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Carbon-carbon double bonds do not freely rotate like carbon-carbon single bonds. Why? OA) Overlap of the sp2 orbitals of the carbon-carbon o bond would be lost. B) The shorter bond length of the double bond makes it more difficult for the attached groups to pass each other. C) The shorter bond length of the double bond makes it more difficult for the attached groups to pass each other. D) Overlap of the two 2p orbitals of the p bond would be lost, i.e. the p bond would be broken.

Carbon-carbon double bonds do not freely rotate like carbon-carbon single bonds. Why? OA) Overlap of the sp2 orbitals of the carbon-carbon o bond would be lost. B) The shorter bond length of the double bond makes it more difficult for the attached groups to pass each other. C) The shorter bond length of the double bond makes it more difficult for the attached groups to pass each other. D) Overlap of the two 2p orbitals of the p bond would be lost, i.e. the p bond would be broken.

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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**Carbon-carbon double bonds do not freely rotate like carbon-carbon single bonds. Why?** - **A)** Overlap of the sp2 orbitals of the carbon-carbon σ bond would be lost. - **B)** The shorter bond length of the double bond makes it more difficult for the attached groups to pass each other. - **C)** The shorter bond length of the double bond makes it more difficult for the attached groups to pass each other. *(Selected option)* - **D)** Overlap of the two 2p orbitals of the π bond would be lost, i.e. the π bond would be broken.
Transcribed Image Text:**Carbon-carbon double bonds do not freely rotate like carbon-carbon single bonds. Why?** - **A)** Overlap of the sp2 orbitals of the carbon-carbon σ bond would be lost. - **B)** The shorter bond length of the double bond makes it more difficult for the attached groups to pass each other. - **C)** The shorter bond length of the double bond makes it more difficult for the attached groups to pass each other. *(Selected option)* - **D)** Overlap of the two 2p orbitals of the π bond would be lost, i.e. the π bond would be broken.
**Question:** Which of the following alkenes reacts the fastest with HCl? **Options:** - **A)** CH₃CH₂CH₂CH₂CH=CH₂ - **B)** trans-CH₃CH₂CH=CHCH₂CH₃ - **C)** cis-CH₃CH₂CH=CHCH₂CH₃ - **D)** (CH₃)₂C=CHCH₂CH₃ **Explanation:** There are four options provided for this question. Each option represents a different alkene structure. The question is asking which structure reacts the fastest with hydrochloric acid (HCl). - **Option A** is a straight-chain alkene with the formula CH₃CH₂CH₂CH₂CH=CH₂. - **Option B** is a trans-alkene with the formula trans-CH₃CH₂CH=CHCH₂CH₃. - **Option C** is a cis-alkene with the formula cis-CH₃CH₂CH=CHCH₂CH₃. - **Option D** is a branched alkene with the formula (CH₃)₂C=CHCH₂CH₃. The expected reaction rate can be influenced by factors such as the stability of the resulting carbocation, steric hindrance, and the structure of the alkene (cis vs. trans).
Transcribed Image Text:**Question:** Which of the following alkenes reacts the fastest with HCl? **Options:** - **A)** CH₃CH₂CH₂CH₂CH=CH₂ - **B)** trans-CH₃CH₂CH=CHCH₂CH₃ - **C)** cis-CH₃CH₂CH=CHCH₂CH₃ - **D)** (CH₃)₂C=CHCH₂CH₃ **Explanation:** There are four options provided for this question. Each option represents a different alkene structure. The question is asking which structure reacts the fastest with hydrochloric acid (HCl). - **Option A** is a straight-chain alkene with the formula CH₃CH₂CH₂CH₂CH=CH₂. - **Option B** is a trans-alkene with the formula trans-CH₃CH₂CH=CHCH₂CH₃. - **Option C** is a cis-alkene with the formula cis-CH₃CH₂CH=CHCH₂CH₃. - **Option D** is a branched alkene with the formula (CH₃)₂C=CHCH₂CH₃. The expected reaction rate can be influenced by factors such as the stability of the resulting carbocation, steric hindrance, and the structure of the alkene (cis vs. trans).
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