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RE Chemistry SyllabusArdsley High School - 2005-2006CONTENTSUNIT 1 MEASUREMENT Scientific method, controlled experiment Making a graph Scientific notation International System of Units: Base units, Derived units, SI prefixes Uncertainty in measurement: Accuracy versus precision, significant figures Calculations: Percentage error, density Converting between units using ratio and proportion, Problem Solving Short introduction to the periodic table Reference Tables C, D, T and the periodic table
UNIT 2 MATTER AND ENERGYTypes of matter: elements, compounds, and mixtures, particle diagrams Properties of Matter: Physical and chemical properties, intensive and extensive properties Physical and chemical changes Laws: Conservation of Mass, Definite proportion, Conservation of Energy Phases of matter: solid, liquids and gases Forms of energy, heat, temperature and the different temperature scales Phase changes, Heat of vaporization, Heat of fusion, the Heating, and the Cooling curve Endothermic and exothermic changes, introduction to potential energy diagrams, activation energy Calorimeter problems Separation of mixtures: distillation, filtration, chromatography Reference Tables B, I, S and T
UNIT 3 ATOMIC STRUCTUREModels of the atom: Dalton, J.J. Thomson, Rutherford, Bohr and the Present day model Protons, neutrons, and electrons Atomic number, Mass number, isotopes, weighted average mass The Nature of light: wavelength, frequency and the speed of light Electromagnetic Radiation, Continuous spectrum and bright line spectrum Electron configurations, valance electrons, the ground state and the excited state, electron configuration of ions Lewis dot diagrams Reference Table O and the periodic table
UNIT 4 NUCLEAR CHEMISTRYBelt of Stability, n/p ratio Types of radiation, natural radioactivity, nuclear equations, artificial transmutation, nuclear fission and nuclear fusion, half life questions, radioactive waste, uses and dangers of radioisotopes, nuclear reactors Reference Tables N, O and the periodic table
UNIT 5 THE PERIODIC TABLEStructure of the Periodic Table: Groups, periods, and blocks Metals, nonmetals, and metalloids, transition elements Names and properties of the groups: alkali metals, alkaline earth metals, halogens and noble gases Allotropes Properties of the elements: atomic radius, ionic radius, metallic character, ionization energy, electronegativity, and reactivity Trends in the periodic table Isoelectronic series Reference Table S and the periodic table
UNIT 6 BONDINGReasons for chemical bonding, the nature of chemical bonds, energy changes associated with chemical bonding Types of bonds between atoms: ionic, covalent, metallic Dot diagrams and Lewis structures Properties of ionic crystals, properties of molecular compounds, properties of metals The shapes of molecules and the VSEPR theory Polar and nonpolar molecules Molecular attraction: dipole – dipole attractions, Hydrogen bonds, London dispersion forces, molecule – ion attractions Reference Table S, I and the periodic table
UNIT 7 FORMULAS AND EQUATIONS Chemical formulas: empirical and molecular formulas Nomenclature: ionic and covalent compounds, the traditional method, and the stock system Chemical equations: word equation, formula equations, balancing equations The five types of chemical reactions, predicting if a chemical reactions will occur or not, finding the products of a single replacement reaction, and of a double replacement reaction The driving force of a double replacement reaction Reference Tables E, F, J, S and the periodic table
UNIT 8 ORGANIC CHEMISTRY Organic compounds: properties, bonding, molecular formulas, structural formulas, condensed structural formulas and isomers, Homologous series of hydrocarbons: alkanes, alkenes, alkynes Functional groups: halides, alcohols, organic acids, aldehydes, ketones, ethers, esters, amines and amides Naming organic compounds: IUPAC system and common names Organic reactions: combustion, substitution, addition, esterification, and saponification, Polymers: natural and synthetic, addition and condensation polymerization Reference Tables P, Q, R and the periodic table
UNIT 9 THE MATHEMATICS OF CHEMISTRYFormula mass, gram formula mass, moles, number of particles Converting between moles and grams Problems involving formulas: percentage composition, percent water in a hydrate, finding the empirical formula and the molecular formula Problems involving equations: moles to moles, limiting reactant problems using particle diagrams Reference Table T and the periodic table
UNIT 10 GASES Pressure: meaning, how it is measured, units The Kinetic Molecular Theory, average kinetic energy The gas laws: Boyles Law, Charles Law, Gay-Lussac’s law and Combined gas Law Avogadro’s hypothesis How are pressure and the number of gas particles related? How is temperature and the velocity of a gas related? Ideal gases and nonideal gases Reference Tables A, T and the periodic table
UNIT 11 SOLUTIONSProperties of solutions, Solubility factors, solubility curves, solution equilibrium Saturated, unsaturated, and supersaturated solutions, dilute and concentrated solutions Ways of expressing solution concentration: Molarity, Percent by Mass, Percent by Volume, Parts per Million Colligative Properties: Boiling point elevation, freezing point depression, molecular verses ionic Phase equilibrium and equilibrium vapor pressure, boiling point Reference Tables G, H, T and the periodic table
UNIT 12 KINETICS AND EQUILIBRIUMKinetics: factors that affect reaction rates Potential energy diagrams How to use Table I Equilibrium: Types of equilibrium: solution, phase, chemical Le Chatelier’s principles, the common ion effect, Law of chemical equilibrium, finding the value of the equilibrium constant Entropy Reference Table I and the periodic table
UNIT 13 ACIDS AND BASES Electrolytes, Operational and conceptual definitions, Arrhenius theory, alternate acid- base theory Reactions involving acids and bases: reactions of acids with metals, neutralizations reactions pH scale, acid - base indicators Acid – Base titration Reference Tables J, K, L, M and the periodic table
UNIT 14 REDOX AND ELECTROCHEMISTRY Oxidation numbers, identifying oxidation and reduction, half reactions Recognizing redox reactions Oxidizing agents and reducing agents Electrochemistry: types of electrochemical Cells: Galvanic (voltaic) cells, Electrolytic Cells Electrolysis, electroplating, balancing simple redox reactions Reference Table J and the periodic table |
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Created by Karen Tutnauer" |