Ch 10 Ppt

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  1. In terms of distance, what are gases? They have what? 
    We can do what to form a __.
    Compared to solids, they are __. Why is this?
    • far apart
    • elastic energy
    • compress them to form a liquid
    • not as rigid as solids 
    • solids can't flow
  2. What are intermoleuclar forces?
    attractions between "molecules" that hold them together
  3. What are intramolecular forces?
    forces holding together particles, such as polar covaluent bonds
  4. __ form between atoms of different __. This is described as a __, one type of __ force.
    • polar covalent bonds
    • electronegativity
    • bond dipole
    • intramolecular force
  5. What is a dipole moment?
    • the measure of net molecular polarity or charge separation 
    • u= Q ' r
    • r= distance between charges
  6. Dipole moments are expressed in __.
    debyes (D)
  7. Polarity can be illustrated with an __.
    electrostatic potential map
  8. What do electrostatic potential maps show?
    electron-rich groups as red and electron-ppor groups as blue-green
  9. The greater the charge, the __ the dipole moment.
  10. If you have a non-polar moment, will it have a dipole moment?
    What is the minimum requirement of a diploe moment?
    • no 
    • must have a polar attraction
  11. If arranged asymmetrically, what happens with the dipole moment?
    What is it called? Where does it occur?
    • they will not cancel each other out
    • net dipole moment
    • toward lone pair
  12. The individual bond polarities do not cancel. Therefore, the molecule has a __. In other words, the molecule is __.
    • dipole moment
    • polar
  13. The individual bond polarities cancel. Therefore, the molecule does not have a __. In other words the molecule is __.
    • dipole moment
    • nonpolar
  14. What are intermolecular forces?
    • attractions between "molecules" that hold them together
    • much weaker than intramolecular forces
  15. Types of intermolecular forces?
    • ion-dipole forces
    • van der waals forces: dipole-dipole forces; London dispersion forces; hydrogen bonds
  16. Ion-dipole forces
    the result of electrical interactions between an ion and the partial charges on a polar molecule
  17. Dipole-dipole forces
    result of electrical interactions among dipoles on neighboring moleucles
  18. Do you get a complete charge with a dipole species?
    no; partial
  19. Melting point of ion-dipole?
    higher due to stronger forces
  20. The higher the molecular weight, the more likely what?
    it'd become a solid
  21. As the dipole moment incresaes, what?
    the intermolecular forces increases
  22. As the intermolecular forces increase, what happens?
    the boiling point incresaes
  23. London Dispersion Forces
    the result of the motion of electrons which gives the molecule a short-lived dipole moment. This induces temporary dipoles in neighboring molecules
  24. There may be instances where both electrons are at one part of the molecule instead of shared. This is called __
    instantaneous dipoles; they are not fixed
  25. The bigger hte molecule is, what?
    the more likely this is to occur (the instataneous dipoles)
  26. hydrogen bond
    an attractive force between a H atom bonded to  very electronegative atom and an unshared electron pair on another electronegative atom
  27. Hydrogen bonds are (stronger/ weaker) than ordinary attractions.
  28. What characteristics does hydrogen bonding give to water?
    • higher melting point
    • solidifying causes it to expand; ice is less dense
    • huge temp. changes in desert due to no H2O available since water is a great absorber of heat
  29. Strength of covalent bond weaker than hydrogen.
    false: stronger
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Ch 10 Ppt
2013-01-31 22:28:37
CHM 112

Ch 10
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