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Electrochimica Acta 46 (2001) 12771284
On the adsorption of pure ethylene glycol on mercury
Claudio Fontanesi a,*,1, Luca Benedetti1 a, R. Andreoli1 a, Marcello Carla b
a Department of Chemistry, Uni6ersity of Modena and Reggio Emilia, Via Campi 183, 41100 Modena, Italyb Department of Physics, Uni6ersity of Florence, L. go E. Fermi 4, 50125 Florence, Italy
Received 30 June 2000; received in revised form 26 October 2000
Abstract
The standard Gibbs energy of adsorption of pure liquid ethylene glycol (EG) on mercury is assessed to range
between 50 and 60 kJ mol1, about twothree times with respect to water (21 kJ mol1). This evidence is
obtained on the basis of a series of indirect and independent experimental results. Moreover, ab-initio calculations are
performed to account for the interaction energy relating the isolated EG molecule and a cluster of seven (or four) Hg
atoms: three different geometrical approaches of the EG molecule with respect to the cluster are considered (top,
hollow, bridge) as well as three EG conformations (trans, cis, cis-OH, the last one with an intramolecular hydrogen
bond). The deepest minimum in the energy versus (Hgcluster EGmolecule) distance potential energy curve, amounting to
80 kJ mol1, is obtained in the case of the cis conformation of EG. In particular, it is found that this stabilizing
energy is essentially due to the oxygenmercury atoms interaction, giving rise also to an appreciable charge transfer
coefficient from the EG molecule to the Hg cluster. Finally, in this conformation, the EG adsorbed layer is also
stabilized by an attractive energy term effective among vicinal interacting molecules. 2001 Elsevier Science B.V. All
rights reserved.
Keywords: Ethylene glycol; Mercury; Adsorption; Ab-initio calculation
www.elsevier.nl/locate/electacta
1. Introduction
The comparative study of the adsorption of a series
of aromatic derivatives on mercury in the same experi-
mental conditions, but from two solvents, water and
ethylene glycol (EG) [1], has assured the reliability of
the so called Intrinsic adsorption Gibbs free energy,
DGINT a value related to the virtual process [2]:
Adsorbate(pure)+Hg X Hg(Adsorbate)
in that this value is really intrinsic, i.e. it can be fully
related to the molecular properties (experimental and
calculated) of the adsorbed species alone, only when
solvation effects in the adsorbed state are negligible
[3,4]. The electrochemical and thermodynamic proce-
dure to obtain this evidence has, as a direct conse-
quence, that the DGINT of EG on mercury, related
again to the virtual process: EG(l,pure)+Hg X Hg(EG)
should amount to $51 kJ mol1, with no other
direct experimental evidence. Taking into account theadsorption of water on uncharged mercury,
H2O(l,pure)+Hg X Hg(H2O), a value ofDGINT$21
kJ mol1 has been achieved by a direct measurement
from the vapor phase of water and using a classical
thermodynamic cycle [5,6], a confirmation ofDGINT for
EG is crucial to preview, for example, the adsorbability
of EG on Hg from its aqueous solution and to asses its
greater interaction, with respect to water, on a molecu-
lar level, toward the mercury atoms as suggested by the
great and negative DGEG value as previously estimated.
* Corresponding author. Tel.: +39-059-378462; fax: +39-
059-373543.
E-mail address: [email protected] (C. Fontanesi).1 ISE member.
0013-4686/01/$ - see front matter 2001 Elsevier Science B.V. All rights reserved.
PII: S 0 0 1 3 - 4 6 8 6 ( 0 0 ) 0 0 7 1 2 - X
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C. Fontanesi et al. /Electrochimica Acta 46 (2001) 127712841278
Table 1
Hardness (p), softness (|) and absolute electronegativity ()
for the three components of the system Hg, H2O, EGa
pcalc | exppexp |calc exp calc
0.18Hg 5.54 4.9
8.7H2O 0.109.5 0.11 3.1 3.5
7.2 0.14EG (cis) 3.9
7.36 0.136EG (cis-OH) 3.957.39 0.135 3.96EG (trans)
a For EG three comformers are considered: i.e. the cis, then
a cis form characterized by an intermolecular OH bond and
trans.
the application of the hard and soft concept [8] to the
competitive three-component system: water Hg EG
(i.e. who is substituted by who on the uncharged mer-
cury surface); (d) a quantum mechanical calculation of
the interaction energy between one EG molecule and a
sheet composed of seven Hg atoms, calculated by the
similar performance of a water molecule on a mercury
layer [9,10].
2. Calculation and procedure
The mercury surface has been simulated using clus-
ters of seven Hg atoms for the on top disposition and
of four Hg atoms for the hollow and bridge site
positions.
Three different conformers for the EG molecule has
been considered in the potential energy surfaces (PESs)
calculations: cis, trans, and cis-OH (i.e. featuring an
intramolecular hydrogen bond).
The geometry of the three EG conformers has been
fully optimized at the RMP2/6-31g* level of the theory.The geometrical parameters of the Hg cluster, inter-
atomic HgHg distance (0.3 nm) and hexagonal sym-
metry, are taken from an experimental X-ray
diffraction study on liquid Hg by Bosio et al. [11]. The
Hg cluster EG molecule PESs calculations were car-
ried out by means of the GAUSSIAN 94 program, using
a LanL2DZ basis set with MP2 (frozen cores) electron
correlation [12]. The PESs were calculated keeping both
the Hg cluster and EG internal geometries frozen, while
varying their reciprocal distance and orientation.
The MNDO Hamiltonian, as implemented in the
AMPAC program [13], was used to calculate Mulliken
atomic net charges and the HOMO and LUMO energy
values of water and EG; the latter to be used in the
application of the hard and soft concept (Table 1).
This choice allows the comparison with previously pub-
lished results [14].
For both EG and water, the interaction energy active
between a couple of molecular species, A A, is calcu-
lated taking into account both the dispersion energy
term (d) and the electrostatic contribution (el). The
first is calculated by using the Buckingham dispersion
energy function [14].
In the case of ethylene glycol, the different trans, cis
and cis-OH conformations are considered with the CCbond essentially disposed coplanar and also with the
two oxygen atoms pointing towards the mercury layer
(Fig. 1).
Variations in EGEG, qEGEG and rEGEG are ofy/4
radiants for the angles and of 0.01 A, for the distance.
For water, the disposition suggested as the more stable
is accounted for: the oxygen atoms facing the Hg
surface, and the dipole moment parallel to the surface
are in someway a little tilted towards the bulk; a
perpendicular disposition is considered also [15,16].
In this paper this attempt is pursued taking into
account the following four independent arguments: (a)
a relation associating the DGINT for a generic adsorbate
to its molecular dimension which is proportional to the
number of solvent molecules (water) dislodged from the
surface of Hg in the adsorption process [3]; (b) a brief
re-examination of the only thermodynamic study [7]
regarding the adsorption of EG from water on Hg; (c)
Fig. 1. Mutual disposition of EG and water molecules for the
calculation of intermolecular energy contributions. The Hg
surface corresponds to the paper plane. Three different confor-
mations of EG are considered, and also two different mutual
disposition of the EG cis conformation. For water two differ-
ent mutual dispositions are taken into account.
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C. Fontanesi et al. /Electrochimica Acta 46 (2001) 12771284 1279
Table 2
Calculated intermolecular interaction energy (d and el) for
adsorbed EG in different conformations and water molecules a
el (kJ mol1)d (kJ mol
1)
EG (cis, planar) 4.9 0.2
5.1 +2.1EG (cis,
perpendicular)
EG (cis-OH) 1.35.20.39.2EG (trans)
3.8Water (planar) 1.6
+1.01.2Water (perpendicular)
a For mutual disposition of the molecules see Fig. 1.
MNDO Hamiltonian implemented in the AMPAC pro-
gram [13].
A minimum value (which invariably corresponds to a
maximized packed disposition) in energy is obtained
from several relative minima. Both d and el reported
values (Table 2) correspond to almost the same configu-
ration between interacting molecules. For the different
compounds, the equilibrium distance r is determined by
the Van der Waals radii.Experimental adsorption data are taken from the
literature and in some cases revised.
3. Results and discussion
The comparative study of the adsorption process of
aromatic derivatives from water and EG solutions
[1,3,17] leads to the conclusion that by itself EG
should be adsorbed on bare mercury, from its pure
liquid phase, with a value of DGEG$51 kJ
mol1
(provided that to the same virtual process, butregarding water, a value of DGw=kJ mol1 has been
assigned). Now for a very large set of organic adsor-
bates, all of them aromatics and reasonably interacting
with the mercury surface in the same mechanistic way,
i.e. through a liquid-like adsorption process and with
planar disposition of the aromatic moiety on the elec-
trode surface [2,5], a good linear relation was obtained
relating the molecular hindrance of the individual ad-
sorbate (proportional to the number, w, of solvent
molecules, in the case water, dislodged in the adsorp-
tion process) and the DGADS,INT value. The relationship
shown in Fig. 2 is highly satisfying, despite the large
variety of molecular structures of the adsorbates (no. 38
compounds, one more point than previously reported
have been included combining the results from Refs.
[1,4]). The meaning of this relation sets on the crucial
role, on a energetic ground, played by the process of
substitution of solvent molecules covering the Hg sur-
face worked by the adsorbing species [6,18], much more
than on the fact that all compounds are aromatics;
actually, when aromatics are perpendicularly adsorbed,
their adsorption energy is almost the same [14], inde-
pendent of the aromatic character of the individual
compound.
So, solely referring to the molecular dimension andon the hindrance occupied on the electrode surface, a
tentative extension to non-aromatic molecules of the
relation in Fig. 2 can be attempted.
Therefore, when the adsorption of EG on mercury
with the OH groups interacting with the surface is
considered, a number of 2.1 water molecules (statisti-
cally) has to be replaced, wEG=2.1, taking into account
the following molecular areas, respectively: AEG=0.31
nm2 and Aw=0.14 nm2 ([3,7] and references therein
cited). Then the extrapolation in the plot of Fig. 2 at
Slightly different relative minima of d are so ob-
tained and the absolute one is chosen for the discus-
sion. Using the same reciprocal configurations and
procedure for the rotation of angles and distances, the
intermolecular electrostatic term is then calculated:
el=1
4y0 %NAi=1 %NBk=1 qiqkri,k where 0 is the vacuum permittivity, NA and NB are the
number of atoms of the two distinguished individual
molecules A and B (note that both A and B are the
same chemical species), qi and qk are the MO SCF net
charges localized on atoms i, k belonging to the distin-
guished individual species A and B, respectively. MO
SCF net charges of each atom, concerning the unper-
turbed isolated molecule, are calculated using the
Fig. 2. Intrinsic adsorption Gibbs energy of aromatic com-
pounds in relation to their individual area occupied on the
mercury surface, which is proportional to the number (ww) of
water molecules dislodged from the surface itself in the ad-
sorption process.
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C. Fontanesi et al. /Electrochimica Acta 46 (2001) 127712841280
wEG=2.1 gives a DGEG of about 50 kJ mol1, as
well as for w=1, a DGw value of about 20 kJ mol1
is obtained, thus corresponding to the process involving
a water molecule (mole) self-replacing at the interface,
according to two different energetic states, the bulk and
the surface. This result, completely independent of that
obtained in Ref. [1], is valuable cause it arises by an
extrapolation procedure. Let us now consider the ad-
sorption process of EG from water, for which thefollowing thermodynamic balance can be considered:
DGEG=DGADS,EG+DGsol,EG+wEGDGw (1)
taking into account the solution of pure EG in water
(DGsol,EG), the experimental measurement of EG ad-
sorbed on Hg from water (DGADS,EG) and the substitu-
tion of wEG=2.1 molecules/moles of water by each EG
molecules/moles, wEGDGw. The only experimental
value of DGADS,EG cited in the literature amounts to
8.4 kJ mol1 [7] (at Epzc, the potential of zero
charge), so that DGEG=DGsol,EG52.5 (kJ mol1).
The value to be ascribed to DGsol,EG depends on the
choice of the standard state regarding the solution,
which has to be the same of that involved for the
evaluation of DGADS,EG. For the solution of EG in
water (not an equilibrium process):
EGpure,liquidEGsolution
DGsol,EG=vEG,solutionvEG,pure,liquid
Moreover:
vEG,solution=vEG,pure,liquid+RT ln(a(X)/aX) (2)
the reference function for the activity is selected as the
molar fraction (X) (the relevant standard state is activ-
ity=X=1) and:
vEG,solution=vEG,solution+RT ln(a(c)/ac ) (3)
In this second case, the reference function for the
activity is selected as the molar concentration (c) (the
relevant standard state is activity=c=1).
Eqs. (2) and (3) correspond to the same physical state
of the system, then:
vEG,pure,liquid(X)+RT ln(a(X)/aX)
=vEG,solution(c)+RT ln(a(c)/ac )
Note that aX=1 as well as ac=1. The use of the
Frumkin isotherm to define the DGADS,EG, as in the
mentioned case [7], involves the choice of activity=c=
1 (molarity), so that
DvEG,sol=vEG,solutionvEG,pure,liquid=RT ln(X,c=1)
(the solution is supposed ideal, aX. When c=1,
X=0.01871 and DvEG,sol=9.85 kJ mol1. In this
way a value of DvEGl=62 kJ mol1 can be
achieved; a value not so far from that previously ob-
tained (sensitivity on wEG90.2 involves the term wEG
DGw, a variation of about 94 kJ mol1).
Furthermore, whether the interaction adsorbate
electrode surface implies a partial charge transfer and/
or a molecular rearrangement, that is the adsorption
process is intermediate between a pure physisorption
and a true covalent bond (see the DGADS,INT values in
Fig. 2), then this kind of interaction could be related to
the concept of absolute hardness, p; this is a quantity
defined by Parr and Pearson [8,19] by an operative
procedure in connection with the ionization potential EIand the electron affinity EA of whatever chemical sys-
tem, molecules, atoms, ions, radicals: p=(EIEA)/2,
the EI and EA quantities can be substituted by the
EHOMO and ELUMO of the corresponding chemical enti-
ties considered as isolated systems. So, hard molecules
show a large HOMOLUMO gap, and on the contrary
soft molecules a lower one: softness=|=1/p. The
interaction between two systems is favored if both of
them are soft: the mercury metal at the point of zero
charge is considered to be relatively soft [20]. The plot
reported in Ref. [4] clearly shows that soft adsorbates
are more active on the surface, at least in terms of the
DGINT value. In this view, let us now consider the most
favorite couple between components of the actual three
components system: H2OHgEG (Table 1). Because
the hardness concept and its value are based on
electron affinity and ionization potential, for liquid
mercury (atomic) they came from the experimental
evidence, while for molecular systems, they have to be
calculated sometimes.
From the data reported (for experimental values see
Refs. [21,22]), mercury turns out to be the most soft
one with respect to both water and EG, but water is
more hard than EG.
For EG, the soft and hard character have been
calculated taking into account three possible conform-
ers: cis, cis-OH (the cis conformer characterized by an
intramolecular OH bond) and trans.
So, an initial system composed by Hg and adsorbed
water (a softhard couple) will change, in the presence
of EG in solution, into a more stable arrangement, Hg
and adsorbed EG, corresponding to a couple with more
softsoft character. On a quantitative ground, EG has
to show an intrinsic adsorption energy higher than
water.
3.1. Theoretical outcomes
To confirm the reliability of this DGEG value, in the
absence of a direct measurement of the adsorption of
EG gas on liquid mercury, a calculation of this energy
of interaction between a molecule of EG and a cluster
of four or seven Hg atoms (anyway simulating a mer-
cury surface) has been performed.
The presence of a minimum in energy (total) of the
whole adduct has been investigated varying both the
distance of the EG molecule from the central mercury
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C. Fontanesi et al. /Electrochimica Acta 46 (2001) 12771284 1281
Fig. 3. Top-1 disposition of a molecule on Hg ( cis conformer)
on a seven atom cluster of mercury. Top view (left) and side
view (right).Fig. 6. Disposition of a EG molecule (trans conformer) on the
seven mercury atoms cluster (top view).atom of the cluster and the disposition of the two
oxygen atoms of EG with respect to Hg atoms.
Five different dispositions have been characterized
and the proper different denominations assigned for
similarity to those regarding a water molecule interact-
ing with a mercury layer. Moreover, three different
molecular conformations of the isolated EG molecule
have been taken into account: cis, trans and a cis-OH.
This because a cis conformation has been suggested by
experiments as the most stable for EG in the pure
liquid bulk and even in the gas phase and the existence
of the intramolecular hydrogen bond has been also
proposed [2325].So, for the cis conformer, the top-1 disposition in-
volves the two oxygen atoms pointing toward the Hg
layer (Fig. 3). In the top-2 arrangement, the two CO
bonds are forced parallel to the metal layer and finally
the top-3 disposition features the two oxygen atoms
pointing away from the mercury layer, toward the bulk.
Furthermore, another two dispositions have been also
considered: the hollow one (Fig. 4a), and the bridge
disposition (Fig. 4b).
Fig. 5 clearly shows that for the cis conformer, the
most stable structure interacting with Hg is that regard-
ing the top-1 disposition. This kind of disposition in-
volves two oxygen atoms of EG pointing towards the
Hg layer and interact, contemporarily, with three Hg
atoms by approaching the cavity among them; the
minimum of the total cluster energy corresponds to
81 kJ mol1.
For the EG trans conformer, taking into account the
role played by the interaction of the two oxygen atoms
of EG with Hg, only the disposition shown in Fig. 6
has been investigated because any other arrangement of
the EG molecule should be pointing at least one oxygen
atom toward the bulk. In this case the minimum in
energy of the cluster plus EG corresponds to about
43 kJ mol1 (Fig. 7). In our calculations, the dipolemoment of the Hg7 EG cluster depends linearly on the
distance between the mercury plane and the oxygen
atoms, this result indicates that the HgEG energetic
interaction is mainly of electrostatic nature. In fact, the
oxygens of EG bear a negative net charge which origi-
nates a negative electrostatic potential field more local-
ized (intense) than the positive one; such a negative
electrostatic potential field can account for the leading
role played by the orientation of the oxygens with
respect to the mercury. This view is also supported by
Fig. 4. Hollow (left) and bridge (right) disposition of a
molecule of EG (cis conformer) on a cluster of four mercury
atoms.
Fig. 5. Total electronic energy of the Hg clusterEG molecule
adduct (cis conformer) at varying the distance from the CC
axis of EG from the mercury cluster.
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C. Fontanesi et al. /Electrochimica Acta 46 (2001) 127712841282
Fig. 7. Total electronic energy of the Hg clusterEG molecule
adduct (trans conformer) at varying the distance from the CC
axis of EG from the mercury cluster.
the fact that none of the occupied MOs show a signifi-
cant bonding nature between the Hg and the EG
molecule and is in line with theoretical studies concern-
ing the adsorption of water on mercury [26].
Finally, the cis conformation of EG with the in-
tramolecular hydrogen bond has been studied, finding a
shallow minimum in energy, 0.5 kJ mol1 for the
disposition set out in Fig. 8.
The energetic scheme for the different types of inter-actions is summarized in Fig. 9.
The process simulated by using quantum mechanical
methods is then:
EG(g)+Hg(l)Hg(EG) DU
and the relevant calculated quantity results a DU value,
which is not directly comparable to the DGEG value
previously obtained; it can be transformed into a DH
value with the assumptions that EG(g) is a pure ideal
gas (P=1 bar, T=298 K) and that the volume of a
mole of EG adsorbed on mercury with respect to the
molar volume of the gas is negligible; so,D
H=D
URTDn=DU2.5 kJ mol1.
Now, when the gas liquid phase change is consid-
ered for EG [27], it can be obtained the relation (3):
EG(l)EG(g) (a)
EG(g)+Hg(l)Hg(EG) (b)
EG(l)+Hg(l)Hg(EG) (4)
suitable combination of the relevant thermodynamic
function variations yields:
and considering T=298 K:
DG(1)
=DH(1)
TDS(1)
(5)
DG(1)=DUTDS(1)+62.4
provided that the main entropic contribution is due to
the process (a)2; then:
DG(1)=DU+15.8 (6)
Fig. 8. Disposition of a EG molecule (cis-OH conformer) on
the seven mercury atoms cluster (top view).
Fig. 9. Energy diagram (three different EG conformers) for the
formation of the EGHg cluster adduct.
2 Regarding the EG adsorption, as suggested by experi-
ments, no close packing of adsorbed molecules can be re-
vealed, so that a not negligible degree of freedom of the
adsorbed species on the metal surface has to be accounted for.
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C. Fontanesi et al. /Electrochimica Acta 46 (2001) 12771284 1283
This relation gives rise now to a value of DG1 of
about 65 kJ mol1 only when DU for the top-1
disposition without an intra-molecular hydrogen bond
is considered in the interaction with the mercury clus-
ter. This result is fully comparable with the outcome
characterized by the previously reported methods in the
first section of this paper.
3.2. The interaction between EG adsorbed molecules
In a crude view, the interaction energy among ad-
sorbed and then vicinal EG molecules can be repre-
sented by the values of d and el (see Section 2)
reported in Table 2 for different conformations of EG
and also for at least two different mutual dispositions
of EG molecules on the surface, planar and perpendicu-
lar, but anyway with the two oxygen atoms pointing
toward the metal surface. This last arrangement is
however the one that gives rise to the deepest energy
minimum when the interaction of EG with Hg in the
top-1 disposition is considered.The dispersion energy term, d, is always negative,
pointing out an attractive interaction among EG
molecules, while the electrostatic one, el is in some
cases positive (smaller than d).
These two terms represent a different approach to the
same problem of the energetic interaction, because the
electrostatic ones, due to the net charges localized on
vicinal molecules which give rise to el, are just con-
tained (but not explicitly) in the empirical parameteriza-
tion of the Buckingham term d [14].
At this level of the discussion, any interaction of the
first EG layer toward the bulk (i.e. the presence of asecond or a third layer of oriented EG) is completely
neglected.
Anyway, the most stable disposition of EG on the
mercury layer, i.e. a cis-conformation in the top-1
configuration, shows to be stabilized also by an attrac-
tive interaction among vicinal molecules, mainly on the
basis of the d value. On the reliability of this value,
which now is crucial, one can get some answers devel-
oping the conclusions obtained by Trasatti [7] on the
adsorption process of EG from water on mercury. For
that process, a substitution of water molecules ad-
sorbed on the Hg surface by the EG molecules can besuggested:
EG(solution)+Hg(water)
X Hg(EG)+water(solution)
In terms of energetic contributions, taking into ac-
count the linearized Frumkin isotherm and the relations
discussed in the Refs. [28,29] one can suggest that:
2RT AF(EG)=EGwEGwater (7)
where AF(EG) represent the Frumkin interaction
parameter of the macroscopic adsorption process, EGand water have the usual meaning till now discussed
(they can be represented by d or el and wEG=2.2 is
obtained taking into account a molecular area of 0.31
nm2 for EG and 0.14 nm2 for water [1,3,7].
In fact, wEG corresponds to the number of molecules/
moles of water displaced by the adsorption of one
molecule/mole of EG.The experimental evidence shows an adsorption be-
havior of EG from water [7] of Langmurian type, i.e.
with AF(EG)=0.
Of course this does not imply that an energetic
interaction between two nearest EG adsorbed molecules
is not effective; on the contrary, it let the reliability of
d or el for EG to be estimated from the corresponding
value for water, and this procedure can be checked for
different conformations of EG and different EG dispo-
sitions on mercury and water as well, taking into ac-
count the data reported in Table 2 and the relation (7)
with an AF(EG)
value=0.
The ratio EG/water should result equal to wEG=2.2,
and from Table 2 it can be observed that for the
couples d,EG cis(planar and perpendicular) and d,water(planar and perpendicular) a value for the ratio range
between 3.06 and 4.18, not so far from the value of 2.2.
A value of 2.3 is anyway obtained when el is used for
the d,EG cis( perpendicular) and d,water(perpendicular),
but unfortunately those two terms are individually pos-
itive, i.e. indicating a repulsive interaction (moreover,
the pure perpendicular disposition of water is not con-
sidered the most favorable one).
All other combinations of EG and water give rise to
values corresponding to a ratio far from 2.2.
It is worth mentioning that this rigid modeling and
crude view of the interaction regarding EG and water
molecules among themselves only partially and poorly
account for the disposition suggested in Refs. [7,15], in
which the EG molecules are considered to be in some
way tilted toward the bulk as well as for water, so that
an intermediate disposition should be much more
reasonable.
3.3. Some conclusions
Data based on independent approaches involvingindirect experimental procedures and classic thermody-
namics lead to the evaluation of the Standard Gibbs
energy of adsorption of pure liquid EG on mercury: it
should range between 51 and 62 kJ mol1.
The value is confirmed taking into account the quan-
tum mechanical simulation of the interaction of a
molecule of EG gas on a cluster of mercury atoms, but
only for the cis conformation involving the pointing of
the two oxygen atoms towards the mercury layer. In
this case, a partial charge transfer coefficient from EG
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C. Fontanesi et al. /Electrochimica Acta 46 (2001) 127712841284
to mercury can also be calculated (0.077 electrons)
for the top-1 disposition.
This theoretical result suggests that the trans confor-
mation of EG can be not favored in the interaction
with mercury as well as the cis one but showing the
intramolecular hydrogen bond, cause the hydrogen
bond should prevent the stabilizing allocation of each
of the oxygen atoms among the Hg atoms of the
cluster.Moreover, the calculated dispersion energy term for
EG-cis confirms a stabilizing effect among vicinal inter-
acting molecules and suggesting at least a pseudo-per-
pendicular disposition of each molecule in the adsorbed
layer on mercury.
Acknowledgements
Planning and development of the studies here pre-
sented form a part of an Italian National Research
Project entitled Elettrocatalisi ed Elettrosintesi, Coor-dinatore Scientifico Professor Rolando Guidelli. The
authors would like to thank the Italian Ministero dell
Universita e della Ricerca Scientifica e Tecnologica
(Programmi di Ricerca Scientifica di Rilevante Interesse
Nazionale) for financial support.
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