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Chemistry Forums for Students => Inorganic Chemistry Forum => Topic started by: Altered State on December 02, 2012, 04:46:02 PM

Title: Aluminium Chloride as lewis acid
Post by: Altered State 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
Title: Re: Aluminium Chloride as lewis acid
Post by: 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]-
Title: Re: Aluminium Chloride as lewis acid
Post by: Altered State 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