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Chapter 20: Problem 7

As we read across the first-row transition metals from left to right, the +2 oxidation state becomes more stable in comparison with the +3 state. Why is this so?

Short Answer

Expert verified
+2 oxidation state becomes more stable than the +3 state in transition metals as we move across the period, because the removal of one more electron to reach +3 state disrupts the stable half-filled or completely filled d-orbital configuration created in the +2 state.

Step by step solution

01

Understanding Transition Metal Atomic Structures

In transition metals, 4s orbital is filled before the 3d orbitals. The 4s and 3d orbitals are quite close in energy. When moving across the period, electrons are added one at a time to the 3d orbital.
02

Explaining the Stability of +2 Oxidation State

When the transition metal is oxidized to a +2 state, the two 4s electrons are lost. This results in a more stable half-filled or completely filled d-orbital configuration which lower energy state and hence more stable.
03

Comparing +2 and +3 Oxidation States

When the metal is further oxidized to the +3 state, one of the 3d electrons is removed. This disrupts the lower energy, more stable half-filled or completely filled d-orbital configuration, making the +2 oxidation state more stable than the +3 state.

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