# What is the molecular shape of C2Cl2?

The molecular shape of the ${C}_{2} C {l}_{2}$ molecule is linear.
Starting with its Lewis structure, the ${C}_{2} C {l}_{2}$ molecule has a total of 22 valence electrons, 4 from each of the two carbon atoms and 7 from each of the two chlorine atoms. Thus, its Lewis structure must account for 22 valence electrons.
So, the two carbon atoms are bonded to the two chlorine atoms through a single bond, and through a triple bond to each other. The triple bond accounts for $\text{3" * "2 = 6}$ electrons, while the two single bonds add $\text{2" * "2 = 4}$ electrons.
The 3 lone pairs around each of the two chloride atoms add up to $\text{2" * "(3" * "2) = 12}$ electrons, which brings the total to the required 22 electrons.
According to VSEPR Theory, the molecular geometry of the molecule will be linear, since each of the two carbon atoms has a coordination number and a steric number equal to 2, with a bond angle of ${\text{180}}^{\circ}$.