Course Overview

This course provides a comprehensive introduction to the foundational concepts of general chemistry, focusing on the structure of atoms and molecules, chemical bonding, reactivity, stoichiometry, and chemical equilibrium. The curriculum is designed to build a strong conceptual framework for understanding chemical phenomena and laboratory practices.

Course Structure and Weekly Topics

• Mathematical Tool Box: Covers essential mathematical skills for chemistry, including dimensional analysis and significant figures.

• Atomic Structure and Light: Introduces atomic theory, the nature of light, and their interrelationship.

• Light Absorption and Emission: Explores how atoms interact with light, including absorption spectra and emission processes.

• Electron Configuration and Periodic Trends: Examines electron arrangements and trends in the periodic table.

• Ionic and Covalent Bonding: Discusses the formation and properties of ionic and covalent compounds, including crystal structures.

• Intermolecular Forces: Analyzes the forces between molecules and their effects on physical properties.

• Chemical Reactions and Stoichiometry: Focuses on reaction types, balancing equations, and quantitative relationships in reactions.

• Acids, Bases, and Equilibrium: Covers acid-base theory, titrations, and the concept of chemical equilibrium.

Laboratory Safety and Personal Protective Equipment (PPE)

Laboratory Safety Requirements

Because the classroom is also a laboratory environment, strict safety protocols must be followed to ensure the well-being of all participants. Proper attire and equipment are mandatory during all laboratory activities.

• No food or drink is allowed in the laboratory.

• Closed-toe shoes must be worn at all times. The front of the foot must be completely covered.

• Appropriate goggles must be worn during all lab activities and whenever chemicals or glassware are in use. Goggles must be impact-rated and provide splash protection.

Acceptable goggles are indirectly vented or unvented for splash protection and meet ANSI Z87.1 or ANSI Z87+ standards. Not acceptable goggles may provide impact protection but lack splash protection, which is essential in a chemistry laboratory.

Course Learning Outcomes

Unit 1: Atoms

• Use dimensional analysis to relate quantities and perform unit conversions.

• Identify isotopes and determine the number of protons, neutrons, and electrons.

• Calculate molar masses and convert between grams, moles, and number of particles.

• Describe electromagnetic radiation in terms of wavelength, frequency, energy, and color.

• Explain the relationship between absorbance, concentration, and molar absorptivity using Beer's Law:

• Use the Rydberg equation to calculate energies of absorption and emission:

• Relate photon energy to wavelength or frequency:

• Predict periodic trends such as ionization energy, electron affinity, and atomic/ionic radius.

Unit 2: Molecules

• Translate between names and empirical formulas for ionic compounds.

• Identify trends in lattice energy and common crystal structures (SC, FCC, BCC).

• Build molecular models and draw Lewis structures, including isomers and resonance forms.

• Assign formal charges and identify functional groups in organic molecules.

• Predict molecular geometry using VSEPR theory and distinguish between polar and nonpolar molecules.

• Explain the relative strengths of intermolecular forces and their effects on boiling points.

Unit 3: Reactions

• Identify evidence of chemical reactions and predict products.

• Classify reactions (precipitation, acid-base, redox) and balance equations.

• Apply stoichiometry to determine limiting reactants, yields, and concentrations.

• Determine empirical and molecular formulas from experimental data.

• Estimate reaction enthalpies using bond energies.

Unit 4: Equilibrium

• Classify compounds as acids or bases and define buffer characteristics.

• Describe equilibrium as a dynamic state and calculate equilibrium constants ().

• Use and to predict reaction direction and extent.

• Calculate pH of weak acid and base solutions.

• Apply Le Chatelier’s Principle to predict changes in equilibrium.

Assessment and Grading

• Homework (Mastery Questions): 5%

• Quizzes: 10%

• Graded Laboratory Activities: 20%

• Exam 1: 15%

• Exam 2: 20%

• Final Exam: 30%

All grading disputes must be addressed within a week of the assignment being returned. Any curve will be applied only at the end of the quarter.

Laboratory Schedule Highlights

• Density and concentration measurements

• Isotope activity

• Absorption and emission spectroscopy

• Periodic trends and solid-state structures

• Molecular structure modeling

• Chromatography and acid-base titrations

• Equilibrium experiments

Academic Honesty and Inclusivity

• Collaboration is encouraged except where individual work is specified. All collaborators must be credited appropriately.

• Academic dishonesty will be reported and may result in severe penalties.

• The course strives for an inclusive environment, respecting all backgrounds and perspectives.

Additional Information

• Required textbook: Chemistry, OpenStax

• Access to a personal computer with Microsoft Excel and reliable internet is necessary.

• Financial support is available for students in need.