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

The ionic character of a bond is determined by the electronegativity difference ($\Delta \chi$) between the two atoms in the bond. The greater the electronegativity difference, the greater the ionic character.

Step2: Find electronegativity values

The electronegativity values from the Pauling scale are: $\chi_H = 2.20$, $\chi_{Cl}=3.16$, $\chi_{Zn}=1.65$, $\chi_{K} = 0.82$, $\chi_O=3.44$, $\chi_I = 2.66$.

Step3: Calculate electronegativity differences

For $K - O$: $\Delta\chi=\vert0.82 - 3.44\vert= 2.62$.
For $Zn - Cl$: $\Delta\chi=\vert1.65 - 3.16\vert = 1.51$.
For $H - Cl$: $\Delta\chi=\vert2.20 - 3.16\vert=0.96$.
For $I - I$: $\Delta\chi=\vert2.66 - 2.66\vert = 0$.

Step4: Order bonds by ionic character

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

Answer:

$K - O>Zn - Cl>H - Cl>I - I$