1. Bires, 2007 Slide 1 Back Chapter 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. cationanion cationanion

2. Bires, 2007 Slide 2 Back Naming 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 MagnesiumChlorine Name Chloride

3. Bires, 2007 Slide 3 Back Common anions 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

4. Bires, 2007 Slide 4 Back Multiple Nonmetal 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-” Carbon dioxide Boron trifluoride Carbon tetrachloride Mono in front of a single anion is optional (older) Carbon monoxide

5. Bires, 2007 Slide 5 Back Special Cations : d-block metals Transition metals (d-block): –d-block electrons can migrate into the s and p orbitals. –metals can have several charges when bonding. –Use a Roman Numeral to show the cation’s charge: Fe 2+ Co 3+ Sn 4+ Cr 6+ Iron(II)Cobalt(III)Tin(IV)Chromium(VI) Identify the ions and charges on: V 4+ Cu 2+ Tin (II)Nickel(IV) D-block metals do not follow the octet rule when bonding

6. Bires, 2007 Slide 6 Back Oxidation number –charge that an atom would have when it bonds. The oxidation number of hydrogen in H 2 O is +1. The oxidation number of oxygen in H 2 O 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. (H 2 ) Can you figure the oxidation numbers of the following atoms? Li + Mg 2+ CaSAgCl AlF 3 O 2 +1+2-2-1 +3 0 Some elements can change their oxidation numbers in chemical reactions. You need to predict the oxidation based on the location in the p-table

7. Bires, 2007 Slide 7 Back Polyatomic ions Polyatomic ion: –Ion composed of more than one element. (big) –stable units that bond like individual atoms. Polyatomic ions used in class are: NO 3 - “nitrate”charge of -1 OH - “hydroxide”charge of -1 C 2 H 3 O 2 - “acetate” charge of -1 SO 4 2 - “sulfate”charge of -2 CO 3 2 - “carbonate” charge of -2 PO 4 3- “phosphate”charge of -3 NH 4 + “ammonium”charge of +1

8. Bires, 2007 Slide 8 Back Naming With Polyatomic Ions Use the cation as normal…. Add the name of the polyatomic anion. Here, the compound is Copper (II)sulfate. Copper (II) sulfate Lithium nitrate Lead nitrate

9. Bires, 2007 Slide 9 Back Nomenclature Practice… Name the following: Identify the following compounds: Notice how the NO 3 - polyatomic is placed in ( ) Calcium chloride Barium sulfate Sodium nitrate Strontium fluoride Carbon tetraiodide Copper (II) nitrate (careful) Potassium iodide Boron trichloride Lithium nitrate

10. Bires, 2007 Slide 10 Back Empirical Formula / Molecular 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 ) The empirical formula is useful in determining Percent Composition = mass % of one element in a compound. Calculate the % composition of oxygen in each of these compounds % composition = element mass (g) / empirical formula mass (g) End of chapter 7

11. Bires, 2007 Slide 11 Back CCSD Syllabus Objectives 7.4: Oxidation numbers 8.1: Symbols and Names 8.2: Polyatomic Ions 8.3: Formulas 8.4: Nomenclature 8.5: Empirical/Molecular Formula