Question

Identify the incorrect statement.

• A. Ability of Fluorine to stabilise higher oxidation states in transition metals is due to the low lattice enthalpy of the fluorides.
• B. The second and third ionisation enthalpies of Mn$^{2+}$ and Fe$^{3+}$ respectively have lower values than expecte(D)
• C. Transition metals readily form alloys because their metallic radii are within about 15% of each other.
• D. C$^{2+}$ acts as reducing agent while Mn$^{2+}$ acts as an oxidising agent though both the ions have d\^4 configuration.

Hint:

In transition metal 6256d60dc6a8bca7110c99d1, the stability of higher oxidation states is largely influenced by the metal's electronegativity and the ligand's ability to stabilize these states, rather than by the lattice enthalpy.

Answer 1

The Correct Option is A

- Statement (A) is incorrect. The ability of Fluorine to stabilize higher oxidation states in transition metals is not due to the low lattice enthalpy of fluorides. In fact, it is primarily because Fluorine has a high electronegativity, which allows it to effectively stabilize the metal in higher oxidation states by accepting electrons. The low lattice enthalpy of fluorides does not directly contribute to this stabilization. - Statement (B) is correct. The second and third ionisation enthalpies of Mn$^{2+}$ and Fe$^{3+}$ are indeed lower than expected because of the stability of the d$^5$ and d$^10$ electron configurations in Mn$^{2+}$ and Fe$^{3+}$ ions respectively. - Statement (C) is correct. Transition metals tend to form alloys because their metallic radii are similar, typically within about 15% of each other, which allows for easy mixing and formation of solid solutions. - Statement (D) is correct. C$^{2+}$ acts as a reducing agent, while Mn$^{2+}$ acts as an oxidizing agent despite both having a d$^4$ configuration because of their respective positions and behavior in redox reactions.