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Binary Ionic Compounds (Type I)

Binary Ionic Compounds (Type I). Contain a cation and anion The cation is always named first and the anion second. Binary Ionic Compounds (Type I). A monatomic cation takes its name from the name of the element

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Binary Ionic Compounds (Type I)

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  1. Binary Ionic Compounds (Type I) • Contain a cation and anion • The cation is always named first and the anion second

  2. Binary Ionic Compounds (Type I) • A monatomic cation takes its name from the name of the element • A monatomic anion is named by taking the first part of the element name and adding -ide

  3. LiI Lithium Iodide AgBr Silver Bromide KF Potassium Fluoride Li3N Lithium Nitride MgO Magnesium Oxide Binary Ionic Compounds (Type I) Practice

  4. Binary Ionic Compounds (Type II) • Involves metals that can form more than one cation • In this case, the charge on the metal ion must be specified with Roman numerals

  5. Binary Ionic Compounds (Type II) • An older system uses the ending -ic on the cation with the higher charge and -ous on the cation with lower charge

  6. CuCl CuCl2 Fe2O3 Copper(I) Chloride Copper(II) Chloride Iron(III) Oxide Binary Ionic Compounds (Type II) Practice

  7. HgO CoCl2 MnO2 Mercury(II)Oxide Cobalt(II) Chloride Manganese (IV) Oxide Binary Ionic Compounds (Type II) Practice

  8. Ionic Compound with Polyatomic Ions • You must MEMORIZE your polyatomic ions!!!! • There are a few hints… • Night-rate NO3- • Night-right NO2-

  9. Ionic Compound with Polyatomic Ions • the polyatomic in a series with less oxygen atoms ends in -ite, the other -ate (The ate ate the ite)

  10. Ionic Compounds with Polyatomic Ions Continued • In summary… • per _ ate 1 more Oxygen • _ate • _ite 1 less Oxygen • hypo_ite 2 less Oxygen

  11. NaOH NH4Cl NaC2H3O2 CaCO3 Sodium Hydroxide Ammonium Chloride Sodium Acetate Calcium Carbonate Practice with Polyatomics

  12. KBrO3 FeSO4 Mn(OH)2 Potassium Bromate Iron (II) Sulfate Manganese (II) Hydroxide Practice with Polyatomics

  13. Binary Covalent Compounds • Formed between two nonmetals • The first element is the full element name • The second element is as if it were an anion

  14. Binary Covalent Compounds • Prefixes are used to denote number of atoms present • “mono” is never used on cation!

  15. Prefixes Used In Binary Covalent Compounds • Mono- 1 • Di- 2 • Tri- 3 • Tetra- 4 • Penta- 5 • Hexa- 6 • Hepta- 7 • Octa- 8

  16. PCl3 NO2 CO N2O5 phosphorus trichoride nitrogen dioxide carbon monoxide dinitrogen pentoxide Practice with Binary Covalent Compounds

  17. Naming Acids • Acid can be viewed as a molecule with one or more H+ ions attached • Rules depend on whether or not oxygen is present

  18. Naming Acids • If the anion DOES NOT contain oxygen the acid is named with the prefix hydro- and the suffix -ic

  19. Naming Acids Continued • If the anion DOES contain oxygen, the acid name is formed from the root name of the anion with a suffix added

  20. Naming Acids Continued • If the anion ends in -ate, the -ate turns to -ic • If the anion ends in -ite, the -ite turns to -ous

  21. HF HCl HNO3 H2SO4 hydrofluoric acid hydrochloric acid nitric acid sulfuric acid Practice Naming Acids

  22. HC2H3O2 HCN H2S HNO2 acetic acid hydrocyanic acid hydrosulfuric acid nitrous acid Practice Naming Acids

  23. The Secret To Nomenclature Is… • Practice! • Practice!! • Practice!!!

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