Which one of the following arrangements does not give the correct picture of the trends indicated against it?

Question

Which one of the following arrangements does not give the correct picture of the trends indicated against it? (A)  F2 > Cl2 > Br2 > I2 Oxidising power (B)  F2 > Cl2 > Br2 > I2 Electron gain enthalpy (C)  F2 > Cl2 > Br2 > I2 Bond dissociation energy (D)  F2 > Cl2 > Br2 > I2 Electronegativity

Tardigrade Admin · Accepted Answer

Generally, bond dissociation energy follows the electronegativity trend. But in the case of halogens, a small change is there.
Fluorine is more electronegative than Chlorine. But Fluorine is very small compared to Chlorine. The bond length of Fluorine is less than Chlorine. There are more repulsions between Fluorine atoms in

F_{2}

because of the abovementioned reasons.
If repulsions are there bond dissociation energy decreases. But in Chlorine, it doesn't happen. It has enough size and repulsions are less so the order of bond energy is:

C l_{2} > B r_{2} > F_{2} > I_{2}

Q. Which one of the following arrangements does not give the correct picture of the trends indicated against it?

$F_{2} > C l_{2} > B r_{2} > I_{2}$ Oxidising power

$F_{2} > C l_{2} > B r_{2} > I_{2}$ Electron gain enthalpy

$F_{2} > C l_{2} > B r_{2} > I_{2}$ Bond dissociation energy

$F_{2} > C l_{2} > B r_{2} > I_{2}$ Electronegativity

Q. Which one of the following arrangements does not give the correct picture of the trends indicated against it?

F2​>Cl2​>Br2​>I2​ Oxidising power

F2​>Cl2​>Br2​>I2​ Electron gain enthalpy

F2​>Cl2​>Br2​>I2​ Bond dissociation energy

F2​>Cl2​>Br2​>I2​ Electronegativity

$F_{2} > C l_{2} > B r_{2} > I_{2}$ Oxidising power

$F_{2} > C l_{2} > B r_{2} > I_{2}$ Electron gain enthalpy

$F_{2} > C l_{2} > B r_{2} > I_{2}$ Bond dissociation energy

$F_{2} > C l_{2} > B r_{2} > I_{2}$ Electronegativity