Question

question 4 (1 point) which of the following bonds is the most polar? electronnegativity values: k: 0.8 h: 2.1 br: 2.8 cl: 3.0 o: 3.5 f: 4.0 o - f h - cl h - br k - cl

Explanation:

Step1: Recall polarity - electronegativity relation

Polarity of a bond depends on electronegativity difference ($\Delta\chi$) between the two atoms in the bond. The formula for $\Delta\chi$ is $\Delta\chi=\vert\chi_1 - \chi_2\vert$, where $\chi_1$ and $\chi_2$ are electronegativities of the two atoms.

Step2: Calculate $\Delta\chi$ for O - F

$\Delta\chi_{O - F}=\vert3.5 - 4.0\vert= 0.5$

Step3: Calculate $\Delta\chi$ for K - Cl

$\Delta\chi_{K - Cl}=\vert0.8 - 3.0\vert = 2.2$

Step4: Calculate $\Delta\chi$ for H - Br

$\Delta\chi_{H - Br}=\vert2.1-2.8\vert = 0.7$

Step5: Calculate $\Delta\chi$ for H - Cl

$\Delta\chi_{H - Cl}=\vert2.1 - 3.0\vert=0.9$

Step6: Compare the values

We have $\Delta\chi_{O - F}=0.5$, $\Delta\chi_{K - Cl}=2.2$, $\Delta\chi_{H - Br}=0.7$, $\Delta\chi_{H - Cl}=0.9$. Since $2.2>0.9 > 0.7>0.5$, the K - Cl bond has the highest electronegativity difference.

Answer:

K - Cl