Which of the foll A. F2> Cl2> Br2> I2Oxidising power.
B. MI <MBr<MCl< MF Ionic character of metal halide.
C. F2> Cl2> Br2> I2 Bond dissociation enthalpy.
D. HI <HBr<HCl< HF Hydrogen-halogen bond strength.
I2 has more oxidizing power than halogen atoms because of large size of iodine it can easily accommodate electrons. Down the group size of the atom increases and oxidizing power also increases. therefore the order is F2< Cl2< Br2< I2
IONIC CHARACTER: the bond in which large electronegativity difference exists between two atoms.
Ionic character increases with increase in electronegativity of halogens
Therefore the order is MI <MBr<MCl< MF
BOND DISSOCIATION ENTHALPY: the amount of energy required to break the bond
As the bond length increases, bond dissociation enthalpy decreases.
More amount of energy is required to break the bond of small length. Bomd length of F-F is small hence it requires more energy to dissociate than Cl-Cl, Br-Br, I-I.
Hence the order of bond dissociation enthalpy is:
F2> Cl2> Br2> I2
Therefore bond dissociation enthalpy also increases.
Hence the correct options are (ii)and(iii)
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