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Ionic Compounds: Naming

Ionic Compounds: Naming. Naming Binary Ionic Compounds. Always name metal [(+) cation] first 2. Write stem of non-metal [(-) anion] 3. Add ending “ ide ” to non-metal. Stems of nonmetals. The First Step in Naming. Find metal on PT

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Ionic Compounds: Naming

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  1. Ionic Compounds: Naming

  2. Naming Binary Ionic Compounds • Always name metal [(+) cation] first 2. Write stem of non-metal [(-) anion] 3. Add ending “ide” to non-metal

  3. Stems of nonmetals

  4. The First Step in Naming • Find metal on PT • If metal has only one oxidation state it’s easy • If metal has more than one oxidation state, there’s an extra step

  5. Metals with one oxidation state(name metal, stem non-metal, add “ide”) • CaO • BaS • AlN • LiCl • Al2Se3 • Na2O • K3N • MgF2 calcium oxide barium sulfide aluminum nitride lithium chloride aluminum selenide sodium qxide potassium nitride magnesium fluoride

  6. Metals with more than 1 oxidation state • figure out which oxidation # for metal ion • Ex: Fe can be Fe+2or Fe+3 • FeO and Fe2O3 • two different compounds • cannot name both iron oxide • every formula has 1 name only

  7. FeO and Fe2O3 • Compounds are electrically neutral • Oxygen is -2 1 O which is -2 FeO so Fe must be +2 Name: iron (II) oxide (roman numeral II represents +2 charge on Fe)

  8. each Fe is +3 iron (III) oxide FeO and Fe2O3 • Compounds are electrically neutral • Oxygen is -2 each O is -2 Fe2O3 3 O’s 3(-2) = -6 total negative charge total positive charge must be +6

  9. Name the following titanium (III) chloride • TiCl3 • Mn2O4 • Co2O3 • PdBr2 • AuCl3 • MoN • MnO • TiO manganese (IV) oxide cobalt (III) oxide palladium (II) bromide gold (III) chloride molybdenum (III) nitride manganese (II) oxide titanium (II) oxide

  10. SO42- CO32- PO43- OH1- POLYATOMIC IONS • Table E: groups of covalently bonded atoms that have a charge (+) or (–) • polyatomic ions have “names” • (-) polyatomic ions can form ionic bonds with (+) metal ions

  11. Ternary Compounds • contain 3 or more elements • usually contain a polyatomic ion • if polyatomic is (+) it’s bonded to a non-metal • if polyatomic is (–) it’s bonded to a metal • sometimes 2 polyatomics are bonded together

  12. Formulas with polyatomics • What’s the formula for the compound formed from Al+3 and SCN-1? • The charges must add up to zero, so write the symbols, positive first! Al(SCN)3

  13. Try a few more: NaOH • Na+1 and OH-1 • K +1 and HCO3-1 • Mg+2 and CO3-2 • Li +1 and NO3-1 • Ca+2 and SO4-2 KHCO3 MgCO3 LiNO3 CaSO4

  14. These are more challenging: Mg3(PO4)2 • Mg+2 and (PO4)-3 • Al+3 and (NO3)-1 • Fe+2 and OH-1 • Hg2+2 and SCN-1 • Mg+2 and HCO3- • Al+3 and C2O42- Al(NO3)3 Fe(OH)2 Hg2(SCN)2 Mg(HCO3)2 Al2(C2O4)3

  15. More challenging Zn(NO3)2 • zinc + nitrate ion • magnesium + hydroxide ion • lithium + carbonate ion • potassium + sulfateion • calcium + phosphate ion • beryllium + chlorate ion Mg(OH)2 Li2CO3 K2SO4 Ca3(PO4)2 Be (ClO3)2

  16. Naming compounds with polyatomics • polyatomic ions have names (Table E) • Naming similar to binary naming • Rules: • positive always written first • if (+)’ve ion is a metal, check to see how many oxidation states it has • if more than 1, need roman numeral • if (–)’ve ion is polyatomic - 2nd part of name is name of polyatomic (don’t modify ending)

  17. Name the following sodium hydroxide • NaOH • KHCO3 • LiNO3 • CaSO4 • Al(NO3)3 • Fe(OH)2 • CuSO4 • CuSCN potassium hydrogen carbonate lithium nitrate calcium sulfate aluminum nitrate iron (II) hydroxide copper (II) sulfate copper (I) thiocyanate

  18. Summary for Binary Ionic Compounds • Compounds are electrically neutral • Formula: positive ion goes first • If metal has more than 1 oxidation state, name has roman numeral • Name = metal + stem of nonmetal + ide

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