Unit 7 The P Block Elements (Intext Questions-12)
Intext Questions
7.26 Considering the parameters such as bond dissociation enthalpy, electron gain enthalpy and hydration enthalpy, compare the oxidising power of $\mathrm{F_2}$ and $\mathrm{Cl_2}$.
Answer Fluorine is a much stronger oxidizing agent than chlorine. The oxidizing power depends on three factors. 1. Bond dissociation energy 2. Electron gain enthalpy 3. Hydration enthalpy The electron gain enthalpy of chlorine is more negative than that of fluorine. However, the bond dissociation energy of fluorine is much lesser than that of chlorine. Also, because of its small size, the hydration energy of fluorine is much higher than that of chlorine. Therefore, the latter two factors more than compensate for the less negative electron gain enthalpy of fluorine. Thus, fluorine is a much stronger oxidizing agent than chlorine.Show Answer
Answer Anomalous behaviour of fluorine (i) It forms only one oxoacid as compared to other halogens that form a number of oxoacids. (ii) Ionisation enthalpy, electronegativity, and electrode potential of fluorine are much higher than expected.Show Answer
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Answer
Sea water contains chlorides, bromides, and iodides of $\mathrm{Na}, \mathrm{K}, \mathrm{Mg}$, and $\mathrm{Ca}$. However, it primarily contains $\mathrm{NaCl}$. The deposits of dried up sea beds contain sodium chloride and carnallite, $\mathrm{KCl} . \mathrm{MgCl_2} \cdot 6 \mathrm{H_2} \mathrm{O}$. Marine life also contains iodine in their systems. For example, sea weeds contain upto $0.5 \%$ iodine as sodium iodide. Thus, sea is the greatest source of halogens.
