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Independent and Dependent Variables - identify the independent variable, dependent variable, experimental and control groups in three studies [not interactive]
Use a variety of appropriate notations (e.g., exponential, functional, square root). Math.1
Select and apply appropriate methods for computing with real numbers and evaluate the reasonableness of the results. Math.2
Apply algebraic properties, formulas, and relationships to perform operations on real-world problems (e.g., solve for density, determine the concentration of a solution in a variety of units: ppm, ppb, molarity, molality, and percent composition) calculate heats of reactions and phase changes, and manipulate gas law equations. Math.3
Interpret rates of change from graphical and numerical data (e.g., phase diagrams, solubility graphs, colligative properties, nuclear decay or half-life). Math.4
Analyze graphs to describe the behavior of functions (e.g., concentration of a solution, phase diagrams, solubility graphs, colligative properties, nuclear decay half-life).
Math.5
Model real-world phenomena using functions and graphs. Math.6
Apply and interpret algebraic properties in symbolic manipulation (e.g., density, concentration of a solution, chemical equations, effect of volume, temperature or pressure on behavior of a gas, percent composition of elements in a compound, molar mass, number of moles, and molar volume, amount of products or reactants given mole, molarity, volume at STP or mass amounts, heat loss or gain using mass, temperature change and specific heat, and half-life of an isotope). Math.7
Apply and communicate measurement units, concepts and relationships in algebraic problem-solving situations. Math.8
Select appropriate units, scales, and measurement tools for problem situations involving proportional reasoning and dimensional analysis. Math.9
Select, construct, and analyze appropriate graphical representations for a data set. Math.10
Identify and solve different types of stoichiometry problems (e.g., volume at STP to mass, moles to mass, molarity). Math.11
Calculate the amount of product expected in an experiment and determine percent yield. Math.12
Convert among the quantities of a substance: mass, number of moles, number of particles, molar volume at STP. Math.13
Identify the contributions of major atomic theorists: Bohr, Chadwick, Dalton, Planck, Rutherford, and Thomson. 1.1
Compare the Bohr model and the quantum mechanical electron-cloud models of the atom. 1.2
Draw Bohr models of the first 18 elements. 1.3
Interpret a Bohr model of an electron moving between its ground and excited states in terms of the absorption or emission of energy. 1.4
Use the periodic table to identify an element as a metal, nonmetal, or metalloid. 1.5
Apply the periodic table to determine the number of protons and electrons in a neutral atom. 1.6
Determine the number of protons and neutrons for a particular isotope of an element. 1.7
Explain the formation of anions and cations, and predict the charge of an ion formed by the main-group elements. 1.8
Sequence selected atoms from the main-group elements based on their atomic or ionic radii. 1.9
Sequence selected atoms from the main-group elements based on first ionization energy, electron affinity, or electronegativity. 1.10
Determine an atom’s Lewis electron-dot structure or number of valence electrons from an element’s atomic number or position in the periodic table. 1.11
Represent an atom’s electron arrangement in terms of orbital notation, electron configuration notation, and electron-dot notation. 1.12
Compare s and p orbitals in terms of their shape, and order the s, p, d and f orbitals in terms of energy and number of possible electrons. 1.13
Compare and contrast the major models of the atom (e.g., Democritus, Thomson, Rutherford, Bohr, and the quantum mechanical model). SPI 1.1
Interpret the periodic table to describe an element’s atomic makeup. SPI 1.2
Describe the trends found in the periodic table with respect to atomic size, ionization energy, electron affinity, or electronegativity. SPI 1.3
Determine the Lewis electron-dot structure or number of valence electrons for an atom of any main-group element from its atomic number or position in the periodic table. SPI 1.4
Represent an electron’s location in the quantum mechanical model of an atom in terms of the shape of electron clouds (s and p orbitals in particular), relative energies of orbitals, and the number of electrons possible in the s, p, d and f orbitals. SPI 1.5
Identify a material as an element, compound or mixture; identify a mixture as homogeneous or heterogeneous; and/or identify a mixture as a solution, colloid or suspension. 2.1
Identify the solute and solvent composition of a solid, liquid or gaseous solution. 2.2
Express the concentration of a solution in units of ppm, ppb, molarity, molality, and percent composition. 2.3
Describe how to prepare solutions of given concentrations expressed in units of ppm, ppb, molarity, molality, and percent composition. 2.4
Investigate factors that affect the rate of solution. 2.5
Describe how to prepare a specific dilution from a solution of known molarity. 2.6
Determine the colligative properties of a solution based on the molality and freezing point or boiling points of the solvent. 2.7
Use a solubility graph, composition of a solution and temperature to determine if a solution is saturated, unsaturated or supersaturated. 2.8
Classify properties and changes in matter as physical, chemical, or nuclear. 2.9
Use calorimetry to: identify unknown substances through specific heat, determine the heat changes in physical and chemical changes, determine the mass of an object, and determine the change in temperature of a material. 2.10
Perform calculations on heat of solvation, heat of reaction, and heat of formation, and heat of phase change. 2.11
Use particle spacing diagrams to identify solids, liquids, or gases. 2.12
Distinguish among solid, liquid, and gaseous states of a substance in terms of the relative kinetic energy of its particles. 2.13
Use a phase diagram to correlate changes in temperature and energy with phases of matter. 2.14
Graph and interpret the results of experiments that explore relationships among pressure, temperature, and volume of gases. 2.15
Distinguish among elements, compounds, solutions, colloids, and suspensions. SPI 2.1
Identify properties of a solution: solute and solvent in a solid, liquid or gaseous solution; procedure to make or determine the concentration of a solution in units of ppm, ppb, molarity, molality, percent composition, factors that affect the rate of solution, and colligative properties. SPI 2.2
Classify a solution as saturated, unsaturated, or supersaturated based on its composition and temperature and a solubility graph. SPI 2.3
Classify a property of change in matter as physical, chemical, or nuclear. SPI 2.4
Compare and contrast heat and temperature changes in chemical and physical processes. SPI 2.5
Investigate similarities and differences among solids, liquids and gases in terms of energy and particle spacing. SPI 2.6
Predict how changes in volume, temperature, and pressure affect the behavior of a gas. SPI 2.7
Determine the type of chemical bond that occurs in a chemical compound. 3.1
Differentiate between ionic and covalent bond models. 3.2
Identify the chemical formulas of common chemical compounds. 3.3
Employ a table of polyvalent cations and polyatomic ions to name and describe the chemical formula of ionic compounds. 3.4
Convert percent composition information into the empirical or molecular formula of a compound. 3.5
Apply information about the molar mass, number of moles, and molar volume to the number of particles of the substance. 3.6
Balance an equation for a chemical reaction. 3.7
Classify a chemical reaction as composition, decomposition, single replacement, double replacement, and combustion. 3.8
Use activity series or solubility product table information to predict the products of a chemical reaction. 3.9
Predict the products of a neutralization reaction involving inorganic acids and bases. 3.10
Interpret a chemical equation to determine molar ratios. 3.11
Convert between the following quantities of a substance: mass, number of moles, number of particles, and molar volume at STP. 3.12
Solve different types of stoichiometry problems (e.g., volume at STP to mass, moles to mass, molarity). 3.13
Determine the amount of expected product in an experiment and calculate percent yield. 3.14
Calculate the amount of heat lost or gained by a substance based on its mass, change in temperature, and specific heat during physical and chemical processes. 3.15
Research applications of thermal changes in nuclear reactions. 3.16
Identify a substance as an acid or base according to its formula. 3.17
Investigate the acidity/basicity of substances with various indicators. 3.18
Write the nuclear equation involving alpha or beta particles based on the mass number of the parent isotope and complete symbols for alpha or beta emissions. 3.19
Determine the half-life of an isotope by examining a graph or with an appropriate equation. 3.20
Write a balanced nuclear equation to compare nuclear fusion and fission. 3.21
Describe the benefits and hazards of nuclear energy. 3.22
Analyze ionic and covalent compounds in terms of how they form, names, chemical formulas, percent composition, and molar masses. SPI 3.1
Identify the reactants, products, and types of different chemical reactions: composition, decomposition, double replacement, single replacement, combustion. SPI 3.2
Predict the products of a chemical reaction. SPI 3.3
Balance a chemical equation to determine molar ratios. SPI 3.4
Convert among the following quantities of a substance: mass, number of moles, number of particles, molar volume at STP. SPI 3.5
Identify and solve stoichiometry problems: volume at STP to mass, moles to mass, and molarity. SPI 3.6
Classify substances as acids or bases based on their formulas and how they react with various indicators. SPI 3.7
Describe radioactive decay through a balanced nuclear equation and through an analysis of the half-life concept. SPI 3.8
Compare and contrast nuclear fission and fusion. SPI 3.9
Relate the laws of conservation of mass/energy to thermal changes that occur during physical, chemical or nuclear processes. SPI 3.10
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sound | 
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interactive lesson | 
a quiz | 
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