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Chapter 20: Problem 34

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

Short Answer

Expert verified
A thermodynamically stable species may still be chemically reactive due to stored potential energy that can trigger a reaction when the activation energy threshold is surpassed. Conversely, a thermodynamically unstable species might not react because, despite being in high energy state, the activation energy barrier may be too high to be surpassed with the available energy, or the species may be sterically hindered.

Step by step solution

01

Define Thermodynamic Stability

Firstly, clarify what is meant by a thermodynamically stable species. A substance is considered thermodynamically stable if its formation from its elements is associated with the release of energy (exothermic process), or if its entropy is high. The concept is linked to the law of minimum energy where systems strive to reach a state of minimal energy.
02

Define Chemical Reactivity

Now define chemical reactivity. Chemical reactivity is the tendency of a substance to undergo a chemical change. This usually involves the making or breaking of bond structures and is influenced by factors such as temperature, concentration and the presence of a catalyst.
03

Explain why a thermodynamically stable species can be chemically reactive

Thermodynamically stable species can still be chemically reactive due to the concept of activation energy. Even though a species is in a stable state, it can still have potential energy stored in its bonds. This energy can be released when the substance comes into contact with another substance, provided that the activation energy is surpassed, leading to a reaction.
04

Define Thermodynamic Instability

A thermodynamically unstable species, on the other hand, is a species that has high energy or low entropy. It is not at its lowest possible energy state, and so, in theory, it should react to go towards a lower energy state.
05

Explain why a thermodynamically unstable species may be unreactive

Despite being thermodynamically unstable, a species may be unreactive due to kinetic factors. The activation energy barrier may be much higher than the available energy, preventing the species from reacting. A substance can also be sterically hindered, preventing other reactants from accessing the reactive site.

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Most popular questions from this chapter

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

Write the electron configurations of these ions: \(\mathrm{V}^{5+}\) \(\mathrm{Cr}^{3+}, \mathrm{Mn}^{2+}, \mathrm{Fe}^{3+}, \mathrm{Cu}^{2+}, \mathrm{Sc}^{3+}, \mathrm{T}_{1}^{4+}\)

A student prepared a cobalt complex that has one of the following structures: \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}\right] \mathrm{Cl}_{3}\), \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{5} \mathrm{Cl}\right] \mathrm{Cl}_{2},\) or \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}_{2}\right] \mathrm{Cl} .\) Explain how the student would distinguish among these possibilities by an electrical conductance experiment. At the student's disposal are three strong electrolytes: \(\mathrm{NaCl}, \mathrm{MgCl}_{2},\) and \(\mathrm{FeCl}_{3},\) which may be used for comparison purposes.

Copper is also known to exist in +3 oxidation state, which is believed to be involved in some biological electron transfer reactions. (a) Would you expect this oxidation state of copper to be stable? Explain. (b) Name the compound \(\mathrm{K}_{3} \mathrm{CuF}_{6}\) and predict the geometry of the complex ion and its magnetic properties. (c) Most of the known Cu(III) compounds have square planar geometry. Are these compounds diamagnetic or paramagnetic?

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) \(\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{2-}\)
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