Introduction to Chemistry: Course Syllabus and Topic Overview

Course Syllabus Overview

Introduction

This syllabus outlines the topics, schedule, and laboratory activities for an introductory college-level chemistry course. The course covers fundamental concepts in chemistry, including measurement, matter, atomic structure, chemical reactions, and more. Each week introduces new chapters and laboratory experiments designed to reinforce theoretical knowledge with practical experience.

Course Topics and Weekly Breakdown

Week	Topics	Laboratory Activities
1	Ch 1: The Chemical World, Introduction to Chemistry Ch 2: Measurement and Problem Solving	Safety Check-in, Significant Figures
2	Ch 2: Significant Figures, Dimensional Analysis Ch 3: Properties of Matter	Experiment: Glassware, Quiz 1
3	Ch 3: Properties of Matter Ch 4: Atomic Theory, Elements	Experiment: Density Determination, Report
4	Ch 4: Atomic Theory, Periodic Properties Ch 5: Molecules and Compounds	Experiment: Separation of Mixtures, Quiz 2
5	Ch 5: Molecules and Compounds Ch 6: Chemical Composition	Experiment: Types of Reaction, Quiz 3
6	Ch 6: Chemical Composition, Formulas, Nomenclature	Experiment: Copper Reactions, Quiz 4
7	Ch 6: Molar Mass, Empirical and Molecular Formulas Ch 7: Writing and Balancing Equations	Experiment: Types of Reaction, Report
8	Ch 7: Types of Reactions Ch 8: Stoichiometry I	Experiment: Reactions between Ions, Report
9	Ch 10: Chemical Bonding, Lewis Structures	Experiment: pH, Quiz 5
10	Ch 10: Chemical Bonding, Lewis Structures	Problem Set: VSEPR, Molecular Modeling
11	Ch 11: KMT, Pressure, Ideal Gas Law	Experiment: Reaction of Mg/HO, Quiz 6
12	Ch 11: KMT, Pressure, Ideal Gas Law Ch 12: Liquids, Solids, Phase Changes	Experiment: MyHC, Quiz 7
13	Ch 13: Solutions	Experiment: Concentration of CaCl2, Report
14	Ch 14: Acids and Bases	Experiment: Titration of Acetic Acid, Quiz 8
15	Ch 14: Titrations, Review	Experiment: pH, Final Check-out

Key Chapter Summaries

Ch 1: The Chemical World

This chapter introduces the scope of chemistry, the scientific method, and the importance of chemistry in everyday life.

• Chemistry: The study of matter, its properties, and the changes it undergoes.

• Scientific Method: A systematic approach to research and experimentation.

• Application: Chemistry is used in medicine, engineering, environmental science, and more.

Ch 2: Measurement and Problem Solving

Focuses on the use of measurements, units, and significant figures in chemical calculations.

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

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

• Example Equation: $\text{Value in new units} = \text{Value in old units} \times \frac{\text{Conversion factor}}{1}$

Ch 3: Matter and Energy

Explores the classification of matter, physical and chemical properties, and the concept of energy.

• Matter: Anything that has mass and occupies space.

• States of Matter: Solid, liquid, gas.

• Energy: The capacity to do work; includes kinetic and potential energy.

Ch 4: Atoms and Elements

Describes atomic theory, structure of atoms, and the periodic table.

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

• Element: A pure substance consisting of only one type of atom.

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

Ch 5: Molecules and Compounds

Discusses chemical bonding, molecular structure, and nomenclature.

• Molecule: Two or more atoms bonded together.

• Compound: A substance composed of two or more different elements.

• Chemical Formula: Represents the types and numbers of atoms in a molecule.

Ch 6: Chemical Composition

Covers molar mass, empirical and molecular formulas, and percent composition.

• Molar Mass: The mass of one mole of a substance, measured in grams per mole.

• Empirical Formula: The simplest whole-number ratio of atoms in a compound.

• Example Equation: $\text{Molar mass} = \sum (\text{atomic mass of each element} \times \text{number of atoms})$

Ch 7: Chemical Reactions

Introduces types of chemical reactions and how to write and balance chemical equations.

• Chemical Reaction: A process in which substances are transformed into new substances.

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

• Example Equation: $\text{CH}_4 + 2\text{O}_2 \rightarrow \text{CO}_2 + 2\text{H}_2\text{O}$

Ch 8: Quantities in Chemical Reactions (Stoichiometry)

Explains how to calculate amounts of reactants and products in chemical reactions.

• Stoichiometry: The quantitative relationship between reactants and products.

• Mole Ratio: Used to convert between amounts of substances in a reaction.

• Example Equation: $\text{Moles of A} \times \frac{\text{Moles of B}}{\text{Moles of A}} = \text{Moles of B}$

Ch 9: Electrons in Atoms and the Periodic Table

Describes electron configuration and its influence on chemical properties.

• Electron Configuration: The arrangement of electrons in an atom.

• Periodic Trends: Patterns in properties such as atomic radius, ionization energy, and electronegativity.

Ch 10: Chemical Bonding

Explores ionic, covalent, and metallic bonding, as well as Lewis structures and molecular geometry.

• Ionic Bond: Formed by the transfer of electrons between atoms.

• Covalent Bond: Formed by the sharing of electrons between atoms.

• Lewis Structure: Diagram showing the arrangement of electrons in a molecule.

Ch 11: Gases

Discusses the properties of gases, kinetic molecular theory, and gas laws.

• Ideal Gas Law: Relates pressure, volume, temperature, and number of moles. $PV = nRT$

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

Ch 12: Liquids, Solids, and Intermolecular Forces

Examines the structure and properties of liquids and solids, and the forces between molecules.

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

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

Ch 13: Solutions

Describes the formation, concentration, and properties of solutions.

• Solution: A homogeneous mixture of two or more substances.

• Concentration: Amount of solute in a given amount of solvent, often measured in molarity. $\text{Molarity} = \frac{\text{moles of solute}}{\text{liters of solution}}$

Ch 14: Acids and Bases

Explores the properties, definitions, and reactions of acids and bases.

• Acid: Substance that donates a proton (H+).

• Base: Substance that accepts a proton (H+).

• pH Scale: Measures acidity or basicity of a solution. $\text{pH} = -\log[\text{H}^+]$

Ch 15: Chemical Equilibrium

Discusses reversible reactions and the concept of equilibrium.

• Chemical Equilibrium: The state in which the forward and reverse reactions occur at equal rates.

• Equilibrium Constant: $K = \frac{[\text{products}]}{[\text{reactants}]}$

Ch 16: Oxidation and Reduction

Explains redox reactions and the transfer of electrons.

• Oxidation: Loss of electrons.

• Reduction: Gain of electrons.

• Redox Reaction: A chemical reaction involving electron transfer.

Ch 17: Radioactivity and Nuclear Chemistry

Introduces nuclear reactions, types of radiation, and applications of radioactivity.

• Radioactivity: The spontaneous emission of particles or energy from unstable nuclei.

• Nuclear Reaction: Changes in the nucleus of an atom, including fission and fusion.

Laboratory Component

Laboratory experiments are integrated throughout the course to reinforce theoretical concepts. Activities include measurement techniques, chemical reactions, separation of mixtures, titrations, and molecular modeling.

Final Examination

The final exam covers all topics listed above and is scheduled for Thursday, December 11, 10:30am – 12:30pm.