State true or false :
`3d^0 4s^0` electronic configuration exhibits by `Ti^(+4)`

Explanation

To determine whether the statement regarding the electronic configuration of \( \text{Ti}^{+4} \) being \( 3d^0 \, 4s^0 \) is true or false, we can follow these steps:

### Step 1: Identify the Atomic Number of Titanium
- Titanium (Ti) has an atomic number of 22.

### Step 2: Write the Ground State Electronic Configuration of Titanium
- The ground state electronic configuration of titanium can be written as:
\[ \text{Ti: } [\text{Ar}] \, 3d^2 \, 4s^2 \]
where [Ar] represents the electron configuration of Argon, which accounts for the first 18 electrons.

### Step 3: Determine the Configuration for \( \text{Ti}^{+4} \)
- When titanium is in the \( +4 \) oxidation state, it loses 4 electrons.
- The electrons are removed first from the 4s orbital and then from the 3d orbital.

### Step 4: Remove Electrons from the Configuration
- Removing 2 electrons from the \( 4s^2 \) gives \( 4s^0 \).
- Removing 2 electrons from the \( 3d^2 \) gives \( 3d^0 \).

### Step 5: Write the Final Configuration for \( \text{Ti}^{+4} \)
- Therefore, the electronic configuration for \( \text{Ti}^{+4} \) is:
\[ \text{Ti}^{+4}: [\text{Ar}] \, 3d^0 \, 4s^0 \]

### Conclusion
- Since the electronic configuration of \( \text{Ti}^{+4} \) is indeed \( 3d^0 \, 4s^0 \), the statement is **True**.

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