
Chemistry
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Atomic and Molecular Structure
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The periodic table
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Experimental basis for Thomson’s discovery of the electron
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Rutherford’s nuclear atom
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illikan’s oil drop experiment
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Einstein’s explanation of the photoelectric effect
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Planck’s relationship
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Chemical Bonds
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Biological, chemical, and physical properties of matter
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Electronegativity and ionization energy
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Van der Waals forces
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Conservation of Matter and Stoichiometry
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Conservation of atoms in chemical reactions
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Balanced equations
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Gases and Their Properties
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Kinetic molecular theory
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Diffusion of gases
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Gas laws, relations between the pressure, temperature, and volume
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Standard temperature and pressure (STP)
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Dalton’s law of partial pressures
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Acids and Bases
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Acids, bases, and salts are three classes of compounds that form ions
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pH scale to characterize acid and base solutions
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Buffers stabilize pH in acid–base reactions
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Solutions
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Homogeneous mixtures of two or more substances
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Definitions of solute and solvent
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Concentration of a solute in grams per liter, molarity, ppm and percent composition
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Molality of a solute in a solution and depressed freezing or elevated boiling point
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Solution separation or purification by chromatography and distillation
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Chemical Thermodynamics
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Energy exchange or transform in all chemical reactions and physical changes of matter
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Release Exothermic or absorb Endothermic thermal energy
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Hess’s law to calculate enthalpy change
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Gibbs free energy equation
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Reaction Rates
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Chemical reaction rates factors influence the frequency of collision of reactant molecules
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Role of a catalyst
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Role of activation energy
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Chemical Equilibrium
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Le Chatelier’s principle
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Organic Chemistry and Biochemistry
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Large molecules (polymers), such as proteins, nucleic acids, and starch
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Hydrocarbons to complex polymers and biological molecules
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Amino acids are the building blocks of proteins
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Nuclear Processes
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Change in mass in E=mc2 significant in nuclear reactions