The Ionic Character of the following molecules is:
N2 < IO2< KBr< K2O< LiF : N-N < I-O < K-Br < K-O < Li-F
The difference in electronegativity between two atoms is the guiding principle to check about the Ionic bond. Since F is the highest electronegative element andit has the huge electronegativity difference with that of Li which makes it the strongest ionic compound and Li-F, the strongest Ionic bond.
In case of K2O the electronegativity of O is par compared to the metal K that makes it Ionic compound but less Ionic compared to LiF.
KBr is an Ionic compound but less Ionic compared to K2O as the O is more electronegative compared to Br.
In case of IO2 the difference is not that much which makes it less ionic and incase of N2, the electronegativity is zero that makes it least Ionic.
Can someone tell me what's wrong woth this? 2. 0/5.88 points Previous Answers ChangE7 9.E.033. D...