why LiCl is not considered as a ionic compound?
why LiCl is not considered as a ionic compound?
Actually LiCl is an ionic compound. But the ionic character LiCl is less compared to others metals like NaCl, KCl, RbCl, CsCl down the group.
It is said that a bond between atoms with similar electronegativity values are said to be covalent. A bond between atoms whose electronegativity values differ by less than 2 units are said to be polar covalent. A bond between atoms whose electronegativity values differ by 2 units or more are said to be largely ionic.
When compared the difference in the electronegativity values of the compounds LiCl, NaCl, KCl, RbCl, CsCl increases from 2.0 to 2.3 down the group, showing increase in ionic character.
LiCl = 2.00 (where EN of Li = 1.0 and Cl = 3.00)
NaCl = 2.1 (where EN of Na = 0.9 and Cl = 3.00)
KCl = 2.2 (where EN of K = 0.8 and Cl = 3.00)
RbCl = 2.2 (where EN of Rb = 0.8 and Cl = 3.00)
CsCl = 2.3 (where EN of Cs = 0.7 and Cl = 3.00)
Hence LiCl shows less ionic character.
Actually LiCl is an ionic compound. But the ionic character LiCl is less compared to others metals like NaCl, KCl, RbCl, CsCl down the group.
It is said that a bond between atoms with similar electronegativity values are said to be covalent. A bond between atoms whose electronegativity values differ by less than 2 units are said to be polar covalent. A bond between atoms whose electronegativity values differ by 2 units or more are said to be largely ionic.
When compared the difference in the electronegativity values of the compounds LiCl, NaCl, KCl, RbCl, CsCl increases from 2.0 to 2.3 down the group, showing increase in ionic character.
LiCl = 2.00 (where EN of Li = 1.0 and Cl = 3.00)
NaCl = 2.1 (where EN of Na = 0.9 and Cl = 3.00)
KCl = 2.2 (where EN of K = 0.8 and Cl = 3.00)
RbCl = 2.2 (where EN of Rb = 0.8 and Cl = 3.00)
CsCl = 2.3 (where EN of Cs = 0.7 and Cl = 3.00)
Hence LiCl shows less ionic character.
