CHEM 280: Introduction to Chemistry

Course Overview

This course provides an overview of general chemistry, introducing foundational concepts essential for further study in chemistry and related sciences. Students will explore topics such as stoichiometry, atomic and molecular structure, chemical bonding, thermochemistry, kinetics, equilibrium, acids and bases, and the chemical properties of elements. Laboratory sessions reinforce theoretical knowledge through hands-on experiments.

Course Structure

• Delivery Mode: Blended learning (combination of online asynchronous and on-campus/online synchronous sessions)

• Duration: 10 weeks

• Credits: 4

• Lecture Hours: 43 (Face-to-Face: 3.5, Online Asynchronous: 13.5)

Course Learning Outcomes

Upon successful completion of this course, students will be able to:

1. Evaluate the chemical and physical properties of atoms, ions, chemical bonds, Lewis structures, radioactivity, and VSEPR theory as they relate to trends in the Periodic Table.

2. Predict and solve chemical reactions using basic stoichiometry, the octet rule, properties of solutions, and dimensional analysis, including related mathematical problems.

3. Synthesize chemical principles by analyzing and interpreting data obtained from laboratory experiments.

4. Apply the principles of chemical energetics and intermolecular forces to predict the chemical and physical properties of molecules.

5. Recognize and examine the structure and function of biochemical components of living organisms, such as carbohydrates, lipids, proteins, and nucleic acids, as they relate to biological molecules and real-life applications.

Main Topics and Subtopics

Atomic Structure and the Periodic Table

Understanding the structure of atoms and how this relates to the organization of the Periodic Table is fundamental in chemistry.

• Atoms and Ions: Atoms consist of protons, neutrons, and electrons. Ions are charged species formed by the gain or loss of electrons.

• Periodic Trends: Properties such as atomic radius, ionization energy, and electronegativity change predictably across periods and groups.

• Radioactivity: Some elements have unstable nuclei that emit radiation as they decay to more stable forms.

• VSEPR Theory: Valence Shell Electron Pair Repulsion theory predicts the shapes of molecules based on electron pair repulsions.

• Example: Sodium (Na) loses one electron to form Na+; chlorine (Cl) gains one electron to form Cl-.

Chemical Bonding and Molecular Structure

Chemical bonds form when atoms share or transfer electrons, resulting in molecules or compounds with specific properties.

• Ionic Bonds: Formed by the transfer of electrons from metals to nonmetals.

• Covalent Bonds: Formed by the sharing of electrons between nonmetals.

• Lewis Structures: Diagrams that show the bonding between atoms and the arrangement of valence electrons.

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

• Example: Water (H2O) has a bent molecular shape due to two lone pairs on oxygen, as predicted by VSEPR theory.

Stoichiometry and Chemical Reactions

Stoichiometry involves the calculation of reactants and products in chemical reactions using balanced chemical equations.

• Balancing Equations: Ensures the conservation of mass in chemical reactions.

• Mole Concept: The mole is a unit for counting atoms, molecules, or ions. Avogadro's number () defines one mole.

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

• Example: (2 moles of hydrogen react with 1 mole of oxygen to produce 2 moles of water).

Thermochemistry and Chemical Energetics

Thermochemistry studies the energy changes that occur during chemical reactions, particularly heat exchange.

• Enthalpy (): The heat content of a system at constant pressure.

• Endothermic vs. Exothermic: Endothermic reactions absorb heat (); exothermic reactions release heat ().

• Example: Combustion of methane is exothermic: ; kJ/mol.

Kinetics and Equilibrium

Chemical kinetics examines the rates of reactions, while equilibrium describes the state where forward and reverse reactions occur at equal rates.

• Rate Law: Expresses the relationship between the rate of a reaction and the concentration of reactants.

• Equilibrium Constant (): The ratio of product concentrations to reactant concentrations at equilibrium.

• Example: For the reaction ,

Acids, Bases, and Solutions

Acids and bases are important classes of compounds with characteristic properties and reactions in aqueous solutions.

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

• Bases: Substances that accept protons or donate hydroxide ions (OH-).

• pH Scale: Measures the acidity or basicity of a solution:

• Example: Hydrochloric acid (HCl) is a strong acid; sodium hydroxide (NaOH) is a strong base.

Biochemical Molecules

The course introduces the structure and function of key biochemical molecules found in living organisms.

• Carbohydrates: Sugars and starches that provide energy.

• Lipids: Fats and oils used for energy storage and cell membranes.

• Proteins: Polymers of amino acids with structural and catalytic roles.

• Nucleic Acids: DNA and RNA, which store and transmit genetic information.

• Example: Glucose (C6H12O6) is a simple sugar used in cellular respiration.

Laboratory Skills and Data Analysis

Laboratory sessions develop practical skills in measurement, observation, and data interpretation.

• Measurement: Use of laboratory equipment to measure mass, volume, and temperature.

• Data Analysis: Interpreting experimental results, calculating yields, and identifying sources of error.

• Example: Determining the concentration of an acid by titration with a standard base.

Course Materials

• Textbook: Introductory Chemistry Plus Mastering Chemistry by Tro, N. J. (Pearson, 7th Edition)

• Laboratory Manual: Laboratory Manual for General, Organic, and Biological Chemistry by Timberlake, Karen (Pearson Education)

Grading Scale

The following table summarizes the letter grades and their corresponding grade points:

Assessment and Evaluation

• Formative Assessments: Ongoing assignments, quizzes, and discussions to provide feedback and support learning.

• Summative Assessments: Major assignments and exams to measure student achievement of course outcomes.

Sample Assignment Breakdown

General Education Program Outcomes

• Employ effective oral and written communication skills

• Interpret quantitative data using mathematical principles

• Locate and evaluate information from multiple sources

• Demonstrate critical thinking skills

Additional Info

• All assignments must be submitted online unless otherwise noted.

• Late and make-up work policies are strictly enforced.

• Students are responsible for obtaining all required course materials.