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Chemistry II

Chemistry II is an advanced level course that is an elective designed for students who have completed Chemistry and desire a broader, in-depth study of the content found in the science field of chemistry. Chemistry is the study of matter, its composition and its changes. This course is designed to prepare students to be critical and independent thinkers who are able to function effectively in a scientific and technological society, and to build upon and extend the chemistry concepts, skills and knowledge from the previous chemistry class. This course is designed not only to prepare a student for college chemistry but to make the college chemistry experience much easier as the student will have already studied much of the material reserved for college chemistry at the high school level. Students will engage in active inquiries, investigations and hands-on activities for a minimum of 50% of the instructional time to develop conceptual understanding and research/laboratory skills as they evaluate the academic requirements and prepare for occupational opportunities in biology, chemistry, engineering, and technology. Safety instruction is integrated into all activities. The West Virginia Standards for 21st Century Learning include the following components: 21st Century Content Standards and Objectives and 21st Century Learning Skills and Technology Tools. All West Virginia teachers are responsible for classroom instruction that integrates learning skills, technology tools and content standards and objectives.
SC.S.CII.1
Natural and Application of Science

Students will

·         demonstrate an understanding of history and nature of science as a human endeavor encompassing the contributions of diverse cultures and scientists.

·         demonstrate the ability to use the inquiry process to solve problems.

·         relate science-technology-societal issues while using a variety of sources to construct and defend their solutions

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    • SC.PD.CII.1
    Distinguished Above Mastery Mastery Partial Mastery Novice
    Chemistry II students at the distinguished level in the nature and applications of science:

    implement safe practices as they design, conduct, and revise experiments to solve real world problems, analyze data for errors, and base conclusions on observations and experimental evidence, and

    relate science-technology-societal issues while using a variety of sources to construct solutions and defend their ideas to an authentic audience.

    		 Chemistry II students at the above mastery level in the nature and applications of science:

    implement safe practices as they design, conduct, and revise experiments, analyze data for errors, and base conclusions on observations and experimental evidence, and


    relate science-technology-societal issues while using a variety of sources to construct and defend their solutions.

    		 Chemistry II students at the mastery level will in the nature and applications of science:

    implement safe practices as they design, conduct, and revise experiments and base conclusions on observations and experimental evidence, and



    relate science-technology-societal issues while using a variety of sources to construct and defend their solutions.

    		 Chemistry II students at the partial mastery level in the nature and applications of science:

    implement safe practices as they conduct and revise experiments, then base conclusions on observations and experimental evidence, and



    relate science-technology-societal issues while using a variety of sources to construct their solutions.

    		 Chemistry II students at the novice level in the nature and applications of science:

    implement safe practices as they conduct experiments and base conclusions on observations and experimental evidence, and




    relate science-technology-societal issues while using a variety of sources to construct their solutions.
    Number Objective
    SC.O.CII.1.1
    		implement safe procedures and practices when manipulating equipment, materials, organisms, and models.
    SC.O.CII.1.2
    		formulate scientific explanations based on historical observations and experimental evidence, accounting for variability in experimental results.
    SC.O.CII.1.3
    		conduct and/or design investigations that incorporate the skills and attitudes and/or values of scientific inquiry (e.g., established research protocol, accurate record keeping, replication of results and peer review, objectivity, openness, skepticism, fairness, or creativity and logic).
    SC.O.CII.1.4
    		design, conduct, evaluate and revise experiments (e.g., compose a question to be investigated, design a controlled investigation that produces numeric data, evaluate the data in the context of scientific laws and principles, construct a conclusion based on findings, propose revisions to investigations based on manipulation of variables and/or analysis of error, or communicate and defend the results and conclusions).
    SC.O.CII.1.5
    		draw conclusions from a variety of data sources to analyze and interpret systems and models (e.g., use graphs and equations to measure and apply variables such as rate and scale, evaluate changes in trends and cycles, or predict the influence of external variances such as potential sources of error, or interpret maps).
    SC.O.CII.1.6
    		investigate, compare and design scientific and technological solutions to address personal and societal problems.
    SC.O.CII.1.7
    		given current science-technology-societal issues, construct and defend potential solutions.
    SC.O.CII.1.8
    		relate societal, cultural and economic issues to key scientific innovations.
    SC.O.CII.1.9
    		synthesize concepts across various science disciplines to better understand the natural world (e.g., form and function, systems, or change over time).
    SC.S.CII.2
    Content of Science

    Students will

    ·         demonstrate knowledge, understanding and applications of scientific facts, concepts, principles, theories and models as delineated in the objectives.

    ·         demonstrate an understanding of the interrelationships among physics, chemistry, biology, earth/environmental sciences and astronomy.

    ·         apply knowledge, understanding and skills of science subject matter/concepts to daily life experiences.

    SC.PD.CII.2
    Distinguished Above Mastery Mastery Partial Mastery Novice
    Chemistry II students at the distinguished level:

    utilize VSEPR theory to make predictions about valence bonds that can be used to compare and contrast binding forces;

    justify the ideal gas laws on the basis of the kinetic-molecular theory;

    predict theoretical yield, limiting reactant, excess reactant, percent yield, and experimental error from a designed experiment that includes the appropriate stoichiometric applications;

    design an experiment to illustrate the effect of changing concentration on the colligative properties of solutions, change of state, and molar mass;

    evaluate systems based on the physical and chemical dynamic equilibrium concepts that include equilibrium constants and system directional change according to Le Chatelier’s principle;

    design an effective battery using the voltage calculated from the Nernst equation;



    design and conduct experiments to collect and graphically analyze data to investigate reaction rate and predict reactant order;


    design and conduct experiments to experimentally and mathematically demonstrate the first and second law of thermodynamics including the reaction spontaneity;


    calculate and explain the relationships among weak acids, pH, pOH, pK, Ka, Kb, Kw, ionization constants, and percent ionization, Ksp;

    prove the presence of specific cations and anions in an unknown mixture through experimental data;

    solve complex problems involving radioactive decay and write nuclear equations for decay, fission, and fusion;

    perform calculations involving the addition of a strong acid or base to a buffer; experimentally justify the hydrolysis of a salt and equivalence point of a titration curve, and

    evaluate organic structures and compounds based on functional groups.

    		 Chemistry II students at the above mastery level:

    utilize VSEPR theory to explain valence bonding; and the types of binding forces;


    assess the ideal gas laws on the basis of the kinetic-molecular theory;

    explain from experimental data and appropriate stoichoimetric applications the limiting reactant, excess reactant, and theoretical yield;


    evaluate experiments that effect colligative properties and states of matter by changing concentration;



    illustrate physical and chemical dynamic equilibrium concepts by calculating equilibrium constants and applying Le Chatelier’s principle to predict system change:


    predict the voltage using the Nernst equation and use this to compare chemical cells;



    demonstrate reactant order, rate constants, reaction rate laws, rate calculations and predict the effect of temperature on rate changes;


    demonstrate experimentally and mathematically applications of Hess’s Law, spontaneous reactions, and the second law of thermodynamics;


    explain weak electrolytes, ionization constants, and percent ionization;




    design a qualitative analysis for an unknown mixture;


    investigate the similarities and differences between radioactive processes, nuclear fission, and fusion;

    predict the pH of a salt from its formula then calculate the pH of the salt; write the reaction of hydrolyzed salt; interpret the effect of a buffer on an aqueous system, and

    differentiate, classify and characterize simple organic functional groups and compounds.

    		 Chemistry II students at the mastery level:

    investigate valence bonds and binding forces;



    interpret the ideal gas laws on the basis of the kinetic-molecular theory;

    perform stoichiometric calculations utilizing Avogadro’s concepts, significant figures, and mathematical applications for molar mass, theoretical yield, and limiting reactant;

    explain by concentration calculations the effect of changing concentration on the colligative properties of solutions and on changes of state;

    explain the physical and chemical dynamic equilibrium concepts through calculation of equilibrium constants and application of Le Chatelier’s principle;


    identify oxidation numbers for the ions that are used to calculate the electron movement in a redox reaction and calculate the voltage using the Nernst equation;

    determine reactant order, rate constants, and reaction rate laws using rate calculation and describe the effect of temperature on rate changes;

    determine the heat of formation, heat of reaction, heat of vaporization and heat of fusion while using applications of Hess’s Law and use the second law of thermodynamics;


    identify weak electrolytes, pH, pOH, pK, Ka, Kb, Kw, Ksp and calculate pH and pOH; measure pH with indicator papers and electronic meters;

    analyze a solution that contains known cations and a solution that contains known anions;

    express radioactive decay in an equation format and solve simple problems for the half-life of an isotope;

    identify the components of a buffer and the use of buffers, and




    recognize and classify simple organic functional groups.

    		 Chemistry II students at the partial mastery level:

    match types of bonding forces including all that contain valence bonds;


    explain the ideal gas laws on the basis of the kinetic-molecular theory;

    perform stoichiometric calculations utilizing Avogadro’s concepts, significant figures, and mathematical applications for molar mass, theoretical yield, and limiting reactant;

    calculate molar mass and concentration then describe the effect of changing concentration on colligative properties and change of state:

    describe the physical and chemical dynamic equilibrium concepts that include the calculation of equilibrium constants and Le Chatelier’s principle;


    use oxidation numbers for ions in a compound to calculate the electron movement in a redox reaction and calculate the voltage using the Nernst equation;

    estimate reactant order using rate constants, reaction rate laws, rate calculations, and temperature’s influence on rate changes;


    state the second law of thermodynamics and applications of Hess’s Law that include calculations of the free energy of formation and the free energy of reaction;

    identify weak electrolytes, pH, pOH, pK, Ka, Kb, Kw, Ksp and calculate pH and pOH; measure pH with indicator papers and electronic meters;

    construct a data table for cation and anion analysis;


    categorize by using the properties of the different types of radiation emitted during radioactive decay;


    identify salts that undergo hydrolysis and match the reaction for the ion with water; interpret a titration curve to identify the equivalence point, and


    identify simple organic functional groups and compounds.

    		 Chemistry II students at the novice level:

    describe valence bonds and types of binding forces;



    state the ideal gas laws and describe their basis on kinetic molecular theory;

    calculate theoretical yield that is expressed in correct significant figures and determine the molar mass, theoretical yield, and limiting reactant;


    match molar mass and the effect of concentration changes on colligative properties and changes of state;


    define physical and chemical dynamic equilibrium concepts, equilibrium constants and Le Chatelier’s principle;



    recognize the oxidation numbers for ions in a compound used to calculate the electron movement in a redox reaction and match the voltage using the Nernst equation;

    match reactant order, rate constants, or reaction rate laws, calculate the rate of reaction and describe the effect of temperature on rate changes;

    identify Hess’s Law and the dependence of free energy on enthalpy and entropy changes:




    define weak electrolytes, pH, pOH, pK, Ka, Kb, Kw, Ksp; calculate pH and pOH and measure pH with indicator papers or electronic meters;

    identify the colors of specific cation and anion precipitates;


    identify a nuclear equation and generally describe radioactive decay;


    identify the equivalence point on a titration curve, and




    match simple organic functional groups and compounds.
    Number Objective
    SC.O.CII.2.1
    		identify types of binding forces such as:
    • ionic
    • covalent
    • metallic
    • van der Waals forces (including London)
    and relate binding forces to state, structure, and properties of matter.
    SC.O.CII.2.2
    		investigate the valence bond including the concepts of:
    • hybridization of orbitals
    • resonance
    • formation of sigma and pi bonds
    and demonstrate an understanding of the VSEPR theory.
    SC.O.CII.2.3
    		apply the principles of chemical reactivity, products of chemical reactions, and relationships on periodic table to predict the ions in a descriptive chemistry experiment.
    SC.O.CII.2.4
    		interpret the ideal gas laws on the basis of the kinetic-molecular theory.
    SC.O.CII.2.5
    		relate Avogadro’s hypothesis and its relation to the mole concept.
    SC.O.CII.2.6
    		define changes of state, including critical temperatures and triple points, based on the kinetic molecular theory.
    SC.O.CII.2.7
    		calculate concentration and explain the effect of changing concentration on the colligative properties of solutions.
    SC.O.CII.2.8
    		identify oxidation numbers for ions and for any element in a compound to calculate the electron movement in a redox reaction and calculate the voltage using the Nernst equation.
    SC.O.CII.2.9
    		explain physical and chemical dynamic concepts; calculate equilibrium constants Kp, Kc, Ksp, Ka, and apply Le Chatelier’s principle.
    SC.O.CII.2.10
    		use experimental data and graphical analysis to determine reactant order, rate constants, and reaction rate laws, calculate the rate of reaction and explain the effect of temperature on rate changes.
    SC.O.CII.2.11
    		determine the heat of formation, heat of reaction, heat of vaporization and heat of fusion; apply Hess’s Law.
    SC.O.CII.2.12
    		using the second law of thermodynamics, calculate the free energy of formation, free energy of reaction and the dependence of free energy on enthalpy and entropy changes.
    SC.O.CII.2.13
    		perform all calculations with attention given to significant figures, precision of measured values, and the use of logarithmic and exponential relationships.
    SC.O.CII.2.14
    		calculate molar masses from gas density, freezing-point, and boiling-point measurements.
    SC.O.CII.2.15
    		experimentally determine the properties of acids:
    • identify weak electrolytes;
    • define pH, pOH, pK, Ka, Kb, Kw, ionization constant, percent ionization, Ksp;
    • calculate pH and pOH;
    • measure pH with indicator papers and electronic meters;
    • recognize salts that undergo hydrolysis
    • write a reaction for the ion with water
    • interpret a titration curve to identify the equivalence point and
    • calculate the range of a buffer.
    SC.O.CII.2.16
    		perform stoichiometric calculations to produce values for theoretical yield and to decide the limiting reactant of a given chemical reaction.
    SC.O.CII.2.17
    		recognize simple organic functional groups and classify simple organic compounds by name.
    SC.O.CII.2.18
    		given the reactants, anticipate the products and create balanced equations for nuclear reactions.

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