This is Btec Applied Science Unit 14 Assignment D (Making designer chemicals) which was awarded a distinction and contains all the practical results. This is an example of a Distinction level assignment, and you may use it as a guide to help you achieve a distinction and finish this assignment.
Unit 14: Applications of Organic Chemistry
D: Investigate organic chemistry reactions in order to gain skills in preparative organic chemistry.
Assignment Title: Making designer chemicals
Ethyl Ethanoate: Ethyl acetate (also known as ethyl ethanoate, acetic acid ethyl ester, acetoxy ethane,
1-acetoxyethane, EtOAC, ETAC, EA) is an organic ester compound with the molecular formula C4H8O2.
It's a clear liquid with a fruity odour that's commonly found in glues and nail polish removers.
Preparation of ethyl ethanoate:
Mechanism: By combining ethanol with ethanolic acid and utilising concentrated sulfuric acid as a
catalyst, ester ethyl ethanoates are created. This process can be reversed and is gradual. To lessen the
likelihood of reverse reactions, esters are immediately removed using distillation.
For the purpose of making the ensuing
mechanics clear, all stages are displayed as one-way reactions. The formulation of the process is
impacted since the reverse reaction occurs in a totally different manner.
Concentrated sulfuric acid releases protons (hydrogen ions) to acetic acid in the first stage. A proton is
taken up by one of the single pairs of oxygen double-bonded to carbon, which then binds to carbon.
This illustration of the structure is inaccurate because oxygen acquires a positive charge when a proton
is transferred to it. The majority of the positive charge is spread among the carbon atoms, which are
located along the right edge of the ion. To put it another way, we may think of this structure as the
outcome of electron pair changes.
, As seen by the two arrows, each of the many configurations contributes to the ion's overall structure.
The connection will not automatically transition between her two separate setups as a result. Resonance
structures or canonical forms refer to several sorts of structures. The atoms of carbon and oxygen each
have a little positive charge. Each bond—which can range in size from single to double—between two
oxygen and carbon atoms is identical.
The positive charge on the carbon atom is attacked in step 2 by one of the lone pairs of electrons on the
oxygen atom of the ethanol molecule.
A proton (hydrogen ion) travels from the lower oxygen atom to the upper oxygen
atom in the third step. A other component of the mixture picks it up, and it is then approximately
reflected back to an oxygen atom. By forming a bond with an unpaired electron on the unreacted
ethanol molecule, this is accomplished. The finished item appears as follows:
Water molecules and ions are split apart in step 4. Production ions are now closely resembling the
finished product and are displayed in a fashion that represents it. The youngest ion has the same
structure as that described in step 1 in this process. Actually, the positive charge is dispersed along the
ion's edges, and the positioning of the charge on one of the oxygen
atoms also plays a role.
Step 5 involves removing hydrogen from oxygen by interacting with the bisulphate ions produced in step
1.
The ester was prepared and the sulfuric acid catalyst was renewed.
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