NOMENCLATURE

1
NOMENCLATURE

• Chapter 5

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Charges on Common Ions
-4
-3
-2
-1
1
2
3
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Table 5.1 Common Simple Cations and Anions
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Chemical Bonds

• - the forces that hold two or more atoms together
  to form a compound.
• - the two types of chemical bonds are
• 1. Ionic bonds.
• NaCl KI
• 2. Covalent bonds.
• H2O CH4

metal nonmetal
two nonmetals
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Chemical Bonds(continued)

• Ionic Bonding Force of attraction between
  oppositely charged ions.
• - Chemical compounds must have a net charge of
  zero.
• 1. Both cations and anions must be present.
• 2. The number of cations and anions must be
  such that the net charge is zero.

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Writing Formulas for Ionic Compounds
Charge must equal zero for each compound.
1 1- 0 2 2- 0 6 6- 0
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COMPOUNDS FORMED FROM IONS

• CATION ANION ---gt
• COMPOUND
• Na Cl- --gt NaCl
• A neutral compound requires equal number of ()
  and (-) charges.

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Chemical Bonds(continued)

• Covalent bonding results from atoms sharing
  electrons.
• Molecule a collection of covalently-bonded
  atoms.
• H2O C12H22O11

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Common Names

• sugar of lead
• blue vitriol
• quicklime
• Epsom salts
• milk of magnesia
• gypsum
• laughing gas

lead(II) acetate copper(II) sulfate calcium
oxide magnesium sulfate magnesium
hydroxide calcium sulfate dinitrogen monoxide
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Common Names - Exceptions

• H2O water, steam, ice
• NH3 ammonia
• CH4 methane
• NaCl table salt
• C12H22O11 table sugar

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Types of Cations

• Type I Cations
• only one charge
• Group I ions
• Group II ions
• Aluminum
• Cadmium
• Silver
• Zinc
• Memorize Table 5.1, page 129

• Type II Cations
• more than one charge
• transition elements
• elements under the stairstep
• Memorize Table 5.2, page 133

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Metal Cations

• Type I
• Metals that can only have one possible charge
• Determine charge by position on the Periodic
  Table
• Type II
• Metals that can have more than one possible
  charge
• Determine metal cations charge from the charge
  on anion

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Naming Compounds
Binary Ionic Compounds

• 1. Cation first, then anion
• 2. Monatomic cation name of the element
• Ca2 calcium ion
• 3. Monatomic anion root -ide
• Cl? chloride
• CaCl2 calcium chloride

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Naming Compounds(continued)
Binary Ionic Compounds (Type II)

• - metal forms more than one cation
• - use Roman numeral in name
• CuCl2 Cu2 is cation
• CuCl2 Copper (II) chloride
• Cupric chloride

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Naming Compounds(continued)
Binary compounds (Type III)

• - Compounds between two nonmetals
• - First element in the formula is named first.
• - Second element is named as if it were an anion.
• - Use prefixes (Table 5.3 on page 137).
• - Never use mono- for the first element.
• P2O5 diphosphorus pentoxide

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Prefixes

• Drop last a in the prefix if the name begins
  with vowel

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Figure 5.1 A flow chart for naming binary
compounds.
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Common Nomenclature Mistakes

• Compounds
• SO3 --Sulfur trioxide
• NO2 -- Nitrogen dioxide
• NO3 -- Nitrogen trioxide
• NH3 -- Ammonia

• Polyatomic ions
• SO32- -- Sulfite ion
• NO21- -- Nitrite ion
• NO31- -- Nitrate ion
• NH41 --Ammonium ion

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MOLECULAR FORMULAS

• Formula for glycine is C2H5NO2
• In one molecule there are
• 2 C atoms
• 5 H atoms
• 1 N atom
• 2 O atoms

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Molecular Modeling
Drawing of glycine
Ball stick
Space-filling
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POLYATOMIC IONS

• Groups of atoms with a charge.
• MEMORIZE the names and formulas in Table 5.4,
  page 142.

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Table 5.4 Names of Common Polyatomic Ions
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Patterns for Polyatomic Ions

• -ate ion
• chlorate ClO3-
• -ate ion plus 1 O ? same charge, per- prefix
• perchlorate ClO4-
• -ate ion minus 1 O ? same charge, -ite suffix
• chlorite ClO2-
• -ate ion minus 2 O ? same charge, hypo- prefix,
  -ite suffix
• hypochlorite ClO-

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Some Common Polyatomic Ions

• NH4 ammonium ion One of the few common
  polyatomic cations

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Some Common Polyatomic Ions

• CO32- carbonate ion
• HCO3- bicarbonate ion
• - hydrogen carbonate ion

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Some Common Polyatomic Ions

• SO42- sulfate ion
• SO32- sulfite ion

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Some Common Polyatomic Ions

• NO3- nitrate ion
• NO2- nitrite ion

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Figure 5.2 Overall strategy for naming chemical
compounds
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NOMENCLATURE OF COMPOUNDS
Binary -- 2 elements
Ternary -- (3 elements) - Ionic
(metal ion polyatomic ion)
Ca3(PO4)2 -- calcium phosphate FeSO4 -- iron
(II) sulfate -- ferrous sulfate
Type I - Ionic (Type I metal
nonmetal) Group I, II, Al3, Ag1, Cd2,
Zn2 NaCl -- Sodium Chloride
Type II - Ionic (Type II metal nonmetal) All
other metals Fe2S3 -- iron (III) sulfide
-- ferric sulfide
Type III - covalent (2 nonmetals) CO2 -- carbon
dioxide
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Binary Acids

• made up of two elements -- hydrogen and a
  nonmetal
• named by using
• prefix hydro root of nonmetal ic acid
• HCl -- hydrochloric acid
• H2Se -- hydroselenic acid

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Table 5.5 Names of Acids that Do Not Contain
Oxygen
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Ternary Acids (oxyacids)

• contain three elements -- hydrogen, nonmetal,
  and oxygen.
• most oxygen per root of nonmetal ic
  acid
• less oxygen root of nonmetal ic acid
• less oxygen root of nonmetal ous acid
• least oxygen hypo root of nonmetal ous
  acid

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Ternary Acids(continued)

• HBrO4 perbromic acid
• HBrO3 bromic acid
• HBrO2 bromous acid
• HBrO hypobromous acid
• H3PO4 phosphoric acid
• H3PO3 phosphorous acid
• H3PO2 hypophosphorus acid

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Figure 5.3 A flow chart for naming acids
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Salt Nomenclature (continued)

• Ternary salts ( metal and polyatomic ion)
• name of positive ion root of nonmetal ate or
  ite
• If the salt comes from an ic acid, change ic to
  ate.
• H2CO3 carbonic acid Na2CO3 sodium carbonate
• H3PO4 phosphoric acid K3PO4 potassium
  phosphate
• If the salt comes from an ous acid, change ous to
  ite.
• H2SO3 sulfurous acid Li2SO3 lithium sulfite
  
• HClO hypochlorous acid NaClO sodium
  hypochlorite

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Chemical Nomenclature

• Name each of the following
• CuCl
• HgO
• Fe2O3
• MnO2
• PbCl2
• CrCl3

copper(I) chloride cuprous
chloride mercury(II) oxide mercuric
oxide iron(III) oxide ferric
oxide manganese(IV) oxide manganic
oxide lead(II) chloride plumbous
chloride chromium(III) chloride chromic
chloride
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Chemical Nomenclature

• Name each of the following
• P4O10
• N2O5
• Li2O2
• Ti(NO3)4
• SO3
• SF6
• O2F2

tetraphosphorus decoxide dinitrogen
pentoxide lithium peroxide titanium(IV)
nitrate sulfur trioxide sulfur hexafluoride dioxyg
en difluoride
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Writing the Formulas from the Names

• For Type III compounds, use the prefixes to
  determine the subscripts
• For Type I, Type II, polyatomic Compounds and
  Acids
• Determine the ions present
• Determine the charges on the cation and anion
• Balance the charges to get the subscripts

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Determining the Charge on a Cation Au2S3

• Determine the charge on the anion
• Au2S3 - the anion is S, since it is in Group 6A,
  its charge is -2
• Determine the total negative charge
• since there are 3 S in the formula, the total
  negative charge is -6
• Determine the total positive charge
• since the total negative charge is -6, the total
  positive charge is 6
• Divide by the number of cations
• since there are 2 Au in the formula the total
  positive charge is 6, each Au has a 3 charge