7.27 Give two examples to show the anomalous behaviour of fluorine. 

<p><strong>7.27</strong></p><p>The reasons for the anomalous behaviour of fluorine are as follows:</p><p>The smallest size of fluorine</p><p>The highest electronegativity</p><p>Low bond dissociation enthalpy of F-F bond</p><p>Non-availability of d-orbitals in its valence shell The anomalous properties are as follows;</p><p>Fluorine shows only one oxidation state-1 while all other halogens show variable oxidation states like</p><p>-1, +1, +3, +5, +7 (due to small size, high electronegativity)</p><p>Fluorine forms strong hydrogen bonding in its hydrides unlike other halogens. (due to high hydration energy than other elements)</p><p>The compounds of fluorine have higher ionic character than other halogens. (due to high electronegativity forming polar interactions)</p><p>Fluorine has no tendency to form polyhalide ion whereas other halogen form polyhalideion (due to non-availability of d orbitals in valence shell)</p>

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