The dipole moment of HCl is 1.03 D. If the H | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(D) Dipole moment is the product of the magnitude of charge and the separation between charges. $P = q 	imes d$ For a fully ionic bond,one electron i

Vedclass · Accepted Answer

$17$

Vedclass · Answer

(D) Dipole moment is the product of the magnitude of charge and the separation between charges. $P = q 	imes d$ For a fully ionic bond,one electron is transferred from hydrogen to chlorine. Magnitude of charge,$q = 1.6 	imes 10^{-19} \ C$. Bond length,$d = 1.26 \ \mathring{A} = 1.26 	imes 10^{-10} \ m$. Theoretical dipole moment,$P_{theoretical} = 1.6 	imes 10^{-19} \ C 	imes 1.26 	imes 10^{-10} \ m = 2.016 	imes 10^{-29} \ Cm$. Since $1 \ D = 3.335 	imes 10^{-30} \ Cm$,$P_{theoretical} = \frac{2.016 	imes 10^{-29}}{3.335 	imes 10^{-30}} \ D \approx 6.045 \ D$. Percentage ionic character = $\frac{	ext{Experimental dipole moment}}{	ext{Theoretical dipole moment}} 	imes 100$ $= \frac{1.03 \ D}{6.045 \ D} 	imes 100 \approx 17.04 \ \%$. Thus,the percentage of ionic character is approximately $17 \ \%$.

The dipole moment of $HCl$ is $1.03 \ D$. If the $H-Cl$ bond distance is $1.26 \ \mathring{A}$,what is the percentage of ionic character in the $H-Cl$ bond? ............. $\%$

Similar Questions

Which of the following molecules will have polar bonds but zero dipole moment?

If $HCl$ were purely ionic,its expected dipole moment would be $6.12 \, D$. However,the experimental dipole moment is $1.03 \, D$. Calculate the percentage ionic character. (in $\%$)

Which of the following has a dipole moment of zero?

Which of the following has the highest dipole moment?

Arrange the following molecules from most to least polar ($I$,$II$,$III$,$IV$,$V$ respectively): $CH_4$,$CF_2Cl_2$,$CF_2H_2$,$CCl_4$,$CCl_2H_2$.

Vedclass Test Series

Exam Paper Generator

Online Exam Module