Intermolecular farces

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Karolina herrera1F
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Joined: Sat Feb 02, 2019 12:15 am

Intermolecular farces

Postby Karolina herrera1F » Tue Jul 16, 2019 10:09 pm

Can someone please explain what would be the intermolecular forces of O=C=O and N=N. Can O=C=O be a a dipole? Or can it not because it has both oxygens on each of the sides? Would N=N just be non polar?

Brian Kwak 1D
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Re: Intermolecular farces

Postby Brian Kwak 1D » Wed Jul 17, 2019 10:04 am

dipole moment would be calculated by the electronegativity difference between the atoms then you use that to figure out the intermolecular force. The dipole moment cancels in CO2 due to the shape. N2 has no dipole moment because there is no electronegativity difference. So the only forces would London dispersion.
Last edited by Brian Kwak 1D on Wed Jul 17, 2019 10:46 am, edited 3 times in total.

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Re: Intermolecular farces

Postby Chem_Mod » Wed Jul 17, 2019 10:09 am

Both CO2 and N2 are nonpolar molecules. The molecular shape of CO2 and N2 is linear. There is no dipole moment for N2 since there is no difference in electronegativity between the two Ns. There is a difference in electronegativity between C and O but those dipole moments cancel each other out since the molecular shape is linear. Therefore, there are weak intermolecular forces for CO2 and N2 called London dispersion forces or induced dipole-induced dipole forces.


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