The document discusses valence electrons and how they are involved in bonding. It explains that the number of valence electrons is equal to the group number for main group elements. Binary salts are formed through ionic bonding as metals lose electrons to form cations and nonmetals gain electrons to form anions. The charge on ions is the group number for positive ions and the group number minus 8 for negative ions. Compound formulas are written with the metal cation written first followed by the nonmetal anion. A homework worksheet is assigned to practice naming ionic compounds.

1. 6/14/2011
VALENCE ELECTRONS
• Outer shell e- are involved in “bonding”
• Gain/lose/share
• # e- in atom =
• e- seem to be arranged in energy levels
• Highest energy level electrons
• Largest distance from + nucleus
• “A” group number = # valence electrons
• (“A” groups are “main” group elements)
FORMULAS FOR BINARY SALTS
• Ionic bonding
• Cation – Metals lose e- fairly easily
• Anions – Nonmetals attract e-
Pg 35-39
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CHARGE OF IONS
MAIN GROUP ELEMENTS
• Positive charge = + group number
• Negative charge = group # - 8
FORMULAS FOR COMPOUNDS
• Metal + Nonmetal
• Metal loses e- to non-metal
Na Cl
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3. 6/14/2011
HANDOUT PRACTICE
Name Cation Anion formula
Sodium bromide
Calcium iodide
Barium oxide
Aluminum chloride
Lithium nitride
Magnesium sulfide
Strontium fluoride
OTHER METALS
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4. 6/14/2011
• Iron (III) chloride
• Lead (IV) sulfide
• Lead (II) sulfide
• Cr2O3
• MnO2
All metals except Group IA, IIA, Al, Ag, Zn, Cd should
use RN in their names – these can all have variable
“oxidation” numbers (charges)
POLYATOMIC ION
• Note root/suffixes
• Group has the charge
• Covalent bonding within group
• Overall extra electrons or too few electrons
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5. 6/14/2011
• Sodium sulfate
• Calcium bicarbonate
• Ammonium phosphate
• Manganese (IV) oxide
• FeSO4 Fe2(SO4)3
• Sodium oxalate
Pg 137 – common compounds
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6. 6/14/2011
Homework – answers will be on bb
– but Please do the worksheet
before looking at the answers
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7. 6/14/2011
REVIEW NAMING
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