Chapter 6 - Nomenclature

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Chapter 6 - Nomenclature

• Chemical Names
• Formulas

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Introduction to Chemical Bonding

• Two types of Bonding
• Ionic Bonding - transfer of electrons
• Covalent Bonding - sharing of electrons

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• Bonding takes place at the highest energy level,
  s and p sublevels.
• If there are less than half the electrons between
  the s and p sublevels, the atom will lose the
  electrons.
• If there are half or more electrons between the s
  and p sublevels, the atom will gain electrons.

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• Know the trends on the periodic table for how
  many electrons will be gained or lost.

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Ionic Bonding

• Because there is a transfer of electrons,
  elements will lose or gain electrons.
• If an element loses or gains electrons, it will
  then become a charged particle - ion.
• Positive ion - cation
• Negative ion - anion

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Cations

• Substance that has lost electrons.
• The charge is equal to the number of electrons
  that are transferred.
• Ca2 - calcium that has transferred two
  electrons to another substance (anion).
• Mg2 - magnesium that has transferred two
  electrons to another substance (anion).

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Anion

• Substance that has gained electrons.
• The charge is equal to the number of electrons
  that are transferred.
• F1- - fluorine that has accepted one electron
  from another substance (cation).
• O2- - oxygen that has accepted two electrons
  from another substance (cation).

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Ionic Bonding

• Ionic bonding is the accepting or donating of
  electrons.
• Metals are donors.
• Nonmetals are acceptors.
• Hence, ionic bonding will occur between metals
  and nonmetals.

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Oxidation Numbers

• Possible charges on an element.
• Any single element, by itself, has a charge of
  zero.
• An element takes on a charge when put with other
  elements.

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Basic Rules of Oxidation Numbers

• Group 1 elements are always 1.
• Group 2 elements are always 2.
• Group 3 elements are always 3
• Group 17 elements will be 1-.
• Group 16 elements will be 2-.
• Group 15 elements will be 3-.

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Other Elements

• Ag 1
• Zn 2 Cd 2
• Al 3 Ga 3 In 3

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Other Elements with Multiple Charges

• Cr2 and Cr3
• Fe2 and Fe3
• Co2 and Co3
• Ni2 and Ni3
• Cu and Cu2
• Sn2 and Sn4
• Pb2 and Pb4

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Writing Formulas from Ions

• The total overall charge of a compound is zero.
• Use subscripts to balance the charge to zero.

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• Ca2 and S2-
• CaS
• Na and Cl-
• NaCl
• Ba2 and N3-
• Ba3N2

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Writing Ions from Compounds

• Go with what you know.

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• MgCl2
• Mg2 and Cl-
• CuBr2
• Cu2 and Br-
• FeCl3
• Fe3 and Cl-

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Polyatomic Ions

• Many atomed charged particle that acts as a
  single unit.
• Polyatomic ions have specific names. Use the
  names.
• Common polyatomic ions include
• Nitrate ____________
• Sulfate ____________
• Phosphate ____________
• Carbonate ____________
• Hydroxide ____________
• Chlorate ____________

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Other Polyatomic Ions

• Ammonium NH4
• Permanganate MnO4-
• Bromate BrO3-
• Iodate IO3-
• Acetate C2H3O2-
• Chromate CrO42-
• Dichromate Cr2O72-

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Changing the Oxygen

• Per - _____ - ate
• _____ - ate
• _____ - ite
• Hypo - _____ - ite
• _____ - ide

? Move down lose 1 oxygen each step ?Move up
gain 1 oxygen each step
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• Ba2 and SO42-
• BaSO4
• Na and ClO3-
• NaClO3
• Fe2 and CO32-
• FeCO3

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• KNO3
• K and NO3-
• CoSO4
• Co2 and SO42-
• LiClO3
• Li and ClO3-

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More than one of the Polyatomic Ion Needed to
Balance the Charge

• If more than one of the polyatomic ions is needed
  to balance the charge, you must use parentheses
  () around the ion.
• Ba(NO3)2
• Ba2 and NO3-

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• Mg2 and ClO3-
• Mg(ClO3)2
• Fe3 and SO42-
• Fe2(SO4)3
• Co3 and NO3-
• Co(NO3)2

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Naming Ionic Compounds

• Binary Ionic Compounds - Types 1 2
• A compound that contains a positive ion (cation)
  and a negative ion (anion).
• Bi- means two
• Positive ion is written first, negative ion is
  written second in a chemical formula.

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Type 1 - Binary Ionic Compound

• The cation of a Type 1 has only one possible
  charge.
• Name the first element (cation) as is.
• Name the second element (anion) as is with an
  ending of -ide.
• Example CaCl2
• Calcium chloride

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More Examples

• NaBr - Sodium bromide
• MgO - Magnesium oxide
• KBr - Potassium bromide
• BaS - Barium sulfide

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Type 2 - Binary Ionic Compounds

• The cation has multiple charges - copper can have
  a charge of 1 or 2.
• Determine which charge is being used. Use the
  anion as the guide.
• Name the element as is.
• Use a Roman numeral to indicate the charge being
  used.

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• Name the anion as is, using an ending of -ide
  as with Type 1 compounds.
• Example CuCl2
• Copper (II) chloride
• MnO2 - Manganese (IV) oxide
• NiO - Nickel (II) oxide

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Naming Type 1 2 with Polyatomic Ions

• Form compounds called ternary compounds -
  compound that contains atoms of three different
  elements.
• Polyatomic Ion - many atomed charged particle
  acting as a single unit.
• poly - many
• atomic - atom
• ion - charged particle

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Type 1 2 Compounds with Polyatomic Ions

• Name the cation using the rules for Type 1 or
  Type 2 compounds.
• Name the polyatomic ion as is - use the name on
  the chart.
• Examples
• NaNO3 - sodium nitrate
• BaSO4 - barium sulfate

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Name these

• LiOH - lithium hydroxide
• Mg(NO3)2 - magnesium nitrate
• CrCl3 - chromium (III) chloride
• Al2O3 - aluminum oxide
• CoBr2 - cobalt (II) bromide
• Fe2O3 - iron (III) oxide

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Covalent Bonding

• Covalent bonding involves the sharing of
  electrons between substances.
• Molecule - smallest neutral unit of a substance
  that still has the properties of the substance.
• Molecular formula - shows the kinds of numbers of
  atoms present in a molecule of a compound.
• Occurs between nonmetals and nonmetals.

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• Because these are molecules and are covalently
  bonded, ions are not formed - there is no
  transferring of electrons to form ions.
• Prefixes are used in naming nonmetal-nonmetal
  compounds.

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Prefixes

• mono - 1
• di- - 2
• tri- - 3
• tetra- - 4
• penta- - 5
• hexa- - 6
• hepta- - 7
• octa- - 8
• nona- - 9
• deca- - 10

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Prefixes

• Only used for nonmetal-nonmetal compounds.
• Mono- is never used on the first element.
• Second element always has a prefix.

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Naming Molecular Compounds

• Name the first element as is. If there is more
  than one of the first element, you must use a
  prefix.
• Name the second element with a prefix to indicate
  how many atoms there are and add the ending
  -ide.
• Example
• CO2 - carbon dioxide

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Name these

• N2O - dinitrogen monoxide
• PCl3 - phosphorus trichloride
• SF6 - sulfur hexafluoride
• P4O6 - tetraphosphorus hexaoxide
• SO2 - sulfur dioxide
• NO3 - nitrogen trioxide
• SO4 - sulfur tetraoxide

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Naming Acids

• When dissolved in water, certain molecules
  produce hydrogen ions - H.
• These substances are called acids.
• An acid can be viewed as a molecule with one or
  more H ions attached to an anion.
• The rules for naming acids depend on whether the
  anion contains oxygen.

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Naming Acids

• Identify the compound as being an acid - the
  first element is hydrogen (two exceptions are
  H2O and H2O2)
• Find the anion on the chart.
• Name the anion.
• Following across to the name of the acid.
• Name the acid.

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Naming Acids

• If you move up the chart, you gain oxygen.
• If you move down the chart, you lose an oxygen.
• Start with what you know - usually the -ate group.

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Examples

• HCl
• The chloride ion (anion) is a single element and
  ends in -ide.
• It is at the bottom of the chart.
• Move across and the name of this acid is
  hydrochloric acid.

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• H3PO4
• The anion is phosphate.
• Move across to the acids and the name of this
  acid is phosphoric acid.
• H2SO4
• The anion is sulfate.
• Move across to the acids and the name of this
  acid is sulfuric acid.

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• HClO2
• Identified as an acid.
• The anion is ClO21-, which is one less oxygen
  than chlorate, ClO31-.
• Lose an oxygen, move down the chart.
• Move down the chart and the name of the anion is
  chlorite.
• Move across to the acid and the name of this acid
  is chlorous acid.

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Name these

• HNO3 - nitric acid
• H2CO3 - carbonic acid
• H2SO3 - sulfurous acid
• HNO2 - nitrous acid
• HC2H3O2 - acetic acid
• HClO4 - perchloric acid