1. Special ions Some transition metals lose different numbers of electrons when they become ions, because they don’t have normal valence electrons They can have different charges as cations, and must be written with roman numerals representing their charge Examples: Ti 3+ = Titanium IIIFe 2+ = Iron II W 6+ = Tungsten VI Mo 5+ = Molybdenum V Cu + =Copper IV 4+ =Vanadium IV

2. Name  Formula Yttrium (III) nitride copper (I) bromide Gold (I) phosphide Chromium(II) fluoride YN CuBr Au 3 P CrF 2

3. Name these 2 compounds: CoS a.Figure out which ions form the compound because the ion charge could be important. Since S forms S 2-, Co must be Co 2+ b. Name the ions, cation first, then anion c. Change ending to –ide if it’s a pure element. cobalt (II)sulfide d. Transition metals always get a roman numeral to indicate their charge! Na 2 SO 4 sodium sulfate <-correct Common mistakes: sodium(II)sulfate sodium(I)sulfate sodium sulfide

4. Formula  Name Na 2 O CuS LiBr CuCl Sodium Oxide Copper (II) Sulfide Lithium Bromide Copper (I) Chloride

5. Name  Formula Ammonium Phosphate Iron (II) Nitrate Sodium Sulfate Silver Acetate (NH 4 ) 3 PO 4 Fe(NO 3 ) 2 Na 2 SO 4 AgC 2 H 3 O 2

6. Formula  Name Fe(OH) 3 Mg(NO 3 ) 2 NiCO 3 Cd(HCO 3 ) 2 Iron (III) Hydroxide Magnesium Nitrate Nickel (II) Carbonate Cadmium (II) bicarbonate

7. Lattice Energy, Solubility, etc Transition metal cations work the same as regular metal cations in crystal lattices, lattice energy, and solubility Ex: VS has lower lattice energy than VS 2 –the charges in VS are 2+ and 2- while the charges in VS 2 are 4+ and 2- –Therefore VS is more soluble than VS 2