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Molecular Compounds

Molecular Compounds. Molecular Compounds. Molecular Compounds form between nonmetals and nonmetals. (ex. S 2 O 4 ) Covalent bonds form when atoms share electrons. Neither atoms gain or lose electrons because their electronegativity values are very close.

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Molecular Compounds

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  1. Molecular Compounds

  2. Molecular Compounds • Molecular Compounds form between nonmetals and nonmetals. (ex. S2O4 ) • Covalent bonds form when atoms share electrons. • Neither atoms gain or lose electrons because their electronegativity values are very close.

  3. Naming Binary Molecular Compounds • To name molecular compounds, use prefixes to show how many atoms of each element there are. • Exception: do not show a prefix if the first element has only one atom. • Note: Do NOT reduce if the element ratio is not in lowest terms. • Similar to ionic compounds – last element ends in -ide

  4. Prefix # atoms mono 1 di 2 tri 3 tetra 4 penta 5 hexa 6 hepta 7 octa 8 nona 9 deca 10

  5. Name the following molecular (covalent) compound: SiF4 • Monosilicon fluoride • Sulfur fluoride • Monosilicontetrafluoride • Silicon tetrafluoride • Silicon quadfluoride

  6. Name the following molecular (covalent) compound: SO3 • Sulfur trioxide • Sulfur oxide • Sulfur dioxide • Monosulfur trioxide

  7. Name the following molecular (covalent) compound: S2F6 • Sulfur fluoride • Sulfur hexafluoride • Disulfur fluoride • Disulfur hexafluoride

  8. Acid Nomenclature • In general, names of acids will begin with hydrogen. • If the anion does not contain oxygen, the acid begins with hydro and ends in –ic • HCl = hydrochloric acid • HBr = • HCN =

  9. Acids containing oxygen • If the acid contains oxygen, the acid does not have hydro at the start and either ends in ic or ous. • If the anion ends in –ate use –ic • HNO3 = nitric acid • If the anion ends in –ite use –ous • H2SO3 = sulfurous acid

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