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Ionic Nomenclature

Ionic Nomenclature. Naming Ionic Compounds. Ionic Compounds Review. Ionic compounds are made of positive and negative ions. Also known as “salts”. Polyatomic ions are groups of atoms that behave as a single ion: Examples: CO 3 -2 CN -1 SO 4 -2. Naming Ionic Compounds.

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Ionic Nomenclature

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  1. Ionic Nomenclature Naming Ionic Compounds

  2. Ionic Compounds Review • Ionic compounds are made of positive and negative ions. • Also known as “salts”. • Polyatomic ions are groups of atoms that behave as a single ion: • Examples: • CO3-2 • CN-1 • SO4-2

  3. Naming Ionic Compounds • Two types of ionic compounds: • Binary, contains 2 elements • NaCl, MgBr2, Fe2O3 • Ternary, contains 3 elements • Two of the elements are in a polyatomic ion • NaNO3, NH4Cl, Cr2(SO4)3

  4. Naming Binary Ionic Compounds • Some metal ions have only one possible charge: • Group 1A metal ions all have +1 charge. • Group 2A metal ions all have +2 charge. • Ag+1, Zn+2, Cd+2, Al+3, Ga+3 • For fixed charge cations, name as element. • Na+1 = sodium ion • Ca+2 = calcium ion • Ag+1 = silver ion • Ga+3 = gallium ion • Name anion as stem of element’s name followed by suffix –ide. • Cl-1 = chloride ion • S-2 = sulfide ion • N-3 = nitride ion

  5. Fixed Charge Metal Ions Li+1 Be+2 Al+3 Na+1 Mg+2 K+1 Ca+2 Ga+3 Zn+2 Rb+1 Sr+2 Ag+1 Cd+2 Cs+1 Ba+2 Fr+1 Ra+2

  6. Naming Binary Ionic Compounds • NaCl • KBr • MgF2 • CaO • AgI • Al2S3 • Zn3P2 sodium chloride potassium bromide magnesium fluoride calcium oxide silver iodide aluminum sulfide zinc phosphide

  7. Naming Binary Ionic Compounds • Most metals can form multiple cations. • Iron can form Fe+2 ions or Fe+3 ions. • Copper can form Cu+1 ions or Cu+2 ions. • For variable charge cations, name as element w/ Roman numeral in ( ) to indicate charge. • Fe+2 = iron(II) ion • Fe+3 = iron(III) ion • Cu+1 = copper(I) ion • Cu+2 = copper(II) ion • Pb+2 = lead(II) ion • Pb+4 = lead(IV) ion

  8. Variable Charge Metal Ions

  9. Naming Binary Ionic Compounds • The compound must be electrically neutral. • Use the charge of the anion to figure out the charge of the metal. • Example: Fe2O3 • (2 x Fe) + (3 x -2) = neutral • (2 x Fe) – 6 = neutral • (2 x Fe) = +6 • Fe = +3 • iron(III) oxide • Example: FeO • Fe + -2 = neutral • Fe = +2 • iron(II) oxide

  10. Naming Binary Ionic Compounds • FeCl2 • Fe2Se3 • CuBr • CuS • CrO • CrI3 • PbF2 • PbS2 iron(II) chloride iron(III) selenide copper(I) bromide copper(II) sulfide chromium(II) oxide chromium(III) iodide lead(II) fluoride lead(IV) sulfide

  11. Naming Ternary Ionic Compounds • Name metal as you would for a binary, with charge as a Roman numeral if necessary. • Name polyatomic anions as themselves.Know these: • CO3-2 = carbonate • NO3-1 = nitrate • PO4-3 = phosphate • SO4-2 = sulfate • OH-1 = hydroxide • ClO-1 = hypochlorite • ClO3-1 = chlorate • C2H3O2-1 = acetate • CH3COO-1 = acetate • CN-1 = cyanide

  12. Naming Ternary Ionic Compounds • Only one polyatomic cation: • NH4+1 = ammonium • Name it, then name the anion properly.

  13. Naming Ternary Ionic Compounds • LiNO3 • Mg(OH)2 • Fe2(SO4)3 • Zn(C2H3O2)2 • AlPO4 • NH4Cl • Cr(CN)2 lithium nitrate magnesium hydroxide iron(III) sulfate zinc acetate aluminum phosphate ammonium chloride chromium(II) cyanide

  14. Writing Formulas From Names • To write an ionic formula from a name, write the ions with their proper charges, then criss-cross. • Don’t forget that polyatomic ions need parentheses if there’s more than one of them. • Write the formula for iron(III) hydroxide • iron(III) = Fe+3 • hydroxide = OH-1 • iron(III) hydroxide  Fe+3 + OH-1 Fe(OH)3 • Write the formula for potassium sulfate • potassium = K+1 • sulfate = SO4-2 • potassium sulfate  K+1 + SO4-2  K2SO4

  15. Writing Formulas From Names • calcium carbonate  • sodium oxide  • aluminum cyanide  • potassium acetate  • copper(II) hydroxide  • gold(III) sulfide  Ca+2 + CO3-2 Na+ + O-2 Al+3 + CN-1 K+1 + C2H3O2-1 Cu+2 + OH-1 Au+3 + S-2 CaCO3 Na2O Al(CN)3 KC2H3O2 Cu(OH)2 Au2S3

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