Understanding Transition Metal Oxidation States

This question asks us to match specific transition metals from List I with their maximum common oxidation states provided in List II. Transition metals are known for exhibiting variable oxidation states, primarily due to the participation of their (n-1)d and ns electrons in bonding.

To solve this, let's determine the maximum common oxidation state for each metal listed:

Analyzing Each Transition Metal and Its Maximum Oxidation State

• A. Ti (Titanium): Titanium is in Group 4. Its electronic configuration is \([Ar] 3d^2 4s^2\). It can lose its two 4s electrons and up to two 3d electrons. The maximum oxidation state typically observed for Titanium is +4 (losing all 4 valence electrons).
• B. V (Vanadium): Vanadium is in Group 5. Its electronic configuration is \([Ar] 3d^3 4s^2\). It can lose its two 4s electrons and up to three 3d electrons. The maximum oxidation state observed for Vanadium is +5 (losing all 5 valence electrons).
• C. Mn (Manganese): Manganese is in Group 7. Its electronic configuration is \([Ar] 3d^5 4s^2\). It can lose its two 4s electrons and up to five 3d electrons. The maximum oxidation state observed for Manganese is +7 (losing all 7 valence electrons), for example in permanganate (\(\text{MnO}_4^-\)).
• D. Cu (Copper): Copper is in Group 11. Its electronic configuration is \([Ar] 3d^{10} 4s^1\). Common oxidation states are +1 (losing the 4s electron) and +2 (losing the 4s electron and one 3d electron). While higher oxidation states are possible under specific conditions, the maximum common oxidation state is +2.

Now let's look at the oxidation states given in List II:

• I. 7
• II. 4
• III. 5
• IV. 2

Matching List I and List II

Based on our analysis of the maximum oxidation states:

• Titanium (Ti) has a maximum oxidation state of +4. This matches List II item II.
• Vanadium (V) has a maximum oxidation state of +5. This matches List II item III.
• Manganese (Mn) has a maximum oxidation state of +7. This matches List II item I.
• Copper (Cu) has a maximum common oxidation state of +2. This matches List II item IV.

Detailed Matching

This gives us the matching sequence: A - II, B - III, C - I, D - IV.

Revision Table: Transition Metals and Oxidation States

Additional Information: Oxidation States of Transition Metals

Transition metals typically exhibit multiple oxidation states because the energy difference between the (n-1)d and ns orbitals is small. This allows electrons from both subshells to be involved in bonding.

The maximum oxidation state for the first row transition metals generally increases from Scandium (Sc, +3) up to Manganese (Mn, +7), where all the 4s and 3d electrons can participate in bonding. After Manganese, the maximum oxidation state tends to decrease or become less common, as the 3d electrons become more tightly held and pairing occurs. For example, Iron (Fe) commonly shows +2 and +3, Cobalt (Co) +2 and +3, Nickel (Ni) +2, Copper (Cu) +1 and +2, and Zinc (Zn) only +2.

The stability of different oxidation states varies depending on the specific metal and the ligands or counterions present.