Ch 2 notes Pt. 2

  1. Four regions of electron density =
    four hybrid orbitals
  2. How many shapes are there in organic chem?
    only three
  3. What is an sp3?
    an orbital that has a saturated center
  4. SP2 in terms of four bonds?
    has three sigma bonds and the p orbital will be a pi bond
  5. Explain charges with pi bonds.
    • + with +
    • - with -
    • they have to be parallel and in phase¬†
    • weaker and more exposed
  6. The pi bond is __ to the plane of the molecule.
  7. Every carbon carbon bond has only one __.
    sigma bond
  8. Isomers:
    stereoisomers (geometric isomers)
    • compounds don't rotate
    • configuration around double bonds determines the compound
  9. Those isomers that have different connectivities are __.
    structural isomers (constitutional)
  10. Bonds
    • London Dispersion forces
    • hydrogen bond
    • dipole dipole
  11. A greater surface area will result in __
    a higher melting point
  12. Explain BP in terms of constiutional isomers.
    the least branched isomer will have hte greatest boiling poin because they can stack the together

    the most branched has the lowest boiling point
  13. Bonding takes place in __.
    constructive overlap
  14. __ is shorter than __.
    • sp2
    • sp3
  15. Lone pairs are very strongly __.
  16. More polar bonds are __.
    they are more polar because the direction of NH3 does not cancel out as much as NCl3
  17. Intermolecular Forces
    London Dispersion forces
    • very weak
    • temporary dipoles
    • more increased SA, the better chance at keeping together¬†
    • affects solubility and properties
  18. Hydrogen bonding
    - strongest of intermolecular forcesmust contain NH or OH
Card Set
Ch 2 notes Pt. 2