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Covalent bonding

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Covalent bonding

  1. 1. Covalent BondingBonding models formethane, CH4. Models areNOT reality. Each has itsown strengths andlimitations.
  2. 2. CA Standards Students know atoms combine to formmolecules by sharing electrons to formcovalent or metallic bonds or by exchangingelectrons to form ionic bonds. Students know chemical bonds betweenatoms in molecules such as H2, CH4, NH3,H2CCH2, N2, Cl2, and many large biologicalmolecules are covalent. Students know how to draw Lewis dotstructures.
  3. 3. The Octet Rule and Covalent Compounds Covalent compounds tend to form so thateach atom, by sharing electrons, has an octetof electrons in its highest occupied energy level. Covalent compounds involve atoms ofnonmetals only. The term “molecule” is used exclusively forcovalent bonding
  4. 4. The Octet Rule: The Diatomic Fluorine MoleculeF 1s 2s 2p Each has seven valenceF electrons 1s 2s 2p F F
  5. 5. The Octet Rule: The Diatomic Oxygen MoleculeO 1s 2s 2p Each has six valenceO electrons 1s 2s 2p O O
  6. 6. The Octet Rule:The Diatomic Nitrogen MoleculeN 1s 2s 2p Each has five valenceN electrons 1s 2s 2p N N
  7. 7. Lewis StructuresLewis structures show how valence electrons are arranged among atoms in a molecule.Lewis structures Reflect the central idea that stability of a compound relates to noble gas electron configuration.Shared electrons pairs are covalent bonds and can be represented by two dots (:) or by a single line ( - )
  8. 8. The HONC RuleHydrogen (and Halogens) form one covalentbondOxygen (and sulfur) form two covalent bonds One double bond, or two single bondsNitrogen (and phosphorus) form three covalentbonds One triple bond, or three single bonds, or one double bond and a single bondCarbon (and silicon) form four covalent bonds. Two double bonds, or four single bonds, or a triple and a single, or a double and two singles
  9. 9. Completing a Lewis Structure -CH3Cl Make carbon the central atom (it wants themost bonds, 4) Add up available valence electrons:  C = 4, H = (3)(1), Cl = 7 Total = 14 Join peripheral atoms Hto the central atom withelectron pairs. .. .. .. H .. C Cl Complete octets on .. ..atoms other than Hhydrogen with remainingelectrons
  10. 10. Bond Length and Bond EnergyBond Length (pm) Energy (kJ/mol)C-C 154 346C=C 134 612C C 120 835C-N 147 305C=N 132 615C N 116 887C-O 143 358C=O 120 799C O 113 1072N-N 145 180N=N 125 418N N 110 942
  11. 11. Resonance Occurs when more than one valid Lewis structure can be written for a particular molecule. These are resonance structures. The actual structure is an average of the resonance structures.
  12. 12. Resonance in Benzene, C6H6

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