Question

the c₂h₂cl₂ molecule can exist in either of the following two forms: part 1 of 2 what is the hybridization of c in the molecule? part 2 of 2 which structure has a dipole moment?

Explanation:

Step1: Determine hybridization of C

Each C atom in $C_2H_2Cl_2$ has a double - bond and two single - bonds. The number of electron - groups around each C is 3 (2 single - bonds and 1 double - bond). According to the VSEPR theory and hybridization rules, when the number of electron - groups is 3, the hybridization is $sp^2$.

Step2: Analyze dipole moment

In the first structure (cis - isomer), the bond dipoles of the C - Cl bonds do not cancel out due to the non - symmetric arrangement of the Cl atoms around the double bond. In the second structure (trans - isomer), the bond dipoles of the C - Cl bonds are equal in magnitude but opposite in direction and cancel each other out. So, the cis - isomer has a dipole moment.

Answer:

Part 1 of 2: $sp^2$
Part 2 of 2: The first (cis - isomer) structure