Question contains Statement-1 and Statement-2 and has the following choices (a), (b), (c) and (d), out of which ONLY ONE is correct. (a) Statement- 1 is True, Statement- 2 is True; Statement- 2 is a correct explanation for Statement-1 (b) Statement- 1 is True, Statement- 2 is True; Statement- 2 is NOT a correct explanation for Statement-1 (c) Statement- 1 is True, Statement- 2 is False (d) Statement-1 is False, Statement- 2 is True Statement 1 \(\mathrm{CH}_{3}-\mathrm{CH}=\mathrm{CH}-\mathrm{CH}_{3}\) is more reactive towards \(\mathrm{HBr}\) compared to ethylene. and Statement 2 The carbocation formed in \(\mathrm{CH}_{3} \mathrm{CH}=\mathrm{CH}-\mathrm{CH}_{3}\) during the addition of \(\mathrm{HBr}\) is more stabilized compared to the cation formed from ethylene.

Step by step solution

01

Statement 1: Reactivity towards HBr

First, let's determine if CH3-CH=CH-CH3 (2-Butene) is more reactive towards HBr than ethylene. When we add HBr to an alkene, a carbocation is formed, and the one that is more stable will form more quickly and thus will be more reactive. Adding HBr to 2-Butene: CH3-CH=CH-CH3 + HBr → CH3-CH(+)-CHBr-CH3 Adding HBr to ethylene: H2C=CH2 + HBr → H2C(+)-CH2Br Now, let's compare the stability of these two carbocations.

02

Statement 2: Carbocation Stability

The carbocations formed in the reaction are secondary (in 2-Butene) and primary (in ethylene) carbocations. Generally, carbocation stability increases in the order: primary < secondary < tertiary. In this case, the carbocation formed in the reaction with 2-Butene is more stable than the one formed from ethylene, because a secondary carbocation is more stable than a primary carbocation. With these analyses, we can see that both statements are true, and statement 2 correctly provides an explanation for the higher reactivity of 2-Butene towards HBr compared to ethylene. Hence, the answer is: (a) Statement- 1 is True, Statement- 2 is True; Statement- 2 is a correct explanation for Statement-1

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