Chemical Laboratory Techniques
-utilization of metric measurement: including dimensional analysis, significant figures, accuracy and precision, percent error. (lab)
-identification of substances through determination of physical/chemical properties
-separation of substances according to physical properties (lab)
-organization of gathered data through charts and graphs
General Chemistry Knowledge
-apply vocabulary necessary to communicate general chemistry
-define, identify, and give examples of chemical vs physical change or property.
-recognize symbols, elemental nomenclature, and equation expression
-identify and organize the various components of matter into a logical order
-explain the Law of Conservation of Matter and Energy relating to a reaction.(lab)
-explain the current model an atom /subatomic particles;
relative mass, charge, and position.
-describe the forces that enable the atom to maintain it's integrity.
-describe the contributions of previous scientists to the development of the current theory of the atom: Dalton, Bohr, Rutheford, de Broglie and Heisenberg.
-describe neutral atoms in terms of atomic number, atomic mass, electron configuration, atomic orbitals, electric potential, atomic radius, and placement on
the periodic table. (computer lab)
-define and describe isotopes in terms of atomic mass and atomic number.
-contrast ionic and covalent compounds in terms of valancey,
-utilize qualitative analysis to determine the composition of a compound.
-write a balanced formula; use the correct nomenclature for compounds.
-identify types of reactions concentrating on predicting types of products formed .
-write a balanced equation for a reaction (Stoichiometry).
-recognize the mole and its equivalents as the measurement
-express moles as representative particles, volume at STP, and molar mass.
-apply quantitative analysis in equations and laboratory experience.
States of Matter
-describe the states of matter with regard to internal organization
-utilize the Gas Laws to determine the effect of change on the states of matter.
-describe the various bonds required to form compounds with respect to valencey.
-covalent bonds: hybridization, octet rule, polar vs non polar bonds
-ionic bonds: crystalline formation, shape relating to coordination number
-special cases: metallic bonds, hydrogen bonds, van der Waals forces.
Chemistry of Solutions
-define and describe solutions in terms of particle size
-describe solutions in terms of: electrolytic potential.
-interpret and calculate molarity and molality.
-account for factors that affect the rate of solubility of a substance in solution.
-define and determine the rate of reaction for a chemical
-utilize the Keq, Ka, Kb, Ksp to determine product formation in reaction.
-describe the affects of catalysts, changes in pressure/temperatureon the rate
-calculate the entropy within a reaction.
Acid Base Chemistry
-compare and contrast the Arrhenius, Lewis, or Bronsted-Lowery
concept of an
acid and base.
-determine the strength of an acid or base utilizing pH, Ka, Kb.
-calculate titration curves to determine the equivalency point of an
acid/ base reaction.
-define and identify oxidation-reduction reactions in terms
of electron transfer.
-write balanced equations for a oxidation-reduction reaction
-describe the applications of Oxidation-Reduction reactions in electrochemistry.
-express and calculate mathematically the disintegration
of radioactive isotopes.
-express the types of radiation in terms of composition, symbol, charge, and mass.
-define and calculate the half-life of a radioisotope, state applications of half-life.
-compare and contrast nuclear fission and nuclear fusion.
-Identify and name organic compound by chains, bond type,
and functional groups.
-describe the phenomena of isomerism and stereoisomerism.
-compare and contrast straight chain hydrocarbons to aromatic hydrocarbons.
-identify types of reactions in organic chemistry and predict products.
-molecules of importance to industry and biochemistry.
Assessment: Laboratory experiences will gently move the
student from contrived labs
to authentic laboratory experiences where students will be responsible for generating laboratory procedures to solve problems in the chemistry field. Students must be able to communicate their laboratory findings, as well
as, general chemistry knowledge both in oral and written form. Formal testing will also be done as students pass important benchmarks in the curriculum.