- #36
hariharan venkatasu
- 66
- 3
Thanks for the excellent answer
https://en.m.wikipedia.org/wiki/18-electron_rulehariharan venkatasu said:In post number 35 it has been mentioned that"It has 4 electrons in its outer shell and it would like an additional two pair"How come this is so when it has only two electrons?Please clarify this.I am sorry for a late communication
The 18-electron rule is a general rule of thumb like the Octet rule for predicting stability in transition metal complexes. In the case of zinc chloride, you get 10 electrons from the ##Zn^{2+}## and 2 electrons each from the chlorides, giving 14 electrons. Thus this compound is electron deficient, and can accept four more electrons (or 2 pairs) to satisfy the 18-electron rule. This is the broad reason why zinc chloride is a good Lewis acid.hariharan venkatasu said:Thank you for your information about the wikipedia article.However I don't find any clarification for my question.Could you please elaborate on this?
hariharan venkatasu said:Normally I used to see your reply quickly and promptly. There is an unusual delay in your replying.Could you kindly expedite your reply for post 41?Thanking you.
hariharan venkatasu said:Could you please reply to my post 41?I am eagerly waiting for the answers for my queries.Thanking you.
What do you mean "left" zinc chloride molecule? Chloride do act as a ligand.hariharan venkatasu said:These chlorides are the ones that left zinc chloride molecule
--Do they act as ligands and form coordinate bond?
That kind of way of writing electron configuration are the ones you see in introductory high school textbooks (at least over here in Japan), but they are not very good in explaining the actual electronic configuration.--The configuration of zinc is 2,8,18,2.Does it mean zinc will have one more 18 electron?
--What will be the ultimate configuration of zinc chloride after accepting the extra electrons?
Could you please answer these also?