Which of the following pairs of molecules wil | vedclass

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(B) molecule has a permanent dipole moment if it is polar,meaning the vector sum of its individual bond dipoles is non-zero.$CO_2$ is a linear molecul

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$NO_2$ and $O_3$

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(B) molecule has a permanent dipole moment if it is polar,meaning the vector sum of its individual bond dipoles is non-zero.$CO_2$ is a linear molecule with a symmetric structure,so its bond dipoles cancel out,resulting in a net dipole moment of $0$.$SiF_4$ has a tetrahedral geometry,which is highly symmetric,leading to a net dipole moment of $0$.$NO_2$ is a bent molecule due to the presence of an unpaired electron on the nitrogen atom,which results in a non-zero net dipole moment.$O_3$ (ozone) is also a bent molecule with a non-zero net dipole moment due to its angular structure.Therefore,the pair $NO_2$ and $O_3$ both possess a permanent dipole moment.

Which of the following pairs of molecules will have a permanent dipole moment?

Similar Questions

Which of the following does not possess a permanent 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:

Arrange the following compounds in increasing order of dipole moment:
$CH_3CH_2CH_3$,$CH_3CH_2NH_2$,$CH_3CH_2OH$

If an $AB_3$ molecule (containing four atoms) has a dipole moment of zero and another has a non-zero dipole moment,what does this indicate about their shapes?

Which molecule has both non-polar and polar bonds,but the molecule as a whole is polar?

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