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July 10, 2025, 02:24:04 am
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Author Topic: Benzene  (Read 2682 times)  Share 

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WhoTookMyUsername

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Benzene
« on: April 23, 2011, 12:04:36 pm »
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I'm a tad confused about the properties of Benzene.
Does anyone know chemicals / molecules with similar chemical propities to Benzene?
And also why is ethane etc. not similar in reactions, but similar in structure?
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taiga

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Re: Benzene
« Reply #1 on: April 23, 2011, 12:15:11 pm »
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Ethane isn't similar in structure to Benzene at all.

Benzene is cyclic in nature, ethane is a two carbon chain (I'm not sure what it is specifically called).

Another cyclic compound you may see in VCE is Cyclohexane; C6H12, except the carbons are bonded in a circular nature.
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burbs

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Re: Benzene
« Reply #2 on: April 23, 2011, 12:19:25 pm »
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This is ridiculous, you are only like 2 chapters behind me and are in year 11.

But yeah, they are completely different structurally. Similarities they have are... both are hydrocarbons and share the general properties of them?
« Last Edit: April 23, 2011, 12:21:53 pm by burbs »
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burbs

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Re: Benzene
« Reply #3 on: April 23, 2011, 01:00:21 pm »
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Quote from: Bazza16 on April 23, 2011, 12:51:10 pm
okay thanks, i'll have a look at aromatic hydrocarbons.
This is necessary for a project we're doing, we have to present about a molecule, and i chose Benzene not knowing its complexity :(

Yeah we figured. How would you show the double bonds? Benzene double bonds move. Your project just jumped from Styrofoam and toothpicks to needing a motor!
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pi

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Re: Benzene
« Reply #4 on: April 23, 2011, 01:13:20 pm »
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Quote from: burbs on April 23, 2011, 01:00:21 pm
Yeah we figured. How would you show the double bonds? Benzene double bonds move.

There are no double bonds... Look up resonance for more info.
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pi

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Re: Benzene
« Reply #5 on: April 23, 2011, 01:18:46 pm »
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Quote from: Bazza16 on April 23, 2011, 01:15:45 pm
lol. I think i'll just do double bonds and single bonds and talk about the limitations of the model and cop a B

Dude, everyone cops at least an A...
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Water

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Re: Benzene
« Reply #6 on: April 23, 2011, 01:19:29 pm »
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Quote from: pi on April 23, 2011, 01:18:46 pm
Quote from: Bazza16 on April 23, 2011, 01:15:45 pm
lol. I think i'll just do double bonds and single bonds and talk about the limitations of the model and cop a B

Dude, everyone cops at least an A...

Disappointed in you Bazza, B's not good enough.

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« Last Edit: January 15, 2017, 05:53:59 pm by pi »
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burbs

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Re: Benzene
« Reply #7 on: April 23, 2011, 02:08:59 pm »
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Quote from: pi on April 23, 2011, 01:13:20 pm
Quote from: burbs on April 23, 2011, 01:00:21 pm
Yeah we figured. How would you show the double bonds? Benzene double bonds move.

There are no double bonds... Look up resonance for more info.

Aren't there alternating double bonds?

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« Last Edit: January 15, 2017, 05:53:11 pm by pi »
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burbs

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Re: Benzene
« Reply #8 on: April 23, 2011, 02:16:02 pm »
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Right yeah, delocalised electrons. I still think I've read in quite a few places that there are double bonds.
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EDIT: seriously if anyone knows what I am confusing, please let me know... CONFUS.
« Last Edit: April 23, 2011, 02:28:49 pm by burbs »
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vexx

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Re: Benzene
« Reply #9 on: April 23, 2011, 02:38:53 pm »
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Quote from: burbs on April 23, 2011, 02:16:02 pm
Right yeah, delocalised electrons. I still think I've read in quite a few places that there are double bonds.
*waits for Mao*


EDIT: seriously if anyone knows what I am confusing, please let me know... CONFUS.

it's a ring of delocalised electrons, where the bonds are basically all equal in length with them being somewhere between a single and double bond.. so the benzene ring shares the double bonds.
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Andiio

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Re: Benzene
« Reply #10 on: April 23, 2011, 02:52:44 pm »
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I thought it was alternating double bonds as well. :\
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Re: Benzene
« Reply #11 on: April 23, 2011, 02:56:14 pm »
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This is resonance as someone mentioned above. It is where the theoretical molecule isn't the same as what we observe. To explain this discrepancy we say that the electron pairs are able to jump around between adjacent atoms to form partial double bonds.
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burbs

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Re: Benzene
« Reply #12 on: April 23, 2011, 04:52:07 pm »
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Oh right, thanks man. Was confusing me.
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Re: Benzene
« Reply #13 on: April 23, 2011, 07:46:16 pm »
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Quote from: burbs on April 23, 2011, 04:52:07 pm
Oh right, thanks man. Was confusing me.
This website is fantastic for all things chem: http://www.chemguide.co.uk/
Here is their page on benzene, with lots of extra detail. Only if you're interested in learning a bit more... http://www.chemguide.co.uk/basicorg/bonding/benzene1.html
Yes - resonance is electron sharing where you find the 'real' structure / observed structure is a combination of two 'drawn' structures.
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Re: Benzene
« Reply #14 on: April 26, 2011, 07:15:09 pm »
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Quote from: Graphite on April 23, 2011, 02:56:14 pm
This is resonance as someone mentioned above. It is where the theoretical molecule isn't the same as what we observe. To explain this discrepancy we say that the electron pairs are able to jump around between adjacent atoms to form partial double bonds.

I don't agree with this. Electrons aren't confined to 'bonds'. Classical models only allow single and double bonds. The only way to explain the structure of benzene using classical models is that the bonds are alternating.

In more advanced theory (ones that treat electrons with quantum mechanics), you have delocalisation.
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