1. Ionic Bonds and Nomenclature
Unit 2 Notes

2. IONIC BONDING
Ionic Bond - strong attraction (electrostatic attraction) formed between a cation (+) and anion (-)
The cation and anion are formed when a metal donates electrons to a nonmetal in order to fulfill the octet rule (8 valence electrons)

3. IONIC BONDING
The cation and anion are formed when a metal donates electrons to a nonmetal in order to fulfill the octet rule (8 valence electrons)
Extra e-
Needs one more e-
Valence shell
Valence shell
Full valence
shells (8 e- )

5. Oxidation State - the charge that an atom forms

6. Determine the oxidation states of cation & anion
STEPS TO WRITING IONIC FORMULAS for TYPE I BINARY COMPOUNDS
Determine the oxidation states of cation & anion
Balance the charges of your cation and anion so that the overall charge of the ionic compound is ZERO
Write the symbol of the cation first and the anion second with the correct number subscript from balancing the charges (if the subscripts are equal, they cancel!)

7. Examples Cation Anion Cation Charge Anion Charge Formula Magnesium
Chlorine
Lithium
Phosphorus
Francium
Oxygen
Barium
Nitrogen
Cesium
Selenium

8. STEPS TO WRITING IONIC NAMES for TYPE I BINARY COMPOUNDS
Identify the cation and anion
Name the cation by its element name
Name the anion by changing the last part of its element name to “-ide” (ex. “Bromine” changes to “Bromide”)
Write down the full name of the ionic compound by writing the cation name first and the anion name second
Ca + Br = CaBr2 Mg + O = MgO Al + O = Al2O3 Be + N = Be3N2

9. Examples Cation Anion Cation Charge Anion Charge Formula Name
Magnesium
Chlorine
Mg+2
Cl-1
MgCl2
Lithium
Phosphorus
Li+1
P-3
Li3P
Francium
Oxygen
Fr+1
O-2
Fr2O
Barium
Nitrogen
Ba+2
N-3
Ba3N2
Cesium
Selenium
Cs+1
Se-2
Cs2Se

11. Ag will always form a +1 charge and Zn will always form a +2 charge
Transition metals (d-block) can form many different oxidation states. Therefore, their oxidation state will always be given.
Exceptions!
Ag will always form a +1 charge and Zn will always form a +2 charge

12. STEPS TO WRITING IONIC NAMES for TYPE II BINARY COMPOUNDS
Same as Binary compounds except you must add the roman numerals in parentheses after the cation
Examples:
CuCl2
Fe2O3
Fe2O3 Iron (III) oxide
CuCl Copper (I) chloride
CuCl2 Copper (II) chloride
PbS Lead (II) sulfide
PbS2 Lead (IV) sulfide

13. POLYATOMIC IONS
Group of atoms that together form a single ion with a positive or negative charge
Always goes in parentheses if more than one

14. STEPS TO WRITING IONIC NAMES for TERNARY (POLYATOMIC) COMPOUNDS
Follow the same steps for naming as before, using the given charge of the polyatomic,
except you NEVER change the name of the polyatomic while naming!
Na2SO4 sodium sulfate
KH2PO4 potassium dihydrogen phosphate
Fe(NO3)3 iron (III) nitrate
Mn(OH)2 manganese (II) hydroxide
Na2SO3 sodium sulfite
Calcium hydroxide Ca(OH)2
Sodium phosphate Na3PO4
Ammonium dichromate (NH4)2Cr2O7
Cobalt (II) perchlorate Co(ClO4)2
Copper (II) nitrite Cu(NO2)2

15. Examples Cation Anion Cation Charge Anion Charge Formula Name Lithium
Sulfate
Ammonium
hydroxide
Magnesium
Phosphorous
Iron (III)
Nitrate
Zinc
Chlorite