The order of electronegativity for halogens is
A.F > Cl > Br > I
B.I > Br > Cl > F
C.I > Cl > Br > F
D.Cl > F > Br > I

Hint- We know that the Electronegativity decreases down the group as the size of the atom increases when moving from top to bottom.

Complete step by step answer:
We must remember that the fluorine (F) has the highest electronegativity among all the given elements. As mentioned that higher the electronegativity value an element attains, the more strongly that element attracts the shared electrons around them. Hence, option A is correct.
The tendency of an atom to attract a bonding pair of electrons towards it is known as electronegativity. The Pauling scale (a scientific driven scale) is the most commonly used to measure electronegativity. F (the most electronegative element) carries a value of 4.0 in the Pauling scale and values range down to Cs and Fr which are the lowest electronegative at 0.7 on the scale.
As we know that going down the group electronegativity decreases because the atomic number of atoms increases down the group and thus there is an increase in the distance between these valence electrons and nucleus of atoms and there is a greater atomic radius between these atoms.

Note: We can also know that there are also some important exceptions of the above rules which include lanthanides, actinides and noble gases. If in a table the atoms are equally electronegative, then both have the same tendency to attract the bonding pair of electrons around them. We can find this type of bond in $H_2$ or $Cl_2$ molecules.