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Most transition metals display several oxidation states, yet zinc shows essentially only one. The reason zinc does not exhibit variable oxidation states is:

1. completely filled np-orbitals
2. completely filled (n-1)d orbitals
3. completely filled ns-orbitals
4. the inert pair effect

Correct answer: completely filled (n-1)d orbitals

Solution

Zinc has a completely filled 3d10 subshell, so its d-electrons are not available for bonding; it only loses the two 4s electrons to give +2.

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