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 and conversions are studied in this chapter: scientific notation, metric system of units, difference between intensive/extensive and between accuracy/precision, significant figures, calculated numerical results and dimensional analysis.
Scientific Notation The Metric System of Units and Standards Intensive vs. Extensive Properties Energy and Power in Chemistry Accuracy vs. Precision Number of Significant Figures Calculated Numerical Results Dimensional Analysis
Atoms and molecules are studied in this chapter: elements in chemistry, states of matter, atomic theory, difference between atoms, isotopes and ions, chemical nomenclature of compounds.
Elements in Chemistry States of Matter The Atomic Theory Atoms Isotopes Ions Polyatomic Ions Naming Chemical Nomenclature Acids Naming
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.
The Law of Constant Composition Empirical vs. Molecular Formulas Chemical Reactions Balancing Chemical Equations Group Properties Periods Mass, Mole and Avogrado's Number
Early quantum theory is studied in this chapter: ionization energies, wave model of light, photons and photoelectric effect, wave-particle duality, quantization of the energy of the electron in a hydrogen atom and electronic transitions.
First Ionization Energies Ionization Energy and Periodicity Wave Model of Light Photons and Photoelectric Effect Wave-Particle Duality Quantization Electronic Transitions
Quantum theory and atomic structure are studied in this chapter: Heisenberg uncertainty principle, Schrödinger equation, quantum numbers, electron spin, atomic energy states and electron configuration, Pauli exclusion principle, Hund’s rule, excited states, periodicity of atomic radii, ionization energy and electron affinity.
Quantum Theory Azimuthal Quantum Number Magnetic Quantum Number Electron Spin Atomic Energy States Pauli Exclusion Principle Electron Configuration Hund’s Rule Excited States Atomic Radii, Ionization Energies and Periodicity
Ionic bonds and compounds are studied in this chapter: the difference between ionic and covalent bonds, the ionic charges and chemical formulas, the transition metal ions, the sizes of ions, the ionic bond energies.
Ionic and Covalent Bonds Ionic Charges and Chemical Formulas Transition Metal Ions Sizes of Ions Ionic Bond Energies
Covalent bonds and Lewis formulas are studied in this chapter: electron sharing, Lewis structures, formal charges, resonance hybrids, free radicals, expanded valence shells, electronegativity, polar bonds and dipole moments.
Covalent Bonds Lewis Structures Formal Charges Resonance Hybrids Free Radicals Expanded Valence Shells Electronegativity Bond Energies Polar Bonds & Dipole Moments
Molecular geometries are studied in this chapter: molecular shape, VSEPR theory and prediction of molecular geometry, lone pair effects, the relation between structure and dipole moment, optical isomers and chirality.
Molecular Shape VSEPR Theory VSEPR and Prediction of Molecular Geometry Lone Pair Effects Structure and Dipole Moment Isomers and Chirality
The covalent bonding is studied in this chapter: valence bond theory, molecular orbital theory, multiple bonds, hybridization and hybrid orbitals, molecular orbital diagrams.
Theories for Bond Formation and Structure 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