halogenated ethers bearing several f or cl atoms have been known for many years as narcotic gases . in these derivatives ,
the presence of one or several halogen atoms tends to make the ch bonds more acidic , which gives rise to specific interactions with surrounding enzymes and neuroreceptors [ 16 ] .
enflurane ( chclf - cf2-o - chf2 ) , a volatile anaesthetic , is characterized by two ch bonds which can interact with neighboring molecules .
the structures of the stable conformers of this molecule have been reported in earlier works [ 79 ] .
the basicity of enflurane and its interaction with guest molecules have been investigated as well [ 1013 ] .
recently , the atmospheric chemistry of halogenated ethers , such as isoflurane ( cf3-chcl - o - chf2 ) , desflurane ( cf3-chf - o - chf2 ) and sevoflurane ( ( cf3)2-ch - o - ch2f ) have been studied in the reaction with chlorine atoms and oh radicals , with respect to the global warming potentials of these compounds .
lane and coworkers   studied the reaction of enflurane with chlorine atom and the problems of ozone depletion .
it is therefore important to investigate the interaction between halogenated ethers and water , which is one of the major constituents of the atmosphere .
as far as we know , no theoretical or experimental data have been reported for the enflurane - water complexes .
, we will discuss the structures , binding energies and enthalpies of formation of the hydrogen bonded enflurane complexes with water .
the stabilization energies of the complexes have been determined at the mp2/6311++g(d , p ) and ccsd(t)/complete basis set ( cbs ) levels of theory . to estimate the role of the cooperativity or anti - cooperativity effects , the three - body contributions to the total binding energies
have been calculated . in the second part , the cl halogen bonded complexes between enflurane and water
full geometry optimizations followed by the calculations of vibrational frequencies and infrared intensities were performed for the two most stable conformers of enflurane and their complexes with water using an ab initio second order mller - plesset perturbation method combined with the 6311++g(d , p ) basis set [ 16 , 17 ] . the counterpoise cp - corrected gradient optimization , which eliminates the basis set superposition error ( bsse ) , has been used in all calculations of the minimum energy structures of the complexes investigated . the proton affinity ( pa ) as well as the deprotonation energy ( dpe ) were calculated as the negative enthalpy change and the enthalpy change of the reactions ( 1 ) and ( 2 ) , respectively , assuming standard conditions in the gas phase . 

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				 \begin{document}$$ { \rm{a}}{{{\rm{h}}}_{{({\rm{g } } ) } } } + { { { \rm{h}}}_{{({\rm{g}})}}}^ { + } \ ;   \to { \rm{a}}{{{\rm{h}}}_{{2({\rm{g}})}}}^ { + } { \rm{pa } } =   - \delta { { { \rm{h}}}^{{298 } } } $ $ \end{document}2\documentclass[12pt]{minimal } 
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				 \begin{document}$$ { \rm{a}}{{{\rm{h}}}_{{({\rm{g } } ) } } } \to { { { \rm{a}}}_{{({\rm{g}})}}}^ { - } + { { { \rm{h}}}_{{({\rm{g}})}}}^ { + } \ ; \;{\rm{dpe } } = \delta { { { \rm{h}}}^{{298 } } } $ $ \end{document}where ah  =  isolated enflurane molecule .
the total stabilization energies of the enflurane - water complexes were determined at the mp2/6311++g(d , p ) and ccsd(t)/complete basis set ( cbs ) levels of theory .
the ccsd(t)/cbs stabilization energy was calculated as the sum of the mp2/cbs stabilization energy and the ccsd(t ) correction term .
the mp2/cbs energy was extrapolated from the mp2 energies evaluated with the aug - cc - pvdz and aug - ccpvtz basis sets .
the ccsd(t ) correction term ( the difference between the ccsd(t ) and mp2 interaction energies ) was determined with the aug - cc - pvdz basis set [ 21 , 22 ] . enthalpies of formation of the enflurane - water complexes under standard conditions , in the gas phase , were calculated at the mp2/6311++g(d , p ) and ccsd(t)/cbs levels .
the ccsd(t)/cbs enthalpy was determined as the sum of the ccsd(t)/cbs electronic energy and the zero - point vibrational energy and the thermal correction to enthalpy obtained by the mp2/6311++g(d , p ) method .
the evaluation of the three - body contribution ( e3b ) to the total interaction energy ( eint ) of the enflurane complex with two water molecules was performed at the mp2/6311++g(d , p ) and ccsd(t)/cbs levels of theory .
the value of e3b was obtained as the difference between eint of the complex and the sum of three pairwise ( two - body ) interaction energies , e2b .
the negative value of e3b means a cooperative effect , while the positive one corresponds to an anti - cooperative interaction in the three - body unit .
natural bond orbital ( nbo ) analysis has been applied to calculate charges on individual atoms , orbital occupancies , hybridizations , and the second - order interaction energy ( e ) between the donor and acceptor orbitals .
it should be mentioned that nbo method evaluates the energies of orbitals and the 2nd - order stabilization energies only in this case , when the 1-electron effective hamiltonian operator is well defined ( e.g. , fock or kohn - sham operator ) .
therefore , in the mp2 calculations , the nbo analysis has been performed at the scf level .
the two most stable structures of enflurane optimized at the mp2/6311++g(d , p ) level of theory are shown in fig.1 .
conformers i and ii differ in energy by only 0.07  kcal  mol . it should be mentioned that the stability order of the conformers is slightly different from that obtained at the mp2/6311g(2d ) level in our earlier studies .
conformers i and ii of the present work correspond to the b and c conformers of ref .
let us notice that in i , the two ch bonds are in a trans position , and in ii , the two ch groups adopt the cis position . 
 fig .
1structures of two most stable conformers of enflurane optimized at the mp/6311++g(d , p ) level of theory and the numbering of atoms structures of two most stable conformers of enflurane optimized at the mp/6311++g(d , p ) level of theory and the numbering of atoms the structures of enflurane ( i and ii ) complexes with one water molecule ( 1 - 1 ) are illustrated in fig . 
2 . as is seen , in the 1 - 1 complexes involving both conformers , water interacts with enflurane through ch 
ow hydrogen bonds , with the c1h5  ow or c4h12  ow distances varying between 2.23 and 2.32   . weak interaction between one of the f atoms and the h atom of water is also possible , the hw  f distances being much longer ( between 2.60 and 2.87   ) .
o3 complex has been found on the potential energy surface . in the ia complex ( fig . 
o3 distance is too long ( 2.80   ) to be classified as a true hydrogen bond . 

2structures of enflurane complexes with one water molecule optimized at the mp2/6311++g(d , p ) level .
the dot lines indicate selected intermolecular distances ( in angstroms ) , angles are in degrees structures of enflurane complexes with one water molecule optimized at the mp2/6311++g(d , p ) level .
the dot lines indicate selected intermolecular distances ( in angstroms ) , angles are in degrees the structures of enflurane complexes with two water molecules ( 12 ) are shown in fig . 
it is important to notice that in these complexes , the intermolecular distances remain approximately the same as in the 1 - 1 complexes , the ch  ow distances varying between 2.23 and 2.34   , and the owhw
 f distances being between 2.41 and 2.61   . in ia and ic , the o13h14 
f11 intermolecular angles are markedly larger ( 146 and 152 , respectively ) than the oh  f intermolecular angles in the remaining complexes ( 100110 ) .
further , the c4h12  ow hydrogen bonds tend to be more linear than the c1h5  ow .
it is worth mentioning that in the enflurane dimer , the o3 atoms do not participate in the interaction .
the two enflurane molecules having the trans conformation are held together by ch  f hydrogen bonds . 

3structures of enflurane complexes with two water molecules optimized at the mp2/6311++g(d , p ) level .
the dot lines indicate selected intermolecular distances ( in angstroms ) , angles are in degrees structures of enflurane complexes with two water molecules optimized at the mp2/6311++g(d , p ) level .
the dot lines indicate selected intermolecular distances ( in angstroms ) , angles are in degrees the enthalpy of deprotonation and protonation of the two conformers are presented in table  1 . 

table 1enthalpies of deprotonation of h5 or h12 atoms and proton affinities ( pa ) of o3 for the two most stable conformers of enflurane ( under standard conditions ) , calculated at the mp2/6311++g(d , p ) and ccsd(t)/cbs levels [ all values in kcal  mol]conformerhhidpe ( c1h5)365.6363.1dpe ( c4h12)367.5367.3pa150.3151.8iidpe ( c1h5)365.2362.8dpe ( c4h12)368.6368.1pa154.5156.4the numbering of atoms is shown in fig . 
1calculated as sum of e and zero - point vibrational energy and thermal correction to enthalpy obtained at the mp2 levelpa  =  h enthalpies of deprotonation of h5 or h12 atoms and proton affinities ( pa ) of o3 for the two most stable conformers of enflurane ( under standard conditions ) , calculated at the mp2/6311++g(d , p ) and ccsd(t)/cbs levels [ all values in kcal  mol ] the numbering of atoms is shown in fig .  1 calculated as sum of e and zero - point vibrational energy and thermal correction to enthalpy obtained at the mp2 level in the present systems , the ch 
this can be related to a larger basicity ( pa  =  165  kcal  mol ) and a lower acidity ( dpe  =  390  kcal  mol ) of water molecule , in comparison to the corresponding values calculated for the two conformers of enflurane .
h2o ( pa(o )  =  174  kcal  mol ) is stabilized by an owhw 
o interaction , while in the chfclochf2  h2o complex ( pa(o )  =  155  kcal  mol ) , the ch 
o , showing the predominance of the ch  ow hydrogen bond over the owhw  o interaction .
in contrast , the complex between ch2fcho ( pa(o )  =  161  kcal  mol , dpe(ch )  =  352.3  kcal  mol ) and water shows a preference for a cyclic structure , the owhw  o hydrogen bond being shorter than the ch 
table  2 lists the binding energies for the interaction of the i and ii conformers of enflurane with one water molecule calculated at the mp2/6311++g(d , p ) and ccsd(t)/cbs levels of theory .
the ccsd(t)/cbs stabilization energies for the ia , ib , iia and iib complexes are 5.89 , 5.04 , 4.67 and 4.66  kcal  mol , respectively .
these results indicate that ia and ib are more stable than the iia and iib complexes . 

table 2binding energies ( e and e ) and enthalpies of formation ( hf and hf ) of the enflurane - water complexes , calculated at the mp2/6311++g(d , p ) and ccsd(t)/cbs levels [ all values in kcal  mol]iaibiiaiibe4.594.163.833.85e5.895.044.674.66hf3.062.732.432.42hf4.353.583.293.22corrected for bsseenthalpy of formation under standard conditionszero - point vibrational energy and thermal correction to enthalpy obtained at the mp2 level binding energies ( e and e ) and enthalpies of formation ( hf and hf ) of the enflurane - water complexes , calculated at the mp2/6311++g(d , p ) and ccsd(t)/cbs levels [ all values in kcal  mol ] enthalpy of formation under standard conditions zero - point vibrational energy and thermal correction to enthalpy obtained at the mp2 level table  2 also shows the values of the enthalpies of formation of the enflurane - water complexes , calculated at both levels of theory ( under standard conditions in the gas phase ) .
the ccsd(t)/cbs calculated enthalpies of formation are 4.35 , -3.58 , 3.29 and 3.22  kcal  mol for the ia , ib , iia and iib complexes , respectively .
the negative value of enthalpy implies that the formation of the enflurane - water complexes is the exothermic process .
binding energies and dpes vary in a very small range and no correlation could be found between these two parameters as in the case of the halogenated ethers and water complexes .
cooperative and anti - cooperative effects have been the subject of many studies [ 23 , 2934 ] .
table  3 collects the total binding energies , sum of the pairwise interaction energies and the three - body contribution ( e3b ) to the interaction energies of the two complexes of enflurane with two water molecules ( ic and iic , shown in fig . 
3 ) , calculated at the mp2/6311++g(d , p ) and ccsd(t)/cbs levels of theory . 

table 3total binding interaction energy ( eint ) , sum of pairwise interaction energies ( e2b ) , and the three - body contribution ( e3b ) of enflurane ( enf ) complexes with water ( a and b ) molecules .
calculations performed at the mp2/6311++g(d , p ) and ccsd(t)/cbs levels [ all values in kcal  mol]mp2ccsd(t)iciiciciiceint9.017.6011.419.56e2b8.947.7511.329.68e3b0.070.150.090.12corrected for bsse total binding interaction energy ( eint ) , sum of pairwise interaction energies ( e2b ) , and the three - body contribution ( e3b ) of enflurane ( enf ) complexes with water ( a and b ) molecules .
calculations performed at the mp2/6311++g(d , p ) and ccsd(t)/cbs levels [ all values in kcal  mol ] as follows from this table , the ccsd(t)/cbs absolute value of the total interaction energy of ic amounts to 11.41  kcal  mol , and is larger ( by 1.85  kcal  mol ) than that of the complex iic . for the ic complex , the value of e3b is negative and very small ( 0.09  kcal  mol ) , which indicates that the cooperativity is negligible . in the case of the iic complex ,
the value of e3b is positive and small ( 0.12  kcal  mol , about 1  % of eint ) which implies the presence of a very weak anti - cooperative effect .
examples of the cooperativity effects have been recently illustrated in the cyclic complexes between cycloethers and h2o where both ch  ow and owhw  o are strengthened . as expected , with regard to the ic complex ( negligible cooperativity )
there is no change in the intermolecular ch  ow distances , in comparison to ia and ib , while in the iic complex ( a small anticooperativity ) the c1h5  o13 and c4h12 
o16 distances are longer , by 0.05 and 0.02   , than the corresponding distances in the iia and iib complexes , respectively .
complex formation with water results in a contraction of the ch bond involved in the ch  ow interaction along with a blue shift ( between 18 and 26  cm ) of the corresponding vibration .
blue shifts of the same order of magnitude ( between 19 and 25  cm ) were predicted for the complexes between enflurane and acetone ( i conformer , bound with water at the c1h5 and c4h12 sites ) . as seen in table  4 , an ir intensity increase was predicted for the complexes formed at the c1h5 bond , while an ir intensity decrease was predicted for the complexes formed at the c4h12 bond .
let us notice that the analogous variations of ir intensity have been observed experimentally   in our earlier work on enflurane complexes with acetone . 

table 4c - h distances ( r in  ) , frequencies (  in cm ) and corresponding infrared intensities ( a in km  mol ) of c - h stretching vibration in two conformers of enflurane and their complexes with water molecules .
calculations performed at the mp2/6311++g(d , p ) levelc1h5rraai1.09031855ia1.0890.0013204 + 1911 + 6ib1.0900.0003186 + 150ic1.0890.0013203 + 1811 + 6ii1.09031765iia1.0890.0013202 + 2612
+ 7iib1.0900.000317516 + 1iic1.0890.0013199 + 237 + 2c4h12i1.089321012ia1.0880.0003215 + 5111ib1.0880.0013229 + 1975ic1.0880.0013233 + 2375ii1.089320514iia1.0890.0003205015 + 1iib1.0880.0013229 + 2468iic1.0880.0013226 + 21410the corresponding structures are shown in figs .  1 and 2,changes in the bond length in comparison to the isolated conformer ,
changes in the (c - h ) frequency in comparison to the isolated conformer , changes in the ir intensity ( a ) c - h distances ( r in  ) , frequencies (  in cm ) and corresponding infrared intensities ( a in km  mol ) of c - h stretching vibration in two conformers of enflurane and their complexes with water molecules . calculations performed at the mp2/6311++g(d , p ) level the corresponding structures are shown in figs .  1 and 2 , changes in the bond length in comparison to the isolated conformer ,
changes in the (c - h ) frequency in comparison to the isolated conformer , changes in the ir intensity ( a ) the selected results from the nbo analysis are collected in table  5 . as seen in this table ,
the contraction of the c1h5 and c4h12 bonds mainly results from the decrease in occupancy of the corresponding *(ch ) orbital .
a small increase of the s - character of the c atom may also contribute to this contraction , which has been largely discussed in earlier works [ 3543 ] .
the interaction with water also leads to a decrease of the positive charge on c and an increase of this charge on the h atom . 

table 5electron density in the (ch ) and *(ch ) orbitals and the s - character of the valence orbital on the c atom ( in % ) in isolated i and ii conformers and their complexes with h2oc1h5**%  s - char% s - chari1.98600.029727.2ia1.98550.00050.02790.001828.31.1ib1.98600.00000.02960.000127.20ic1.98540.00060.02780.001928.21ii1.98710.029426.8iia1.98680.00030.02760.0018281.2iib1.98730.00020.02940.000026.80iic1.98690.00020.02760.001827.91.1c4h12i1.99420.034730.2ia1.99430.00010.03400.000730.30.1ib1.99440.00020.03310.001631.41.2ic1.99430.00010.03260.002131.61.4ii1.99420.035230.1iia1.99420.00000.0354 + 0.0002300.1iib1.99430.00010.03340.001831.41.3iic1.99430.00010.03340.001831.31.2changes of  ,  * and s - char , respectively , caused by interaction with water molecules electron density in the (ch ) and *(ch ) orbitals and the s - character of the valence orbital on the c atom ( in % ) in isolated i and ii conformers and their complexes with h2o changes of  ,  * and s - char , respectively , caused by interaction with water molecules the values of the hyperconjugation energies ( e ) in the isolated conformers and their h2o complexes are collected in table  6 . in all the systems
, there is an intermolecular charge transfer from the lone pair orbital ( lp ) of the o atom of water ( ow ) to the *(c1h5 ) or *(c4h12 ) orbitals , as indicated by the corresponding second - order interaction energies ( einter ) in table  6 .
these energies are moderate , ranging from 1.8 to 3.6  kcal  mol , and are somewhat larger for the complexes formed at the c4h12 bond . 

table 6intermolecular second - order interaction energies ( e , kcal  mol ) in the i and ii complexes of enflurane with h2oiiaibiclpow    *(c1h5)1.941.84lpow    *(c4h12)3.613.54iiiiaiibiiclpow    *(c1h5)2.121.76lpow    *(c4h12)3.503.19 intermolecular second - order interaction energies ( e , kcal  mol ) in the i and ii complexes of enflurane with h2o finally , it should be noted that the interaction between enflurane and water results in a small perturbation of the normal vibrational modes of water . for the ic(1 ) complex as for example , the  and (oh ) stretching frequencies are red - shifted , by 13 and 12  cm , respectively , while the (oh ) bond frequency is blue - shifted by 12  cm .
it is also worth stressing that in contrast to most of the oh  o hydrogen bonds , the intensity ratio v(oh)/(oh ) is larger than 1 .
studies of the electrostatic potentials of the halogen bonded systems show that the lone electron pairs of the halogen atom bonded to the carbon atom form a belt of negative electrostatic potential around its central part leaving the outermost region positive , the so called -hole [ 44 , 45 ] . the halogen bonding was explained as a noncovalent interaction between a covalently bound halogen on one molecule and a negative site of another [ 4449 ] .
the structures of the halogen bonded enfluraneoh2 complexes optimized at the mp2/6311++g(d , p ) level are illustrated in fig.4 . 

4structures of halogen bonded complexes of enflurane with water molecule optimized at the mp2/6311++g(d , p ) level .
the dot lines indicate selected intermolecular distances ( in angstroms ) , angles are in degrees structures of halogen bonded complexes of enflurane with water molecule optimized at the mp2/6311++g(d , p ) level .
the dot lines indicate selected intermolecular distances ( in angstroms ) , angles are in degrees the c1-cl7 bond distance is equal to 1.748   in two complexes , thus , it is shorter by 0.004   relative to that in the enflurane monomers ( 1.752   ) .
the contraction of this bond is concomitant with an increase of the (c1cl7 ) stretching frequency ( blue - shift ) by + 2 and + 4  cm , in the i d and iid complexes , respectively .
the infrared intensities of the corresponding stretching mode decrease by 6 and 12  km  mol , respectively . as depicted in fig.4 , the intermolecular cl7o13 distances in the i d and iid complexes are equal to 3.17 and 3.18   , respectively .
these values are smaller than the sum of the van der waals radii of the chlorine and oxygen atoms , 3.27   . the analogous ( clo ) distance , in the halogen bonded enfluraneformaldehyde complex was found to be 3.30   . in biological molecules with the halogen bond , the average cclo angle is between 160 and 180 . in
the i d and iid complexes , the c1cl7o13 angles are 176.8 and 166.3 , respectively .
nbo analysis has revealed that in the halogen bonded enfluranewater complexes , the cl atom shows the largest change of the atomic charge , in comparison to isolated molecules . in i d and iid , the charge on cl increases by 0.026 and 0.023 e , respectively . as was mentioned earlier , the chlorine atom has three lone electron pairs which form a belt of negative electrostatic potential around the central part of this atom , leaving the outermost region positive ( -hole ) .
one of them ( lp(2)o13 ) is involved in the formation of the halogen bond , and it overlaps with the *(c1cl7 ) orbital of enflurane . in both the complexes considered , the second - order interaction energies ( e ) between the donor ( lp(2)o13 ) and acceptor ( *(c1cl7 ) ) orbitals are smaller than 0.5  kcal  mol .
the ccsd(t)/cbs stabilization energies for the i d and iid complexes are 1.81 and 1.89  kcal  mol , respectively .
thus , the halogen bonded enfluraneoh2 complexes are weaker than the hydrogen bonded enfluraneoh2 complexes , by more than 3  kcal  mol .
the two most stable structures of enflurane optimized at the mp2/6311++g(d , p ) level of theory are shown in fig.1 .
conformers i and ii differ in energy by only 0.07  kcal  mol . it should be mentioned that the stability order of the conformers is slightly different from that obtained at the mp2/6311g(2d ) level in our earlier studies .
conformers i and ii of the present work correspond to the b and c conformers of ref .
let us notice that in i , the two ch bonds are in a trans position , and in ii , the two ch groups adopt the cis position . 
 fig .
1structures of two most stable conformers of enflurane optimized at the mp/6311++g(d , p ) level of theory and the numbering of atoms structures of two most stable conformers of enflurane optimized at the mp/6311++g(d , p ) level of theory and the numbering of atoms the structures of enflurane ( i and ii ) complexes with one water molecule ( 1 - 1 ) are illustrated in fig . 
2 . as is seen , in the 1 - 1 complexes involving both conformers , water interacts with enflurane through ch 
ow hydrogen bonds , with the c1h5  ow or c4h12  ow distances varying between 2.23 and 2.32   . weak interaction between one of the f atoms and the h atom of water is also possible , the hw  f distances being much longer ( between 2.60 and 2.87   ) .
o3 complex has been found on the potential energy surface . in the ia complex ( fig . 
o3 distance is too long ( 2.80   ) to be classified as a true hydrogen bond . 

2structures of enflurane complexes with one water molecule optimized at the mp2/6311++g(d , p ) level .
the dot lines indicate selected intermolecular distances ( in angstroms ) , angles are in degrees structures of enflurane complexes with one water molecule optimized at the mp2/6311++g(d , p ) level .
the dot lines indicate selected intermolecular distances ( in angstroms ) , angles are in degrees the structures of enflurane complexes with two water molecules ( 12 ) are shown in fig . 
it is important to notice that in these complexes , the intermolecular distances remain approximately the same as in the 1 - 1 complexes , the ch  ow distances varying between 2.23 and 2.34   , and the owhw
 f distances being between 2.41 and 2.61   . in ia and ic , the o13h14 
f11 intermolecular angles are markedly larger ( 146 and 152 , respectively ) than the oh  f intermolecular angles in the remaining complexes ( 100110 ) .
further , the c4h12  ow hydrogen bonds tend to be more linear than the c1h5  ow .
it is worth mentioning that in the enflurane dimer , the o3 atoms do not participate in the interaction .
the two enflurane molecules having the trans conformation are held together by ch  f hydrogen bonds . 

3structures of enflurane complexes with two water molecules optimized at the mp2/6311++g(d , p ) level .
the dot lines indicate selected intermolecular distances ( in angstroms ) , angles are in degrees structures of enflurane complexes with two water molecules optimized at the mp2/6311++g(d , p ) level .
the dot lines indicate selected intermolecular distances ( in angstroms ) , angles are in degrees the enthalpy of deprotonation and protonation of the two conformers are presented in table  1 . 

table 1enthalpies of deprotonation of h5 or h12 atoms and proton affinities ( pa ) of o3 for the two most stable conformers of enflurane ( under standard conditions ) , calculated at the mp2/6311++g(d , p ) and ccsd(t)/cbs levels [ all values in kcal  mol]conformerhhidpe ( c1h5)365.6363.1dpe ( c4h12)367.5367.3pa150.3151.8iidpe ( c1h5)365.2362.8dpe ( c4h12)368.6368.1pa154.5156.4the numbering of atoms is shown in fig . 
1calculated as sum of e and zero - point vibrational energy and thermal correction to enthalpy obtained at the mp2 levelpa  =  h enthalpies of deprotonation of h5 or h12 atoms and proton affinities ( pa ) of o3 for the two most stable conformers of enflurane ( under standard conditions ) , calculated at the mp2/6311++g(d , p ) and ccsd(t)/cbs levels [ all values in kcal  mol ] the numbering of atoms is shown in fig .  1 calculated as sum of e and zero - point vibrational energy and thermal correction to enthalpy obtained at the mp2 level in the present systems , the ch 
this can be related to a larger basicity ( pa  =  165  kcal  mol ) and a lower acidity ( dpe  =  390  kcal  mol ) of water molecule , in comparison to the corresponding values calculated for the two conformers of enflurane .
h2o ( pa(o )  =  174  kcal  mol ) is stabilized by an owhw 
o interaction , while in the chfclochf2  h2o complex ( pa(o )  =  155  kcal  mol ) , the ch 
o , showing the predominance of the ch  ow hydrogen bond over the owhw  o interaction .
in contrast , the complex between ch2fcho ( pa(o )  =  161  kcal  mol , dpe(ch )  =  352.3  kcal  mol ) and water shows a preference for a cyclic structure , the owhw  o hydrogen bond being shorter than the ch 
table  2 lists the binding energies for the interaction of the i and ii conformers of enflurane with one water molecule calculated at the mp2/6311++g(d , p ) and ccsd(t)/cbs levels of theory .
the ccsd(t)/cbs stabilization energies for the ia , ib , iia and iib complexes are 5.89 , 5.04 , 4.67 and 4.66  kcal  mol , respectively .
these results indicate that ia and ib are more stable than the iia and iib complexes . 

table 2binding energies ( e and e ) and enthalpies of formation ( hf and hf ) of the enflurane - water complexes , calculated at the mp2/6311++g(d , p ) and ccsd(t)/cbs levels [ all values in kcal  mol]iaibiiaiibe4.594.163.833.85e5.895.044.674.66hf3.062.732.432.42hf4.353.583.293.22corrected for bsseenthalpy of formation under standard conditionszero - point vibrational energy and thermal correction to enthalpy obtained at the mp2 level binding energies ( e and e ) and enthalpies of formation ( hf and hf ) of the enflurane - water complexes , calculated at the mp2/6311++g(d , p ) and ccsd(t)/cbs levels [ all values in kcal  mol ] enthalpy of formation under standard conditions zero - point vibrational energy and thermal correction to enthalpy obtained at the mp2 level table  2 also shows the values of the enthalpies of formation of the enflurane - water complexes , calculated at both levels of theory ( under standard conditions in the gas phase ) .
the ccsd(t)/cbs calculated enthalpies of formation are 4.35 , -3.58 , 3.29 and 3.22  kcal  mol for the ia , ib , iia and iib complexes , respectively .
the negative value of enthalpy implies that the formation of the enflurane - water complexes is the exothermic process .
binding energies and dpes vary in a very small range and no correlation could be found between these two parameters as in the case of the halogenated ethers and water complexes .
cooperative and anti - cooperative effects have been the subject of many studies [ 23 , 2934 ] .
table  3 collects the total binding energies , sum of the pairwise interaction energies and the three - body contribution ( e3b ) to the interaction energies of the two complexes of enflurane with two water molecules ( ic and iic , shown in fig . 
3 ) , calculated at the mp2/6311++g(d , p ) and ccsd(t)/cbs levels of theory . 

table 3total binding interaction energy ( eint ) , sum of pairwise interaction energies ( e2b ) , and the three - body contribution ( e3b ) of enflurane ( enf ) complexes with water ( a and b ) molecules .
calculations performed at the mp2/6311++g(d , p ) and ccsd(t)/cbs levels [ all values in kcal  mol]mp2ccsd(t)iciiciciiceint9.017.6011.419.56e2b8.947.7511.329.68e3b0.070.150.090.12corrected for bsse total binding interaction energy ( eint ) , sum of pairwise interaction energies ( e2b ) , and the three - body contribution ( e3b ) of enflurane ( enf ) complexes with water ( a and b ) molecules .
calculations performed at the mp2/6311++g(d , p ) and ccsd(t)/cbs levels [ all values in kcal  mol ] as follows from this table , the ccsd(t)/cbs absolute value of the total interaction energy of ic amounts to 11.41  kcal  mol , and is larger ( by 1.85  kcal  mol ) than that of the complex iic . for the ic complex , the value of e3b is negative and very small ( 0.09  kcal  mol ) , which indicates that the cooperativity is negligible . in the case of the iic complex ,
the value of e3b is positive and small ( 0.12  kcal  mol , about 1  % of eint ) which implies the presence of a very weak anti - cooperative effect .
examples of the cooperativity effects have been recently illustrated in the cyclic complexes between cycloethers and h2o where both ch  ow and owhw  o are strengthened . as expected , with regard to the ic complex ( negligible cooperativity )
there is no change in the intermolecular ch  ow distances , in comparison to ia and ib , while in the iic complex ( a small anticooperativity ) the c1h5  o13 and c4h12 
o16 distances are longer , by 0.05 and 0.02   , than the corresponding distances in the iia and iib complexes , respectively .
complex formation with water results in a contraction of the ch bond involved in the ch  ow interaction along with a blue shift ( between 18 and 26  cm ) of the corresponding vibration .
blue shifts of the same order of magnitude ( between 19 and 25  cm ) were predicted for the complexes between enflurane and acetone ( i conformer , bound with water at the c1h5 and c4h12 sites ) . as seen in table  4 , an ir intensity increase was predicted for the complexes formed at the c1h5 bond , while an ir intensity decrease was predicted for the complexes formed at the c4h12 bond .
let us notice that the analogous variations of ir intensity have been observed experimentally   in our earlier work on enflurane complexes with acetone . 

table 4c - h distances ( r in  ) , frequencies (  in cm ) and corresponding infrared intensities ( a in km  mol ) of c - h stretching vibration in two conformers of enflurane and their complexes with water molecules .
calculations performed at the mp2/6311++g(d , p ) levelc1h5rraai1.09031855ia1.0890.0013204 + 1911 + 6ib1.0900.0003186 + 150ic1.0890.0013203 + 1811 + 6ii1.09031765iia1.0890.0013202 + 2612
+ 7iib1.0900.000317516 + 1iic1.0890.0013199 + 237 + 2c4h12i1.089321012ia1.0880.0003215 + 5111ib1.0880.0013229 + 1975ic1.0880.0013233 + 2375ii1.089320514iia1.0890.0003205015 + 1iib1.0880.0013229 + 2468iic1.0880.0013226 + 21410the corresponding structures are shown in figs .  1 and 2,changes in the bond length in comparison to the isolated conformer ,
changes in the (c - h ) frequency in comparison to the isolated conformer , changes in the ir intensity ( a ) c - h distances ( r in  ) , frequencies (  in cm ) and corresponding infrared intensities ( a in km  mol ) of c - h stretching vibration in two conformers of enflurane and their complexes with water molecules . calculations performed at the mp2/6311++g(d , p ) level the corresponding structures are shown in figs .  1 and 2 , changes in the bond length in comparison to the isolated conformer ,
changes in the (c - h ) frequency in comparison to the isolated conformer , changes in the ir intensity ( a ) the selected results from the nbo analysis are collected in table  5 . as seen in this table ,
the contraction of the c1h5 and c4h12 bonds mainly results from the decrease in occupancy of the corresponding *(ch ) orbital .
a small increase of the s - character of the c atom may also contribute to this contraction , which has been largely discussed in earlier works [ 3543 ] .
the interaction with water also leads to a decrease of the positive charge on c and an increase of this charge on the h atom . 

table 5electron density in the (ch ) and *(ch ) orbitals and the s - character of the valence orbital on the c atom ( in % ) in isolated i and ii conformers and their complexes with h2oc1h5**%  s - char% s - chari1.98600.029727.2ia1.98550.00050.02790.001828.31.1ib1.98600.00000.02960.000127.20ic1.98540.00060.02780.001928.21ii1.98710.029426.8iia1.98680.00030.02760.0018281.2iib1.98730.00020.02940.000026.80iic1.98690.00020.02760.001827.91.1c4h12i1.99420.034730.2ia1.99430.00010.03400.000730.30.1ib1.99440.00020.03310.001631.41.2ic1.99430.00010.03260.002131.61.4ii1.99420.035230.1iia1.99420.00000.0354 + 0.0002300.1iib1.99430.00010.03340.001831.41.3iic1.99430.00010.03340.001831.31.2changes of  ,  * and s - char , respectively , caused by interaction with water molecules electron density in the (ch ) and *(ch ) orbitals and the s - character of the valence orbital on the c atom ( in % ) in isolated i and ii conformers and their complexes with h2o changes of  ,  * and s - char , respectively , caused by interaction with water molecules the values of the hyperconjugation energies ( e ) in the isolated conformers and their h2o complexes are collected in table  6 . in all the systems
, there is an intermolecular charge transfer from the lone pair orbital ( lp ) of the o atom of water ( ow ) to the *(c1h5 ) or *(c4h12 ) orbitals , as indicated by the corresponding second - order interaction energies ( einter ) in table  6 .
these energies are moderate , ranging from 1.8 to 3.6  kcal  mol , and are somewhat larger for the complexes formed at the c4h12 bond . 

table 6intermolecular second - order interaction energies ( e , kcal  mol ) in the i and ii complexes of enflurane with h2oiiaibiclpow    *(c1h5)1.941.84lpow    *(c4h12)3.613.54iiiiaiibiiclpow    *(c1h5)2.121.76lpow    *(c4h12)3.503.19 intermolecular second - order interaction energies ( e , kcal  mol ) in the i and ii complexes of enflurane with h2o finally , it should be noted that the interaction between enflurane and water results in a small perturbation of the normal vibrational modes of water . for the ic(1 ) complex as for example , the  and (oh ) stretching frequencies are red - shifted , by 13 and 12  cm , respectively , while the (oh ) bond frequency is blue - shifted by 12  cm .
it is also worth stressing that in contrast to most of the oh  o hydrogen bonds , the intensity ratio v(oh)/(oh ) is larger than 1 .
studies of the electrostatic potentials of the halogen bonded systems show that the lone electron pairs of the halogen atom bonded to the carbon atom form a belt of negative electrostatic potential around its central part leaving the outermost region positive , the so called -hole [ 44 , 45 ] . the halogen bonding was explained as a noncovalent interaction between a covalently bound halogen on one molecule and a negative site of another [ 4449 ] .
the structures of the halogen bonded enfluraneoh2 complexes optimized at the mp2/6311++g(d , p ) level are illustrated in fig.4 . 

4structures of halogen bonded complexes of enflurane with water molecule optimized at the mp2/6311++g(d , p ) level .
the dot lines indicate selected intermolecular distances ( in angstroms ) , angles are in degrees structures of halogen bonded complexes of enflurane with water molecule optimized at the mp2/6311++g(d , p ) level .
the dot lines indicate selected intermolecular distances ( in angstroms ) , angles are in degrees the c1-cl7 bond distance is equal to 1.748   in two complexes , thus , it is shorter by 0.004   relative to that in the enflurane monomers ( 1.752   ) .
the contraction of this bond is concomitant with an increase of the (c1cl7 ) stretching frequency ( blue - shift ) by + 2 and + 4  cm , in the i d and iid complexes , respectively .
the infrared intensities of the corresponding stretching mode decrease by 6 and 12  km  mol , respectively . as depicted in fig.4 , the intermolecular cl7o13 distances in the i d and iid complexes are equal to 3.17 and 3.18   , respectively .
these values are smaller than the sum of the van der waals radii of the chlorine and oxygen atoms , 3.27   .
the analogous ( clo ) distance , in the halogen bonded enfluraneformaldehyde complex was found to be 3.30   . in biological molecules with the halogen bond ,
the i d and iid complexes , the c1cl7o13 angles are 176.8 and 166.3 , respectively .
nbo analysis has revealed that in the halogen bonded enfluranewater complexes , the cl atom shows the largest change of the atomic charge , in comparison to isolated molecules . in i
d and iid , the charge on cl increases by 0.026 and 0.023 e , respectively . as was mentioned earlier , the chlorine atom has three lone electron pairs which form a belt of negative electrostatic potential around the central part of this atom , leaving the outermost region positive ( -hole ) .
one of them ( lp(2)o13 ) is involved in the formation of the halogen bond , and it overlaps with the *(c1cl7 ) orbital of enflurane . in both
the complexes considered , the second - order interaction energies ( e ) between the donor ( lp(2)o13 ) and acceptor ( *(c1cl7 ) ) orbitals are smaller than 0.5  kcal  mol .
the ccsd(t)/cbs stabilization energies for the i d and iid complexes are 1.81 and 1.89  kcal  mol , respectively .
thus , the halogen bonded enfluraneoh2 complexes are weaker than the hydrogen bonded enfluraneoh2 complexes , by more than 3  kcal  mol .
1 ) in the enflurane complexes with one and two water molecules , the ch  ow hydrogen bonds are formed , with the ch  ow distances varying between 2.23 and 2.32   . a weak interaction between one of the f atoms and
the h atom of water is also possible , the hw  f distances being longer ( between 2.41 and 2.87   ) . no stable owhw 
this is line with our earlier results on enflurane dimer , where we have shown that the o atoms of enflurane ( oenf ) do not participate in hydrogen bonding .
2 ) the ch bonds involved in the ch  ow interaction are contracted with respect to those in isolated enflurane .
this is accompanied by a blue shift ( between 18 and 26  cm ) of the corresponding (ch ) stretching frequencies . for (ch )
vibrations an increase of the ir intensity was predicted for the complexes formed at the c1h5 bond , while a decrease of the ir intensity was calculated for the complexes formed at the c4h12 bond .
similar effects have been found in our earlier experimental and theoretical studies of the enflurane complexes with acetone .
3 ) the ccsd(t)/cbs stabilization energies of the hydrogen bonded enflurane - water complexes vary between 5.89 and 4.66  kcal  mol .
the values of the enthalpies of formation of these complexes , calculated at the same level of theory , range between 4.35 and 3.22  kcal  mol .
4 ) the ccsd(t)/cbs calculated three - body contribution to the total binding energy of the hydrogen bonded enflurane complex with two water molecules shows that the cooperativity effects are very weak .
5 ) the cl halogen bonding has been found in two enflurane complexes with water .
the intermolecular ( clo ) distances ( 3.17 and 3.18   ) are smaller than the sum of the corresponding van der waals radii .
the ccsd(t)/cbs stabilization energies for these complexes are 1.81 and 1.89  kcal  mol .
this indicates that the halogen bonded enfluraneoh2 complexes are weaker than the hydrogen bonded enflurane - water complexes .
 increase of the atmospheric concentration of halogenated organic compounds is partially responsible for a change of the global climate . in this work 
 we have investigated the interaction between halogenated ether and water , which is one of the most important constituent of the atmosphere . 
 the structures of the complexes formed by the two most stable conformers of enflurane ( a volatile anaesthetic ) with one and two water molecules were calculated by means of the counterpoise cp - corrected gradient optimization at the mp2/6311++g(d , p ) level . in these complexes the ch  
 ow hydrogen bonds are formed , with the h  ow distances varying between 2.23 and 2.32   . 
 a small contraction of the ch bonds and the blue shifts of the (ch ) stretching vibrations are predicted . 
 there is also a weak interaction between one of the f atoms and the h atom of water , with the hw  
 f distances between 2.41 and 2.87   . 
 the ccsd(t)/cbs calculated stabilization energies in these complexes are between 5.89 and 4.66  kcal  mol1 , while the enthalpies of formation are between 4.35 and 3.22  kcal  mol1 . 
 the cl halogen bonding between enflurane and water has been found in two complexes . 
 the intermolecular ( clo ) distance is smaller than the sum of the corresponding van der waals radii . 
 the ccsd(t)/cbs stabilization energies for these complexes are about 2  kcal  mol1.figurecomplex between enflurane and water molecules 
Introduction
Theoretical methods
Results and discussion
Hydrogen bonded enflurane complexes with water
Halogen bonded enflurane complexes with water
Conclusions