CHEM 280 General Chemistry Syllabus and Study Guide

Course Overview

Introduction to General Chemistry

This course provides a comprehensive introduction to general chemistry, covering foundational topics such as atomic structure, chemical bonding, chemical reactions, stoichiometry, gases, solutions, acids and bases, nuclear chemistry, and introductory organic and biochemistry. The course is designed for students in health sciences and related fields, emphasizing both theoretical understanding and practical laboratory skills.

Course Learning Outcomes

• Evaluate chemical and physical properties of atoms, ions, chemical bonds, and compounds.

• Understand atomic structure and periodic trends using the Periodic Table.

• Interpret chemical reactions and apply stoichiometric relationships.

• Apply laboratory techniques for measurement, safety, and chemical analysis.

• Analyze the properties of biomolecules and their roles in biological systems.

Course Outline

Weekly Topics and Objectives

Week	Main Topic	Objectives
1	Scientific Method, Measurement, Safety	Describe the components of the scientific method. Apply measurement techniques and safety protocols in laboratory settings.
2	Periodic Table Properties and Compound Nomenclature	Identify atomic structure and periodic trends. Write correct chemical formulas and names for compounds.
3	Moles, Chemical Compounds, and Reactions	Perform mole-to-gram conversions. Balance chemical equations and predict products.
4	Electron Configuration and Stoichiometry	Write electron configurations for atoms and ions. Apply stoichiometric relationships to chemical reactions.
5	VSEPR Theory, Molecular Shapes, and Chemical Bonding	Draw Lewis structures and predict molecular shapes. Explain intermolecular forces and their effects on physical properties.
6	Gas Laws and Solutions	Apply gas laws to solve problems involving pressure, volume, and temperature. Calculate solution concentrations and predict changes in solutions.
7	Acid-Base Titration and Introduction to Organic Chemistry	Identify and classify acids and bases. Perform acid-base titrations and calculate pH. Recognize basic organic functional groups.
8	Nuclear Chemistry and Introduction to Biochemistry	Describe types of radioactivity and nuclear reactions. Explain the effects of radiation and its applications. Identify biomolecules and their functions in living systems.
9	Comprehensive Review	Demonstrate understanding of all course components.
10	Reflection	Discuss the role of chemistry in health sciences and everyday life.

Key General Chemistry Topics

Atoms and Elements

Atoms are the fundamental units of matter, composed of protons, neutrons, and electrons. Elements are defined by their atomic number, which is the number of protons in the nucleus. The periodic table organizes elements by increasing atomic number and groups elements with similar chemical properties.

• Atomic Number (Z): Number of protons in the nucleus.

• Mass Number (A): Sum of protons and neutrons.

• Isotopes: Atoms of the same element with different numbers of neutrons.

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

Chemical Bonding

Chemical bonds are forces that hold atoms together in compounds. The main types are ionic, covalent, and metallic bonds. The Valence Shell Electron Pair Repulsion (VSEPR) theory predicts molecular shapes based on electron pair repulsion.

• Ionic Bonds: Formed by the transfer of electrons from one atom to another.

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

• Lewis Structures: Diagrams showing the arrangement of valence electrons.

• VSEPR Theory: Predicts the geometry of molecules based on electron pair repulsion.

Chemical Reactions and Stoichiometry

Chemical reactions involve the transformation of reactants into products. Stoichiometry is the quantitative relationship between reactants and products in a chemical reaction.

• Balancing Equations: Ensures the conservation of mass and atoms.

• Mole Concept: The mole is a unit for counting particles; $1 ext{ mole} = 6.022 imes 10^{23}$ particles.

• Stoichiometric Calculations: Use balanced equations to calculate amounts of reactants and products.

Gases and Gas Laws

Gases are described by pressure, volume, temperature, and amount. The gas laws relate these variables.

• Boyle's Law: $P_1V_1 = P_2V_2$ (at constant temperature)

• Charles's Law: $\frac{V_1}{T_1} = \frac{V_2}{T_2}$ (at constant pressure)

• Ideal Gas Law: $PV = nRT$

Solutions

Solutions are homogeneous mixtures of solute and solvent. Concentration is commonly expressed in molarity ($M$).

• Molarity: $M = \frac{\text{moles of solute}}{\text{liters of solution}}$

• Solubility: The ability of a substance to dissolve in a solvent.

Acids and Bases

Acids donate protons ($H^+$), while bases accept protons. The strength of acids and bases is measured by their dissociation in water.

• pH Scale: $pH = -\log[H^+]$

• Titration: A technique to determine the concentration of an acid or base using a neutralization reaction.

Nuclear Chemistry

Nuclear chemistry studies the changes in atomic nuclei, including radioactivity and nuclear reactions.

• Types of Radioactivity: Alpha ($\alpha$), beta ($\beta$), and gamma ($\gamma$) decay.

• Half-life: The time required for half of a radioactive sample to decay.

Organic and Biochemistry (Introduction)

Organic chemistry focuses on carbon-containing compounds, while biochemistry studies the chemical processes in living organisms.

• Hydrocarbons: Compounds containing only carbon and hydrogen.

• Functional Groups: Specific groups of atoms that determine the properties of organic molecules.

• Biomolecules: Carbohydrates, proteins, lipids, and nucleic acids.

Lab Techniques and Procedures

Measurement and Safety

• Use of personal protective equipment (PPE) in the laboratory.

• Accurate measurement of mass, volume, and temperature.

• Calculation of density and specific heat.

Chemical Analysis

• Performing titrations to determine concentration.

• Observing chemical reactions and recording data.

• Applying safety protocols to prevent accidents.

Grading Scale

Grade	Points Scale
A	4.0
A-	3.7
B+	3.3
B	3.0
B-	2.7
C+	2.3
C	2.0
D+	1.7
D	1.0
F	0.0

Additional Info

• Course includes both lecture and laboratory components.

• Assignments, quizzes, and exams are used to assess understanding.

• Attendance and participation are required for successful completion.

• Refer to the course syllabus for detailed policies and procedures.