CHEM 191: Principles of Chemistry I – Syllabus & Core Concepts Study Guide

Course Overview

Introduction to General Chemistry

This course, CHEM 191: Principles of Chemistry I, provides a foundational understanding of the composition, structure, properties, and changes of matter. It emphasizes the molecular framework for chemical phenomena, including atomic theory, chemical bonding, periodic trends, and chemical reactions. The course is designed for science majors and fulfills a core requirement in the Chemistry Core Concentration.

• Instructor: Dr. Jane Thibeault

• Lectures: MWF 9:00 – 9:50 AM

• Office Hours: MW 12:00 – 1:30 PM, R 12:00 – 2:00 PM

• Textbook: Chemistry: A Molecular Approach, 6th Edition, Nivaldo J. Tro

Learning Objectives

Core Competencies in Chemistry

Upon completion of this course, students will be able to:

1. Interpret and apply the scientific method in the context of chemical research and experimental investigation.

2. Describe and predict chemical properties of matter and classify substances at the atomic and molecular level.

3. Explain periodic trends and relate atomic structure to elemental properties.

4. Name and classify chemical compounds, including ionic, covalent, and organic compounds, using standard nomenclature rules.

5. Analyze and manipulate chemical equations to describe and predict outcomes of acid-base, redox, and precipitation reactions.

6. Evaluate energy changes in chemical reactions using basic thermodynamic principles, including enthalpy and entropy.

7. Explain the physical behavior of gases using kinetic molecular theory and other gas laws.

8. Draw and interpret Lewis structures, including resonance and expanded octets.

9. Predict molecular geometry and polarity using VSEPR theory.

Course Topics & Schedule

Major Topics Covered

The following topics are covered throughout the semester, each corresponding to textbook chapters and weekly lectures:

• The Scientific Method: Principles and application in chemistry.

• Units, Energy, & Problem Solving: SI units, dimensional analysis, and energy concepts.

• Atomic Theory: Historical models, key experiments, and structure of the atom.

• Periodic Table & Periodic Trends: Organization, trends in atomic properties.

• Chemical Bonding & Molecular Models: Ionic, covalent, and metallic bonding; Lewis structures.

• Nomenclature: Naming ionic and covalent compounds.

• Chemical Equations & Stoichiometry: Balancing equations, mole concept, reaction yields.

• Solutions & Solubility: Solution concentration, precipitation reactions.

• Acid-Base & Redox Reactions: Definitions, reaction types, and balancing.

• Gas Laws: Pressure, volume, temperature relationships; ideal and real gases.

• Thermodynamics: Laws of thermodynamics, enthalpy, entropy, and free energy.

• Light & Spectroscopy: Electromagnetic spectrum, atomic emission, and absorption.

• Electron Configuration: Aufbau principle, Hund’s rule, Pauli exclusion.

• Molecular Geometry & Polarity: VSEPR theory, dipole moments.

• Bond Energies & Lengths: Covalent bond strength and molecular stability.

Grading & Assessment

Course Grading Breakdown

Grades are determined by performance on homework, quizzes, exams, laboratory assignments, and a cumulative final exam. The following table summarizes the point distribution:

Component	Points
Homework & Chapter Reviews	200
Quizzes	100
Exams (1-3)	300
Laboratory	250
Final Exam	150
Total	1000

Letter Grade Conversion

Percentage	Letter Grade
93–100	A
90–92.9	A-
87–89.9	B+
83–86.9	B
80–82.9	B-
77–79.9	C+
73–76.9	C
70–72.9	C-
65–69.9	D+
60–64.9	D
0–59.9	F

Key Concepts & Definitions

Scientific Method in Chemistry

The scientific method is a systematic approach to research and experimentation in chemistry. It involves:

• Observation

• Formulation of hypotheses

• Experimentation

• Analysis of data

• Drawing conclusions

Example: Determining the composition of an unknown compound by conducting controlled experiments and analyzing results.

Atomic Theory & Structure

Atomic theory describes the nature of atoms as the fundamental building blocks of matter. Key models include:

• Democritus: Proposed that matter is composed of indivisible particles called atoms.

• Dalton: Developed the first modern atomic theory, stating that atoms of each element are identical and combine in fixed ratios to form compounds.

Key Equation:

$\text{Atomic Mass} = \sum (\text{isotope mass} \times \text{fractional abundance})$

Chemical Bonding

Chemical bonds are forces that hold atoms together in compounds. Types include:

• Ionic bonds: Formed by the transfer of electrons between metals and nonmetals.

• Covalent bonds: Formed by the sharing of electrons between nonmetals.

• Metallic bonds: Involve a 'sea' of delocalized electrons among metal atoms.

Example: Sodium chloride (NaCl) is an ionic compound; water (H2O) is covalent.

Periodic Table & Trends

The periodic table organizes elements by increasing atomic number and groups elements with similar properties. Important trends include:

• Atomic radius: Decreases across a period, increases down a group.

• Ionization energy: Increases across a period, decreases down a group.

• Electronegativity: Increases across a period, decreases down a group.

Chemical Equations & Stoichiometry

Chemical equations represent chemical reactions using symbols and formulas. Stoichiometry involves quantitative relationships between reactants and products.

Key Equation:

$\text{Moles} = \frac{\text{mass (g)}}{\text{molar mass (g/mol)}}$

Example: Balancing the reaction: $2H_2 + O_2 \rightarrow 2H_2O$

Gas Laws

Gas laws describe the behavior of gases in terms of pressure, volume, temperature, and amount.

• Boyle's Law: $P_1V_1 = P_2V_2$ (at constant temperature)

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

• Ideal Gas Law: $PV = nRT$

Thermodynamics

Thermodynamics studies energy changes in chemical reactions.

• First Law: Energy cannot be created or destroyed.

• Enthalpy ($\Delta H$): Heat change at constant pressure.

• Entropy ($\Delta S$): Measure of disorder.

• Gibbs Free Energy ($\Delta G$): $\Delta G = \Delta H - T\Delta S$

Lewis Structures & VSEPR Theory

Lewis structures depict the arrangement of electrons in molecules. VSEPR theory predicts molecular shapes based on electron pair repulsion.

• Example: Water (H2O) has a bent shape due to two lone pairs on oxygen.

Course Policies & Support

Attendance, Assignments, and Exams

• Homework and quizzes are assigned regularly and completed online via Mastering Chemistry.

• Three major exams and a cumulative ACS final exam are scheduled throughout the semester.

• Laboratory work constitutes 25% of the final grade.

• Missed assignments and exams require documentation and instructor approval for make-up.

Academic Integrity

• All students must adhere to university policies regarding academic honesty and intellectual property.

• Use of AI tools for assignments or coursework is prohibited.

Support Resources

• Office hours and email support are available for questions and academic help.

• Tutoring is offered through the university’s Tutoring Center.

Course Progression & Next Steps

Advancement in Chemistry Curriculum

• A grade of C- or higher in CHEM 191 is required to enroll in CHEM 192 (Principles of Chemistry II).

• CHEM 301 (Organic Chemistry) requires successful completion of CHEM 192 with a C- or higher.

Additional info: This study guide summarizes the syllabus and core concepts for CHEM 191, providing a structured overview for exam preparation and course success.