The Forces Within

The bond between Fluorine and Carbon is Slightly Covalent. This is determined by use of an electro-negativity chart. Carbon has an electro-negativity of 2.5, while Fluorine has that of 4.0. The difference between these atoms is used to determine the bond. If the number is below 1.7, the bond is covalent. If it is above 1.7, the bond is ionic. Since the difference is 1.5, which is a number very close to 1.7, the bond is Slightly Covalent. The image below is a model of the C2F4 molecule. 


The blue represents Carbon
The green represents Fluorine 

hand-drawn and edited by Jessica Woodbine

This is a model of the molecule C2F4 (Teflon). It is a non-polar molecule, because the charges are distributed evenly and there is 2 or more lines of symmetry. The arrow shows that the electro-negativity of Carbon is less than that of Fluorine and is therefore more positive. The shape of this molecule is linear -- there is no central atom. Between the bonds is a 120 degree angle. 

In order to bond with another molecule, C2F4 would experience one or two kinds of forces. In the instance of bonding with H2O, C2F4 would experience London Dispersion Forces and Hydrogen bonding. 

London dispersion forces are the weak attraction that every molecule experiences. They occur when electrons in two adjacent molecules move into positions that make temporary or partial dipoles. 

Hydrogen bonding occurs when a Hydrogen comes into contact with an oxygen, nitrogen or fluorine. In this case, the hydrogen from the water molecule bonds to the fluorine in the Teflon molecule.