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Chapter 23: Problem 81

The only diamagnetic ion of the following group is (a) \(\mathrm{Cr}^{2+} ;\) (b) \(\mathrm{Zn}^{2+} ;\) (c) \(\mathrm{Fe}^{3+} ;\) (d) \(\mathrm{Ag}^{2+} ;\) (e) \(\mathrm{Ti}^{3+}\).

Short Answer

Expert verified
The only diamagnetic ion out of the given groups is \(\mathrm{Zn}^{2+}\)

Step by step solution

01

Understand the electronic configuration of Ions

Know the electronic configuration of given ions. An ion is diamagnetic if it does not have any unpaired electrons in its outer shell. Thus, we have to identify the ion with all paired electrons.
02

Analyze each given ion

Analyze each ion: Chromium ion \(\mathrm{Cr}^{2+}\) has configuration [Ar] 3d4. Zinc ion \(\mathrm{Zn}^{2+}\) has configuration [Ar] 3d10. Iron ion \(\mathrm{Fe}^{3+}\) has configuration [Ar] 3d5. Silver ion \(\mathrm{Ag}^{2+}\) has configuration [Kr] 4d8. Titanium ion \(\mathrm{Ti}^{3+}\) has configuration [Ar] 3d1.
03

Identify the diamagnetic ion

From the configurations given above, only zinc ion \(\mathrm{Zn}^{2+}\) has all paired electrons. It has no unpaired electrons in its outer shell. Therefore, out of the given ions, \(\mathrm{Zn}^{2+}\) is diamagnetic.

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Most popular questions from this chapter

Three properties expected for transition elements are (a) low melting points; (b) high ionization energies; (c) colored ions in solution; (d) positive standard electrode (reduction) potentials; (e) diamagnetism; (f) complex ion formation; (g) catalytic activity.

Although Au reacts with and dissolves in aqua regia (3 parts \(\mathrm{HCl}+1\) part \(\mathrm{HNO}_{3}\) ), Ag does not dissolve. What is (are) the likely reason(s) for this difference?

Explain why gold dissolves in aqua regia but not in \(\mathrm{HNO}_{3}(\mathrm{aq})\).

Which of the first transition series elements exhibits the greatest number of different oxidation states in its compounds? Explain.

Covalent bonding is involved in many transition metal compounds. Draw Lewis structures, showing any nonzero formal charges, for the following molecules or ions: (a) \(\mathrm{Hg}_{2}^{2+} ;\) (b) \(\mathrm{Mn}_{2} \mathrm{O}_{7} ;\) (c) \(\mathrm{OsO}_{4}\). [Hint: In (b), there is one \(\mathrm{Mn}-\mathrm{O}-\text { Mn linkage in the molecule. }\rfloor\)
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