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Chapter 23: Problem 88

Explain why \(\mathrm{Zn}, \mathrm{Cd},\) and \(\mathrm{Hg}\) resemble the group 2 metals in some of their properties.

Short Answer

Expert verified
Zn, Cd, and Hg resemble the group 2 metals in their electron configurations and oxidation states. They have a full inner shell and typically exhibit a +2 oxidation state due to the loss of the two s orbital electrons, much like Group 2 metals.

Step by step solution

01

Understanding Transition Metals

Zn, Cd, and Hg are transition metals. Transition metals are elements whose atoms have an incomplete inner shell. They are characterized by multiple oxidation states.
02

Understanding Group 2 Metals

Group 2 metals, also known as alkaline earth metals, have a full inner shell and exhibit a single oxidation state of +2.
03

Electron Configuration of Zn, Cd, Hg

The electron configuration of Zn, Cd, and Hg indicates that they also have a full inner shell. This is because each of these elements has two electrons in their outermost s orbital. Zn = [Ar] 4s2,3d10; Cd = [Kr] 5s2,4d10; Hg = [Xe] 6s2,4f14,5d10.
04

Comparing with Group 2 Metals

Like the group 2 metals, Zn, Cd and Hg also exhibit a single +2 oxidation state. This +2 state arises from the loss of the two s orbital electrons present in their ground state. This implies that they exhibit similar chemical behavior to group 2 metals.
05

Conclusion

Therefore, Zn, Cd and Hg resemble the Group 2 metals in some of their properties because of their electron configuration. They have a full inner shell and exhibit an oxidation state of +2 due to the loss of the two s orbital electrons, much like Group 2 metals.

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