Download Naming Ionic Compounds with Transition Metals

*Transition metals are unusual because
many of them are able to form several
different ions.
*Iron has two different charge options, it
can form Fe+2 or Fe+3 ions.
*In order to know the charge of the
metal, it has to be given in the name.
*The bracket system makes it easy to
find formulas of transition metal
compounds.
*The charge of the metal is given in the
name as a Roman numeral.
*The charge of the non-metal is from the
periodic table like normal.
*Example:
Copper (II) chloride
*The charge of the copper ion is +2 from
the Roman number
Cu+2 Cl-1
CuCl2
Crossover the numbers to
get the formula
1. Nickel (III) sulfide
Ni2S3
2. Chromium (II) bromide
3.
CrBr2
Manganese (IV) fluoride
MnF4
4. Copper (II) oxide
Cu2O2 reduces to CuO
*When we name a transition metal ionic
compound, we MUST include the charge
of the metal ion in brackets.
*The charge is given as a Roman number.
Co2O3
these two elements are
cobalt and oxygen, so
the name will be
cobalt ( ) oxide
Co2 O3
Reverse crossover the
charges UP to see what
the charge will be
for each element
Co+3 O-2
*the cobalt has a +3 charge
*We need to check that the
charge on the non-metal is
correct. Oxygen does have
a -2 charge.
The name will be:
Cobalt (III) oxide
1.FeO
*Iron (II) oxide
2.Ni2O3
*Nickel (III) oxide
3.MnBr4
*Manganese (IV) bromide
4.NiO
*Nickel (II) oxide
5.AuF
*Gold (I) fluoride