Ionic Compounds with Transition
Metals
P 83
What is different about transition
metals?
• Transition metals are located in the “d” block on the
periodic table. Since they are filling the energy level
that is NOT valence, there is some instability in the
electrons… they sometimes will move into the
valance rather than the “d” sublevel.
• Due to this, transition metals will often have more
than one charge. For example, Iron can have either
a +2 or +3 charge.
• Therefore, the rules for naming transition metals
must consider the charge of the transition metal as
part of the name
Elements in Groups 3-12
• Write the name of the first element in
the compound
• Determine the charge through “reverse
crossing out”
• Use a Roman numeral in parentheses
after the first name of the compound to
represent the charge of the positive
element
Elements in Groups 3-12 (cont)
• Write the root of the 2nd element in the
compound
• Add the ending –ide to the root of the
name of the 2nd element
Examples
• NiO = nickel (II) oxide
• Ni2O3= nickel (III) oxide
• FeO = iron (II) oxide
• Fe2O3 = iron (III) oxide
How do you know the charge to
write a formula?
• Look at the Roman numeral in the
name. That is the charge of the metal.
• Silver and Zinc both have “fixed”
charges – that is, they don’t have more
than one charge. Their charge is
always +1.