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Covalent Compounds

Covalent Compounds. January 2015. Covalent Compounds. Covalent Bond – chemical bond that results from sharing electrons Molecule – formed when two or more atoms are bonded covalently. Naming Binary Compounds. First element named first Second elements ending is changed to –ide

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Covalent Compounds

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  1. Covalent Compounds January 2015

  2. Covalent Compounds • Covalent Bond – chemical bond that results from sharing electrons • Molecule – formed when two or more atoms are bonded covalently

  3. Naming Binary Compounds • First element named first • Second elements ending is changed to –ide • Use prefixes to indicate the number of each atom • Examples: • N2O – dinitrogen monoxide • CCl4 – carbon tetrachloride

  4. Prefixes • Mono – • Di- • Tri- • Tetra- • Penta- • Hexa- • Hepta- • Octa- • Nona- • Deca-

  5. Diatomics • There are seven elements that always exist as diatomics • Always exist bonded to themselves in nature • Example: H2 • H BrONClIF or BrINClHOF

  6. Practice – Name or give the Formula • NF3 • P2O5 • F2 • OBr2 • BF3 • CH4 • NO • BN • Carbon disulfide • Selenium • Nitrogen trihydride • Sulfur dioxide • Phosphorous pentabromide • Xenon hexafluoride • Tetraarsenic decoxide • Trinitrogen nonoxide

  7. Answers • Nitrogen trifluoride • Diphosphorus pentoxide • Fluorine • Oxygen dibromide • Boron trifluoride • Carbon tetrahydride • Nitrogen monoxide • Boron mononitride • CS2 • Se • NH3 (ammonia) • SO2 • PBr5 • XeF6 • As4O10 • N3O9

  8. Naming Binary Acids • Contains Hydrogen and one other element • The first word has the prefixhydro- , the rest of the first word consists of the root of the second element plus the suffix–ic • The second word is always acid • Example • HCl : hydrochloric acid • H2S : hydrosulfuric acid

  9. Practice • HBr • HI • H3P • Hydrofluoric acid • Hydroselenic acid • Hydrochloric acid • Hydrobromic acid • Hydroiodic acid • Hydrophosphoric acid • HF • H2Se • HCl

  10. Naming Oxyacid's • Contains both a hydrogen and an oxyanion (polyatomic) • Keep the root of the oxyanion • Include prefixesper- and hypo- as part of the name • If the oxyanion ends in –atereplace with –ic • If the oxyanion ends in –itereplace with –ous • The second word is acid • Example • HNO3 : nitric acid • HClO : hypochlorous acid

  11. Practice • H2SO4 • HClO4 • H3PO4 • Carbonic acid • Acetic acid • nitrous acid • Sulfuric acid • Perchloric acid • Phosphoric acid • H2CO3 • HC2H3O2 • HNO2

  12. What is the formula for hydroxic acid? • H2O • HOH

  13. Formation of Covalent Bonds

  14. Look at Fluorine • Fluorine has 7 valence electrons, it needs 1 more electron to form an octet • As two fluorine atoms approach one another attractive forces and repulsive forces act upon the two atoms • Once that atoms are close enough together they bond covalently to form a fluorine molecule.

  15. Structures Electron Dot Structure Lewis Structure

  16. Practice – Lewis Structures • PH3 • H2S • CCl4

  17. Answers • or • or • or

  18. Single Covalent Bonds • They are also called sigma bonds (σ) • Sigma bonds occur when the shared pair of electrons is centered between the two atoms

  19. Multiple Covalent Bonds • Atoms can share more than one pair of electrons with another atom • Double or Triple bonds • Oxygen and Nitrogen • Multiple covalent bonds consist of one sigma and at least one pi bond (π) • Pi bonds form when parallel orbitals overlap and share electrons

  20. How many Sigma and Pi bonds are there? C2H2 C2H4

  21. More Lewis Structures • NF3 • CO2 • SiF4 • CH4 • OCl2 • NCl3

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