Theoretical Calculations of Metol as Corrosion Inhibitor of Steel
Theoretical Calculations of Metol as Corrosion Inhibitor of Steel
Journal of the Korean Chemical Society. 2009. Dec, 53(6): 671-676
Copyright © 2009, The Korean Chemical Society
  • Received : September 01, 2009
  • Accepted : November 10, 2009
  • Published : December 20, 2009
Export by style
Cited by
About the Authors
Gökhan Gece

Described here for the first time is an investigation on geometrical and electronic molecular structure of metol (N-methyl-p-aminophenol sulphate) as corrosion inhibitor of steel using density functional theory (DFT) calculations. Quantum chemical parameters such as highest occupied molecular orbital energy (E HOMO ), lowest unoccupied molecular orbital energy (E LUMO ), energy gap (ΔE), Mulliken charges ( q M ) and natural atomic ( q n ) charge have been calculated both for gas and aqueous phases by using B3LYP/6-31G+(d,p) basis set. The relation between the inhibition efficiency and quantum chemical parameters have been discussed in order to elucidate the inhibition mechanism of the title compound.
Corrosion is the destructive attack of metal or alloy chemically or electrochemically against its environment which leads to loss of useful properties of materials. 1 The protection of metals against corrosion can be achieved by adding inhibitors in small concentrations to its environment. 2
A survey of literature presents the applicability of organic compounds, particularly those containing O, S and/or N atoms in their long carbon chain/aromatic structure, as corrosion inhibitors for mild steel in acidic media. 3 Among these compounds, metol(N-methyl-p-aminophenol sulphate) has attracted much attention since it has been successfully used as a photographic developer, 4 , 5 analgesic-antipyretic agent, 6 , 7 and corrosion inhibitor. 8
Although experimental work 9 provide valuable information on the corrosion inhibition efficiency of metol, a deep understanding of the inhibition property remains unclear. The advancements in computer simulation techniques hold promise that questions regarding the inhibitive properties of such compounds can be addressed at the atomic level. Hence, more corrosion studies contain substantial quantum chemical calculations in recent years. 10 To date, however, no study has been performed to investigate the corrosion inhibition efficiency of metol by using quantum chemical calculations.
The objective of the present paper is to study the effect of structural parameters of metol on its inhibition efficiency of corrosion of steel by using density functional theory (DFT) methods. Molecular orbital calculations are performed looking for good theoretical parameters to characterize the inhibition property of inhibitor, which will be helpful to gain insight into the mechanism of the corrosion inhibition.
Among quantum chemical methods for evaluation of corrosion inhibitors, density functional theory (DFT) has some merits. 11 B3LYP, a version of the DFT method that uses Becke’s three-parameter functional (B3) and includes a mixture of HF with DFT exchange terms associated with the gradient corrected correlation functional of Lee, Yang, and Parr (LYP). 12
It has been shown that the B3LYP functional correctly reproduces not only the thermochemical properties of atoms and molecules, for which it has been designed, but also the ground state of strongly correlated electronic systems. 13 , 14 Besides, it has much less convergence problems than those commonly found for pure DFT methods. Thus, B3LYP was used in this paper to carry out the calculations. Full geometry optimization of the title compound was carried out at the B3LYP/6-31G+(d,p) level, both in the gas and aqueous phases, using the Gaussian 03 software package. 15
In the process of geometry optimization for the fully relaxed method, convergence of all the calculations and the absence of imaginary values in the wavenumbers confirmed the attainment of local minima on the potential energy surface. Some characteristics of the electronic structure were studied using natural bond orbital (NBO) 16 and Mulliken 17 population analysis. The details of the outermost valance electrons were obtained through the analysis of the highest occupied and lowest unoccupied molecular orbitals (HOMO and LUMO).
Metol is a derivative of 4-aminophenol which exists as half-salt complex cation in acidic media. 18 Since the free compound is unstable in air and light, it is usually marketed as the sulfate salt. It contains amino and hydroxyl groups attached to a benzene ring ( . 1 ). The benzene ring is strictly planar and the hydroxyl oxygen atom and the amine nitrogen lie in the benzene plane ( . 2 ).
Calculated geometric parameters are listed in 1 along with the experimental data. When the X-ray structure of the title compound is compared with its optimized counterpart, no significant conformational discrepancies are observed between them. The bond distances and bond angles concerning the carbon, oxygen and nitrogen atoms calculated by DFT calculation at B3LYP/6-31+G(d,p) level of theory agree satisfactorily with the values found in X-ray cristallographic data. 19 The average distances of N(11)-C(2) (1.47 A) correspond to typical carbonnitrogen single bonds (1.42 ~ 1.47 A), 20 , 21 and N(11)-C(13) bond length (1.50 A) is longer than pure carbon-nitrogen single bond due to the excess positive charge which leads to a repulsion between N and C atoms. The bond angles range from 116° to 123° around the C sites, from 115° to 120° around the N sites, and from 117° to 122° around the O sites. The bond angle of N(11)-C(2)-C(1) close to 120° as well as the bond length of N(11)-C(2) (1.47 A) confirm the sp 2 hybridization of carbon atom. In general, most of the optimized bond lengths are found to be slightly longer than the experimental ones due to the existence of crystal field in the solid state which connects molecules together with the intermolecular interactions.
PPT Slide
Lager Image
The molecular structure of metol.
PPT Slide
Lager Image
Optimized structure of metol.
Optimized and experimental geometric parametersof the title compound in the ground state
PPT Slide
Lager Image
aFor numeration please see Fig. 2. bValues from Ref. 19.
Although the charge on an atom in a molecule is not a physical observable, the atomic charge concept can offer insights into a variety of phenomena. A number of schemes for assigning charges to atoms within a molecule have been developed. Perhaps the most widely used of these is the Mulliken charge ( qM ), although the simple design of this measure brings with it potential problems. 22 The natural charge ( qn ) derived from natural population analysis (NPA) 23 is a theoretically cleaner approach which avoids many of the potential pitfalls associated with qM . In previous studies, 24 - 26 it is confirmed that intense total charge density distribution on a molecule enhances the possibility of that molecule to adsorb more strongly on the metal surface. Thus, inhibition efficiency of metol can be explained in terms of the atomic charges.
Atomic charges (e) of the title compound
PPT Slide
Lager Image
Atomic charges (e) of the title compound
The Mulliken ( qM ) and natural ( qn ) atomic charges for the title compound calculated at B3LYP/6-31+G (d,p) level in both gas and aqueous phases are presented in 2 . It can be seen from this table that the natural charges of the O17 atom and carbon atoms of benzene ring (C4, C5 and C6) have bigger negative atomic charges. The O17 atom possesses a considerable excess of electrons, implying that it is the most favourable site for interaction with the metal surface. Also C13 atom is substantially charged, but it is passivated with H atoms. A high positive charge on the nitrogen atom of amino group appears to be necessary to prevent the excess amount of negative charge from accumulating on the metal atom. Because of this balancing, carbon atoms of benzene ring are negatively charged. Consequently, these positive and negative charges fulfill the optimum conditions for interaction of metol with steel surface.
The inhibition effect of inhibitor compound is usually ascribed to adsorption of the molecule on metal surface. There can be physical adsorption (physisorption) and chemical adsorption (chemisorption) depending on the adsorption strength. When chemisorption takes place, one of the reacting species acts as an electron pair donor and the other one acts as an electron pair acceptor, so the energies of the frontier molecular orbitals should be considered. The reactive highest occupied molecular orbital (HOMO) and lowest unoccupied molecular orbital (LUMO) of any molecule are referred to as frontier molecular orbitals, after the pioneering work of Fukui. 27
Terms involving the frontier molecular orbitals could provide dominative contribution, because of the inverse dependence of stabilization energy on orbital energy difference. 28 Moreover, the gap between the HOMO and LUMO energy levels of the molecules was another important factor that should be considered. . 3 shows the distributions and energy levels of the HOMO and LUMO orbitals computed at the B3LYP/6-31+G(d,p) level for the title compound. Reportedly, excellent corrosion inhibitors are usually those organic compounds who not only offer electrons to unoccupied orbital of the metal, but also accept free electrons from the metal. 10
High values of E HOMO have a tendency of the molecule to donate electrons to appropriate acceptor molecules with low energy, empty molecular orbitals. Increasing values of E HOMO facilitate adsorption and therefore enhance the inhibition efficiency, by influencing the transport process through the adsorbed layer. 29 Similar relations were found between the corrosion rates and ΔE = E LUMO – E HOMO . 30 - 33 The energy of the lowest unoccupied molecular orbital indicates the ability of the molecule to accept electrons. The lower the value of E LUMO , the more probable it is that the molecule would accept electrons. Consequently, lower values of the energy difference (ΔE) will render good inhibition efficiency, because the energy to remove an electron from the last occupied orbital will be low.
Based on the discussions above, it is useful to compare the electronic properties of metol with those of 2-aminophenol 34 and 3-aminophenol, 35 which have been previously reported to act as effective corrosion inhibitors for aluminium and mild steel, respectively. For this purpose, the computational data on aminophenols recently published by Abrahao et al . 36 have been used for the sake of comparison.
PPT Slide
Lager Image
Molecular orbital surfaces for HOMO and LUMO of metol computed at B3LYP/6-31+G(d,p).
In 3 , certain quantum chemical parameters related to the molecular electronic structures of 2-aminophenol, 3-aminophenol and metol are presented, such as: E HOMO , E LUMO and ΔE = E LUMO – E HOMO . The calculated data for 2-aminophenol, 3-aminophenol and metol in gas phase and the results of aqueous phase calculations have been compared. In all cases, higher values of HOMO energy and lower values of energy gap (ΔE) have been obtained for aqueous phase calculations of these compounds. It could be readily seen from 3 , metol shows a relative higher value of HOMO energy and a lower value of LUMO energy considering the results of both gas and aqueous phase calculations, which is in favor of bonding with metal surface. The author, therefore, predicted that the adsorption of metol on the steel surface might be achieved by the interaction of frontier orbital between iron atoms and metol molecule. The similar interactions between organic heterocyclic molecules and iron atoms have already been reported in other documents. 37 , 38
Orbital energies for HOMO and LUMO, the HOMO-LUMO energy gap (ΔE) of 2-aminophenol, 3-aminophenol and metol
PPT Slide
Lager Image
aG: gas phase (ε = 1.0), A: aqueous phase (ε = 78.39). bGas phase data calculated at (6-31+G(d) level taken from Ref. 36. cGas and aqueous phase data calculated at (6-31+G(d,p) level.
The natural bond orbital (NBO) analysis transforms molecular orbital wave functions into onecentre (lone pair) and two-centre (bond) representations. 16 This kind of categorization represents a chemically appealing point of view, since it highlights the individual bonds and lone pairs that play a role in the chemical process. 39 The diagonal elements of the Fock matrix in an NBO representation represent the energies of localized bonds, antibonds and lone pair, while the off-diagonal elements represent bond-antibond, lone-pair-antibond and normally small antibond-antibond interactions. The larger the E (2) value, the more intensive is the interaction between electron donors and electron acceptors, i.e., the more donating tendency from electron donors to electron acceptors and the greater the extent of conjugation of the whole system. Delocalization of electron density between occupied Lewis-type (bond or lone pair) NBO orbitals and formally unoccupied (antibond or Rydgberg) non-Lewis NBO orbitals correspond to a stabilizing donor-acceptor interaction. For each donor NBO( i ) and acceptor NBO( j ), the stabilization energy E (2) associated with electron delocalization between donor and acceptor is estimated as 40
Second-order perturbation theory analysis of the Fock matrix in natural bond orbital (NBO) basis, calculated at B3LYP/6-31+G(d,p) level
PPT Slide
Lager Image
aEnergy difference between donor and acceptor i and j NBO orbitals. bFock matrix element between i and j NBO orbitals. cEnergy of hyper conjugative interactions.
PPT Slide
Lager Image
where q i is the donor orbital occupancy, ε i , ε j are diagonal elements (orbital energies) and F ij is the off-diagonal NBO Fock matrix element. The results of second-order perturbation theory analysis of the Fock Matrix at B3LYP/6-31+G(d,p) level of theory are presented in 4 . NBO analysis revealed that the n (O17) → σ(C4-C5) interactions give the strongest stabilization to the system of the title compound by 12 kcal mol -1 .
The electronic and geometrical properties of metol obtained with the B3LYP exchange-correlation functional, proved to provide an appropriate description of (N-methyl-p-aminophenol sulphate), are consistent with the experimental data. According to the computed quantum chemical parameters, the corrosion inhibition property of the metol can be attributed to the presence of heteroatom and p electrons on benzene ring. These factors play the vital role in the adsorption of the inhibitor and the formation of coordinate bond with metal. The adsorption of inhibitor on the steel surface can occur either directly by the interactions between the p electrons of the inhibitor and the vacant d-orbitals of metal surface atoms. The interaction causes the adsorption of metol on corroding sites of metals and prevents the anodic reaction.
The author thanks Prof. Z. Kantarcı for allowing the use of Gaussian03program package for the calculations and Prof. S. Bilgiç for her unfailing counsels.
Uhlig H. H. , Revie R. W. 1985 Corrosion and Corrosion Control Wiley & Sons New York
Jones D. A. 1992 Principles and Prevention of Corrosion Macmillan New York
Sanyal B. 1981 Prog. Org. Coat. 9 (2) 165 -    DOI : 10.1016/0033-0655(81)80009-X
Henney K. , Dudley B. 1939 Handbook of Photography Whittlesey House New York
Lunar L. , Sicilia D. , Rubio S. , Pérez-Bendito D. , Nickel U. 2000 Water Res. 34 1791 -    DOI : 10.1016/S0043-1354(99)00339-5
Cekic S. D. , Filik H. , Apak R. 2005 J. Analytical Chem. 60 1019 -    DOI : 10.1007/s10809-005-0230-7
Chu Q. , Jiang L. , Tian X. , Ye J. 2008 Anal. Chim. Acta 606 246 -    DOI : 10.1016/j.aca.2007.11.015
Kirk R. , Othmer D. 1994 Encyclopedia of Chemical Technology Wiley & Sons New York
Praveen B. M. , Venkatesha T. V. 2009 Int. J. Electrochem. Sci. 4 267 -
Gece G. 2008 Corros. Sci. 50 2981 -    DOI : 10.1016/j.corsci.2008.08.043
Lopez N. , Illas F. 1998 Phys. J. Chem. B 102 1430 -    DOI : 10.1021/jp972626q
Lee C. , Yang W. , Parr R. G. 1988 Phys. Rev. B 37 785 -    DOI : 10.1103/PhysRevB.37.785
Feng X. B. 2004 Phys. Rev. B 69 155107 -    DOI : 10.1103/PhysRevB.69.155107
Mackrodt W. C. , Middlemiss D. S. , Owens T. G. 2004 Phys. Rev. B 69 115119 -    DOI : 10.1103/PhysRevB.69.115119
Frisch M. J. 2004 Gaussian 03 Gaussian Inc. Wallingford CT
Reed A. E. , Weinhold F. 1983 J. Chem. Phys. 78 4066 -    DOI : 10.1063/1.445134
Mulliken R. S. 1955 J. Chem. Phys. 23 1833 -    DOI : 10.1063/1.1740588
Forester A. R. , Wardell J. L. 1971 Rodd’s Chemistry of Carbon Compounds Elsevier Publishing Co. Amsterdam
Cavalca L. , Gasparri G. F. , Mangia A. , Pelizzi G. 1970 Acta Cryst. B26 498 -    DOI : 10.1107/S0567740870002716
Yang J. G. , Pan F. Y. , Yan H. 2006 Chinese J. Struct. Chem. 25 1435 -
Allen F. H. , Kennard O. , Watson D. G. , Brammer L. , Orpen A. G. , Taylor R. 1987 J. Chem. Soc. Perkin Trans. II S1 -    DOI : 10.1039/p298700000s1
Bachrach S. M. 1994 Reviews in Computational Chemistry VCH New York
Reed A. E. , Weinstock R. B. , Weinhold F. A. 1985 J. Chem. Phys. 83 735 -    DOI : 10.1063/1.449486
Zhang D. Q. , Cai Q. R. , Gao L. X. , Lee K. Y. 2008 Corros. Sci. 50 3615 -    DOI : 10.1016/j.corsci.2008.09.007
Eddy N. O. , Ibok U. J. , Ebenso E. E. , El Nemr A. , El Ashry E. H. 2009 J. Mol. Model. 15 1085 -    DOI : 10.1007/s00894-009-0472-7
Cruz J. , Pandiyan T. , García-Ochoa E. 2005 J. Electroanal. Chem. 583 8 -    DOI : 10.1016/j.jelechem.2005.02.026
Fukui K. , Yonezawa T. , Nagata C. , Shingu H. 1954 J. Chem. Phys. 22 1433 -    DOI : 10.1063/1.1740412
Fang J. , Li J. 2002 J. Mol. Struct. (Theochem) 593 179 -    DOI : 10.1016/S0166-1280(02)00316-0
Fouda A. S. , Abu-Elnader H. M. , Soliman M. S. 1986 Bull. Korean Chem. Soc. 7 (2) 97 -
Pang X. , Hou B. , Li W. , Liu F. , Yu Z. 2007 Chin. J. Chem. Eng. 15 909 -    DOI : 10.1016/S1004-9541(08)60024-5
Bouklah M. , Hammouti B. , Benkaddour M. , Benhadda T. 2005 J. Appl. Electrochem. 35 1095 -    DOI : 10.1007/s10800-005-9004-z
Martinez S. , Valek L. , Stipanović Oslaković I. 2007 J. Electrochem. Soc. 154 C671 -    DOI : 10.1149/1.2777882
Şahin M. , Gece G. , Karcı F. , Bilgiç S. 2008 J. Appl. Electrochem. 38 809 -    DOI : 10.1007/s10800-008-9517-3
Müller B. , Shadid M. , Kinet G. 1999 Corros. Sci. 30 1323 -    DOI : 10.1016/S0010-938X(98)00186-3
Hür E. , Bereket G. , Duran B. , Özdemir D. , Şahin Y. 2007 Prog. Org. Coat. 60 153 -    DOI : 10.1016/j.porgcoat.2007.07.026
Abrahão O. Jr. , Pançonato Teixeira T. S. , Madurro J. M. , da Hora Machado A. E. , Brito-Madurro A. G. 2009 J. Mol. Struct. (Theochem) 913 28 -    DOI : 10.1016/j.theochem.2009.07.013
Li Y. , Zhao P. , Liang Q. , Hou B. 2005 Appl. Surf. Sci. 252 1245 -    DOI : 10.1016/j.apsusc.2005.02.094
Zhao P. , Liang Q. , Li Y. 2005 Appl. Surf. Sci. 252 1596 -    DOI : 10.1016/j.apsusc.2005.02.121
Reed A. E. , Curtiss L. A. , Weinhold F. 1988 Chem. Rev. 88 899 -    DOI : 10.1021/cr00088a005
Gutowski M. , Chalasinski G. 1993 J. Chem. Phys. 98 4728 -    DOI : 10.1063/1.465106