Understanding The Chemistry in Context, Classification of Matter and Physical and Chemical Properties

1.1 Describe how chemistry and engineering helped transform aluminum from a precious metal into an inexpensive structural material. 1.2 Explain the usefulness of the macroscopic, microscopic, and symbolic perspectives in understanding chemical systems. 1.3 Identify properties of and changes in matter as physical or chemical 1.4 Identify properties of matter as extensive or intensive 1.5 Draw pictures to illustrate simple chemical phenomena (like the differences among solids, liquids, and gases) on the molecular scale. 1.6 Use appropriate ratios to convert measurements from one unit to another. 1.7 Express the results of calculations using the correct number of significant figures.

Understanding The Atoms Structure,, Molecules, and Ions

2.1 Outline milestones in the development of modern atomic theory 2.2 Summarize and interpret the results of the experiments of Thomson, Millikan, and Rutherford 2.3 Describe the three subatomic particles that compose atoms 2.4 Define isotopes and give examples for several elements 2.5 Explain the basic behavior of waves, including travelling waves and standing waves 2.6 Describe the wave nature of light 2.7 Describe the Bohr model of the hydrogen atom 2.8 Extend the concept of wave–particle duality that was observed in electromagnetic radiation to matter as well 2.9 Understand the general idea of the quantum mechanical description of electrons in an atom, and that it uses the notion of three-dimensional wave functions, or orbitals, that define the distribution of probability to find an electron in a particular part of space 2.10 List and describe traits of the four quantum numbers that form the basis for completely specifying the state of an electron in an atom 2.11 Write and interpret symbols that depict the atomic number, mass number, and charge of an atom or ion 2.12 Define the atomic mass unit and average atomic mass 2.13 Derive the predicted ground-state electron configurations of atoms 2.14 Identify and explain exceptions to predicted electron configurations for atoms and ions 2.15 Relate electron configurations to element classifications in the periodic table

Understanding The Periodic Table

3.1 Describe and explain the observed trends in atomic size, ionization energy, and electron affinity of the 3.2 elements 3.3 State the periodic law and explain the organization of elements in the periodic table 3.4 Predict the general properties of elements based on their location within the periodic table 3.5 Identify metals, nonmetals, and metalloids by their properties and/or location on the periodic table 3.6 Define ionic and molecular (covalent) compounds 3.7 Predict the type of compound formed from elements based on their location within the periodic table 3.8 Determine formulas for simple ionic compounds 3.9 Derive names for common types of inorganic compounds using a systematic approach 3.10 Symbolize the composition of molecules using molecular formulas and empirical formulas 3.11 Represent the bonding arrangement of atoms within molecules using structural formulas

Chemical Bonding and Molecular Geometry

4.1 Explain the formation of cations, anions, and ionic compounds 4.2 Predict the charge of common metallic and nonmetallic elements, and write their electron configurations 4.3 Describe the formation of covalent bonds 4.4 Define electronegativity and assess the polarity of covalent bonds 4.5 Write Lewis symbols for neutral atoms and ions 4.6 Draw Lewis structures depicting the bonding in simple molecules 4.7 Explain the concepts of polar covalent bonds and molecular polarity 4.8 Assess the polarity of a molecule based on its bonding and structure

Understanding The Composition of Substances and Solutions

5.1 Calculate formula masses for covalent and ionic compounds 5.2 Define the amount unit mole and the related quantity Avogadro’s number Explain the relation between mass, moles, and numbers of atoms or molecules, and perform calculations deriving these quantities from one another 5.3 Compute the percent composition of a compound 5.4 Determine the empirical formula of a compound 5.5 Determine the molecular formula of a compound 5.6 Describe the fundamental properties of solutions 5.7 Calculate solution concentrations using molarity 5.8 Perform dilution calculations using the dilution equation 5.9 Define the concentration units of mass percentage, volume percentage, mass-volume percentage, parts-permillion (ppm), and parts-per-billion (ppb) 5.10 Perform computations relating a solution’s concentration and its components’ volumes and/or masses using these units

Understanding The Stoichiometry of Chemical Reactions

6.1 Derive chemical equations from narrative descriptions of chemical reactions. 6.2 Write and balance chemical equations in molecular, total ionic, and net ionic formats. 6.3 Define three common types of chemical reactions (precipitation, acid-base, and oxidation-reduction) 6.4 Classify chemical reactions as one of these three types given appropriate descriptions or chemical equations 6.5 Identify common acids and bases 6.6 Predict the solubility of common inorganic compounds by using solubility rules 6.7 Compute the oxidation states for elements in compounds 6.8 Explain the concept of stoichiometry as it pertains to chemical reactions 6.9 Use balanced chemical equations to derive stoichiometric factors relating amounts of reactants and products 6.10 Perform stoichiometric calculations involving mass, moles, and solution molarity 6.11 Explain the concepts of theoretical yield and limiting reactants/reagents. 6.12 Derive the theoretical yield for a reaction under specified conditions. 6.13 Calculate the percent yield for a reaction.

Understanding The Stoichiometry of Chemical Reactions

6.1 Derive chemical equations from narrative descriptions of chemical reactions. 6.2 Write and balance chemical equations in molecular, total ionic, and net ionic formats. 6.3 Define three common types of chemical reactions (precipitation, acid-base, and oxidation-reduction) 6.4 Classify chemical reactions as one of these three types given appropriate descriptions or chemical equations 6.5 Identify common acids and bases 6.6 Predict the solubility of common inorganic compounds by using solubility rules 6.7 Compute the oxidation states for elements in compounds 6.8 Explain the concept of stoichiometry as it pertains to chemical reactions 6.9 Use balanced chemical equations to derive stoichiometric factors relating amounts of reactants and products 6.10 Perform stoichiometric calculations involving mass, moles, and solution molarity 6.11 Explain the concepts of theoretical yield and limiting reactants/reagents. 6.12 Derive the theoretical yield for a reaction under specified conditions. 6.13 Calculate the percent yield for a reaction.

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Understanding The Electrochemistry

7.1 Define electrochemistry and a number of important associated terms 7.2 Split oxidation-reduction reactions into their oxidation half-reactions and reduction half-reactions 7.3 Produce balanced oxidation-reduction equations for reactions in acidic or basic solution 7.4 Identify oxidizing agents and reducing agents 7.5 Use cell notation to describe galvanic cells 7.6 Describe the basic components of galvanic cells 7.7 Determine standard cell potentials for oxidation-reduction reactions 7.8 Use standard reduction potentials to determine the better oxidizing or reducing agent from among several possible choices 7.9 Relate cell potentials to free energy changes 7.10 Use the Nernst equation to determine cell potentials at nonstandard conditions 7.11 Perform calculations that involve converting between cell potentials, free energy changes, and equilibrium constants 7.12 Classify batteries as primary or secondary 7.13 List some of the characteristics and limitations of batteries 7.14 Provide a general description of a fuel cell 7.15 Define corrosion 7.16 List some of the methods used to prevent or slow corrosion 7.17 Describe electrolytic cells and their relationship to galvanic cells 7.18 Perform various calculations related to electrolysis

Understanding The Electrochemistry

7.1 Define electrochemistry and a number of important associated terms 7.2 Split oxidation-reduction reactions into their oxidation half-reactions and reduction half-reactions 7.3 Produce balanced oxidation-reduction equations for reactions in acidic or basic solution 7.4 Identify oxidizing agents and reducing agents 7.5 Use cell notation to describe galvanic cells 7.6 Describe the basic components of galvanic cells 7.7 Determine standard cell potentials for oxidation-reduction reactions 7.8 Use standard reduction potentials to determine the better oxidizing or reducing agent from among several possible choices 7.9 Relate cell potentials to free energy changes 7.10 Use the Nernst equation to determine cell potentials at nonstandard conditions 7.11 Perform calculations that involve converting between cell potentials, free energy changes, and equilibrium constants 7.12 Classify batteries as primary or secondary 7.13 List some of the characteristics and limitations of batteries 7.14 Provide a general description of a fuel cell 7.15 Define corrosion 7.16 List some of the methods used to prevent or slow corrosion 7.17 Describe electrolytic cells and their relationship to galvanic cells 7.18 Perform various calculations related to electrolysis

Understanding The Entropy and the Second Law of Thermodynamics

8.1 describe the scientific and economic obstacles to more widespread recycling of plastics 8.2 explain the concept of entropy in your own words. 8.3 deduce the sign of DS for many chemical reactions by examining the physical state of the reactants and products. 8.4 state the second law of thermodynamics in words and equations and use it to predict spontaneity. 8.5 state the third law of thermodynamics. 8.6 use tabulated data to calculate the entropy change in a chemical reaction. 8.7 derive the relationship between the free energy change of a system and the entropy change of the universe. 8.8 use tabulated data to calculate the free energy change in a chemical reaction. 8.9 explain the role of temperature in determining whether a reaction is spontaneous. 8.10 use tabulated data to determine the temperature range for which a reaction will be spontaneous.

Thermochemistry

9.1 Define energy, distinguish types of energy, and describe the nature of energy changes that accompany 9.2 chemical and physical changes 9.3 Distinguish the related properties of heat, thermal energy, and temperature 9.4 Define and distinguish specific heat and heat capacity, and describe the physical implications of both 9.5 Perform calculations involving heat, specific heat, and temperature change 9.6 Explain the technique of calorimetry 9.7 Calculate and interpret heat and related properties using typical calorimetry data 9.8 State the first law of thermodynamics 9.9 Define enthalpy and explain its classification as a state function 9.10 Write and balance thermochemical equations 9.11 Calculate enthalpy changes for various chemical reactions 9.12 Explain Hess’s law and use it to compute reaction enthalpies

Understanding the Chemical Kinetics

10.1 explain the role of chemical kinetics in the formation and destruction of ozone in the atmosphere. 10.2 . 10.3 define the rate of a chemical reaction and express the rate in terms of the concentrations of individual reactants or products. 10.4 10.5 use the method of initial rates to determine rate laws from experimental data. 10.6 use graphical methods to determine rate laws from experimental data 10.7 explain the role of a catalyst in the design of practical chemical reactions

Nuclear Structure and Stability Nuclear Equations Radioactive Decay Transmutation and Nuclear Energy Uses of Radioisotopes Biological Effects of Radiation

11.1 explain that equilibrium is dynamic and that at equilibrium, the forward and backward reaction rates are equal. State these ideas in your own words. 11.2 write the equilibrium constant expression for any reversible reaction. 11.3 calculate equilibrium constants from experimental data. 11.4 calculate equilibrium composition from initial data and the numerical value of the equilibrium constant. 11.5 calculate molar solubility from Ksp or vice versa. 11.6 write equilibrium constants for the dissociation of weak acids and weak bases and use them to calculate pH or the degree of ionization. 11.7 use LeChatelier’s principle to explain the response of an equilibrium system to applied stresses. 11.8 calculate the new equilibrium composition of a system after an applied stress. 11.9 explain the importance of both kinetic and equilibrium considerations in the in the design of industrial chemical processes. 11.10 list chemical reactions important in the production and weathering of concrete.

Understanding of Nuclear chemistry,

2. 12.1 Describe nuclear structure in terms of protons, neutrons, and electrons 12.2 Explain trends in the relative stability of nuclei 12.3 Identify common particles and energies involved in nuclear reactions 12.4 Write and balance nuclear equations 12.5 Recognize common modes of radioactive decay 12.6 Identify common particles and energies involved in nuclear decay reactions 12.7 Write and balance nuclear decay equations 12.8 Calculate kinetic parameters for decay processes, including half-life 12.9 Describe common radiometric dating techniques 12.10 Describe the synthesis of transuranium nuclides 12.11 Explain nuclear fission and fusion processes 12.12 Relate the concepts of critical mass and nuclear chain reactions 12.13 Summarize basic requirements for nuclear fission and fusion reactors 12.14 List common applications of radioactive isotopes 12.15 Describe the biological impact of ionizing radiation 12.16 Define units for measuring radiation exposure 12.17 Explain the operation of common tools for detecting radioactivity 12.18 List common sources of radiation exposure in the US

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