If $B-Cl$ bond has a dipole moment, explain why $BCl_3$, molecule has zero dipole moment.
If $B-Cl$ bond has a dipole moment, explain why $BCl_3$, molecule has zero dipole moment.
As a result of the difference in the electronegativities of $\mathrm{B}$ and $\mathrm{Cl}$, the $\mathrm{B}-\mathrm{Cl}$ bond is polar in nature.
However, the $\mathrm{BCl}_{3}$ molecule is non-polar. This is because $\mathrm{BCl}_{3}$ is trigonal planar in shape. It is a symmetrical molecule.
Hence, the respective dipole-moments of the $\mathrm{B}-\mathrm{Cl}$ bond cancel each other, there by causing a zero-dipole moment.
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- [JEE MAIN 2019]
Which reaction involves a change in the electron pair geometry for the underlined element ?
Which reaction involves a change in the electron pair geometry for the underlined element ?
The incorrect statement regarding above reactions is
$\mathop {Al}\limits_{Metal} \xrightarrow{{HCl(aq.)}}'X' + Gas\,'P'$
$\mathop {Al}\limits_{metal} \xrightarrow[{ + {H_2}O}]{{NaOH\,(aq.)}}'Y' + Gas\,'Q'$
The incorrect statement regarding above reactions is
$\mathop {Al}\limits_{Metal} \xrightarrow{{HCl(aq.)}}'X' + Gas\,'P'$
$\mathop {Al}\limits_{metal} \xrightarrow[{ + {H_2}O}]{{NaOH\,(aq.)}}'Y' + Gas\,'Q'$