Question

arrange the highlighted bonds in the table below in decreasing order of polarity. that is, pick 1 for the most polar bond, pick 2 for the next most polar bond, and so on.

bond	polarity
:f: :f—p—f:	2
:f: :f s f: :f:	3 (least polar)

Explanation:

Step1: Recall electronegativity concept

Polarity of a bond depends on electronegativity difference between atoms in the bond. Fluorine (F) is the most electronegative element.

Step2: Analyze Cl - F bond

In the Cl - F bond, chlorine (Cl) has an electronegativity of 3.16 and fluorine (F) has an electronegativity of 3.98. The electronegativity difference $\Delta\chi=3.98 - 3.16=0.82$.

Step3: Analyze P - F bond

For the P - F bond, phosphorus (P) has an electronegativity of 2.19 and fluorine (F) has an electronegativity of 3.98. The electronegativity difference $\Delta\chi = 3.98-2.19 = 1.79$.

Step4: Analyze S - F bond

In the S - F bond, sulfur (S) has an electronegativity of 2.58 and fluorine (F) has an electronegativity of 3.98. The electronegativity difference $\Delta\chi=3.98 - 2.58 = 1.4$.

Step5: Compare electronegativity differences

Since $1.79>1.4>0.82$, the P - F bond is the most polar, followed by the S - F bond and then the Cl - F bond.

Answer:

1. P - F
2. S - F
3. Cl - F