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Chemistry AP
  

Chemistry – AP

Recommended Prerequisite:  Chemistry I; Algebra II

Grades Offered:  10 - 12

Credit:  ½ - 1

SDE Course Code:  3225

MNPS Course Code: SCI6211

 

Course Description:

 This course is designed to meet the College Board requirements to prepare students to take the AP exam, which may result in the awarding of college credit.  The course will cover the atomic structure and the interaction of atoms.  Students will study stoichiometry, equation balancing, problem solving, states of matter, oxidation-reduction reactions, equilibrium, kinetics, thermodynamics, periodicity of the elements, bonding, basic organic chemistry and environmental chemistry.

 

Course of Study:

 

  • Structure of Matter
    • provides evidence of the atomic theory
    • determines atomic masses by chemical and physical means
    • determines the atomic number, mass number and isotopes
    • investigates atomic spectra, quantum numbers, and atomic orbitals in relation to electron levels
    • predicts periodic relationships such as atomic radii, ionization energies, electron affinities, and oxidation states
    • explains the states, structures, and properties of matter via discussion of ionic, covalent, metallic, hydrogen bonding, van der Waals forces, polarity of bonds, and electronegativities
    • uses the knowledge of Lewis structures, hybridization of orbitals, resonance, sigma and pi bonds, and VSEPR theory to explain and illustrate chemical bonding
    • relates the geometry of ions, structural isomerism of simple organic molecules and coordination of complexes, dipole moments of molecules and their relationship to properties of these structures
    • determines nuclear equations, half-lives, and radioactivity of matter

 

  • States of Matter
    • calculates the variables of pressure, temperature, volume, density, and mass of an ideal gas and explains deviation of real gases from ideal gases
    • interprets the ideal gas laws based on the kinetic molecular model and relates kinetic energy to changes in temperature
    • explains states of matter using Avogadro’s hypothesis and the mole concept
    • explains all properties of liquids and solids using the kinetic molecular theory
    • interprets phase diagrams of one component systems, including phase changes, critical points and the triple point
    • relates the structure of solids and lattice heat energies
    • calculates concentration of solutions including molarity and molality
    • identifies types of solutions and the factors affecting solubility
    • relates Rault’s Law and colligative properties of nonvolatile solutes to concepts of solutions and describes the non-ideal behavior to solutions

 

  • Reactions
    • explains acid-base reactions including the concepts of Arhenius, Bronsted-Lowery, and Lewis, as well as coordination complexes and amphoterism
    • predicts precipitation reactions
    • analyzes oxidation-reduction (redox) reactions by: assign oxidation numbers, investigate the role of electron in redox reactions, relate redox to electrochemistry, electrolytic and galvanic cells, Faraday’s laws, standard half-cell potentials, Nernst equation, and predicting the direction of redox reactions
    • writes net ionic equations by predicting the ionic and molecular species present
    • balances equations including redox
    • determines mass and volume relations with emphasis on the mole concept, empirical formulas and limiting reactants
    • utilizes concepts of dynamic equilibrium, Le Chatelier’s Principle and equilibrium constants
    • calculates equilibrium constants for chemical reactions including gaseous, acid and bases, solubility product
    • investigates common ion effect, buffers and hydrolysis
    • calculates and uses experimental data to determine reactant order, rate constants, rate-determining step, reaction rate law, and reaction rates
    • explains state functions within the three laws of thermodynamics
    • applies the laws of thermodynamics to equilibrium constants and electrode potential

 

  • Descriptive Chemistry
    • predicts chemical reactivity and products of chemical reactions
    • explains relationships in the periodic table: horizontal, vertical, and diagonal with examples from major groups (families) and the first series of transition elements
    • understands basic organic chemistry; hydrocarbons and functional groups (structure, nomenclature, chemical properties)

 

  • Chemical Calculations
    • solve problems and express correctly in significant digits, precision of measured values, using logarithmic and exponential relationships to solve: percentage composition; empirical and molecular formulas; molar masses from gas density, freezing-point, and boiling-point measurements; gas laws, including the ideal gas law, Dalton’s law and Graham’s law; stochiometric relations using the mole concept and titrations results; mole fractions, molar and molal solutions; Faraday’s laws of electrolysis; equilibrium constants and their applications, including their use in simultaneous equilibria; standard electrode potentials and their use, the Nernst equation; thermodynamic and thermochemical calculations,; and kinetic calculations.

 

  • Chemistry Laboratory
    • Demonstrates proficiency in the following skills: synthesis of compounds (solid and gas); separations(precipitation and filtration, dehydration, centrifugation, distillation, chromatography); observing and recording phase changes; titration using indicators and meters; spectroscopy and colorimetry; devising and utilizing a scheme for qualitative analysis of ions in solutions; and gravimetric analysis

 

Standards:

MNPS standards for AP Chemistry can be accessed at: 
http://www.mnps.org/PageFactory.aspx?PageID=3353

State and College Board AP Chemistry standards can be found at:   http://www.collegeboard.com/student/testing/ap/sub_chem.html?chem

 

 

Textbooks:     Chemistry, 6th edition; Zumdahl and Zumdahl Houghton Mifflin Company

                       

 

Recommended/Required Resources:

  • Laboratory facility with access to a source of water and electricity for lab equipment; required
  • Extensive use of the laboratory for instruction with emphasis on use of the microscale(small-scale) experiments, which allow for sophisticated labs to be completed and /or repeated with fewer resources and less time.
  • Completion of the College Board recommended laboratory experiments
  • Computer-based probe ware such as light sensors, motion detectors, heat probes, pH meters, etc. (recommended)