MADISON ACADEMY CHEMISTRY AND HONORS CHEMISTRY SCIENCE PACING GUIDE QUARTER 1 VOCABULARY

Transcription

1 CHEMISTRY AND HONORS CHEMISTRY SCIENCE PACING GUIDE QUARTER 1 VOCABULARY Chemistry Substance Mass Weight Model Scientific Method Hypothesis Observation Qualitative Data Quantitative Data Control Independent Variable Dependent Variable Theory Scientific Law SI Units Base Unit Second (s) Meter (m) Kelvin Temperature Scale (K) Absolute Zero Fahrenheit Celcius Kilogram (kg) Derived Unit Volume Liter (L) Cubic centimeter (cm 3 ) Density Scientific Notation Dimensional Analysis Prefix Conversion Factor Precision Accuracy Error Percent Error Exact Number Measured Number Significant Figures (SF s) Scientific Notation States of Matter Solid Liquid Gas Vapor Physical Properties Extensive Property Intensive Property Physical Change Phase Change Chemical Properties Chemical Change Law of Conservation or Mass Mixtures Homogeneous Solution Heterogeneous Chromatography Filtration Distillation Conductivity Matter Pure Substance Element Compound Atoms Dalton s Atomic Theory Cathode Ray Subatomic Particles Proton Neutron Electron Nucleus Atomic Mass Unit (amu) Atomic Number Mass Number Isotope Atomic Symbol Atomic Mass Weighted Average Radioactivity Radiation Nuclear Reaction Radioactive Decay Alpha Radiation Nuclear Equation Beta Radiation Beta Particle Gamma Ray Electromagnetic radiation Wavelength Frequency Amplitude Electromagnetic spectrum Quantum Planck s Constant Photoelectric Effect Photon Bright Line Spectra Atomic Emission Spectrum Ground State Quantum Number Heisenberg Uncertainty Principle Quantum Mechanical Model (Atom) Orbital Principal Quantum Number Principal Energy Level Energy Sublevel Electron Configuration Aufbau Principle Pauli Exclusion Principle Hund s Rule Valence Electron Electron Dot Structure Periodic Law Group Period Representative Element Transition Element Metal Alkali Metal Alkaline Earth Metals Transition Metal Inner Transition Metal Lanthanide Series Actinide Series Nonmetal Halogen Noble Gas Metalloid s block p block d block f block Atomic radius (trend) Ion Ionization Energy Ionic Radius (trend) Electronegativity (trend)

2 CHEMISTRY AND HONORS CHEMISTRY SCIENCE PACING GUIDE Standards 1st 9 Weeks Resources ACT Activity Approximate pacing number of days (41) Lab Safety and Basic Data Analysis Skills QC I.A.1.f Safely use laboratory equipment and techniques when conducting scientific investigations. Glencoe Matter and Change Read Chapter 1 Chapter 2 Graphing Lab Safety 1 day QC I.A.2.a-c, e-g; II.A.1.b Use Mathematics and measurement in science appropriately. 6 days HS.CHEM.4. Plan and conduct an investigation to classify properties of matter as intensive (e.g., density, viscosity, specific heat, melting point, boiling point) or extensive (e.g., mass, volume, heat) and demonstrate how intensive properties can be used to identify a compound Glencoe Matter and Change Ch. 3 5 days

3 HS.CHEM.1. Obtain and communicate information from historical experiments (e.g., work by Mendeleev and Moseley, Rutherford's gold foil experiment, Thomson's cathode ray experiment, Millikan's oil drop experiment, Bohr's interpretation of bright line spectra) to determine the structure and function of an atom and to analyze the patterns represented in the periodic table. Glencoe Matter and Change Chapters days HS.CHEM.2. Develop and use models of atomic nuclei to explain why the abundance-weighted average of isotopes of an element yields the published atomic mass ( QC V.E.a,b) Not in HS.CHEM. Describe alpha, beta, and gamma decay, half-life and fission and fusion Write appropriate equations for nuclear decay reactions, using particle balance; describe how the nucleus changes during these reactions and compare the resulting radiation with regard to penetrating ability. HS.CHEM.3. Use the periodic table as a systematic representation to predict properties of elements based on their valence electron arrangement. HS.CHEM.3.a. Analyze data such as physical properties to explain periodic trends of the elements, including metal/nonmetal/metalloid behavior, electrical/heat conductivity, electronegativity and electron affinity, ionization energy, and atomic-covalent/ionic radii, and how they relate to position in the periodic table. Glencoe Matter and Change Chapter 6 3 days

4 CHEMISTRY AND HONORS CHEMISTRY SCIENCE PACING GUIDE QUARTER 2 VOCABULARY Chemical Bond Cation Anion Ionic Bond Ionic Compound Crystal Lattice Electrolyte Lattice Energy Formula Unit Monatomic Ion Polyatomic Ion Oxyanion Electron Sea Model Delocalized Electon Metallic Bond Alloy Covalent Bond Molecule Lewis Structure Sigma Bond Pi Bond Endothermic Reaction Exothermic Reaction Oxyacid Structural Formula Space Filling Model Ball and Stick Model Resonance Coordinate Covalent Compound Valence Shell Electron Pair Repulsion VSEPR Lewis Structure Single Bond Double Bond Triple Bond Lone Pair (Unshared) Hybridization Polarity Polar Covalent Bond Nonpolar Covalent Bond Dipole Polar Molecule Nonpolar Molecule Chemical Reaction Reactant Product Chemical Equation Coefficient Solid (s) Liquid (l) Aqueous (aq) Gas (g) Synthesis Reaction Combustion Reaction Decomposition Single-Replacement Reaction Activity Series Double-Replacement Reaction Precipitate Aqueous Solution Solute Solvent Complete Ionic Reaction Spectator Ion Net Ionic Equation Oxidation-Reduction REaction Redox Oxidation Reduction Oxidation Number Oxidizing Agent Reduction Agent Oxidation-Number Method Species Half-Reaction

5 CHEMISTRY AND HONORS CHEMISTRY SCIENCE PACING GUIDE Standards 2nd 9 Weeks Resources ACT Activity Approximate pacing number of days (41) HS.CHEM.3.c. Use the periodic table as a model to derive formulas and names of ionic and covalent compounds Glencoe Matter and Change Chapters days HS.CHEM.3.b. Develop and use models (e.g., Lewis dot, 3-D ball-and-stick, space-filling, valence-shell electron-pair repulsion [VSEPR]) to predict the type of bonding and shape of simple compounds.

6 HS.CHEM.5. Plan and conduct investigations to demonstrate different types of simple chemical reactions based on valence electron arrangements of the reactants and determine the quantity of products and reactants. Glencoe Matter and Change Ch. 9 Redox Ch days Review for Final Exam 1

7 CHEMISTRY AND HONORS CHEMISTRY SCIENCE PACING GUIDE QUARTER 3 VOCABULARY Mole Avogadro s Number Formula Unit Conversion Factor Subscripts Molar Mass Percent Composition Empirical Formula Molecular Formula Hydrate Stoichiometry Law of Conservation of Mass Mole Ratio Limiting Reactant Excess Reactant Theoretical Yield Actual Yield Percent Yield Energy Law of Conservation of Energy Chemical Potential Energy Kinetic Energy Heat calorie Joule Specific Heat Calorimeter Thermochemistry System Surroundings Universe Enthalpy Enthalpy (Heat) of Reaction Exothermic Endothermic Thermochemical Equation Enthalpy of Combustion Molar Enthalpy of Vaporization Molar Enthalpy of Fusion Hess s Law Standard Enthalpy of Formation Kinetic-Molecular Theory Elastic Collision Temperature Diffusion Graham s Law of Effusion Pressure Barometer Pascal Atmosphere Dalton s Law of Partial Pressures Intermolecular Forces Dispersion Force Dipole-Dipole Force Hydrogen Bond Viscosity Surface Tension Surfactant Crystalline Solid Unit Cell Allotrope Amorphous Solid Melting Point Vaporization Evaporation Vapor Pressure Boiling Point Freezing Point Condensation Deposition Phase Diagram Triple Point

8 CHEMISTRY AND HONORS CHEMISTRY SCIENCE PACING GUIDE Standards 3rd 9 Weeks Resources ACT Activity Approximate pacing number of days (41) HS.CHEM.5. Plan and conduct investigations to demonstrate different types of simple chemical reactions based on valence electron arrangements of the reactants and determine the quantity of products and reactants. Glencoe Matter and Change Chapter 10 6 days HS.CHEM.5.a. Use mathematics and computational thinking to represent the ratio of reactants and products in terms of masses, molecules, and moles.

9 HS.CHEM.5.a. Use mathematics and computational thinking to represent the ratio of reactants and products in terms of masses, molecules, and moles. Glencoe Matter and Change Ch days HS.CHEM.5.b. Use mathematics and computational thinking to support the claim that atoms, and therefore mass, are conserved during a chemical reaction. HS.CHEM.11. Construct an explanation that describes how the release or absorption of energy from a system depends upon changes in the components of the system. Glencoe Matter and Change Chapter 15 (Sections 1-4) 3.5 days HS.CHEM.11a. Develop a model to illustrate how the changes in total bond energy determine whether a chemical reaction is endothermic or exothermic. HS.CHEM.11b. Plan and conduct an investigation that demonstrates the transfer of thermal energy in a closed system (e.g., using heat capacities of two components of differing temperatures).

10 HS.CHEM.9. Analyze and interpret data (e.g., melting point, boiling point, solubility, phase-change diagrams) to compare the strength of intermolecular forces and how these forces affect physical properties and changes. Glencoe Matter and Change Chapter days HS.CHEM.10. Plan and conduct experiments that demonstrate how changes in a system (e.g., phase changes, pressure of a gas) validate the kinetic molecular theory.

11 CHEMISTRY AND HONORS CHEMISTRY SCIENCE PACING GUIDE QUARTER 4 VOCABULARY Pressure Volume Temperature Direct proportional/ relationship Inverse proportional/ relationship Boyle s Law Absolute Zero Charles s Law Gay-Lusaac s Law Combined Gas Law Avogadro s Principle Molar Volume Standard Temperature and Pressure Ideal Gas Constant Ideal Gas Law Suspension Colloid Brownian Motion Tyndall Effect Soluble Miscible Insoluble Immiscible Concentration Molarity Molality Solvation Heat of Solution Unsaturated Solution Saturated Solution Supersaturated Solution Henry s Law Colligative Property Vapor Pressure Lowering Boiling Point Elevation Freezing Point Depression Osmosis Osmotic Pressure Acidic Solution Basic Solution Arrhenius Model Bronsted-Lowry Model Conjugate Acid Conjugate Base Conjugate Acid-Base Pair Amphoteric Lewis Model Strong Acid Weak Acid Acid Ionization Constant Strong Base Weak Base Base Ionization Constant Ion Product Constant for Water ph poh Neutralization Reaction Salt Titration Titrant Equivalence Point Acid-Base Indicator End Point Salt Hydrolysis Buffer Buffer Capacity Reversible Reaction Chemical Equilibrium Law of Chemical Equilibrium Equilibrium Constant Le Chatelier s Principle

12 CHEMISTRY AND HONORS CHEMISTRY SCIENCE PACING GUIDE Standards 4th 9 Weeks Resources ACT Activity Approximate pacing number of days (41) HS.CHEM.10a. Develop a model to explain the relationship between the average kinetic energy of the particles in a substance and the temperature of the substance (e.g., no kinetic energy equaling absolute zero [0K or o C]). Glencoe Matter and Change Ch HS.CHEM.7. Plan and carry out investigations to explain the behavior of ideal gases in terms of pressure, volume, temperature, and number of particles. HS.CHEM.7 a. Use mathematics to describe the relationships among pressure, temperature, and volume of an enclosed gas when only the amount of gas is constant. HS.CHEM.7 b. Use mathematical and computational thinking based on the ideal gas law to determine molar quantities. HS.CHEM.6. Use mathematics and computational thinking to express the Glencoe Matter and Change Ch days

13 concentrations of solutions quantitatively using molarity. HS.CHEM.6 a. Develop and use models to explain how solutes are dissolved in solvents. HS.CHEM.6 b. Analyze and interpret data to explain effects of temperature on the solubility of solid, liquid, and gaseous solutes in a solvent and the effects of pressure on the solubility of gaseous solutes. HS.CHEM.6 c. Design and conduct experiments to test the conductivity of common ionic and covalent substances in a solution. Glencoe Matter and Change Chapter 18 6 days HS.CHEM.6 d. Use the concept of ph as a model to predict the relative properties of strong, weak, concentrated, and dilute acids and bases (e.g., Arrhenius and Brønsted-Lowry acids and bases).

14 HS.CHEM.8. Refine the design of a given chemical system to illustrate how LeChâtelier's principle affects a dynamic chemical equilibrium when subjected to an outside stress (e.g., heating and cooling a saturated sugar- water solution). Glencoe Matter and Change Chapter 17 (sections 1&2) 2 days Introduce Organic Chemistry If time allows. Not a standard. Review for Final Exam Glencoe Matter and Change Chapter 21 1 day