General Chemistry Syllabus Overview

Course Description

This introductory General Chemistry course focuses on the study of matter, its structure, properties, transformations, and applications. It provides foundational knowledge essential for further studies in science, engineering, and health-related fields.

General Objective

• To understand the fundamental principles of chemistry and apply them to solve problems related to physical and chemical phenomena.

Learning Outcomes

• Explain atomic structure and the organization of the periodic table.

• Interpret chemical bonding and properties of compounds.

• Solve stoichiometric problems involving chemical equations and quantities.

• Analyze states of matter and properties of solutions.

• Apply concepts of chemical equilibrium, acids, and bases to various chemical systems.

Core Topics and Units

Unit 1: Introduction to Chemistry and Measurements

• Matter: Definition, classification, and properties.

• Measurement: Units, significant figures, and scientific notation.

• Physical vs. Chemical Properties: Distinction and examples.

• Example: Measuring the mass and volume of a substance to determine its density.

Unit 2: Atomic Structure and Quantum Theory

• Atomic Models: Historical development from Dalton to quantum models.

• Subatomic Particles: Protons, neutrons, and electrons.

• Quantum Numbers: Principal, angular momentum, magnetic, and spin quantum numbers.

• Example: Electron configuration of oxygen:

Unit 3: Periodic Table and Periodic Properties

• Periodic Law: Organization of elements by atomic number.

• Trends: Atomic radius, ionization energy, electron affinity, and electronegativity.

• Example: Explaining why sodium is more reactive than magnesium based on periodic trends.

Unit 4: Chemical Bonding and Molecular Geometry

• Ionic and Covalent Bonds: Formation and properties.

• Lewis Structures: Representation of molecules.

• VSEPR Theory: Predicting molecular shapes.

• Example: Drawing the Lewis structure and predicting the geometry of (linear).

Unit 5: Chemical Reactions and Stoichiometry

• Types of Reactions: Synthesis, decomposition, single and double displacement, combustion.

• Balancing Equations: Conservation of mass.

• Stoichiometric Calculations: Mole-mass, mass-mass, and limiting reactant problems.

• Example: Calculating the mass of water produced from 10 g of hydrogen gas and excess oxygen.

Unit 6: States of Matter

• Solid, Liquid, Gas: Properties and differences.

• Kinetic Molecular Theory: Explanation of gas behavior.

• Phase Changes: Melting, boiling, sublimation, etc.

• Example: Using the ideal gas law:

Unit 7: Solutions and Concentrations

• Types of Solutions: Homogeneous mixtures, solubility.

• Concentration Units: Molarity, molality, percent composition.

• Example: Preparing a 1.0 M NaCl solution by dissolving 58.44 g of NaCl in 1 L of water.

Unit 8: Thermochemistry

• Energy Changes: Endothermic and exothermic processes.

• First Law of Thermodynamics: Conservation of energy.

• Enthalpy (): Heat flow at constant pressure.

• Example: Calculating the heat released in the combustion of methane.

Unit 9: Chemical Equilibrium

• Dynamic Equilibrium: Forward and reverse reactions at equal rates.

• Equilibrium Constant (): Expression and calculations.

• Le Châtelier's Principle: Predicting shifts in equilibrium.

• Example: Writing the equilibrium expression for

Unit 10: Acids, Bases, and Ionic Equilibrium

• Definitions: Arrhenius, Brønsted-Lowry, and Lewis concepts.

• pH and pOH: Calculations and significance.

• Buffer Solutions: Composition and function.

• Example: Calculating the pH of a 0.01 M HCl solution:

Unit 11: Introduction to Organic and Biochemistry

• Basic Organic Structures: Hydrocarbons, functional groups.

• Biochemical Relevance: Importance of organic molecules in biological systems.

• Example: Identifying functional groups in glucose.

Teaching Strategies

• Lectures, problem-solving sessions, laboratory experiments, collaborative learning, case studies, and applied activities.

Assessment Methods

Basic Bibliography

• Brown, LeMay, Bursten. Química: La Ciencia Central.

• Chang y Goldsby. Química.

• Petrucci, Herring, Madura. Química General.