1. IONIC BONDS ION - charged atom
1. Bonds formed by transferring electrons between atoms
2. Electronegativity difference is approx. > 2.0
3. Metal + Nonmetal Metal loses e Nonmetal gains e-
ION - charged atom
1. Cation (+ charge); metal Na Ca Al+3
Sodium Ion Calcium Ion Aluminum Ion
2. Anion (- charge); nonmetal I S P-3
Iodide Ion Sulfide Ion Phosphide Ion
3. Results in Noble Gas electron configuration for each atom
K: 1s22s2p63s2p64s1
19 p e-
Cl: 1s22s2p63s2p5
17 p e- e- e-

2. e- e- e-
19 p e-
K+1:1s22s2p63s2p6
17 p e-
Cl-1: 1s22s2p63s2p6
Now, both exhibit Noble Gas e- configuration
“8 valence electrons”
complete filled s & p orbitals
Ionic compounds are composed of “ions”

3. NAMING IONIC COMPOUNDS
IA + VIIA COMPOUNDS
Combine in 1:1 ratio High melting point >5000C
NAMING IONIC COMPOUNDS
BINARY
REGULAR METAL (1 charge)
1st: Name of element
2nd: Name changed to -ide ending
SrI2
Strontium Iodide
IRREGULAR METAL (2+ charges)
1st: Name of element
common name w/ roman numeral
or “derived name”
2nd: Name changed to -ide ending
Pb3P2
Lead II Phosphide
Plumbous Phosphide

4. Metallic Elements & Charges to Know+1 H +2 +3 Li Na Mg
+6,2,3
+2,3
+2,3
+2,3
+1,2 Al K Ca Cr Fe Co Ni Cu Zn Ag Sn Ba Au Hg Pb
+1,2
+2,4 U

5. Nonmetallic Elements & Charges to Know
+4,-4 He Ne Ar Kr Xe Rn -3 -2 -1 C N O F Si P S Cl Br I

6. Elements & Charges to Know+1 H
+4,-4 He Ne Ar Kr Xe Rn +2 +3 -3 -2 -1 Li C N O F Na Mg
+6,2,3
+2,3
+2,3
+2,3 Al Si P S Cl
+1,2 K Ca Cr Fe Co Ni Br Cu
Zn+2
Ag+1 Sn I Ba Au Hg Pb
+1,2
+2,4 U

7. POLYATOMICS radicals, polyatomic ions
Group of 2+ elements combined together to make a group with an overall charge
SO SO NO NO PO PO4-3
Sulfite Sulfate Nitrite Nitrate Phosphite Phosphate
OH CO HCO3- 1
Hydroxide Carbonate Hydrogen Carbonate or Bicarbonate
C2H3O O2-2
Acetate Peroxide
Halide Pattern
ClO hypochlorite
ClO2 chlorite
ClO3 chlorate
ClO4 perchlorate
fluorine fluor
bromine brom
iodine iod

8. NaCl ine ide BaF2 ine ide 2nd: Element name, ending
NH3: Ammonia NH4+1: Ammonium Ion
Complete Molecule Itself Polyatomic Ion; needs Anion to complete cmpd.
NH4Cl NH4C2H3O (NH4)2SiO3
Ammonium Ammonium Ammonium
Chloride Acetate Silicate
2nd: Element name, ending
changed to “–ide”
1st : Name of element
NaCl
ine
ide
Sodium
Chlor
BaF2
Barium
ine
ide
Fluor

9. MULTIPLE CHARGED METALS
IRREGULAR METALS
Metals w/ 2 or more charges
Use: 1) Roman Numeral to indicate the charge
2) Derivative Name
Copper I
Copper II
Iron II
Iron III
Cuprous
Cupric
Ferrous
Ferric
-OUS lowest charge
-IC highest charge

10. Fe2O3 FeO Fe2 O3 Fe O No subscripts +3 +2 -2 -2 charge “O” –2
= charge “Fe” +2
Charge on “Fe” = +3
Iron III Oxide
Ferric Oxide
Iron II Oxide
Ferrous Oxide

11. . . . . . . . . . . Na3PO4 Mg(NO2)2 Sodium Phosphate Magnesium Nitrite
REGULAR METAL
FeSO Fe2(SO3)3
Iron II Sulfate Iron III Sulfite
Ferrous Sulfate Ferric Sulfite
IRREGULAR METAL
Electron Dot Structure
Use the total # of valence e-’s
Cl: 1s22s2p63s2p5
Recall writing e- structure:
& Hund’s Rule
K: 1s22s2p63s2p64s1 . . . . . . K Cl . .
Use chem. symbol & # valence e-: K . Cl .

12. ACIDS -- BASES Acid: 1st element, cation, is “H+1” Base: Metal + OH
Anion, OH-1
Ca(OH) LiOH CuOH
Calcium Hydroxide Lithium Hydroxide Copper I Hydroxide
Cuprous Hydroxide
Oxides IA Peroxides
Li2O Lithium Li2O2
Na2O Sodium Na2O2
K2O Potassium K2O2
Oxide Peroxide
O O-1---> O2-2
NH4OH
Ammonium Hydroxide
MnO4-1: Permanganate
MnO4-2: Manganate
Mercury I or II
Hg Hg+1--Hg+1 Hg2+1

13. Halogen Acid Pattern
F, Cl, Br, I
1 “O”
2 “O”
3 “O”
4 “O”
-ClO3
-ClO
-ClO2
-ClO4
Hypochlorite
Chlorite
Chlorate
Perchlorate
Hypochlorous
Acid
Chlorous
Acid
Chloric
Acid
Perchloric
Acid
-ITE
Change ending to “OUS”
-ATE
Change ending to “IC”

14. Sn+2SO4-2 Sn+4SO4-2 Sn2(SO4)4 Sn(SO4)2 SnSO4 REVIEW HIGHLIGHTS
Simple Ion: single atom or element w/ associated charge
F Ca Sb+3
Complex Ion: group of elements w/ overall charge
C2H3O NH OH-1
Molecule: covalent; nonmetal + nonmetal
atoms combine in any ratio, not simplest ratio
C2H C4H C4H8
Formula Unit: compound; ionic; metal + nonmetal
atoms always combine in simplest ratio
Tin II Sulfate Tin IV Sulfate
Sn+2SO4-2
Sn+4SO4-2
Sn2(SO4)4
Sn(SO4)2
SnSO4
Reduce added subscript number to lowest form

15. IONIZATION ENERGY ELECTRON AFFINITY
E required to remove e- from atom in its gaseous state
Na + E > Na+1 + e Mg + E > Mg+2 + 2e-
Trend: increases L2R across row decreases down column
ELECTRON AFFINITY
E released when gaining an e- to an atom in its gaseous state
O + 2e > O-2 + E Br + e > Br-1 + E
The Z=5, 6, 7, group 4A, & group 7A elements not easily gain or lose e-
Tend to form Covalent Bonds

16. OXIDATION - REDUCTION “REDOX”
Reduction: gain electron Oxidation: lose electron
H2(g) + O2(g) > H2O(g)
Both H2 & O2 are diatomics: charge on each 0
In the cmpd. H is +1 & O is -2
H: from 0 to +1 charge, loses e-, oxidized (reducing agent)
O: from 0 to -2 charge, gain e-, reduced (oxidizing agent)
Four IONs that play an important role in biochemical processes
Na+1
Ca+2
K+1
Mg+2

17. REDOX – Reduction/Oxidation
LEO
the lion says
GER-r-r-r-r-r
Gain
Electron
Reduce
Lose
Electron
Oxidize

18. REDOX – Reduction/Oxidation
OIL
RIG
Oxidize Is
Lose
Reduce Is
Gain