Question

Out of
$C{{H}_{2}}C{{l}_{2}},C{{H}_{4}},CC{{l}_{4}},{{H}_{2}}O,CHC{{l}_{3}},p-dichlorobenzene,o-cresol,p-xylene,SC{{l}_{2}},B{{F}_{3}},IBr\ and\ \text{C}{{\text{H}}_{\text{2}}}\text{O}$, non-zero value of dipole moment are:

Answer 1

Hint: A dipole moment can be shown in those compounds in which separation of charges can be seen. Therefore we can say that dipole moment arises in ionic bonds as well as in covalent bonds. Dipole moments also occur due to the difference in electronegativity between two chemically bonded atoms.

Complete answer:
A bond dipole moment generally measures the polarity of a chemical bond between two atoms in a molecule. It gives us the concept of electric dipole moment which is generally used to measure the separation of negative and positive charges in a system.
Dipole moment also depends upon the structural properties of any compound or we can say on its bond angle. For symmetrical structures bond angle will be zero while for unsymmetrical structures it shows some value.
Out of this compounds$C{{H}_{2}}C{{l}_{2}}$,${{H}_{2}}O$,$CHC{{l}_{3}}$,$o-cresol$,$SC{{l}_{2}}$,$IBr\ and\ \text{C}{{\text{H}}_{\text{2}}}\text{O}$have non-zero dipole moments this can be explained on the basis that the individual bonds are not able to cancel each other. Therefore, the net dipole moment is non zero. Whereas the compounds $C{{H}_{4}},CC{{l}_{4}}$, $p-dichlorobenzene$, $p-xylene$and $B{{F}_{3}}$have zero dipole moments as their individual moment cancel each other effect.
Thus we can say that 7 compounds$C{{H}_{2}}C{{l}_{2}}$,${{H}_{2}}O$,$CHC{{l}_{3}}$,$o-cresol$,$SC{{l}_{2}}$,$IBr\ and\ \text{C}{{\text{H}}_{\text{2}}}\text{O}$have non-zero dipole moments.

Note:
Dipole moment is a vector quantity i.e. it has both magnitude as well as direction. Due to the property of a vector quantity it can also be zero as two oppositely charged bond dipoles can cancel each other.