Abstract
Background
The alternative quantum mechanical description of total energy given by Bohmian theory was merged with the concept of the golden ratio and its appearance as the Heisenberg imbalance to provide a new densitybased description of the valence atomic state and reactivity charge with the aim of clarifying their features with respect to the socalled DFT ground state and critical charge, respectively.
Results
The results, based on the socalled double variational algorithm for chemical spaces of reactivity, are fundamental and, among other issues regarding chemical bonding, solve the existing paradox of using a cubic parabola to describe a quadratic charge dependency.
Conclusions
Overall, the paper provides a qualitativequantitative explanation of chemical reactivity based on more than half of an electronic pair in bonding, and provide new, more realistic values for the socalled “universal” electronegativity and chemical hardness of atomic systems engaged in reactivity (analogous to the atomsinmolecules framework).
Keywords:
Electronegativity; Chemical hardness; Bohmian mechanics; Heisenberg imbalance equation; Slater electronic densityGraphical abstract
Introduction
Recently, the crucial problem regarding whether chemical phenomena are reducible to physical ones has had an increasingly strong impact on the current course of conceptual and theoretical chemistry. For instance, the fact that elements arrange themselves in atomic number (Z) triads in approximately 50% of the periodic system seems to escape custom ordering quantifications [1,2]. The same applies to the following: the fascinating golden ratio (τ) limit for the periodicity of nuclei beyond any physical firstprinciple constants, which provides specific periodic laws for the chemical realm [36]; the fact that atoms have no definite atomic radii in the sense of a quantum operator, and even the Aufbau principle, which, although chemically workable, seems to violate the Pauli Exclusion Principle [7]; at the molecular level, the wellcelebrated reaction coordinate, which, although formally defined in the projective energy space, does not constitute a variable to drive optimization in the course of chemical reactions, appearing merely as a consequence of such reactions [8]; the problem of atoms in molecules [9], i.e., how much of the free atoms enter molecules and how much independency the atoms preserve in bonding; and chemical bonding itself, which ultimately appears to be reinterpreted as a special case of bosonic condensation with the aid of bondons – the quantum bosons of chemical bonding, which, without being elementary, imbue chemical compounds with a specific reality [10,11].
In the same context, the specific measure of chemical reactivity, electronegativity (χ), which lacks a definite quantum operator but retains an observable character through its formal identity with the macroscopic chemical potential χ=μ[12,13], was tasked with carrying quantum information within the entanglement environment of Bohmian mechanics [1417] and has thus far been identified with the square root of the socalled quantum potential χ = V_{Q}^{1/2}[6].
However, the striking difference between an atom as a physical entity, with an equal number of electrons and protons (thus in equilibrium), and the same atom as a chemical object, with incomplete occupancy in its periphery quantum shells (thus attaining equilibrium by changing accepting or releasing electrons), is closely related to the electronegativity phenomenology in modeling chemical reactivity. Moreover, this difference triggers perhaps the most important debate in conceptual chemistry: the ground vs. valence state definition of an atom.
The difficulty may be immediately revealed by considering the variation in the total energy (of the ground and/or valence state – see below for an explanation of their difference) around the physical equilibrium (neutral atom) attained between the release (by ionization, I) and receipt (through affinity, A) of electrons toward chemical equilibrium (in molecules, chemical bonding). Accordingly, the curve passing through these points apparently only behaves as shown in Figure 1(a), while in all systems (with numerical I and A), the obtained interpolating curve presents a minimum toward accepting electrons (see Figure 1(b)), thus confirming the electronegativity concept as a chemical reality, although with a predicted fractional charge (for example, the critical charge N^{*}) on an atom at chemical equilibrium (i.e., not reducible/comprehensible to/by an ordinary physical description of atoms).
Figure 1. The two energy curves (thick lines) for the quantum atom in (a) the apparent or reactive ground state and (b) the shifted or critical ground state.
However, the physicaltochemical paradox continues in an even more exciting fashion as follows. When, in light of the above discussion, electronegativity is recognized with the twopoint limits shown in Figure 1(b), namely [13,18]
the limits represent tangents to a curve that does not describe chemical equilibrium but an excited state driven by the parabolic form
which happens to correspond to the celebrated density functional theory (DFT) working energy expression [13,1921] written in terms of electronegativity and chemical hardness, respectively defined as follows [13,2225]:
The point is that curve (2) is not chemically minimized, although it is very often assumed to be in the DFT invoked by the chemical reactivity literature [13,2629]; however, the curve cannot be considered indicative of a sort of ground state (neither reactive nor critical states of Figure 1). Additionally, by comparing the curves of Figure 1 (a) and (b), the curve of eq. (2) occurs above both the reactive and critical curves of Figure 1; it thus should represent the chemical valence state with which to operate. Therefore, much caution should be taken when working with eq. (2) in assessing the properties of atoms, molecules, atoms in molecules, etc. Nevertheless, this is another case of chemistry not being reducible to physics and should be treated accordingly. It is worth noting that Parr, the “father” of eq. (2) and a true pioneer of conceptual density functional theory [30,31], had tried to solve this dichotomy by taking the “valence as the ground state of an atom in a perturbed environment”. This statement is not entirely valid because perturbation is not variation such that it may be corrected by applying the variational principle to eq. (2), for example. In fact, using such variation should be considered a double variational technique that is necessary to arrive at the celebrated chemical reactivity principles of electronegativity and chemical hardness, as recently shown [32].
The current line of work takes a step forward by employing the double variation of the parabolic energy curve of type (2) to provide the quantum (DFT) valence charge of an atom (say, N^{**}) and to compare it either quantitatively and qualitatively with the chemical critical charge N^{*}. The goal of these efforts is to gain new insight into the valence state and chemical reactivity at the quantum level. To this end, the relation of Bohmian mechanics to the concept of the golden ratio will be essential and will be introduced in the following.
The consequences of the joint consideration of Bohmian mechanics and the golden ratio for the main atomic systems will be explored, and the quantum chemical valence state will be accordingly described alongside the socalled universal electronegativity and chemical hardness, refining the work of Parr and Bartolotti [33] as well as generalizing the previous BohmianBoeyens approach [3,4].
Background methods
Two apparently disjoint theories of matter will be employed to characterize the quantum valence of an atom: Bohmian mechanics – furnishing the main equation for total energy – and the fundamental quantum mechanics through the Heisenberg combined with de Broglie principles providing the waveparticle indeterminacy framework in which the golden ration dependency of Z/N naturally appears as quantifying the valence states of atoms considered the “ground state” of the atomic chemical reactivity.
Bohmian mechanics
Because of the need to reduce Copenhagen’s indeterminacy for quantum phenomena, i.e., by associating it the quantum description of “Newtonian” forms of motion, though by preserving probability densities, quantum averages, etc., the socalled “minimalist” quantum theory may be formulated following the Bohm quantum mechanical program as follows.
One begins with the general eikonal wavefunction form [14]
which represents the midway between wave and particle mechanics because it contains both information regarding HamiltonJacobi theory and the WentzelKramersBrillouin (WKB) approximation [34] through the principal phase function S(r,t) while preserving the amplitude relationship with the systems’ quantum density:
In this framework, the Schrödinger equation,
decomposes into real and imaginary parts. The real part can be expressed as follows:
representing a continuous “fluid” of particles driven by the “guidance” momentum:
moving under a joint external potential V(r) as well as under the socalled quantum potential influence:
The consequences are nevertheless huge. For example, this methodology allows for the interpretation of the trajectories orthogonal to constant surfaces, by cancelling the Laplacian of the wave fronts ∇ _{r}^{2}S(r, t) = 0, which are obtained from eqs. (8) and (9) as the quantum equation of motion:
Equation (11) resembles the classical Newtonian accelerationforce relationship only in a formal way; in fact, it generalizes it: it prescribes acceleration motion even in the absence of an external classical potential. This is essential in explaining why the interquark forces increase with the increase in interquark distances, no matter how great a separation is considered (a specific quantum effect), due to the presence of a quantum potential that does not fall off with distance as V does. It also nicely explains the observed interference patterns in doubleslit experiments in the absence of classical forces. Alike, eq. (11) also appears suited for modeling chemical reactivity for the valence atoms as free particles in a virtually infinite potential environment to characterize their reactive behavior. In this regard, it is worth considering for such atoms the uniform motion by having ∂ p/∂ t = 0 through the timeconstant associated wavefront condition and action S(r=cnst.,t)=cnst. (equivalent with Lagrangean constancy), in all given chemical spacepoints (atomic basins within molecule complex) [35]. This picture is also equivalently to have
applied to eq. (8). By doing so, one obtains
which can be rearranged as follows:
such that the total energy of a the valence system is now entirely driven by the quantum potential:
At this point, one can see that when turning to electronegativity and combining eq. (15) with DFT definition (3), one obtains a generalization of the previous Boeyens formulation [6]:
which is the variation in the quantum potential with electron exchange under a constant classical or external potential.
However, for a quantum characterization of the valence state, we are interested in how the energy described by eq. (15) varies under a quantum potential (10)
when the above relations (6) and (10) are substituted into eq. (15).
It is worth noting that although we obtained the total energy (17) in the Bohmian mechanics context, it showcases a clear electronic density dependency, not under a density functional (as DFT would require) but merely as a spatial function, which is a direct reflection of the entanglement behavior of Bohmian theory through the involvement of a quantum potential. However, in most cases, and especially for atomic systems, eq. (17) will yield numerical values under custom density function realizations.
Golden ratio imbalance for valence states of atoms
Atomic stability and periodicity remain major issues in the structural theories of matter; fortunately, they both have been largely solved by waveparticle (W/P) complementarily quantum behavior; phenomenologically, such relationship can be expressed as “WAVE ⊗ PARTICLE = constant”, while it may be quantized (by Planck’s constant h) in the light of Heisenberg principle as [36]
Remarkably, when fixing the particle’s observable property, say O, while letting wave information to vary, say ΔO, equation (18a) takes the workable form
having as the preeminent realization the Bohrde Broglie formulation ^{a}, leading with the first rationalization of the atomic periodicity [37]. However, when about the atomic chemical reactivity a similar analysis may be provided in terms of the number of electrons to atomic number ratio (N/Z): one may fix the observable (“particle”) character of the reactive atomic system by the ratio itself
while modeling its evolving (“wave”) character by the natural variation of the previous ratio in terms of exchanged electrons respecting the neutral state:
When combining eqs. (19a) and (19b) into eq. (18b) on the lowest quantized state (n_{O}=1), the “ground state” of atomic reactivity that is the atom in its valence state so to speak, and within atomic units’ formulation (i.e. by putting h=1, since the actual reactivity quantification involves only numbers with no dimension), one has the so called Heisenberg imbalance equation for valence atoms
that can be rewritten as
Eq. (20b) has the elementary acceptable solution
which establishes, the direct “chemical” connection between the number of electrons and the atomic charge by means of the golden ratio
generalizing the “physical” connection between nuclear (cosmic) synthesis at high pressure and atomic stability in the gas phase (Z=N); one has therefore the actual physicaltochemical electronic charge – atomic number relationships
Worth remarking the results of type (20) and (22), here based on chemical reactivity specialization of Heisenberg type equations (18a) and/or (18b), were previously obtained at the level of neutronprotonic imbalance, inside the atomic nuclei, based on wellfounded empirical observations [6]. The present golden ratio appearance is ultimately sustained also by the deviation from the N=Z condition for socalled “quark atoms” (as another way in considering the atoms in a quantum valence state), earlier identified as true matter’s entities responsible for matter’s reactivity at the atomic level [38].
Therefore the atomic structure branching (22) can be regarded as the present golden ratio extension to valence atom and as such employed; actually, its consequences regarding the characterization of the quantum valence states of atoms within the Bohmian quantum potential are the main aims of the present endeavor and will be discussed next.
Atomic implementation and discussion
On Slater density for valence atoms
Density is considered a “goldmine” in current computational and conceptual quantum chemistry due to its link with observable quantities, energy density functionals in particular, as celebrated by DFT [13,20,39,40]. However, to quantitatively approach the chemical phenomenology presented in Figure 1, involving the ionizationtoaffinity atomic description, the general Slater [33] density (involving the orbital parameter ξ dependency) will be here employed for the first trial on modeling the combined Bohmian and goldratio features of valence atom; it assumes the general (trough still crude) working form:
For the reactivity at the valence atomic level, or for some outer shell (n) considered at the atomic frontier, one may assume almost electronic free motion or at least electronic motion under almost vanishing nuclear potential V(r); this way the density (23a), while entering the quantum potential (10) recovers the negative kinetic energy by the virial identity (14). Analytically, since eqs. (6), (10) and (23a), one has ∇ _{r}^{2}ρ^{1/2} = ξ^{2}ρ^{1/2} and the actual valence atomic virial realization looks like
Equation (24) leaves with the identity:
that may be further rewritten with the help of the atomic Bohrde Broglie relationship (see the note ^{a}) to provide the atomic frontier radii shelldependency
Remarkably, the same result is obtained when employing a far more reach atomic shell structure description, namely when starting with the full atomic radial Schrödinger density [25]
and imposing the nullgradient condition [41], ∇_{r}ρ_{n}(r, ξ) = 0, in accordance with the celebrated Bader condition of electronic flux of atomsinmolecules [9,42], to yield:
The identity between eqs. (25b) and (25c) gives sufficient support to the present Slater density approach eq. (23a) in modeling the valence atoms or the atoms at their frontiers approaching reactivity (i.e. atomsinmolecules complexes by chemical reactions).
Quantum chemical bonding and reactivity indices
Once convinced by the usefulness of the Slater density form (23a) for the present valence atomic analysis, one will next employ it under the so called ParrBartolotti form [33]
such that to obey the Nnormalization condition, as required by DFT [4347],
by applying the Slater integral recipe
It nevertheless showcases the parametric ξ dependency that can be smeared out by considering the variational procedure
upon applying the total atomic energy
where the components are individually evaluated within a radial atomic framework with the respective results for [21,48]
● kinetic energy
● nucleuselectronic interaction
● interelectronic interaction (see also Appendix)
With these results, the optimum atomic parameter is quantified by the electronic number as follows:
which immediately releases the working electronic density
Having the completely analytical density in terms of number of reactive electrons as in eq. (33), worth pointing here on the so called sign problem relating with its variation, e.g., its gradient, the gradient of its square root, etc. Although this problem usually arises in density functional theory when specific energy functionals are considered in gradient forms, see for instance ref. [49], there is quite instructive discussing the present behavior and its consequences.
For instance, one can adapt either eqs. (25b) or (25c) through considering the present form (32) for the orbital exponent to be
Here, one combines the frontier and maximum atomic radii with atomsinmolecules phenomenology, as above indicated, to arrive to the present identification for the number of valence electrons possible to be involved in the same chemical bonding state as being N_{bonding} in (25d). Accordingly, the Figure 2 reveals interesting features of the present SlaterParrBartolotti atomic density with quantum potential:
● the fact that the (covalent) bond length is proportional to the atomic radii and in inverse correlation with bonding order is well known [50], and this it is also nicely reflected in eq. (25d); however, changing the sign to negative radii as surpassing the threshold 21/5 and fixing in fact the limit N_{bonding}=4, is consistent with maximum bond order met in Nature; it is also not surprising this selfreleased limit connects with golden ratio by the goldenspiral optimization of bondorder [51]; more subtle, it connects also with the 4π symmetry of two spherical valence atoms making a chemical bond (Figure 2, inset): such “spinning” reminds of the graviton symmetry [52] (the highest spherical symmetry in Nature, with spin equal 2) and justifies the recent treatments of chemical bonding by means of the quasiparticles known as bondons [10,53], as well as the use of the 4D complex projective geometry in modeling the chemical space as a nonEuclidian one, eventually with a timespace metrics including specific “gravitational effects” describing the bonding [51];
● the “gap” between the atomic systems contributing 2 to 3 electrons to produce chemical
bond is about double of the golden ratio,
Figure 2. Representation of the bonding length as a function of bonding electrons from valence atoms in molecule(s), based on eq. (25d), while marking the double golden ratio 2τ gap between the bonding lengths of the second and third bonding order, as well as the forbidden chemical bonding region for N_{bonding} ≥21/5 for the electrons participating in the same bonding. Further connection of chemical bonding and the 4D space to model it is suggested by the inset picture illustrating the 2fold (4π) spinning symmetry of the adduct atom respecting the bonding direction, after [51].
Having revealed the chemical bonding information carried by the density (33) when considered for combined valence atomsinmolecules, it is next employed on energetically describing the atomic reactivity as a propensity for allowing electronic exchanging and bonding. As such, it leaves the total quantum (Bohmian) energy in (17) with the compact form
Note that the actual working total energy is not that obtained by replacing the density (33) in eqs. (31a)(31c) and then in total energy (30) because here the doublevariational procedure was considered; that is, the first optimization condition was considered as in eq. (29), and the resulting (optimum) density (33) was then employed in the quantum energy (17), which in turn was obtained by applying the variational eq. (12) to the perceived phase transition in the Bohm eikonal wavefunction (5). To emphasize the accuracy of eq. (17) over that of (30) with density (33), when one considers the last case, eq. (30) yields the following nonquadratic form for energy:
which is not appropriate for describing the valence state of an atom, as eq. (2) prescribes, despite being similar in form to the Bohmianbased result of eq. (34a). Thus, the previous limitation of the ParrBartolotti conclusion [33] and the paradox raised in describing the valence (parabolically) state with the optimized atomic density (33) are here solved by the double (or the orthogonal) variational implementation, as recently proved to be customary for chemical spaces [32]. In the light of this remark one may explain also the sign difference between the “physical” energy (34b) and that obtained for the “chemical” situation (34a): through simple variational procedure for “physical” energy (30) the result (34b) is inherently negative – modeling systems stability in agreement with the upper branch of eq. (22), whereas the double variational algorithm employing optimized density (33) into the Bohmian shaped energy (17) it produces the positive output (34a) associated with activation energy characteristic for chemical reactivity corresponding to the lower branch of eq. (22).
Therefore, to be accurate, one should consider the quantum potential related optimized energy (34a) instead of simply the orbital optimized one of eq. (34b). Therefore, assuming that eq. (34a) appropriately describes the atomic valence state in DFT (see the upper/reactive curve in Figure 1b), the next task is to search for the quantum valence charge for which the valence energy approaches its optimum value (or the “ground state” of the atomic chemicalreactivity, i.e. the previously goldenratio quantification of the valence atomic state); to this aim, at this point, one can employ the golden ratio relationship (21a) and first rewrite eq. (34a) as
which is minimized at the value
However, one must again apply the doublevariational procedure, now in terms of number of electrons, i.e., reconsidering eq. (36) with the golden ratio at the reactive (chemical) electronic level of eq. (22) such that a second equation is formed
with the positive solution
This expression avails of the significance of the maximum number of electrons, for a given atom, possibly engaged in a reactive environment by either (or both) accepting or (and) ceding electrons to or from its valence state, see Table 1.
Table 1. Synopsis of the critical charges in the physical ground state (N^{*}) as well as for chemical reactive (valence) state (N^{**}) for atoms of the first four periods of the periodic table of elements, as computed from the minimum point of associated interpolations of ionization and electronic affinities[33]and of eq. (38), respectively
The result of this process is different from the expected physical result (N_{STABIL}=Z) according to the upper branch of eq. (22), which is higher than the physical one until reaching the carbon system (Z_{INTRCHANGE}=6.8), while continuing below it thereafter (see Figure 3).
Figure 3. The comparative shapes of the valence electrons to be engaged in chemical reactivity (continuous curve) computed using eq. (38) based on the combined optimal Bohm total energy (35) with the golden ratio imbalance of eq. (22), respecting the stable physical case (dotdashed curve), and of their differences (dashed curve); all originate at the 0^{th}atom (the neutron, Z=0).
The above interchange (effective) atomic number through which the chemical (reactive) state is associated with lower charge respecting the physical state may be also be found at the energetic level based on quantum equation (34a), as specialized for the two branches of Figure 3 for the N(Z) dependence. Thus, the chemical (reactive) state takes the analytic form
and interchanges with the ground state E_{Q1}(N_{STABLE} → Z) at the points {3.5,6.8}, as observed also from Figure 4; however, the interchanging point beyond which all chemical atomic systems are more stable in the chemical or reactive state than in the physical ground state is consistently recovered.
Figure 4. The same comparative shapes shown in Figure3, here at the level of energy (34a) specialized for the reactive and the stable N(Z) dependencies of Figure3; the various plots successively display increasingly large atomic Zranges to better emphasize the chemical vs. physical behavior (see text).
Nevertheless, the energetic analysis also reveals the atomic systems Be, B and C to be situated over the corresponding physical stable states; this may explain why boron and carbon present special chemical phenomenology (e.g., triple electronic bonds and nanosystems with long Cbindings, respectively), which is not entirely explained by ordinary physical atomic paradigms [5560].
The energetic discourse may be complete with the electronegativity and chemical hardness evaluations by applying the DFT definitions (3) and (4) to physical and chemical energies, respectively. In the first case, expression (34b) is applied to provide the following socalled “universal” forms of Parr and Bartolotti [33]:
The result, nevertheless, appears to be an unusually higher increase in chemical hardness than in electronegativity, which certainly cannot be used to model a reactiveengaged tendency because it is more stable (by chemical hardness) than reactive (by electronegativity); it is, however, consistent with the physical stability of the system, provided by the single variational procedure through which eq. (34b) was produced.
Instead, to chemically model reactivity, the double variation procedure is applied and eq. (34a) is substituted into eqs. (3) and (4), though by considering also the double reactive procedure for charge as well, i.e., by considering eq. (38) with the golden ratio information of (22) to respectively yield the results
Remarkably, the actual electronegativity of (42) obtained by the quantum Bohm and golden ratio double procedure yields sensible results similar to those of the single variational approach (40); however, the chemical hardness of (43) is approximately 5fold lower than its “stable” counterpart (41), affirming therefore the manifestly reactive framework it produces – one described by a quadratic equation (34a) instead of a cubic one (34b).
Charge waves in gauge chemical reactivity
Finally, one considers the chemical reactivity discussion as based on the gauge reaction that equilibrates the chemical bond by symmetrical bond polarities [25]
such that the reactive electrons are varied on the reunited intervals of eq. (1); such analysis was previously employed to fundament systematic electronegativity and chemical hardness definitions by the averaging (through the integration) factor
along the reaction path accounting for the acidic (electron accepting, 0 ≤ N ≤ +1) and basic (electron donating, –1 ≤ N ≤ 0) chemical behaviors.
In this scaled (gauge) context of reactivity, the foregoing discussion is dedicated to investigating the link between the critical ground state charge (N^{*}) and the valence or reactive state (N^{**}). While the first appears as a consequence of naturally fitting the three points in Figure 1 (the ionization, neutral and affinity states), with the effect of biasing the minimum of the energetic curve in Figure 1b with respect to the apparent ParrDFT curve in Figure 1a, and is thus derived graphically (see Figure 5), the valence charge is based on the combined quantum energy and golden ratio information in eq. (38). Both are reported for the indicated number of atomic systems of the periodic table of elements in Table 1. One notes, for instance, that while the critical ground state charge N^{*} always lies in the range [0.5,1], the valence charge N^{**} may span the interval [0,1]; one may interpret such behavior as being associated with the difference between the fraction Â½ and integer “1” in driving the principles of chemical reactivity and the electrophilicity equalization principle in particular, when the “quantum transition” 1/2→1 is required in the energy exchange of chemical systems for it to be valid for both electronegativity and chemical reactivity principles [61]; nevertheless such scaling it is equivalent with above acidicbasic gauge averaging of eq. (44b). This way, the valence charge problem may be extended to the interval [0,2], at its turn seen as a gauge transformation of the chemical reactivity charge domain [−1, +1], where one reencounters the challenging problem of whether the “One electron is less than half what an electron pair is” [62], the response to which is generally complex but may here be approached through the following steps.
First, by employing the data presented in Table 1, one constructs the socalled “continuous” ground and valence charge states by appropriately fitting over the first four periods of elements, here restrained to 10^{th}order polynomials. This is performed by interpolating every three points of the 32 elements presented in Table 1, although by spanning the atomic number range Z ∈ [1, 53], thus yielding (see also the allied representations of Figure 6):
Equations (45a) and (45b) are then combined into a sort of special charge wave function based on their difference on the golden ratio scale (see Figure 6 for graphical representation)
with the peculiar property that its squareintegrated form over the Zrange of interpolation gives
The result (47) has the following conceptual fundamental quantitative interpretation: the difference between the ground and valence optimum charges is regulated by the golden ratio scale, or in other terms,
such that it provides a sort of normalization corrected by the golden ratio value; it also fulfills the interesting relationship:
In any case, the present analysis provides the qualitative result that the difference between the critical ground state and optimal valence charges is more than half of an electronic pair, giving rise to the significant notion that chemical reactivity is not necessarily governed by a pair of electrons but governed by no less than half of a pair and is related to the golden ratio (τ > 0.5).
However, fractional values in general and those related to the golden ratio particular, may be interpreted as a consistent manifestation of the quantum mechanical (i.e., wave functional) approach of chemical phenomena, here at the reactivity level. Moreover, the quadratic critical charge function (46), as shown in Figure 7, clearly reveals that a higher contribution to electronic pair chemistry is given by the third period of elements and by the third and fourth transitional elements in particular, a result that nicely agrees with the geometrical interpretation of the chemical bond, particularly the crystal ligand field paradigm of inorganic chemistry [9].
Figure 7. The linear and quadratic charge “wave function” of eq. (46).
Also a local analysis of the type of charge that is dominant in atomic stability, i.e., the critical physical ground state or the chemical valence reactive state based on eqs. (45a) and (45b), respectively, may be of considerable utility in refined inorganic chemistry structurereactivity analysis. To the same extent, it depends on the degree of the polynomials used to interpolate the critical and valence charges over the concerned systems; however, through the present endeavor, we may assert that the analysis should be of the type (48), which in turn remains a sort of integral version of the imbalance equation (20a), in this case for the groundvalence charge gap states of a chemical system.
Conclusions
Aiming to hint at the solution to the current debate regarding the physical vs. chemical definition of an atom and as a special stage of a larger project regarding quantum chemical orthogonal spaces, the present work addresses the challenging problem of defining and characterizing valence states with respect to the ground state within conceptual density functional theory. We are aware of the earlier warnings raised by Parr and Bartolotti and others [18,33,63] regarding the limits of density functional theory and of the total energy of atomic systems combined with a Slaterbased working density to provide a quadratic form in terms of system charge, as required by the general theory of chemical reactivity of atoms and molecules in terms of electronegativity and chemical hardness. Fortunately, we discovered that the Bohmian form of the total energy of such atomic systems provides, instead, the correct behavior, although it is only densityfunctiondependent and not a functional expression. Moreover, this finding was reached through the socalled double variational procedure, which, as emphasized earlier, was likely to reproduce the chemical reactivity principles of electronegativity and chemical hardness in an analytical manner; however, such a double analytical variational approach is consistent with the recent advanced chemical orthogonal spaces approaches of chemical phenomenology [64] as being at least complementary to the physical description of manyelectronic systems when they are engaging in reactivity or equilibrium as the atomsinmolecules Bader theory prescribes [9,42]. With the present Bohmian approach, the total energy is in fact identified with the quantum potential, thus inherently possessing nonlocality and appropriate reactivity features, which are manifested even over long distances [10,11,53]; this also generalizes the previous Boeyens electronegativity formulation of electronegativity [5,6] from the direct relationship between a quantum potential and its charge derivative. The double algorithm was also implemented to discriminate the valence from the ground state charges, this time by using the golden ratio imbalance equation as provided by adaption of the Heisenberg type relationship to chemical reactivity for atoms. This corresponds to an analytical unfolding of the physical and chemical imbalance of the electronic charge stability of atomic systems, paralleling the deviation from the equal electrontoproton occupancy in physical systems toward electron deficiency in the valence states of chemical systems. This dichotomy was implemented by the golden ratio presented in eq. (22). As a consequence, the difference between valence and ground state charge systems is naturally revealed and allows for the explanation of chemical reactivity and bonding in terms of fractional electron pairs, althrough driven by the golden ratio under the socalled physicaltochemical charge difference wave function and associated normalizations, all of which represent elaborated or integral forms of the basic imbalance atomic equation. The present results are based on 10^{th}order polynomial fitted over 32 elements from the first 54 elements of the first four periods of periodic table of elements and can be further pursued by performing such systematic interpolations that preserve the golden ratio relationships, as advanced herein; they may also provide a comprehensive picture of how valence electrons may always be projected/equalized/transposed into ground state electrons within the perspective of further modeling chemical reactions when chemical reactivity negotiates the physical molecular stabilization of atoms in molecules.
Endnotes
^{a} For circular orbits, the lowest ones in each atomic shells – including the valence ones, one has ΔO=Δr=2πr, with r the orbital radii thereof, while O=p is the fixed particle’s momentum on that orbit; therefore, when combined into eq. (18b) they provide the celebrated Bohrde Broglie relationship rp=nħ solving the atomic spectra of Hydrogen atom in principal quantum numbers (n).
Appendix: Semiclassical interelectronic energy
For the interelectronic interaction, see Figure 8; in evaluating V_{ee}[ξ] of eq. (31c), the twoelectronic density is approximated by the Coulombic two monoelectronic density product, thus neglecting the secondorder density matrix effects associated with the exchangecorrelation density.
However, for the analytical evaluation of the electron–electron repulsion energy using the density (23b), much care must be taken. For instance, one has to use the electrostatic Gauss theorem, which states that the classical electrostatic potential outside a uniform spherical shell of charge is just what it would be if that charge were localized at the center of the shell and that the potential everywhere inside such a shell is that at the surface, [21,48] see Figure 8. Therefore, the electronic repulsion energy becomes
which recovers the expression presented by eq. (31c), when the Slater integral type of Eq. (28) is also employed. Note that the electron–electron repulsion term was written by also considering the FermiAmaldi (N1)/N factor [13], which ensures the correct selfinteraction behavior: when only one electron is considered, the selfinteraction energy must be zero, V_{ee} (N→1)→0.
Competing interests
The author declares he has no competing interests.
Acknowledgements
This work was supported by CNCSUEFISCDI agency through the research project TE16/20102013 within the PN IIRUTE20091 framework. Inspiring discussions with Profs. Boeyens (University of Pretoria, South Africa) and von Szentpaly (Stuttgart University, Germany) are kindly acknowledged. Constructive referees’ comments and stimulus is also sincerely thanked. This paper is dedicated to Prof. Robert G. Parr for his pioneering quantum work on atomic valence states.
References

Putz MV: Big chemical ideas in the context: the periodic law and the Scerri’s Periodic Table.

Scerri ER: The Periodic Table – Its Story and Its Significance. OxfordNew York: Oxford University Press; 2007. PubMed Abstract

Boeyens JCA: Emergent Properties in Bohmian Chemistry. In Quantum Frontiers of Atoms and Molecules. Edited by Putz MV. New York: Nova Publishers Inc; 2011:191.

Boeyens JCA: New Theories for Chemistry. Amsterdam: Elsevier; 2005.

Boeyens JCA: Chemistry from First Principles. HeidelbergBerlin: Springer; 2008.

Boeyens JCA, Levendis DC: Number Theory and the Periodicity of Matter. HeidelbergBerlin: Springer; 2008.

Kaplan IG: Is the Pauli exclusive principle an independent quantum mechanical postulate?
Int J Quantum Chem 2002, 89:268276. Publisher Full Text

Scerri ER: Just how ab initio is ab initio quantum chemistry?

Bader RFW: Atoms in Molecules  A Quantum Theory. Oxford: Oxford University Press; 1990.

Putz MV: The bondons: The quantum particles of the chemical bond.
Int J Mol Sci 2010, 11:42274256. PubMed Abstract  Publisher Full Text  PubMed Central Full Text

Putz MV: Quantum Theory: Density, Condensation, and Bonding. Toronto: Apple Academics & CRC Press; 2012.

Parr RG, Donnelly RA, Levy M, Palke WE: Electronegativity: the density functional viewpoint.
J Chem Phys 1978, 68:38013808. Publisher Full Text

Parr RG, Yang W: Density Functional Theory of Atoms and Molecules. New York: Oxford University Press; 1989.

Bohm D: A suggested interpretation of the quantum theory in terms of “hidden” variables. I.
Phys Rev 1952, 85:166179. Publisher Full Text

Bohm D: A suggested interpretation of the quantum theory in terms of “hidden” variables. II.
Phys Rev 1952, 85:180193. Publisher Full Text

Bohm D, Vigier JP: Model of the causal interpretation of quantum theory in terms of a fluid with irregular fluctuations.
Phys Rev 1954, 96:208216. Publisher Full Text

Cushing JT: Quantum Mechanics – Historical Contingency and the Copenhagen Hegemony. Chicago & London: The University of Chicago Press; 1994. PubMed Abstract  Publisher Full Text

Von Szentpály L: Modeling the charge dependence of total energy and its relevance to electrophilicity.
Int J Quant Chem 2000, 76:222234. Publisher Full Text

Ayers PW, Parr RG: Variational principles for describing chemical reactions: the Fukui function and chemical hardness revisited.
J Am Chem Soc 2000, 122:20102018. Publisher Full Text

Geerlings P, De Proft F, Langenaeker W: Conceptual density functional theory.
Chem Rev 2003, 103:17931874. PubMed Abstract  Publisher Full Text

Putz MV: Contributions within Density Functional Theory with Applications in Chemical Reactivity Theory and Electronegativity. Parkland: Dissertation.com; 2003.

Parr RG: Density functional theory.
Annu Rev Phys Chem 1983, 34:631656. Publisher Full Text

Parr RG, Pearson RG: Absolute hardness: companion parameter to absolute electronegativity.
J Am Chem Soc 1983, 105:75127516. Publisher Full Text

Putz MV: Absolute and Chemical Electronegativity and Hardness. New York: Nova Publishers Inc.; 2008.

Putz MV: Systematic formulation for electronegativity and hardness and their atomic scales within density functional softness theory.
Int J Quantum Chem 2006, 106:361389. Publisher Full Text

Chattaraj PK, Parr RG: Density functional theory of chemical hardness.
Struct Bond 1993, 80:1125. Publisher Full Text

Chattaraj PK, Sengupta S: Popular electronic structure principles in a dynamical context.

Chattaraj PK, Maiti B: HSAB principle applied to the time evolution of chemical reactions.
J Am Chem Soc 2003, 125:27052710. PubMed Abstract  Publisher Full Text

Chattaraj PK, Duley S: Electron affinity, electronegativity, and electrophilicity of atoms and ions.
J Chem Eng Data 2010, 55:18821886. Publisher Full Text

Ayers PW, Parr RG: Variational principles for describing chemical reactions: reactivity indices based on the external potential.
J Am Chem Soc 2001, 123:20072017. PubMed Abstract  Publisher Full Text

Kohn W, Becke AD, Parr RG: Density functional theory of electronic structure.
J Phys Chem 1996, 100:1297412980. Publisher Full Text

Parr RG, Bartolotti LJ: On the geometric mean principle of electronegativity equalization.
J Am Chem Soc 1982, 104:38013803. Publisher Full Text

Kleinert H: Path Integrals in Quantum Mechanics, Statistics, Polymer Physics, and Financial Markets. 3rd edition. Singapore: World Scientific; 2004.

Guantes R, Sanz AS, MargalefRoig J, MiretArtés S: Atom–surface diffraction: a trajectory description.
Surf Sci Rep 2004, 53:199330. Publisher Full Text

Putz MV: On Heisenberg uncertainty relationship, its extension, and the quantum issue of waveparticle duality.
Int J Mol Sci 2010, 11:41244139. PubMed Abstract  Publisher Full Text  PubMed Central Full Text

Pauling L, Wilson EB: Introduction to Quantum Mechanics with Applications to Chemistry. New York: Dover Publications; 1985.

Lackner KS, Zweig G: Introduction to the chemistry of fractionally charged atoms: electronegativity.
Phys Rev D 1983, 28:16711691. Publisher Full Text

Hohenberg P, Kohn W: Inhomogeneous electron gas.
Phys Rev 1964, 136:B864B871. Publisher Full Text

Putz MV: Density functionals of chemical bonding.
Int J Mol Sci 2008, 9:10501095. PubMed Abstract  Publisher Full Text  PubMed Central Full Text

Ghosh DC, Biswas R: Theoretical calculation of absolute radii of atoms and ions. Part 1. The atomic radii.
Int J Mol Sci 2002, 3:87113. Publisher Full Text

Bader RFW: Definition of molecular structure: by choice or by appeal to observation?
J Phys Chem A 2010, 114:74317444. PubMed Abstract  Publisher Full Text

Dreizler RM, Gross EKU: Density Functional Theory. Heidelberg: Springer Verlag; 1990.

Kryachko ES, Ludena EV: Energy Density Functional Theory of Many Electron Systems. Dordrecht: Kluwer Academic Publishers; 1990.

Cramer CJ: Essentials of Computational Chemistry. Chichester: Wiley; 2002.

Capelle K: A bird'seye view of densityfunctional theory.
Braz J Phys 2006, 36:13181343. Publisher Full Text

Jensen F: Introduction to Computational Chemistry. Chichester: John Wiley & Sons; 2007.

Parr RG: The Quantum Theory of Molecular Electronic Structure. ReadingMassachusetts: WA Benjamin, Inc.; 1972.

Cohen AJ, MoriSánchez P, Yang W: Challenges for density functional theory.
Chem Rev 2012, 112:289320. PubMed Abstract  Publisher Full Text

Petrucci RH, Harwood WS, Herring FG, Madura JD: General Chemistry: Principles & Modern Applications. 9th edition. New Jersey: Pearson Education, Inc.; 2007. PubMed Abstract  Publisher Full Text

Boeyens JC, Levendis DC: The structure lacuna.
Int J Mol Sci 2012, 13:90819096. PubMed Abstract  Publisher Full Text  PubMed Central Full Text

Hawking S: The Universe in a Nutshell. New York: Bantam Books; 2001.

Putz MV, Ori O: Bondonic characterization of extended nanosystems: application to graphene's nanoribbons.

Boeyens JCA: A molecular–structure hypothesis.
Int J Mol Sci 2010, 11:42674284. PubMed Abstract  Publisher Full Text  PubMed Central Full Text

March NH: Electron Density Theory of ManyElectron Systems. New York: Academic; 1991.

Wentorf RH Jr: Boron: another form.
Science 1965, 147:4950. PubMed Abstract  Publisher Full Text

Eremets MI, Struzhkin VV, Mao H, Hemley RJ: Superconductivity in Boron.
Science 2001, 293:272274. PubMed Abstract  Publisher Full Text

van Setten MJ, Uijttewaal MA, de Wijs GA, de Groot RA: Thermodynamic stability of boron: the role of defects and zero point motion.
J Am Chem Soc 2007, 129:24582465. PubMed Abstract  Publisher Full Text

Widom M, Mihalkovic M: Symmetrybroken crystal structure of elemental boron at low temperature.

Putz MV (Ed): Carbon Bonding and Structures: Advances in Physics and Chemistry. DordrechtLondon: Springer Verlag; 2011.
Cataldo F, Milani P (Series Editors): Carbon Materials: Chemistry and Physics, Vol. 5.

Putz MV, Mingos DMP (Eds): Applications of Density Functional Theory to Chemical Reactivity. BerlinHeidelberg: Springer Verlag; 2012. [Struct Bond]

Ferreira R: Is one Electron less than half what an electron pair is?
J Chem Phys 1968, 49:24562457. Publisher Full Text

Bergmann D, Hinze J: Electronegativity and charge distribution.
Struct Bond 1987, 66:145190. Publisher Full Text

Putz MV: Chemical Orthogonal Spaces. Kragujevac: Kragujevac University Press; 2012.
[Gutman I (Series Editor): Mathematical Chemistry Monographs, Vol. 14].