CHEM 1201 General Chemistry I Syllabus and Chapter Overview

CHEM 1201 General Chemistry I: Syllabus Overview

Course Description

This course provides a comprehensive introduction to the fundamental principles of chemistry, including chemical theory, quantitative approaches, and problem-solving strategies. It is designed for students pursuing science and engineering majors and covers essential topics in general chemistry.

Integrated Learning Core Statement

• Emphasizes scientific reasoning, quantitative skills, and the application of chemical principles to real-world problems.

• Develops critical thinking and analytical skills through laboratory and lecture components.

Chapter Breakdown and Key Topics

Chapter 1: Introduction: Matter and Measurement

This chapter introduces the basic concepts of matter, energy, and the methods used to measure chemical quantities.

• Matter and Its Properties: Definition of matter, states of matter (solid, liquid, gas), and physical vs. chemical properties.

• Units of Measurement: SI units, conversion factors, and dimensional analysis.

• Uncertainty in Measurement: Significant figures and accuracy vs. precision.

• Example: Calculating the density of a substance using mass and volume measurements.

Chapter 2: Atoms, Molecules, and Ions

This chapter explores the structure of atoms, the formation of molecules and ions, and the basics of chemical nomenclature.

• Atomic Theory: Historical development, subatomic particles (protons, neutrons, electrons).

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

• Molecules and Ions: Formation of covalent and ionic compounds.

• Chemical Formulas: Empirical and molecular formulas.

• Naming Compounds: Rules for naming ionic and molecular compounds.

• Example: Writing the formula for sodium chloride and naming H2O as water.

Chapter 3: Chemical Reactions and Stoichiometry

This chapter covers the representation of chemical reactions, balancing equations, and quantitative relationships in reactions.

• Chemical Equations: Reactants, products, and the law of conservation of mass.

• Balancing Equations: Ensuring equal numbers of atoms on both sides.

• Stoichiometry: Calculating amounts of reactants and products using mole ratios.

• Limiting Reactant: The reactant that determines the amount of product formed.

• Percent Yield: $\text{Percent Yield} = \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \times 100\%$

• Example: Determining the limiting reactant in a reaction between hydrogen and oxygen.

Chapter 4: Reactions in Aqueous Solution

This chapter focuses on the behavior of substances in water, types of reactions, and solution stoichiometry.

• Electrolytes and Nonelectrolytes: Substances that conduct electricity in solution.

• Types of Reactions: Precipitation, acid-base, and redox reactions.

• Net Ionic Equations: Showing only the species that participate in the reaction.

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

• Example: Writing the net ionic equation for the reaction between NaCl and AgNO3.

Chapter 5: Thermochemistry

This chapter introduces the study of energy changes in chemical reactions, including heat, work, and enthalpy.

• Energy and Work: Definitions and units.

• First Law of Thermodynamics: $\Delta E = q + w$ (change in internal energy equals heat plus work)

• Enthalpy: $\Delta H$ as the heat change at constant pressure.

• Calorimetry: Measuring heat changes in reactions.

• Example: Calculating the enthalpy change for the combustion of methane.

Chapter 6: Electronic Structure of Atoms

This chapter examines the arrangement of electrons in atoms and the principles governing their behavior.

• Electromagnetic Radiation: Relationship between wavelength, frequency, and energy ($E = h\nu$).

• Quantum Numbers: Describe electron energy levels and orbitals.

• Electron Configurations: Aufbau principle, Pauli exclusion principle, Hund's rule.

• Example: Writing the electron configuration for oxygen: 1s2 2s2 2p4.

Chapter 7: Periodic Properties of the Elements

This chapter explores trends in the periodic table, including atomic size, ionization energy, and electron affinity.

• Periodic Law: Properties of elements are periodic functions of their atomic numbers.

• Trends: Atomic radius, ionization energy, electron affinity, metallic character.

• Example: Comparing the atomic radius of sodium and chlorine.

Chapter 8: Basic Concepts of Chemical Bonding

This chapter discusses the types of chemical bonds, Lewis structures, and bond polarity.

• Ionic and Covalent Bonds: Transfer vs. sharing of electrons.

• Lewis Structures: Representation of molecules showing valence electrons.

• Bond Polarity: Electronegativity differences and dipole moments.

• Example: Drawing the Lewis structure for CO2.

Chapter 9: Molecular Geometry and Bonding Theories

This chapter covers the shapes of molecules and theories explaining chemical bonding.

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

• Hybridization: Mixing of atomic orbitals to form new hybrid orbitals.

• Molecular Polarity: Determined by shape and bond polarity.

• Example: Predicting the geometry of methane (CH4) as tetrahedral.

Chapter 10: Gases

This chapter introduces the properties of gases and the laws governing their behavior.

• Gas Laws: Boyle's Law ($P_1V_1 = P_2V_2$), Charles's Law ($\frac{V_1}{T_1} = \frac{V_2}{T_2}$), Ideal Gas Law ($PV = nRT$).

• Kinetic Molecular Theory: Explains the behavior of gases at the molecular level.

• Example: Calculating the pressure exerted by a gas in a container.

Chapter 11: Liquids and Intermolecular Forces

This chapter examines the properties of liquids and the forces that hold molecules together.

• Intermolecular Forces: London dispersion, dipole-dipole, hydrogen bonding.

• Properties of Liquids: Viscosity, surface tension, vapor pressure.

• Phase Changes: Melting, boiling, condensation.

• Example: Explaining why water has a high boiling point due to hydrogen bonding.

Chapter 12: Solids and Modern Materials

This chapter (time permitting) covers the structure and properties of solids and introduces modern materials.

• Types of Solids: Ionic, covalent, metallic, molecular.

• Crystal Structures: Arrangement of particles in solids.

• Example: Describing the structure of sodium chloride as a crystalline solid.

Chapter 13: Properties of Solutions

This chapter (time permitting) discusses the formation and properties of solutions.

• Solubility: Factors affecting the ability of substances to dissolve.

• Concentration Units: Molarity, molality, percent composition.

• Colligative Properties: Effects of solute particles on boiling point, freezing point, and osmotic pressure.

• Example: Calculating the boiling point elevation of a salt solution.

Grading Scheme

Course Component	Points
Exams	800
ALEKS Homework	100
Quizzes	100
Total	1000

Letter grades are assigned based on the percentage of total points earned.

Additional Info

• Students are encouraged to utilize tutoring resources and supplemental instruction for academic success.

• Attendance, participation, and completion of assignments are essential for mastering course material.

• Refer to the official syllabus for detailed policies on exams, grading, and academic integrity.