[Qwertyqwerty]

What are the factors that determine the strength of an Ionic bond?
Taking the example of LiF and K₂0, why does LiF have a stronger bond strength?

[PaintYourFuture]

Electronegativity

[jp92celtic]

look at a table of electronegativity values and calculate the difference between your two atoms

[Qwertyqwerty]

Isn't there a way to find it out without looking at the electronegativity table? Some general rules one might follow?

The question I had was :
Arrange the bonds in order of the increasing ionic character of the molecules :
LiF, K₂O, SO₂, N₂ and ClF₃

Of which the answer was
N₂<SO₂<ClF₃<LiF<K₂O

I can't understand as to why K₂O has a stronger ionic character than LiF.

[jp92celtic]

as a general rule, looking at the periodic table can help:
N₂ obviously has equal EN values, and shares perfectly equally (covalent)
SO₂ has S and O which are both in the same column, one above the other, so they are relatively close in EN.
ClF₃ has the same situation as above but are to the right (more EN)
LiF are hugely separated left to right, but are in the same row as each other.
K₂O is also separated a lot left to right, but K is two whole rows below O, so therefore it has the greatest difference in EN.

[Qwertyqwerty]

Finally understood. Thank you