Solutions
- Concepts of solutions
- Concentration of a solution
- Chromatography and distillation
- Concentration of ions in a solution
- Factors that influence solubility
- General rules for solubility; types of solutions
- Ionic and covalent compounds
Conservation of Matter and Stoichiometry
- Conservation of mass, energy, and charge
- Types of chemical reactions
- Moles; volume of gas at STP
- Properties of mixtures/pure substances
- Changes in matter
- Energy transformations/exchanges involved in chemical reactions
- Thermal energy - random motion of atoms and molecules
- Temperature - average kinetic energy of the particles
- Physical/chemical change
- Exothermic/endothermic reactions
- Intermolecular forces - hydrogen bonding
- Physical properties of substances
- Verify the law of conservation of energy
- Activation energy in a chemical reaction
- Forward/reverse reactions
- Catalyzed/uncatalyzed reaction
- Entropy
Oxidation and Reduction
- Balancing reactions
- Corrosion; electroplating
- Voltaic/electrolytic cells; electrolysis
Atomic and Molecular Structure
- Properties of subatomic particles
- Stable/unstable isotopes
- Periodic table; physical characteristics of an element
- Periodic table; chemical characteristics of an element
- Periodic table - elements
- Periodic table - elements; trends in ionization energy
- Periodic table- number of electrons available for bonding
- Nucleus of an atom- mass, size etc.
- Periodic table- elements; nuclear accelerators
- Quantum electron configuration - reactivity with other elements
- Thomson’s discovery of the electron
- Rutherford’s nuclear atom
- Millikan’s oil drop experiment
- Einstein's explanation of the photoelectric effect
- Bohr model of the atom
- Spectral lines
- Planck's relationship
Chemical Equations
- Elements/compounds - scientific nomenclature
- Chemical and nuclear reactions
- Balancing equations
Gases and Their Properties
- Kinetic Molecular Theory; Collision Theory
- Gas laws
- Standard temperature and pressure (STP)
- Celsius/Kelvin temperature
- Dalton’s law of partial pressures (composition of gases)
- Graham’s law (diffusion of gases)
- Universal Gas Law
- Kinetic/potential energy to explain properties
Chemical Bonding
- Characteristics of atoms involved in chemical bonding
- Influence of intermolecular forces
- Arrangement of atoms in substances
- Electrostatic attraction
- Lewis dot structures
- Degree of polarity; ionization energy
- van der Waals forces/hydrogen bonding
- Chemical bonds
- Molecular polarity
Nuclear Processes
- Ionizing/penetrating power
- Protons and neutrons
- Transmutation; spontaneous decay; nuclear reactions
- Substructures – quarks
- Equations to represent nuclear reactions
- Radioactive elements - half-life
Acids, Bases and Salts
- Acids, bases, and salt solutions; neutralization reactions
- Effects of acids and bases on an ecological system
- pH value/scale
- Arrhenius, Bronsted-Lowry, and Lewis acid–base definitions
- Calculate pH from the hydrogen-ion concentration
- Stabilizing pH in acid–base reactions
- Titration
- Rate of a chemical reaction
Chemical Thermodynamics
- Exothermic/endothermic thermal energy
- Problems involving heat flow/temperature changes
- Specific/latent heat
- Hess’s law to calculate enthalpy change
- Gibbs free energy equation
- Le Chatelier’s principle
Chemical Equilibrium
- Forward/reverse reaction rates
- Equilibrium constant
- Potential energy diagram
- Organic compounds
- saturated/unsaturated hydrocarbons
Organic Chemistry and Biochemistry
- Functional groups
- Formation of large molecules
- Bonding characteristics of carbon
- Amino acids - building blocks of proteins
- Simple linear hydrocarbons/isomers
- Isomers of organic compounds
- R-group structure of amino acids
- Organic reactions
- Structural formulas
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