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Chapter 6: Problem 21

What is the difference between a transition state and an intermediate?

Short Answer

Expert verified
Transition states are high-energy, unstable points, while intermediates are more stable, isolatable species with finite lifetimes during a reaction.

Step by step solution

01

Define Transition State

A transition state is a high-energy, unstable arrangement of atoms that occurs during a chemical reaction. It represents a point along the reaction pathway at which bonds are in the process of breaking and forming, and it cannot be isolated or observed directly.
02

Define Intermediate

An intermediate is a relatively stable species formed during the transformation from reactants to products in a chemical reaction. Intermediates have finite lifetimes, can be isolated in some cases, and exist in energy valleys between transition states.
03

Compare Stability

Transition states are higher in energy and less stable than intermediates. While transition states exist momentarily at the peak of the energy barrier, intermediates occupy valleys, making them more stable, although possibly short-lived.
04

Existence and Observation

A transition state cannot be isolated or observed because it exists momentarily at the highest energy point. Conversely, an intermediate has a finite lifetime and, in some reactions, can be detected or isolated using advanced techniques.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Transition State
In the realm of chemical reactions, the transition state is a crucial concept. It represents a fleeting moment during a reaction when reactants are transformed into products. This state is extremely high in energy and very unstable. Think of it as the summit of a mountain, where neither the path up nor down lies but rather a critical point in-between.
The transition state exists only for a fraction of a second as bonds are in the process of breaking and forming. This transitory nature explains why it's not possible to directly observe or isolate a transition state. Its fleeting existence makes it a theoretical construct rather than an entity we can capture and study directly. Scientists often use tools like computational chemistry to predict and model this energetic peak.
  • High energy
  • Very unstable
  • Represents a peak in the reaction pathway
  • Cannot be isolated
Reaction Intermediate
Unlike the transition state, a reaction intermediate is a more tangible concept in chemical reactions. It is a stable species that forms between the initial reactants and the final products during a reaction. Consider it a temporary rest stop on a journey from start to finish.
Intermediates have a definitive, albeit usually short, lifetime and can sometimes be isolated or detected, thanks to advancements in analytical techniques. They reside in energy valleys between the peaks of transition states, making them more stable than those fleeting transition states.
  • Relatively stable
  • Can be isolated in some cases
  • Exists in energy valleys
  • Finite lifetime
Energy Barrier
The energy barrier is the obstacle that reactants must overcome to convert into products during a chemical reaction. It represents the energy required to reach the peak of the transition state from the reactants.
Imagine riding a bike up a hill where the top of the hill symbolizes the transition state, and the energy barrier is the effort it takes to get there. The height of this energy hill determines the speed of the reaction; the lower the barrier, the faster the reaction.
The concept of the energy barrier helps to explain why some reactions happen quickly while others are slow. It sets the pace for how efficiently a reaction can proceed from reactants to products.
  • Energy required to reach the transition state
  • Influences reaction speed
  • Key factor in reaction mechanisms

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Most popular questions from this chapter

Despite the limitations of radical chlorination of alkanes, the reaction is still useful for synthesizing certain halogenated compounds. For which of the following compounds does radical chlorination give a single monochloro product?

A The reaction of hydroxide ion with chloromethane to yield methanol and chloride ion is an example of a general reaction type called a nucleophilic substitution reaction: $$ \mathrm{HO}^{-}+\mathrm{CH}_{3} \mathrm{Cl} \rightleftarrows \mathrm{CH}_{3} \mathrm{OH}+\mathrm{Cl}^{-} $$ The value of \(\Delta H^{\circ}\) for the reaction is \(-75 \mathrm{~kJ} / \mathrm{mol}\), and the value of \(\Delta S^{\circ}\) is \(+54 \mathrm{~J} /(\mathrm{K} \cdot \mathrm{mol})\). What is the value of \(\Delta G^{\circ}\) (in \(\mathrm{kJ} / \mathrm{mol}\) ) at \(298 \mathrm{~K} ?\) Is the reac- tion exothermic or endothermic? Is it exergonic or endergonic?

Which reaction is more energetically favored, one with \(\Delta G^{\circ}=-44 \mathrm{~kJ} / \mathrm{mol}\) or one with \(\Delta G^{\circ}=+44 \mathrm{~kJ} / \mathrm{mol}\) ?

When a mixture of methane and chlorine is irradiated, reaction commences immediately. When irradiation is stopped, the reaction gradually slows down but does not stop immediately. Explain.

Draw the structures of the two carbocation intermediates that might form during the reaction of 2 -methylpropene with \(\mathrm{H}_{3} \mathrm{O}^{+}\) (Problem \(6.39\) ). We'll see in the next chapter that the stability of carbocations depends on the number of alkyl substituents attached to the positively charged carbon-the more alkyl substituents there are, the more stable the cation. Which of the two carbocation intermediates you drew is more stable?
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