(Polar molecules, Non-polar molecules, etc.)

Moderators: Chem_Mod, Chem_Admin

Annie Chantasirivisal_4G
Posts: 114
Joined: Wed Sep 18, 2019 12:21 am


Postby Annie Chantasirivisal_4G » Wed Nov 20, 2019 7:28 pm

Estimate the bond angles of peroxyacetylnitrate. *I don't know how to attach an image sorry :c*

Does anyone understand why angle b has to be 109.5 degrees?

I can see that the other two angles are trigonal planar so it explains the 120 degrees, which I assumed also applied to angle b, but since oxygen has two single bonds connected to carbon and oxygen, does that mean that it has two lone pairs on the other side? Which then makes it a tetrahedral with four electron-dense regions? But then why is it 109.5 degrees instead of less than 109.5 degrees?

Tyler Angtuaco 1G
Posts: 130
Joined: Wed Sep 11, 2019 12:16 am

Re: 2.63

Postby Tyler Angtuaco 1G » Wed Nov 20, 2019 7:38 pm

The image in the book does not include lone pairs, but to determine angle b, we have to consider the VSEPR shape of oxygen with the lone pairs in mind (lone pairs exist because of the octet rule). Keeping in mind that lone-pair to lone-pair repulsion is strongest, oxygen would have a tetrahedral electron arrangement but bent shape. Thus, we know that the bond angles are slightly less than 109.5 degrees because of the tetrahedral electron arrangement.

Return to “Determining Molecular Shape (VSEPR)”

Who is online

Users browsing this forum: No registered users and 1 guest