July 12, 2020, 08:54:31 PM
Forum Rules: Read This Before Posting


Topic: synthesize acetic acid from alkyl halide  (Read 23566 times)

0 Members and 1 Guest are viewing this topic.

polly

  • Guest
synthesize acetic acid from alkyl halide
« on: March 31, 2004, 05:13:47 PM »
Hi!  How do you synthesize acetic acid starting with any alkyl halide and acetylene.  Would it just be KMnO4/H3O+ ??  Also, when synthesizing a (well I can't name this structure so I will do my best to describe it- it is trans with 2 benzene groups attached by a 2 propene in the middle)- hope that makes sense.  The question is how do you snthesize this using any alkyl halide and acetylene?  Can you use NaH2,NH3 twice as 2 separate steps and from there use Li/NH3??

Thanks!



Edit: edited title for better indexing. Mitch
« Last Edit: April 24, 2004, 06:52:52 PM by Mitch »

GCT

  • Guest
Re:synthesis
« Reply #1 on: April 01, 2004, 02:43:00 PM »
React the acetylene with NaNH2 (or Na) to produce an acetylide anion, alkylate using an methyl halide (chloride), then oxidize completely.

I'm not quite sure what you're referring to in your second question.  Perhaps end substituded propene by two benzenes...if so I have an idea what you'll need.

polly

  • Guest
Re:synthesis
« Reply #2 on: April 01, 2004, 08:31:42 PM »
Thanks for your input.  I will try and explain the second material better.  There is a double bond in the middle.  Coming off both sides of the double bond in a trans manner is an ethyl benzene on each side.  The ethyl part is atached to the double bond.  My question is can you form this by using acetylene and then adding an ethyl benzene with NaNH2,NH3, THF on two separate occasions and then use Li/NH3 to cut the tripple bond to double and form a trans product??  If not, how would you make it?  I hope that is more clear.  I wish I could draw it and show you but I have no idea how to do that on the computer.

Thanks

polly

  • Guest
Re:synthesis
« Reply #3 on: April 01, 2004, 08:33:35 PM »
PS- I goofed on the first email- I meant 2 butene not propene- Sorry!

Offline Mitch

  • General Chemist
  • Administrator
  • Sr. Member
  • *
  • Posts: 5294
  • Mole Snacks: +376/-2
  • Gender: Male
  • "I bring you peace." -Mr. Burns
    • Chemistry Blog
Re:synthesis
« Reply #4 on: April 01, 2004, 08:49:43 PM »
Can you post a picture? Just use Paint and save it as a JPeg?
Most Common Suggestions I Make on the Forums.
1. Start by writing a balanced chemical equation.
2. Don't confuse thermodynamic stability with chemical reactivity.
3. Forum Supports LaTex

polly

  • Guest
Re:synthesis
« Reply #5 on: April 01, 2004, 09:02:36 PM »
I hope this works...

polly

  • Guest
Re:synthesis
« Reply #6 on: April 01, 2004, 09:09:55 PM »
When reacting acetylene with NaNH2/CH2Cl, then oxidize to make acetic acid (CH3CO2), would you end up with too many carbons?
« Last Edit: April 01, 2004, 09:13:30 PM by polly »

Offline Mitch

  • General Chemist
  • Administrator
  • Sr. Member
  • *
  • Posts: 5294
  • Mole Snacks: +376/-2
  • Gender: Male
  • "I bring you peace." -Mr. Burns
    • Chemistry Blog
Re:synthesis
« Reply #7 on: April 01, 2004, 09:20:41 PM »
I don't suppose you have learned the Wettig reaction yet? Is there anything in particular that you have to start with?
Most Common Suggestions I Make on the Forums.
1. Start by writing a balanced chemical equation.
2. Don't confuse thermodynamic stability with chemical reactivity.
3. Forum Supports LaTex

polly

  • Guest
Re:synthesis
« Reply #8 on: April 01, 2004, 09:53:36 PM »
No, I have not learned the wettig reaction yet, but would love to learn it.  I need to start both reactions with any alkyl halide (if needed) and acetylene.

haiph12

  • Guest
Re:synthesis
« Reply #9 on: April 02, 2004, 10:04:27 AM »
You can do :
CH3Cl + Mg  --  CH3MgCl (grinhar)
acetylene + 2CH3MgCl --  ClMg-CC-MgCl + 2CH4
 ClMg-CC-MgCl  + H2  ---  ClMg-CH=CH-MgCl (cat: Pd)
2C6H5CH2Cl  +  ClMg-CH=CH-MgCl   --- The (cis- product) + by product
 ::)
 ;D
« Last Edit: April 02, 2004, 10:26:28 AM by haiph12 »

haiph12

  • Guest
Re:synthesis
« Reply #10 on: April 02, 2004, 10:20:15 AM »
CH3Cl + Mg  --  CH3MgCl (grinhar)
acetylene + 2CH3MgCl --  ClMg-CC-MgCl + 2CH4

2C6H5CH2Cl + ClMg-CC-MgCl  --- C6H5CH2-CC-CH2C6H5(A) + MgCl2
A + NaNH2(NH3) ---  trans(the desire product)
 :o

haiph12

  • Guest
Re:synthesis
« Reply #11 on: April 02, 2004, 10:33:58 AM »
Can you understand the grinhar compound?
CH3Cl  + Mg ---  CH3MgCl ( in ete)
RMgCl + HA --  RH  +  AMgCl
RMgCl  + R'Cl ---  RR'  +  MgCl2 :'( :-*
 ;D ;D ;D

haiph12

  • Guest
Re:synthesis
« Reply #12 on: April 02, 2004, 10:43:21 AM »
Can You search the name reaction on:

http://www.monomerchem.com/display4.html
hi hi:
Are you a student or pupil

GCT

  • Guest
Re:synthesis
« Reply #13 on: April 02, 2004, 11:14:59 AM »
Yes you would also end up with the oxidized methyl group...to the acid.  You can separate this from the acetic acid though.

Reactions are usually very specific and even if alternatives were to work there is usually only few reactions which are realistically plausible given the product one desires.  This is why I doubt that the wittig reaction would be a good choice (more input later).

Also


Quote
CH3Cl + Mg  --  CH3MgCl (grinhar)
acetylene + 2CH3MgCl --  ClMg-CC-MgCl + 2CH4
ClMg-CC-MgCl  + H2  ---  ClMg-CH=CH-MgCl (cat: Pd)
2C6H5CH2Cl  +  ClMg-CH=CH-MgCl  --- The (cis- product) + by product

This simply will not work, there are many flaws.  First of all, the hydrogens of acetylene are acidic, the reaction is too costly and too long, some of the products are incorrect.

I hope I did not sound condenscending.

I'll reply to Polly's question on the next post.

GCT

  • Guest
Re:synthesis
« Reply #14 on: April 02, 2004, 11:22:43 AM »
Polly, for your second question, this is what I can think of for now...

Use two equivalents of a toulene halide (Ar-CH3I) and two equivalents of the base NaNH2 as reagents to react with the acetylene.  This will yield an di-anionic acetylene and thus will react with two of the halides to for your desired compound...use a suitable reducing agent to go from reduce to the double bond...depending on which reducing agent you use you can form either the trans or cis products.  If you still need help feel free to ask.

Sponsored Links