Alright, i have a project due tomorrow, and i need your help..
Aluminum Chloride (AlCl3)
I'm trying to make this into a Lewis Structure, but I'm not sure if im right or not..this is what i have so far..
. . . .
: CL = Al - CL:
| . .
. .
: CL:
. .
So im saying that Cl in the left, has a double bond, while the rest of the Cl have single bonds..
Cl has 7 electrons around it and Al has 3 electrons
Hope you can bare with me, i'm so confused, and hope you guys can help me out..
2007-11-13 13:16:51 · 2 answers · asked by Oliver B 2 in Science & Mathematics ➔ Chemistry
Al is one of those elements that does not follow the Lewis rules. The only thing you can do is draw Al with x on three sides. These are Al valence electrons. Next, put Cl next to each x. Put * between each Cl and the Al. Draw six more *'s on the remaining three sides of the Cl's. These are valence electrons of Cl. That gives Al a sextet. Too bad, Dr. Lewis!
2007-11-13 13:23:42 · answer #1 · answered by steve_geo1 7 · 0⤊ 0⤋
each Cl is bonded to the aluminum with a single bond and poor aluminum is stuck without an octet. by double bonding the chlorine you have a very bad formal charge (i don't know if you have learned that but it does) its better to leave it with all single bonds.
2007-11-13 21:23:02 · answer #2 · answered by Rando B 2 · 0⤊ 0⤋