Discuss some atoms which have multiple oxidation states. Hand out table of multiple oxidations. Discuss rules for writing correct unit formulas for binary ionic compounds.
Outline and discuss the nomenclature for binary compounds and use specific examples. Introduce how to distinguish between multiple oxydation states by the use of roman numerals. Discuss with examples the use of "ic" and "ous" when naming iron oxide compounds.
Define polyatomic ions, how they react in a chemical reaction, how to write the correct formula which involves a polyatomic ion, an how to use the table of polyatomic ions to correctly write the formula and correctly name the compound,
Determination of differences in melting, boiling and hardness of ionic compounds based on intermolecular attraction strength which is a function of radii differences. Discuss how ionic compounds are formed by repeating patterns of ions, with no single ionic compound but with formula units. Discuss uni-positive, uni-negative, di-positive and di-negative ions. Define oxidation numbers and what an argonone represents.
Practice ionic compound formula determination by using ionic valences.
Discuss why ionic compounds are crystalline and not units.
View diagram of sodium chloride crystal.
Discuss lattice energy.
Determine why sodium fluoride has a greater lattice energy than the chl=oride or the iodide by determining the inter-ionic distances and graphing them vs. the lattice energies.
Elicit that the lattice energy is directly related to the size of the ions bonded, smaller ionic radii produce stronger inter-ionic forces and greater lattice energy.
Discuss physical properties as a function of inter-ionic forces, how strongly the particles are attracted to each other.
Complete reviewing the HW questions assigned.
Discuss how cations are formed, the position on the periodic table where atoms are found that produce cations. Discuss the formation of +2 and +3 ions by the transition metals, and how they are indicated on paper.
Show how anions are formed by the acceptance of electrons, usually into the s and p sub shells in the last primary quaantum energy level.
List group numbers 15,16,17, the number of valence electrons in each group, and how many electrons can be added to each atom in the different groups to produce an anion.
Define binary ionic compound and oxide.
Use examples to prove that in binary compounds, the net electric charge must be zero.
Discuss how the ionization energy of an atom was determined in the late 30's by bombarding ground state elements in the vapor phase with electrons of varying energy. The energy needed to "knock" an electron out of its valence orbit could be recorded for each of the elements. This energy became the ionization energy of the atom.
Introduce the energy which holds an electron added to the valence orbit. Define this as the electronegativity of the atom. View from a table the electronegativity values of both metal and non metal atoms. Elicit why non metals atoms will possess a higher value than metal atoms will.
Question how a neutral atom can become a positive or negative ion. Discuss the valence electrons and the valence electron orbitals.
Elicit from a sample configuration, what is required to remove a single electron from the last orbital.
Look up on a chart the energy required to remove a single valence electron from an atom of lithium.
Compare it to an atom of sodium, discuss why there is a difference.
Define first electronegativity.
Discuss why non metals have a higher electronegativity than metals.
View and discuss atomic radius increase and decrease.
Run a lab which demonstrates the ionization of sodium chloride compared to sucrose.
Determine why solid sodium chloride will not conduct a current but dissolved will.
Elicit why solid sucrose will not conduct a current, and neither will dissolved sucrose.
Show the non conduction of pure water.
Have Joshua define ions and how ions may form. Define and explain the chemical definition of a bond, and specifically an ionic bond.
Have Joshua write on the board the orbital electron designation for helium, neon, argon, and krypton. From the orbitals, write the Lewis dot formula for each.
Define inert elements, and note that each listed gas is classed as an inert gas.
Based on the Lewis formula, elicit that each atom has a completed valence electron shell, containing full s and p orbitals.
Explore the octet rule
Review chapter through the series of questions presented at the end of the chapter. Work configuration questions using both long orbital designation and noble gas designation. Examples also include Lewis dot diagrams, and how to determine the elements by their electron configurations
Session Minutes
45
Minutes Student Attended
45
Lesson Comments
Joshua sometimes works to quickly and becomes a little sloppy. He corrected all answers due to "quickness"
Work 3-4 configuration questions out of the text. Introduce the old definition and the newer definition for the term "valence electrons".
Discuss the Lewis dot method for showing the valence electrons in an atom.
Work through a number of questions which utilize the Lewis method of assigning valence electrons, and solving problems using the Lewis method.
