Give two examples to show the anomalous behaviour of fluorine.
(N/A) The anomalous behaviour of fluorine is due to its small size,high electronegativity,low $F-F$ bond dissociation enthalpy,and absence of $d$-orbitals in its valence shell.
$i$. Fluorine forms only one oxoacid $(HOF)$,whereas other halogens form a number of oxoacids (e.g.,$HOCl, HOClO, HOClO_2, HOClO_3$).
$ii$. The ionisation enthalpy,electronegativity,and electrode potential of fluorine are much higher than expected compared to other halogens.
$i$. Fluorine forms only one oxoacid $(HOF)$,whereas other halogens form a number of oxoacids (e.g.,$HOCl, HOClO, HOClO_2, HOClO_3$).
$ii$. The ionisation enthalpy,electronegativity,and electrode potential of fluorine are much higher than expected compared to other halogens.
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