Nomenclature Chapter 5 1

Classifying Binary Compounds Compounds containing a metal and a nonmetal are Type Compounds containing two nonmetals Compounds containing H and a nonmetal = 4

Metal Cations Type I Type II Metals that can only Determine charge by Metals that can have Determine metal cation’s charge from 6

Naming Binary Type II Compounds Cu+1 and N-3 Hg+2 and O-2 Cr+3 and P-3 Sn+4 and Cl-1 Ni+4 and S-2 Iron (III) phosphide Manganese (II) fluoride Gold (I) telluride Lead (IV) bromide Cobalt (III) arsenide

Ionic Compounds Sometimes you can use the reverse of the criss-cross method When naming compounds,

Naming Ionic Compounds Examples Au2S MnO Fe3N2 CuCl2 NiS2 Cr3P2 PbF4 HgI

Type III - Binary Compounds of 2 Nonmetals These binary compounds always start with a nonmetal or a metalloid. Name first element in formula first, Name the second element in the formula However, remember 10

Type III Binary Molecular Compounds Use a prefix in front of Never use the prefix mono- Prefixes: 1-mono, 2-di, 3-tri, 4-tetra,5-penta, 6-hexa, 7-hepta, 8-octa, 9-nona, 10-deca, 11-undeca, 12-dodeca. To write the formula for binary molecular compounds,

Binary Molecular Compounds Examples Naming Compounds SiF2 C3Cl9 S4I7 P5O10 Writing Formulas Nitrogen trichloride Triphosphorus pentoxide Hexasulfur monofluoride Diselenium pentabromide

Figure 5.1: A flow chart for naming binary compounds.

Ionic Compounds Ternary ionic compounds – contain atoms of three or more different elements, usually a polyatomic ion. Writing the formulas for ternary compounds is done in the same way as binary compounds. The polyatomic ions stays together though.

Ionic Compounds When you need more than one polyatomic ion in your formula, put parentheses around the ion, and how many of them you need outside the parentheses as a subscript. NEVER MOVE SUBSCRIPTS OF THE IONS, ONLY THE CHARGES!!!

Writing Formulas for Ternary Ionic Compound Examples Calcium sulfate Ca+2 and SO4-2 Sodium chlorate Na+1 and ClO3-1 Magnesium hydroxide Mg+2 and OH-1 Potassium phosphate K+1 and PO4-3 Iron (III) carbonate Fe+3 and CO3-2 Tin (IV) chromate Sn+4 and CrO4-2 Nickel (II) dihydrogen phosphate Ni+2 and H2PO4-1 Chromium (III) sulfate Cr+3 and SO4-2 Copper (II) acetate Cu+2 and C2H3O2-1 Iron (II) permanganate Fe+2 and MnO4-1

Ionic Compounds When naming ternary compounds, name the cation (first symbol in the formula unless it is ammonium, NH4+1) first, and then the rest of the formula, which will only have one name, unless it contains hydrogen.

Naming Ternary Ionic Compounds Ca(NO3)2 KClO3 BaSO3 AlPO4 CuOH Ni3(PO3)4 Fe(CN)2 Mn(HCO3)3 Au2CO3 Cr2HPO4

Acids Naming & Writing Formulas for Acids All acids begin with a hydrogen, and are neutral compounds. In all acids, the cation is the hydrogen ion, H+1. Anions change their endings when they become acids.

Acids -ide ions become hydro root ic acid Ex: chloride becomes hydrochloric acid -ate ions become root ic acid Ex: nitrate becomes nitric acid -ite ions become root ous acid Ex: chlorite becomes chlorous acid

Acids Naming & Formula Writing Examples Writing Formulas for Acids Sulfuric acid Hydroarsenic acid Perchloric acid Hypoiodous acid Naming Acids H3PO3 HI HCN H2C4H4O6

Hydrates Naming & Writing Formulas for Hydrates Hydrates – compounds that have a certain number of water molecules attached to each formula unit. To name hydrates, use the same prefixes you used for naming binary molecular compounds and add –hydrate after the prefix.

Hydrates To write the formula for compounds containing hydrates you simply have to determine how many molecules are present by looking at the prefix written before the hydrate. If you see a substance where it says it is anhydrous, that means it does not have any water molecules attached to each formula unit.

Naming and Formula Writing Examples for Hydrates CuSO4 5H2O FeCl2 3H2O Ca3(PO4)2 8H2O Sodium thiosulfate tetrahydrate Magnesium hydroxide dihydrate Stannic nitrate octahydrate