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what is the covalent bond for Nitogen and Fluride

WHAT IS THE Covalent bond for nitrogen and flouride with the work with 

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Stanton D. | Tutor to Pique Your Sciences InterestTutor to Pique Your Sciences Interest
4.6 4.6 (42 lesson ratings) (42)
N and F can (reluctantly) form the molecule NF3. All bonds are single polar covalent.
Surprisingly, it is not a very reactive molecule, though it has specific uses in semiconductor etching. It's also a potent greenhouse-effect gas.
An analog is NCl3, formed by reaction of excess bleach with a little ammonia. (This reaction proceeds vigorously! NCl3 is a nerve gas; also likely to make lower-chlorinated amount amines, very odorous, very toxic.)
Really, tutors, you can Google molecules to check them out, before declaring them DOA ...
Dick B. | Math and Science TutorMath and Science Tutor
4.9 4.9 (72 lesson ratings) (72)

Can you clarify the question?


Sorry.  I should have put this in the comments.

Patrick S. | Pre-Medical Student Loves to Help People Achieve Their GoalsPre-Medical Student Loves to Help People...

I am guessing that this is a Lewis Structure question... There will be a double bond between N and F. One of F's valence electrons is "donated" to N, (I think the convention is to draw an "X" through the F  electron and an arrow leading to the position of N to which it was moved) then you are able to represent the second bond.

As Dick B. commented, the formation of an NF molecule is highly unlikely due to the electronegativity of Fluorine. So, this structure is strictly hypothetical.


I suppose you could create a Lewis structure for a hypothetical NF molecule, but that's about as likely (probably less so) as an O8 molecule.

 Fluorine is too electronegative to donate any electrons to anything.  If you could somehow make an NF species, it would likely be a radical, and would combine with the next thing it sees.  Just as likely, it would break apart, and reform the elements N2 and F2.

I suppose that I should have used another term rather than "donate."  I was just attempting to provide the answer for what I believed to be the question that was being asked. I am assuming that the person asking the question had these two elements' hypothetical molecule as part of a Lewis Structure assignment. That being said, I agree with your comment. 

I do not understand why textbooks/instructors would ask such a question. On the other hand, they probably just wanted to provide a scenario wherein the student must manipulate the valence electrons as they are in the hypothetical NF molecule.