Answer
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Hint: The bond dipole moment uses the idea of an electric dipole moment to measure the polarity of a chemical bond within a molecule. It occurs whenever there is a separation of positive and negative charges. The bond dipole μ is given by: ${ \mu =\delta d }$
Complete step by step solution:
As there are two Cl groups present in ortho makes an acute angle according to the equation;
Dipole moment, D = $ \sqrt { { d }_{ 1 }^{ 2 }{ +d }_{ 2 }^{ 2 }{ +d }_{ 1 }{ d }_{ 2 }{ cosx } }$
where, x = angle between the groups
A.
Here, the dipole moment is ${ 0 }$ as ${ Cos90 }^{ \circ }$ = ${ 0 }$.
B.
The dipole moment of ${ 1,2-dichlorobenzene }$ is ${ 2.54D }$,so
C.
The dipole moment of ${ 1,3-dichlorobenzene }$ is ${ 1.72D }$.
D.
Here, there will be some dipole moment, not zero.
The order of dipole moment is: ${ 1,2-dichlorobenzene }$ ${ 1,3-dichlorobenzene }$ ${ 1,4-dichlorobenzene }$.
Trans-dichlorobenzene has zero dipole moment as it is symmetrical and the dipole moment will cancel out.
Hence, the correct option is A.
> Factors affecting dipole moment:
1) Polarity of molecule
2) Magnitude of charge
3) Geometry of molecule
4) The boiling point of the element.
5) Position of bond and lone pair of electrons in a molecule.
6) The dipole moment depends upon the bond length.
Note: The possibility to make a mistake is that you may choose option C. But in ${ 1,3-dichlorobenzene }$ they are not parallel and hence they will not cancel out completely, it has some dipole moment.
Complete step by step solution:
As there are two Cl groups present in ortho makes an acute angle according to the equation;
Dipole moment, D = $ \sqrt { { d }_{ 1 }^{ 2 }{ +d }_{ 2 }^{ 2 }{ +d }_{ 1 }{ d }_{ 2 }{ cosx } }$
where, x = angle between the groups
A.
Here, the dipole moment is ${ 0 }$ as ${ Cos90 }^{ \circ }$ = ${ 0 }$.
B.
The dipole moment of ${ 1,2-dichlorobenzene }$ is ${ 2.54D }$,so
C.
The dipole moment of ${ 1,3-dichlorobenzene }$ is ${ 1.72D }$.
D.
Here, there will be some dipole moment, not zero.
The order of dipole moment is: ${ 1,2-dichlorobenzene }$ ${ 1,3-dichlorobenzene }$ ${ 1,4-dichlorobenzene }$.
Trans-dichlorobenzene has zero dipole moment as it is symmetrical and the dipole moment will cancel out.
Hence, the correct option is A.
> Factors affecting dipole moment:
1) Polarity of molecule
2) Magnitude of charge
3) Geometry of molecule
4) The boiling point of the element.
5) Position of bond and lone pair of electrons in a molecule.
6) The dipole moment depends upon the bond length.
Note: The possibility to make a mistake is that you may choose option C. But in ${ 1,3-dichlorobenzene }$ they are not parallel and hence they will not cancel out completely, it has some dipole moment.
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