raman spectroscopic studies of the stretching band from water up to 6 kbar at 290 k
TRANSCRIPT
Chemical Physics Letters 379 (2003) 427–431
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Raman spectroscopic studies of the stretching bandfrom water up to 6 kbar at 290 K
Qiang Sun a,*, Haifei Zheng a, Ji-an Xu b, E. Hines c
a School of Earth and Space Science, Peking University, Beijing 100871, Chinab Geophysical Laboratory, Carnegie Institute of Washington, Washington 20008, USA
c Anvil Department, Charles and Colvard Ltd., Morrisville 27560, USA
Received 30 September 2002; in final form 15 July 2003
Published online: 17 September 2003
Abstract
Raman scattering studies of the stretching band from liquid water have been conducted up to 6 kbar at 290 K. It
shows that the ðv1Þmax decreases with increasing pressure initially and reaches the minimum at about 2 kbar, and in-
creases with higher pressure up to about 4 kbar, then decreases with increasing pressure up to 6 kbar. This is accordance
with the behavior of rOO at high pressure. Additionally, the influence of pressure on water structure is also discussed.
� 2003 Elsevier B.V. All rights reserved.
Water is the most ubiquitous and intriguing
fluid in nature. A comprehensive molecular theory
for water is needed for two reasons. First, this
substance is a major chemical constituent of ourplanet�s surface and as such it may have been in-
dispensable for the genesis of life. Second, it ex-
hibits a fascinating array of unusual properties
both in pure form and as a solvent [1]. Therefore,
water has been the subject of numerous experi-
mental and theoretical investigations. However, in
comparison with its simplicity at the molecular
level, water is a complex and poorly understoodliquid.
* Correspondence author.
E-mail address: [email protected] (Q. Sun).
0009-2614/$ - see front matter � 2003 Elsevier B.V. All rights reserv
doi:10.1016/j.cplett.2003.07.028
In contrast with studies of water at high tem-
perature, especially in supercritical water, there
have not been many experimental works of the
effect of high hydrostatic pressure on hydrogenbonding in water [2–8]. From the energy-dispersive
X-ray diffraction technique (EDXD), Okhulkov
et al. [3] have found that the average separation
between nearest molecules rOO decreases with the
pressure rise up to �2 kbar, but at higher pressures
it begins to grow and reach the initial value at
4–5 kbar, then decreases with increasing pressure.
Although Bellissent-Funel and Bosio [9] seem toconfirm qualitatively the behavior of rOO, some
authors [10] reckoned this result as debatable. In
Raman scattering experiments, because of the
large scatter of experimental points, Walrafen and
Abebe [2] approximated their data with a linear
fit. Cavaille and Combes [4] definitely indicate a
ed.
428 Q. Sun et al. / Chemical Physics Letters 379 (2003) 427–431
singularity in the pressure range 2–3 kbar, but
their data points are scarce and seem to contra-
dictory to the behavior of rOO because the
stretching vibration increases up to 2 kbar then
decreases with increasing pressure.
In this letter, experiments were conducted inMoissanite anvil cells [11] to study the change of
the stretching vibration band of water up to 6 kbar
at 290 K. In order to control the increase of ex-
perimental pressure and obtain dense data points,
1-mm thick Cr1Ni18Ti9 stainless steel was applied
as gasket and the sample chamber was 600 lm in
diameter. Experimental pressure was calculated
according to Raman shift of the 464 cm�1 peak ofquartz. This is because the Raman shift was more
obvious ((9� 0.5) cm�1/GPa [12]), the pressure
could be determined more accurately. H2O used in
experiments was ion-distilled water and tempera-
ture was 290 K. During experiments, pressure was
applied and maintained for three minutes before
Raman spectra were measured, in order to attain
the hydrostatic pressure distribution of the system.Raman spectra were obtained using a confocusal
micro-Raman system Reshaw1000. The excitation
wavelength was the 514.5 nm line of an Arþ
ion laser operating at 25 mW. The spectra were
Fig. 1. (a) Raman spectra of the H2O stretching vibrations up to 6 kba
quartz.
recorded with scan times 1, accumulation times of
10 s, slit of 50 lm and ocular of 50. The resolution
was �1 cm�1.
The stretching vibration bands of water at
various pressure and 290 K are listed in Fig. 1(a)
and (b), shows the Raman behaviors of the 464cm�1 peak of quartz. The 464 cm�1 peak of quartz
is related to bending vibrations of the intra-tetra-
hedral O–Si–O angles [13]. According to Schmidt
and Ziemann�s studies [12], the pressure can be
calculated by
P ðMPaÞ ¼ 0:36079 � ½ðDvpÞ464�2 þ 110:86 � ðDvpÞ464:
The pressure calculated using the equation has anuncertainty of �50 MPa. The peak maximum is
determined by fitting the spectra using JANDELANDEL
SCIENTIFICCIENTIFIC PEAKFITEAKFIT v4.04 computer program. In
the process of determining ðv1Þmax, in order to
eliminating error, the symmetric stretching band of
water is all taken from 2500 to 4000 cm�1, and the
same fitted parameters are used in determining
ðv1Þmax. Fig. 2 shows the changes of the stretchingvibration maximum of water ðv1Þ with increasing
pressure, and the dashed lines in the figure refer to
linear square treatment of the data. It means that
higher pressure can make the ðv1Þmax shift to lower
r at 290 K. (b) The pressure dependence of the 464 cm�1 peak of
Fig. 2. Pressure dependence of the stretching vibration maxi-
mum ððv1ÞmaxÞ of H2O at 290 K. The uncertainty of pressure is
±50 MPa [12]. The determination of ððv1ÞmaxÞ is described in the
text. The uncertainties of pressure and wavenumber are all re-
flected in the data symbols. The dashed lines are the least square
fitted lines.
Q. Sun et al. / Chemical Physics Letters 379 (2003) 427–431 429
wavenumber initially and reaches the minimum at
about 2 kbar, and ðv1Þmax increases with increasing
pressure up to about 4 kbar, then decreases with
increasing pressure up to 6 kbar. In other words,
there exists discontinuity in liquid water at about 2
and 4 kbar. These are different from Walrafen andAbebe�s studies [2] and Cavaille and Combes�s re-sults [4]. We attribute the reason to the scarce data
points in their experiments.
As for water molecules, besides the covalent
bonds in H2O produced by orbital overlap be-
tween inharmonic sp3 hybrid orbits of oxygen
atom and 1s orbit of hydrogen atom, there also
exists strong hydrogen bond interactions betweenwater molecules. It is well known that many of the
unique properties of water are attributed to the
result of three-dimensional hydrogen bonding
network formed between water molecules. There-
fore, the OH stretching vibration of water is also a
strong function of the hydrogen bond strength.
The behavior of ðv1Þmax reflects the change of hy-
drogen bond. So, from the change of ðv1Þmax up to6 kbar at 290 K, we can conclude that the hy-
drogen bond energy decreases up to 2 kbar, and
increases up to 4 kbar, then decreases with in-
creasing pressure up to 6 kbar. This is accordance
with the behavior of rOO measured by Okhulkov
et al. [3].
The structure of liquid water has been the
subject of numerous investigations and remains
controversial. Up to now, most of models can be
divided into two categories: (a) the mixture/inter-
stitial and (b) the distorted hydrogen bond (con-
tinuum) categories [14]. In the former, the mixturemodels postulate the simultaneous existence of two
or more relatively long-lived structures in the li-
quid, such as the �flickering-cluster� model pro-
posed by Frank and Wen [15]. Different and
discrete combinations of hydrogen-bonded mole-
cules are assumed to coexist as evidenced by the
existence of isosbestic points which are well known
in the spectroscopy of reversible chemical reac-tions [16]. The second and currently the most fa-
vored model, is based on the assumption that the
structure relaxes on a time scale that is similar to
that observed in other liquids, and water is
thought to exist as a continuous network of mol-
ecules interconnected by somewhat distorted hy-
drogen bonds [17,18]. Recently, an outer structure
two-state model was put forward and applied toexplain the anomalous properties of the liquid
[19,20]. Very simply speaking, the outer two-state
model is a mixture of ice-Ih- and ice-II-type
bonding, locally rearranging on picosecond time-
scales with average compositions that depend on
the temperature and pressure.
As for water molecules, apart from the uni-
versal van der Waals� interaction, a specific inter-action-hydrogen bonding also exists, and many of
the unique properties of water are attributed to the
result of three-dimensional hydrogen bonding
network formed between water molecules. It is
well known that the hydrogen bond in liquid water
arises as a result of electrostatic interaction be-
tween a hydrogen atom and some excess of nega-
tive charge on a neighboring oxygen atombelonging to another molecule. Such a bond is
much weaker than the usual chemical bonds but,
like the latter, it reveals quite a noticeable orien-
tation correlation. In order to maximize hydrogen
bond, each water molecule tends to interact with
its around molecules, then on time scales less than
the lifetime of a hydrogen bond, more complicated
molecular structural unit can be formed. And thisstructural unit can be called water molecular
concentration �cluster�. However, it should be
430 Q. Sun et al. / Chemical Physics Letters 379 (2003) 427–431
noted that the molecular cluster of liquid water
can only be termed as �V-structure� [21]. In other
words, it is the time averaging of the molecular
coordinates. At this point, the structure of liquid
water is different from that of ice.
In liquid water, the distribution of electriccharges on the oxygen atom in the water molecule
allows it to form two �legal� bonds with hydrogen
atoms belonging to the same molecule, and two
�illegal� bonds with the hydrogen atoms of other
molecules. Each pair of the bonds forms a nearly
tetrahedral angle (105�–109�). Thus, each molecule
of water can join four water molecules, thereby
forming a tetrahedron around it. Ohtomo et al.[22] have shown that a combined analysis of X-ray
and neutron diffraction data suggests the presence
of tetrahedral pentamer clusters. Such a molecular
configuration is a primary element of the structure
of ice and an inescapable attribute of any reason-
able model of the water structure.
On the other hand, according to theoretical
calculation for water cluster (H2O)n (n ¼ 6, 5), themost stable structure should be quasi-planar mo-
lecular cyclic hexamer and pentamer [23,24]. The
reason for the dominance of pentagons and
hexagons in bulk water systems is that these are
the smallest polygons that can produce O–O–O
angles near the optimum (tetrahedral) value,
which maximizes the hydrogen bond energy [25]. It
has been found that near a melting line, local orderof liquid phase structure is like the local order of
the solid phase [26,27]. Studies have shown that
normal ice (Ih) consists of regular arrays of
hexagons. From this, it can be deduced that there
should exist cyclic water hexamer in liquid water
near melting point. In order to maximize hydrogen
bond, each water molecule should be tetrahedrally
hydrogen bonded to their neighbors. At this time,the local structure of liquid water just resemble the
local structure of ice Ih [16]. From these, we con-
clude that there also should exist phase transition
in liquid water just like ice (Ih), but the changes of
physical and chemical properties in water phase
transition should be much weaker than those in ice
phase transition. In fact, the phase transitions of
ice (Ih)! ice (III) and ice (III)! ice (V) respec-tively occurs at about 2 and 3.7 kbar. Studies have
suggested that the minimum of viscosity [28] and
the maximum of self-diffusion [29,30] are observed
around 2 kbar. From the above discussion, We
conclude that, just like ice phase transition ice
(Ih)!ice (III)! ice (V), there also exists water
phase transition water (Ih)!water (III)!water
(V). It can be foreseen that the longitudinal waveof liquid water should attain minimum at 2 kbar.
In mathematical character, it can be termed as
�inflexion�, which is different from the �discontinu-ity� from ice Ih to ice III phase transition.
Acknowledgements
The authors sincerely thank Charles and Col-
vard Ltd, USA to provide the Moissanite anvils
generously. This work is supported by the Na-
tional Natural Science Foundation of CHINA
(Grant Nos. 40103005 and 10032040).
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