Which one of the following statements is NOT correct about the compounds of alkaline earth metals?

Which one of the following statements is NOT correct about the compounds of alkaline earth metals?
  1. Basic nature increases from $\mathrm{Mg}(\mathrm{OH})_2$ to $\mathrm{Ba}(\mathrm{OH})_2$
  2. Thermal stability decreases from $\mathrm{BeCO}_3$ to $\mathrm{BaCO}_3$
  3. Solubility of sulphates in water decreases from $\mathrm{BeSO}_4$ to $\mathrm{BaSO}_4$
  4. Nitrates of these on heating give oxides

Solution

$\mathrm{Be}(\mathrm{OH})_2$ is amphoteric, but the hydroxides of Mg , $\mathrm{Ca}, \mathrm{Sr}$ and Ba are basic. The strength increases from Mg to Ba . Carbonates of group 2 elements become more thermally stable down the group. The larger compounds require more heat than the lighter compounds in order to decompose. $\begin{array}{lll} \mathrm{BeCO}_3 & \mathrm{MgCO}_3 \mathrm{CaCO}_3 \mathrm{SrCO}_3 & \mathrm{BaCO}_3 \\ \lt 100^{\circ} \mathrm{C} 540^{\circ} \mathrm{C} & 900^{\circ} \mathrm{C} & 1290^{\circ} \mathrm{C} \\ 1360^{\circ} \mathrm{C} \end{array}$
The solubility of the sulphates in water decreases down the group. $\mathrm{Be}\gt\mathrm{Mg} \gg \mathrm{Ca}\gt\mathrm{Sr}\gt\mathrm{Ba}$. The higher solubilities of $\mathrm{BeSO}_4$ and $\mathrm{MgSO}_4$ have high enthalpy of solvation of the smaller $\mathrm{Be}^{2+}$ and $\mathrm{Mg}^{2+}$ ions. On heading, the alkaline earth metal nitrates decompose 10 give metal oxide, nitrogen dioxide and oxygen $2 \mathrm{M}\left(\mathrm{NO}_3\right)_2 \xrightarrow{\Delta} 2 \mathrm{MO}+4 \mathrm{NO}_2+\mathrm{O}_2(\mathrm{M}=\mathrm{Be}, \mathrm{Mg},$ $\mathrm{Ca})$

Asked in: AP EAMCET 2024 (21 May Shift 2)

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