1 / 9

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.

clio
Download Presentation

Molecular Compounds

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript


  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

More Related