November 26, 2024, 11:29:18 AM
Forum Rules: Read This Before Posting


« previous next »
Pages: [1]   Go Down

Topic: Aluminium Chloride as lewis acid  (Read 3435 times)

0 Members and 2 Guests are viewing this topic.

Offline Altered State

  • Full Member
  • ****
  • Posts: 270
  • Mole Snacks: +24/-4
  • Gender: Male
    • Chemistry Hall
Aluminium Chloride as lewis acid
« on: December 02, 2012, 04:46:02 PM »
I'm looking for any good explanation about why are Aluminium Chloride and other compounds like it that don't seem so, good lewis acids.
I'm studying Chemistry at University, but I don't have Inorganic Chemistry yet this year.

Greetings
Logged

Offline Hunter2

  • Sr. Member
  • *****
  • Posts: 2296
  • Mole Snacks: +189/-50
  • Gender: Male
  • Vena Lausa moris pax drux bis totis
Re: Aluminium Chloride as lewis acid
« Reply #1 on: December 03, 2012, 01:32:14 AM »
AlCl3 can assoziate with other atomes of free electon pair. It has a lack of electrons.

AlCl3 + Cl- => [AlCl4]-
Logged

Offline Altered State

  • Full Member
  • ****
  • Posts: 270
  • Mole Snacks: +24/-4
  • Gender: Male
    • Chemistry Hall
Re: Aluminium Chloride as lewis acid
« Reply #2 on: December 03, 2012, 11:12:41 AM »
Quote from: Hunter2 on December 03, 2012, 01:32:14 AM
AlCl3 can assoziate with other atomes of free electon pair. It has a lack of electrons.

AlCl3 + Cl- => [AlCl4]-

Is that a coordination complex reaction?


I saw this in other page:

AlCl3 ----> (water) --> Al3+ 3Cl-

Al3+ + 6H2O ---->  Al(H2O)63+

Al(H2O)63+ + H2O ----> Al(OH-)(H2O)52+ + H3O+

Is that the same? Is it not? Is it corret aswell?


Thanks
Logged
Pages: [1]   Go Up
« previous next »
Sponsored Links