Ionic Compounds
Na+
by kind permission of Nick Kim.
Valence Electron Facts
 the electrons involved in
bonding
 The # of valence electrons is
the same as the group number
for the atom (1A, 2A, etc)
Valence Electrons and Metals
Electron Configuration & Lewis Dot
Structures of Metals
Symbol
Atomic No.
e config
Lewis dot
 H
1
1s1
H
 Li
3
1s2 2s1
Li
 Be
4
1s2 2s2
Be
 B
5
1s2 2s2 2p1 B
Naming Positive Ions
• The name of the cation is the same as
the name of the element plus the term
ion
• magnesium
magnesium ion
•
lithium ion
lithium
Negative Ions
 the electrons involved in
bonding
 The # of valence electrons is
the same as the group number
for the atom (5A, 6A, etc)
Valence Electron and Nonmetals
Electron Configuration & Lewis Dot
Structure of Nonmetals
Symbol
Atomic No.
e config
1s2 2s2 2p3
Lewis dot
N
7
N
O
8
1s2 2s2 2p4
O
F
9
1s2 2s2 2p5
F
Naming Negative Ions
• The name of the anion uses the root of
the element and the ending -ide plus
ion
• oxygen
ox ide ion
•
fluor ide ion
fluorine
Ionic Bonding
Ionic Bonding – the strong vs the weak
Ionic Bonding – e config style
Na
3p
3p
3s
3s
2p
2p
2s
2s
Na
1s
Cl
1s
Ionic Bonding – Lewis dot
style
Na + Cl 
+
Na
Cl
Ionic Bonding – e config style
Na
3p
3p
3s
3s
2p
2p
2s
2s
Mg
1s
Cl
1s
Ionic Bonding – Lewis dot
style
Mg + _Cl 
+2
Mg
+
Cl
_
More Ionic Bonding and
Lewis dot practice
 _K + _Cl 
 _Ca + _ Cl 
 _Ba + _F 
 _Na + _O 
Multivalent Ions
Metal Ions with more than one charge
Metal Ions with More than One Ionic Charge
- (Inner Transition and Metalloids)
Symbol
Stock Name
Classical Name
Cr+2
chromium (II) ion
chromous ion
Cr+3
chromium (III) ion
chromic ion
Mn+2
manganese (II) ion
manganous ion
Mn
manganese (III) ion
manganic ion
Fe+2
iron (II) ion
ferrous ion
Fe+3
iron (III) ion
ferric ion
Co+2
cobalt (II) ion
cobaltous ion
Co+3
cobalt (III) ion
cobaltic ion
Cu+1
copper (I) ion
cuprous ion
Cu+2
copper (II) ion
cupric ion
Hg+1
mercury (I) ion
mercurus ion
Hg+2
mercury (II) ion
mercuric ion
Sn+2
tin (II) ion
stannous ion
Sn+4
tin (IV) ion
stannic ion
Pb+2
lead (II) ion
plumbous ion
Pb+4
lead (IV) ion
plumbic ion
+3
Practice Naming Simple
Ions
Polyatomic Ions
Collections of tightly bound atoms that
behave as a unit and carry a charge
examples
SO3-2 sulfite ion
NO2 -2  nitrite ion
ClO2-1  chlorite ion
SO4-2  sulfate ion
NO3-1  nitrate ion
ClO3-1  chlorate ion
Complicated
Ions
Polyatomic Ions
Formula
Name
H2PO4-1
dihydrogen phosphate ion
PO3-3
phosphite ion
PO4-3
phosphate ion
-1
C2H3O2
acetate ion
HSO3-3
hydrogen sulfite ion
HSO4-4
hydrogen sulfate ion
HCO3-1
hydrogen carbonate ion
NO2-1
nitrite ion
NO3-1
nitrate ion
CN-1
cyanide ion
OH-1
hydroxide ion
MnO4-1
permanganate ion
ClO-1
hypochlorite ion
ClO2-1
chlorite ion
ClO3-1
chlorate ion
ClO4-1
perchlorate ion
HPO4-2
hydrogen phosphate ion
C2O4-2
oxalate ion
SO3-2
sulfite ion
SO4-2
sulfate ion
CO3-2
carbonate ion
CrO4-2
chromate ion
Cr2O7-2
dichromate ion
SiO3-2
silicate ion
IO2-1
iodite ion
NH4+1
ammonium ion
Practice Naming
Polyatomic Ions and Acids
Ionic Compounds
• composed of cations and anions
• electrically neutral
• total + charge = total – charge
• Strong vs weak forces (electronegativity)
• formula units
• usually solid at room temperature
• have high melting points
• conduct electricity