If $HCl$ molecule is completely polarized,the expected value of the dipole moment is $6.12 \ D$,but the experimental value of the dipole moment is $1.03 \ D$. Calculate the percentage ionic character.
- A$17$
- B$83$
- C$50$
- D$0$
Explore More
Similar Questions
The dipole moments of $CCl_{4}$,$CHCl_{3}$ and $CH_{4}$ are in the order:
Experiments show that the $H_2O$ molecule has a dipole moment,while $CO_2$ does not. Which of the following structures best represents this fact?
Medium
View SolutionWhich of the following molecules is non-polar in nature?
Which of the following substances has the lowest dipole moment?
Easy
View SolutionWhich compound exhibits the maximum dipole moment among the following?
DifficultJEE MAIN 2015
View SolutionVedclass Products
For Students
Vedclass Test Series
Mock tests in real JEE/NEET style with performance analysis. 5-day free trial.
Start Free TrialFor Teachers
Exam Paper Generator
Generate Set A/B/C/D exam papers from 7.5L+ questions in 2 minutes. 3 chapters free.
Try FreeFor Institutes
Online Exam Module
Live online exams with unlimited students, 360° analytics & white-label branding.
See Demo