General Chemistry 1

Introduction to general concepts of chemistry: scientific method, periodic table, atomic theory, bonding, quantum theory, atomic structure, Lewis formulas, molecular geometry, VSEPR theory, molecular orbital theory.
Chapters
Concepts
Quizzes
Exercises
Exams
The scientific method is studied in this chapter: scientific notation, properties of matter, difference between intensive and extensive, metric system of units - SI base units, scientific measurement and uncertainty, difference between accuracy and precision, significant figures, calculated numerical results, dimensional analysis
Scientific Method and Notation The Properties of Matter States of Matter The International System of Units Scientific Measurement Uncertainty in Measurement Calculated Numerical Results Dimensional Analysis
Atoms are studied in this chapter: elements in chemistry, atomic theory, atomic structure, difference between isotopes and ions, cations vs. anions, chemical nomenclature of ions and acids
Atoms and Elements The Atomic Theory Atomic Structure Ions - Cations & Anions Naming Ions Naming Acids
The periodic table and chemical periodicity are studied in this chapter: law of constant composition, molecular and molar masses, difference between empirical and molecular formula, chemical reactions and how to balance a chemical equation, groups and periods in the periodic table and their properties.
Group Properties The Periodic Table Masses and Mole Number Average Atomic Mass The Mole
Early quantum theory is studied in this chapter: properties of waves, wave model of light, quantization of energy, photons and photoelectric effect, atomic line spectra, electronic transition, the line spectrum of hydrogen, Rydberg-Balmer equation, wave-particle duality
Wave Model of Light Photons and Photoelectric Effect Wave-Particle Duality Atomic Line Spectra The Line Spectrum of Hydrogen
Quantum theory and atomic structure are studied in this chapter: Heisenberg uncertainty principle, Schrödinger equation, quantum numbers, electron spin, energies of atomic orbitals and electron configuration, Pauli exclusion principle, Hund’s rule, excited states, core vs. valence electrons
Quantum Theory Quantum Numbers Electron Spin Electronic Structure Principles Arrangement of Electrons Excited States Core vs. Valence Electrons
Periodic trends of the elements are studied in this chapter: effective nuclear charge, periodicity of atomic radius, ionization energy and electron affinity, electron configuration of ions, sizes of ions, isoelectronic series
Periodicity in Properties of Elements Electron Configuration of Ions Sizes of Ions Effective Nuclear Charge
Ionic and covalent compounds are studied in this chapter: difference types of bonding, ionic compounds and their chemical formula, empirical vs. molecular formula, the law of constant composition, naming binary compounds, ionic bond energies
Naming Binary Compounds The Law of Constant Composition Empirical vs. Molecular Formula Types of Bonding Ionic Compounds Ionic Bond Energies Covalent Compounds
The representation of molecules is studied in this chapter: Lewis structures, formal charges, resonance hybrids, electronegativity and polarity, dipole moment and percent ionic character, expanded valence shells
Lewis Structures Formal Charge Resonance Forms Exceptions to the Octet Rule Electronegativity & Polarity Dipole Moment & Percent Ionic Character The Octet Rule
Molecular geometries are studied in this chapter: VSEPR theory, VSEPR notation, lone pair effect, electron-domain geometry vs. molecular geometry, prediction of molecular geometry, deviation from ideal bond angles, polarity of molecules, isomers
VSEPR Theory Lone Pair Effect Prediction of Molecular Geometry Deviation from Ideal Bond Angles Molecular Geometry and Polarity Isomers
The covalent bonding is studied in this chapter: valence bond theory, molecular orbital theory, multiple bonds, hybridization and hybrid orbitals, molecular orbital diagrams.
Valence Bond Theory Multiple Bonds and Hybridization Hybrid Orbitals Molecular Orbital Theory Molecular Orbital Diagrams
Midterm 1 includes 6 questions and it covers Chapters 1, 2 and 3 of General Chemistry 1. At the end of the test you can see the answers and determine whether you have solved the questions. You have 1 hour to resolve Midterm 1.
Questions
60 Minutes
Midterm 2 includes 5 questions and it covers chapters 1 to 6 of General Chemistry 1 (mainly chapters 4, 5 and 6). At the end of the test you can see the answers and determine whether you have solved the questions. You have 1 hour to resolve Midterm 2.
Questions
60 Minutes
Final Exam includes 10 questions and it covers all chapters of General Chemistry 1. At the end of the test you can see the answers and determine whether you have solved the questions. You have 2 hours to resolve Final Exam.
Questions
120 Minutes