Homework 6.1 c

Moderators: Chem_Mod, Chem_Admin

Isabel Nakoud 4D
Posts: 101
Joined: Fri Sep 28, 2018 12:27 am

Homework 6.1 c

Postby Isabel Nakoud 4D » Tue Nov 13, 2018 10:27 pm

This problem comes from Homework 6.1 (c) on the 6th edition textbook.

For the molecule H2SeO4 , why can Hydrogen Bonding exist as an intermolecular force? Shouldn't the forces only be London or Dipole-Dipole?

jguiman4H
Posts: 31
Joined: Fri Sep 28, 2018 12:29 am

Re: Homework 6.1 c

Postby jguiman4H » Tue Nov 13, 2018 10:32 pm

Image

I used the above for reference. The 2 hydrogens are bonded to their respective oxygens. This is enough for hydrogen bonding because the hydrogens will get their partial positive as O is the most electronegative element present.

All that is needed for hydrogen bonding is an "H atom covalently bonded to an electronegative element and close to another electronegative atom with an available lone pair". Thus, if this selenic acid molecule interacts with another one, hydrogen bonding will occur.


Return to “Interionic and Intermolecular Forces (Ion-Ion, Ion-Dipole, Dipole-Dipole, Dipole-Induced Dipole, Dispersion/Induced Dipole-Induced Dipole/London Forces, Hydrogen Bonding)”

Who is online

Users browsing this forum: No registered users and 1 guest