2. Everything has a Name
Elements can combine to form millions of different compounds
The tiniest units of a compound that still retains the characteristics of the compound are:
molecules or
formula units composed of charged atoms i.e. ions

3. Molecular Compounds
are substances that are composed of a single kind of molecule.
their molecules are made up of 2 or more atoms that act as a unit
the units are electrically neutral
have low melting and low boiling points
exist as solids, liquids or gases at room temperature

4. Ions and Ionic Compounds
not all compounds are molecular
some compounds are made up of formula units that are groups of charged particles called ions
an ion forms when an atom gives up or accepts one or more electrons

5. Positive Ions Metal atoms tend to lose electrons
and become positively charged i.e. cations
e.g. Li Li+1
lithium atom lithium ion
p+ = p + =
e - = e - =
n0 = n0 =

6. +1

7. Negative Ions Nonmetallic atoms tend to gain electrons
and become negatively charged i.e. anions
e.g. Cl Cl-1
chlorine atom chloride ion
p+ = p + =
e - = e - =
n0 = n0 =

8. -1

9. Positive Ions Mg Mg+2 magnesium atom magnesium ion p+ = p + =
e - = e - =
n0 = n0 =

10. +2

11. Negative Ions O O-2 oxygen atom oxide ion p+ = p + = e - = e - =
n0 = n0 =

12. -2

13. 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 lithium ion

14. Naming Negative Ions
The name of the anion uses the root of the element and the ending -ide plus ion
oxygen oxide ion
fluorine fluoride ion

15. +2, +3
+1, +2

16. 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+3
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

17. Practice Naming Simple Ions

18. Polyatomic Ions
Collections of tightly bound atoms that behave as a unit and carry a charge
examples
SO3-2 sulfite ion SO4-2  sulfate ion
NO2 -2  nitrite ion NO3-1  nitrate ion
ClO2-1  chlorite ion ClO3-1  chlorate ion

19. Complicated Ions Polyatomic Ions Formula Name H2PO4-1
dihydrogen phosphate ion
PO3-3
phosphite ion
PO4-3
phosphate ion
C2H3O2-1
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
Complicated Ions
Polyatomic Ions

20. Complicated Ions Common Acids Common Acids Formula Name HCl
hydrochloric acid
H2CO3
carbonic acid
H3PO4
phosphoric acid
HC2H3O2 or CH3COOH
acetic acid
H2SO4
sulfuric acid
HNO3
nitric acid

21. Practice Naming Polyatomic Ions and Acids