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Unit 2 : Chapter 4

Unit 2 : Chapter 4. Nomenclature International naming system. Rules for a molecular formula for an ionic compound. A molecule is made of a positive and negative charged ion. The positive ion (cation) is written first. The negative ion (anion) is written second.

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Unit 2 : Chapter 4

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  1. Unit 2 : Chapter 4 Nomenclature International naming system

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

  3. 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

  4. 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

  5. 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

  6. Examples: CO Carbon monoxide CO2 N2O4

  7. Polyatomic – must memorize the names! • Oxy anions: elements with oxygen acting as polyatomic ions • More than large number of oxygen (per-)(-ate) • Large number of oxygen (-ate) • Small number of oxygen (-ite) • Less than small number of oxygen (hypo-)(-ite) Example: perchlorate ClO4-1 chlorate ClO3-1 chlorite ClO2-1 hypochlorite ClO1-1

  8. MgSO4 MgSO3 LiNO2 LiNO3

  9. Naming Acids – when dissolved in H2O they produce free protons (H+) • If anion doesnot contain oxygen • Use prefix (hydro-) with suffix (-ic) on the anion example HS 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 HClO4perchlorate perchloric acid HClO3 chlorate chloric acid HClO2 chlorite chlorous acid HClO hypochloritehypochlorous acid

  10. HCl HNO3 HNO2

  11. 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

  12. Writing Formula’s

  13. 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.

  14. Cubic Tetragonal • Monoclinic Orthorhombic • Triclinic Hexagonal

  15. Crystal shape lab 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

  16. Review • H2O use any that have 2 or more atoms • H, or He, or C • 14 total atoms, 2 N, 8 H, 1 C, 3 O • Os, Atomic # 76, Atomic mass 190, 76 p+ ,76 e-, 114 n • Yttrium, Atomic # 39, Atomic mass 89, 39 p+, 39 e-, 50 n • N 7 7 7 7 14 Be 4 4 4 5 9 Be 4 4 4 6 10 7. 199 F (round atomic mass to nearest whole number) • Column containing F, Cl, Br, I, At • charged particle made of an atom that has gained or lost e- • e- • Ba  Ba+2 + 2 e- 1 e- + F  F-1 • Potassium chloride, Lead (II) iodide, Calcium nitrate, Nitrogen dioxide, Acetic acid • MgO, CoCl2 , (NH4)2S, CO, HBr

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