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Prob 2. Arrange the bonds in order of increasing ionic character in the molecules: LiF, K2O, N2, SO2 and ClF3 Sol. N2 Mera question is how come the ionic character is higher in SO2 than in ClF3 ?? Both have the same electronegativity difference..??then?? Please thx in advance to all those take pain in answering me GOD BLESS!!!

Prob 2. Arrange the bonds in order of increasing ionic character in the molecules:




LiF, K2O, N2, SO2 and ClF3




Sol. N2 < ClF3 < SO2 < K2O < LiF

Mera question is how come the ionic character is higher in SO2 than in ClF3 ??
Both have the same electronegativity difference..??then??
Please thx in advance to all those take pain in answering me GOD BLESS!!!

Grade:12

2 Answers

Sudheesh Singanamalla
114 Points
10 years ago

the key here is that there are 3 F atoms in ClF3 and only two O atoms in SO2.... and as already told you that the difference b/w the electronegativity of F and O is bit high....so definitely ClF3 will be more ionic than SO2....

when you arrange all of them now...

N2 < SO2 < ClF3 < K2O < LiF

 

ClF3 is more ionic than SO2 ..

i think the given solution in the problem you have given is incorrect , maybe a printing mistake , but here is the solution above.

 

source : it came for my school exam , and i got it right :D

Dhdhdfkfkf
13 Points
2 years ago
SO2 have low polarisation than CLF3 therefore more covalent character of CLF3 and hence SO2 have high ionic characters

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