Question

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

• A. $T{l}^{+}$ is more stable than $A{l}^{3+}$
• B. $T{l}^{+}$ is more stable than $A{l}^{+}$
• C. $A{l}^{+}$ is more stable than $A{l}^{3+}$
• D. $T{l}^{3+}$ is more stable than $A{l}^{3+}$

Answer 1

Answer: (B)

$T{l}^{+}$ is more stable than $A{l}^{+}$

$T{l}^{+}$ is more stable than $A{l}^{+}$

$T{l}^{+}|Tl(-0.34)$ V is less negative than $A{l}^{+}|Al(+0.55)$ V or oxidation potential is more.

$T{l}^{+}$ is weaker oxidizing agent than $A{l}^{+}$