High School Chemistry
2017-2018 Course Outline

                                                                   
Required Text: Conceptual Chemistry, John Suchocki, 2nd Edition

COMPETENCY GOAL 1: The learner will develop abilities necessary to do and understand scientific inquiry.

1.01 Design, conduct and analyze investigations to answer questions related to chemistry.
  • Identify questions and suggest hypotheses. 
  • Identify variables. 
  • Use a control when appropriate. 
  • Select and use appropriate measurement
    tools. 
  • Collect and organize data in tables,
    charts and graphs. 
  • Analyze and interpret data. 
  • Explain observations. 
  • Make inferences and predictions. 
  • Explain the relationship between
    evidence and explanation. 
  • Identify how scientists share findings. 
COMPETENCY GOAL 2: The learner will build an understanding of the structure and properties of matter.

2.01 Analyze the historical development of the current atomic theory.
  • Early contributions: Democritus and Dalton. 
  • The discovery of the electron: Thomson and Millikan. 
  • The discovery of the nucleus, proton and neutron: Rutherford and Chadwick. 
  • The Bohr model. 
  • The quantum mechanical model
2.02 Examine the nature of atomic structure
  • Subatomic particles: protons, neutrons,
    and electrons. 
  • Mass number. 
  • Atomic number. 
  • Isotopes. 
2.03 Apply the language and symbols of chemistry.
  • Name compounds using the IUPAC conventions. 
  • Write formulas of simple compounds from their names. 
2.04 Identify substances using their physical properties:
  • Melting points. 
  • Boiling points. 
  • ï Density.
  • ï Solubility. 
2.05 Analyze the basic assumptions of kinetic molecular theory and its applications:
  • Ideal Gas Equation. 
  • Combined Gas Law
  • Boyles Law
  • Charles Law
2.06 Assess bonding in metals and ionic compounds as related to chemical and physical properties.
  • Describe how ions are formed and which arrangements are stable (filled d-level, or half- filled d-level). 
  • Appropriately use the term cation as a positively charged ion and anion as negatively charged ion
  • Predict ionic charges for representative elements based on valence electrons. 
  • Describe ionic bond’s intermolecular attraction as electrostatic attraction. 
2.07 Assess covalent bonding in molecular compounds as related to molecular geometry and chemical and physical properties.
  • Apply the concept that sharing electrons form a covalent compound that is a stable (inert gas) arrangement. 
  • Determine that a bond is predominately covalent by the location of the atoms on the Periodic Table (nonmetals combined with nonmetals) or when ΔEN < 1.7. 
  • Know that the diatomic elements have single, double, or triple bonds (For example: F2, O2, N2).
  • Describe carbon bonds as either single, double or triple bonds.
  • Apply the relationship between bond energy and length of single, double, and triple bonds (conceptual, no numbers).
  • Draw Lewis (dot diagram) structures for simple compounds with one central atom.
2.08 Assess the dynamics of physical equilibria.
  • Interpret phase diagrams. 
  • Factors that affect phase changes. 
COMPETENCY GOAL 3: The learner will build an understanding of regularities in chemistry.

3.01 Analyze periodic trends in chemical properties and use the periodic table to predict properties of elements.
  • Groups (families). 
  • Periods. 
  • Representative elements (main group) and transition elements. 
  • Identify alkali metals, alkaline earth metals, halogens, and noble gases based on location on periodic table.
  • Electron configuration and energy levels. 
  • Ionization energy. 
  • Atomic and ionic radii. 
  • Electronegativity. 
  • Write electron configurations, including noble gas abbreviations (no exceptions to the general rules). Included here are extended arrangements showing electrons in orbitals. 
  • Identify s, p, d, and f blocks on Periodic Table. 
  • Identify an element based on its electron configuration. (Students should be able to identify elements which follow the general rules, not necessarily those which are exceptions.) 
  • Determine the number of valence electrons from electron configurations. 
  • Predict the number of electrons lost or gained and the oxidation number based on the electron configuration of an atom. 
  • Define ionization energy. 
  • Know group and period general trends for ionization energy. 
  • Apply trends to arrange elements in order of increasing or decreasing ionization energy. 
  • Explain the reasoning behind the trend. 
  • Atomic and ionic radii 
  •  Define atomic radius and ionic radius. 
  • Know group and period general trends for atomic radius. 
  • Apply trends to arrange elements in order of increasing or decreasing atomic radius. 
  • Compare cation radius to neutral atom. 
  • Compare anion radius to neutral atom. 
  • Explain the reasoning behind the trend. 
  • Define electronegativity. 
  • Know group and period general trends for electronegativity. 
  • Apply trends to arrange elements in order of increasing or decreasing electronegativity. 
  • Explain the reasoning behind the trend. 
  • Use differences in electronegativity to predict bond type (ionic, polar covalent, and nonpolar covalent).
3.02 Apply the mole concept, Avogadro’s number and conversion factors to chemical calculations:
  • Particles to moles. 
  • Mass to moles. 
  • Volume of a gas to moles. 
  • Molarity of solutions. 
  • Empirical and molecular formula. 
  • Percent composition. 
3.03 Calculate quantitative relationships in chemical reactions (stoichiometry):
  • Moles of each species in a reaction. 
  • Mass of each species in a reaction. 
  • Volumes of gaseous species in a
    reaction. 
COMPETENCY GOAL 4: The learner will build an understanding of energy changes in chemistry.

4.01 Analyze the Bohr model in terms of electron energies in the hydrogen atom.
  • The spectrum of electromagnetic energy. 
  • Emission and absorption of
    electromagnetic energy as electrons change energy levels. 
4.02 Analyze the law of conservation of energy, energy transformation, and various forms of energy involved in chemical and physical processes.
  • Differentiate between heat and temperature. 
  • Analyze heating and cooling curves. 
  • Calorimetry, heat of fusion and heat of
    vaporization calculations. 
  • Endothermic and exothermic processes
    including interpretation of potential
    energy. 
4.03 Analyze the relationship between entropy and disorder in the universe.
  • Understand entropy as a measure of disorder. 
  • Recognize that the entropy of the universe is increasing. 
  • Explain that, along with a tendency for systems to proceed toward the lowest energy level, they also move in the direction of the greatest entropy. (Increasing Entropy: solid → liquid → gas; Ionic compounds → ions in solution) 
COMPETENCY GOAL 5: The learner will develop an understanding of chemical reactions.

5.01 Evaluate various types of chemical reactions
  • Analyze reactions by types: single replacement, double replacement (including acid-base neutralization), decomposition, synthesis, and combustion of simple hydrocarbons. 
  • Predict products. 
  • Identify a reaction by type. 
  • Predict product(s) in a reaction using the reference tables. 
  • Identify acid-base neutralization as double replacement. 
  • Write and balance ionic equations. 
  • Write and balance net ionic equations for double replacement reactions. 
  • Recognize that hydrocarbons (C,H molecule) and other molecules containing C, H, and O burn completely in oxygen to produce CO2 and water vapor. 
5.02 Evaluate the law of conservation of matter to the balancing of chemical equations.
  • Write and balance formulas and equations
  • Write net ionic equations.
5.03 Assess the physical and chemical properties of acids and bases.
  • General properties of acids and bases. 
  • Concentration and dilution of acids and bases.
  • Distinguish between acids and bases based on formula and chemical properties. 
  • Buffer systems
  • Ionization and the degree of dissociation (strengths) of acids and bases. 
  • Indicators. 
  • Acid-base titration. 
  • pH and pOH. 
  • Compute concentration (molarity) of acids and bases in moles per liter (3.02). 
  • Solve dilution problems: M1V1 = M2V2. 
  • Differentiate between concentration (molarity) and strength (degree of dissociation). No calculation involved. 
  • Use pH scale to identify acids and bases.
  • Relate the color of indicator to pH using pH ranges provided in a table. Range should involve various values of pH (for example: 3.3 or 10.8). 
  • Determine the concentration of an acid or base using titration. Interpret titration curve for strong acid/strong base. 
5.04 Analyze oxidation/reduction reactions with regard to the transfer of electrons.
  • Assign oxidation numbers to elements in REDOX reactions 
  • Identify the elements oxidized and reduced. 
  • Write simple half reactions. 
  • Assess the practical applications of
    oxidation and reduction reactions. 
5.05 Analyze the factors that affect the rates of chemical reactions.
  • The nature of the reactants. 
  • Temperature.
  • Concentration.
  • Catalyst.