Textbook Question
Show how you might synthesize the following compounds starting with bromobenzene, and alkyl or alkenyl halides of four carbon atoms or fewer.
c. dec-5-ene
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16. Conjugated Systems
Allylic Halogenation
7:37 minutesProblem 8a,b,c
Textbook Question
When Br2 is added to buta-1,3-diene at –15 °C, the product mixture contains 60% of product A and 40% of product B. When the same reaction takes place at 60 °C, the product ratio is 10% A and 90% B.
a. Propose structures for products A and B. (Hint: In many cases, an allylic carbocation is more stable than a bromonium ion.)
b. Propose a mechanism to account for formation of both A and B.
c. Show why A predominates at –15 °C and B predominates at 60 °C.
Verified step by step guidance1
Step 1: Analyze the reaction conditions and the hint provided. The reaction involves buta-1,3-diene and Br2, which suggests an electrophilic addition mechanism. The hint about allylic carbocations being more stable than bromonium ions indicates that resonance stabilization plays a key role in the formation of products.
Step 2: Propose structures for products A and B. Begin by considering the electrophilic addition of Br2 to buta-1,3-diene. The intermediate formed is likely a resonance-stabilized allylic carbocation. Product A is likely the 1,2-addition product (bromine adds to adjacent carbons), while product B is likely the 1,4-addition product (bromine adds to carbons separated by one double bond). Draw the structures of both products based on these addition patterns.
Step 3: Propose a mechanism for the formation of both A and B. Start with the attack of Br2 on the π-electrons of buta-1,3-diene, forming a bromonium ion or a resonance-stabilized allylic carbocation. Show how the intermediate rearranges to allow for 1,2-addition (leading to product A) and 1,4-addition (leading to product B). Use resonance structures to explain the stability of the intermediate and the formation of both products.
Step 4: Explain why product A predominates at -15 °C and product B predominates at 60 °C. At lower temperatures (-15 °C), the reaction is under kinetic control, favoring the formation of the product that forms faster (product A, 1,2-addition). At higher temperatures (60 °C), the reaction is under thermodynamic control, favoring the more stable product (product B, 1,4-addition). Discuss the energy barriers and stability of the products to support this explanation.
Step 5: Summarize the key concepts involved in this problem: electrophilic addition to conjugated dienes, resonance stabilization of intermediates, and the distinction between kinetic and thermodynamic control. Highlight how temperature influences the product distribution and the importance of understanding reaction mechanisms in organic chemistry.
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Video duration:
7mKey Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Electrophilic Addition Reactions
Electrophilic addition reactions involve the addition of an electrophile to a nucleophile, typically across a double bond. In the case of buta-1,3-diene reacting with Br2, the double bond acts as a nucleophile, attacking the electrophilic bromine. This reaction can lead to the formation of different products depending on the stability of intermediates formed during the process.
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Stability of Carbocations
Carbocations are positively charged carbon species that can form during reactions involving alkenes. Their stability is influenced by factors such as the degree of substitution (primary, secondary, tertiary) and resonance. In this reaction, the hint suggests that an allylic carbocation, which is stabilized by resonance with adjacent double bonds, may be more stable than the bromonium ion intermediate, affecting the product distribution.
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Temperature Effects on Reaction Mechanisms
Temperature can significantly influence the outcome of chemical reactions by affecting the kinetics and thermodynamics of the process. At lower temperatures, reactions may favor pathways that lead to more stable intermediates, resulting in a higher yield of product A. Conversely, at higher temperatures, the reaction may favor the formation of product B due to increased energy allowing for less stable intermediates to form, thus altering the product distribution.
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