Science, Grade 9 - 12, Chemistry, 2005
1.) Differentiate among pure substances, mixtures, elements, and compounds.
• Distinguishing between intensive and extensive properties of matter
• Contrasting properties of metals, nonmetals, and metalloids
• Distinguishing between homogeneous and heterogeneous forms of matter
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2.) Describe the structure of carbon chains, branched chains, and rings.
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3.) Use the periodic table to identify periodic trends, including atomic radii, ionization energy, electronegativity, and energy levels.
• Utilizing electron configurations, Lewis dot structures, and orbital notations to write chemical formulas
• Calculating the number of protons, neutrons, and electrons in an isotope
• Utilizing benchmark discoveries to describe the historical development of atomic structure, including photoelectric effect, absorption, and emission spectra of elements
Example: Thompson's cathode ray, Rutherford's gold foil, Millikan's oil drop, and Bohr's bright line spectra experiments
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4.) Describe solubility in terms of energy changes associated with the solution process.
• Using solubility curves to interpret saturation levels
• Explaining the conductivity of electrolytic solutions
• Describing acids and bases in terms of strength, concentration, pH, and neutralization reactions
• Describing factors that affect the rate of solution
• Solving problems involving molarity, including solution preparation and dilution
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5.) Use the kinetic theory to explain states of matter, phase changes, solubility, and chemical reactions.
Example: water at 25 degrees Celsius remains in the liquid state because of the strong attraction between water molecules while kinetic energy allows the sliding of molecules past one another
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6.) Solve stoichiometric problems involving relationships among the number of particles, moles, and masses of reactants and products in a chemical reaction.
• Predicting ionic and covalent bond types and products given known reactants
• Assigning oxidation numbers for individual atoms of monatomic and polyatomic ions
• Identifying the nomenclature of ionic compounds, binary compounds, and acids
• Classifying chemical reactions as composition, decomposition, single replacement, or double replacement
• Determining the empirical or molecular formula for a compound using percent composition data
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7.) Explain the behavior of ideal gases in terms of pressure, volume, temperature, and number of particles using Charles's law, Boyle's law, Gay-Lussac's law, the combined gas law, and the ideal gas law.
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8.) Distinguish among endothermic and exothermic physical and chemical changes.
Examples:
- endothermic physical—phase change from ice to water,
- endothermic chemical—reaction between citric acid solution and baking soda,
- exothermic physical—phase change from water vapor to water,
- exothermic chemical—formation of water from combustion of hydrogen and oxygen
• Calculating temperature change by using specific heat
• Using Le Châtelier's principle to explain changes in physical and chemical equilibrium
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9.) Distinguish between chemical and nuclear reactions.
• Identifying atomic and subatomic particles, including mesons, quarks, tachyons, and baryons
• Calculating the half-life of selective radioactive isotopes
• Identifying types of radiation and their properties
• Contrasting fission and fusion
• Describing carbon-14 decay as a dating method
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