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What are the coordination complexes of iron that the AP board requires students to know?
Answer 1:

Here is the outline for chemistry out of the College Board "Acorn" book.

  1. Structure of Matter
    1. Atomic theory and atomic structure
      1. Evidence of the atomic theory
      2. Atomic masses; determination by chemical and physical means
      3. Atomic number and mass number; isotopes
      4. Electron energy levels; atomic spectra, quantum numbers, atomic orbitals
      5. Periodic relationships including, for example, atomic radii, ionization energies, electron affinities, oxidation states
    2. Chemical bonding
      1. Binding forces
        1. Types: ionic, covalent, metallic, hydrogen bonding, van der Waals (including London dispersion forces)
        2. Relationships to states, structure, and properties of matter
        3. Polarity of bonds, electronegativities
      2. Molecular models
        1. Lewis structures
        2. Valence bond: hybridization of orbitals, resonance, sigma and pi bonds
        3. VSEPR
      3. Geometry of molecules and ions; structural isomerism of simple organic molecules and coordination complexes; dipole moments of molecules; relation of properties to structure
    3. Nuclear chemistry; nuclear equations, half-lives, and radioactivity; chemical applications
  2. States of Matter
    1. Gases
      1. Laws of ideal gases
        1. Equation of state for an ideal gas
        2. Partial pressures
      2. Kinetic-molecular theory
        1. Interpretation of ideal gas laws on the basis of this theory
        2. Avogadros hypothesis and the mole concept
        3. Dependence of kinetic energy of molecules of temperature
        4. Deviations from ideal gas laws
      3. Liquids and solids
      4. 1. Liquids and solids from the kinetic-molecular viewpoint
        2. Phase diagrams of one-component systems
        3. Changes of state, including critical points and triple points
        4. Structure of solids; lattice energies
        C. Solutions
        1. Types of solutions and factors affecting solubility
        2. Methods of expressing concentration (The use of normalities is not tested.)
        3. Raoults law and colligative properties (nonvolatile solutes); osmosis
        4. Non-ideal behavior (qualitative aspects)
        III. Reactions
        A. Reaction types
        1. Acid-base reactions; concepts of Arrhenius, Brnsted-Lowry, and Lewis; coordination complexes; amphoterism
        2. Precipitation reactions
        3. Oxidation-reduction reactions
        a. Oxidation number
        b. The role of of the electron in oxidation-reducation
        c. Electrochemistry:
        electrolytic and galvanic cells; Faradays laws; standard half-cell potentials; Nernst equation; prediction of the direction of redox reactions
        B. Stoichiometry
        1. Ionic and molecular species present in chemical systems: net ionic equations
        2. Balancing of equations including those for redox reactions
        3. Mass and volume relations with emphasis on the mole concept, including empirical formulas and limiting empirical formulas and limiting reactants
        C. Equilibrium
        1. Concept of dynamic equilibrium, physical and chemical; Le Chateliers principle; equilibrium constants
        2. Quantitative treatment
        a. Equilibrium constants for gaseous reactions: Kp, Kc
        b. Equilibrium constants for reactions in solution
        (1) Constants for acids and bases; pK; pH
        (2) Solubility product constants and their and their application to precipitation and the dissolution of slightly soluble compounds
        (3) Common ion effect; buffers; hydrolysis
        D. Kinetics
        1. Concept of rate of reaction
        2. Use of experimental data and graphical analysis to determine reactant order, rate constants, and reaction rate laws.
        3. Effect of temperature charge on rates
        4. Energy of activation; the role of catalysts
        5. The relationship between the rate-determining step and a mechanism
        E. Thermodynamics
        1. State functions
        2. First law: change in enthalpy; heat of formation; heat of reaction; Hesss law; heats of vaporization and fusion; calorimetry
        3. Second law: entropy; free energy of formation; free energy of reaction; dependence of change in free energy on enthalpy and entropy changes.
        4. Relationship of change in free energy to equilibrium constants and electrode potentials
        IV. Descriptive Chemistry
        A. Chemical reactivity and products of chemical reactions
        B. Relationships in the periodic table; horizontal, vertical, and diagonal with examples from alkali metals, alkaline earth metals, halogens, and the first series of transition elements



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