Select the incorrect statement.

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(NONE) $1$. The stability of peroxides $(O_2^{2-})$ and superoxides $(O_2^-)$ of alkali metals increases as the size of the alkali metal cation increa

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$NaOH$ does not form a hydrated salt.

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(NONE) $1$. The stability of peroxides $(O_2^{2-})$ and superoxides $(O_2^-)$ of alkali metals increases as the size of the alkali metal cation increases. This is because larger cations stabilize larger anions more effectively through lattice energy effects. Thus,statement $(a)$ and $(c)$ are correct.$2$. $NaOH$ is highly hygroscopic and absorbs moisture from the atmosphere to form a concentrated solution,but it does not form a stable crystalline hydrated salt like $LiOH \cdot H_2O$. Thus,statement $(b)$ is correct.$3$. The solubility of alkali metal halides depends on the balance between lattice energy and hydration energy. $LiF$ has very high lattice energy due to the small size of both $Li^+$ and $F^-$,making it sparingly soluble. $CsI$ has low lattice energy,but its solubility is limited by the very low hydration energy of the large $Cs^+$ and $I^-$ ions. However,the statement provided in $(d)$ is generally accepted in textbooks as a correct explanation for the solubility trends of these specific salts. $4$. Upon re-evaluating the options,all statements provided are scientifically correct. If this is a multiple-choice question where one must be incorrect,there may be a typo in the source. However,based on standard chemical principles,all statements are true.

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The incorrect statement regarding the above reactions is:
$Al_{(metal)} \xrightarrow[HCl]{(aq.)} 'X' + \text{Gas } 'P'$
$Al_{(metal)} \xrightarrow[NaOH (aq.)]{+ H_2O} 'Y' + \text{Gas } 'Q'$

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