Lewis Structure/Cyclic Molecule:
![Picture](/uploads/4/8/7/7/48775307/1430423516.png)
Paradichlorobenzene is a non-polar molecule because the
chlorines are on opposite sides of each other on the benzene
ring and the four hydrogens are all across from each other.
This is a cyclic molecule so there is no" AX" form.
chlorines are on opposite sides of each other on the benzene
ring and the four hydrogens are all across from each other.
This is a cyclic molecule so there is no" AX" form.
Intermolecular Forces:
![Picture](/uploads/4/8/7/7/48775307/5697398.jpg)
The intermolecular forces that can act on Paradichlorobenzene are Hydrogen-bonding and dispersion. The hydrogen of C6H4Cl2 attracts to the hydrogen of H2S, so hydrogen bonding occurs. Another intermolecular force that acts on Paradichlorobenzene is dispersion. Dispersion acts on any and all adjacent molecules.
Nature of the Bond:
![Picture](/uploads/4/8/7/7/48775307/8294899.jpg?250)
If the bond is less than 1.7 it is covalent but if the bond is greater than 1.7 it is ionic. The nature of the carbon to hydrogen bond in paradichlorobenzene is highly covalent because it is less than 1.7 and it is nowhere close to 1.7. The nature of the carbon to chlorine bond is moderately covalent because it is less than 1.7 but not extremely far from 1.7.