Course Overview

Introduction to Principles of Chemistry I

This course provides a foundational study of chemistry, emphasizing the development of critical thinking and problem-solving skills. Topics are presented in the context of the basic principles of chemistry, with a focus on atomic and molecular structure, chemical reactions, and the properties of matter. The course is designed for science majors and fulfills a General Education requirement in the Natural Sciences.

• Course Code: CHM 1001

• Credits: 3

• Instructor: Dr. Darlene D’Allessi Gandolfi

• Class Meeting Times: Tues/Thurs, 9:50 AM – 11:05 AM

• Location: BR 108

Main Topics Covered

1. Matter and Measurements

This topic introduces the concept of matter, its classification, and the methods used to measure its properties.

• Matter: Anything that has mass and occupies space.

• Classification: Elements, compounds, and mixtures.

• Measurement: Use of SI units, precision, and accuracy.

• Example: Measuring the mass of a sample using a balance and recording the value in grams (g).

2. Atoms, Molecules, and Ions

This section covers the structure of atoms, the formation of molecules, and the nature of ions.

• Atom: The smallest unit of an element, consisting of protons, neutrons, and electrons.

• Molecule: Two or more atoms bonded together.

• Ion: An atom or molecule with a net electric charge due to the loss or gain of electrons.

• Example: Sodium ion () and chloride ion () combine to form sodium chloride ().

3. Mass Relations & Stoichiometry

Stoichiometry involves the calculation of reactants and products in chemical reactions using balanced equations.

• Law of Conservation of Mass: Mass is neither created nor destroyed in a chemical reaction.

• Stoichiometric Calculations: Use of mole ratios from balanced equations.

• Formula:

• Example: Calculating the amount of produced from the combustion of .

4. Chemical Reactions & Solution Stoichiometry

This topic explores different types of chemical reactions and the quantitative relationships in solutions.

• Types of Reactions: Synthesis, decomposition, single replacement, double replacement, combustion.

• Solution Stoichiometry: Calculating concentrations and volumes in reactions involving solutions.

• Formula: (for dilution calculations)

• Example: Determining the concentration of after dilution.

5. Gases and Gas Laws

This section covers the properties of gases and the laws that describe their behavior.

• Properties of Gases: Compressibility, expansion, low density.

• Gas Laws: Boyle’s Law, Charles’s Law, Avogadro’s Law, Ideal Gas Law.

• Formula: (Ideal Gas Law)

• Example: Calculating the pressure exerted by a gas in a container.

6. Thermochemistry

Thermochemistry studies the energy changes that occur during chemical reactions.

• Energy: The capacity to do work or produce heat.

• Enthalpy (): The heat content of a system at constant pressure.

• Formula: (heat calculation)

• Example: Calculating the heat absorbed by water when heated.

7. Electronic Structure & the Periodic Table

This topic examines the arrangement of electrons in atoms and how this relates to the periodic table.

• Electronic Configuration: Distribution of electrons among atomic orbitals.

• Periodic Trends: Atomic radius, ionization energy, electronegativity.

• Example: Explaining why fluorine is more electronegative than sodium.

8. Chemical Bonding

Chemical bonding describes how atoms combine to form molecules and compounds.

• Types of Bonds: Ionic, covalent, metallic.

• Lewis Structures: Diagrams showing the arrangement of electrons in molecules.

• Example: Drawing the Lewis structure for .

9. Liquids and Solids

This section explores the properties and structures of liquids and solids.

• Liquids: Definite volume, indefinite shape, ability to flow.

• Solids: Definite shape and volume, particles arranged in a fixed pattern.

• Example: Comparing the melting points of ionic and molecular solids.

Course Learning Objectives

• Apply the scientific method to solve chemical problems.

• Use chemical terminology and symbols to describe atomic and molecular structures.

• Understand and perform calculations in chemistry, including stoichiometry and gas laws.

• Describe and explain chemical phenomena, reactions, and physical properties of matter.

• Predict chemical outcomes and describe bonding and molecular geometry.

• Distinguish between different types of chemical and physical changes.

Required Course Materials

• Textbook: Chemistry: Principles & Reactions, 8th Edition by Masterton & Hurley

• Online Learning Platform: OWLv2 (for assignments and quizzes)

• Supplemental Materials: Study guides and problem sets (as assigned)

Course Schedule

Weekly Topics and Assessments

Additional info: The schedule continues with review sessions and exams as indicated in the syllabus.

Grading Scheme

• OWL Assignments: 50 pts

• Quizzes: 50 pts

• Exams: 200 pts

• Final Exam: 100 pts

• Total: 400 pts

Course Policies

• Attendance: Required for all lectures. Absences must be excused for illness, emergencies, or university-sponsored trips.

• Homework: Assigned problems from the textbook and online platform (OWL).

• Quizzes: Six quizzes released on OWL, covering key chapters.

• Exams: Three midterm exams and one final exam. No make-up exams except for documented emergencies.

• Academic Integrity: Cheating and plagiarism are not tolerated. Use of generative AI (e.g., ChatGPT) is prohibited for assignments and exams.

• Electronic Devices: Cell phones and other devices must be silenced during class.

Textbook Chapters

• Chapter 1: Matter and Measurements

• Chapter 2: Atoms, Molecules, and Ions

• Chapter 3: Mass Relations & Stoichiometry

• Chapter 4: Reactions & Solution Stoichiometry

• Chapter 5: Gases and Gas Laws

• Chapter 6: Thermochemistry

• Chapter 7: Electronic Structure & the Periodic Table

• Chapter 8: Chemical Bonding

• Chapter 9: Liquids and Solids

Additional Info

• Course uses OWLv2 for assignments and quizzes.

• Supplemental study guides and problem sets are provided.

• Final exam is cumulative and cannot be dropped.