Answer :
Final answer:
An easy-to-pull acidic hydrogen is preferred by the Grignard reagent due to a lower reaction energy pathway. Le Chatelier's principle explains how the reaction adjusts to maintain equilibrium. Also, weaker oxidizing agents are preferred when preparing hydrogen bromide and hydrogen iodide.
Explanation:
The Grignard reagent would prefer the easy-to-pull acidic hydrogen of a solvent because this process involves a pathway with a lower reaction energy. This occurs as the Grignard reagent, when in an acidic solution, interacts with the conjugate base that's produced. This base is known to contain other bonded water molecules that can act as acids, facilitating the step-wise transfer of protons.
In relation to this, Le Châtelier's principle is applicable, which states that a system in equilibrium will adjust to counteract any imposed change. For example, if the reaction is exothermic such as in the case of MgF2's solubility decreasing with rising temperature, the equilibrium will shift towards the reactants' side. This in turn results in less reagent dissolving.
Analogously, hydrogen bromide and hydrogen iodide can't be prepared using an oxidizing agent like sulfuric acid. A weaker oxidizing agent, such as phosphoric acid, is instead used. Lastly, it's important to note that these reactions are reversible, a vital element in the chemistry of organic compounds.
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