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Rachel Yu 1G
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Joined: Fri Aug 09, 2019 12:15 am


Postby Rachel Yu 1G » Mon Nov 11, 2019 2:08 pm

Explain the difference between boiling points of AsF3 (63 C) and AsF5 (-53 C)

The Lewis structure for AsF3 has three As-F bonds and a lone pair whereas AsF5 had five As-F bonds. Is AsF3 a polar molecule because the As-F bonds create an unequal electron distribution with the presence of the lone pair, therefore having dipole interactions?

Parker Smith
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Joined: Thu Jul 25, 2019 12:15 am

Re: 3F.15

Postby Parker Smith » Mon Nov 11, 2019 2:14 pm

I believe AsF3 is a non polar molecule. The highly electronegative fluorines will direct electron density around themselves, while the lone pair around the Arsenic non bonding domain will remain. Thus, the molecule will have a net negative charge surrounding its entirety.

Lauren Tanaka 1A
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Re: 3F.15

Postby Lauren Tanaka 1A » Tue Nov 12, 2019 5:47 pm

The boiling point of AsF3 will be higher than AsF5 since based on the Lewis structures you can determine that AsF3 is polar and AsF5 is nonpolar based on a net partial negative charge. Thus the dipole-dipole interactions for AsF3 will be stronger than AsF5 causing the boiling point to be higher.

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Re: 3F.15

Postby dtolentino1E » Tue Nov 12, 2019 5:52 pm

a higher boiling point means that the elements in the molecule are highly attracted to each other i.e. the intermolecular forces are strong. because AsF3 is a polar molecule (F, as the most electromagnetic element, creates a dipole) the bonds between the elements are stronger and will take more energy to break apart (become a gas)

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