Home
Class 11
CHEMISTRY
If the molecule of HCl were totally pola...

If the molecule of HCl were totally polar, the observed value of dipole moment is 1.03 D (debye) but the experimental value of dipole moment was 6.12 D. Calculate the percentage ionic character.

A

17

B

83

C

50

D

zero

Text Solution

Verified by Experts

The correct Answer is:
A
% of ionic character
` = ("Experimental value of dipole moment")/("Expected value of dipole moment")`
`= (1.03)/(6.12) xx 100 = 16.83%~~ 17%`
Promotional Banner

Similar Questions

Explore conceptually related problems

If the molecule of HCl were totally polar, the expected value of dipole moment is 6-12 D (debye) but the experimental value of dipole moment was 1.03 D. Calculate the percentage ionic character.

A polar molecule AB have dipole monment 3.2 D (Debye) while the bond length is 1.6Å . Find the percentage ionic character in the molecule.

Dipole moment of is 1.5 D . The dipole moment of is

The dipole moment of is 1.5 D. The dipole moment of is

The observed dipole moment of HI is 0.38D. Calculate the percentage ionic character of the H-I bond distance is 1.61Å .