If the bond length and dipole moment of a dia | vedclass

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(C) The dipole moment of a purely ionic bond is calculated as $\mu_{	ext{theoretical}} = q 	imes d$.
Given: bond length $d = 1.25 \ \mathring{A} =

Vedclass · Accepted Answer

$16.66$

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(C) The dipole moment of a purely ionic bond is calculated as $\mu_{	ext{theoretical}} = q 	imes d$.
Given: bond length $d = 1.25 \ \mathring{A} = 1.25 	imes 10^{-8} \ cm$.
The charge of an electron $q = 4.8 	imes 10^{-10} \ esu$.
$\mu_{	ext{theoretical}} = 1.25 	imes 10^{-8} \ cm 	imes 4.8 	imes 10^{-10} \ esu = 6.0 	imes 10^{-18} \ esu \ cm = 6.0 \ D$.
Given experimental dipole moment $\mu_{	ext{experimental}} = 1.0 \ D$.
Percent ionic character $= \frac{\mu_{	ext{experimental}}}{\mu_{	ext{theoretical}}} 	imes 100 = \frac{1.0}{6.0} 	imes 100 = 16.66 \%$.

If the bond length and dipole moment of a diatomic molecule are $1.25 \ \mathring{A}$ and $1.0 \ D$ respectively,what is the percent ionic character of the bond?

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