Step 1: Find valence e- in all atoms. Add them together.
C:4
H:2x1=2
F=2x7=14
Total=20

Step2: Find octet e- for each atom and add them together.
C:8
H:2x2=4
F=2x8=16
Total=28

Step3: Subtract step 1 total from step 2.This step gives you number of bonding e-.
28-20=8e-

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

8e-/2= 4 bond pairs.

Step 5: Find the number of nonbonding (lone pairs) e-. Subtract step 3 number from step 1.
20-8= 12e-=6 lone pairs
Use information from step 4 and 5 to draw the lewis structure.
Put atom(s) with lowest electro negativity in the center. Arrange the remaining atoms around it. Finally put the bond pairs and lone pairs of electrons on the atoms.

Molecular shape of CH₂Cl₂

According to VSEPR notation the number of central atomsA=1,number of surrounding atomsX=4,number of lone pairs on central atom E=0
For VSEPR Notation AX₄ molecular shape is tetrahedral.

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