Bires, 2009 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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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

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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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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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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

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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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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

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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• NHNH44

++ “ammoniumammonium” charge of +1+1

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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 (II) nitrate(II) for Lead is optional

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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 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

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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 )– Can use fractions of moles (.33mol : .66mol)

42ON

2NO

6126 OHC

OCH 2

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