Download Course Outline - Hicksville Public Schools

Mr. Hafiz Regents Chemistry Course Outline
I.
Introduction : lab safety; elements, compounds, mixtures; scientific
notation; density; significant figures; metric system; diatomic elements;
phases of matter; particle diagrams; physical and chemical changes
II.
Physical Behavior of Matter: forms of energy; law of conservation of matter
and energy; heat vs. temperature; Kelvin temperature scale; endothermic vs.
exothermic; heat and cooling curves; calorimetry; calculation of heart gained
and lost during phase changes; pressure, temperature and volume relating to
gases; barometer; manometers; Boyles Law; Charles Law; Gay Lusscac Law;
Combined Gas Law
III.
Atomic: atomic theory; sub-atomic particles; bright line spectrum; Dalton’s
Model; Rutherford’s Model; Thomson Model; Bohr Model; Electron Cloud
Quantum Mechanical Model; NYS electron configuration; electron dot
structures; weighted average atomic mass; isotopes
IV.
Bonding: Ionic, Covalent, Metallic bonding; electrolytes vs. non electrolytes;
intermolecular forces; electron dot structures
V.
Periodic Table: history; alkali metals; alkaline earth metals; halogens; nobles
gases; transition metals; metal, non-metals vs. metalloids; periodic trends of
ionization energy, electronegativity, atomic radius; size of atoms vs. their ions
VI.
Naming Compounds, Formula Writing, Types of Reactions and
Balancing Equations
VII.
Stoichiometry: mole concept; formula mass, gfm, molar volume, mole
conversions of mass/mole and mole/mass; determination of molecular formula
from empirical formula and molecular mass; Avogadro’s hypothesis; percent
composition; hydrate calculations
VIII. Solutions: factors affecting the rate and solubility; interpretation of solubility
curves; colligative properties; separation of mixtures including filtration,
distillation and chromatography
IX.
Kinetics and Equilibrium: molecular collision theory; factors affecting rates
of reactions; PE diagrams; enthalpy, entropy; types of equilibrium including
solution, phase, chemical; Le Chatelier’s Principle
X.
Nuclear: properties and notations of alpha, beta, gamma emissions;
writing nuclear equations; artificial vs. natural transmutation; half life
calculations; fission vs. fusion reactions; nuclear reactors; benefits and risks of
nuclear energy
XI.
Acids and Bases: operational definition vs. conceptual definition including
Arrhenius Theory, Bronsted Lowry Theory ; strengths of acids and bases; pH
scale; prediction of salts after neutralization reaction; titration calculations
including monohydroxy, dihydroxy bases and monoprotic, diprotic and
triprotic acids
XII.
Redox: determination of oxidation numbers; oxidation and reduction
reactions; writing balanced half reactions; voltaic/galvanic cells, electrolytic
cells
XIII. Organic: hydrocarbons including alkanes, alkenes and alkynes; functional
groups; drawing structural formulas given name; naming organic compounds
given structural formulas given IUPAC rules; identification of alcohols as
primary, secondary and tertiary