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Chapter 20: Problem 2

Why is zinc not considered a transition metal?

Short Answer

Expert verified
Zinc isn't considered a transition metal because its common ion, Zn^2+, has a fully-filled d orbital, and zinc usually forms compounds with only a +2 oxidation state, unlike typical transition metals.

Step by step solution

01

Define Transition Metals

Transition metals are chemical elements that are found in the middle of the periodic table, specifically in Groups 3-12. They have two main properties: they form at least one ion with a partially-filled d orbital, and they have multiple oxidation states.
02

Analyze Zinc's Properties

Zinc, symbol Zn, is an element in Group 12 of the periodic table. It forms a common ion, Zn^2+, which has a completely filled d orbital (3d10). In terms of oxidation states, zinc generally has only +2 oxidation state in its compounds.
03

Compare Zinc to Transition Metals

In comparing zinc to the defined characteristics of transition metals, it becomes clear that zinc does not meet the two crucial properties. Zinc's common ion doesn't have a partially-filled d orbital and it has only one usual oxidation state, unlike transition metals that display multiple oxidation states.

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Most popular questions from this chapter

Give the oxidation numbers of the metals in these species: (a) \(\mathrm{K}_{3}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]\) (b) \(\mathrm{K}_{3}\left[\mathrm{Cr}\left(\mathrm{C}_{2} \mathrm{O}_{4}\right)_{3}\right]\) (c) \(\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{2-}\)

Why do transition metals have more oxidation states than other elements? Give the highest oxidation states for scandium to copper.

In a dilute nitric acid solution, \(\mathrm{Fe}^{3+}\) reacts with thiocyanate ion \(\left(\mathrm{SCN}^{-}\right)\) to form a dark-red complex: $$\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+}+\mathrm{SCN}^{-} \rightleftharpoons \mathrm{H}_{2} \mathrm{O}+\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{5} \mathrm{NCS}\right]^{2+}$$ The equilibrium concentration of \(\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{5} \mathrm{NCS}\right]^{2+}\) may be determined by how darkly colored the solution is (measured by a spectrometer). In one such experiment, \(1.0 \mathrm{~mL}\) of \(0.20 \mathrm{M} \mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{3}\) was mixed with \(1.0 \mathrm{~mL}\) of \(1.0 \times 10^{-3} M \mathrm{KSCN}\) and \(8.0 \mathrm{~mL}\) of dilute \(\mathrm{HNO}_{3}\). The color of the solution quantitatively indicated that the \(\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{5} \mathrm{NCS}\right]^{2+}\) concentration was \(7.3 \times 10^{-5} M\). Calculate the formation constant for \(\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{5} \mathrm{NCS}\right]^{2+}\)

Without referring to the text, write the ground-state electron configurations of the first-row transition metals. Explain any irregularities.

Explain why a thermodynamically stable species may be chemically reactive and a thermodynamically unstable species may be unreactive.
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