Nomenclature International naming system Unit 4 Nomenclature International naming system

[ ] Types of Bonding Ionic Bonding – between a metal & non-metal Transfer of e- resulting in a positive ion and a negative ion that are attracted to each other. Metal – outer energy level (valence orbitals) are emptied Non – metal – outer energy level (valence orbitals) fill to have the configuration of the next Noble gas. Covalent Bonding: between Non-metals Sharing of e- in such a way as to complete the outer energy level (valence orbitals) of both (all) atoms. All atoms end up with the e- configuration of Noble gases. [ ]

Rules for a molecular formula for an ionic compound A molecule is made of a positive and negative charged ion. The positive ion is written first. The negative ion is written second. (+) + (-) = 0, the total charge on a molecule must equal zero. Use subscripts to indicate the number of each ion to use.

Inorganic binary compounds type I one atom type (+) cations maintain atom name one atom type (-) anions change name (-ide) (+) cation is followed by the (-) anion Example: NaCl Sodium chloride CaF2

Inorganic type II – some anions form multiple charges (the Transition metals) Use Roman numerals to indicate charge example: CuCl – copper (I) chloride, CuCl2 – copper (II) chloride Or/ higher charge name ends with (-ic) while lower charge name ends with (-ous) example: FeCl3 ferric chloride FeCl2 ferrous chloride SnI4 SnI2 2 naming methods: new & old

Binary Covalent type III – 2 nonmetals 1st element in formula named first with full element name 2nd element named as if anion, end with –ide Prefixes used to denote number of atoms present Mono is never used for 1st element mono - 1 hexa - 6 di - 2 hepta - 7 tri - 3 octa - 8 tetra - 4 nona - 9 penta - 5 dec - 10

Examples: CO Carbon monoxide CO2 N2O4

Polyatomic – must memorize the names! Oxy anions: elements with oxygen acting as polyatomic ions Large number of oxygen (-ate) Small number of oxygen (-ite) More than large number of oxygen (per-) Less than small number of oxygen (hypo-) Example: perchlorate ClO4-1 chlorate ClO3-1 chlorite ClO2-1 hypochlorite ClO1-1 There are a few polyatomic ions without oxygen !

MgSO4 MgSO3 LiNO2 LiNO3

Naming Acids – when dissolved in H2O they produce free protons (H+) If anion does not contain oxygen Use prefix (hydro-) with suffix (-ic) on the anion example H2S hydrosulfuric acid If anion does contain oxygen If anion ends in (-ate) use root name with (-ic) H2SO4 sulfuric acid If anion ends in (-ite) use root name with (-ous) H2SO3 sulfurous acid When multiple oxyanion use Example HClO4 perchlorate perchloric acid HClO3 chlorate chloric acid HClO2 chlorite chlorous acid HClO hypochlorite hypochlorous acid

HCl HNO3 HNO2

Combining ions to form compounds and write formulas. 1. Positive and negative ions combine to form neutral compounds. 2. When writing formulas, write the positive ions first. Write the negative ions second. 3. The electrical charge for a compound must be neutral (zero). Examples: Sodium chloride Barium sulfide Zinc iodide Nickel phosphate Ammonium carbonate

Writing Formula’s Oxide O-2 Iodide I-1 Sulfate SO4-2 Cyanide CN-1 Hydrogen H+1 Barium Ba+2 Chromium Cr+3

Review 1. Potassium chloride Lead (II) iodide Calcium nitrate Nitrogen dioxide Acetic acid 2. MgO CoCl2 (NH4)2S CO HBr

Periodic Table Crossword Down 2. Affinity 8. Ramsey 14. Ionization 34. Actinide 37. Mosely Across 6. Carbon 12. Transition 33 Lanthanide

Crystals All solids form geometric figures in which the atoms and molecules are arranged in a regular repeating pattern. Solid geometric figures are called crystals. Crystals have plane surfaces that are at definite angles to one another. There are 6 crystal structures.

Cubic Tetragonal Monoclinic Orthorhombic Triclinic Hexagonal

Crystal shape lab PbS FeS2 ZrSiO4 Ca6Al3OH or F(SiO4)5 SiO2 CaCO3 S 1. Cr2K2(SO4)4.24H2O PbS FeS2 ZrSiO4 Ca6Al3OH or F(SiO4)5 SiO2 CaCO3 S BaSO4 CaSO4.2H2O Ni(NH4)2(SO4)2.6H2O CuSO4.5H2O