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| ------ Dipole Dipole, ______ Hydrogen |
If you were to put 2 Ethanol molecules next to each other, they would have 3 types of intermolecular forces bonding them together. The first force would be London Dispersion. This happens between all molecules, no matter what (see below). The second force would be Dipole Dipole (see below). Because Ethanol is a polar molecule, it has positive and negative ends. This allows itself to bond to other Ethanol molecules, as seen by the dotted line above. The third and strongest intermolecular force would be the Hydrogen bond between H and O (see below).
London Dispersion- The weakest of the 3 listed intermolecular forces, this attraction takes place between every molecule. The attraction is caused by the exchange of electrons between molecules.
Dipole Dipole- This attraction, shown by the dotted line, is the positive end (Hydrogen) of a dipole being attracted to the negative end (Oxygen) of another dipole.
Hydrogen Bonding- The strongest bond of the three, it takes place between a Hydrogen and the F, N, or O of another molecule. This bond is shown by the full line above.
Thank you sooo much!!! I really needed this :D!
ReplyDeletethis is actually wrong because hydrogen bonds can't happen on a hydrogen that is bonded to a carbon atom, it only happens on fluorine, oxygen, and nitrogen
ReplyDeletebruh, its talking about INTERmolecular forces, therefore meaning that its the bonds BETWEEN molecules, and the C-H bond you're talking about is an INTRAmolecular bond
Deleteget shrek'd by the king of chemistry, you doofus
surely talking about inter molarcule read carefully...
Delete