Why LiCl is more covalent than NaCl?
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Answered by
23
It is a small difference between the electronegativity of lithium (o,98) and sodium (0,93) - for Li the value is higher.
Abhi05:
I was looking for a more detailed answer.... anyway, thanks... ☺️
ur welcome
nd maybe will edit is soon
btw which topics should be covered in this ques?
fajan's rule, I guess...
ohk
is it correct ques or becoz is kcl instead of nacl
It's correct. One of the last year's half yearly paper's question.
ok
Answered by
138
Heya user !!
Here's the answer you are looking for
Both LiCl and NaCl ought to be ionic compounds but LiCl is covalent but NaCl is ionic.
This is because of the small size of cation and large size of anion in LiCl. Since, the size of cation is small, it's polarising power is large. And since the anion is small, it's polarisability is more. Since covalency of a compound is directly proportional to the polarising power of the cation and polarisability of anion, LiCl is covalent.
Whereas in case of NaCl, the size of both cation and anion are nearly same, so polarising power of Na is not as much as Li in LiCl and polarisability of Cl in NaCl is not as much as Cl in LiCl.
Therefore, LiCl is more covalent than NaCl.
★★ HOPE THAT HELPS ☺️ ★★
Here's the answer you are looking for
Both LiCl and NaCl ought to be ionic compounds but LiCl is covalent but NaCl is ionic.
This is because of the small size of cation and large size of anion in LiCl. Since, the size of cation is small, it's polarising power is large. And since the anion is small, it's polarisability is more. Since covalency of a compound is directly proportional to the polarising power of the cation and polarisability of anion, LiCl is covalent.
Whereas in case of NaCl, the size of both cation and anion are nearly same, so polarising power of Na is not as much as Li in LiCl and polarisability of Cl in NaCl is not as much as Cl in LiCl.
Therefore, LiCl is more covalent than NaCl.
★★ HOPE THAT HELPS ☺️ ★★
Thanks!! just what i needed..
Welcome :-)
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