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Chemical Nomenclature

Chemical Nomenclature. 1. Binary Covalent Compounds 2. Binary Ionic Compounds - Type I 3. Binary Ionic Compounds - Type II 4. Ionic Compounds & Polyatomic (Complex) Ions 5. Hydrated Ionic Compounds. Type I Binary Ionic Compounds.

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Chemical Nomenclature

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  1. Chemical Nomenclature 1. Binary Covalent Compounds 2. Binary Ionic Compounds - Type I 3. Binary Ionic Compounds - Type II 4. Ionic Compounds & Polyatomic (Complex) Ions 5. Hydrated Ionic Compounds

  2. Type I Binary Ionic Compounds • The metal cations in these compounds have only ONE possible charge. Na+ Zn2+ Al3+ Ca2+ sodium zinc aluminum calcium The charges are memorized or predicted using a periodic table! • The cations are bonded to nonmetal anions: O2- N3- F- Br - oxide nitride fluoride bromide Notice that simple anions are always named with the suffix “ide”

  3. In an ionic compound, the charges of the cations and anions must always cancel out. • Subscripts are used if more than one atom is needed to cancel the charges: sodium chloride: Na+ and Cl-® NaCl lithium oxide: Li+ and O2-® Li2O aluminum bromide: Al3+ and Br -® AlBr3 zinc nitride: Zn2+ and N3-® Zn3N2 potassium iodide: K+ and I-® KI silver phosphide: Ag+ and P3-® Ag3P

  4. Examples: Type I Binary Ionic Compounds Write the formula: K+ O2- K2O Name the compound: Potassium oxide

  5. Examples: Type I Binary Ionic Compounds Write the formula: Zn2+ Cl- ZnCl2 Name the compound: zinc chloride

  6. Examples: Type I Binary Ionic Compounds Write the formula: Ag+ S2- Ag2S Name the compound: silver sulfide

  7. Examples: Type I Binary Ionic Compounds Write the formula: Al3+ N3- AlN Name the compound: aluminum nitride

  8. Examples: Type I Binary Ionic Compounds Write the formula: Ga3+ O2- Ga2O3 Name the compound: gallium oxide

  9. Examples: Type I Binary Ionic Compounds Write the formula: Ca2+ I- CaI2 Name the compound: calcium iodide

  10. Examples: Type I Binary Ionic Compounds Write the name: K3N potassium nitride Write the ions: K+ N3-

  11. Examples: Type I Binary Ionic Compounds Write the name: AgI silver iodide Write the ions: Ag+ I-

  12. Examples: Type I Binary Ionic Compounds Write the name: ZnBr2 zinc bromide Write the ions: Zn2+ Br -

  13. Examples: Type I Binary Ionic Compounds Write the names: Al2O3 aluminum oxide Write the ions: Al3+ O2-

  14. Examples: Type I Binary Ionic Compounds Write the names: Ba3P2 barium phosphide Write the ions: Ba2+ P3-

  15. Examples: Type I Binary Ionic Compounds Write the name: LiH lithium hydride Write the ions: Li+ H-

  16. Type II Binary Ionic Compounds • These are ionic compounds where the metal cation can form TWO different charges. Fe2+ iron (II) Fe3+ iron (III) Ni2+ nickel (II) Ni3+ nickel (III) Co2+ cobalt (II) Co3+ cobalt (III) Cu+ copper (I) Cu2+ copper (II) Au+ gold (I) Au3+ gold (III) Sn2+ tin (II) Sn4+ tin (IV) An older system uses suffixes and Latin names, -ous for the lower charge, -ic for the higher charge: Ferrous & Ferric, Cuprous & Cupric, Stannous & Stannic

  17. Examples: Type II Binary Ionic Compounds • Write the formulas: • iron (II) oxide • copper (II) chloride • tin (IV) sulfide • cupric nitride • nickel (III) oxide • ferrous iodide • cobalt (III) selenide • Write the names: • Fe2O3 • SnS • NiBr2 • CuS • Pb3P2 • CuBr • FeCl3

  18. Polyatomic (Complex) Ions • All of the cations and anions so far have been simple ions - single atoms that have lost or gained electrons. • A molecule is a particle that forms when two or more atoms bond together. • A complex ion is a charged molecule. Complex ions may be cations or anions. examples: nitrate: NO3- sulfate: SO42- hydroxide: OH-

  19. Writing formulas with Complex Ions a) Ammonium chloride NH4Cl b) Silver sulfate Ag2SO4 c) Aluminum hydroxide Al(OH)3 d) Calcium phosphate Ca3(PO4)2 e) Iron (III) nitrite Fe(NO2)3 f) Copper(II) permanganate Cu(MnO4)2 g) Ammonium dichromate (NH4)2Cr2O7 h) Zinc acetate Zn(CH3COO)2

  20. Things to Notice • Most complex ions are anions. Ammonium, NH4+, is the most common complex cation. • Several complex ions form a short series of ions. The ions differ only in the number of oxygen atoms: perchorate ClO4- sulfate SO42- chlorate ClO3- sulfite SO32- chlorite ClO2- hypochlorite ClO- nitrate NO3- nitrite NO2-

  21. If an ion carries a charge like “-2” or “-3”, a series of related ions can be formed by adding hydrogen cations (H+) while still leaving a net charge: examples: Sulfide: S2- hydrogen sulfide: HS- (bisulfide) Sulfate: SO42- hydrogen sulfate: HSO4- (bisulfate) Carbonate: CO32- hydrogen carbonate: HCO3- (bicarbonate) Phosphate: PO43- hydrogen phosphate: HPO42- dihydrogen phosphate: H2PO4-

  22. More Formulas with Complex Ions a) Sodium bicarbonate NaHCO3 b) Nickel (II) hydrogen sulfide Ni(HS)2 c) Aluminum perchlorate Al(ClO4)3 d) Barium dihydrogen phosphate Ba(H2PO4)2 e) Iron (III) sulfite Fe2(SO2)3 f) Cuprous bisulfate CuHSO4 g) Zinc periodate Zn(IO4)2 h) Lithium selenite Li2SeO3

  23. Hydrated Ionic Compounds • A HYDRATE is an salt that has water molecules trapped within its crystals. • Every hydrate has a certain number of water molecules associated with each formula unit of the ionic compound. The number of water molecules is indicated by using prefixes. mono hexa di hepta tri octa tetra nona penta deca CuSO4 · 5 H2O copper (II) sulfate pentahydrate MgCO3 ·10 H2O magnesium carbonate decahydrate

  24. Examples of hydrates: • Write the formulas: copper(II) fluoride tetrahydrate CuF2·4 H2O calcium nitrate trihydrate Ca(NO3)2 ·3 H2O • Write the names: MgSO4· 7 H2O magnesium sulfate heptahydrate FeCl2 · H2O iron (II) chloride monohydrate

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