The correct answer is (3) A-I, B-III, C-II, D-IV.
Let's go through each element in List I and its corresponding information in List II.
A. \(Cr^{3+}\): Chromium (Cr) in the +3 oxidation state means it has lost three electrons. The electron configuration of a neutral chromium atom is \([Ar] 3d^5 4s^1\). When three electrons are removed to form \(Cr^{3+}\), it results in a \(d^3\) configuration.
B. \(Mn^{5+}\): Manganese (Mn) in the +5 oxidation state means it has lost five electrons. The electron configuration of a neutral manganese atom is \([Ar] 3d^5 4s^2\). When five electrons are removed to form \(Mn^{5+}\), it results in a \(d^2\) configuration. In general, species with unpaired electrons are paramagnetic because unpaired electrons create magnetic moments.
C. \(Cu^{+}\): Copper (Cu) in the +1 oxidation state means it has lost one electron. The electron configuration of a neutral copper atom is \([Ar] 3d^9 4s^2\). When one electron is removed to form \(Cu^{+}\), it results in a \(d^{10}\) configuration.
D. \(Ti^{4+}\): Titanium (Ti) in the +4 oxidation state means it has lost four electrons. The electron configuration of a neutral titanium atom is \([Ar] 3d^2 4s^2\). When four electrons are removed to form \(Ti^{4+}\), it results in a \(d^0\) configuration. A \(d^0\) configuration means all the electrons are paired, resulting in no net magnetic moment, making it diamagnetic.
So, the correct match is: 3. A-I, B-III, C-II, D-IV |
