General Chemistry I: Course Syllabus and Foundational Concepts

General Chemistry I: Course Overview

Introduction

This document outlines the structure, expectations, and foundational topics for a General Chemistry I course. It serves as a guide for students to understand the course objectives, assessment methods, and key content areas essential for success in college-level chemistry.

Instructor and Course Information

• Instructor: Dr. Jamie Schneider

• Office: CSH 257

• Email: [e-mail]

• Office Hours: M 9:00–10:30 am, W 1:30–3:00 pm (or by appointment)

• Course Location: Ag Sci 200

• Format: Face-to-face

• Meeting Times: MWF 11:00–11:50 am

• Discussion (PLTL): Thursdays, scheduled as assigned

Course Description

This course is the first in the general chemistry sequence, providing a foundation for further study in chemistry and related sciences. It covers atomic and molecular structure, bonding, intermolecular forces, chemical formulas and equations, stoichiometry, and introductory thermodynamics and kinetics.

Course Objectives

By the end of this course, students should be able to:

• Visualize matter as consisting of atoms with internal structures dictating their chemical and physical behavior.

• Differentiate between and describe ionic and covalent bonding.

• Predict the geometric structures of chemical compounds and explain how geometry influences chemical and physical behavior.

• Identify intermolecular forces and explain their effects on properties of substances.

• Utilize intermolecular forces to explain and diagram properties of molecules.

• Quantify matter changes in terms of balanced chemical reactions, stoichiometry, and limiting reactants.

• Describe the role of energy exchange in chemical reactions.

Required Materials

• Textbook: "Chemistry: An Atoms-Focused Approach" by Gilbert, Kirss, Bretz, Foster, 3rd ed. (eBook or print)

• Online Resources: Canvas, Aktiv Learning, OpenStax General Chemistry (optional)

• Calculator: Scientific calculator (non-programmable, e.g., TI-30XS)

Major Topics Covered

• Measurement and Uncertainty: Units, significant figures, precision, and accuracy.

• Atoms and Elements: Atomic theory, atomic structure, periodic table, mole concept.

• Bonding and Molecular Structure: Ionic and covalent bonding, Lewis structures, molecular geometry, polarity.

• Intermolecular Forces and Solutions: Types of intermolecular forces, phase changes, solubility, phase diagrams.

• Stoichiometry: Balancing chemical equations, mole relationships, limiting reactants, percent yield.

• Chemical Reactions in Water: Electrolytes, concentration calculations, precipitation, acid-base, and redox reactions.

• Thermodynamics and Energy: First law of thermodynamics, enthalpy, calorimetry, heat capacity.

Assessment and Grading

Assessment Components

Assessment	Description	Percent of Final Grade
Worksheets & MC Questions	In-class worksheets and multiple choice for self-check	8%
Homework (Aktiv Online)	Weekly assignments	10%
Quizzes	Weekly quizzes (Tuesday/Thursday)	12%
PLTL Participation	Participation in peer-led discussion	8%
Exams	3 exams (see schedule)	45%
Final Exam	Cumulative	15%

Grading Scale

Grade	Percent Range
A	93–100
A-	90–92
B+	87–89
B	83–86
B-	80–82
C+	77–79
C	73–76
C-	70–72
D+	67–69
D	63–66
D-	60–62
F	59 and below

Course Policies and Support

• Homework: Assigned weekly, due on Monday and Wednesday via Aktiv Learning.

• Quizzes: Two per week, due Tuesday and Thursday evenings via Quiz A.

• PLTL (Peer-Led Team Learning): Required participation in weekly discussion sections.

• Attendance: Required for all exams and PLTL sessions.

• Accommodations: Available for students with documented disabilities through the Disability Resource Center.

• Academic Integrity: Adherence to university policies on honesty and conduct is expected.

• Support Services: Counseling, academic support, and inclusivity resources are available.

Key Chemistry Concepts (Expanded)

Measurement and Uncertainty

• Significant Figures: Digits in a measurement that are known with certainty plus one estimated digit.

• Precision vs. Accuracy: Precision refers to the reproducibility of measurements; accuracy refers to how close a measurement is to the true value.

• Example: Measuring the mass of a sample multiple times and calculating the average and deviation.

Atoms and Elements

• Atomic Theory: All matter is composed of atoms, which are the smallest units of elements.

• Atomic Structure: Atoms consist of protons, neutrons, and electrons.

• Periodic Table: Organizes elements by increasing atomic number and similar chemical properties.

• Mole Concept: 1 mole = $6.022 \times 10^{23}$ particles (Avogadro's number).

• Example: Calculating the number of atoms in a given mass of an element.

Bonding and Molecular Structure

• Ionic Bonding: Transfer of electrons from one atom to another, forming ions.

• Covalent Bonding: Sharing of electron pairs between atoms.

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

• Molecular Geometry: The 3D arrangement of atoms in a molecule, predicted by VSEPR theory.

• Example: Drawing the Lewis structure and predicting the shape of $\ce{H2O}$.

Intermolecular Forces and Solutions

• Types of Forces: London dispersion, dipole-dipole, hydrogen bonding.

• Phase Changes: Transitions between solid, liquid, and gas states.

• Solubility: The ability of a substance to dissolve in another substance.

• Example: Explaining why water has a high boiling point due to hydrogen bonding.

Stoichiometry

• Balancing Equations: Ensuring the same number of each atom on both sides of a chemical equation.

• Mole Relationships: Using coefficients in balanced equations to relate amounts of reactants and products.

• Limiting Reactant: The reactant that is completely consumed first, limiting the amount of product formed.

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

• Example: Calculating the amount of product formed from given reactant quantities.

Chemical Reactions in Water

• Electrolytes: Substances that dissociate into ions in water, conducting electricity.

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

• Precipitation Reactions: Formation of an insoluble product from two soluble reactants.

• Acid-Base Reactions: Transfer of protons ($\ce{H+}$) between reactants.

• Redox Reactions: Transfer of electrons between species.

• Example: Identifying the precipitate in a reaction between $\ce{NaCl}$ and $\ce{AgNO3}$.

Thermodynamics and Energy

• First Law of Thermodynamics: Energy cannot be created or destroyed, only transferred or transformed.

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

• Calorimetry: Measurement of heat flow in a chemical reaction.

• Heat Capacity ($C$): $q = C \Delta T$

• Example: Calculating the heat absorbed by water when its temperature increases.

Additional Information

• Students are expected to adhere to university policies on academic integrity, inclusivity, and accommodations.

• Support services are available for academic, personal, and accessibility needs.