Question

list the following bonds in order of decreasing ionic character: the zinc - chlorine bond in zncl₂, the potassium - oxygen bond in k₂o, the hydrogen - chlorine bond in hcl, the iodine - iodine bond in i₂.

Explanation:

Step1: Recall ionic - character concept

Ionic character is determined by the electronegativity difference ($\Delta\chi$) between the two atoms in a bond. Larger $\Delta\chi$ means higher ionic character.

Step2: Find electronegativity values

Electronegativity values from the Pauling scale: $K = 0.82$, $O=3.44$, $Zn = 1.65$, $Cl = 3.16$, $H=2.20$, $I = 2.66$.

Step3: Calculate $\Delta\chi$ for each bond

For $K - O$ in $K_2O$: $\Delta\chi=3.44 - 0.82=2.62$.
For $Zn - Cl$ in $ZnCl_2$: $\Delta\chi = 3.16-1.65 = 1.51$.
For $H - Cl$ in $HCl$: $\Delta\chi=3.16 - 2.20 = 0.96$.
For $I - I$ in $I_2$: $\Delta\chi=2.66 - 2.66=0$.

Step4: Order the bonds

Based on the $\Delta\chi$ values, the order of decreasing ionic character is $K - O$ bond in $K_2O>Zn - Cl$ bond in $ZnCl_2>H - Cl$ bond in $HCl>I - I$ bond in $I_2$.

Answer:

Potassium - oxygen bond in $K_2O$ > Zinc - chlorine bond in $ZnCl_2$ > Hydrogen - chlorine bond in $HCl$ > Iodine - iodine bond in $I_2$