General Chemistry I (CHEM 1307) Syllabus and Study Guide

Course Overview

Introduction to General Chemistry I

This course is the first in a two-semester sequence covering fundamental topics in chemistry. It focuses on understanding chemical formulas, the structure and properties of atoms and molecules, different types of chemical reactions, and the states and behavior of matter. The curriculum is designed for students majoring in physical sciences and other STEM fields, as well as those fulfilling a core science requirement.

• Chemistry 1307 is a prerequisite for Chemistry 1107.

• Topics include atomic theory, chemical bonding, stoichiometry, thermodynamics, and intermolecular forces.

• Emphasis on problem-solving, critical thinking, and quantitative reasoning.

Course Structure and Grading

Grading Breakdown

Student performance is assessed through a combination of homework, in-class activities, tests, and a final exam.

Category	% of Final Grade
Post-Class Questions/In-class activities	12.5
Homework	12.5
Three tests	45 (15% each)
Final Exam	30

Note: All assignments within each category are weighted equally. Attendance is not incorporated into your 1307 course grade.

Lecture Schedule and Topics

Weekly Topics Overview

The following is a summary of the major topics covered each week, along with associated textbook readings:

Week	Topic	Textbook Readings
1	Scientific method, SI units, significant figures, dimensional analysis, temperature, density, classification of matter	Ch. 1
2	Fundamental chemical laws, Dalton's atomic theory, modern structure, molecules, ions, periodic table, naming compounds	Ch. 2
3	Counting by weighing and moles, the mole, molar mass, percent composition, empirical formulas, chemical equations, balancing chemical equations, stoichiometric calculations, limiting reagents	Ch. 3
4-5	Types of chemical reactions: precipitation, acid-base, oxidation-reduction (redox); reaction, composition of solutions, balancing oxidation and simple oxidation-reduction reactions	Ch. 4.1-4.9
6-7	Properties of gases, pressure, gas laws and their application, gas mixtures and partial pressure, stoichiometry of gases, kinetic-molecular theory of gases, diffusion/effusion	Ch. 5.1-5.7
7-9	Introduction to thermodynamics, energy, first law, enthalpy, calorimetry, energy and enthalpy, endothermic and exothermic reactions, calorimetry	Ch. 6.1-6.3
11	Hess's Law, enthalpies of formation	Ch. 6.4 & 6.7
9	Electromagnetic radiation, nature of matter, Bohr model, quantum model, quantum numbers, orbitals, shapes, electron spin, Pauli Principle, Aufbau Principle	Ch. 7
12-13	Periodic trends, ionization energy, electron affinity, atomic radii, ionic radii, isoelectronic ions, partial ionic character, covalent bond, bond dipoles, Lewis structures, Octet rule, exceptions, resonance and VSEPR	Ch. 8
15-16	Intermolecular forces, liquid state, vapor pressure and changes of state, phase diagrams and review	Ch. 10.1, 10.2, 10.3, 10.8

Additional info: Exam dates and schedule are subject to change.

Key Concepts and Definitions

Scientific Method and Measurement

• Scientific Method: A systematic approach to research involving observation, hypothesis, experimentation, and analysis.

• SI Units: International System of Units used for standard measurements in science (e.g., meter, kilogram, second).

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

• Dimensional Analysis: Technique for converting between units using conversion factors.

• Density: Mass per unit volume, calculated as $d = \frac{m}{V}$.

Atomic Theory and Structure

• Dalton's Atomic Theory: All matter is composed of atoms; atoms of the same element are identical; atoms combine in simple whole-number ratios to form compounds.

• Periodic Table: Arrangement of elements by increasing atomic number, showing periodic trends in properties.

• Molecules and Ions: Molecules are groups of atoms bonded together; ions are charged particles formed by loss or gain of electrons.

Stoichiometry and Chemical Reactions

• Stoichiometry: Calculation of reactants and products in chemical reactions using balanced equations.

• Mole Concept: The mole is a counting unit for atoms/molecules; $1 \text{ mole} = 6.022 \times 10^{23}$ entities.

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

• Types of Reactions: Precipitation, acid-base, oxidation-reduction (redox).

Gases and Gas Laws

• Pressure: Force per unit area exerted by gas particles.

• Gas Laws: Relationships between pressure, volume, temperature, and amount of gas (e.g., Boyle's Law, Charles's Law, Ideal Gas Law).

• Ideal Gas Law: $PV = nRT$

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

Thermodynamics and Calorimetry

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

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

• Calorimetry: Measurement of heat changes in chemical reactions.

• Hess's Law: The total enthalpy change for a reaction is the sum of the enthalpy changes for individual steps.

Atomic Structure and Quantum Theory

• Electromagnetic Radiation: Energy transmitted through space as waves (e.g., light).

• Quantum Numbers: Numbers that describe the properties of atomic orbitals and electrons.

• Electron Configuration: Arrangement of electrons in an atom's orbitals.

• Pauli Exclusion Principle: No two electrons in an atom can have the same set of quantum numbers.

Chemical Bonding and Molecular Structure

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

• Octet Rule: Atoms tend to gain, lose, or share electrons to achieve eight valence electrons.

• VSEPR Theory: Valence Shell Electron Pair Repulsion theory predicts molecular shapes based on electron pair repulsion.

• Resonance: Delocalization of electrons in molecules with multiple valid Lewis structures.

Intermolecular Forces and States of Matter

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

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

• Phase Diagrams: Graphical representation of the states of matter under different conditions of temperature and pressure.

Course Learning Outcomes

• Use dimensional analysis with proper attention to units and significant figures.

• Name and classify inorganic compounds.

• Determine empirical and molecular formulas from empirical data.

• Understand and use the mole concept in stoichiometry of reactions and solutions.

• Balance chemical equations and use stoichiometric relationships in calculations.

• Identify different types of reactions (precipitation, neutralization, oxidation-reduction) and predict reactant amounts.

• Apply thermodynamic and molecular theory to processes involving gases.

• Assess the basic concepts of thermodynamics and the role of energy and enthalpy in chemical reactions and processes.

• Understand the basic concepts of quantum theory, determine electron configurations of atoms, and use periodic trends to make predictions about atomic properties.

• Use Lewis structures and chemical bonding and determine the molecular geometry of molecules using VSEPR theory.

• Explain the intermolecular attractive forces that determine the properties of the states of matter and phase changes.

Required Materials

• Cengage Unlimited 4-month Access (includes digital access to the textbook and online homework)

• Chemistry by Steven Zumdahl, Susan A. Zumdahl & Donald DeCoste, 10th edition, Cengage Learning (2016)

Additional Information

• Calculator: Only scientific calculators are permitted for tests; programmable calculators and those with Wi-Fi are not allowed.

• Attendance: Participation is important for success but is not graded.

• Homework: Online homework is assigned regularly; students are encouraged to complete all assignments, even after the due date, for practice.

• Exams: Three midterm tests and a cumulative final exam; the final exam grade may replace the lowest midterm grade.

• Support: Peer review sessions, tutoring, and online resources are available for additional help.