<p> NAMES AND FORMULAS FOR ATOMS WITH MORE THAN ONE VALENCE</p><p>Some metals can form more than one kind of ion (and therefore have more than one valence). These elements can create multiple compounds with the same element.</p><p>Table of Multiple Valence Ions Element Ionic charges Roman Numeral antimony (Sb) 3+, 5+ III, V arsenic (As) 3+, 5+ III, V chromium (Cr) 2+, 3+ II, III copper (Cu)*** 1+, 2+ I, II iron (Fe)*** 2+, 3+ II, III lead (Pb)*** 2+, 4+ II, IV manganese (Mn) 2+, 4+ II, IV mercury (Hg) 1+, 2+ I, II nickel (Ni) 2+, 3+ II, III tin (Sn)*** 2+, 4+ II, IV</p><p>Example If Iron “Fe” was to react with Chlorine “Cl” it can happen in different ways. Fe can be Fe2+ or Fe3+ so...</p><p>2+ 1- 3+ 1- (i) Fe + Cl (FeCl2)(ii) Fe + Cl (FeCl3)</p><p> Since both of these compounds cannot be called iron chloride we need a different way to name these compounds</p><p>Naming Multiple Valence Compounds 1. Use the reverse crisscross rule to determine the valence of the metal 2. Use the name for the metal 3. In brackets put the valence using Roman Numerals 4. Write the name of the non- metal with the “ide” ending 2+ 1- 3+ 1- (FeCl2) Fe + Cl (FeCl3) Fe + Cl Iron (II) chloride Iron (III) chloride Multiple Valence Compounds</p><p>Name the following Write the formulas for the following</p><p>1. SnCl2 ______1. Tin(II) sulphide ______</p><p>2. FeI3 ______2. Iron(III) oxide ______</p><p>3. SnH4 ______3. Lead (IV) fluoride ______</p><p>4. Pb3N2 ______4. Tin (II) oxide ______</p><p>5. Cu2O ______5. Copper(I) sulphide ______</p><p>6. CuO ______6. Copper (II) sulphide ______</p><p>7. PbS ______7. Iron (II) nitride ______</p><p>8. Cu3P2 ______8. Iron(III) nitride ______</p><p>9. PbCl4 ______9. Tin(II) nitride ______</p><p>10. FeF2 ______10. Tin(IV) phosphide ______</p><p>11. FeF3 ______11. Lead(II) phosphide ______</p><p>12. Cu4C ______12. Lead(IV) phosphide ______</p><p>13. Sn2Si ______13. Copper(I) silicide______</p><p>14. Pb3P4 ______14. Copper(II) chloride ______</p><p>15. SnC ______15. Tin(IV) chloride ______</p><p>16. PbBr2 ______16. Tin(II) bromide ______</p><p>17. PbBr4 ______17. Lead(II) bromide ______</p><p>18. CuBr ______18. Lead(IV) oxide ______</p><p>19. SnI2 ______19. Copper (I) oxide ______</p><p>20. CuS ______20. Copper (II) fluoride ______</p><p>21. Sb3P5 ______21. Manganese (II) phosphide______</p><p>22. AsN ______22. Manganese (IV) fluoride______</p><p>23. CrF2 ______23. antimony (III) oxide ______</p><p>24. MnO ______24. Nickel (III) oxide ______</p><p>25. Hg2O ______25. mercury (II) fluoride ______</p>