Question

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

Explanation:

Step1: Recall polarity rule

The greater the electronegativity difference ($\Delta\chi$) between two atoms in a bond, the more polar the bond.

Step2: Calculate differences for possible bonds

Assume we consider common bonds. For example, if we consider K - F bond, $\Delta\chi=4.0 - 0.8=3.2$; for K - O, $\Delta\chi = 3.5 - 0.8 = 2.7$; for K - Cl, $\Delta\chi=3.0 - 0.8 = 2.2$; for K - Br, $\Delta\chi=2.8 - 0.8 = 2.0$; for H - F, $\Delta\chi=4.0 - 2.1 = 1.9$; for H - O, $\Delta\chi=3.5 - 2.1 = 1.4$; for H - Cl, $\Delta\chi=3.0 - 2.1 = 0.9$; for H - Br, $\Delta\chi=2.8 - 2.1 = 0.7$. The largest $\Delta\chi$ value is for the K - F bond.

Answer:

The K - F bond is the most polar.