The dipole moment is a vector quantity. In the trans isomer of 2-butene, the dipoles of substituents are equal in magnitude but opposite in direction, resulting in a net dipole moment of zero (\(\mu = 0\)). However, in the cis isomer, the dipoles do not cancel out, making the molecule polar with \(\mu > 0\). Thus, the dipole moment of the cis form is greater than the trans form.
Cis isomer: \(\mu > 0\), Trans isomer: \(\mu = 0\).
Therefore, both the assertion and reason are true, and the reason correctly explains the assertion.
The incorrect statements regarding geometrical isomerism are:
(A) Propene shows geometrical isomerism.
(B) Trans isomer has identical atoms/groups on the opposite sides of the double bond.
(C) Cis-but-2-ene has higher dipole moment than trans-but-2-ene.
(D) 2-methylbut-2-ene shows two geometrical isomers.
(E) Trans-isomer has lower melting point than cis isomer.
Given below are two statements:
Statement (I):
are isomeric compounds.
Statement (II): are functional group isomers.
In the light of the above statements, choose the correct answer from the options given below: