Nomenclature

1
Nomenclature

• How Do We Name Compounds?

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Systematic Naming

• Compounds are made up of two or more elements
• Name should tell us how many and what type of
  atoms
• Too many compounds to remember all the names

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Metals
4
Metals

• Qualities of Metals
• Luster shiny
• Ductile think making it into wires
• Malleable hammer it into sheets
• Good conductors of heat and electricity

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Transition Metals
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Non-metals
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Metalloids or Semimetals
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• Anion
• Negative ion
• Has gained electrons
• Non metals form anions

• Cation
• Positive ion
• Formed by losing electrons
• Metals form cations

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Ionic Compounds

• Made of cations and anions
• Metals and nonmetals
• Electrons lost by the cation are gained by the
  anion

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Ionic Compounds
Sodium is cation
1-
1
Cl
Na
Chlorine is anion
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Charges on Ions
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Naming Ions

• Metal ion is written first in both name and
  formula
• It is named directly from element which formed
  the ion.
• Will nearly always be the positive ion or
  cation
• Transition metals can have more than one type of
  charge
• Indicate the charge with roman numerals in
  parenthesis. Iron(II) or Iron(III)
• Exceptions
• Silver always 1
• Cadmium and Zinc always 2

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Name these

• Na 1
• Ca 2
• Al 3
• Fe 3
• Fe 2
• Pb 2
• Li 1

• Sodium
• Calcium
• Aluminum
• Iron (III)
• Iron (II)
• Lead (II)
• Lithium

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Write Formulas for these

• Potassium ion
• Magnesium ion
• Copper (II) ion
• Chromium (IV) ion
• Barium ion
• Mercury (II) ion

• K1
• Mg2
• Cu2
• Cr4
• Ba2
• Hg2

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Naming Anions

• Anions are always the same.
• Change the element ending to -- ide
• F1- Fluorine to Fluoride

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Name These

• Chloride
• Nitride
• Bromide
• Oxide
• Iodide
• Strontium

• Cl1-
• N3-
• Br 1-
• O2-
• I1-
• Sr2

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Write These

• Sulfide ion
• Iodide ion
• Phosphide ion
• Strontium ion

• S2-
• I1-
• P3-
• Sr2

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Polyatomic Ions

• Tightly bound groups of atoms acting as a single
  ion.
• Names given in table in book. (pg 123)
• Most are anions that contain oxygen. Names end
  in ate (one more O), or ite (one less O).
• SO32- sulfite SO42- sulfate
• Exceptions Ammonium cation NH41, Cyanide CN-,
  and hydroxide OH-

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Naming Binary Ionic Compounds

• 2 elements involved
• Ionic metal (cation) and a non-metal (anion)
• Naming is easy with elements in representitive
  groups
• NaCl Na Cl- sodium chloride
• MgBr2 Mg2Br- magnesium bromide

You MUST charge balance EVERYTIME you write a
formula for an ionic compound!!!
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Naming Binary Ionic Compounds

• The problem comes with the transition metals.
• Need to figure out their charges
• All ionic compounds will have a neutral charge
• Same number of and charges
• Use the anion to determine the charge on the
  positive ion.

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Naming Binary Ionic Compounds

• Try naming these
• KCl
• Na3N
• CrN
• ScP
• PbO
• PbO2
• Na2Se

• Potassium chloride
• Sodium nitride
• Chromium (III) nitride
• Scandium (III) phosphide
• Lead (II) oxide
• Lead (IV) oxide
• Sodium selenide

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Ternary Ionic Compounds

• Will have polyatomic ions
• At least 3 elements
• Use yellow sheet
• Name these ions
• NaNO3
• CaSO4
• CuSO3
• (NH4)2O

• LiCN
• Fe(OH)3
• (NH4)2CO3
• NiPO4

• Sodium nitrate
• Calcium sulfate
• Copper (II) sulfite
• Ammonium oxide

• Lithium cyanide
• Iron (III) hydroxide
• Ammonium carbonate
• Nickel (III) phosphate

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Writing Formulas(charge balancing)

• Net charge must add to zero. Get charges of
  cation/anion
• Balance the charges
• Put polyatomics in parenthesis

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Writing Formulas

• Write formula for calcium chloride
• Calcium is Ca2
• Chloride is Cl1-
• Ca2Cl-1 would have a 1 charge
• Need another Cl1-
• Ca2Cl2-1 CaCl2

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Writing Formulas

• Crisscross method

Calcium chloride
CaCl2
Ca2 Cl1-
No need to write the one
Iron (III) sulfide
Fe 3 S2-
Fe 2 S3
Fe2S3
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Write Formulas for These

• Lithium sulfide
• Tin (II) oxide
• Tin (IV) oxide
• Magnesium fluoride
• Copper (II) sulfate
• Iron (III) phosphide
• Iron (III) sulfide
• Ammonium chloride
• Ammonium sulfide

• Li2S
• SnO
• SnO2
• MgF2
• CuSO4
• FeP
• Fe2S3
• (NH4)Cl
• (NH4)2S

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Things to Look For

• If cations have ( ), the roman numeral is their
  charge.
• If anions end in ide they probably are off the
  periodic table (monoatomic)
• If anion ends in ate or ite it is a polyatomic
  ion

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Types of Reactions

• Millions of reactions
• Too many to remember
• They fall into several categories
• We will focus on Double Replacement in todays lab

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Double Replacement

• Two things replace each other
• Reactants must be two ionic compounds or acids.
• Usually in aqueous solution
• NaOH FeCl3 ?
• The positive ions change place
• NaOH FeCl3 ? Fe3OH- Na1Cl-1
• NaOH FeCl3 ? Fe(OH)3 NaCl

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Double Replacement

• Will only happen if one of the products
• Doesnt dissolve in water and forms a solid
• (look at solubility rules)
• Or is a gas that bubbles out
• Or is a covalent compound usually water

After adding lead nitrate
Potassium iodide
2KI(aq) Pb(NO3)2 (aq) ? 2KNO3(aq) PbI2 (s)
PbI2 lead (II) iodide is insoluble
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General Rules for the Water Solubilities of
Common Ionic Compounds

• Compounds that are mostly soluble
• All nitrates
• Alkali metal (group 1A) and ammonium compounds
• Chlorides, bromides, and iodides, except for
  those of Pb2, Ag, Hg2
• Sulfates except for those of Sr2, Ba2, Pb2,
  and Hg2
• CaSO4 is slightly soluble

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General Solubility Rules

• Compounds that are mostly insoluble
• Carbonates, hydroxides, and sulfides, except for
  ammonium compounds and those of the group 1A
  metals. (The hydroxides and sulfides of Ca2,
  Sr2, and Ba2 are slightly to moderately
  soluble.)

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EXAMPLE 1

• Na2S(aq) Cd(NO3)2(aq) ?
• What will the products be?
• Na2S(aq) Cd(NO3)2(aq) ? CdS(s) NaNO3(aq)
• Double replacement occurs because cadmium sulfide
  is insoluable forms solid and no longer
  participates in reaction.
• Balanced equation?
• Na2S(aq) Cd(NO3)2(aq) ? CdS(s) 2NaNO3(aq)

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Ionic Equations Showing the Ions

• Ionic equations show all free ions (ions that are
  free to move around when dissolved in a liquid
  usually water).
• Ions that are not directly involved in the
  reaction are spectator ions.
• A net ionic equation is one in which spectator
  ions are NOT shown.

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EXAMPLE 2

• NaOH (aq) MgSO4 (aq) ?
• What will the products be?
• NaOH (aq) MgSO4 (aq) ? Mg(OH)2 (s) Na2SO4
  (aq)
• Double replacement occurs because hydroxides of
  2A metals are insoluable.
• Balanced Chemical Equation?
• 2NaOH (aq) MgSO4 (aq) ? Mg(OH)2 (s) Na2SO4
  (aq)

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Ionic Equations of Example 2

• 2NaOH (aq) MgSO4 (aq) ? Mg(OH)2 (s) Na2SO4
  (aq)
• Ionic Equation
• 2Na 2OH- Mg2 SO42- ? Mg(OH)2 (s) 2Na1
  SO42-
• Net Ionic Equation (w/o spectator ions)
• 2Na 2OH- Mg2 SO42- ? Mg(OH)2 (s) 2Na1
  SO42-
• 2OH- Mg2 ? Mg(OH)2 (s)