Why `Ti^(+4)` complex are diamagnetic?

Answer

To understand why \( \text{Ti}^{+4} \) complexes are diamagnetic, we can follow these steps:

### Step 1: Determine the Atomic Number and Electronic Configuration of Titanium
Titanium has an atomic number of 22. Its electronic configuration is:
\[ \text{Ti}: [\text{Ar}] 3d^2 4s^2 \]

### Step 2: Identify the Oxidation State
In the question, we are considering the titanium ion in the +4 oxidation state, denoted as \( \text{Ti}^{+4} \).

### Step 3: Remove Electrons for the Oxidation State
To achieve the +4 oxidation state, titanium must lose a total of 4 electrons. The electrons are removed first from the 4s subshell and then from the 3d subshell:
\[ \text{Ti}^{+4}: 3d^0 4s^0 \]

### Step 4: Analyze the Electron Configuration
After losing 4 electrons, the electron configuration of \( \text{Ti}^{+4} \) shows that there are no electrons left in the 3d or 4s subshells:
\[ \text{Ti}^{+4}: 3d^0 4s^0 \]

### Step 5: Determine the Presence of Unpaired Electrons
Since there are no electrons in the 3d or 4s subshells, there are no unpaired electrons in \( \text{Ti}^{+4} \).

### Step 6: Conclude the Magnetic Properties
A substance is classified as diamagnetic if it has no unpaired electrons. Since \( \text{Ti}^{+4} \) has no unpaired electrons, it is diamagnetic. Therefore, the magnetic moment is equal to zero:
\[ \text{Magnetic Moment} = 0 \quad \Rightarrow \quad \text{Diamagnetic} \]

### Final Conclusion
Thus, \( \text{Ti}^{+4} \) complexes are diamagnetic because they do not contain any unpaired electrons.

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