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(C) $(i)$ $\mathop {Al^{3+}}\limits_{	ext{Most stable}}$ $\xrightarrow{E^o = -1.66} Al \xleftarrow{E^o = +0.55} \mathop {Al^{+}}\limits_{	ext{Less s

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$Tl^{+}$ is more stable than $Al^{+}$

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(C) $(i)$ $\mathop {Al^{3+}}\limits_{	ext{Most stable}}$ $\xrightarrow{E^o = -1.66} Al \xleftarrow{E^o = +0.55} \mathop {Al^{+}}\limits_{	ext{Less stable}}$$(ii)$ $\mathop {Tl^{3+}}\limits_{	ext{Less stable}}$ $\xrightarrow{E^o = +1.26} Tl \xleftarrow{E^o = -0.34} \mathop {Tl^{+}}\limits_{	ext{Most stable}}$For $Al$,the reduction potential of $Al^{3+}/Al$ is $-1.66 \ V$,indicating $Al^{3+}$ is highly stable. For $Tl$,the reduction potential of $Tl^{+}/Tl$ is $-0.34 \ V$,while $Tl^{3+}/Tl$ is $+1.26 \ V$. $A$ more negative reduction potential for the $M^{+}/M$ couple indicates higher stability of the $M^{+}$ ion relative to the metal. Comparing the stability of $Tl^{+}$ and $Al^{+}$,$Tl^{+}$ is more stable due to the inert pair effect and its lower reduction potential compared to $Al^{+}$. Thus,$Tl^{+}$ is more stable than $Al^{+}$.

Element	$M^{3+}/M$	$M^{+}/M$
$Al$	$-1.66$	$+0.55$
$Tl$	$+1.26$	$-0.34$

Consider the following standard electrode potentials ($E^o$ in volts) in aqueous solution:

Element $M^{3+}/M$ $M^{+}/M$

$Al$ $-1.66$ $+0.55$

$Tl$ $+1.26$ $-0.34$

Based on these data,which of the following statements is correct?

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Consider the following standard electrode potentials ($E^o$ in volts) in aqueous solution: Element $M^{3+}/M$ $M^{+}/M$ $Al$ $-1.66$ $+0.55$ $Tl$ $+1.26$ $-0.34$ Based on these data,which of the following statements is correct?