

• Periodic Trends: Patterns in properties such as atomic radius, ionization energy, and electronegativity across the periodic table.

Example: The periodic table organizes elements by increasing atomic number, revealing recurring chemical properties.

Chemical Reactions and Stoichiometry

Chemical reactions involve the transformation of substances through breaking and forming chemical bonds. Stoichiometry is the quantitative study of reactants and products in chemical reactions.

• Balanced Chemical Equations: Represent the conservation of mass in reactions.

• Stoichiometric Calculations: Use mole ratios to determine amounts of substances involved.

Formula:

$\text{Moles} = \frac{\text{Mass}}{\text{Molar Mass}}$

Example: Calculating the amount of product formed from a given amount of reactant using mole ratios.

Thermochemistry

Thermochemistry studies the energy changes that occur during chemical reactions, focusing on heat transfer and enthalpy.

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

• Calorimetry: Experimental measurement of heat changes in reactions.

Formula:

$q = m c \Delta T$

where $q$ is heat, $m$ is mass, $c$ is specific heat, and $\Delta T$ is temperature change.

Example: Determining the heat absorbed or released in a reaction using calorimetry data.

Chemical Bonding and Molecular Geometry

This topic explores how atoms bond to form molecules and the shapes those molecules take.

• Ionic and Covalent Bonds: Types of chemical bonds formed by electron transfer or sharing.

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

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

Example: Drawing the Lewis structure for $\ce{H2O}$ and predicting its bent geometry.

Gases and Their Properties

The behavior of gases is described by physical laws relating pressure, volume, temperature, and amount.

• Ideal Gas Law: $PV = nRT$

• Gas Properties: Pressure, volume, temperature, and moles.

Example: Calculating the volume of a gas at given temperature and pressure using the ideal gas law.

Assessment and Grading

Grading Breakdown

Assignment Type	Points
In-Class Quizzes (10 x 10 pts)	100
Homework Problems (10 x 10 pts)	100
Laboratory Grade (11 labs x 22 pts + Safety Quiz + Bonus/Make-up)	250
Classroom Assignment (Presentation)	100
Regular Exams (3 x 100 pts)	300
Final Comprehensive Exam	150
Total	1000

Letter Grade Scale:

Grade	Score Range
A	900 - 1000 (90% to 100%)
B+	870 - 899 (87% up to 90%)
B	800 - 869 (80% up to 87%)
C+	770 - 799 (77% up to 80%)
C	700 - 769 (70% up to 77%)
D+	670 - 699 (67% up to 70%)
D	600 - 669 (60% up to 67%)
F	below 600 (below 60%)

Attendance and Laboratory Policy

Lecture and Laboratory Attendance

• Lecture Attendance: Required for successful completion; excused absences must be documented.

• Laboratory Attendance: Mandatory; missing more than 25% of labs (more than three sessions) results in failure to complete course requirements.

• Lab Reports: Due at the start of the next lab following completion; late submissions incur penalties.

Safety: Proper safety attire and behavior are required in all laboratory sessions.

Support and Resources

Instructor and Administrative Contacts

• Instructor: Dr. Jamshed Ayub ([e-mail])

• Program Director: Dr. Mark Young ([e-mail])

• Division Chairperson: Professor William Kelvey ([e-mail])

• Administrative Associate: Ms. Christine Herrmann ([e-mail])

Students are encouraged to communicate concerns and seek support as needed. Disability support services and academic integrity policies are in place to ensure a fair and supportive learning environment.

Additional Information

• Course policies, grading, and assignment details are available on the college website and in the course catalog.

• Technology requirements include access to a computer with internet and Microsoft Office.

• Final ACS Comprehensive Exam is scheduled for Dec. 15, 2025, from 8:00 - 10:00 AM.