Step 1: Find valence e- for all atoms. Add them together.

Xe:8
F:7x2=14

Total=22

Step2: Find octet e- for each atom and add them together.

Xe:10*
F:8x2=16

*Xe should get 10 electrons for its octet so that it can form 2 bonds with side atoms.

Total=26

Step3: Gives you bonding e-. Subtract step 1 total from step 2

26-22=4e-

Step 4: Find number of bonds by diving the number in step 3 by 2(because each bond is made of 2 e-)

4e-/2= 2 bond pairs

Step 5: Find the number of nonbonding (lone pairs) e-. Subtract step 3 number from step 1.

22-4= 18e-=9 lone pairs

Use information from step 4 and 5 to draw the lewis structure.

Lewis dot structure of Xef₂

Alternatively a dot method can be used to draw the lewis structure.
Calculate the total valence electrons in the molecule.
Xe:8
F:7x2=14

Total=22

Put Xenon in center and arrange chlorine atoms on the sides.Arrange electrons until fluorine atoms get 8 electrons.( Xenon gets 10 electrons, which is an expanded octet)