Question

Does $ C{F_4} $ have a polar bond?

Answer 1

Hint: In this question, we should first find out the hybridization of a given compound by which we can find the shape of the compound. After that we will check whether the compound contains polar or nonpolar bonds. With the help of electronegativity of the elements in the compound, we can predict the polar or nonpolar nature of the bond.

Complete answer:
To find the polarity of the compound, there are following step needed:
Step-1: First of all we have to find the hybridization of in the compound which is:

Hence the hybridization of carbon atom in $ C{F_4} $ compound is $ s{p^3} $ so the shape of compound $ C{F_4} $ is tetrahedral with four $ C - F $ bonds pointing towards the corners of a tetrahedron as shown in the following figure:

Step-2: Check whether each bond in the structure is polar or nonpolar which depends upon electronegativity difference. If electronegativity difference between the bonds is greater than $ 0.4 $ , then the bond will be polar but if it is less than $ 0.4 $ then it will be nonpolar.
As we know that Fluorine electronegativity is $ 4.0 $ whereas the electronegativity of Carbon is $ 2.5 $ , thus their electronegativity difference is more than $ 0.4 $ , i.e. 1.5 so each $ C - F $ bond is very polar. Hence, the bonds of the given compound are polar then the geometric sketch of the $ C{F_4} $ compound is:

Note:
You can use Lewis structure as an alternative for prediction of polarity of the bond of the compound. Lewis structure is also known as Lewis dot formulas, are the diagrams which show the bonding between atoms of the molecule. It also shows the lone pairs of electrons that exist in the molecule.