Which of the following substances has the low | vedclass

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(B) The dipole moment of a molecule depends on its symmetry and the polarity of its bonds.$A$. $cis-but-2-ene$ has a non-zero dipole moment due to its

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$CH_3-C \equiv C-CH_3$

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(B) The dipole moment of a molecule depends on its symmetry and the polarity of its bonds.$A$. $cis-but-2-ene$ has a non-zero dipole moment due to its $cis$ configuration.$B$. $but-2-yne$ $(CH_3-C \equiv C-CH_3)$ is a linear,symmetric molecule where the bond dipoles cancel each other out,resulting in a net dipole moment of $0 \ D$.$C$. $but-1-yne$ $(CH_3CH_2C \equiv CH)$ has a terminal alkyne group,which possesses a small dipole moment.$D$. $but-1-en-3-yne$ $(CH_2=CH-C \equiv CH)$ has both double and triple bonds,creating a polar structure with a significant dipole moment.Therefore,$but-2-yne$ has the lowest dipole moment.

Which of the following substances has the lowest dipole moment?

Similar Questions

Which of the following molecules is polar?

What is the unit of dipole moment? Also,write the formula for dipole moment.

Consider the following:
Assertion $(A)$: Dipole moment of $NF_3$ is lesser than $NH_3$.
Reason $(R)$: In $NF_3$,the orbital dipole due to lone pair of electrons is in the opposite direction to the resultant dipole moment of the three $N-F$ bonds.
The correct answer is:

Both $BF_3$ and $NH_3$ are covalent molecules. However,$BF_3$ is non-polar while $NH_3$ is polar. What is the reason for this?

Which one is a polar molecule?

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