12.17 part b

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Grace Ramey 2K
Posts: 57
Joined: Thu Jul 27, 2017 3:01 am

12.17 part b

Postby Grace Ramey 2K » Mon Dec 04, 2017 9:30 pm

Can someone specifically explain why SO3 is an acidic compound? I am confused because it doesn't have any protons (H+ atoms) to give off. Also, when I drew out the Lewis structure, it appears like a relatively stable molecule.

Thank you for your help!

Isabella Zizolfi 2F
Posts: 21
Joined: Fri Sep 29, 2017 7:05 am

Re: 12.17 part b

Postby Isabella Zizolfi 2F » Mon Dec 04, 2017 10:08 pm

1) It is a nonmetal so this means that it forms acidic oxides
2) it takes e- so it is an electron acceptor

Alexander Peter 1F
Posts: 20
Joined: Wed Jun 28, 2017 3:00 am

Re: 12.17 part b

Postby Alexander Peter 1F » Mon Dec 04, 2017 10:13 pm

When you drew out the structure, you saw that there are 3 double-bonds between S and the O's. To my understanding, because these bonds are between atoms of different electronegativity, SO3 will act as a Lewis Acid. When exposed to an appropriate Lewis Base, one pi-electron pair should shift towards a more negative atom (the electron base).

Amy Zheng 2l
Posts: 57
Joined: Fri Sep 29, 2017 7:04 am

Re: 12.17 part b

Postby Amy Zheng 2l » Tue Dec 05, 2017 11:55 pm

Because S is a nonmetal


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