General Chemistry I (CHEM-1311) Syllabus and Study Guide

Course Overview

This course provides a comprehensive introduction to the fundamental principles of chemistry for science majors, health sciences, and engineering students. Topics include measurements, properties and classification of matter, atomic structure, chemical reactions, stoichiometry, periodicity, chemical bonding, molecular structure, solutions, gases, and an introduction to thermodynamics and descriptive chemistry.

• Modality: In-person

• Meeting Times: 8:00-9:50 AM, Tuesdays and Thursdays

• Location: WHI Room 212

• Credits: 3

Course Topics and Weekly Schedule

The following schedule outlines the main topics covered in the course, aligned with standard General Chemistry I curriculum:

Key Learning Outcomes

• Define the fundamental properties of matter.

• Classify matter, compounds, and chemical reactions.

• Determine the basic nuclear and electronic structure of atoms.

• Identify trends in chemical and physical properties using the Periodic Table.

• Describe bonding and molecular shapes.

• Solve stoichiometric problems and perform unit conversions.

• Write and balance chemical equations; use nomenclature rules.

• Apply gas laws and kinetic molecular theory.

• Analyze the role of energy in chemical and physical changes.

Major Topics and Concepts

Matter and Measurement

• Matter: Anything that has mass and occupies space. Classified as elements, compounds, and mixtures.

• Measurement: Quantitative description of properties using units (SI system). Includes length (meter), mass (kilogram), time (second), temperature (kelvin), and amount (mole).

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

• Dimensional Analysis: Method for converting between units using conversion factors. Example: To convert 25.0 cm to meters:

Atoms, Molecules, and Ions

• Atom: The smallest unit of an element that retains its chemical properties.

• Molecule: Two or more atoms bonded together.

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

• Atomic Structure: Atoms consist of protons, neutrons, and electrons. Protons and neutrons are in the nucleus; electrons occupy orbitals around the nucleus.

• Isotopes: Atoms of the same element with different numbers of neutrons.

• Example: and are isotopes of carbon.

Chemical Reactions and Stoichiometry

• Chemical Reaction: Process in which substances (reactants) are transformed into new substances (products).

• Stoichiometry: Quantitative relationship between reactants and products in a chemical reaction.

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

• Mole Concept: 1 mole = entities (Avogadro's number).

• Example Calculation: To find moles from grams:

Reactions in Aqueous Solution

• Solution: Homogeneous mixture of two or more substances.

• Solvent: The substance present in the greatest amount (usually water in aqueous solutions).

• Types of Reactions: Precipitation, acid-base, and redox reactions.

• Net Ionic Equation: Shows only the species that actually change during the reaction.

• Example: Net ionic:

Gases

• Gas Laws: Describe the relationships between pressure, volume, temperature, and amount of gas.

• Ideal Gas Law:

• Kinetic Molecular Theory: Explains the behavior of gases in terms of particle motion.

• Example: Calculate the volume of 1.00 mol of an ideal gas at STP (, ):

Thermochemistry

• Thermochemistry: Study of energy changes in chemical reactions.

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

• Enthalpy (): Heat change at constant pressure.

• Calorimetry: Measurement of heat flow.

• Example: (where = heat, = mass, = specific heat, = temperature change)

Electronic Structure of Atoms

• Quantum Mechanics: Describes the behavior of electrons in atoms.

• Principal Quantum Number (): Indicates the main energy level.

• Electron Configuration: Distribution of electrons among orbitals.

• Example: Electron configuration of oxygen:

Periodic Table and Periodicity

• Periodic Law: Properties of elements are periodic functions of their atomic numbers.

• Trends: Atomic radius, ionization energy, electron affinity, and electronegativity vary predictably across periods and groups.

• Example: Atomic radius decreases across a period and increases down a group.

Chemical Bonding and Molecular Structure

• Ionic Bond: Electrostatic attraction between oppositely charged ions.

• Covalent Bond: Sharing of electron pairs between atoms.

• Lewis Structures: Diagrams showing bonding and lone pairs.

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

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

Liquids and Intermolecular Forces

• Intermolecular Forces: Forces between molecules, including hydrogen bonding, dipole-dipole, and London dispersion forces.

• Properties: Affect boiling point, melting point, and solubility.

• Example: Water has a high boiling point due to strong hydrogen bonding.

Assessment and Grading

Grading Scale

Student Success Tips

• Attend all classes and participate actively.

• Read and review the textbook and class notes regularly.

• Complete all assignments and practice problems.

• Seek help promptly when needed.

• Use available resources such as tutoring, library, and online materials.

• Prepare for exams by reviewing objectives and practicing problems.

Required Materials

• Textbook: Brown, LeMay Jr, Bersten, Murphy, Woodward, Stoltzfus. Chemistry: The Central Science, 14th or 15th ed., Pearson.

• Calculator: Scientific calculator (cell phones not permitted during exams).

Additional Information

• Comprehensive final exam is required for all students.

• Make-up exams are not given except as specified; final exam may replace one missed exam.

• Academic integrity and attendance policies are strictly enforced.

• Canvas is used for course management and assignments.

• Support services are available for tutoring, library access, and student needs.

Additional info: This guide summarizes the syllabus and key study topics for General Chemistry I, providing a structured overview for exam preparation and course success.