AP Objectives Of Atomic Structure And Periodic Table

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History of Atom and Atomic Structure

The student should be able to :

1. Trace the development of atomic theory and the structure of the atom from the Greeks to the present (Dalton, Thompson, Rutherford, Bohr, and charge cloud model).

2. Explain photoelectric effect (Einstein) and how it relates to the concept of the electron and the atom. (physical example of why electrons can only be "in" energy levels)

3. Explain what light is in terms of DeBroglie, Planck (particle characteristics), and light characteristics.

4. Be able to calculate energy, wavelength and frequency using all appropriate equations and how the variable relate to each other (e.g. direct vs, indirect proportion).
5. Be able to calculate Energy changes for electrons going between energy levels using Bohr's energy equation (E=2.79

6. Be able to explain the difference between a continuous spectrum, emission spectra, and absorption spectra. Also know the components of the emission and absorption spectra including how it relates to the movement of an electron.

Atomic Structure and Quantum Mechanics

The student should be able to:

1. Explain the Charge Cloud Model of the atom and how it relates to the electron. Also, give the big picture of where the electrons are "located" and why it is so important that we know where the electrons are.

2. Explain the difference between classical (Newtonian) mechanics and quantum mechanics.

3. Explain the contribution of Bohr, Planck and deBroglie to Quantum Mechanics.

4. Explain Heisenberg Uncertainty Principle with respect to the electron.

5. Explain how Schrodinger's equation helped in understanding the location (highest probability of finding) of the electron and the establishment of subenergy levels and orbtials.

6. Define what a node is, what it means with respect to standing wave and the number of nodes in an energy level.

7. Generate the subenergy from lowest energy (closest to the nucleus) to the highest subenergy level (farthest from nucleus). Should be able to do this just from the Periodic Table.

8. Know the 3 rules of filling in electron in subenergy / orbital including name and what it means (Aufbau Principle, Hund'sRule, and Pauli Exclusion Principle)

9. Understand that only Hydrogen atom has degenerate subenergy levels and orbitals.

10. Determine the correct electron configuration for any atom (Remember to write the last subenergy levels out as orbitals) including the half-half and half-full exceptions.
11. Explain the significance of the wave function (and its square).

12. Explain the penetrating effect of electrons and how it determine which subenergy levels are filled with electrons first.

13. Be able to determine the number of valence electrons for any "s" or "p" block element. Also, explain which one of Zinc electrons are lost when forming its cation (goes to understand of penetrating effect of electron).

History of Periodic Table and Periodic Trends

Each student will be able to:

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Last edited March 14, 2018 9:42 am (diff)