May 01, 2024, 04:22:17 PM
Forum Rules: Read This Before Posting


« previous next »
Pages: [1]   Go Down

Topic: Valence electrons  (Read 1867 times)

0 Members and 1 Guest are viewing this topic.

Offline AdiDex

  • Full Member
  • ****
  • Posts: 305
  • Mole Snacks: +16/-12
  • Gender: Male
Valence electrons
« on: January 19, 2016, 07:53:09 AM »
I am Really confused ?? How can these Oxygen molecules can be stable than O=O ??  even in these pictures oxygen molecules do not have 12 electrons ..!! and no positive charge is shown .!!

these are pics from March's Advance Organic chemistry Edition 6th and 7th ..!! Anybody please help .

Logged

Offline Hunter2

  • Sr. Member
  • *****
  • Posts: 2181
  • Mole Snacks: +168/-48
  • Gender: Male
  • Vena Lausa moris pax drux bis totis
Re: Valence electrons
« Reply #1 on: January 19, 2016, 10:17:34 AM »
Each Oxygen is [He]2s2sp4. Together 6 Electrons on the outer shell. Together 12 if 2 Atoms built a molecule.
Logged

Offline AdiDex

  • Full Member
  • ****
  • Posts: 305
  • Mole Snacks: +16/-12
  • Gender: Male
Re: Valence electrons
« Reply #2 on: January 19, 2016, 12:38:26 PM »
look at the highlighted pictures ...!! Those do not have 12 electrons .
Logged

Offline mjc123

  • Chemist
  • Sr. Member
  • *
  • Posts: 2053
  • Mole Snacks: +296/-12
Re: Valence electrons
« Reply #3 on: January 19, 2016, 01:05:33 PM »
They are wrong. Double bonded O2 has two lone pairs on each O. Single bonded O2 has two lone pairs and an unpaired electron on each O. (Actually the unpaired electrons are in degenerate π bonding orbitals, so the molecule has effectively a double bond, but it's hard to show this in Lewis structures.)
Logged
Pages: [1]   Go Up
« previous next »
Sponsored Links