November 24, 2024, 02:59:50 AM
Forum Rules: Read This Before Posting


« previous next »
Pages: [1]   Go Down

Topic: Deactivator strength?  (Read 2234 times)

0 Members and 2 Guests are viewing this topic.

Offline aspiringphysician

  • Regular Member
  • ***
  • Posts: 33
  • Mole Snacks: +0/-0
  • ♥ sweet as C12H22O11 ♥
Deactivator strength?
« on: September 05, 2013, 01:50:13 PM »
Why is a carboxylic acid a stronger deactivator (i.e. more electron-withdrawing) than an ester?
Logged
"Now, before you get all 'high-and-mighty', remember that some PLANTS have more complex genomes than YOU!" ~ Dr. Linn

Offline Archer

  • Chemist
  • Sr. Member
  • *
  • Posts: 1001
  • Mole Snacks: +85/-20
  • Gender: Male
Re: Deactivator strength?
« Reply #1 on: September 05, 2013, 03:15:29 PM »
Quote from: aspiringphysician on September 05, 2013, 01:50:13 PM
Why is a carboxylic acid a stronger deactivator (i.e. more electron-withdrawing) than an ester?

Can you explain to us why either acids or esters are deactivators first of all?

I.e. what mechanism makes them deactivate an aromatic ring.
Logged
“ I love him. He's hops. He's barley. He's protein. He's a meal. ”

Denis Leary.
Pages: [1]   Go Up
« previous next »
Sponsored Links