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1.15 Bonding in Methane and Orbital Hybridization

1.15 Bonding in Methane and Orbital Hybridization. Structure of Methane. tetrahedral bond angles = 109.5° bond distances = 110 pm but structure seems inconsistent with electron configuration of carbon. Electron configuration of carbon. only two unpaired electrons

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1.15 Bonding in Methane and Orbital Hybridization

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  1. 1.15Bonding in Methane andOrbital Hybridization

  2. Structure of Methane tetrahedral bond angles = 109.5° bond distances = 110 pm but structure seems inconsistent withelectron configuration of carbon

  3. Electron configuration of carbon only two unpaired electrons should form sbonds to only two hydrogen atoms bonds should be at right angles to one another 2p 2s

  4. sp3 Orbital Hybridization Promote an electron from the 2s to the 2p orbital 2p 2s

  5. sp3 Orbital Hybridization 2p 2p 2s 2s

  6. sp3 Orbital Hybridization Mix together (hybridize) the 2s orbital and the three 2p orbitals 2p 2s

  7. sp3 Orbital Hybridization 4 equivalent half-filled orbitals are consistent with four bonds and tetrahedral geometry 2p 2 sp3 2s

  8. Shapes of orbitals p s

  9. Nodal properties of orbitals p + – + s

  10. Shape of sp3 hybrid orbitals take the s orbital and place it on top of the p orbital p + – + s

  11. + Shape of sp3 hybrid orbitals reinforcement of electron wave in regions where sign is the same destructive interference in regions of opposite sign s + p + –

  12. – Shape of sp3 hybrid orbitals orbital shown is sp hybrid analogous procedure using three s orbitals and one p orbital gives sp3 hybrid shape of sp3 hybrid is similar sp hybrid +

  13. + – Shape of sp3 hybrid orbitals hybrid orbital is not symmetrical higher probability of finding an electron on one side of the nucleus than the other leads to stronger bonds sp hybrid

  14. + – – The C—H s Bond in Methane In-phase overlap of a half-filled 1s orbital of hydrogen with a half-filled sp3 hybrid orbital of carbon: + sp3 s H C gives a s bond. + H—C s C H

  15. Justification for Orbital Hybridization consistent with structure of methane allows for formation of 4 bonds rather than 2 bonds involving sp3 hybrid orbitals are stronger than those involving s-s overlap or p-p overlap

  16. 1.16sp3 Hybridization and Bonding in Ethane

  17. Structure of Ethane tetrahedral geometry at each carbon C—H bond distance = 110 pm C—C bond distance = 153 pm C2H6 CH3CH3

  18. The C—C s Bond in Ethane In-phase overlap of half-filled sp3 hybridorbital of one carbon with half-filled sp3hybrid orbital of another. Overlap is along internuclear axis to give a s bond.

  19. The C—C s Bond in Ethane In-phase overlap of half-filled sp3 hybridorbital of one carbon with half-filled sp3hybrid orbital of another. Overlap is along internuclear axis to give a s bond.

  20. 1.17sp2 Hybridization and Bonding in Ethylene

  21. Structure of Ethylene C2H4 H2C=CH2 planar bond angles: close to 120° bond distances: C—H = 110 pm C=C = 134 pm

  22. sp2 Orbital Hybridization Promote an electron from the 2s to the 2p orbital 2p 2s

  23. sp2 Orbital Hybridization 2p 2p 2s 2s

  24. sp2 Orbital Hybridization Mix together (hybridize) the 2s orbital and two of the three 2p orbitals 2p 2s

  25. sp2 Orbital Hybridization 3 equivalent half-filled sp2 hybrid orbitals plus 1 p orbital left unhybridized 2p 2 sp2 2s

  26. sp2 Orbital Hybridization p 2 of the 3 sp2 orbitalsare involved in s bondsto hydrogens; the otheris involved in a s bondto carbon 2 sp2

  27. sp2 Orbital Hybridization s p s 2 sp2 s s s

  28. p Bonding in Ethylene the unhybridized p orbital of carbon is involved in p bondingto the other carbon p 2 sp2

  29. p Bonding in Ethylene each carbon has an unhybridized 2p orbital axis of orbital is perpendicular to the plane of the s bonds p 2 sp2

  30. p Bonding in Ethylene side-by-side overlap of half-filledp orbitals gives a p bond double bond in ethylene has a s component and a p component p 2 sp2

  31. 1.18sp Hybridization and Bonding in Acetylene

  32. HC CH Structure of Acetylene C2H2 linear bond angles: 180° bond distances: C—H = 106 pm CC = 120 pm

  33. spOrbital Hybridization Promote an electron from the 2s to the 2p orbital 2p 2s

  34. sp Orbital Hybridization 2p 2p 2s 2s

  35. spOrbital Hybridization Mix together (hybridize) the 2s orbital and one of the three 2p orbitals 2p 2s

  36. sp Orbital Hybridization 2 equivalent half-filled sp hybrid orbitals plus 2 p orbitals left unhybridized 2p 2 p 2 sp2 2s

  37. sp Orbital Hybridization 2 p 1 of the 2 sp orbitalsis involved in a s bondto hydrogen; the otheris involved in a s bondto carbon 2 sp2

  38. sp Orbital Hybridization s 2 p s 2 sp2 s

  39. p Bonding in Acetylene the unhybridized p orbitals of carbon are involved in separatep bonds to the other carbon 2 p 2 sp2

  40. p Bonding in Acetylene one p bond involves one of the p orbitals on each carbon there is a second p bond perpendicular to this one 2 p 2 sp2

  41. p Bonding in Acetylene 2 p 2 sp2

  42. p Bonding in Acetylene 2 p 2 sp2

  43. 1.19Which Theory ofChemical Bonding is Best?

  44. Three Models Lewis most familiar—easiest to apply Valence-Bond (Orbital Hybridization) provides more insight than Lewis model ability to connect structure and reactivity to hybridization develops with practice Molecular Orbital potentially the most powerful method but is the most abstract requires the most experience to use effectively

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