Question

Which of the following is correctly matched with the given property?

• A. $\underset{}{M g S O_{4} < C a S O_{4} < S r S O_{4}} < BaSO_{4}\left(Solubility in water\right)$
• B. $\underset{}{B e C O_{3} > M g C O_{3} >}CaCO_{3}>SrCO_{3}>BaCO_{3}\left(Thermal Stability\right)$
• C. $\underset{}{NaOCl > NaOBr >}NaOI\left(Oxidising nature\right)$
• D. $\underset{}{F_{2} > \left(Cl\right)_{2} > \left(Br\right)_{2}}>I_{2}\left(Bond energy\right)$

Answer 1

Answer: (C)

The greater the lattice enthalpy, the more stable is the ionic compound. The ionic compound of the large cation with a small anion or small cation with a large anion are readily soluble in water.
Solubility order: $MgSO_{4}>CaSO_{4}>SrSO_{4}>BaSO_{4}$
Thermal stability: $BaCO_{3}>SrCO_{3}>CaCO_{3}>MgCO_{3}>BeCO_{3}$
The correct order of Oxidising nature is $NaOCl>NaOBr>NaOI$
Electronegativity of halogen increases, the tendency to gain of electron increases, so oxidising nature increases.
Bond energy order of halogens is $Cl_{2}>Br_{2}>F_{2}>I_{2}$