In Chapter 8, we discussed modeling of chemical reactions, calculation of the activation energy of reaction and structure of transition state, etc. In this article, we will discuss how these routine calculations are used to guide our synthetic planning.
Let’s start with two practical questions for the following alkylation of pyrazole 1 (Figure 1). Will the alkylation be selective on N-1 or N-2? If it is not selective, will there be a reliable way to estimate the product ratio?
First, we calculate for the Electrostatic Potential Map (Chapter 3) of the two tautomeric forms of pyrazole 1 to estimate the relative acidity of the NH group (Figure 2, A and B). The electrostatic potential of the NH group in tautomer A (281 kJ/mol) is found to be slightly higher than that in tautomer B (266 kJ/mol). However this difference may not be consequential, since after deprotonation, charge is delocalized within the pyrazole molecule. Indeed, HOMO calculated for the resultant pyrazole anion shows similar lobe size on N-1 and N-2 (Figure 2, C). These couldn’t help us to differentiate the two potential alkylation pathways.
QM calculation enables us to model stepwisely the bond forming & breaking process in a chemical reaction, establish the transition state structures, estimate the associated activation energy, compare the relative difference of competing paths, and calculate for the potential product ratio.
For the pyrazole alkylation in consideration, we assume a SN2 mechanism, with pyrazole N gradually approaches the alkyl halide, forming the C-N bond and breaking the C-X bond in a concerted manner.
We set up two calculations, using CH3Br as our generic alkylating reagent, one approaches N1 of pyrazole 1, and the other interacts with N2, starting with a C-N distance of 3.8 Å, and calculate for the system energy with a step size of 0.1 Å (Figure 3).
Energy of the system starts to rise when the distance between C-N atoms is shortened to 3.0 Å, indicating that the reactant molecules start to interact. When the bond length is shortened to about 2.1 Å, the energy level reaches the peak, reaction reaches the transition state. The energy difference between these two points is our estimated activation energy.
Activation energy calculated for N-1 and N-2 alkylation is 10.77 and 9.24 kcal/mol, respectively (Figure 3), suggesting that the reaction will occur more readily at N-2.
Plugging into Arrhenius Equation the estimated difference in activation energies ( , 1.53 kcal/mol), an estimated product ratio of ~13:1 at 25 ºC is obtained.
Experimentally, when we alkylated pyrazole 1 at 25 ° C, an N-2 to N-1 product ratio of 10:1 was obtained, close to the estimation!
Table 1 illustrates how changes in relative difference in activation and reaction temperature affects product ratio, an important consideration in our synthetic planning and execution.
For a reaction with two competing pathways, with a difference of 1.4 kcal/mol in activation energy, the product ratio will be 11:1 with reaction run at 25 ºC; the ratio will decrease to 6:1 when the reaction temperature is raised to 125 ºC.
We found in practice that when the activation energy difference is around 1.4 kcal/mol, we can empirically adjust reaction temperature and solvent to optimize the ratio. On the other hand, if the calculated activation energy difference is above 3 kcal/mol, it is difficult to reverse the intrinsic bias.
In summary, through QM calculations of competing alkylation paths of pyrazole, we could calculate the difference in their activation energies, estimate the ratio of the products, and use the result to guide our synthetic planning and execution.
Alkylation of pyrazole 3 with simple alkyl halide is N-1 selective. However, reaction with chloroacetamide 4 provides only N-2 alkylation product. Such reversal in selectivity is predictable. Please stay tuned for our following chapters.
In the next article, we’ll discuss QM modeling of SNAr reaction of polyhalogenated heterocyclic substrates.
This article is written and edited by Wang Shouliang, Wang Jian, Guqin Shi, Wang Qiuyue, Pan Dong, and John S. Wai.
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