Question

The most stable oxidation state of titanium is

• A. \(Ti^{3+}\)
• B. \(Ti^{2+}\)
• C. \(Ti^{4+}\)
• D. \(Ti^{5+}\)

Hint:

Ti(4+) has the stable argon core with no d electrons.

Answer 1

The Correct Option is C

Step 1: Understanding the Concept:
The most stable oxidation state of an early transition metal is usually the one that gives an empty \(d\) subshell. This is a noble gas configuration and is very stable.

Step 2: Titanium:
Titanium has atomic number 22 and configuration \([Ar]\,3d^{2}4s^{2}\). It has four valence electrons.

Step 3: Remove all valence electrons:
Losing all four gives \(Ti^{4+}\) with configuration \([Ar]\). It is the most stable state. Compounds like \(TiO_2\) and \(TiCl_4\) are common.

Step 4: Other options:
\(Ti^{3+}\) has one \(3d\) electron and is easily oxidised to +4. \(Ti^{2+}\) is a strong reducing agent and is rare. \(Ti^{5+}\) would need the removal of an electron from the argon core, so it does not exist.

Final Answer:
The most stable state is +4. \[ \boxed{Ti^{4+}} \]