Test 3 Question 2

Moderators: Chem_Mod, Chem_Admin

Adela Henry 1I
Posts: 30
Joined: Fri Apr 06, 2018 11:03 am
Been upvoted: 1 time

Test 3 Question 2

Postby Adela Henry 1I » Tue Jun 05, 2018 8:07 pm

Hi, for question 2 I had to find the most stable lewis structure for TiCl4. I thought I had did it right because of the formal charges but it was wrong. Could someone please explain the answer?
Thanks

kimberlysanchez-1E
Posts: 30
Joined: Tue Nov 14, 2017 3:01 am

Re: Test 3 Question 2

Postby kimberlysanchez-1E » Tue Jun 05, 2018 8:10 pm

What do you mean? How did your structure look?

Andre-1H
Posts: 39
Joined: Fri Apr 06, 2018 11:01 am

Re: Test 3 Question 2

Postby Andre-1H » Tue Jun 05, 2018 8:15 pm

The answer is titanium connected to 4 chlorines by a single bond. The question tells you that the molecule must be neutral (sum of formal charges is 0), which means that it is highly likely that all chlorine atoms have 3 lone pairs and one bond. 4 chlorines with 7 valence electrons and 1 titanium with 4 valence electrons give you a structure that looks like this https://www.mjlphd.net/blog/on-the-use- ... rachloride except with lone pairs around the chlorine. Let me know if you need anything else

Adela Henry 1I
Posts: 30
Joined: Fri Apr 06, 2018 11:03 am
Been upvoted: 1 time

Re: Test 3 Question 2

Postby Adela Henry 1I » Tue Jun 05, 2018 8:17 pm

This is what I did.
#2.jpg

Jennifer 1G
Posts: 29
Joined: Wed Nov 15, 2017 3:03 am

Re: Test 3 Question 2

Postby Jennifer 1G » Tue Jun 05, 2018 8:18 pm

I got full credit on this question by using single bonds, so Ti has 8 electrons and each Chlorine has an octet!
I just saw the picture posted. Ti should be in the center I believe.

Adela Henry 1I
Posts: 30
Joined: Fri Apr 06, 2018 11:03 am
Been upvoted: 1 time

Re: Test 3 Question 2

Postby Adela Henry 1I » Tue Jun 05, 2018 8:20 pm

Oh, I see. Thank you guys for your help!


Return to “Lewis Structures”

Who is online

Users browsing this forum: No registered users and 1 guest