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1.16 Names of Ionic Compounds Examples:, Lecture notes of Chemistry

The Nomenclature of Compounds. – system of naming ... name of the element + ion (Ca2+ → calcium ... Examples: • Name the compounds: PF5, CrF3, N2O3,. Fe2O3.

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The Nomenclature of Compounds
system of naming compounds
common and systematic names
1.15 Names of Ions
Monoatomic cations
name of the element + ion (Ca2+ calcium
ion)
Roman numeral for the charge of the ion, if more
than one charges are possible (Fe2+ iron(II)
ion, Fe3+ iron(III) ion)
Monoatomic anions
root of element name + -ide + ion (Cl-
chloride ion, O2-oxide ion)
Polyatomic ions -Table 1.3
oxoanions
root of element name + -ate + ion (SO42-sulfate
ion)
oxoanions with different number of O atoms -hypo-
(per-) + root of element name + -ite (-ate) + ion
(ClO-hypoclorite, ClO2-chlorite, ClO3-
chlorate, ClO4-perchlorate ion)
H-containing anions -add “hydrogen” to the
name (H2PO4-dihydrogen phosphate ion)
1.16 Names of Ionic Compounds
Name of cation + name of anion (MgSO4
magnesium sulfate, Co2S3cobalt(III) sulfide)
Charge balance -Co23+S32-2x(+3) + 3x(-2) = 0
Cross rule -Al3+, SO42-Al2(SO4)3
Hydrates -ionic compounds containing a definite
proportion of water (CoCl2·6H2O cobalt(II)
chloride hexahydrate); Greek prefixes -mono-, di-,...)
Examples:
Give the systematic names of: Na2HPO4,
CuSO4·5H2O, MnBr2, KIO4.
sodium hydrogen phosphate (Na+ , HPO42-)
copper(II) sulfate pentahydrate (Cu2+, SO42-)
manganese(II) bromide (Mn2+, Br-)
potassium periodate (K+, IO4-)
pf3

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The Nomenclature of Compounds

  • system of naming compounds
    • common and systematic names

1.15 Names of Ions

  • Monoatomic cations
    • name of the element + ion (Ca2+^ → calcium ion)
    • Roman numeral for the charge of the ion, if more than one charges are possible (Fe2+^ → iron(II) ion, Fe3+^ → iron(III) ion)
  • Monoatomic anions
  • root of element name + -ide + ion (Cl-^ → chlor ide ion, O2-^ → ox ide ion)
  • Polyatomic ions - Table 1.
  • oxoanions
  • root of element name + -ate + ion (SO 4 2-^ → sulf ate ion)
  • oxoanions with different number of O atoms - hypo- ( per- ) + root of element name + -ite (- ate ) + ion (ClO-^ → hypo clor ite , ClO 2 -^ → chlor ite , ClO 3 -^ → chlor ate , ClO 4 -^ → per chlor ate ion)
  • H-containing anions - add “hydrogen” to the name (H 2 PO 4 -^ dihydrogen phosphate ion)

1.16 Names of Ionic Compounds

  • Name of cation + name of anion (MgSO 4 → magnesium sulfate, Co 2 S 3 → cobalt(III) sulfide)
  • Charge balance - Co 2 3+S 3 2-^ → 2x(+3) + 3x(-2) = 0
  • Cross rule - Al3+, SO 4 2-^ → Al 2 (SO 4 ) 3
  • Hydrates - ionic compounds containing a definite proportion of water (CoCl 2 ·6H 2 O → cobalt(II) chloride hexahydrate); Greek prefixes - mono-, di- ,... )

Examples:

  • Give the systematic names of: Na 2 HPO 4 ,

CuSO 4 ·5H 2 O, MnBr 2 , KIO 4.

  • sodium hydrogen phosphate (Na+^ , HPO 4 2-)
  • copper(II) sulfate pentahydrate (Cu^2 +^ , SO 4 2-)
  • manganese(II) bromide (Mn^2 +^ , Br-)
  • potassium periodate (K+^ , IO 4 - )

1.17 Names of Molecular Compounds

  • Binary molecular compounds
    • name of 1st^ element + root for 2nd^ element + ide
    • Greek prefixes for the # of atoms of each type; mono- can be omitted except for O

Examples:

  • N 2 O → di nitrogen mon ox ide
  • SF 4 → sulfur tetra fluor ide
  • H 2 S → di hydrogen sulf ide
    • Acids - release H+^ in water
      • Aqueous solutions of binary compounds containing H (HCl(aq), H 2 S(aq), HCN(aq), ...) - hydro- + root of element + -ic + acid ( hydro chlor ic acid, hydro sulfur ic acid, hydro cyan ic acid)
      • Oxoacids - parent acids of oxoanions; the # of acidic H atoms equals the charge of the anion (HNO 3 , H 2 SO 3 , H 3 PO 4 , ...Table 1.8) - root of element + -ic + acid - for anions ending on -ate (HNO 3 → nitric acid) - root of element + -ous + acid - for anions ending on -ite (H 2 SO 3 → sulfurous acid)

Examples:

  • Name the acids: HBr(aq), HClO, H 2 CO 3 ,

HBrO 4

  • hydro brom ic acid ← (Br-)
  • hypochlor ous acid ← (ClO-^ hypochlor ite )
  • carbon ic acid ← (CO 3 2-^ carbon ate )
  • perbrom ic acid ← (BrO 4 -^ perbrom ate )