Review definition of polyatomic ions.
Using table of polyatomic ions, their chemical names and charge, demonstrate in precise steps the method used to write the correct chemical ionic formula for the compound formed between some typical cations and polyatomic anions.
Distribute HW sheet and work a few typical examples of the way to form, and correctly write, the ionic formulas.
Indicate the correct chemical names along with the common name ofter used.

Fill in class activity sheet which requires Lewis dot formulas to be sketched for a variety of atoms. The valence electrons are determined by using the periodic table.
Introduce polyatomic ions. Define the term and use examples of some common polyatomic ions to strengthen the definition.
Stress the importance of allocating the charge to the total ion, which is placed in parenthesis.

Lab demonstrating the formation of ions by showing the property of electrical conduction when ionization occurs. A sample of purified water is tested for conductivity as a base solvent. A variety of solids in powder form are tested for conductivity using a voltmeter. The substances all proved to be non conducting. After solution formation, each was tested again with the results noted. All solutions which now demonstrated conductivity were noted and their ionization formulas written to show ions formed.

Elicit definition of valence numbers for an atom.
Outline how the valence numbers can be determined from the group number.
List the positive valence numbers and the negative valence numbers for groups 1,2,13,15,16,17.
Practice writing ionic formulas using Lewis dot formulas and a net zero charge.

Explain how the group numbers and the period numbers can be used to determine the valence electrons in an atom.
Discuss the division of the periodic table into metal an non metal atoms.
Show how metal atoms lose electrons and non metal atoms gain electrons to. become ions.
Discuss the Lewis dot formula of atoms
Use pre printed blank atom energy level diagrams to show the formation of ionic bonds.
Review the definition of bond and ionic bond

Review how atoms will form ions, by losing or gaining electrons.
Sketch the atomic configuration for argon, an inert gas, and also sketch along side it the configuration for sodium with 1 electron less, and chlorine containing one electron more.
Review the octet rule. Determine the charge on the sodium ion and the charge on the chloride ion.
Demonstrate the transfer of one electron from sodium to chlorine, the bond formed by the opposite charge attractions, the completion of the octet for each atom, and indicate that the bond is an ionic bond.
Define ionic bond.

Review definition of valence electrons and valence shells or energy level.
Review maximum electrons which can be placed into each of the primary quantum level shells.
Use neon as the primary example, show the electron configuration of sodium (one electron greater than neon) and fluorine (one electron less than neon). Indicate that sodium can obtain a stable neon configuration by donating an electron, and fluorine can obtain stability ( reach an octet) by accepting an electron.

Define valence shells and and valence electrons.
List the maximum number of electrons which each principle energy level may contain.
Use examples of atoms from atomic number 1 to atomic number 10 to show the electron configuration in each primary quantum number shell.
Sketch the electron configuration found in neon, argon, krypton and xenon. Note the presence of 8 electrons and state the octet rule

View video which reinforces the concepts of primary energy levels, sub levels, and orbitals.
Work a series of electron configuration problems, starting with the simplest, hydrogen, and working up to more complex atoms.
Use a printout of the sub shell and orbital energy levels to aid the placing of electrons in the proper orbitals.

Review the 3 major principles for assigning electrons to an atom.
Introduce orbitals, their letter designations and how many electrons can be placed in each orbital. Write the electron configuration for 5-6 sample atoms, using both the numerical and the electron position diagrams.
Use the lab to view the energy released when neon, argon, and hydrogen are excited in the vapor form. View the radiant energy released using the student spectroscope.