List the 3 principles which define how electrons can be arranged in an atom.
The Aufbau principle, the Pauli exclusion principle, and the Hund rule.
Discuss each principle, use examples and then discuss the notation used for each sub level and orbital.
Work 3-4 atomic electron configurations using both the letter designations and the electron spin designations. Have Joshua work 3-4 electron designations using higher atomic number atoms.
Note the filled orbitals occurring with the inert gases, and the partially unfilled orbitals occurring with other than inert gases. Elicit a shorthand method to designate electron configurations for atoms located between inert gas atomic numbers

Test covering chapters 1 and 3.

Indicate how the configuration of electrons around the nucleus depends on the principle quantum number, the orbital, and the spin.
Discuss Heisenberg's uncertainty principle and Pauli's exclusion principle.
Show the relationship between the principle quantum number, the sub-level, and the orbitals. List the orbitals as s,p,d,f and how how many of each are located in each sublevel.

Work a lab using the flame tests on a series of ions which demonstrate the wavelength of light energy given off when an electron moves from an excited state to a lower or ground state.
In class, introduce the Bohr atom theory showing the electron energy level(s) for hydrogen. Discuss the equation used to determine the energy in photons emitted by an electron, along with the determination of the frequency. Introduce Bohr's first quantum number, n, to indicate the energy levels,. Discuss why the Bohr theory only holds true for hydrogen.

Outline Bohr's proposed theory regarding the hydrogen atom and the energy levels allowable.
Discuss the ground state and the excited state, and how an atom will reach an excited state of energy.
Use Planck's formula to indicate how to determine the difference in energy between electron levels in hydrogen.
Introduce Bohr's quantum numbers for each level, and why Bohr's atomic theory only really works for hydrogen

I subbed for Joshua's chemistry class today. His sub plans were to complete pg. 130 #106, pg. 131 #125-129, and pg. 140 #s 1-2. The questions were on isotopes and radioactive decay.

Discuss the wave/particle theory of light. Use diagrams to list and then define the main characteristics of waves. These include the wavelength, amplitude, and frequency.
Present the formula which relates the frequency and wavelength to the velocity.
Introduce the quantum concept, Quanta, and photon.
Discuss Planck's formula and how it applies to the photoelectric effect. Discuss the threshold value for photons to release a photoelectron from a metal surface.

Discuss atomic mass units and how that differs from atomic mass.
Elicit how the atomic mass is determined from the weighted average of all the natural isotopes in a sample.
Use chlorine as the example and show how to determine the atomic mass step by step.
Have Joshua work a problem involving boron to arrive at the atomic mass.
Discuss Carbon -12 as the element used to compare all element atomic mass units to.
Relate that the AMU 's are whole numbers based on the number of protons and neutrons in the atom.

Lab to determine the percent by mass of carbon in a sample of glucose.
Calculations and math formulas are derived

Outline and discuss the original formation of ions using a cathode ray tube and high speed electron collisions with a metal.
Define isotope in terms of protons and neutrons. Show how symbols are used to indicate the atomic mass and the atomic number. Use the symbols to key the elements and their isotopes.
Use a series of examples.