Which of the following molecules has the lowe | vedclass

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(B) The dipole moment depends on molecular symmetry and the polarity of bonds.$1$. $CH_3-C \equiv C-CH_3$ (but$-2-$yne) is a linear and centrosymmetri

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$CH_3-C \equiv C-CH_3$

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(B) The dipole moment depends on molecular symmetry and the polarity of bonds.$1$. $CH_3-C \equiv C-CH_3$ (but$-2-$yne) is a linear and centrosymmetric molecule. Due to its high symmetry, the dipole moments of the $C-CH_3$ bonds cancel each other out, resulting in a net dipole moment of $0 	ext{ D}$.$2$. $CH_3-CH_2-C \equiv CH$ (but$-1-$yne) and $CH_2=CH-C \equiv CH$ (but$-1-$en$-3-$yne) are asymmetric, leading to a non-zero net dipole moment.$3$. $cis-	ext{but-}2	ext{-ene}$ has a non-zero dipole moment due to its polar nature and lack of a center of symmetry.Therefore, $CH_3-C \equiv C-CH_3$ has the lowest dipole moment.

Which of the following molecules has the lowest dipole moment?

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