Chemistry
Grade-9
Easy
Question
Among the following series of transition metal ions, the one where all metal ions have 3d2 electronic
configuration is [At. Nos. Ti = 22, V = 23, Cr = 24, Mn = 25]
- Ti3+, V2+, Cr3+, Mn4+
- Ti+, V4+, Cr6+, Mn7+
- Ti4+, V3+, Cr2+, Mn3+
- Ti2+, V3+, Cr4+, Mn5+
Hint:
D-block elements are also called transition metals. In transition elements, the valence electrons are present in the d-orbital. We have to know the electronic configuration of the given metal atoms. The positive charge on the transition metal ion indicated the number of electrons lost by the respective transition metal atom.
The correct answer is: Ti2+, V3+, Cr4+, Mn5+
The correct answer is Ti2+, V3+, Cr4+, Mn5+
The electronic configuration of Titanium is [Ar]3d24s2. This means to get the electronic configuration of 
, titanium has to lose two electrons.
After losing two electrons from the 4s orbital and one electron from the 3d orbital Vanadium will get a 3d2 electronic configuration. So, V3+ has a 3d2 electronic configuration.
The electronic configuration of Chromium is [Ar]3d54s1. This means to get the electronic configuration of 3d2, Chromium has to lose four electrons
After losing three electrons from the 3d orbital and two electrons from the 4s orbital Manganese will get a 3d2 electronic configuration. So, Mn5+ has a 3d2 electronic configuration.
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