MCQ
The dipole moment of $HCl$ is $1.03\, D$, if $H-Cl$ bond distance is $1.26\,\overset{o}{\mathop{A}}\,,$ what is the percentage of ionic character in the $H-Cl$ bond? ............. $\%$
- A$60$
- B$39$
- C$29$
- ✓$17$
i.e., $P=q \times d$
here compound is $HCl$,you know as well, $HCl$ is ionic compound in which one electron transfers from hydrogen to chlorine.
so, magnitude of charge on dipole, $q =1.6 \times 10^{-19} \,C$
and seperation between charges $=$ bond length $=1.26 A ^{\circ}=1.26 \times 10^{-10} \,m$
so, dipole moment, $P =1.6 \times 10^{-19} \times 1.26 \times 10^{-10}\, Cm$ $=2.016 \times 10^{-29}\, Cm$
we know, $1 D =3.335 \times 10^{-30}\, Cm$ [ Debay, $D$ is the unit of dipole moment ] $=2.016 \times 10^{-29} /\left(3.335 \times 10^{-30}\right)$
$=20.16 / 3.335$
$=6.0449\, D$
now, percentage ionic character $=$ experimental value/ theoretical value $\times 100$ $=1.03 \,D / 6.0449 \,D \times 100$
$=0.170 \times 100$
$=17.00\, \%$
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where $K_c$ is the equilibrium constant
$(I)\,C{H_3}O\mathop C\limits^ \oplus {H_2}$ is more stable than $C{H_3}\mathop C\limits^ \oplus {H_2}$
$(II)\,M{e_2}\mathop C\limits^ \oplus H$ is more stable than $C{H_3}C{H_2}\mathop C\limits^ \oplus {H_2}$
$(III)\,C{H_2} = CH - \mathop C\limits^ \oplus {H_2}$ is more stable than $C{H_3}C{H_2}\mathop C\limits^ \oplus {H_2}$
$(IV)\,C{H_2} = \mathop C\limits^ \oplus H$ is more stable than $C{H_3}\mathop C\limits^ \oplus {H_2}$