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goblinko [34]
3 years ago
9

A variation of the acetamidomalonate synthesis can be used to synthesize threonine. The process involves the following steps: Et

hoxide ion deprotonates diethyl acetamidomalonate, forming enolate anion 1; Enolate anion 1 makes a nucleophilic attack on acetaldehyde, forming tetrahedral intermediate 2; Protonation of the oxyanion forms alcohol 3; Acid hydrolysis yields dicarboxyamino alcohol 4; Decarboxylation leads to the final amino acid. Write out the mechanism on a separate sheet of paper, and then draw the structure of tetrahedral intermediate 2.

Chemistry
1 answer:
ipn [44]3 years ago
7 0

Answer:

See figure 1

Explanation:

For this reaction, we have the production of a carbanion as the first step. The base "ethoxide" can remove a hydrogen-producing a negative charge in the carbon (<u>enolate anion 1</u>). Then this negative charge can attack the carbon of the carbonyl group in the molecule acetaldehyde and the <u>tetrahedral intermediate 2</u> is form. In the next step, we have the protonation of the oxygen to produce <u>alcohol 3</u>. A continuation we have the hydrolysis of the ester groups to produce the <u>Dicarboxyamino alcohol</u> and finally, we have a decarboxylation reaction we will produce the amino acid <u>Threonine</u>.

To further explanations see figure 1

I hope it helps!

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The AP Biology teacher is measuring out 638.0 g of dextrose (C6H12O6) for a lab. How many moles of dextrose is this equivalent t
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The AP Biology teacher is measuring out 638.0 g of dextrose (C6H12O6) for a lab the moles of dextrose is this equivalent to is 3.6888 moles.

<h3>What are moles?</h3>

A mole is described as 6.02214076 × 1023 of a few chemical unit, be it atoms, molecules, ions, or others. The mole is a handy unit to apply due to the tremendous variety of atoms, molecules, or others in any substance.

To calculate molar equivalents for every reagent, divide the moles of that reagent through the moles of the restricting reagent. The calculation is follows:

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In reality, energy conversion from burning fuel is never 100% efficient. Significant loss of energy due to heating occurs. If th
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Explanation:

This question is asking for the inductive reactance, which is calculated as follows:

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3 years ago
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