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Chapter 20: Problem 10

Describe the interaction between a donor atom and a metal atom in terms of a Lewis acid-base reaction.

Short Answer

Expert verified
A donor atom, which is a Lewis base, donates a pair of nonbonding electrons to the metal atom, acting as a Lewis acid, which accepts the electron pair. This results in a Lewis acid-base complex.

Step by step solution

01

Defining Lewis Acid and Lewis Base

Lewis Acids and Bases are defined contrary to the traditional acidic and basic substances. A Lewis base is any substance, such as the OH- ion, that can donate a pair of nonbonding electrons. A Lewis acid is any substance, like the H+ ion, that can accept a pair of nonbonding electrons.
02

Identifying the Donor Atom

According to the Lewis base definition given in step 1, a donor atom must be a Lewis base. This is because Lewis bases are known to donate a pair of nonbonding electrons.
03

Identifying the Metal Atom

The metal atom in this interaction would be considered as a Lewis acid. This is because metals have few valence electrons and have the capacity to accept additional electron pairs from a base.
04

Describing the Interaction

In terms of a Lewis acid-base reaction, a donor atom (Lewis base) donates a pair of nonbonding electrons, which are accepted by the metal atom (Lewis acid). This results in the creation of a Lewis acid-base complex.

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Most popular questions from this chapter

Explain these facts: (a) Copper and iron have several oxidation states, whereas zinc exists in only one. (b) Copper and iron form colored ions, whereas zinc does not

The formation constant for the reaction \(\mathrm{Ag}^{+}+\) \(2 \mathrm{NH}_{3} \rightleftharpoons\left[\mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}\right]^{+}\) is \(1.5 \times 10^{7}\) and that for the reaction \(\mathrm{Ag}^{+}+2 \mathrm{CN}^{-} \rightleftharpoons\left[\mathrm{Ag}(\mathrm{CN})_{2}\right]^{-}\) is 1.0 \(\times 10^{21}\) at \(25^{\circ} \mathrm{C}\) (see Table 17.4 ). Calculate the equilibrium constant at \(25^{\circ} \mathrm{C}\) for the reaction $$\left[\mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}\right]^{+}+2 \mathrm{CN}^{-} \rightleftharpoons\left[\mathrm{Ag}(\mathrm{CN})_{2}\right]^{-}+2 \mathrm{NH}_{3}$$

How many geometric isomers are in these species: (a) \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{2} \mathrm{Cl}_{4}\right]^{-},(\mathrm{b})\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{3} \mathrm{Cl}_{3}\right] ?\)

Aqueous copper(II) sulfate solution is blue in color. When aqueous potassium fluoride is added, a green precipitate is formed. When aqueous potassium chloride is added instead, a bright-green solution is formed. Explain what is happening in these two cases.

The complex ion \(\left[\mathrm{Ni}(\mathrm{CN})_{2} \mathrm{Br}_{2}\right]^{2-}\) has a square planar geometry. Draw the structures of the geometric isomers of this complex.
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