Arrange the bonds in order of increasing ioni | vedclass

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(C) The ionic character of a bond depends on the difference in electronegativity between the bonded atoms. Larger electronegativity difference leads t

Vedclass · Accepted Answer

$N_2 < SO_2 < ClF_3 < K_2O < LiF$

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(C) The ionic character of a bond depends on the difference in electronegativity between the bonded atoms. Larger electronegativity difference leads to higher ionic character.$1$. $N_2$ (non-polar covalent,$\Delta EN = 0$)$2$. $SO_2$ (polar covalent,$\Delta EN \approx 0.9$)$3$. $ClF_3$ (polar covalent,$\Delta EN \approx 1.0$)$4$. $K_2O$ (ionic,$\Delta EN \approx 2.6$)$5$. $LiF$ (ionic,$\Delta EN \approx 3.0$)Therefore,the increasing order of ionic character is: $N_2 < SO_2 < ClF_3 < K_2O < LiF$.

Arrange the bonds in order of increasing ionic character in the molecules: $LiF$,$K_2O$,$N_2$,$SO_2$,and $ClF_3$.

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