Ti doesn't exist in +1 oxdn. state as it has 2es- in its 4s orbital which is too few es- to lose or share as compared to other elements in the middle of d block.

Titanium (Ti) doesn't exist in 1 oxidation state:

Introduction:
Titanium (Ti) is a chemical element with the atomic number 22 and belongs to the d-block of the periodic table. It is a transition metal known for its strength, low density, and corrosion resistance. While titanium can exhibit multiple oxidation states, it does not exist in the +1 oxidation state due to various factors.

Explanation:
1. Electronic Configuration:
The electronic configuration of titanium is [Ar] 3d^2 4s^2. In its ground state, titanium has two valence electrons in the 4s orbital and two unpaired electrons in the 3d orbital. The loss of one electron would result in the formation of the +1 oxidation state. However, due to the higher stability associated with a half-filled 3d orbital, titanium prefers to lose all four of its valence electrons and form the +4 oxidation state.

2. Energy Considerations:
The energy required to remove one electron from the 4s orbital is relatively low compared to removing an electron from the 3d orbital. The 4s orbital is further from the nucleus and experiences less shielding from inner electrons, making it easier to remove an electron. As a result, titanium tends to lose its 4s electrons first, leading to the formation of the +2 oxidation state, where it loses both 4s electrons.

3. Stability of +4 Oxidation State:
The +4 oxidation state of titanium is the most stable due to the completely empty 4s and half-filled 3d orbitals. This configuration maximizes the stability of the atom by achieving a lower energy state. The +4 oxidation state allows titanium to form stable compounds with various elements and exhibit its characteristic properties.

Conclusion:
In conclusion, titanium (Ti) does not exist in the +1 oxidation state due to its electronic configuration, energy considerations, and the stability associated with the +4 oxidation state. Understanding the oxidation states of elements is crucial in predicting their chemical behavior and forming compounds with other elements.