/sci/ - Science & Math » Thread #12578567

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WHY THE FUCK HOW?

Anonymous Wed 13 Jan 23:28:35 2021 No.12578567 View Reply Original Report

Quoted By: >>12578572 >>12578578 >>12578586 >>12578688 >>12578832

How the fuck does the whole fucking triple connection breaks just to reconnect a single connection afterwards between the two Carbon molecules?

WHY NOT BREAK ONLY TWO AND CONNECT TO THE OTHERS AFTER? Someone has a sane explanation for this?

Anonymous

Anonymous Wed 13 Jan 2021 23:29:30 No.12578572 Report

Quoted By:

>>12578567
Molecules be cray

Anonymous

Anonymous Wed 13 Jan 2021 23:30:06 No.12578578 Report

Quoted By: >>12578589

>>12578567
Triple bonds are unstable
They’re like electron clouds prime to fuck some proton pussy

Anonymous

Anonymous Wed 13 Jan 2021 23:32:28 No.12578586 Report

Quoted By: >>12578598

>>12578567
Has to do with the shape of the orbitals on the carbon with the triple bond. Introducing energy is like putting a ball (bond) on a slope, it's going to travel downhill.

Anonymous

Anonymous Wed 13 Jan 2021 23:32:47 No.12578589 Report

Quoted By: >>12578636

>>12578578
yea but then the double bonds acts the same FUCKING WAY BRO. THEY WILL BREAK WHOLE JUST TO RECONNECT SINGLE AFTERWARDS?

ANYONE HAS SANE FUCKING EXPLANATION FOR THIS SHIT? NO FUCKING WAY NATURE ACTUALLY ACTS THIS WAY? YOU'VE ALL BEEN FUCKING LIED TO. CHEMISTRY FUCKS, WHAT DO YOU HAVE TO SAY????????????????

Anonymous

Anonymous Wed 13 Jan 2021 23:34:20 No.12578598 Report

Quoted By: >>12578625

>>12578586
what? can you draw a picture or something?

Anonymous

Anonymous Wed 13 Jan 2021 23:38:34 No.12578625 Report

Quoted By: >>12578773

>>12578598
A ball is inclined to travel down a slope and rest in a base because of gravity right? That's a metaphor for the state of the carbon electrons.

The electrons are inclined to be in the position with the least amount of resistance. In the case of the OP equation the position happens to be no triple bond when energy is added, and single bonds in the presence of hydrogen.

Anonymous

Anonymous Wed 13 Jan 2021 23:40:43 No.12578636 Report

Quoted By: >>12578773

>>12578589
Double bonds are pretty stable
You gotta look at the orbitals
Orbitals are like dicks
If the dicks are flopping everywhere they’ll fuck proton pussy
If they’re stuck in their pants then they’ll stay in their pants

Anonymous

View Same Google iqdb SauceNAO Catalytic_Hydrogenation_Mechanism.jpg, 64KiB, 1170x579

Anonymous Wed 13 Jan 2021 23:54:30 No.12578688 Report

Quoted By: >>12578773

>>12578567
For the purposes of that problem, all you care about is the energy associated will bond breaking and forming to calculate some enthalpy of reaction. How it breaks isn't of interest. However, it looks like a catalytic hydrogenation reaction which requires a metal catalyst like Pd to be present. Essentially, the hydrogen breaks and bonds to catalyst metal surface where the molecule is also bound to and then a reaction happens. I attached a picture of a double bond because I couldn't find one for a triple bond but the mechanism is probably similar. Catalysts mechanisms are not generally known in great detail although I think some guy got a Noble prize awhile back for figuring out some metal catalysis stuff.

Anonymous

Anonymous Thu 14 Jan 2021 00:24:41 No.12578773 Report

Quoted By: >>12578802 >>12579062

>>12578625
>>12578636
>>12578688
alright thank you. So it seems that there might be a little more to it than what's written in a highschool chemistry textbook. Seems like how the actually reactions happen is probably not set in stone and there might be some nuance to it depending on the situation. I knew little about catalysts and orbits and those were certainly not part of the explanation in the textbook.

To me it seemed like breaking double, triple or quadruple bonds between two atoms just to reform a smaller bound right after would be a waste of time and nature wouldn't actually allow that, but depending on the orbits and catalysts, I mean, yea maybe.

Anonymous

Anonymous Thu 14 Jan 2021 00:36:37 No.12578802 Report

Quoted By:

>>12578773
>To me it seemed like breaking double, triple or quadruple bonds between two atoms just to reform a smaller bound right after would be a waste of time and nature wouldn't actually allow that
It is thermodynamically favorable to form the bonds but if you don't have catalyst you might never see the reaction happen to a great degree (kinetics). The energy of the triple bond molecule and hydrogen is higher than the products of single bond molecule so it is favorable to occur but you have to "get over the hump" (activation energy) so the reaction occurs.

Anonymous

Anonymous Thu 14 Jan 2021 00:47:01 No.12578832 Report

Quoted By:

>>12578567
Breaking two pi bonds is ENERGY EQUIVALENT to breaking two pi bonds and a sigma bond and then reforming that sigma bond.

Anonymous

Anonymous Thu 14 Jan 2021 01:48:58 No.12579062 Report

Quoted By:

>>12578773
>So it seems that there might be a little more to it than what's written in a highschool chemistry textbook
So it seems like you misunderstand your high school (underage b&) textbook. Enthalpy change only depends on the initial and final states, the path between them does not affect the equilibrium of the reaction. Nobody is making any assumptions about transition states here.

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