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Which statement is wrong :
A
Bond energy of $F_2 \gt Cl_2$
B
Electronegativity of F > Cl
C
F is more oxidising than Cl
D
Electron affinity of Cl > F
Detailed Solution
The bond dissociation energy of $F_2$ (about 158 kJ/mol) is less than that of $Cl_2$ (about 242 kJ/mol), because the small F atoms bring their lone pairs close and these repel strongly. So 'bond energy of $F_2 \gt Cl_2$' is wrong.
F is the most electronegative element, more than Cl; true.
$F_2$ is the strongest oxidising agent, stronger than $Cl_2$; true.
The electron affinity of Cl (–349 kJ/mol) is greater than that of F (–328 kJ/mol), because the small size of F causes electron repulsion; true.
So the wrong statement is 'bond energy of $F_2 \gt Cl_2$'.
F is the most electronegative element, more than Cl; true.
$F_2$ is the strongest oxidising agent, stronger than $Cl_2$; true.
The electron affinity of Cl (–349 kJ/mol) is greater than that of F (–328 kJ/mol), because the small size of F causes electron repulsion; true.
So the wrong statement is 'bond energy of $F_2 \gt Cl_2$'.