Arrange the bonds in order of increasing ionic character in the molecules: LiF, K2O, N2, SO2 and ClF3.
Dipole moment helps in calculating the percentage ionic character of polar bonds. It is the ratio of observed dipole moment to the dipole moment for the complete transfer of electrons. Greater the difference in electronegativity of bonding atoms, the greater will be the ionic character.
On this basis, the order of increasing ionic character in the given molecules is
N2 < SO2 < ClF3 < K2O < LiF.
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Welcome to the NCERT Solutions for Class 11 Chemistry - Chapter . This page offers a step-by-step solution to the specific question from Excercise 1 , Question 19: Arrange the bonds in order of increasing ionic character in the molecules: LiF, K2O, N2, SO2 and ClF....
Comments
Finally there is a question correctð
What is the bond order of LiF
Guys this is correct!!!
the electron negativity difference between Li &F ismore as compared to K2O but how ClF3 is less ionic character than SO2
The electronegativity difference between li & F is more as compared to the electronegativity difference between K & o, therefore the ionic character is more in liF as compared to k2o
How is k2o is less ionic in nature then lif