Question 4.29

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Robert Estrada
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Question 4.29

Postby Robert Estrada » Sun Nov 19, 2017 9:40 pm

Can someone explain #29?
The question is: there are three isomers of dicholorobenzene, C6H4Cl2+, which differ in the relative positions of the chlorine atoms on the benzene ring.(A) Which of the three forms are polar? (B) Which has the largest dipole moment?

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Re: Question 4.29

Postby Seth_Evasco1L » Sun Nov 19, 2017 9:45 pm

Symmetry is a large factor in deciding which molecules are polar or non-polar. If I remember correctly, Forms 1 and 2 are polar because the bonded Cl atoms are not opposite of each other on the carbon ring. To decide which is more polar, think of the dipole moments created by the C-Cl bonds as a vector and add them head to tail. I believe Form 1 had the larger dipole moment because the C-Cl dipole moments were headed in nearly the same direction as opposed to the dipole moments in Form 2.

Joyce Lee 1C
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Re: Question 4.29

Postby Joyce Lee 1C » Sun Nov 19, 2017 10:27 pm

The dipole moment for 1 would be largest because the bond vectors for C-Cl are pointing in almost the same direction but in 2 the vectors point in different ways, which cancels out the dipole.

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