Big Idea: Matter & Atoms
Naming Ionic Compounds Naming Covalent Compounds Naming Acids Naming Hydrates
The cation (positive ion) is written first Takes the same name as the element if only forms one charge Use Roman numerals to distinguish charge if element forms more than one charge The anion (negative ion) is written last Use the first part of its element name and add ide is added as the suffix.
Examples Formula Name Ions CuS Copper (II) Sulfide Cu 2+ S 2- CuBr Copper (I) Bromide Cu + Br - Fe 2 O 3 MgO CoI 3 Lithium Fluoride Manganese (II) Oxide Ca 2+ Br -
For polyatomic ions, always use the name assigned to it Do not add an additional suffix (such as ide) Example: CO 3 2- --carbonate ion CaCO 3 calcium carbonate Ammonium, NH 4+, is the only polyatomic cation that you need to know Example: NH 4 Cl ammonium chloride NO 3 - -- nitrate ion NH 4 NO 3 ammonium nitrate
Only three polyatomic ions end in ide CN - OH - O 2-2 cyanide hydroxide peroxide Everything else ending in ide is a monatomic anion
A system for oxo-anions Hypo- -ite ( less oxygens than -ate) -ite ( less oxygen than -ate) -ate Per- -ate ( more oxygen than -ate) All polyatomic ions in such a series carry the same charge
Example with chlorate, ClO 3 - Hypochlorite Chlorite Chlorate Perchlorate Example with sulfate, SO 4 2- Sulfite Sulfate There are no hypo-ite or per-ate for sulfate
Formula Name CuCO 3 K 2 CO 3 Ca(ClO) 2 KClO 4 NaClO 3 LiNO 3 Fe(NO 2 ) 3 NaCH 3 COO
How do you know that something is an ionic compound? Ionic compounds contain either a metal & nonmetal or polyatomic ions If the first word in the compound is a metal or ammonium, it is an ionic compound
Name Aluminum hydrogen sulfate Iron (II) oxide Iron (III) oxide Strontium chromate Potassium chloride Ammonium nitrate Lithium sulfite Formula
Ionic compounds must be neutral compounds. All charges of ions must add up to zero Charges come from the associated group in the periodic table or a list Parenthesis must be used when there is some multiple of a certain polyatomic ion
Examples Calcium chloride Calcium is always 2+ (Group 2A on the periodic table) -ide in Chloride tells you that it is monatomic Chloride is always 1- (Group 7A from the periodic table) Criss-Cross Method Ca 2+ Cl - CaCl 2
Iron (III) Sulfate The iron ion carries a charge of 3+ as the Roman numeral is (III) Sulfate is SO 4 2- is a known anion from your memory Criss Cross Method Fe 3+ SO 4 2- Fe 2 (SO 4 ) 3
These are made of two non-metals or metalloids
Two elements with prefixes where the prefix explains the number of atoms of element 1-mono-, 2-di-, 3-tri-, 4-tetra-,5-penta-, 6-hexa-, 7-hepta-, 8-octa-, 9-nona-, 10-deca- The first name is the first element with the appropriate elemental name and prefix for number of atoms Mono- is NOT used when there is only one atom of the first element The second name is the second element with the correct prefix and the suffix of -ide
Formula Name SiO 2 CO CF 4 N 4 O 4 XeF 6 N 2 O 3 P 4 O 7
Name Carbon dioxide Phosphorus trichloride Sulfur tetrafluoride Disulfur dichloride Iodine monochloride Dinitrogen tetroxide Nitrogen triodide Formula
Formulas for acids usually start with H Hydrogen is always the cation For organic acids, the cation is often placed at the end of the formula instead of in the front Acetic acid Inorganic HC 2 H 3 O 2 Organic CH 3 COOH Two types of acids Acids that contain oxygen (oxyacids) Acids that do not contain oxygen
To name all acids, you must look at the anion Oxygen-containing acids have polyatomic anions The name of the polyatomic anion suffix will change: -ate to -ic -ite to ous Per ate to per ic Hypo ite to hypo ous And the second name is acid
Formula Polyatomic Ion Name Name of Acid HClO 4 Perchlorate Perchloric acid H 2 SO 4 Sulfate Sulfuric acid CH 3 COOH Acetate Acetic acid H 2 SO 3 Sulfite Sulfurous acid HNO 2 Nitrite Nitrous acid
If there is no O then there is a hydro- So the prefix for these acids is hydro The suffix changes from the anion which was ide to ic The second name is acid
Formula Ion Name Name of Acid HCN Cyanide Hydrocynanic acid HCl Chloride Hydrochloric acid HBr Bromide Hydrobromic acid
Name Nitric acid Phosphoric acid Hydrofluoric acid Hydrophosphoric acid Carbonic acid Hypochlorous acid Formula
Hydrates are ionic compounds that trap water within their structures. Both the name and the chemical formula specify how much water is contained within the structure.
Write the formula for the ionic compound using the ionic compound rules from previous slides. Add a dot and the correct number of water molecules taken from the prefix and the word hydrate. Example Sodium sulfate decahydrate Na 2 SO 4 10H 2 O
Barium Chloride Dihydrate FeCl 3 6H 2 O