One example of a hydroflurocarbon in CH2f2 (subscript two's). The C-F bond is polar.?

Where would I mark the partial charges (δ- and δ+) on the C and F atoms of a structure like this: http://img241.imageshack.us/img241/1791/...

One example of a hydroflurocarbon in CH2f2 (subscript two's). The C-F bond is polar.?
Yes, it is polar.


The electronegativity of F is highest (4 on Pauling scale) in whole periodic table.(electronegativity is the power of attracting electrons through a bond). When C combines with F in a covalent bond as the electronegativity of F is higher than C, it attracts electron more than C through a bond. hence the bond gets slightly ionic properties(53%). and obiviously polar properties.


Hence you should give delta- charge to F and delta+ to C.


Thank You!
Reply:partial positive on C








partial negative on F (fluorine is highly electronegative)





C-F bond polar!
Reply:Lancenigo di Villorba (TV), Italy





Yes, it is.


The chemical compound you described is CH2F2 or


DI-FLUORO-METHANE or METHYLEN-FLUORIDE.


Inside the molecule, you distinguish several chemical bonds as Covalent Polar Ones, e.g. C-F's ones.


If you refer to Pauling's Electronegativities, the great Value's Differences existing between Carbon and Fluorine get reason to this conclusion : "Delta+" interests Carbon Atom whilst "Delta-" stands on Fluorine Atoms because the latter ones have the greatest Pauling's Values.





I hope this helps you.
Reply:if the difference of the electronegativities is greater than 0.4 and less than 2.0 then it falls under polar. F-C=4.0-2.55==1.45, so it is polar


non-polar=0%26lt;0.4


ion= %26gt;2.00