A) one unpaired \[{{e}^{-}}\]
B) Two unpaired \[{{e}^{-}}\]
C) three unpaired \[{{e}^{-}}\]
D) no unpaired \[{{e}^{-}}\]
Correct Answer: A
Solution :
Electronic configuration of Ti (atomic number \[=22\]) is: \[1{{s}^{2}},2{{s}^{2}}2{{p}^{6}},3{{s}^{2}}3{{p}^{6}}3{{d}^{2}},4{{s}^{2}}\]. In \[{{[Ti{{({{H}_{2}}O)}_{6}}]}^{+3}}\], Titanium is present in trivalent oxidation state i.e., \[T{{i}^{+3}},\]which is formed by the loss of \[2{{e}^{-}}s\] from \[4s\] orbital and one electron from \[3d\] orbital. Hence \[T{{i}^{+3}}\] ion contains one unpaired electron in \[3d\] orbital hence it is paramagnetic.
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