Question

Which of the following is correctly ranked in order of increasing bond polarity? O-O < O-F Cl-S < Cl-Br Al-O < P-O H-H < N-N B-F < C-F F-O < O-O Li-F < C-O

Answer 1

Answer:

O-O<O-F

option 1 is correct.

Explanation: The bond polarity can be explained on the basis electronegative difference between the atoms.

Greater the electronegativity difference between the two atoms in a bond greater is the polarity of the bond.

Electronegativity difference of a bond between two atoms =EN of atom having higher electronegativity- EN of atom having lower electronegativity

Likewise we can calculate the electronegativity difference for the following bonds and estimate there bond polarities.

1.EN[O-O]=EN(O)-EN(O)=(3.44)-(3.44)=0

EN[O-F]=EN(F)-EN(O)=(3.98)-(3.44)=0.54

So the bond polarity of O-F is more than O-O as it has more electronegativity difference. These two species are correctly arranged as O-O<O-F

2.EN[Cl-S]=EN(S)-EN(Cl)=(3.16)-(2.58)=0.58

EN[Cl-Br]=EN(Cl)-EN(Br)=(3.16)-(2.96)=0.20

So the bond polarity of Cl-S is more than Cl-Br as it has more electronegativity difference. These two species are incorrectly arranged as Cl-S>Cl-Br.

3. EN[Al-O]=EN(O)-EN(Al)=(3.44)-(1.61)=1.83

EN[P-O]=EN(O)-EN(P)=(3.44)-(2.19)=1.25

So the bond polarity of Al-O is more than P-O as it has more electronegativity difference. These two species are incorrectly arranged as Al-O>P-O.

4.EN[H-H]=EN(H)-EN(H)=(2.2)-(2.2)=0

EN[N-N]=EN(H)-EN(N)=(3.04)-(3.04)=0

The electronegativity difference for both the bonds is 0 hence both the bonds would not have any polarity. Hence the mentioned order is incorrect.  

5. EN[B--]=EN(F)-EN(B)=(3.98)-(2.04)=1.94

EN[C-F]=EN(F)-EN(C)=(3.98)-(2.55)=1.43

So the bond polarity of B-- is more than C-F as it has more electronegativity difference. These two species are incorrectly arranged as B-->C-F

6. EN[Li-F]=EN(F)-EN(Li)=(3.98)-(0.98)=3.0

EN[C-O]=EN(O)-EN(C)=(3.44)-(2.55)=0.89.

So the bond polarity of Li-F is more than C-O as it has more electronegativity difference. These two species are incorrectly arranged as Li-F>C-O

7. EN[F-O]=EN(F)-EN(O)=(3.98)-(3.44)=0.54

EN[O-O]=EN(O)-EN(O)=(3.44)-(3.44)=0

So the bond polarity of F-O is more than O-O as it has more

electronegativity difference. So it is incorrectly arranged.

Answer 2

The correct order of increasing polarity of bonds is O-O < O-F.

The polarity of bonds is caused by differences in electronegativity of the bonding atoms. The nature of a bond depends on the relative electronegativity  values of the atoms in the bond. If there is an electronegativity difference less than 0.5, we have a nonpolar covalent bond. An electronegativity difference between 0.5 - 1.00 gives us a polar covalent bond. An electronegativity difference above 1.00 leads an ionic bond between atoms.

Based on this information, we can now decide the order of increasing bond polarity of the bonds as shown. We can see that, the correct order of increasing polarity of bonds is O-O < O-F.

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