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Shapes of and Bond Angles in Simple Molecules

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  • 1. Shapes of and Bond Angles in Simple Molecules

2. Introduction

  • In molecules there are 2 types of electron
  • 1. Bonding Pairs
  • 2. Non-bonding or lone pairs

3.

  • pi - bonds have a very limited impact on shape. sigma-bonds have a much more important effect.

4.

  • Ionic bonds - non-directional
  • Covalent bonds have preferred direction in space
  • All covalent compounds have a particular shape
  • As a result of spatial distribution of orbitals.

5. VSEPR Theory

  • Predict the shapes and bond angles of molecules and molecular ions
  • pairs of electrons that surround the central atom of a molecule or ion are arranged as far apart as possible to minimize electron-electron repulsion.

6. VSEPR Theory

  • The idea can be used to predict the shapes of molecules by following a simple procedure:

7. VSEPR Theory

  • Decide which is the central atom in a molecule.
  • In cases of ambiguity, pick the least electronegative atom as this atom will be better able to share its electrons with the other atoms in the molecule.

8. VSEPR Theory

  • Count up the valence (outer shell) electrons on the central atom.
  • Count up the electrons used by the outer atoms to make bonds with the cental atom.

9. VSEPR Theory

  • The sum of ( 2 ) + ( 3 ) divided by two gives the Valence Shell Electron Pair (VSEP) count.
  • The predicted geometry of the molecule is based on the number of VSEP.
  • i.e. the arrangement of EP around the central atom (both lone pair and bonded pair).

10. VSEPR Theory

  • Electrostatic force of repulsion between electron pair.
  • Repulsion- to attain most comfortable arrangement.
  • Each atom wants an octet of electrons.

11. Types of Repulsion

  • Bonding pair- Bonding pair
  • Lone pair-bond pair
  • Lone pair- lone pair

12. Strength of Repulsion

  • Depends on proximity of electron pairs to central atom
  • Lone pairs closer to central atom- they are delocalized- have no other nucleus to attract them
  • Bond pairs attracted to another nucleus

13. Strength of Repulsion

  • Lone pair- Lone pair repulsion > Lone pair- Bond pair repulsion > Bond pair- Bond pair repulsion

14. Effect of Strength

  • Lone pairs push bond pairs closer
  • Smaller angles result

15. Shapes of Molecules 16. Linear

  • 2 bonded pairs
  • 0 lone pairs
  • Bond angle of 180
  • Examples;BeCl2, CO2, HCN, C2H2

17. 18. Trigonal Planar

  • 3 bonding pairs
  • 0lone pairs
  • Bond angle of 120
  • Examples; BF3, SO3, NO3-, CO32-, C2H4

19. 20. 21. Tetrahedral

  • 4 bonding pairs
  • 0 lone pairs
  • Bond angle of 109.5
  • Examples; NH4+, SO42-, PO43-, Ni(CO)4, CH4

22. 23. 24. Trigonal Pyramidal

  • 3 bonding pairs
  • 1 lone pair
  • Bond angle of 107
  • Examples; PH3, SO32-, NH3

25. 26. Bent/ Non-linear

  • 2 bonding pairs
  • 2 lone pairs
  • Bond angle of 105
  • Example; H2S, SO2, H2O

27. 28. Trigonal Bipyramidal

  • 5 bonding pairs of electrons
  • 0 lone pair
  • Bond angles of 120 and 90
  • Example ; PCl5

29. 30. Octahedral

  • 6 bonding pairs
  • 0 lone pair
  • Bond angle of 90
  • Example; SF6

31. 32. 33. Shapes and Bond Anglesof Simple Organic Compounds 34.

  • Organic Compounds- consisting of carbon and hydrogen mostly

35. 36. 37. 38. 39. 40. 41. Sp2 Hybridization 42. 43.


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