July 16, 2019, 04:34:48 AM
Forum Rules: Read This Before Posting

Topic: Hybridization of Oxygen in Water  (Read 165 times)

0 Members and 1 Guest are viewing this topic.

Offline Varlam

  • Regular Member
  • ***
  • Posts: 25
  • Mole Snacks: +0/-0
Hybridization of Oxygen in Water
« on: June 26, 2019, 04:38:12 PM »
Electon confuguration of Oxygen is 1s2 2s2 2Px2 2Py1 2Pz1

Why does Oxygen form sp3 hybridization, when it simply can share two 1s1 electrons of hydrogens with its 2Py1 and 2Pz1 to make its each orbital have 2 electons.

Offline Corribus

  • Chemist
  • Sr. Member
  • *
  • Posts: 2669
  • Mole Snacks: +429/-20
  • Gender: Male
  • A lover of spectroscopy and chocolate.
Re: Hybridization of Oxygen in Water
« Reply #1 on: June 26, 2019, 10:22:26 PM »
I don't really love the hybridization model except as a tool to understand molecular geometry, but neither here nor there. I think the first thing to point out is that it's clear what you suggest doesn't happen, because the true geometry of water isn't consistent with the kind of bonding you propose. As to the why, well - there are a lot of ways you could answer that, some due to energy, some due to symmetry. I think most of those explanations would be, based on your questions, a little bit beyond your level. So let's just consider what a water molecule would look like without the hybridization: you'd have two hydrogens in perpendicular orientation, then you'd have a lone pair perpendicular in the third direction, and another lone pair (from the 2S orbital of oxygen) spread spherically around the oxygen nucleus, overlapping with the other lone pair and the electrons in the two O-H bonds. Do you see any problems with this, from an energy standpoint?
What men are poets who can speak of Jupiter if he were like a man, but if he is an immense spinning sphere of methane and ammonia must be silent?  - Richard P. Feynman

Sponsored Links