Chemistry
Welcome
Structured Learning Approach
1
Essentials
1.1
Phases and Classification of Matter
1.2
Physical and Chemical Properties
1.3
Measurements
1.3.1
Volume and Density
1.4
Uncertainty, Accuracy, and Precision
1.4.1
Significant Figures
1.4.2
Significant Figures in Calculations
1.4.3
Rounding Rules
1.4.4
Accuracy and Precision
1.5
Mathematical Treatment of Measurement Results
1.6
Temperature
1.7
Practice Exam Problems
1.8
Practice Problems
2
Atoms, Molecules, and Ions
2.1
Evolution of Atomic Theory
2.1.1
Dalton’s Atomic Theory
2.1.2
Thomson
2.1.3
Millikan
2.1.4
Rutherford
2.2
Subatomic Particles
2.3
Atomic Symbolism
2.3.1
Isotopes
2.4
Average Atomic Mass
2.5
Covalent Bonding and Molecules
2.5.1
Molecular Formulas
2.6
The Mole
2.6.1
Conversions
2.7
Practice Problems
3
Electronic Structure and Periodic Properties
3.1
Energy
3.2
Electromagnetic radiation
3.2.1
Wave
3.2.2
Quantum Theory
3.2.3
Energy and Light
3.3
Atomic Line Spectra
3.3.1
Rydberg equation
3.3.2
Wave properites of matter
3.4
Heisenberg uncertainty principle
3.5
Schrodinger Equation
3.6
Quantum numbers
3.7
Pauli Exclusion principle
3.8
Aufbau Principle
3.9
Orbital Diagrams
3.10
Electron Configurations neutral/ions
3.11
Hund’s Rule
3.12
Core/Valence electrons
3.13
Periodic trends
3.13.1
Radii
3.13.2
Ionization energies
3.13.3
Electron Affinities
3.14
Periodic Table
3.14.1
Group Names
3.15
Ionic and Molecular Compounds
3.15.1
Polyatomic ions
3.15.2
Monatomic ions
3.15.3
Ionic bonds and covalent bonds
3.16
Practice Problems
4
Bonding and Molecular Geometry
4.1
Chemical Bonding and Molecular Geometry
4.2
Ionic Bonding
4.2.1
Electron configuration ions
4.3
Covalent bonding
4.3.1
Pure vs polar covalent bond (electronegativity difference)
4.3.2
Electronegativity
4.4
Nomenclature
4.4.1
Ionic compounds
4.4.2
Covalent (Molecular) Compounds
4.4.3
Binary acids
4.4.4
Oxyacids
4.5
Lewis Structures
4.5.1
Octet Rule
4.5.2
Electron-deficient
4.5.3
Hypervalent
4.5.4
Formal Charge
4.5.5
Resonance
4.5.6
VSEPR
4.5.7
Molecular Polarity
4.6
Practice Problems
5
Advanced Bonding Theories
5.1
Practice Problems
6
Composition of Substances and Solutions
6.1
Practice Problems
7
Stoichiometry
7.1
Practice Problems
8
Thermochemistry
8.1
Practice Problems
9
Gases
9.1
Practice Problems
Appendix
A
Symbols, Notation, and Units
A.1
Base SI Units
A.2
Derived SI Units
A.3
Metric Prefixes
A.4
Gas Constants
B
Mathematical Functions
B.1
Polynomials
B.2
Exponentials
B.3
Logarithms
C
SI Units and Conversions
D
Useful Resources
E
Periodic Table
E.1
Categories
E.1.1
Block
E.1.2
Classification
E.1.3
Phase
E.1.4
Gas Phase Type
E.1.5
Magnetic Type
E.1.6
Electrical Type
E.1.7
Decay Mode
E.2
Properties
E.2.1
Atomic Radius
E.2.2
Boiling Point
E.2.3
Density
E.2.4
Electron Affinity
E.2.5
Electronegativity
E.2.6
Half-life
E.2.7
Heat of Fusion
E.2.8
Heat of Vaporization
E.2.9
Ionic Radius (Effective)
E.2.10
Ionization Energy (First)
E.2.11
Ionization Energy (Second)
E.2.12
Ionization Energy (Third)
E.2.13
Melting Point
E.2.14
Percent in Earth’s Crust
E.2.15
Percent in Humans
E.2.16
Percent in Meteorites
E.2.17
Percent in Oceans
E.2.18
Percent in Sun
E.2.19
Percent in Universe
E.2.20
Specific Heat
E.2.21
Thermal Conductivity
E.2.22
Van der Waals Radius
F
Standard State of Elements
G
Standard Thermodynamic Values for Select Substances
H
Standard Reduction Potentials (by name)
I
Standard Reduction Potentials (by potential)
Eric Van Dornshuld, PhD
Chemistry I
4.3
Covalent bonding
4.3.1
Pure vs polar covalent bond (electronegativity difference)
4.3.2
Electronegativity