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Benson Group Increment Theory

Benson Group Increment Theory, or Group Increment Theory, utilizes the experimentally calculated heat of formation for individual atoms to calculate the entire heat of formation for the molecule under investigation. This can be a very quick and convenient way to theoretically determine heats of formation without conducting tedious experimentation. However as useful as it is in thermodynamics, the Benson Group Increment Theory has its limitations, and thus can not always predict the precise heat of formation.

Origin

The Benson Group Increment Theory originated in 1958 when Benson and Buss proposed "Additivity Rules for Estimation of Molecular Properties. Thermodynamic Properties." Within this manuscript, Benson and Buss proposed four approximations: A Limiting Law for Additivity Rules, Zero-Order Approximation. Additivity of Atomic Properties, First Order Approximation. Additivity of Bond Properties, and Second Order Approximation. Additivity of Group Properties." These approximations account for the atomic, bond, and group contributions to heat capacity (Cp), enthalpy (ΔH°), and entropy (ΔS°). The most important of these approximations to the group increment theory is the Second Order Approximation, because this approximation "leads to the direct method of writing the properties of a compound as the sum of the properties of its group."[1]

The Second Order Approximation accounts for two molecular atoms or structural elements that are within relative proximity to one another (approximately 3-5 Angstroms as proposed in the paper). By using a series of disproportionation reactions of symmetrical and unsymmetrical framework, Benson and Buss concluded that neighboring atoms within the disproportionation reaction understudy are not effected by the change. From this they can term a "group" as a polyvalent atom connected together with its ligands. However, they note under all approximations that ringed systems and unsaturated centers do not follow additivity rules due to their preservation under disproprotionation reactions. One can understand this as you must break a ring at more then one site to actually undergo a disproportionation reaction. This holds true with double and triple bonds, as you must break them multiple times to break their structure. They concluded that these atoms must be considered as distinct entities. Hence we see Cd and CB groups which take into account these groups as being individual entities.

Table 1: Heats of formations for alkane chains

From this Benson and Buss concluded that any saturated hydrocarbon can be precisely calculated due to the two groups being a methylene [C-(C)2(H)2] and the terminating methyl group [C-(C)(H)3].[2] Benson later began to compile actual functional groups from the Second Order Approximation.[3][4] Ansylyn and Dougherty explained in simple terms how the group increments, or Benson increments, are derived from experimental calculations.[5] By calculating the ΔΔHf between extended saturated alkyl chains (which is just the difference between two ΔHf values), as shown in the figure to the right, one can approximate the value of the C-(C)2(H)2 group by averaging the ΔΔHf's. Once this is determined, all one needs to do is take the total value of ΔHf subtract the ΔHf caused by the C-(C)2(H)2 group(s), and then divide that number by two (due to two C-(C)(H)3 groups) and you now have the value of the C-(C)(H)3 group. From the knowledge of these two groups, Benson moved forward obtain and list functional groups derived from countless numbers of experimentation from many sources, some of which are displayed below.

Applications

Fig. 1: Simple Benson Model of Isobutyl Benzene

As stated above, BGIT can be used to calculate heats of formation which are important in understanding the strengths of bonds and entire molecules. Furthermore, the method can be utilized to quickly estimate whether a reaction is endothermic or exothermic. Even though BGIT was introduced in 1958 and would seem to be antiquated in the modern age of advanced computing, the theory still finds practical applications. In a 2006 paper, Gronert states: "Aside from molecular mechanics computer packages, the best known additivity scheme is Benson's."[6]

Figure 1 displays a simple application for predicting the standard enthalpy of isobutyl benzene.
Each individual atom is accounted for where CB-(H) accounts for one benzene carbon connecting to two other carbons and a hydrogen atom. This would be multiplied by five, since there are five CB-(H) atoms. The CB-(C) molecule further accounts for the other benzene carbon attaching to the butyl group. The C-(CB)(C)(H) accounts for the carbon linked to the benzene group on the butyl moiety. The 2' carbon of the butyl group would be C-(C)3(H) because it is a tertiary carbon (connecting to three other carbon atoms). The final calculation comes from the CH3 groups connected to the 2' carbon; C-(C)(H)3. The total calculations add to -5.15kcal/mol, which is identical to the experimental value.

Limitations

Though powerful it is, Benson Group Increment Theory do have several limitations which restrict its usage.
1.Not very accurate!
There is a overall 2-3 Kcal/mol error using the Benson Group Increment Theory to calculate the △Hf. The value of each group is estimated on the base of the average △△Hf0shown above and there will be a dispersion around the average △△Hf0. Also, it can only be as accurate as the experimental accuracy. That's the derivation of the error and there is nearly no way to make it more accurate.

2.Not all groups are available!
The Benson Group Increment Theory is based on empirical data and heat of formation. Some groups are too hard to measure, so not all the existing groups are available in the Table above.Sometimes approximation should be made when we meet those unavailable groups. For example, we need to approximate C as Ct and N as NI in C≡N,which clearly cause more inaccuracy, which is another drawback.

3.Not all the situations are accounted for!

In the Benson Group Increment Theory, we assumed that a CH2 always makes a constant contribution to △Hf0 for a molecule. However, a small ring such as cyclobutane leads to a substantial failure for the Benson Group Increment Theory, because of its strain energy.a series of correction terms for common ring systems has been developed, with the goal of obtaining accurate △Hf0 values for cyclic system. Representative values are given in the Table shown below. Note that these are not identically equal to the accepted strain energies for the parent ring system, although ther are quite close. The group increment correction for a cyclobutane is based on △Hf0 values for a number of strutures, and represents an average values that gives the best agreement with the range of experimental data. In contrast, the strain energy of cyclobutane is specific to the parent compound, with there new corrections, it is now possible to predict △Hf0 values for strained ring system, by first adding up all the basic group increments and then adding appropriate ring strain correction values.

File:Beson2.jpg

The same as ring system, other corrections have been made to other situations such as Gauche alkane with a 0.8kcal/mol correction, cis alkene with a 1.0kcal/mol correction, respectively.

Also, the Benson Group Increment Theory fails when conjugation and interactions between functional groups exist[7][8], such as intermolucular and intramolecular hydrogen bonding shown in the right figure, which limits its usage.

References

  1. ^ Benson, S. W. and Buss, J. H. Journal of Chemical Physics 1958, 29, 546-572.
  2. ^ Souders, M.; Matthews, C. S.; and Hurd C. O., Ind. & Eng. Chemistry 1949, 41, 1037-1048
  3. ^ Benson, S. W.; Cruicksh, F. R.; Golden, D. M., et al. Chemical Reviews 1969, 69, 279-324
  4. ^ Benson, S. W.; Cohen, N. Chemical Reviews 1993, 93, 2419-2438
  5. ^ Eric V. Anslyn and Dennis A. Dougherty Modern Physical Organic Chemistry University Science Books, 2006.
  6. ^ Gronert, S. J. Org. Chem.2006,71,1209-1219.
  7. ^ Knoll, H. Schliebs, R. and Scherzer, H. Reaction Kinetics and Catalysis Letters 1978, 8, 469-475.
  8. ^ Sudlow, K. and Woolf, A.A. Journal of Fluorine Chemistry 1995, 71, 31-37.
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