Among the following series of transition metal ions, the one...

Among the following series of transition metal ions, the one where all metal ions have same $3 d$ electronic configuration is: (a) $\mathrm{Ti}^{2+}, \mathrm{V}^{3+}, \mathrm{Cr}^{4+}, \mathrm{Mn}^{5+}$ (b) $\mathrm{Ti}^{3+}, \mathrm{V}^{2+}, \mathrm{Cr}^{3+}, \mathrm{Mn}^{4+}$ (c) $\mathrm{Ti}^{+}, \mathrm{V}^{4+}, \mathrm{Cr}^{6+}, \mathrm{Mn}^{7+}$ (d) $\mathrm{Ti}^{4+}, \mathrm{V}^{3+}, \mathrm{Cr}^{2+}, \mathrm{Mn}^{3+}$

Among the following series of transition metal ions, the one where all metal ions have same $3 d$ electronic configuration is:
(a) $\mathrm{Ti}^{2+}, \mathrm{V}^{3+}, \mathrm{Cr}^{4+}, \mathrm{Mn}^{5+}$
(b) $\mathrm{Ti}^{3+}, \mathrm{V}^{2+}, \mathrm{Cr}^{3+}, \mathrm{Mn}^{4+}$
(c) $\mathrm{Ti}^{+}, \mathrm{V}^{4+}, \mathrm{Cr}^{6+}, \mathrm{Mn}^{7+}$
(d) $\mathrm{Ti}^{4+}, \mathrm{V}^{3+}, \mathrm{Cr}^{2+}, \mathrm{Mn}^{3+}$

Key Concepts

Oxidation State and Electron Count

The oxidation state of a transition metal ion indicates the number of electrons that have been removed from its neutral atom. By using the known electron configuration of the neutral atom, one can calculate the remaining electrons in the 3d orbitals after accounting for the electrons lost due to oxidation, which is essential for comparing different ions.

Isoelectronic Species

Isoelectronic species are atoms or ions that have the same number of electrons and, consequently, the same electronic configuration. In the context of transition metal ions, identifying a series where all ions have the same 3d electron count involves determining which ions, despite differing oxidation states, share an identical configuration in their 3d orbitals.

Transition Metal Ions

Transition metal ions are formed when neutral transition metal atoms lose electrons, often resulting in a variety of oxidation states. Their partially filled d orbitals are crucial in determining their chemical properties and reactivity. Understanding these ions requires considering how electrons are removed, particularly from the s and then the d orbitals, which affects their electronic configuration.

Electronic Configuration of Transition Metals

The electronic configuration of transition metals typically involves the 3d and 4s orbitals. When these metals lose electrons to form ions, electrons are generally removed first from the 4s orbital followed by the 3d orbitals. This pattern is critical to determining the number of electrons present in the 3d subshell of various ions.

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