The common oxidation states of Ti are
(a)`+2, +3`
(b)`+3, +4`
(c)`3,-4`
(d)`+2,+3,+4`

Options

A. `+2, +3`
B. `+3, +4`
C. `3,-4`
D. `+2,+3,+4`

Explanation

To determine the common oxidation states of titanium (Ti), we will analyze its electronic configuration and the stability of its oxidation states.

### Step-by-Step Solution:

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

2. **Determine Possible Oxidation States**:
- Titanium can lose electrons from both the 4s and 3d orbitals.
- The common oxidation states arise from the loss of these electrons.

3. **Common Oxidation States**:
- **+4 Oxidation State**:
- When titanium loses all four electrons (2 from 4s and 2 from 3d), it achieves the configuration of the noble gas Argon:
\[ \text{Ti}^{4+}: [\text{Ar}] 3d^0 4s^0 \]
- **+3 Oxidation State**:
- When titanium loses three electrons (2 from 4s and 1 from 3d), it has the configuration:
\[ \text{Ti}^{3+}: [\text{Ar}] 3d^1 \]
- **+2 Oxidation State**:
- When titanium loses two electrons (2 from 4s), it results in:
\[ \text{Ti}^{2+}: [\text{Ar}] 3d^2 \]
- This state is less stable due to the presence of unpaired electrons in the 3d subshell.

4. **Conclusion**:
- The most stable oxidation states of titanium are +3 and +4, while +2 is also possible but less common.
- Therefore, the common oxidation states of titanium are:
\[ \text{Answer: (d) +2, +3, +4} \]