nomenclature chapter 5
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Nomenclature Chapter 5. Common Names - Exceptions. H 2 O = water, steam, ice NH 3 = ammonia CH 4 = methane NaCl = table salt C 12 H 22 O 11 = table sugar. Naming Starts with Classifying Compounds. Binary Compounds = only 2 elements Compounds containing polyatomic ions - PowerPoint PPT PresentationTRANSCRIPT
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Nomenclature
Chapter 5
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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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Naming Starts with Classifying Compounds
• Binary Compounds = only 2 elements
• Compounds containing polyatomic ions
• Acids = formula often starts with H
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Classifying Binary Compounds
• Compounds containing a metal and a nonmetal are binary ionic– Type I and II
• Compounds containing two nonmetals– Type III
• Compounds containing H and a nonmetal = Acids
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Binary Ionic
• Made of metal cation and nonmetal anion
• Name by naming the ions
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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 cation’s charge from the
charge on anion
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Type I Binary Ionic Compounds
• Contain Metal Cation + Nonmetal Anion• Metal listed first in formula & name¶ Name metal cation first, name nonmetal
anion second¶ Simple metal cation name is the metal name
– simple metals are Groups 1A, 2A and Al, Ga & In
¶ Nonmetal anion named by changing the ending on the nonmetal name to -ide
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Type II Binary Ionic Compounds• Contain Metal Cation + Nonmetal Anion• Metal listed first in formula & name
¶ Name metal cation first, name nonmetal anion second¶ Metal cation name is the metal name followed by a
Roman Numeral in parentheses to indicate its charge– Determine charge from anion charge– Common Type II cations in Table 5.2
¶ Nonmetal anion named by changing the ending on the nonmetal name to -ide
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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 chargesince there are 3 S in the formula, the total negative charge is -6
Determine the total positive chargesince the total negative charge is -6, the total positive charge is +6
Divide by the number of cationssince there are 2 Au in the formula & the total positive charge is +6, each Au has a +3 charge
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Type III - Binary Compounds of 2 Nonmetals
• Name first element in formula first, use the full name of the element
• Name the second element in the formula as if it were an anion– However, remember these compounds do not contain
ions!
• Use a prefix in front of each name to indicate the number of atoms
• Never use the prefix mono- on the first element
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Prefixes
• Drop last “a” in the prefix if the name begins with vowel
octa-8
hepta-7
hexa-6
penta-5
tetra-4
tri-3
di-2
mono-
(not used on first nonmetal)
1
PrefixSubscript
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Compounds Containing Polyatomic Ions
• Polyatomic ions are charged entities that contain more than one atom– Must memorize name, formula and charge– Look for Patterns!!
• Polyatomic compounds contain one or more polyatomic ions
• Name polyatomic compounds by naming cation and anion– Non-polyatomic ions named like Type I and II
• Polyatomic Acids contain H+ and a polyatomic anion
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Patterns for Polyatomic Ions
Elements in the same column on the Periodic Table form similar polyatomic ions– same number of O’s and same charge
ClO3- = chlorate BrO3
- = bromate If the polyatomic ion starts with H, add
hydrogen- before the ions name and add 1 to the chargeCO3
2- = carbonate HCO3- = hydrogen carbonate
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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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Acids
• Contain H+ cation and anion
• Binary acids have H+ cation and a nonmetal anion
• Oxyacids have H+ cation and a polyatomic anion
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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