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Molecular Compounds

Molecular Compounds. Covalent Bonds. Molecular Compounds. Also called covalent compounds A molecule is a neutral group of atoms that are held together by covalent bonds The valence e- are shared by the atoms Covalent bonding usually occurs between 2 non-metals

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Molecular Compounds

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  1. Molecular Compounds Covalent Bonds

  2. Molecular Compounds • Also called covalent compounds • A molecule is a neutral group of atoms that are held together by covalent bonds • The valence e- are shared by the atoms • Covalent bonding usually occurs between 2 non-metals • H2O, CO2, O2, NO

  3. Naming Molecular Compounds • Use prefixes 1 mono- 2 di- 3 tri- 4 tetra- 5 penta- 6 hexa- 7 hepta- 8 octa- 9 nona- 10 deca-

  4. Examples Tetraphosphorousdecoxide • P4O10 • N2O3 • As2O5 • OF2 Dinitrogen trioxide Diarsenicpentoxide Oxygen difluoride

  5. Ionic or Covalent Ionic Sodium Bromide • NaBr • CH4 • Fe2O3 • CO2 • CaO • NH4Cl • SiCl4 Carbon tetrahydride Covalent Iron (III) oxide Ionic Carbon dioxide Covalent Ionic Calcium oxide Ionic Ammonium chloride Silicon tetrachloride Covalent

  6. Diatomic Molecules • H2 • O2 • N2 • Cl2 • Br2 • I2 • F2 • 7 diatomic molecules • No noble gases • Halogens and N, O, H • They are all gases (not noble gases) except for Br and I • “Honclbrif”

  7. Empirical Formula • A formula that represents the lowest integral ratio of atoms of the elements in a compound • C2H4, C3H6 and C4H8 all have the same empirical formula: • CH2 • Examples • C2H6O2 • NaC4H6O2  CH3O NaC4H6O2

  8. Naming Acids AnionAcid NameExample -ide hydro—icHCl hydrochloric acid -ite --ous HNO2 nitrous acid -ate --ic HNO3 nitric acid **only binary acids use “hydro”

  9. Try these. . . Sulfuric Acid • H2SO4 • HF • H3PO4 • H2SO3 • H2CO3 • HNO3 Hydrofluoric Acid Phosphoric Acid Sulfurous Acid Carbonic Acid Nitric Acid

  10. More Practice. . . CaBr2 • Calcium bromide • Chromium (III) acetate • Barium sulfate • Copper (I) sulfide • Sulfur hexafluoride Cr(C2H3O2)3 BaSO4 Cu2S SF6

  11. More Practice. . . Chromium (III) oxalate • Cr2(C2O4)3 • Hg(CN)2 • Cu(ClO4)2 • ZnC4H4O6 Mercury (II) cyanide Copper (II) perchlorate Zinc tartrate

  12. How to Calculate Molar Mass • The mass of a compound • In order to calculate molar mass (also called molecular weight) you add up the masses of each element in the compound • Be aware of subscript numbers that designate the amount of atoms per element • You get the masses from the periodic table • **be careful when rounding the mass

  13. Examples 58.5 g/mol • NaCl • Na = 23 g/mol • Cl = 35.5 g/mol • H2O • H = 1 g/mol (but there are 2) = 2 g/mol • O = 16 g/mol • HNO3 • H = 1 g/mol • N = 14 g/mol • O = 16 g/mol (but there are 3) = 48 g/mol • Ba(NO3)2 • Ba = 137.3 g/mol • N = 14 g/mol (but there are 2) = 28 g/mol • O = 16 g/mol (but there are 6) = 96 g/mol 18 g/mol 63 g/mol 261.3 g/mol

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