NOMENCLATURE

Inorganic Nomenclature

Using different oxidation states

Potassium + oxygen

K O

K2O potassium oxide

Inorganics

Using the same oxidation states

Calcium + oxygen

Ca O

CaO calcium oxide

Inorganics

Using polyatomic ions

calcium + bromate

Ca(BrO3)2

Sample Problems

Beryllium iodide (beryllium + iodine)

BeI2

Calcium carbide (calcium + carbon)

Ca2C

More Problems

Aluminum sulfate

Al2(SO4)3

Ammonium hydroxide

NH4OH

Stock Formulas

Iron (III) Chloride

FeCl3

Tin (II) Nitride

Sn3N2

Naming Compounds

The nonmetal name in a BINARY COMPOUND (two compounds – a metal and nonmetal bonded ionically) has the nonmetal name end in “ide”.

BaBr2 barium bromide

Mg3N2 magnesium nitride

K2S potassium sulfide

Naming using Stock formulas Fe(OH)2

Iron (II) hydroxide

CuSO4

Copper (II) sulfate

Practice Problems

Writing Formulas: 1, 2, 4, 5, 10, 15, 25, 31, 34, 43, 53, 70

Naming Compounds: 154, 160, 163, 166, 172, 179, 181, 201, 228, 234, 242, 280

Now to the additions:

An older system used in place of the Stock system uses suffixes on the metal to indicate a lower or higher oxidation state.

* metals with lower oxidation state: “ous” ending

* metals with higher oxidation state: “ic” ending

Metals use Latin names

Examples:

Iron (II) = ferrous Iron (III) = ferricCopper (1) = cuprous copper (II) = cupricTin (II) = stannous tin (IV) = stannicLead (II) = plumbous lead (IV) = plumbicMercury (I) = mercurous Mercury (II) = mercuric

Chromium (II) = chromous chromium (III) chromic

Cobalt (II) = cobaltous cobalt (III) = cobaltic

Manganese (II) = manganous manganese (III) = manganaic

Binary Covalent Compounds

For binary compounds whose first element is a nonmetal (covalent bonding) use the following prefixes for the number of atoms. The first element will have its normal ending, the second will end in “ide”

1 = mono, 2 = di, 3 = tri, 4 = tetra, 5 = penta,

6 = hexa, 7 = hepta, 8 = octa, 9 = nona,10 = deca, 11 = undeca, 12 = dodeca

Binary Covalent Examples:

SO2 sulfur dioxide

Cl2O7 dichlorine tetrachloride

P2O3 diphosphorus trioxide

P2O5 diphosphorus pentaoxide

Hydrogen Exceptions

For compounds with hydrogen in the middle use either the “bi” prefix or the word “hydrogen”

Examples:NaHSO4 sodium bisulfate or sodium hydrogen sulfate

Ca(HSO4)2 calcium bisulfate or calcium hydrogen sulfate

Another Problem

For phosphate salts with more than 1 type ion, one of which is hydrogen, use the following format:

NaH2PO4 sodium dihydrogen phospate

K2HPO4 potassium monohydrogen phosphate

No Reduction Formulas

Certain formulas are not reduced: The most common one is mercury (I) which is Hg2 2+

Example: Mercury (I) nitrate = Hg2(NO3)2

Mercury (I) chloride = Hg2Cl2

Peroxide

Another example of no reduction is peroxide which is O2 2-

hydrogen peroxide = H2O2

sodium peroxide = Na2O2

Inorganic Acids

Standard “ate” polyatomic ion acids with “ic”

HBrO3 Bromic acid

HClO3 Chloric acid

HNO3 Nitric acid

H3PO4 Phosphoric acid

H2SO4 Sulfuric acid

H2CO3 Carbonic acid

Removing all oxygens

When all oxygens are removed, add a “hydro” prefix (along with “ic” ending)

HBrO3 Bromic acid HBrO Hydrobromic acid

HNO3 Nitric acid HNO Hydronitric acid

Adding an extra oxygen

When an extra oxygen is added, add a “per” prefix, along with “ic” ending

H2CO3 carbonic acid H2CO4

percarbonic acid

HClO3 chloric acid HClO4 perchloric acid

Taking 1 oxygen away

When 1 oxygen is taken away from the normal “ic” ending formula, change “ic” to “ous”

H2SO4 sulfuric acid H2SO3 sulfurous acid

H3PO4 phosphoric acid

H3PO3 phosphorous acid

Taking 2 oxygens away

When 2 oxygens are taken away from normal “ic” ending, change “ic” to “ous” and add a “hypo” prefix”

HNO3 Nitric acid HNO hyponitrous acid

HClO3 chloric acid HClO hypochlorous acid

H3PO2 hypophosphorous acid

Final Homework Problems

3, 6, 16, 22, 44, 50, 55, 67, 89, 96, 100, 113, 120, 127, 135, 147, 150

161, 165, 175, 187, 204, 210, 223, 236, 243, 291, 306, 333, 341, 324