IBDP HL bonding

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IBDP HL bonding

  1. 1. Draw the VESPR structures for 14.1.1 Include bond angles, names of shapes
  2. 2. Bonding AHL• Describe sigma and pi bonds• Explain hybridization in terms of sp sp2 sp3• Explain relationship between Lewis structure, shape and hybridisation
  3. 3. Sigma Bonds• Sigma bonds are all single bonds, and result from axial overlap of orbitals.
  4. 4. π Bonds• Result from sideways overlap of parallel porbitals
  5. 5. Basics• A single bond is a SIGMA bond• A double bond is ONE SIGMA ONE PI• A triple bond is ONE SIGMA TWO PI
  6. 6. Hybridisation – sp3
  7. 7. Hybridisation – sp2
  8. 8. Hybridisation - sp
  9. 9. Homework Task• Using the following molecules create a student help sheet to explain the bonding, the shape, the hybridisation, and number of sigma and pi bonds.• In Carbon Dioxide, Methane and Propene.
  10. 10. Geometry and Hybridisation• All you have to do is count the negative centres, and don’t forget lone pairs• Inorganic : • 4 negative centres is sp3, e.g. NF3 ( 3bp 1nbp in this case ) • 3 negative centres is sp2, e.g. BF3 ( 3bp in this case ) • 2 negative centres if sp• Organic : • sp3 is Td 109.5, e.g. Alkanes • sp2 is Trig Pl 120, e.g. Alkenes, Carbonyl groups • sp is lin 180, e.g. Alkynes
  11. 11. Starter• Explain how sp2 hybridization arises • Use electrons in boxes notation to explain your answer.
  12. 12. When electron pairs are not confinedto two adjacent bonding atoms but extend over 3 or more atoms
  13. 13. Benzene Facts • Planar regular hexagon• All bond angles 120 degrees• Bond lengths intermediate between single and double bonds• Reluctant to undergo addition reactions.
  14. 14. Nitrate Ion
  15. 15. Nitrite Ion Resonance Structures ?
  16. 16. Carbonate Anion
  17. 17. Ozone
  18. 18. Ethanoate
  19. 19. Learning Check • N01/420/H(2) part (a) ONLY

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