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Naming Ionic Compounds

Naming Ionic Compounds. Ionic Compounds. Ionic Bond: A bond that results from the attraction between cations and anions. Cations : Positively charged ions Metals or ammonium Anions: Negatively charged ions Nonmetals and polyatomic ion (excluding ammonium). Naming Ionic Compounds.

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Naming Ionic Compounds

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  1. Naming Ionic Compounds

  2. Ionic Compounds • Ionic Bond: A bond that results from the attraction between cations and anions. • Cations: Positively charged ions • Metals or ammonium • Anions: Negatively charged ions • Nonmetals and polyatomic ion (excluding ammonium)

  3. Naming Ionic Compounds • We will always be ignoring the Metalloids and the Inner Transition Metals • For now we will be ignoring the Transition Metals

  4. Charges!!! 0 +1 +2 -4 +3 -3 -1 -2

  5. Naming Ionic Compounds • NaCl • You always name the cation first: • sodium • You then name the anion: • If not a polyatomic ion change the ending to –ide • chlorine becomes chloride • sodium chloride

  6. Naming Ionic Compounds • Ca3P2 • calcium phosphide • K2O • potassium oxide • BaS • barium sulfide • MgF2 • magnesium fluoride

  7. Naming Ionic Compounds • If it has a polyatomic ion name it as given • KClO3 • potassium chlorate • Ca(BrO4)2 • calcium perbromate • NH4Cl • ammonium chloride

  8. Naming Ionic Compounds • Practice • KCN • Ba(MnO4)2 • BaCl2 • Ca3(PO4)2 • Al2O3 • NH4OH • potassium cyanide • barium permanganate • barium chloride • calcium phosphate • aluminum oxide • ammonium hydroxide

  9. Naming Ionic Compounds • If you have the name and you want to write the formula • sodium sulfide • First write the symbols for each ion with the charge • Na+ and S-2

  10. Naming Ionic Compounds • Determine how many of each ion you need to balance out the charge • two Na+ to every one S-2 • Use subscripts to indicate how many you used and get rid of the charges • Na2S

  11. Naming Ionic Compounds • calcium bromide • CaBr2 • sodium nitrate • NaNO3 • aluminum oxalate • Al2(C2O4)3 • ammonium oxide • (NH4)2O

  12. Naming Ionic Compounds: Using Transition Metals

  13. Naming Ionic Compounds • Transition Metals • Do not have a consistent charge • Copper can have a +1 or a +2 charge • We use roman numerals to indicate the charge • Copper (I) is Cu+1 • Copper (II) is Cu+2

  14. Naming Ionic Compounds • copper (I) sulfate • Cu+1 and SO4-2 • Cu2SO4 • copper (II) sulfate • Cu+2 and SO4-2 • Cu2(SO4)2 • simplifies to CuSO4

  15. Naming Ionic Compounds • iron (III) oxide • Fe2O3 • molybdenum (II) thiocyanate • Mo(SCN)2 • chromium (I) nitride • Cr3N • tin (IV) silicate • Sn(SiO3)2

  16. Naming Ionic Compounds • Practice • titanium (I) nitrate • chromium (II) cyanide • manganese (II) bromide • iron (III) silicate • TiNO3 • Cr(CN)2 • MnBr2 • Fe2(SiO3)3

  17. Naming Ionic Compounds • NiCrO4 • nickel ___ chromate • chromate has a -2 charge • to balance it out nickel must have a +2 charge • nickel (II) chromate

  18. Naming Ionic Compounds • Mo(CN)3 • molybdenum ___ cyanide • cyanide has a -1 charge • to balance out three cyanides nickel must have a +3 charge • molybdenum (III) cyanide

  19. Naming Ionic Compounds • Pb(SO3)2 • lead ___ sulfite • sulfite has a -2 charge • to balance out two sulfites lead must have a +4 charge • lead (IV) sulfite

  20. Naming Ionic Compounds • VO2 • vanadium (IV) oxide • Co2CO3 • cobalt (I) oxalate • SnCr2O7 • tin (II) dichromate

  21. Naming Ionic Compounds • Practice • Ti(MnO4)2 • CoCl2 • CrPO4 • Fe2O3 • NiOH • titanium (II) permanganate • cobalt (II) chloride • chromium (III) phosphate • iron (III) oxide • nickel (I) hydroxide

  22. Naming Ionic Compounds • Three transition metals do NOT transition • Silver – Ag+1 • Zinc – Zn+2 • Cadmium – Cd+2 • AgNO3 • silver nitrate

  23. Charges!!! 0 +1 +2 -4 +3 -3 -1 -2 +2 +1 +2

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