Nomenclature

1
Nomenclature
2
Inorganic Nomenclature

• Using different oxidation states
• Potassium oxygen
• K O
• K2O potassium oxide

3
Inorganics

• Using the same oxidation states
• Calcium oxygen
• Ca O
• CaO calcium oxide

4
Inorganics

• Using polyatomic ions
• calcium bromate
• Ca(BrO3)2

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Sample Problems

• Beryllium iodide (beryllium iodine)
• BeI2
• Calcium carbide (calcium carbon)
• Ca2C

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More Problems

• Aluminum sulfate
• Al2(SO4)3
• Ammonium hydroxide
• NH4OH

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Stock Formulas

• Iron (III) Chloride
• FeCl3
• Tin (II) Nitride
• Sn3N2

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Naming Compounds

• The nonmetal name in a BINARY COMPOUND (two
  compounds a metal and nonmetal bonded
  ionically) has the nonmetal name end in ide.
• BaBr2 barium bromide
• Mg3N2 magnesium nitride
• K2S potassium sulfide

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Naming using Stock formulas

• Fe(OH)2
• Iron (II) hydroxide
• CuSO4
• Copper (II) sulfate

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Practice Problems

• Writing Formulas
• 1, 2, 4, 5, 10, 15, 25, 31, 34, 43, 53, 70
• Naming Compounds
• 154, 160, 163, 166, 172, 179, 181,
• 201, 228, 234, 242, 280

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Now to the additions

• An older system used in place of the Stock system
  uses suffixes on the metal to indicate a lower or
  higher oxidation state.
• metals with lower oxidation state ous ending
• metals with higher oxidation state ic ending
• Metals use Latin names

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Examples

• Iron (II) ferrous Iron (III)
  ferric
• Copper (1) cuprous copper (II) cupric
• Tin (II) stannous tin (IV) stannic
• Lead (II) plumbous lead (IV) plumbic
• Mercury (I) mercurous Mercury (II)
  mercuric
• Chromium (II) chromous chromium (III)
  chromic
• Cobalt (II) cobaltous cobalt (III)
  cobaltic
• Manganese (II) manganous manganese (III)
  manganaic

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Binary Covalent Compounds

• For binary compounds whose first element is a
  nonmetal (covalent bonding) use the following
  prefixes for the number of atoms. The first
  element will have its normal ending, the second
  will end in ide
• 1 mono, 2 di, 3 tri, 4 tetra, 5
  penta,
• 6 hexa, 7 hepta, 8 octa, 9 nona,
• 10 deca, 11 undeca, 12 dodeca

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Binary Covalent Examples

• SO2 sulfur dioxide
• Cl2O7 dichlorine tetrachloride
• P2O3 diphosphorus trioxide
• P2O5 diphosphorus pentaoxide

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Hydrogen Exceptions

• For compounds with hydrogen in the middle use
  either the bi prefix or the word hydrogen
• Examples
• NaHSO4 sodium bisulfate or
• sodium hydrogen sulfate
• Ca(HSO4)2 calcium bisulfate or
• calcium hydrogen sulfate

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Another Problem

• For phosphate salts with more than 1 type ion,
  one of which is hydrogen, use the following
  format
• NaH2PO4 sodium dihydrogen phospate
• K2HPO4 potassium monohydrogen phosphate

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No Reduction Formulas

• Certain formulas are not reduced The most
  common one is mercury (I) which is Hg2 2
• Example
• Mercury (I) nitrate Hg2(NO3)2
• Mercury (I) chloride Hg2Cl2

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Peroxide

• Another example of no reduction is peroxide which
  is O2 2-
• hydrogen peroxide H2O2
• sodium peroxide Na2O2

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Inorganic Acids

• Standard ate polyatomic ion acids with ic
• HBrO3 Bromic acid
• HClO3 Chloric acid
• HNO3 Nitric acid
• H3PO4 Phosphoric acid
• H2SO4 Sulfuric acid
• H2CO3 Carbonic acid

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Removing all oxygens

• When all oxygens are removed, add a hydro
  prefix (along with ic ending)
• HBrO3 Bromic acid HBrO Hydrobromic acid
• HNO3 Nitric acid HNO Hydronitric acid

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Adding an extra oxygen

• When an extra oxygen is added, add a per
  prefix, along with ic ending
• H2CO3 carbonic acid H2CO4 percarbonic
• 
  acid
• HClO3 chloric acid HClO4 perchloric
  acid

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Taking 1 oxygen away

• When 1 oxygen is taken away from the normal ic
  ending formula, change ic to ous
• H2SO4 sulfuric acid H2SO3 sulfurous acid
• H3PO4 phosphoric acid
• H3PO3 phosphorous acid

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Taking 2 oxygens away

• When 2 oxygens are taken away from normal ic
  ending, change ic to ous and add a hypo
  prefix
• HNO3 Nitric acid HNO hyponitrous acid
• HClO3 chloric acid HClO hypochlorous acid
• H3PO2 hypophosphorous acid

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Final Homework Problems

• 3, 6, 16, 22, 44, 50, 55, 67, 89, 96,
• 100, 113, 120, 127, 135, 147, 150
• 161, 165, 175, 187, 204, 210, 223,
• 236, 243, 291, 306, 333, 341, 324