bires, 2007 slide 1 back chapter 7: inorganic nomenclature inorganic –branch of chemistry dealing...
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Bires, 2007 Slide 1
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Chapter 7: Inorganic NomenclatureChapter 7: Inorganic Nomenclature• Inorganic
– branch of chemistry dealing with metals and nonmetals.
• Nomenclature– naming system used to identify
compounds.
• Binary compoundsBinary compounds– simplest compounds– contain only two elements.
• Remember: the cation is placed first, then the anion.
NaCl
2MgCl
LiBr
MgOcation anion
cation anion
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Bires, 2007 Slide 2
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Naming Binary CompoundsNaming Binary Compounds• Begin with the positive ion
– the first element in the compound.
• The cation’s name first part of the compound’s name.
• The anion has its name truncated (shortened) and “–ide” is added.
• The correct name is then… Magnesium Chloride
2MgClMagnesium Chlorine
Name
Chloride
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Bires, 2007 Slide 3
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Common Common anionsanions• O – oxygen, = “oxide”
• H – hydrogen, = “hydride”
• S – sulfur, = “sulfide”
• Cl – chlorine, = “chloride”
• F – fluorine, = “fluoride”
• I – iodine, = “iodide”
• N – nitrogen, = “nitride”
• C – carbon, = “carbide”
• Br – bromine, = “bromide”
• P – phosphorus, = “phosphide”
Some atoms can be positive or negative:
Carbon: -4 or +4
Nitrogen: -3 or +5
Sulfur: -2 or +6
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Bires, 2007 Slide 4
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Multiple Multiple NonmetalNonmetal Anions Anions• When both elements are nonmetals.
– we add a latin-based prefix to the anion.• One anion: “mono-”
• Two anions: “di-”
• Three anions: “tri-”
• Four anions: “tetra-”
2COCarbon dioxide
3BFBoron trifluoride
4CClCarbon tetrachloride
Mono in front of a single anion is optional (older)
Carbon monoxide CO
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Bires, 2007 Slide 5
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Special Special Cations Cations :: d-block metalsd-block metals• Transition metals (d-block):
– d-block electrons can migrate into the s and p orbitals.– metals can have several charges when bonding.– Use a Roman Numeral to show the cation’s charge:
• Fe2+ Co3+ Sn4+ Cr6+
• Iron(II) Cobalt(III) Tin(IV) Chromium(VI)• Identify the ions and charges on:• V4+ Cu2+ Tin (II) Nickel(IV)
D-block metals do not follow the octet rule when bonding
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Bires, 2007 Slide 6
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• Oxidation number– charge that an atom would have when it bonds.
• The oxidation number of hydrogen in H2O is +1.
• The oxidation number of oxygen in H2O is -2.
• Rule 1: The total oxidation numbers of all the atoms in a compound must be zero. (NaCl)
• Rule 2: Oxidation of a free element is zero. (H2)
• Can you figure the oxidation numbers of the following atoms?
• Li+ Mg2+ CaS AgCl AlF3 O2
• +1 +2 -2 -1 +3 0Some elements can change their oxidation numbers in chemical reactions.
You need to predict the oxidation based on the location in the p-table
Common Oxidation States.mov
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Bires, 2007 Slide 7
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Polyatomic ionsPolyatomic ions• Polyatomic ion:
– Ion composed of more than one element. (big)– stable units that bond like individual atoms.
• Polyatomic ions used in class are:
• NO3- “nitrate” charge of -1
• OH- “hydroxide” charge of -1• C2H3O2
- “acetate” charge of -1• SO4
2- “sulfate” charge of -2• CO3
2- “carbonate” charge of -2• PO4
3- “phosphate” charge of -3• NH4
+ “ammonium” charge of +1
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Bires, 2007 Slide 8
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Naming With Polyatomic IonsNaming With Polyatomic Ions• Use the cation as
normal….
• Add the name of the polyatomic anion.
• Here, the compound is Copper (II)sulfate.
4CuSOCopper (II) sulfate
3LiNOLithium nitrate
23)(NOPbLead nitrate
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Bires, 2007 Slide 9
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Nomenclature Practice…Nomenclature Practice…• Name the following:
• Identify the following compounds:
• Notice how the NO3- polyatomic is placed in ( )
2CaCl 4BaSO 3NaNO 2SrF )(4carefulCI
Calcium chloride
Barium sulfate
Sodium nitrate
Strontium fluoride
Carbon tetraiodide
Copper (II) nitrate(careful)
Potassium iodide
Boron trichloride
Lithium nitrate
3LiNO 23)(NOCuKI3BCl
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Bires, 2007 Slide 10
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Empirical FormulaEmpirical Formula / / Molecular FormulaMolecular Formula• Molecular Formula
– shows the actual numbers of atoms in a molecule
• Empirical Formula– reduced form– shows only the ratio of atoms in a molecule:
( 1:2 or 1:2:1 )
• The empirical formula is useful in determining Percent Composition = mass % of one element in a compound.
42ON
2NO
6126 OHC
OCH 2
Calculate the % composition of oxygen in each of these compounds
% composition =
element mass (g) / empirical formula mass (g)
End of chapter 7