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Naming Binary Ionic Compounds: A Complete Guide

Learn how to name binary ionic compounds with clear steps and examples. Understand the rules for metals with one oxidation state and those with multiple states. Discover how to name polyatomic ions and tackle ternary compounds effortlessly.

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Naming Binary Ionic Compounds: A Complete Guide

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  1. Ionic Compounds: Naming

  2. Naming Binary Ionic Compounds • Always name the metal (the cation/+ ion) first 2. Write stem of nonmetal (the anion/ - ion) 3. Add the ending “ide” to the nonmetal

  3. Nitr Ox Fluor Phosph Sulf Chlor Arsen Selen Brom Tellur Iod Hydr is the stem for H Stems of nonmetals

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

  5. Metals with one oxidation state • CaO • BaS • AlN • LiCl • Al2Se3 • Na2O • K3N • MgF2 Calcium Oxide Barium Sulfide Aluminum Nitride Lithium Chloride Aluminum Selenide Sodium Oxide Potassium Nitride Magnesium Fluoride

  6. Metals with > 1 oxidation state • Use the formula to figure out which oxidation state the metal ion has • Ex: Fe can be Fe+2or Fe+3 • Name 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 = 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 There are 3 O’s 3 X (-2) = -6 Total negative charge Total positive charge must be +6

  9. Name the followingHint: Positive Always First 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- OH- POLYATOMIC IONS • group of covalently bonded atoms that have a charge • Table E: (+)’ve or (–)’ve • polyatomic ions have “names” • polyatomic ions can form ionic bonds with oppositely-charged ions

  11. Ternary Compounds • contain 3 or more elements • usually contain a polyatomic ion • if polyatomic is (+) it’s bonded to a nonmetal • 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 NH4+1 and Cl-1? • The charges must add up to zero, so just write the symbols, positive first! NH4Cl

  13. Try a few more: NaOH • Na+ and OH- • K + and HCO3-1 • Mg+2 and CO3-2 • Li + and NO3- • NH4+ and CN- • Ca+2 and SO4-2 KHCO3 MgCO3 LiNO3 NH4CN CaSO4

  14. These are more challenging: Mg3(PO4)2 • Mg+2 and (PO4)-3 • (NH4)+1 and S-2 • Al+3 and (NO3)-1 • Fe+2 and OH-1 • Hg2+2 and SCN-1 • Mg+2 and HCO3- • Al+3 and C2O42- (NH4)2S Al(NO3)3 Fe(OH)2 Hg2(SCN)2 Mg(HCO3)2 Al2(C2O4)3

  15. Be(ClO3)2 Some of the most challenging are Zn(NO3)2 • Zinc + Nitrate ion • Magnesium + Hydroxide ion • Lithium + Carbonate ion • Ammonium ion + Bromine • Potassium + Sulfate ion • Calcium + Phosphate ion • Beryllium + Chlorate ion • Ammonium ion + Sulfate ion Mg(OH)2 Li2CO3 NH4Br K2SO4 Ca3(PO4)2 (NH4)2SO4

  16. Naming compounds with polyatomics • polyatomic ions have names (Table E) • naming is parallel to binary naming • positive always written first • if (+)’ve ion is a metal, check to see how many oxidation states it has • if > 1 name must have a roman numeral • if (–)’ve 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 first, always • If metal has more than 1 oxidation state, name has a roman numeral • Name = metal + stem of nonmetal + ide

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