Register to reply

Delocalization in metals and conjugated systems

by Deadevil
Tags: conjugated, delocalization, metals, systems
Share this thread:
Deadevil
#1
Dec2-13, 11:07 AM
P: 19
Hi Fellow Members,
I am a bit confused about delocalization concept. Since, in organic chemistry we have been told that delocalization only exits between conjugated systems but in inorganic chemistry there is delocalization of electrons in metals with no double bonds. Isn't it confusing, is there a difference between both delocalization. Please help me out.

Thanks
Faisal
Phys.Org News Partner Chemistry news on Phys.org
Building the ideal rest stop for protons
Direct reaction heavy atoms to catalyst surface demonstrated
Cagey material acts as alcohol factory
Borek
#2
Dec2-13, 11:52 AM
Admin
Borek's Avatar
P: 23,393
Delocalization means electron is not bounded to an atom, but can travel much further.

It is possible in conjugated pi systems, it is possible in metals. These are very different systems, but the idea remains the same.
Yanick
#3
Dec2-13, 12:13 PM
P: 380
My limited understanding of each phenomenon is that in a conjugated system the ground electron configuration leads to delocalization whereas in a conductor the valence electron(s) need(s) to overcome the band gap in order to delocalize.

Borek
#4
Dec2-13, 12:30 PM
Admin
Borek's Avatar
P: 23,393
Delocalization in metals and conjugated systems

Not that I feel confident about these things either, but there is no band gap in conductors, that's why they are conductors.
Yanick
#5
Dec2-13, 12:35 PM
P: 380
Quote Quote by Borek View Post
Not that I feel confident about these things either, but there is no band gap in conductors, that's why they are conductors.
Could be, I will do some reading later in the evening. I thought that conductors simply have very small band gaps which are populated at reasonable temperatures according to the Boltzmann distribution. Maybe that is just semantics?

EDIT: Sorry, Borek is correct. Conductors have overlap of valence and conduction bands. See: http://hyperphysics.phy-astr.gsu.edu...lids/band.html
Borek
#6
Dec2-13, 02:05 PM
Admin
Borek's Avatar
P: 23,393
Quote Quote by Yanick View Post
EDIT: Sorry, Borek is correct.
You don't have to be sorry about me being correct

But I am wrong often enough to be happy when I get something right
DrDu
#7
Dec2-13, 02:10 PM
Sci Advisor
P: 3,564
Delocalization always occurs when you can draw several equivalent resonance structures. In organic chemistry, this usually only happens for the pi system, although there are exceptions like e.g. CH5+.
In metals, boron compounds etc. delocalization is more commonplace as metals tend to have more orbitals than electrons, so that more bonding possibilities become possible.
What also matters, i the low electronegativity of metals. This allows for the possibility to include ionic resonance structures, so that not only compounds with alternating bonds will show delocalization.
Deadevil
#8
Dec4-13, 03:47 PM
P: 19
Ok, it means that lewis resonance structure represents only delocalization. bond breakage is only for representation. metal exists as a hybrid structure of lewis resonance structures. Delocalization in metal is due to the increased density of electron in metal. Please Let me know if I am correct.

Thanks
DrDu
#9
Dec5-13, 02:12 AM
Sci Advisor
P: 3,564
Yes, this is basically Pauli's resonating valence bond description of metallic bonding.


Register to reply

Related Discussions
Conjugated polymers Atomic, Solid State, Comp. Physics 2
Slip systems in HCP metals Materials & Chemical Engineering 16
Delocalization of Valence Electrons in Metals Introductory Physics Homework 0
Electron delocalization in Benzophenone Biology, Chemistry & Other Homework 2
Role of Metals in Living Systems Chemistry 3