Read the passage carefully and answer the questions.

Nearly all the transition elements display typical metallic properties such as high tensile strength, ductility, malleability, high thermal and electrical conductivity and metallic lustre. The transition metals (with the exception of Zn, Cd and Hg) are very hard and have low volatility. Their melting and boiling points are high. They have high enthalpies of atomization. Ions of the same charge in a given series show progressive decrease in radius with increasing atomic number. However, the variation within a series is quite small. The filling of 4f before 5d orbital results in a regular decrease in atomic radii called Lanthanoid contraction which essentially compensates for the expected increase in atomic size with increasing atomic number. The net result of the lanthanoid contraction is that the second and the third d series exhibit similar radii (e.g., Zr 160 pm, Hf 159 pm) and have very similar physical and chemical properties. There is an increase in ionisation enthalpy along each series of the transition elements from left to right. The first ionisation enthalpy, in general, increases, but the magnitude of the increase in the second and third ionisation enthalpies for the successive elements, is much higher along a series. One of the notable features of a transition elements is the great variety of oxidation states these may show in their compounds.

Atomic number of V, Mn, Cu and Zn is 23, 25, 29 and 30 respectively. Which of them shows a positive value for the standard electrode potential $E°_{(M^{2+}/M)}$?

Cu

The correct answer is Option (2) → Cu

The complete statement is Copper (Cu) shows a positive standard electrode potential $E^\circ(M^{2+}/M)$.

Vanadium (V) – Vanadium has a negative standard electrode potential because it readily loses electrons and gets oxidised easily. Hence it does not show a positive value.

Manganese (Mn) – Manganese also has a negative electrode potential as it is more reactive and tends to form $Mn^{2+}$ ions easily.

Copper (Cu) – Copper has a positive standard electrode potential. This means copper does not lose electrons easily and is less reactive compared to hydrogen. Therefore, it shows a positive $E^\circ(Cu^{2+}/Cu)$ value.

Zinc (Zn) – Zinc has a negative standard electrode potential because it readily undergoes oxidation to form $Zn^{2+}$.