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Molecular Geometry and Polarization

Molecular Geometry and Polarization. Shapes of Molecules. Valence Shell Electron Pair Repulsion Theory (VSEPR) a. Bonded electrons b. Lone Pairs. 1. Linear (180 o ) BeH 2 CO 2. 2. Trigonal Planar (120 o ) NO 3 -. 3. Tetrahedral (109.5 o ) CH 4.

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Molecular Geometry and Polarization

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  1. Molecular Geometry and Polarization

  2. Shapes of Molecules Valence Shell Electron Pair Repulsion Theory (VSEPR) a. Bonded electrons b. Lone Pairs

  3. 1. Linear (180o) BeH2 CO2

  4. 2. Trigonal Planar (120o) NO3-

  5. 3. Tetrahedral (109.5o) CH4

  6. 4. Trigonal Pyramidal (~107o) NH3

  7. 5. Bent (~104.5o) H2O

  8. O H H

  9. SO2

  10. 6. Trigonal Bipyramid (120o, 90o) PCl5

  11. 7. Octahedral (90o) SF6

  12. Shapes of Molecules Ex: Multiple Bonds: N2 H2CO HCN SO2

  13. Shapes of Molecules

  14. Models Activity

  15. SO22+ SO22- SO2 SO3 SF3- PF4- XeCl5+ BrF4-

  16. Predict the molecular geometry of: SnCl3- O3 SeCl2 CO32- SF4 IF5 ClF3 ICl4-

  17. WarmUp • ClF4- SiCl3- SO2 • SCl4 SeO3 BrCl5 BrCl3

  18. Polar Molecules 1. Polar molecule – Overall, the electrons are attracted more to one end of an entire molecule 2. Non-Polar Molecule – The electrons are spread out evenly over the entire molecule -/ + Partial (not full) charges

  19. Examples: H2 H2O CH4 H2CO

  20. Electron Density H2 H2O CH4 H2CO

  21. Polar Molecules BeCl2 NH3 CO2 SO2 SF6 BCl3 CH2Cl2

  22. SCO CH3F BH2Cl PH3

  23. CHF3 CH2F2 SO3 SO32- NF3 CH3CHO

  24. Hybrid Orbitals • A mixing of the atomic orbitals (s, p, d, f) of the central atom • Electrons no longer move in the old orbitals, but in a new pattern

  25. BeF2 Isolated Be 1s22s2 (Note that all Be: electrons are paired) To bond Be must unpair some electrons: Bonded Be 1s22s12p1 •Be•

  26. Be is called an “sp” hybrid. • Drawings: Isolated BeBeF2

  27. CH4 Isolated C 1s22s22p2 Bonded C 1s22s12p3

  28. Isolated C Bonded C sp3

  29. Effect of Lone Pairs • Lone pairs do count towards hybridization • Ex: H2O

  30. Try BF3

  31. Examples CCl4 NH3 PF5 SF6 XeF4 BrF3

  32. PH3 H2S SF5- SF4 CO32- HCN BrCl3 CH4

  33. H2S SO2 SO22- AsCl5 ClF3 KrF4

  34. Hybrid Orbitals and Multiple Bonds • sigma () bonds – single bonds formed by hybrid orbitals • pi () bonds – double or triple bonds, not formed by hybrid orbitals H H H – H C=C :N=N: H H One  bond One  bond plus One  bond plus one  bond two  bonds

  35. Consider C2H4 • Each C is sp2 • Double bond does not count toward hybridization

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