Introduce the quantum atomic theory. Discuss the ground state of the atom and the principle energy levels determined by their distance from the nucleus.
Using an analogy of an apartment building, introduce sub levels as the number of apartments on each floor. Then introduce orbitals as the rooms in the apartments. List the letters used to identify the orbitals, and how many orbitals can be located in each sub level, and the maximum number of electrons present in each orbital.

This morning, Joshua worked in his Chemistry textbook to answer 8 standardized test questions. He began reading on page 132 to answer multiple choice questions 6,7,8, and 10, and then he worked on page 133 to answer questions 11, 12, 13, and 16. Joshua worked independently and was challenged by only one question.

Multiple choice test on unit 1

Discuss ground state and excited electrons. Indicate how when electrons are excited they are raised to a higher energy level around the nucleus. Elicit when the electron returns to its original, more stable energy level, the energy is emitted in the form of light of various frequencies. Discuss briefly Heisenberg's principle and why the exact location of an electron cannot be positioned.
Use the lab to view the light emitted by different metal ions as the electrons in each are excited and then returned to ground state. The flame test is used.

Review all aspects of the atomic theory up to this point through a series of questions and answers. Introduce the Bohr theory of the atom by writing his hypothesis on the board and discussing the outline of the theory.

Review determination of the atomic number as the number of protons, and the atomic mass as protons plus neutron found in the nucleus.
Elicit a formula for finding the number of neutrons given the atomic number and the atomic mass.
Show how the information for an atom is designated in the atomic symbol box for each atom.
Discuss isotopes and the difference between atomic mass and atomic mass units.
Have Ben solve 2-3 problems determining the atomic mass, the number of protons and electrons, and the number of neutrons only.

Discuss the proton and the determination of the atomic number of an atom.
Introduce the neutron, its mass and lack of charge. Locate it in the nucleus.
Discuss the difference between atomic mass and atomic mass units.
Define how to determine the atomic mass units from the nucleons.
Introduce isotopes.
Explain how the atomic mass (weight) is the sum of the averages of the percentages of neutrons in the nucleus.
Explain the 3 isotopes of hydrogen, and what heavy water is. Discuss the importance of heavy water in collecting heavy hydrogen to produce a nuclear weapon.
View crash course video on early atomic theory

Review the discovery and naming of the electron.
Discuss properties of this sub-particle.
Examine Rutherford's scattering using a diagram. Explain the results and elicit the definition of the atomic nucleus from the data presented by Rutherford.
Discuss the size of the nucleus compared to the size of the atom.

Discuss the electrical neutrality of matter, and how matter can be charged.
Display a photo of a Crooke's tube and explain how the beam of light is produced from the Cathode. Display a magnet bending the ray of light, either toward it or away.
Discuss how the beam must be composed of negative particles.
These particles were released from the metal electrode by the electric current, so they must have been present in the metal atoms. This was the fist indication that the atom was composed o a subatomic negative particle labeled the electron.
The Thompson chocolate chip cookie model of the atom is then presented by Thompson.

Work the calculations from Wed. lab using the experimental numbers.
Work the calculations for the % of carbon in glucose using the atomic mass units as found in the periodic table.
Present the formula on the board and have Ben do all the calculations using a calculator.
Introduce the early thoughts on the atom as presented by Democritus 2000 years ago.
Write a definition for the atom.