1 / 18

Chemistry Inorganic Nomenclature Molecular, Acids, Hydrates

Chemistry Inorganic Nomenclature Molecular, Acids, Hydrates. Do Now: Take out HW to check. CALCULATORS NOT REQUIRED PERIODIC TABLES REQUIRED. Molecular Compounds. Ionic compounds are formed between charged atoms. (Metal + nonmetal)

kaleb
Télécharger la présentation

Chemistry Inorganic Nomenclature Molecular, Acids, Hydrates

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. ChemistryInorganic NomenclatureMolecular, Acids, Hydrates Do Now: Take out HW to check. CALCULATORS NOT REQUIRED PERIODIC TABLES REQUIRED

  2. Molecular Compounds • Ionic compounds are formed between charged atoms. (Metal + nonmetal) • Molecular compounds are formed between two nonmetals, and contain covalent bonds.

  3. Molecular Compounds • In molecular compounds, there is more than one way to put elements together: • N2O, NO2, N2O3, N2, O2, and NO all exist as real compounds. • We need to add Greek prefixes to the names to tell us how many atoms of each element there are.

  4. Greek Prefixes • A prefix is used to denote the number of atoms of each element in the compound (mono- is not used on the first element, however.)

  5. Greek Prefixes • The ending on the second element is changed to –ide. • CO2: carbon dioxide • CCl4: carbon tetrachloride

  6. Greek Prefixes • If the prefix ends with a or o and the second element is oxygen, the two vowels are often meshed into one. • N2O5 : dinitrogenpentoxide (not pentaoxide)

  7. Practice • NO2 • NO • N2O • N2O3 • N2O5

  8. Practice • Tetraphosphoruspentoxide • Sulfur dioxide • Carbon monoxide • Phosphorus pentachloride • Sulfur hexafluoride

  9. Naming Acids • An acid is a compound with H+acting as a cation. • They are polar covalent bonds - in many times, close to ionic.

  10. Naming Acids • If the anion paired with H+ ends in –ide, change the ending to –ic acid and add the prefix hydro. • HCl: hydrochloric acid • HBr: hydrobromic acid • HI: hydroiodicacid

  11. Naming Acids • If the anion ends in –ate, change the ending to –ic acid. • HClO3: chloric acid • HNO3: nitric acid

  12. Naming Acids • If the anion ends in –ite,change the ending to –ousacid. • HClO2: chlorousacid • HNO2: nitrousacid

  13. Exceptions for Sulfur and Phosphorus • H2SO4: sulfuric acid (not sulfic acid) • H3PO4: phosphoric acid (not phosphic)

  14. Practice • HF • H2CrO4 • HClO3 • Hydrosulfuric acid • chloric acid • Phosphoric acid

  15. Naming Hydrates • A hydrate is an ionic compound with water molecules trapped inside the ionic crystal. • These water molecules can be boiled off or re-added.

  16. Naming Hydrates • Their formulas are like normal ionic compounds, with a dot and the number of water molecules trapped per “formula unit” of the ionic compound. • CuSO4•5H2O

  17. Naming Hydrates • CuSO4•5H2O • The word hydrate with a Greek prefix for the number of waters follows the name of the ionic compound. • copper (II) sulfate pentahydrate • CuSO4 5H2O

  18. Practice • CoCl2 • 6H2O • copper (II) chloride dihydrate

More Related