1. Unit 3 ~ Nomenclature (Ch. 5)
And you

2. 3-1 Overview of the Periodic Table(Section 4.8, 4.9, 4.10, 4.1)
The outermost electrons are called valence electrons.
A completely filled valence level = chemically stable or inert.
Elements are arranged in order according to the number of protons (atomic #).
Elements with similar chemical properties are arranged in the same column (also called a group or family).
The group number at the top of the each column indicates the number of valence (outermost) energy level electrons.
Atoms without filled valence (outer) energy levels will lose, gain, or share valence electrons to reach stability, a full valence level.

3. The families

4. The ion table Group gain or loss ion formed name 1 loss of e- + cation
loss 4 most, gain 4 C, Si (in general)
gain 3 e anion
gain 2 e anion
gain 1 e anion

5. Noble gases (group 8) have filled outer energy levels and are therefore very stable and unreactive (inert). 
Transition metals form cations (+ ions) that can vary in charge
With the exception of the inner steps:
Ag+ , Zn+2 ,Cd+2, Al+3, Ga+3, In+3
ALWAYS!!!!!!

6. Metals, Nonmetals, and Metalloids
The zigzag staircase separates metals from nonmetals.
Metals found to the left of the staircase. Properties of metals include shiny (luster), malleable (can be bent), ductile (can be drawn into a wire), and conduct both heat and electricity.
Nonmetals found to the right of the staircase.
Metalloids are all the elements along the border of the zigzag staircase except Aluminum (Al), which is a metal. Metalloids have properties of both metals and nonmetals

8. 3-2 Ionic Bonding (12.1)  
Na + Cl → [Na+][ Cl - ] Mg + Br  [ Br - ][Mg ][ Br - ] Br +2

9. By alternating the + cation with the – anion, you are showing how the ions alternate in the solid, crystal lattice of an ionic compound.

10. Metals metalloids non metals

11. 3-3 Naming Ionic Compounds ~ Type/Class 1 Rules (Section 5.2)
The following Class 1 rules apply to ionic bonds, in particular, a “predictable”
metal + nonmetal.
 Metal cation (+) first; nonmetal anion (-) with “ide” ending. 

12. NaCl
Sodium cation and chlorine anion (Chloride) form:
Sodium Chloride

13. CaCl2 = Calcium chloride
Calcium cation and chlorine anion (chloride) form
Calcium chloride

14. AlBr3
Aluminum cation and Bromine (bromide) anion form
Aluminum Bromide

15. Formulas
Write the metal with its charge and the nonmetal with its charge.
Balance the charges.
The sum of charges for an ionic compound must = zero!
For ionic compounds, reduce subscripts to simplest form.

16. Lithium fluoride = Li+ + F- = LiF
Magnesium iodide = Mg+2 + I- + I- = MgI2
Potassium oxide = K+ + K+ + O = K2O
Beryllium sulfide = Be S = BeS
Silver nitride = Ag+ + N-3 = Ag3N
Aluminum chloride = Al Cl - = AlCl3
Strontium Oxide = Sr O = SrO
Gallium Oxide = Ga O-2 = Ga2O3