In the situation where two Nitroglycerin molecules cam across each other, there would be three forces of attraction: Hydrogen Bonding (as said before), Dipole/Dipole, and London Dispersion Forces
- Hydrogen Bonding is present because Hydrogen is present with Nitrogen as well as Oxygen.
- Dipole/Dipole attraction is present because of the electrostatic attraction between both polar nitroglycerin molecules.
- London Dispersion Forces are present because every molecule has this weak attraction due to the movement of electrons around two atoms.
Max, the general appearance of your blog ad is very organized and easy to follow. Your molecule's lewis structure is accurate and similar to the dash model of nitroglycerin. I can also tell that nitroglycerin is polar due to the fact that it contains solely one line of symmetry. Moreover, I understand that nitroglycerin possesses all three intermolecular forces. Thus, I am convinced that I should purchase nitroglycerin if I am a doctor or someone affiliated with the military.
ReplyDeleteI do not think that nitroglycerin contains hydrogen bonds because the hydrogen is bonded to the carbon atoms. I only know this because I did a project on it where I had to research the molecule.
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