Chemical Forums
Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: KAJLogic on October 08, 2013, 09:50:19 PM
-
There are a couple of things I wanted to double check with you find gentleman. So my professor gave me this sheet for find the bonds. So we get to KrF2, so the sheet tells you to just add the d orbital so the valence would be
10+2(8 ) = 26
My first question is why do we now just ignore the s&p orbitals seems like if we are going to need hybridized orbitals s&p are inevitably going to be involved.
My next question is how does fluorine even bond with d sense each orbital has two electrons which should meet its mathematical limit.
so they do this and obviously get 2 bonds and 9 lone pairs.
EDIT:
Just checking back I would also like to say that I am using THIS (http://www.chemicalforums.com/index.php?PHPSESSID=d2ffb3b8eb2d57e98446272218047144&topic=70835.0) still I just thought that the answer for this might not have to do with hybridized orbitals also I am still very much digesting all that information. But anyways, I think I have the answer so what happens is fluorine causes the d orbital to essentially loose two of its electrons and instead bond with fluorine's electrons. Then my question becomes do these electrons go into krypton's 5s orbital?
-
I see it was read 54 times do I have to word it better?