Introduction to chemistry (Chapter 1)
- What is chemistry
- Problem solving – scientific method
- Matter as particles
- Elements, compounds, atoms, and molecules
- Physical properties – physical changes
- Chemical properties – chemical changes
- Mixtures and pure substances
- Separation of mixtures
- Scientific notation
- Units
- Length, volume, and mass
- Uncertainty and significant figures
- Dimensional analysis
- Density
- Representing the elements
- Lavoisier – Law of conservationof mass
- Proust and Gay-Lussac – Law of constant composition
- Dalton and atomic theory
- Using formulas to represent compounds
- Thomson – electrons
- Rutherford - nucleus
- Isotopes
- The periodic table
- Ions
- Energy and light
- Atomic emission spectra
- The Bohr atom
- Schrodinger – the wave model of the atom
- Electron configuration
- Periodicity
- Ionic compounds
- Molecular compounds
- Acids
- Counting by weighing
- Atomic masses
- The mole
- Molar mass
- Percent composition
- Empirical and molecular formulas
- Evidence
- Equations
- Balancing
- Precipitate reactions
- Acid/base reactions
- Oxidation/reduction reactions
- Synthesis
- Decomposition
- Combustion
- Mole more relationships
- Mass calculations
- Limiting reactants
- Percent yield
- The nature of energy
- Temperature vs heat
- Exothermic and endothermic reactions
- Thermodynamics
- Calorimetry
- Hess’s law
- Energy as a driving force
- Pressure
- Boyle’s law - P * V
- Charles Law - V / T
- Gay-Lussac’s Law – P / T
- Ideal gas law
- Dalton’s law of partial pressures
- Kinetic molecular theory
- Real gases
- Gas stoichiometry
- Types of chemical bonds – ionic vs molecular
- Electronegativity
- Polarity
- Lewis structures
- VSEPR - molecular structure and geometry