Received 12 March 2016; accepted 25 April 2016; published 28 April 2016
Cancer is a leading cause of death in both more and less economically developed countries due to tobacco use, obesity, physical inactivity, and infections  . Ibuprofen drug is a member of the class of drugs termed as non-steroidal anti-inflammatory drugs (NSAIDS), with anti-inflammatory, analgesic, and antipyretic activity. Recently, the regular use of ibuprofen prevents from some certain cancers including prostate, colon, breast, lung, and gastric cancers due to the inhibition of cyclooxygenase-2(COX-2)   . Reduced Risk of Human Lung Cancer by Selective Cyclooxygenase 2 (Cox-2) Blockade was studied by Harris et al.  . The 2-arylpropanoic acids (2-APAs) are an important group of non-steroidal anti-inflammatory drugs, the majority of which are remarked as racemic mixtures because they have asymmetric carbon atom. These drugs exhibit stereoselectivity in both their pharmacological activity, i.e. inhibition of cyclo-oxygenase  . The lattice energy of ibuprofen crystals which is calculated using DFT method agrees with the experimental values especially with polymorphism of the crystals  . The conformational stability of ibuprofen, due to a para-substituted group in the molecule, is carried out using DFT calculations coupled with optical vibrational spectroscopy. The calculated frequencies and intensities prove the presence of the lowest energy conformers in the solid state and intermolecular hydrogen bonds between the carboxylic groups of adjacent molecules leading to formation of dimmers  . In the frame of theoretical studies of ibuprofen, the action of ibuprofen is due to electrophilic attack on the oxygen atoms of carboxyl group  . The superior DFT methods in predicting the structures of ibuprofen are mPW1PW91/6-311++G (d, p) and mPW1PW91/6-311++G (2d, 2p) while B3PW91/6-311++G (2d, 2p) is the best method to predict all vibrational frequencies of the molecule  . In this work, it has been suggested that the anti-cancer effect of the ibuprofen and its analogues is due to their anionic and molecular forms of the drug side by side in the human body specifically for the positive cancer cells.
2. Experimental Work
All melting points of the studied compounds have been determined on a Gallen-Kamp melting point apparatus.
The elemental analyses (C, H, N) were determined using Elementer Analyses system (GmbH, Donaustr-7, D-63452) Hanau, (Germany).
The electronic absorption spectra of the studied compounds had been scanned by uv-2011 PC, uv-vis scanning spectrophotometer (Shimadzu) using 1 cm matched silica cells.
The atomic absorption spectra of the complexes were studied by using an atomic absorption spectrophotometer (Buck Scientific Model 210 GVP).
2.2. Materials and Methods
All materials supplied to our experimental work were bought from the different companies without further purification. Ibuprofen (IBF) was bought from Sigma Aldrich and 2-Phenylpropanoic acid (2-PPA) was bought from Alfa Aesar as well as 3-Phenylpropanoic acid (3-PPA).
Ibuprofen (2.06 g, 0.01 moles) was allowed to be dissolved in a solution of potassium bicarbonate (1.10 g, 0.011 mole) in 80 ml of water. During stirring the solution, CuSO4・5H2O was added slowly (1.25 g, 0.005 mole) in 10 ml of water. The mixture was allowed to be stirred for 30 minutes. The aquamarine precipitated and was collected, washed with water followed by ethanol, and then recrystallized from ether. The product was air-dried,  .
2.0 Mmoles (0.412 g) of ibuprofen react with 2.0 mmoles (0.112 g) of KOH dissolved in 20 mL of distilled water, to give the potassium salt of the ligand. Then 1.0 mmole (0.2195 g) of Zn(CH3COO)2・2H2O (aqueous solution) was added during stirring. The white needle precipitated and collected by filtration, washed several times with distilled water and acetone, then dried in vacuum,  . The melting points of the studied compounds have been presented in Table 1.
3. Method of Calculations
3.1. Spectral Constants
The absolute intensity of band absorption can be calculated and it has been shown that Einstein transition probabilities coefficients,   of the emission, A, and the absorption, B, between two electronic states i.e. the
Table 1. Melting points of ibuprofen, 3-PPA, Copper(II) and Zinc(II) comp- lexes with ibuprofen.
Table 2. Elemental analysis of Copper(II) and Zinc(II) complexes with Ibu- profen.
Table 3. Atomic absorption of Copper(II) and zinc(II) complexes with Ibu- profen.
ground state I, and the excited state f, are given as follows:
e = The charge of the electron
h = Planck’s constant
C = The velocity of light, 3 ´ 1010 cm・sec−1
= The wave number in cm−1
Gf = Degeneracy of the state
Dif = Dipole strength
Substituting the numerical values and assuming that degeneracy of the state is singlet, then:
Mulliken related the quantity Bif to the Oscillator strength, F, which is the measure of the intensity.
Also the Oscillator strength can be related to the absolute intensity as follows:
where: m = The mass of electron
N = The Avogadro’s number
e = Molar extinction coefficient
if a molecule or an atom is in an excited state then, in the absence of an external electromagnetic field, on the average, after a time of where Aif is the Einstein spontaneous transition probability coefficient from the
excited state to the ground state, it will emit a photon. is called the mean lifetime of the excited state. Generally Dif can be calculated numerically as follows:
where is the half width of the absorption band in cm−1. hence, the oscillator strength can be calculated directly as follows:
3.2. DFT Calculations
Computational studies on the isolated molecules in the gas phase were performed by the aid of GAUSSIAN 03 package. Minimum energy structures have been achieved using semi-empirical AM1 method. DFT/6-31**G calculations were performed on the minimum energy structures using the closed shell Hartree-Fock, Becke’s three parameters density functional theory, DFT,   in combination with the Lee, Yang and Parr correlation functional B3LYP. The differentiation between the conformers’ R and S of the ibuprofen drug was based on the total energy difference which has been calculated via SCF using RHF for these types of molecules and UHF for the molecular anions.
With respect to DFT calculations, it has been carried out as B3LYP/6-31**G and the energy of the DFT theory can be represented as a function of the electron density as follows:
where is the electron density
where Ci is the eigenvectors for each eigenfunction Ψi and
where is the total energy Hamiltonian operator. ε is the permittivity of the vacuum.
4. Results and Discussion
4.1. Spectroscopic Studies
Ibuprofen, 2 (4-isobutylphenylpropanoic acid (IBF), is a non-steroidal anti-inflammatory drug (NSAID) which can be used for relieving pain, antipyretic and anti-inflammatory. About 60% of patients improve with any given NSAID and it is advised that if one does not work that another can be used. Ibuprofen may be considered as weak anti-inflammatory than other NSAIDs. IBF molecule has two conformers R and S as shown in the following Figure 1. Ibuprofen has a particularly interesting property, and it can exist as a pair of optical isomers that
Figure 1. Minimum energy structures of Ibuprofen isomers.
are mirror images of each other. These mirror images are non-super-imposable, which are mirror images but not identical. This mirror image property occurs in molecules that have asymmetric carbon atom. The two optical isomers of ibuprofen are identified by the prefixes R− (Levo Rotatory) and S+ (Dextro Rotatory). DFT calculations have been performed according to El-Shahawy,   using the basis set 6-31**G.
From the previous Table 4, it has been shown that the energy difference between the S and R forms is very small being equal to 0.02839 eV which is too small to make a significant difference in the temperature effect, Figure 2, on the spectrum in ethanol solvent,  . Therefore IBF molecules exist in the two forms in a racemic mixture. From the energy difference between the two forms it has been calculated that the ratio between them equal 0.35 of the S-conformer of higher energy this means that the R-form is the predominant form in the IBF drug i.e. 65% at 37˚C. The two forms have nearly the same constants of ionization potential, Ip, and electron affinity Ea, except the dipole moment of the S-form is higher than that of R-form.
From the previous Table 5, it can be concluded that the IBF molecule, even S or R, form has lower energy than those of phenyl derivatives of propanioc acid which have higher ionization potentials than those of IBF forms. The electron affinities of 2-PPA and Zn (IBF)2 are higher than those of the studied compounds. The S-IBF and 2-PPA have the higher dipole moments among all the other compounds.
Regarding the HOMO of IBF molecule even in the R and S-forms, it is ψm in each singlet configuration eigenfunctions of the excited states. From the previous Table 6, it has been noticed that the first excited state of R-form includes the configurations of transitions ψm−2 → ψm+1, ψm → ψm+1, ψm → ψm+3 and ψm → ψm+4. The configuration eigenfunction of highest contribution in the first excited state is that includes the transition ψm → Ψm+1 of eigenvector 0.60334. From the previous Table 7, it can be noticed that the first excited state of S-form is constituted from the configuration eigenfunctions of transitions ψm−2 → ψm+1, ψm−2 → ψm+5, ψm → ψm+1 and ψm → ψm+2 and ψm → ψm+5. The configuration which has high contribution in the transition to the first excited state contains the transition ψm → ψm+1 of eigenvector 0.55621 in case of S-form. In the second singlet excited state of the R-form, the contributions of configuration eigenfunctions containing the transitions ψm−1 → ψm+1 and ψm → ψm+2 are the highest as well as in case of the S-form, Table 6, Table 7. For the R-form, the third excited state includes the highest configuration eigenfunction of the transition ψm−2 → ψm+1 as well as in case of the S-form. It is shown from the previous Table 6, Table 7, that the first transitions from the ground state to the firs excited state for the two conformers lies at the same wavelength 445 nm which has not any change in the uv-spectrum of IBF drug by the temperature effect  .
From the previous Figure 3 and Table 8, of IBF spectra, it has been shown that there is some broadness in the top of the absorption bands in different solvents and of course the temperature effect doesn’t show any change in the relative intensity, Figure 2, due to the very small energy difference between the two conformers R and S
Figure 2. Electronic spectra of Ibuprofen (403 mmol・L−1) in ethanol at different temperature: a = 25˚C; b = 40˚C.
Table 4. DFT-Data of the optical isomers of IBF in the ground state.
Table 5. Comparative DFT parameters of Ibuprofen and some analogues.
N.B. 2-PA is 2-phenyl propanioc acid and 3-PA is 3-phenyl propanioc acid. Ip is the ionization potential, Ea is the electron affinity and Dip. Mom. Is dipole moment.
Table 6. Excitation energies and oscillator strengths of R-form of IBF in the gaseous state.
Figure 3. Electronic spectra of Ibuprofen (403 mmol・L−1 in) (a) EtOH (b) MeOH, (c) Isopropanol, (d) CHCl3, and (e) Cyclohexane.
Table 7. Excitation energies and oscillator strengths of S-form of IBF in the gas phase.
Table 8. Spectral parameters, Einstein probabilities (Aif and Bif), dipole strength (Dif), oscillator strength (Fif), lifetime (τ) and extinction coefficient (εmax) of the electronic transition bands of Ibuprofen in different solvents.
 . However, the maximum absorption band positions exist at the same values 231 and 263 nm even by using different solvents with different polarities indicating to non-polarized ground and excited states for this molecule. The Einstein transition probabilities (Aif and Bif), oscillator strength fif, dipole strength Dif and the life time of excitation τ between the initial (i) and the final (f) electronic states have been calculated according to El-Shahawy   . The spontaneous transition probability Aif, of IBF spectra in different solvents of different polarity has values which are higher at λmax = 231 nm than those at λmax = 263 nm as well as the same situation in the values of the induced transition probability, Bif, of IBF spectra. The dipole strength Dif values are higher at λmax = 231 than those at λmax = 263 nm. The absorption bands at λmax = 231 nm have higher oscillator strengths fif than those at λmax = 263 nm and this appears in Figure 3, that the absorption bands at λmax = 231 nm have higher intensities more than those at λ = 263 nm in different solvents. The life time of the electronic excited states τ, of this molecule has average value ~200 ns for the transitions at λmax = 263 nm but it has lower average value ~45 ns for the transitions at λmax = 231 nm.
The ultraviolet spectra of 2-Phenylpropanoic acid Figure 4, show bands at λ = 257 nm and at λmax = 228 nm which have the induced transition probability (Bf) in different solvents being higher than those of the spontaneous transition probability (Aif) as in the same case of IBF spectra. The molar absoptivities of the two absorption bands at λmax = 231 and λmax = 263 in the IBF spectra are higher, Table 8, than those of absorption bands λmax = 228 and λmax = 257 nm in the spectra of 2-Phenylpropanoic acid, Table 9. The oscillator strengths fif, in 2-Phenylpropanoic acid spectra in different solvents are lower than those of IBF spectral bands. The dipole strengths Dif of 2-Phenylpropanoic acid absorption bands in different solvents are lower than those of IBF but the life times of the excited states of the absorption bands in the spectra of 2-Phenylpropanoic acid are higher than those of IBF spectral bands. From the previous Table 10, the transition energy from the ground state to the first excited state lies at 244 nm which is corresponding to an experimental value at 257 nm, Table 9. This first excited state of minimum energy structure of 2-PPA, Figure 5, is composed from configuration eigenfunctions of the electronic transitions ψm−2 → ψm+1, ψm−2 → ψm+4, ψm → ψm+1, ψm → ψm+2 and ψm → ψm+4. The main configuration eigenfunction in the first excited state having the transition ψm-→ ψm+1 of eigenvector 0.49968. The calculated transition energy to the second excite state at λ = 233 nm has good coincidence with the experimental position at λ = 228 nm and the main configuration eigenfunction of high contribution in the second excited state includes the transition ψm−1−→ ψm+1 of eigenvector 0.49872. The eigenfunction of high contribution in the third excited state includes the transition ψm−2 → ψm+1 of eigenvector 0.46682.
The first calculated electronic transition from the ground state to the first singlet state lies at 236 nm which is not far from the experimental maximum wavelength at 259 nm, Table 11. From comparison point of view between the spectral parameters between 2-PPA and 3-PPA it can be noticed that the Einstein transition probabilities (Aif and Bif), dipole sstrength Dif and oscillator strength Fif of 2-PPA are higher than those of 3-PPA spectral parameters but the life time of excitation of 3-PPA is higher than that of 2-PPA spectral parameters, Table 9,
Figure 4. Electronic spectrum of 2-Phenylpropanoic acid (452 mmol・L−1) in (a) EtOH, (b) MeOH, (c) Isopropanol, (d) CHCl3 and (e) Cyclohexane.
Figure 5. Minimum energy structure of 2-Phenylpropanoic acid (2-PPA).
Table 9. Spectral parameters, Einstein probabilities (Aif and Bif), dipole strength (Dif), oscillator strength (Fif), lifetime (τ) and extinction coefficient (εmax) of the electronic transition bands of 2-Phenylpropanoic acid (2-PPA) in different solvents.
Table 10. Singlet transition energies of 2-Phenylpropanoic acid in gaseous state.
Table 11. Spectral parameters, Einstein probabilities (Aif and Bif), dipole strength (Dif),oscillator strength (Fif), lifetime (τ) and extinction coefficient (εmax) of the electronic transition bands of 3-Phenylpropanoic acid (3-PPA) in different solvents.
Table 11. The first excited state of the minimum energy structure of 3-PPA, Figure 6, includes the transitions ψm−2→ψm+1, ψm−2-→ψm+2 and ψm−2→ψm+4, Table 12. The major transition in the first excited state is coming mainly from the transition ψm−2 → ψm+1, with eigenvector 0.65683. The calculated transition energy between the ground state to the second excited state lies at 234 nm which is not far from the experimental band position 215 nm in the spectra of 3-PPA, Figure 7. The major transition in the second and third excited states include mainly the transition from ψm to ψm+1 with eigenvectors 0.50780 and 0.46741 respectively. From comparison point of view of the spectral parameters, Table 8, Table 9, Table 11 between IBF and propanioc acid derivatives (2-PPA and 3-PPA), it can be noticed that the spectral parameters of IBF and 2-PPA namely Einstein transition probabilities (Aif and Bif) are close to each other but the dipole strengths Dif, oscillator strengths, fif and extinction coefficients εmax, of IBF are higher than those of 2-PPA but the life times of excitation τ, of 2-PPA are higher than those of IBF. From comparison general point of view, the spectral parameters of IBF and 2-PPA are higher than those of 3-PPA except the excitation life times of 3-PPA which are much higher than those of IBF and 2-PPA.
The blue or green colors (aquamarine) of the copper complexes as in the Cu(ligand)2 complex are due to the of absorption band in the region 600 - 900 nm in the spectra. For Cu(IBF)2 complex spectra, Figure 8, it has an absorption band at about λmax = 700 nm which is attributed to d → d transition  . From Table 13, the d → d transition band of copper ion has high life time of excitation more than 2000 ns which is much higher than the excitation time of the band at about λmax = 280 nm, Figure 8. The Einstein transition probabilities (Aif and Bif), dipole strength Dif, molar absorptivities ε and oscillator strength Fif have much higher values at the absorption band at about λmax = 280 nm more than those at about λmax = 700 nm. From Figure 3, Figure 8, it has been noticed that the first excitation band of IBF at λmax = 263, has been red shifted to λmax = 280 nm in the spectra Cu(IBF)2 complex due to some planarity in the complex molecule, Figure 9.
From Table 14 of the spectral data of Zn-complex it can be concluded that this molecule has an absorption absorbance at the same wavelengths of IBF i.e. at λmax = 230 and λmax = 263 nm as well as in the molar absorptivities of IBF, εmax, are not far from those of Zn-complex spectral data. There is satisfied resemblance between the values of the dipole strengths, Dif and life time of excitation, τ in the spectral data of IBF and the complex Table 8 and Table 14, except the oscillator strengths of IBF spectral data, Table 8, are higher than those of the Zn-complex spectral data.
From the minimum energy structure of Zn-complex, Figure 10, shows that the IBF moieties in the complex are perpendicular to each other therefore the absorbance of the complex is confined in the absorption bands of IBF molecule at 228 and 263 nm, Figure 11 as in the case in the spectra of IBF, Figure 3. This appears clearly from their appreciable resemblance between their spectral data, Table 8, Table 14. This coincidence between the spectra of IBF and Zn-complex is coming out from the perpendicularity of the two IBF moieties in the complex therefore the conjugation overall the molecule is interrupted between the two IBF moieties in the complex.
Figure 6. Minimum energy structure of 3-Phenylpropanoic acid (3-PPA).
Figure 7. Electronic spectra of 3-Phenylpropanoic acid (50.7 mmol・L−1) in (a) EtOH, (b) MeOH, (c) Isopropanol, (d) CHCl3, (e) Cyclohexane, (f) Bidistilled water, and (g) Mineral water.
Figure 8. Electronic spectra of Cu-Ibuprofen complex (1.9 mmol・L−1) in (a) EtOH, (b) MeOH, (c) Isopropanol, (d) CHCl3, and (e) Cyclohexane.
Figure 9. Minimum energy structure of Cu(IBF)2 complex.
Figure 10. Minimum energy structure of Zn(IBF)2 complex,  .
Figure 11. Electronic spectra of Zn(IBF) 2.-2H2O complex (1.17 mmol・L−1) in (a) EtOH, (b) MeOH, (c) Isopropanol, (d) CHCl3, (e) Cyclohexane, and (f) Bidistilled water.
Table 12. Singlet transition energies of 3-Phenylpropanoic acid.
Table 13. Spectral parameters, Einstein probabilities (Aif and Bif), dipole strength (Dif), oscillator strength (Fif), lifetime (τ) and extinction coefficient (εmax) of the electronic transition bands of Cu+2 ion in Cu(IBF)2 complex in different solvents.
Table 14. Spectral parameters, Einstein probabilities (Aif and Bif), Dipole strength (Dif), Oscillator strength (Fif), Lifetime (τ) and Extinction coefficient (εmax) of the electronic transition bands of Zn(IBF)2・2H2O in different solvents.
4.2. Anticancer Effect of Ibuprofen Drug
To deepen the denotation of cancer, it is mutual electron transfer between the nucleic acid bases and electron donor or electron acceptor, i.e. free radicals, drugs even some food like grills and fries. Losing an electron from the nucleic acid bases inside the nucleus produces carcinogenic cell in which the nucleus acts as electron donor to any electron acceptor such as in case of Paracetamol metabolite in the liver, NABQI, Figure 12 having high electron affinity being sufficient to withdraw an electron from guanine in the nucleus of liver cell in absence of glutathione  . Therefore the nucleus looses an electron producing cationic nucleus as a free radical which can behave as positive carcinogenic cell. The positive cancer means that the nucleus lacks an electron due to the mutual electron transfer; therefore it behaves abnormally i.e. cancer. This type of cancer can be treated by drugs having spontaneous electron donor character in a certain condition to compensate the electron deficiency from the nucleus such as Ibuprofen drug in its anionic forms.
After administration of Ibuprofen drug, it passes via human stomach of pH ~ 2 and in full stomach of pH ~ 4 - 5 saving the molecular form of the drug AH. After the drug arrival to gastrointestine of pH ~8 - 9, therefore the anionic form A− of Ibuprofen drug exists side by side with the molecular form AH in intestine. The ionization constant of Ibuprofen dsrug pKa = s4.85, using the relation:
Therefore the ratio between anions A− and molecules AH being equal to 1 approximately. The pH value of human blood equals to 7.4 and its pKa = 5.2, hence the ratio between anions A− and molecules AH is still nearly equal to 1. Therefore Ibuprofen drug exists in the intestine and in the blood as the anionic form A− and the molecular form AH. The existence of free molecule of the drug AH together with the anion A− in the intestine establishes equilibrium between them. This mixture is spontaneous electron donor to the carcinogenic cells rendering them being in normal state.
The ionization energy, Ip, of Ibuprofen drug molecule by DFT method in the stomach being equal to, 6.6804 eV, and decreases when the drug arrives to the small intestine at which the pH value lies between 8 - 9 and the value of the ionization potential decreases to 0.9015 eV, table. Therefore the Ibuprofen drug behaves as spontaneous electron donor in the small intestine. In the same way, the electron affinity of Ibuprofen drug molecule in the stomach is equal to 0.81634 eV, table, which decreases in the small intestine to be −1.4392 eV. This means that Ibuprofen drug anion hasn’t the ability to receive an electron from the IBF molecules. Spontaneous electron donor to nucleic acid bases must fulfill the following condition:
Figure 12. Three path ways of Paracetamol metabolism.
where Ip is the ionization potential energy of the anion and Ea(NAB) is the electron affinity of nucleic acid bases.
From comparison point of view with respect to the nucleic acid bases it has been found the following values of the electronic total energy, ionization energy and electron affinity in the following Table 16.
From Table 15, it has been found that guanine has the lowest Ip, 6.1879 among all the other nucleic acid bases hence it acts as an electron donor forming the cationic nucleus of the carcinogenic cell.
Since Ibuprofen in the small intestine has very low ionization energy, 0.9015 eV and the electron affinity values of nucleic acid bases are higher than that of IBF anion; therefore IBF anions in the presence of IBF molecules can act as spontaneous electron donor to compensate the electron deficiency of the carcinogenic cells in the intestine. The presence of the mixture of A− and AH in the blood gives the chance to inhibit different types of cancers such as protostate, lung and breast cancers  -  .
From the previous Table 16, it can be concluded that the anions of (2PPA) and (3-PPA) have Ip values which are lower than that of the anion of IBF therefore these two compounds can act as spontaneous electron donor and can be used as stronger anticancer more than IBF drug. The heat contents (ΔH) of alteration of AH molecule to its A− anion for the studied compounds (IBF, 2-PPA and 3-PPA) have the following values respectively, 352.393, 347.619 and 349.504 k・scal・mol−1 at 37˚C. Therefore this mixture of molecules and anions of the studied compounds are anticancer  -  .
4.3. Metabolism of IBF Drug
The metabolic activation may be via chiral inversion not only leads to higher therapeutic potency; from another hand it may also cause a great risk of acute kidney failure in patients with renal disorder. The side effect of Ibuprofen includes gastrointestinal disturbance and central nervous system (CNS) depression. All of these adverse effects are found to be mild,  . After arrival of ibuprofen to the blood after absorption from the small intestine to follow up via blood of pH 7.4 toward liver where its metabolism takes place to give ibuprofen acylglucuronide,   , oxidation to produce two major metabolites, 2-hydroxyibuprofen (2HIBF) and carboxy-ibupro- fen (CIBF), Figure 13. The other minor oxidation products are: 1-hydroxyibuprofen (1HIBF), 3-hydroxyibu- profen (3HIBF) and 2-(4-carboxyphenyl) propanoic acid (CPPA) were detected in the human urine. CYP2C9 is the predominant enzyme which is responsible for the oxidation metabolism of Ibuprofen (IBF). The DFT Parameters including total electronic energy (TE), ionization potential (Ip) and electron affinity (Ea) of the metabolite products are given in the following Table 17.
Table 15. DFT/6-31G**Parameters of nucleic acid bases (N.A.B.) and IBF drug.
TE is the total energy, Ip is the ionization energy, Ea is the electron affinity.
Table 16. Anions DFT-parameters of IBF Drug and some analogues.
Figure 13. Metabolic pathways for ibuprofen,   ―HPPA has not been detected.
Table 17. Anions DFT-parameters of IBF drug and some analogues.
From comparative point of view, the Ip’s and Ea’s of the metabolite products of IBF, Table 17, Figure 14, with those of nucleic acid bases, Table 15 using the same method of calculations, it can be concluded that all the values of Ip’s and Ea’s of the IBF metabolite products are consistent with those of the nucleic acid bases. Therefore there isn’t possibility of electron transfer between them and the acidic metabolites tend to have some anionic forms in the slightly basic medium in the human blood, 7.4, hence, the metabolite products of IBF are safe from cancer effect in the liver or in the kidney.
From the different values of Ip’s of nucleic acid bases, Table 15, it has been found that guanine has the lowest Ip value among all the other nucleic acid bases, 6.1879 eV and with respect to that of 1HIBF metabolite, 6.8831 eV. The metabolite 1HIBF has an electron affinity being equal to 1.0591 eV. Therefore guanine acts as electron donor with respect to 1HIBF metabolite and the electron transfer energy between them reaches to 3.841 eV which is corresponding to a wavelength being equal to 322 nm. The electron affinity of uracil, 1.8626 eV, Table 15, is higher than that of 2HIBF, 0.8376 eV, and the ionization energy of uracil, 7.3316 eV is higher than that of 2HIBF, 6.598 eV therefore uracil acts as electron acceptor with respect to 2HIBF metabolite to produce the negative cancer of the anionic nucleus. Therefore the electron transfer energy barrier, 4.734 eV (262 nm)
Figure 14. The minimum energy structures of IBF metabolites in the human body.
prevents the electron transfer between them    leading to the absence of the cancer disease in the liver. From general point of view, guanine due to its lowest Ip and low Ea, acts as electron donor producing positive cancer and uracil due to its high Ea and high Ip, acts as an electron acceptor producing negative cancer. Generally, the anion of 3-PPA is more electron donor than that of IBF in Table 16, since 3-PPA anion has the lowest ionization energy. Therefore it is advisable to use this compound instead of IBF as a drug to inhibit positive cancer diseases.
1) It is good for the health to take Ibuprofen drug regularly to avoid cancers of gastrointestine, protostate, breast and lung.
2) 2PPA and 3-PPA are better as anticancer than Ibuprofen drug.
3) Ibuprofen metal ion complexes are not anti-cancers like anions of IBF, 2-PPA and 3-PPa.
 Torre, L.A., Bray, F., Siegel, R.L., Ferlay, J., Lortet-Tieulent, J. and Jemal, A. (2015) Global Cancer Statistics 2012. CA: A Cancer Journal for Clinicians, 65, 87-108. http://dx.doi.org/10.3322/caac.21262
 Akrami, H., Aminzadeh, S. and Fallahi, H. (2015) Inhibitory Effect of Ibuprofen on Tumor Survival and Angiogenesis in Gastric Cancer Cell. Tumor Biology, 36, 3237-3243.
 Harris, R.E., Beebe-Donk, J., Doss, H. and Doss, D.B. (2005) Aspirin, Ibuprofen, and Other Non-Steroidal Anti-In- flammatory Drugs in Cancer Prevention: A Critical Review of Non-Selective COX-2 Blockade (Review). 13, 559- 583. http://dx.doi.org/10.3892/or.13.4.559
 Harris, R.E., Beebe-Donk, J. and Alshafie, G.A. (2007) Reduced Risk of Human Lung Cancer by Selective Cyclooxygenase 2 (Cox-2) Blockade: Results of a Case Control Study. International Journal of Biological Sciences, 3, 328- 334. http://dx.doi.org/10.7150/ijbs.3.328
 Hanlon, G., Kooloobandi, A. and Hutt, A. (1994) Microbial metabolism of 2-Arylpropanoic Acids: Effect of Environment on the Metabolism of Ibuprofen by Verticillium lecanii. Journal of Applied Bacteriology, 76, 442-447. http://dx.doi.org/10.1111/j.1365-2672.1994.tb01100.x
 Li, T. and Feng, S. (2006) Empirically Augmented Density Functional Theory for Predicting Lattice Energies of Aspirin, Acetaminophen Polymorphs, and Ibuprofen Homochiral and Racemic Crystals. Pharmaceutical Research, 23, 2326-2332. http://dx.doi.org/10.1007/s11095-006-9006-5
 Vueba, M., Pina, M. and de Carvalho, L.B. (2008) Conformational Stability of Ibuprofen: Assessed by DFT Calculations and Optical Vibrational Spectroscopy. Journal of Pharmaceutical Sciences, 97, 845-859. http://dx.doi.org/10.1002/jps.21007
 Okulik, N. and Jubert, A.H. (2006) Theoretical Study on the Structure and Reactive Sites of Three Non-Steroidal Anti-Inflammatory Drugs: Ibuprofen, Naproxen and Tolmetin Acids. Journal of Molecular Structure: THEOCHEM, 769, 135-141. http://dx.doi.org/10.1016/j.theochem.2005.10.061
 Liu, L. and Gao, H. (2012) Molecular Structure and Vibrational Spectra of Ibuprofen Using Density Function Theory Calculations. Spectrochimica Acta Part A: Molecular and Biomolecular Spectroscopy, 89, 201-209. http://dx.doi.org/10.1016/j.saa.2011.12.068
 Frazier, D., Lynch, S. and Carlisle, G. (1981) Synthesis and Magnetic Properties of Bis [2-(4-Isobutylphenyl) Propionato] Copper (II). Journal of Inorganic and Nuclear Chemistry, 43, 2747-2748. http://dx.doi.org/10.1016/0022-1902(81)80610-0
 Tita, B., Stefanescu, M. and Tita, D. (2011) Complexes of Anti-Inflammatory Non-Steroidal Drugs from Carboxylic Acids Family 1. Synthesis and Characterization of Zn (II) Complex with Ibuprofen. Revista de Chimie, 62, 1060-1064.
 El-Shahawy, A. (2014) DFT Cancer Energy Barrier and Spectral Studies of Aspirin, Paracetamol and Some Analogues. Computational Chemistry, 2, 6-17. http://dx.doi.org/10.4236/cc.2014.21002
 El-Shahawy, A. (2011) Computational DFT/CI Spectroscopic Structural Studies of Some Complexes of Benzalbarbituric Acid. Journal of Molecular Structure, 987, 232-240.
 El-Shahawy, A.S., Girgis, M.M. and Ismail, M.T. (1987) Nicotinic Acid and Nicotinamide Electronic Structural Studies. Spectrochimica Acta, 43A, 1371-1375.
 Tan, S.C., Patel, B.K., Jackson, S.H.D., Swift, C.G. and Hutt, A.J. (2002) Stereo-Selectivity of Ibuprofen Metabolism and Pharmacokinetics Following the Administration of the Racemate to Healthy Volunteers. British Journal of Anaesthesia, 32, 683-697.
 El-Shahawy, A. and Hammam, A.S. (2004) CNDO/SCF Molecular Orbital Structural Studies And Charge Transfer Complex Formation between 4,4’Dimethoxydiquinine and Uracil. Bull. Bulletin of the Chemical Society of Ethiopia, 18, 193-204. http://dx.doi.org/10.4314/bcse.v18i2.61444