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Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: AdiDex on January 19, 2016, 07:53:09 AM

Title: Valence electrons
Post by: AdiDex 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 .

Title: Re: Valence electrons
Post by: Hunter2 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.

Title: Re: Valence electrons
Post by: AdiDex on January 19, 2016, 12:38:26 PM

look at the highlighted pictures ...!! Those do not have 12 electrons .

Title: Re: Valence electrons
Post by: mjc123 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.)