The species getting oxidized by 1M HBr needs to be identified. Concept introduction: A reducing or a reductant is a species that loses electron/s and gets oxidized in the chemical reaction . The reducing agent is usually in one of its lower probable oxidation states, is recognized as the electron donor. Since, the reducing agent in the redox reaction loses electron/s, reducing agent gets oxidized. An oxidizing agent is an agent which gains the electrons and gets reduced within the chemical reaction. It is also recognized as electron acceptor; it is usually in one of its higher probable oxidation states so that it can reduce after accepting electron/s. Spontaneity of a reaction is dependent on the free energy sign that is Δ G o . It should be negative for a reaction to be spontaneous. Since, Δ G = − n F E o Here, n = number of electrons involved in reaction and F is faraday constant. If the value of E° for a reaction is positive, then the reaction occurs spontaneous.

Question

5. Propose a Synthesis for the molecule below. You may use any starting materials containing 6 carbons or less (reagents that aren't incorporated into the final molecule such as PhзP do not count towards this total, and the starting material can have whatever non-carbon functional groups you want), and any of the reactions you have learned so far in organic chemistry I, II, and III. Your final answer should show each step separately, with intermediates and conditions clearly drawn. H3C CH3

Answer 1

Question

Chapter 17, Problem 46QAP

Interpretation Introduction

Interpretation:

The species getting oxidized by 1M HBr needs to be identified.

Concept introduction:

A reducing or a reductant is a species that loses electron/s and gets oxidized in the chemical reaction. The reducing agent is usually in one of its lower probable oxidation states, is recognized as the electron donor. Since, the reducing agent in the redox reaction loses electron/s, reducing agent gets oxidized.

An oxidizing agent is an agent which gains the electrons and gets reduced within the chemical reaction. It is also recognized as electron acceptor; it is usually in one of its higher probable oxidation states so that it can reduce after accepting electron/s.

Spontaneity of a reaction is dependent on the free energy sign that is ΔGo. It should be negative for a reaction to be spontaneous.

Since,

ΔG=−nFEo

Here, n = number of electrons involved in reaction and F is faraday constant.

If the value of E° for a reaction is positive, then the reaction occurs spontaneous.

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