Question

Identify the oxidation states of titanium (Z = 22) and copper (Z = 29) in their colourless compounds.

• A. $T{i}^{3+},C{u}^{2+}$
• B. $T{i}^{2+},C{u}^{2+}$
• C. $T{i}^{4+},C{u}^{1+}$
• D. $T{i}^{4+},C{u}^{2+}$

Answer 1

Answer: (C)

Electronic configuration of titanium $(Ti)(Z=22)$ is $[Ar{]}_{18}3d^{2}4s^2.$ In case of $T{i}^{4+}$, the electronic configuration will be $[Ar{]}_{18}3d^{0}4s^0$

Similarly, electronic configuration of copper $(Cu)(Z=29)$ is $[Ar{]}_{18}3d^{10}4s^1$ On loosing one electron it acquires stable electronic configuration, i.e $[Ar{]}_{18}3d^{10}$

In both $T{i}^{4+}$ and $C{u}^{+}$ no unpaired electron is present. As a result, no $d-d$ transition occur and therefore these are colourless in nature.