Introduction to Chemistry: Course Syllabus and Topic Overview

Course Syllabus Overview

Introduction

This syllabus outlines the weekly topics, chapters, and laboratory activities for an Introduction to Chemistry college course. The course covers foundational concepts in chemistry, including measurement, matter, atomic structure, chemical reactions, and more. Each week introduces new material and laboratory experiments to reinforce theoretical knowledge.

Weekly Topics and Chapters

Week	Lecture Topics	Lab Activities
1	Ch 1: The Chemical World, Ch 2: Measurement and Problem Solving	Safety, Check-in, Significant Figures
2	Ch 2: Significant Figures, Dimensional Analysis, Density; Ch 3: Properties of Matter	Experiment: Glassware, Quiz 1
3	Ch 3: Properties of Matter (Chemical & Physical), Energy, Specific Heat	Experiment: Density determination, Report
4	Ch 4: Atomic Theory, Periodic Properties, Chemical Nomenclature, Ionic Compounds	Experiment: Separation of Mixture, Quiz 2
5	Ch 5: Quantum Model of Atom, Electron Configuration	Flame Test, Periodic Table, Report
6	Ch 6: Compounds, Formulas, Nomenclature	Copper Experiment, Quiz 3
7	Ch 6: Molar Mass, Empirical and Molecular Formulas; Ch 7: Writing & Balancing Equations	Types of Reaction, Report, Quiz 4
8	Ch 7: Types of Reactions, Stoichiometry I	Reactions between ions, Report
9	Ch 10: Chemical Bonding, Lewis Structures	pH Alarm Experiment
10	Ch 10: Chemical Bonding, Lewis Structures	VSEPR Modeling, Molecular Modeling
11	Ch 11: KMT, Pressure, Ideal Gas Law	Reaction of Mg/HO, Quiz 5
12	Ch 11: KMT, Pressure, Ideal Gas Law; Ch 12: Liquids, Solids, Phase Changes	Reaction of Mg/HO, Quiz 6
13	Ch 13: Solutions	Concentration of CaCl2, Report
14	Ch 14: Acids and Bases	Titration of Acetic Acid, Report
15	Ch 14: Titrations, Ch 15: Chemical Equilibrium	PSH, Acid-Base, Final Check-out

Key Topics Covered

Ch 1: The Chemical World

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

• Understanding the role of chemistry in everyday life and scientific research.

Ch 2: Measurement and Problem Solving

• 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.

• Density: Defined as mass per unit volume. Formula: $\text{Density} = \frac{\text{Mass}}{\text{Volume}}$

Ch 3: Matter and Energy

• Matter: Anything that has mass and occupies space.

• Physical vs. Chemical Properties: Physical properties can be observed without changing the substance; chemical properties describe the ability to undergo chemical changes.

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

• Specific Heat: The amount of heat required to raise the temperature of one gram of a substance by one degree Celsius. Formula: $q = m c \Delta T$

Ch 4: Atoms and Elements

• Atomic Theory: All matter is composed of atoms.

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

• Chemical Nomenclature: Systematic naming of chemical compounds.

Ch 5: Molecules and Compounds

• Quantum Model of Atom: Describes electron arrangement in atoms.

• Electron Configuration: Distribution of electrons among atomic orbitals.

Ch 6: Chemical Composition

• Compounds and Formulas: Chemical formulas represent the types and numbers of atoms in a compound.

• Molar Mass: Mass of one mole of a substance. Formula: $\text{Molar Mass} = \sum \text{Atomic Masses}$

• Empirical and Molecular Formulas: Empirical shows simplest ratio; molecular shows actual number of atoms.

Ch 7: Chemical Reactions

• Types of Reactions: Includes synthesis, decomposition, single replacement, double replacement, and combustion.

• Stoichiometry: Quantitative relationships in chemical reactions.

• Balancing Equations: Ensures the same number of each atom on both sides of the reaction. Example: $\ce{2H_2 + O_2 \rightarrow 2H_2O}$

Ch 10: Chemical Bonding

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

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

Ch 11: Gases

• Kinetic Molecular Theory (KMT): Explains the behavior of gases.

• Ideal Gas Law: $PV = nRT$

• Pressure: Force exerted by gas particles on container walls.

Ch 12: Liquids, Solids, and Intermolecular Forces

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

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

Ch 13: Solutions

• Concentration: Amount of solute in a given amount of solvent. Example: Molarity $M = \frac{\text{mol solute}}{\text{L solution}}$

• Solubility: Ability of a substance to dissolve in another.

Ch 14: Acids and Bases

• Acids: Substances that donate protons ($H^+$).

• Bases: Substances that accept protons.

• Titration: Technique to determine concentration of an acid or base.

Ch 15: Chemical Equilibrium

• Equilibrium: State where forward and reverse reactions occur at equal rates.

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

Additional info: This syllabus provides a comprehensive overview of the topics and laboratory activities for a standard Introduction to Chemistry course, aligning with the chapters listed in the prompt.