which of the following bonds is most polar? a f-f b o-f c o-i d o-cl

Brief Explanations:

The polarity of a bond depends on the electronegativity difference between the two atoms forming the bond. The greater the electronegativity difference, the more polar the bond.

• For option A ($F - F$): The two atoms are the same (both $F$), so the electronegativity difference is $0$. This is a non - polar covalent bond.
• For option B ($O - F$): The electronegativity of $O$ is $3.44$ and of $F$ is $3.98$. The electronegativity difference $\Delta EN=3.98 - 3.44=0.54$.
• For option C ($O - I$): The electronegativity of $O$ is $3.44$ and of $I$ is $2.66$. The electronegativity difference $\Delta EN = 3.44-2.66 = 0.78$.
• For option D ($O - Cl$): The electronegativity of $O$ is $3.44$ and of $Cl$ is $3.16$. The electronegativity difference $\Delta EN=3.44 - 3.16=0.28$.

Since $0.78>0.54>0.28>0$, the $O - I$ bond has the largest electronegativity difference among the given options.

Answer:

C. O - I