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| 2 bonded pairs, 1 lone pair |
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| 3 bonded pairs, 1 lone pair |
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| single bond, end to end overlap |
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side to side over lap
weaker than sigma bond |
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| sigma bond and two pi bonds |
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Term
| Permanent Dipole-Dipole attractions |
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Definition
| Attraction between polar molecules, occurs only between two molecules that are polar (atom with high electron negativity bonds with an atom of low electron negativity). Do not require a lot of energy to break, therefore weaker than covalent bonds |
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| • Hydrogen Bonds: Permanent dipole-dipole attractions between Hydrogen and Nitrogen, Flourine or Oxygen are called hydrogen bonds. Strongest type of permanent dipole-dipole bond. |
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| electrons between two atoms shared equally |
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| Occurs between any pair of molecules. Motion of electrons leads to temporary polarization. |
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| strongest forces to weakest forces |
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Definition
Intramolecular
(Covalent)
Intermolecular:
Permanent Dipole-Dipole attractions (Hydrogen Bonds)
Temporary dipole-dipole attractions (Van der Waals)
London dispersion forces |
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| Fats repel water, don’t dissolve in water: Non polar because hydrogen and carbon have similar electron negativity. |
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| No double or triple bonds, contains as many hydrogens as are possible for the carbons on long chain: not very soluble, not healthy |
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| (same side) Double bond with two carbons on same side of double bond, causes kink in chain, will bend molecule |
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| Carbons on opposite side of double bonds |
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| more than one double bond |
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| Hydrocarbons with only single bonds, in an alkane all C’s are sp3 hybridized and because each C is bonded to the maximum number of other atoms (C or H) alkanes are called saturated hydrocarbons. |
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| same formula, different structure |
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| Bonding with any element in the third group or below |
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| Bonding with any element in the first or second period |
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Definition
| Permanent dipole-dipole or hydrogen bonding |
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