Chemical Structure: Chemical Nomenclature. Inorganic Compounds
Bires, 2009 Slide 1 Back Chapter 7: Inorganic Nomenclature Inorganic –branch of chemistry dealing...
-
Upload
sabina-jenkins -
Category
Documents
-
view
217 -
download
0
Transcript of Bires, 2009 Slide 1 Back Chapter 7: Inorganic Nomenclature Inorganic –branch of chemistry dealing...
Bires, 2009 Slide 1
BackBack
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
Bires, 2009 Slide 2
BackBack
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
Bires, 2009 Slide 3
BackBack
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
Bires, 2009 Slide 4
BackBack
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
Bires, 2009 Slide 5
BackBack
Special Special Cations Cations :: d-block metalsd-block metals• Transition metals (d-block):
– d-block electrons can migrate into the s and p orbitals.– d-block (and p-block with d-electrons) 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
Bires, 2009 Slide 6
BackBack
• 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
Bires, 2009 Slide 7
BackBack
Oxidation PracticeOxidation Practice• Use rules for oxidation to determine the names
of these compounds:
• Write the formulas for these compounds:
LiF 2BaCl 2CoBr 32OFe 42PCrLithium Fluoride
Barium Chloride
Cobalt (II) Bromide
Iron (III) Oxide
Chromium (VI) Phosphide
Titanium (IV) Oxide
Nickel (VI) Nitride
Copper (II) Fluoride
Sodium Oxide
ONa2 2TiO2NiN2CuF
Manganese (VII) Sulfide
72SMn
Bires, 2009 Slide 8
BackBack
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• NHNH44
++ “ammoniumammonium” charge of +1+1
Bires, 2009 Slide 9
BackBack
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 (II) nitrate(II) for Lead is optional
Bires, 2009 Slide 10
BackBack
Nomenclature Practice…Nomenclature Practice…• Name the following:
• Identify the following compounds:
• Notice how the NO3- polyatomic is placed in ( )
2CaCl 4BaSO 3AgNO 4SnF )(4carefulCI
Calcium chloride
Barium sulfate
Silver (I) nitrate
Tin (IV) fluoride
Carbon tetraiodide
Copper (II) nitrate(careful)
Potassium iodide
Boron trichloride
Lithium nitrate
3LiNO 23)(NOCuKI3BCl
Bires, 2009 Slide 11
BackBack
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 )– Can use fractions of moles (.33mol : .66mol)
42ON
2NO
6126 OHC
OCH 2
End of chapter 7 - % comp removed