VSEPR Learning

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I cannot take credit for the flash animations of the molecules, I found them online. I could not find anyone to source for those.

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  • There are only two places in the valence shell of the central atom of BeF2 where electrons can be found.Repulsion between these pairs of electrons can be minimized by arranging them so that they point in opposite directions.Therefore the VSEPR theory predicts that BeF2 should be a linear molecule, with a 180° angle between the two Be-F bonds.
  • There are three places on the central atom in BF3 where valence electrons can be found.Repulsion between these electrons can be minimized by arranging them toward the corner of an equilateral triangle.Therefore this theory predicts the F-B-F bond angle to be 120°
  • Have four regions of electron densityThree bonding regions and one lone pair regionIn the NH3 structure, the angle is less than 109° because the lone pair likes to spread out as much as possible
  • There are 6 places on the central atom in these molecule where valence electrons can be foundThe repulsion between these electrons can be minimized by distributing them toward the corners of the octahedron.The term octahedron means 8 sides, but it is the 6 corners, or vertices, that interest us
  • VSEPR Learning

    1. 1. VSEPR THEORY<br />11 Important Shapes of VSEPR<br />
    2. 2. Linear Structures2 electron domains, 0 lone pairs<br /><ul><li>(AX2)
    3. 3. Angle between bonds: 180°
    4. 4. Example: BeF2, HCN, andCO2</li></li></ul><li>Trigonal Planar Structures3 electron domains, o lone pairs<br /><ul><li>(AX3)
    5. 5. Angle between </li></ul>bonds is 120°<br /><ul><li>Example: BF3, BH3</li></li></ul><li>Bent Structures3 electron domains, 2 bonding pairs, 1 lone pairs or 4 electron domains, 2 bonding pairs, 2 lone pairs<br /><ul><li># of bonding pairs-2
    6. 6. # of lone pairs-1
    7. 7. Example: NO2 </li></ul>OR<br /><ul><li># of bonding pairs-2
    8. 8. # of lone pairs-2
    9. 9. Example: H20</li></li></ul><li>Tetrahedral Structures:(4 electron domains, 0 lone pairs)<br /><ul><li>(AX4)
    10. 10. Angle between bonds is ~109.5°
    11. 11. Example: CH4</li></li></ul><li>Trigonal Pyramidal Structures(4 electron domains, 3 bonding pairs, 1 lone pair)<br /><ul><li>(AX3E)
    12. 12. Bond angles are <120°
    13. 13. Structure is non-planar </li></ul> due to repulsion of <br /> lone-pair<br /><ul><li>Example: NH3—bond angles are </li></ul>107°<br />
    14. 14. TrigonalBypyramidal5 electron domains, 0 lone pairs<br /><ul><li>(AX5)
    15. 15. 120° in plane, and 90° above and below
    16. 16. Example: PCl5 , PF5
    17. 17. Repulsion between 5 pairs of valence electrons on the phosphorous atom in PF5 can be minimized</li></ul> by distributing these electrons towards <br /> the corners.<br />
    18. 18. Seesaw5 electron domains, 4 bonding pairs, 1 lone pair<br /><ul><li>(AX4E)
    19. 19. Example: SF4
    20. 20. 5 regions of electron density
    21. 21. In the see saw structure the lone pair is found in the equatorial plane because the lone pair likes to spread out as much as possible.</li></li></ul><li>T-Shaped5 electron domains, 3 bonding pairs, 2 lone pairs<br /><ul><li>(AX3E2)
    22. 22. Example: ClF3
    23. 23. Lone pairs are again found in the equatorial place because the lone pairs want to spread out as much as possible!</li></li></ul><li>Linear5 Electron Domains, 2 bonding pairs, 3 lone pairs<br /><ul><li>(AX2E3)
    24. 24. Example: XeF2, I3 </li></li></ul><li>Octahedral6 electron domains, 0 lone pairs<br /><ul><li>(AX6)
    25. 25. Example: SF6
    26. 26. All angles are 90° </li></li></ul><li>Square Pyramidal6 electron domains, 5 bonding pairs, 1 lone pair<br /><ul><li>(AX5E)
    27. 27. Example: BrF5</li></li></ul><li>Square Planar6 Electron Domains, 4 bonding pairs, 2 lone pair<br /><ul><li>(AX4E2)
    28. 28. Example: XeF4</li>

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