If the molecule of $HCl$ were totally polar, the expected value of dipole moment is $6.12{\rm{ }}D$ (dbye), but the experimental value of dipole moment was $1.03{\rm{ }}D$. Calculate the percentage ionic character

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JEE CHEMISTRY MCQ: CHEMICAL BONDING & MOLECULAR STRUCTURE

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If the molecule of

HCl

were totally polar, the expected value of dipole moment is

6.12\mathrm{ }D

(dbye), but the experimental value of dipole moment was

1.03\mathrm{ }D

. Calculate the percentage ionic character

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Correct option: A

Option A (17) is correct because the percentage ionic character is calculated by dividing the experimental dipole moment by the theoretical dipole moment and multiplying by 100.

JEE CHEMISTRY MCQ: CHEMICAL BONDING & MOLECULAR STRUCTURE

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