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Properties Of Matter (return to top) |
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1. There are differences and similarities among pure substances and mixtures. (AKSci - A.1) |
• Describe and/or use the techniques of distillation, filtration, chromatography or fractional crystallization to separate or identify a mixture • Use characteristic properties to identify substances. |
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2. Measurement involves both accuracy and precision. (AKSci - B.1) |
• Measurement should be done in the metric system to the maximum accuracy of the apparatus. • Measurements and calculations should consider appropriate significant digits. |
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3. Conversions in chemistry are usually accomplished using the dimensional analysis (factor label method). (AKSci - B.1) |
• Perform multiple step conversions with a variety of conversion factors. |
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4. The number of particles is measured in a unit called mole. (AKSci - A.1) |
• Convert between units of moles, mass and number of particles. |
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5. The concentrations of solutions can be express in a variety of units. This concentration affects physical properties of the solution. (AKSci - A.2) |
• Carry out concentration calculations in molarity, molality, mole fraction, percent composition, ppm, and ppb. • Convert between any of the above. • Using concentrations calculate the boiling point, melting point, vapor pressure, and osmotic pressure of a solution (colligative properties). • Experimentally determine the molar mass of an unknown compound by freezing point depression. • Use solubility rules and reference material to predict solubility of compounds before using them in the lab. • Make saturated, supersaturated, and unsaturated solutions. • Prepare solutions by mass or by dilution. |
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6. There are standard methods of naming and formula writing for elements and compounds (emphasize IUPAC system). (AKSci - A.1) |
• ExName or write formulas of ionic compounds, covalent compounds, and acids. • Show a familiarity with both stock and Latin names of metals, polyatomic ions, and common names of compounds used in chemistry. • Name or give the formula of alkanes, alkenes, alkynes, and aromatic hydrocarbons; as well as functional group derivatives of these. |
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7. Crystalline solids can be classified as ionic, metallic, covalent network, or molecular. (AKSci - A.1) |
• Explain the properties of ionic, metallic, or molecular, or network covalent crystals from their structure and forces holding them together. • Classify in the laboratory a crystalline substance as either ionic, metallic, molecular, or network covalent on the basis of its properties. |
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8. Substances can be classified as acid, base, or neutral. (AKSci - A.1) |
• Determine whether substances (including salts) are acidic, basic, or neutral on physical/chemical properties. |
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Chemical Change (return to top) |
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1. Chemical changes are described with balanced chemical equations. (AKSci - A.2) |
• Balance chemical equations given the reactants and products. • Recognize reaction types and predict products for reactions. • Write equations for dissociation and ionization of electrolytes. • Identify the spectator ions and write net ionic equations for solution reactions with only reactants given. |
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2. Balanced chemical equations are used to make calculations related to chemical reactions. (AKSci - A.2) |
• Determine the amount (mass, gas volume, solutions volume or molarity, number of particles, or moles) of product formed or reactant used knowing an initial amount of one other substance present. • Determine the limiting reagent and calculate the theoretical and actual yield in a chemical reaction given the appropriate data. • Perform a gravimetric analysis experiment and determine the yield. • Prepare inorganic and organic compounds and determine the yield. |
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3. Chemical reactions are frequently studied in solution. (AKSci - A.2) |
• Use solubility rules to predict whether a precipitate forms when electrolyte solutions are mixed. • Use a qualitative analysis scheme to separate and identify unknown ions. • Calculate the volume of a more concentrated solution that must be diluted to obtain a given quantity of more dilute solution. • Calculate the volume of a solution required to react with a volume of a different solution using molarity and the stoichiometry of the reaction. • Write solubility product expressions for insoluble compounds and experimentally determine solubility product constants (Ksp). • Calculate solubility or predict precipitation's using Ksp. |
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4. Reaction rates can be experimentally studied, and can be expressed mathematically. (AKSci - A.2, B.1) |
• Explain the factors that effect reaction rate using collision theory, kinetic and potential energy diagrams, activation energy, and reaction mechanisms. • Collect data on a reactant or product to graph reaction rates and calculate average or instantaneous rates. • Experimentally determine orders of reactions, write rate expressions, and calculate activation energy. • Use integrated forms of the various rate laws in order to analyze reaction rates. |
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5. Electron transfer takes place in redox reactions. Oxidation and reduction are the basis for electrochemistry. (AKSci - A.2) |
• Identify the substance oxidized and reduced, as well as the oxidizing and reducing agents. • Balance redox equations by the electron transfer and/or the half reaction method in acid or basic solution. • Perform a redox titration to determine unknown concentration. • Explain the operation of voltaic and electrolytic cells. • Calculate cell potentials and predict spontaneity for reactions at standard conditions or with different concentrations or temperatures given. |
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6. H+ transfer can take place in a chemical reaction. (AKSci - A.2) |
• Show an understanding of the common acid/base theories and properties. • Identify the acid, base, and conjugates in a reaction involving transfer of H+. • Perform an acid/base titration to determine the concentration of an unknown. |
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7. The strength of an acid and/or base is related to its composition and degree to which it breaks down. (AKSci - A.1, A.2) |
• Identify strong or weak acids/bases based on their formulas or names. • Explain the difference between strong, weak, concentrated, and dilute solutions. • Experimentally determine a Ka or Kb. |
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8. The pH scale gives a level of acidity/basicity for a solution based on the concentration of H+ (or hydronium ion) present. (AKSci - A.2) |
• Experimentally determine pH using indicators, pH meters, and/or test paper. • Interpret pH data to determine level of acidity/basicity. • Identify the dominant species controlling H+ concentration in solution of acids, bases, or salts. • Calculate the ion concentration and pH of both strong and weak acids and bases. • Perform pH titration's of strong and weak acid and base solutions. • Explain how indicators and buffers work in terms of equilibrium shifting. • Perform serial dilutions to study pH and indicators. • Make a buffer in the lab and test its capacity. |
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9. Many reactions consist of both a forward and reverse reaction occurring simultaneously. Through this process equilibrium can be achieved. (AKSci - A.2) |
• Explain how to recognize an equilibrium on the basis of properties and explain the dynamic process involved in equilibrium such as vapor pressure, phase change, solubility, and chemical equilibria. • Study equilibrium systems in the lab. • Write equilibrium expressions and calculate constant or concentrations. • Determine the direction of equilibrium shift using the reaction quotient (Q). |
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Structure Of Matter (return to top) |
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1. Properties of matter, physical and chemical changes can be explained through sketches, models, and descriptions of the particles. (AKSci - A.1, A.2) |
• Construct sketches or models of solids, liquids, and gases. Use these to determine how phase changes proceed. • Construct molecular models to determine shape and molecular polarity in compounds. • Use sketches and models to describe chemical reactions. |
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2. Some chemical and physical changes consist of both a forward and reverse process occurring simultaneously. (AKSci - A.2) |
• Identify the opposing changes and discuss their rates. |
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3. Kinetic molecular theory explains changes in gas volumes, moles, pressure, and temperature. This allows for calculations to be performed relating these quantities. (AKSci - A.1) |
• Use Kinetic Molecular Theory to explain the relationship of pressure, volume, moles, and temperature in gases. • Perform calculations to determine one of the four major variables given the other three (pressure, volume, moles, a temperature) using the ideal gas law. • Calculate the ideal gas constant in a variety of units. • Experimentally verify the molar volume of a gas or study gas stoichiometry using the gas laws. • Derive equations from the gas laws to calculate gas densities or molar masses. • Determine experimentally the relationships of pressure versus volume, pressure versus temperature, and volume versus temperature. Express these relationships in graphs and interpret these graphs. • Calculate the effect of changes in gaseous systems, using the combined gas law. • Derive Graham's law from kinetic energy and use to study diffusion/effusion of gases. • Suggest and recognize practical applications using these relationships. • Compare the behavior of real gases to the ideal gas laws. |
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4. Atoms are composed of protons, neutrons, and electrons. (AKSci - A.1) |
• Write nuclear symbols for atoms, isotopes, or ions. • Determine the number of protons, neutrons, and electrons from a nuclear symbol. • Diagram the formation of ions by electron transfer. |
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5. An atom's electron configuration, particularly the outermost electrons, determines how the atom can Interact with other atoms. Atoms form bonds to other atoms by transferring or sharing electrons. (AKSci - A.1, A.8a) |
• Write an electron configuration and draw orbital diagrams for any atom or ion. • Give the quantum numbers for an electron or identify an electron from a set of quantum numbers. • Determine if a bond between atoms is ionic, polar covalent, or nonpolar covalent on the basis of electronegativity or position on the periodic table. • Explain the difference between ionic, polar covalent or nonpolar covalent bonds. |
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6. An element's location on the periodic table can be used to determine similarities and trends among the elements. (AKSci - A.1 |
• Recognize and explain trends within groups and periods on the periodic chart in quantities/properties such as Ion charges, atomic and ionic size, ionization energy, electron affinity, reactivity, metallic character, and electronegativity. • Identify and relate properties of elements in particular families such as alkali metals, alkaline earth metals, halogens, and noble gases. |
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7. The arrangement of atoms in a molecule determines the molecule's properties. Shapes are particularly important in explaining how molecules interact with others. (AKSci - A.1) |
• Draw Lewis structures of molecules or ions recognizing exceptions to the octet rule, hybridization and resonance. • Determine a molecule's shape and polarity using Valence Shell Electron Pair Repulsion Theory and bond polarities • Determine the type and strength of intermolecular forces based on molecular polarity. Relate the strength of intermolecular forces to physical properties such as boiling point, melting point, surface tension, solubility, vapor pressure, adhesion, cohesion, and viscosity. • Suggest and recognize practical applications using intermolecular forces. • Explain the bonding type, shape, and hybridization of carbon bonds in organic compounds. • Explain the physical and chemical properties of an organic compound on the basis of the shape and polarity of the molecule and functional group present. (i.e.; alcohol, aldehyde, ketone, organic acid, alkane, alkene, alkyne). Prepare a number of different polymers, observe their properties and explain their properties on the basis of their structures (i.e.; nylon, latex, and rubber). |
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8. Nuclear changes are different than chemical changes. The nucleus can change, resulting in a different element and/or radioactivity. (AKSci - A.2) |
• Distinguish between nuclear and chemical reactions. • Write balanced nuclear reactions for emissions or adsorption's • Calculate matter/ energy conversions. • Relate decay to first order chemical reactions. • Calculate half-lives or quantity of a radioisotope remaining after a period of time. • Discuss relevant applications of nuclear chemistry. |
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Energy Change (return to top) |
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1. Temperature is a measurement of average kinetic energy. Heat is a measurement of transferable energy. (AKSci - A.2, A.9) |
• Measure temperature and heat in appropriate units and perform conversions when necessary. • Interpret a graph of kinetic energy versus number of particles and relate this to reaction rates and activation energies. • Perform an experiment (calorimetry) to measure heat flow and or calculate heat capacity. |
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2. Chemical and physical changes can be classified as exothermic or endothermic. Balanced equations with an energy term can be used to calculate energy changes. (AKSci - A.2) |
• Identify reactions as either exothermic or endothermic from experimental data or an equation including an energy term. • Draw enthalpy verses course of reaction diagrams for both endo- and exothermic reactions; and use them to illustrate activation energy and the action of catalysts. • Understand the meaning of enthalpy and be able to use tables of enthalpies of formation. • Write and algebraically manipulate thermochemical equations. • Determine the energy change for a given mass or moles from an equation with an energy term. • Discuss the transitions between potential and kinetic energy in a chemical reaction. • Use the Hess's law equation to calculate heat of reactions. • Perform calorimetry experiments to determine the heat of fusion and/or vaporization of water, as well as heats of solution and reactions. • Describe entropy as a driving force and calculate it from tables of standard values. • Calculate Gibb's free energy and relate it to reaction spontaneity. • Relate free energy to equilibrium constants, and redox cell potentials. |
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3. When energy changes in an isolated atom or molecule, the energy changes in discrete jumps from one value to another. This change in energy occurs when radiation is absorbed or emitted, so the radiation also has discrete energy values. (AKSci - A.2, A.9) |
• Explain the lines in a spectra on the basis of electrons changing between discrete energy level. • Relate energy level transitions to bright line emissions, and calculate variables in light equations. |
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