12.15

Moderators: Chem_Mod, Chem_Admin

Payton Schwesinger 1J
Posts: 45
Joined: Fri Sep 29, 2017 7:04 am

12.15

Postby Payton Schwesinger 1J » Tue Dec 05, 2017 1:39 pm

When drawing the product of the reaction between PF5 and F-, how do you know that the resulting compound, PF6, has a negative charge?

Swetha Sundaram 1E
Posts: 59
Joined: Fri Sep 29, 2017 7:04 am
Been upvoted: 1 time

Re: 12.15

Postby Swetha Sundaram 1E » Tue Dec 05, 2017 2:03 pm

Well PF5 has a neutral charge and by adding the F- ion, it results in the overall compound having a negative charge.

Tasnia Haider 1E
Posts: 55
Joined: Sat Jul 22, 2017 3:01 am

Re: 12.15

Postby Tasnia Haider 1E » Tue Dec 05, 2017 2:25 pm

You can also count the number of electrons each compound or ion has. PF5 would have 40 electrons and F- would have 8 electrons. If PF6 didn't have a charge it would only have 47 electrons, but the structure should have the same number of electrons as its reactants, so it would need an extra electron, and therefore have a negative charge.

Ramya Lakkaraju 1B
Posts: 67
Joined: Fri Sep 29, 2017 7:03 am

Re: 12.15

Postby Ramya Lakkaraju 1B » Thu Dec 07, 2017 4:24 pm

Look at formal charges, you know that phosphorus likes to make 5 bonds since it has a valence number of 5, however in the case of PF6 it is making 6 bonds, resulting in a -1 charge.


Return to “Lewis Acids & Bases”

Who is online

Users browsing this forum: No registered users and 1 guest