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The Solvation of Ca2+ with Gas Phase Clusters of Alcohol Molecules

  • Khadar Duale
  • Anthony J. StaceEmail author
Open Access
Research Article

Abstract

A comprehensive examination of how the identity of an alcohol molecule can change the behavior of a solvated, alkaline earth dication has been undertaken. The metal dication of Ca2+ has been clustered with a range of different alcohols to form [Ca(ROH)n]2+ complexes, where n lies in the range 2–20. Following collisional activation via electron capture from nitrogen gas, complexes for n in the range 2–6 exhibit a switch in reaction product as a function of n. For low values, solvated CaOH+ is the dominant fragment, but as n increases beyond 4, this is displaced by the appearance of solvated CaOR+. A separate study of unimolecular metastable decay by [Ca(ROH)n]2+ complexes found evidence of charge separation to form CaOH+(ROH)n−1 + R+. For two isomers of butanol, the n = 3 complexes were found to follow parallel, but different metastable pathways: one leading to the appearance of CaOH+ and another that resulted in proton abstraction to form ROH2+. These differences have been attributed to the precursor complexes adopting geometries where one ROH molecule occupies a secondary solvation shell. Comparisons were made with a previous study of magnesium complexes; [Mg(ROH)n]2+ show that the difference in second ionization energy Mg+ (15.09 eV) as opposed to Ca+ (11.88 eV) influences behavior. A complex between Ca2+ and 1-chloroethanol is shown to favor the formation of CaCl+ as opposed to CaOH+ as a unimolecular charge separation product, which is attributed to differences in bond energy in the precursor molecule.

Keywords

Calcium dication Clusters Alcohol molecules Charge separation Coulomb fission Switching reactions 

Introduction

Advances in the techniques available for generating metal dication complexes in the gas phase have made it possible to study a wide range of their chemical and spectroscopic properties [1, 2, 3]. Together, the two principal experimental methods for preparing such complexes, namely, electrospray [2] and pick-up [1], have investigated an extensive array of ligands in association with a wide range of metal dications. In this context, the pick-up technique has proved to be particularly versatile, having been shown to generate complexes with ligands ranging from argon [4] through to phosphorus-containing compounds [5]. Limitations in the range of solvents available to electrospray mean that, using this approach, experiments have been primarily restricted to metal dications in association with molecules suspended in water [2]. To date, there has been just one experimental study of the behavior of metal dications in association with ligands that constitute a homologous series [6]. In principle, such a series should provide an opportunity to explore changes in metal ion stability and solvation that may occur as a result of a systematic variation in one or more molecular properties. Such variations could include size (steric effects and differences in geometry between isomers), polarizability, and dipole moment. The earlier study showed the presence of a link between the propensity for metastable decay and the ionization energy of R, the radical that forms the complementary ion as a result of unimolecular charge separation [6]. Presented here are results from a series of experiments that have investigated the behavior of dication complexes consisting of Ca2+ in association with clusters composed of methanol, ethanol, 1,2-propanol, 1,2-butanol, t-butanol, and 1-chloroethanol. Observed chemical processes include unimolecular charge separation and the formation of CaOH+ and R+ and loss of the radicals H⋅ and R⋅, promoted by electron capture. Although there are common patterns of behavior within the range of molecules studied, there are also notable variations that appear to arise from differences in geometry.

The vast majority of previous gas phase studies of Ca2+ complexes have been in association with water molecules and the determination of hydration numbers [7, 8, 9, 10, 11, 12, 13, 14, 15, 16, 17], water ligand–binding energies, and proton transfer reactions. Kebarle and co-workers [7, 8, 9, 10] were able to determine hydration energies by establishing equilibrium conditions in the gas phase. Also observed were charge transfer products resulting from the interaction of doubly charged calcium with water molecules, where the reaction was interpreted in the form of a proton transfer step:

$$ {\left[\mathrm{Ca}{\left({\mathrm{H}}_2\mathrm{O}\right)}_n\right]}^{2+}\to {\left[\mathrm{Ca}\mathrm{OH}{\left({\mathrm{H}}_2\mathrm{O}\right)}_{n-k}\right]}^{+}+{\mathrm{H}}_3{\mathrm{O}}^{+}{\left({\mathrm{H}}_2\mathrm{O}\right)}_{k-2} $$
(1)

Similarly, Armentrout and co-workers have measured the charge-separation barriers for reaction (1) for n = 2 and 3 and determined water molecule–binding energies using threshold collision-induced dissociation [11, 12]. Williams and co-workers used blackbody radiation to measure binding energies and infrared laser spectroscopy to probe more extensive Ca2+ hydration [13, 14, 15]. Binding energies for Ca2+ complexes containing both water molecules and methanol molecules have been determined by Bruzzi and Stace [16, 17]. Theory has provided support for the conditions necessary to promote reaction (1) as a function of the number of water molecules present in these doubly charged complexes [18, 19].

With the exception of methanol as a ligand [18, 19, 20], there appear to have been no other experimental studies of the gas phase coordination and chemistry of the calcium dication in association with high members of the alcohol series. Likewise, liquid-phase studies in the form of experiments and computer simulations have focused primarily on the Ca2+/methanol system and the identification of solvation shells [21, 22]; however, Palka and Hawlicka did include longer-chain alcohols in their calculations on the competition between water and alcohol molecules for the solvation of Ca2+ [23]. Connections between the results presented here and gas-phase reactions observed between singly charged alkaline earth metals and ROH molecules will be discussed below.

Experimental Section

The apparatus used for generation, identification, and detection of gas-phase multiply charged metal–ligand complexes has been described extensively in previous publications [24, 25]. Briefly, mixed neutral clusters were produced by the adiabatic expansion of a gas mixture consisting of alcohol molecules entrained with argon through a pulsed supersonic nozzle. This mixture was generated by flowing argon through a reservoir holding a sample of the alcohol and adjusting the temperature of the latter with an ice bath to achieve optimum signal intensity. Neutral clusters of varying composition, including Arm, Arm(ROH)n, and (ROH)n, then passed through a region where calcium vapor (~ 10−2 mbar) was generated by a Knudsen effusion cell (DCA Instruments, EC-40-63-21) operating at 590 °C. Neutral calcium atoms colliding with the cluster beam produced mixed neutral clusters thought to be of the form CaArm(ROH)n. Since the beam consisted of a wide range of mixed clusters, a shutter at the exit to the oven was used to confirm the presence of calcium by noting differences in signal intensity with the shutter open and closed.

Neutral clusters, some of which contained a single metal atom, then entered the ion source of a high-resolution reverse geometry double focusing mass spectrometer (VG-ZAB-E), where they were subjected to electron ionization at energies of between 70 and 100 eV. Since only ions rather than neutral complexes were detected, it is very likely that extensive ligand evaporation took place following ionization, which is believed to help reduce the internal energy content of complexes. Accordingly, under most experimental conditions, no ion complexes of the form [Ca(Ar)m(ROH)n]z+ were detected. Instead, the recorded mass spectra contained a wide range of both singly and doubly charged complexes formed from different combinations of calcium atoms with each of the alcohol molecules. Also present were very intense signals arising from (ROH)nH+ ions and their fragmentation products. Fortunately, the resolution of the mass spectrometer was sufficient to allow a clear separation of the signals of interest.

In order to monitor the fragmentation patterns of [Ca(ROH)n]2+ complexes, extensive use has been made of the MIKES (mass-analyzed ion kinetic energy spectroscopy) technique [26]. Ions with a specific m/z value were selected using a magnet, and the products of their decay were then identified as they passed through an electrostatic analyzer (ESA). These measurements can provide evidence of the fragmentation pathways adopted by an ion of a certain size, which in turn can often be used to infer details of composition and structure. The MIKES technique can be used to study both unimolecular (metastable) decay and processes induced by collisional activation. A collision cell located between the magnet and the ESA allowed ions to enter and exit, while differential pumping located close to the cell ensured that the background pressure in the flight tube as a whole did not change significantly. Gas (nitrogen) was introduced into the cell via a needle valve, and a sufficient amount was added to reduce the intensity of the precursor ion by ~ 50%. In all cases, fragmentation was being detected in the 2nd field-free region (2nd ffr) between the magnetic and electric sectors.

Under normal circumstances, the laboratory-frame kinetic energy of a fragment ion, Ef, can be calculated from the following expression [26]:

$$ {E}_{\mathrm{f}}=\frac{m_{\mathrm{f}}{q}_{\mathrm{p}}}{m_{\mathrm{p}}{q}_{\mathrm{f}}}{E}_{\mathrm{p}} $$
(2)
where mf and mp are the masses of the fragment and precursor ions, respectively, qf and qp are their charges, and Ep is the initial kinetic energy of the precursor ion. By setting the ion source voltage to 5 kV, the electrostatic analyzer can be scanned to transmit ions with laboratory-frame kinetic energies from 10 keV downwards. Those ions that are recorded between 5 and 10 keV can only have come from reactions involving electron loss by the precursor ion. In order to accurately differentiate between processes taking place within the collision cell and those occurring elsewhere within the flight tube, a voltage, Vc, can be applied to the cell to give a separate, collision-induced signal that can be detected at a kinetic energy Efc given by the expression
$$ {E}_{\mathrm{f}\mathrm{c}}=\frac{m_{\mathrm{f}}{q}_{\mathrm{p}}}{m_{\mathrm{p}}{q}_{\mathrm{f}}}{E}_{\mathrm{p}}+\frac{m_{\mathrm{p}}{q}_{\mathrm{f}}-{m}_{\mathrm{f}}{q}_{\mathrm{p}}}{m_{\mathrm{p}}{q}_{\mathrm{f}}}{V}_{\mathrm{c}} $$
(3)

The precise value of the voltage applied to the cell was calibrated using the known collision-induced reactions of CO22+.

The MIKES technique has been employed to study two types of unimolecular (metastable) fragmentation that takes place in the absence of collisions and where fragmentation relies on the presence of residual internal energy remaining after electron ionization. As will be seen, following ionization sufficient internal energy remains in the complexes to promote two separate pathways: (i) unimolecular charge separation or Coulomb fission (UCS) in small complexes to give products of the form CaOH+, ROH2+, and R+ and (ii) neutral molecule loss in larger complexes. In contrast, collisional activation will be shown to promote a wide range of processes, including electron capture–induced dissociation. In all of the examples that follow, it is the heavier, metal-containing fragment ion that is detected; attempts to detected the lighter R+ or ROH2+ fragments have not been successful because of the much higher levels of instrumental discrimination and background interference.

Results and Discussion

Similar to earlier studies of [Mg(ROH)n]2+ complexes [6, 27, 28], the equivalent Ca2+ system exhibits a series of generic reactions involving both UCS and those induced by the presence of a collision gas, which in this case was nitrogen. The latter reactions can be summarized as follows:

$$ {\left[\mathrm{Ca}{\left(\mathrm{ROH}\right)}_n\right]}^{2+}+{\mathrm{N}}_2\to {\left[\mathrm{Ca}{\left(\mathrm{ROH}\right)}_{n-k}\right]}^{2+}+k\ \mathrm{ROH}+{\mathrm{N}}_2 $$
(4)
$$ {\left[\mathrm{Ca}{\left(\mathrm{ROH}\right)}_{\mathrm{n}}\right]}^{2+}+{\mathrm{N}}_2\to {\mathrm{Ca}}^{+}{\left(\mathrm{ROH}\right)}_{n-k}+k\ \mathrm{ROH}+{{\mathrm{N}}_2}^{+} $$
(5)
$$ {\left[\mathrm{Ca}{\left(\mathrm{ROH}\right)}_n\right]}^{2+}+{\mathrm{N}}_2\to {\mathrm{CaOH}}^{+}{\left(\mathrm{ROH}\right)}_{n-k-\mathrm{l}}+\mathrm{R}+k\ \mathrm{ROH}+{{\mathrm{N}}_2}^{+} $$
(6)
$$ {\left[\mathrm{Ca}{\left(\mathrm{ROH}\right)}_n\right]}^{2+}+{\mathrm{N}}_2\to {\mathrm{CaOR}}^{+}{\left(\mathrm{ROH}\right)}_{n-k-1}+k\ \mathrm{ROH}+\mathrm{H}+{{\mathrm{N}}_2}^{+} $$
(7)

Steps (5)–(7) are identified as electron capture–induced dissociation (ECID) as opposed to intracluster charge transfer; the occurrence of ECID is consistent with a previous interpretation of data on [Mg(ROH)n]2+ and [Mg(NH3)n]2+ complexes [6, 29]. In each case, the reason for this conclusion is that the kinetic energy profiles that accompany these steps are all comparatively narrow, which is in contrast to those reactions that can be unambiguously identified as involving intracluster charge transfer. The latter process results in Coulomb repulsion between the reaction products as they separate, and this leads to much broader kinetic energy profiles. The earlier study of [Mg(NH3)n]2+ complexes [29] illustrated the important contribution electron capture makes to the collision-induced fragmentation of doubly charged, metal-containing clusters. This work also illustrated how different collision gases influenced the efficiency of electron capture, and at the laboratory-frame kinetic energies used in these experiments, it has been found that charge reduction processes have comparatively high cross sections (~ 20 Å2) [30]. At the center of mass velocities used in these experiments, cross sections of this magnitude favor forward scattering, which helps to explain why the nature of the reaction products, i.e., steps (5)–(7), is quite different from that observed when dication complexes are subjected to comparatively low-energy collisions [11, 12]. A study of neutral molecule loss from hydrogen cluster ions at high collision energies also recorded collision cross sections of the order of ~ 20 Å2 [26], which would account for the presence of reaction (4) in many of the MIKE spectra presented below. Individual examples of UCS will be discussed as when they appear in the MIKE spectra.

As a function of size, n, the significance of each of steps (4)–(7) varies according to the nature of the alcohol, ROH, and individual examples will be discussed below. Unlike the equivalent Mg2+ system [6], none of the [Ca(ROH)n]2+ complexes appear to undergo the non-dissociative electron capture step:

$$ {\left[\mathrm{Ca}{\left(\mathrm{ROH}\right)}_n\right]}^{2+}+{\mathrm{N}}_2\to {\mathrm{Ca}}^{+}{\left(\mathrm{ROH}\right)}_n+{{\mathrm{N}}_2}^{+} $$
(8)

This absence could be as a consequence of the mismatch between the ionization energy of N2 (15.63 eV) and the electron affinity of Ca2+ (11.88 eV). In contrast, the close match between N2 and Mg2+ (15.09 eV) could favor electron transfer without dissociation. Since the nitrogen that is introduced as the collision gas has a thermal kinetic energy, no signal for N2+ is ever observed in these experiments.

Although the technique used to form complexes made it possible to generate dications with values of n extending from 2 to 20, those subject to detailed analysis were normally in the range 2 to 6. As will be seen below, these latter values of n were sufficient to establish the changes in behavior that were observed as a function of the size and composition for each [Ca(ROH)n]2+ system. Very rarely was n = 1 observed, which is attributed to instability due to Coulomb fission.

Ca2+/Methanol Complexes

A plot of recorded relative intensities of [Ca(CH3OH)n]2+ complexes as a function of size n is shown in Online Resource 1, where the profile exhibits a very similar trend to those recorded for numerous other metal dication complexes [4, 5, 24, 25] using the pick-up technique. The peak in intensity seen at n = 4 does not necessarily imply any favored coordination number, but is more likely to arise as a consequence of the fragmentation patterns of larger complexes, combined with the observation that, in comparison to complexes where n > 4, [Ca(CH3OH)4]2+ has a higher binding energy [17]. Since the system is not at equilibrium, the natural tendency is for complexes to fragment downwards towards the most stable unit, which itself often represents a compromise between a high binding energy and unimolecular charge separation driven by excess internal energy. Although n = 4 is most frequently the most intense ion in many of the systems studied, that is not always the case [31]. An earlier study of Coulomb fission in a wide range of small metal dication–ligand complexes [20] reported that [Ca(CH3OH)3]2+ showed evidence for the loss of CH3OH2+, but that no similar process could be identified for [Ca(CH3OH)2]2+, which instead loses CH3+. Very similar observations were made for Mg2+ [6]. Figure 1a shows a MIKE scan recorded following the collisional activation of [Ca(CH3OH)3]2+. The presence can be seen of both reactions (6) and (7) above, with the narrow peak profiles, particularly for reaction (6) being indicative of ECID. In contrast to this mix of reaction products, Figure 1b shows the results from a MIKE scan of [Ca(CH3OH)6]2+, where reaction (6) is no longer observed and fragmentation is now dominated by neutral ligand loss together with contributions from reaction (7). This transition from a mixture of CaOH+ and CaOCH3+ fragments to product ions that just contain the latter is gradual, but complete by n = 5.
Figure 1

(a) MIKE spectrum recorded following the collisional activation of [Ca(CH3OH)3]2+. The notation (0/+) identifies the fact that the k = 1 peak includes an underlying USC product C2H5+ that also carries a positive charge. Most of the fragmentation arises from electron capture–induced dissociation where N2+ is also formed and accompanied by processes that lead to neutral products together with the loss of 3 or 4 H atoms. (b) Spectrum recorded following the collisional activation of [Ca(CH3OH)6]2+. The peaks labeled 1–4 correspond to the loss of neutral molecules

Similar switching reactions involving singly charged alkaline earth metal ions in association with both water and methanol molecules have been the subject of experimental and theoretical studies [32, 33, 34, 35, 36, 37, 38, 39]. Since the outcome of electron capture in the experiments discussed here is the generation of a singly charged complex, comparable processes are to be expected. In their study of alkaline-earth metal ions complexed with water, Fuke and co-workers recorded mass spectra showing the presence of two types of ion at low masses: M+(H2O)n and MOH+(H2O)n (M+ = Mg or Ca) with the latter becoming the sole cation beyond n = 5 [32]. This transition was attributed to a difference in hydration energy, with MOH+ being more stable in the presence of large numbers of water molecules [32]. For the case of complexes between singly charged alkaline earth metals and methanol, both photo- and collisional-activation studies have shown evidence of switching reactions [35, 36, 37, 38, 39]. As part of their study of doubly charged metal ions complexed with solvent molecules, Kohler and Leary studied the low-energy collision-induced dissociation of [Ca(CH3OH)4]2+ [18, 19], where they observed CaOCH3+ as the dominant fragment, accompanied by a much weaker signal for CaOH+. Direct, collision-induced bond cleavage was assumed to be responsible for the appearance of these fragments, which, given the comparatively low collision energies used by Kohler and Leary [18, 19], is probably going to be more efficient than ECID. A theoretical analysis by Chan et al. [34] of the intracluster reaction channels available to [Ca(CH3OH)n]2+ and [Mg(CH3OH)n]2+ complexes concluded that switching arises from a more rapid decline in the reaction barrier to the elimination of H from the OH group than for the elimination of CH3. As n increases, solvation helps to stabilize the more polarizable CaOCH3+ ion core [34].

Ca2+/Ethanol Complexes

Figure 2a shows fragment ions recorded following collisions between N2 and [Ca(C2H5OH)2]2+, where two separate series of fragment ions is observed and centered on the formation of either CaOC2H5+ or CaOH+. The strong peak at ~ 7800 eV includes several processes contributing to the formation of CaOH+(C2H5OH), and removal of the collision gas reveals the metastable peak shown in Figure 3. The dish shape to the peak is indicative of Coulomb fission and corresponds to unimolecular charge separation to give C2H5+ as the complementary fragment ion. Earlier analysis of similar charge transfer processes made use of simple one-dimensional potential energy curves to account for the charged fragments [6, 25]. A series of curves depicting possible outcomes for Ca2+ + C2H5OH is shown in Figure 4, where the various positions have been determined through a combination of reaction exothermicities and ion-dipole and ion-induced dipole interaction energies. At best, the curves are semi-quantitative since there is no curve corresponding to proton transfer, as this would require two molecules, and no account has been taken of the influence additional molecules might have on stabilizing either the precursor or fragment ions. Tonkyn and Weisshaar [40] have previously used curves of the type shown in Figure 4 to differentiate between H transfer and electron transfer in collisions between metal dications and molecules; however, in the present case, the outcome is going to be different because the complexes are starting from within the potential well. As Figure 4 shows, the first curve crossing to be encountered correlates with Ca+OH and C2H5+ as reaction products. Slightly higher in energy is a curve crossing that correlates with the products Ca+ + C2H5OH+. Since metastable decay is normally associated with the pathway with the lowest energy barrier, the appearance of a peak for the loss of C2H5+ confirms the ordering of the potential curves seen in Figure 4. Applications of a more rigorous theory to the problem comes from the work of El-Nahas et al. [41] who analyzed the structure and stability of the [MgCH3OH]2+ complex. They concluded that the lowest-energy pathway was that leading to the formation of MgOH+ and CH3+ as charge transfer fragments [41].
Figure 2

(a) As for Fig. 1a, but following the collisional activation of [Ca(C2H5OH)2]2+. In this case, the UCS product is C2H5+. (b) Spectrum recorded following the collisional activation of [Ca(C2H5OH)6]2+. The peaks labeled 1–3 correspond to the loss of neutral molecules

Figure 3

Kinetic energy profile from an expanded section of Fig. 2a, but recorded in the absence of any collision gas. The peak arises from the unimolecular charge separation step: [Ca(C2H5OH)2]2+ → Ca+OH(C2H5OH) + C2H5+

Figure 4

Calculated potential energy curves for Ca+ + C2H5OH, showing the attractive ion-dipole and ion-induced dipole curves and the repulsive coulomb curve corresponding to the appearance of different charge separation products. The curve leading to CaOC2H5+ + H+ has been omitted because of the high energy required to generate H+

By applying a voltage to the collision cell (calibrated to be + 963 V), it is possible to separate reaction steps due to metastable decay from those initiated by collisional activation. Online Resource 1 shows an example where such an approach has been applied to the peak appearing at 7800 eV in Figure 2a. As can be seen, the metastable peak (a) identified in Figure 2a remains in position because it corresponds to decay throughout the entire 2nd ffr. However, a second feature appearing at ~ 7500 eV (b) corresponds to processes taking place within the collision cell, which together with CaOH+(C2H5OH) includes a range of singly charged products associated with the loss of one or more H atoms as a result of electron transfer with the nitrogen collision gas. Individual H atom loss could not be resolved in the present experiments, but is evident in previous studies of a similar nature [6, 28], and the peak width probably corresponds to the loss of 3 to 4 H atoms. A MIKE scan of [Ca(C2H5OH)3]2+ shows very similar reaction products to those seen for [Ca(C2H5OH)2]2+ and includes a strong signal arising from the metastable loss of C2H5+ from the precursor ion. Figure 2b shows the outcome of a scan on [Ca(C2H5OH)6]2+ following collisional activation, where it can be seen that, similar to the equivalent methanol complex, the reaction products are now entirely due to the formation of CaOC2H5+(C2H5OH)m, with no evidence of fragments containing CaOH+. Figure 2b also shows evidence of extensive loss of neutral molecules.

Ca2+/1-Propanol Complexes

Figure 5 shows a MIKE scan recorded following the collision of [Ca(C3H7OH)3]2+ ions with nitrogen. Once again, there is a mix of fragment ions corresponding to the formation of both CaOH+ and CaOC3H7+, with the former product ion no longer appearing once the precursor contains 6 1-propanol molecules. Both the n = 2 and n = 3 complexes exhibit strong metastable signals corresponding to the loss of C3H7+, and similar to that shown in Online Resource 1, metastable and ECID signals can be identified separately following the application of a voltage to the peak seen at ~ 8000 eV in Figure 5. An earlier study of strontium/1-propanol complexes, [Sr(C3H7OH)n]2+, also noted the presence of a strong metastable signal for the appearance of SrOH+ when n = 2, but failed to appreciate the role played by electron transfer in processes induced by collisional activation in complexes where n ≥ 3 [42].
Figure 5

As for Fig. 1a, but following the collisional activation of a complex with 1-propanol, [Ca(C3H7OH)3]2+. In this example, the UCS product is C3H7+

.

Ca2+/2-Propanol Complexes

As Figure 6 shows, there is a very close match between the MIKE scan recorded for 1-propanol and that shown in Figure 5 for 2-propanol. The peaks labeled a and b denote equivalent steps seen in both systems, whereas the peaks labeled c and d, along with that seen at ~ 4000 eV, cannot be assigned. Peak c is at a position that is equivalent to the loss of (CH3)2CHOH + 17 amu, and although the loss of H2O has been observed in protonated clusters of pure 2-propanol [43], the mismatch in mass is sufficient as to rule out that process here. The alternative is the loss of OH rather than water to give CaCH(CH3)2+HOCH(CH3)2; however, the formation of a metal–carbon bond has not been reported in other related studies. As with previous examples, the application of a voltage to the collision cell shows that the peak at ~ 8000 eV can be resolved into a strong metastable component for the loss of C3H7+ together with a range of ECID processes centered on the loss of neutral C3H7 possibly accompanied by the loss of one or two hydrogen atoms.
Figure 6

As for Fig. 1a, but following the collisional activation of a complex with 2-propanol, [Ca((CH3)2CHOH)3]2+. In this example, the UCS product is C3H7+

Ca2+/1-Butanol Complexes

The collisional activation of individual [Ca(C4H9OH)n]2+ complexes for small values of n resulted in sequences of product ions similar to those seen in previous examples, i.e., based on Ca+OC4H9 and CaOH+. Two of the complexes, n = 2 and 3, exhibited strong metastable signals, and an example recorded for [Ca(C4H9OH)3]2+ is shown in Figure 7. However, this particular complex also undergoes a second unimolecular step in the form of
Figure 7

Kinetic energy profile from the UCS decay of a complex with 1-butanol, [Ca(C4H9OH)3]2+ recorded in the absence of any collision gas. The peak arises from the unimolecular charge separation step: [Ca(C4H9OH)3]2+ → Ca+OH(C4H9OH)2 + C4H9+

$$ {\left[\mathrm{Ca}{\left({\mathrm{C}}_4{\mathrm{H}}_9\mathrm{OH}\right)}_3\right]}^{2+}\to {\mathrm{C}\mathrm{aOC}}_4{{\mathrm{H}}_9}^{+}\left({\mathrm{C}}_4{\mathrm{H}}_9\mathrm{OH}\right)+{\mathrm{C}}_4{\mathrm{H}}_9{{\mathrm{OH}}_2}^{+} $$
(9)

A similar observation was made on the corresponding Mg2+ complex, but in that case the two unimolecular reactions were observed for n = 4 rather than 3. The collisional activation of [Ca(C4H9OH)n]2+ complexes for n ≥ 4 resulted in product ions centered on the formation of CaOC4H9+, and no further metastable processes were observed.

Ca2+/2-Butanol Complexes

Complexes containing 2-butanol were not the subject of the earlier study involving Mg2+ [6]. The fragmentation patterns recorded for these complexes were almost identical to those seen for the equivalent series involving 1-butanol including the two metastable steps equivalent to those shown in Figure 7 and by reaction (9).

Ca2+/t-Butanol Complexes

The low vapor pressure of t-butanol resulted in very weak signals for this series of complexes. Signal intensity for the precursor ions peaked at n = 4 and the fragmentation pattern for this ion showed the presence of products containing CaOC(CH3)3+ and CaOH+. However, no metastable processes could be identified and once n = 6 almost all ECID signals had disappeared.

Ca2+/Chloroethanol Complexes

This final example has been chosen in order to explore the preference Ca+ might have for extracting a chlorine atom as opposed to the other two dominant products seen for the unsubstituted alcohol molecules studied above. These experiments were run using the more intense Cl35 isotope. As can be seen in Figure 8a, the collision-induced fragmentation pattern shows just a single reaction product in the form of fragment ions that are centered on the formation of CaCl+. Removal of the collision gas shows the peak seen at ~ 8400 eV to include a strong metastable component arising from the reaction:
Figure 8

(a) As for Fig. 1a, but following the collisional activation of a complex with 1-chloroethanol, [Ca(ClC2H4OH)3]2+. Note the complete absence of any of the ECID products identified following similar experiments on complexes with non-substituted alcohol molecules. (b) Calculated potential energy curves for Ca+ + ClC2H4OH, showing the attractive ion-dipole and ion-induced dipole curves and the repulsive coulomb curve corresponding to the appearance of different charge separation products

$$ {\left[\mathrm{Ca}{\left({\mathrm{C}\mathrm{lC}}_2{\mathrm{H}}_4\mathrm{OH}\right)}_3\right]}^{2+}\to {\mathrm{C}\mathrm{aCl}}^{+}{\left({\mathrm{C}\mathrm{lC}}_2{\mathrm{H}}_4\mathrm{OH}\right)}_2+{\mathrm{C}}_2{\mathrm{H}}_4{\mathrm{OH}}^{+} $$
(10)

Confirmation that reaction (10) is the most facile charge separation route can be seen in Figure 8b, where an analysis of reaction pathways using simple one-dimension potential energy curves, has been extended to include a route leading to the formation of Ca+Cl. As can be seen, the above pathway is the first to be encountered as the reactants move out from the potential well. Since Ca–Cl+ and Ca–OH+ have comparable bond strengths, 435 and 433 kJ mol−1, respectively [44], what appears to favor formation of the former over that of the latter is the ~ 55 kJ mol−1 difference in bond energy between Cl–C2H5OH and HO–C2H5Cl, which are estimated to be ~ 335 kJ mol−1 and ~ 390 kJ mol−1, respectively [44].

Conclusion

An extensive series of experiments have been undertaken to examine the influence different aliphatic alcohols have on the behavior of the dication complexes [Ca(ROH)n]2+. The results provide evidence of two types of switching reactions, each being associated with separate fragmentation pathways and each having a clearly recognizable kinetic energy release profile. The first switching reaction is induced by electron capture from a collision gas (nitrogen) and proceeds via the generation of a singly charged Ca+(ROH)n species. This ion subsequently decays to give a charged core which takes the form of either CaOH+ or CaOR+, with the latter gaining in intensity as n increases. This pattern of behavior matches that seen for a wide range of singly charged alkaline earth/ROH complexes, including those where R=H [32, 33, 34, 35, 36, 37, 38, 39]. A second form of switching reaction is summarized in Table 1 and is associated with those doubly charged [Ca(ROH)n]2+ ions that undergo unimolecular charge separation within the limited values of n as shown. These reactions give in each case two singly charged fragments either of the form CaOH+ as a core together with R+ or CaOR+ as a core together with ROH2+. This latter behavior could be attributed to complexes being formed where at least one molecule occupies a hydrogen-bonded site in the second solvation shell. The geometry of this arrangement would then facilitate the removal of a proton from a first-shell molecule to leave CaOR+ as a core. Examples of where a second solvation shell begins to develop before completion of the first shell have been identified previously in complexes with Mg2+ but not in any involving Ca2+ [6, 13, 14, 45]. Also included in Table 1 are equivalent results recorded for Mg2+ complexes. A qualitative trend observed for the latter was that for the generic metastable step:
Table 1

Summary of the Metastable, Unimolecular, Charge Separation Reactions (UCS) Observed When Each of the Alcohol Molecules Is Coordinated to Ca2+

Ligand

UCS(Ca2+)

n(Ca2+)

n(Mg2+)$

Charge separation

Proton transfer

IE (R)#

CH3OH!

Yes

3

3

CH3+ (n = 2)

CH3OH2+ (n = 3)

9.84

C2H5OH

Yes

3

3

C2H5+ (n = 2,3)

8.12

1-C3H7OH%

Yes

3

4

C3H7+ (n = 2,3)

8.09

2-C3H7OH

Yes

3

C3H7+ (n = 2,3)

7.37

1-C4H9OH

Yes

3

4

C4H9+ (n = 2,3)

C4H9OH2+ (n = 3)

8.02

2-C4H9OH

Yes

3

C4H9+ (n = 3)

C4H9OH2+ (n = 3)

7.25

t-C4H9OH

No

4

6.80

ClC2H4OH

Yes

C2H4OH+

6.70

Also given as IE(R) are the ionization energies of the radicals that are produced as complementary ions during charge separation. For [M(ROH)n]2+ complexes, n is the maximum values for which UCS is observed, where M is either Ca or Mg

!Taken from ref. [20]

$Data for Mg2+ complexes. Taken from ref. [6]

#Ionization energy in eV (taken from the NIST Chemistry WebBook)

%The complex [Sr(1-C3H7OH)2]2+ was also observed to undergo this UCS step [42]

$$ {\left[\mathrm{Mg}{\left(\mathrm{ROH}\right)}_n\right]}^{2+}\to {\mathrm{MgOH}}^{+}{\left(\mathrm{ROH}\right)}_{n-1}+{\mathrm{R}}^{+} $$
(11)

The value of n required to stabilize each complex against unimolecular charge separation increased as the ionization energy of R declined; the relevant data are given in Table 1. There appears to be no evidence of a similar trend in the data recorded for Ca2+, in that all of the complexes require four alcohol molecules to stabilize against charge separation. However, there are differences between Mg2+ and Ca2+, in that the higher ionization energy of the former requires five rather than four molecules of both 1-propanol and 1-butanol to stabilize against UCS.

Notes

Acknowledgements

KD would like to thank the University of Nottingham for the award of a studentship, and AJS would like to thank the Leverhulme Trust for the award of an Emeritus Fellowship.

Supplementary material

13361_2019_2263_MOESM1_ESM.pdf (213 kb)
ESM 1 (PDF 212 kb)

References

  1. 1.
    Stace, A.J.: Metal ion solvation in the gas phase: the quest for higher oxidation states. J. Phys. Chem. A. 106(35), 7993–8005 (2002)CrossRefGoogle Scholar
  2. 2.
    Combariza, M.Y., Fahey, A.M., Milshteyn, A., Vachet, R.W.: Gas-phase ion-molecule reactions of divalent metal complex ions: towards coordination structure analysis by mass spectrometry and some intrinsic coordination chemistry along the way. Int. J. Mass Spectrom. 244(2–3), 109–124 (2005)CrossRefGoogle Scholar
  3. 3.
    Schroder, D., Schwarz, H.: Generation, stability, and reactivity of small, multiply charged ions in the gas phase. J. Phys. Chem. A. 103(37), 7385–7394 (1999)CrossRefGoogle Scholar
  4. 4.
    Walker, N.R., Wright, R.R., Barran, P.E., Cox, H., Stace, A.J.: Unexpected stability of [Cu.Ar]2+, [Ag.Ar]2+, and [Au.Ar]2+ and their larger clusters. J. Chem. Phys. 114(13), 5562–5567 (2001)CrossRefGoogle Scholar
  5. 5.
    Puskar, L., Barran, P.E., Duncombe, B.J., Chapman, D., Stace, A.J.: Gas-phase study of the chemistry and coordination of lead(II) in the presence of oxygen-, nitrogen-, sulfur-, and phosphorous-containing ligands. J. Phys. Chem. A. 109(1), 273–282 (2005)CrossRefGoogle Scholar
  6. 6.
    Wu, B., Duncombe, B.J., Stace, A.J.: The solvation of Mg2+ in gas-phase clusters composed of alcohol molecules. J. Phys. Chem. A. 112(11), 2182–2191 (2008)CrossRefGoogle Scholar
  7. 7.
    Blades, A.T., Jayaweera, P., Ikonomou, M.G., Kebarle, P.: Ion-molecules clusters involving doubly charged metal-ions (M2+). Int. J. Mass Spectrom. Ion Process. 102, 251–267 (1990)CrossRefGoogle Scholar
  8. 8.
    Peschke, M., Blades, A.T., Kebarle, P.: Hydration energies and entropies for Mg2+, Ca2+, Sr2+ and Ba2+ from gas-phase ion-water equilibria determinations. J. Phys. Chem. A. 102(48), 9978–9985 (1998)CrossRefGoogle Scholar
  9. 9.
    Peschke, M., Blades, A.T., Kebarle, P.: Formation, acidity and charge reduction of the hydrates of doubly charged ion M2+ (Be2+, Mg2+, Ca2+, Zn2+). Int. J. Mass Spectrom. 185(SI), 685–699 (1999)CrossRefGoogle Scholar
  10. 10.
    Peschke, M., Blades, A.T., Kebarle, P.: Binding energies for doubly-charged ions M2+=Mg2+, Ca2+ and Zn2+ with the ligands L=H2O, acetone, and N-methylacetamide in complexes MLn 2+ for n=1 to 7 from gas phase equilibria determinations and theoretical calculations. J. Am. Chem. Soc. 122(42), 10440–10449 (2000)CrossRefGoogle Scholar
  11. 11.
    Carl, D.R., Moision, R.M., Armentrout, P.B.: Binding energies for the inner hydration shells of Ca2+: an experimental and theoretical investigation of Ca2+(H2O)x complexes (x=5-9). Int. J. Mass Spectrom. 265(2–3), 308–325 (2007)CrossRefGoogle Scholar
  12. 12.
    Carl, D.R., Armentrout, P.B.: Experimental investigation of the complete inner shell hydration energies of Ca2+: threshold collision-induced dissociation of Ca2+(H2O)x complexes (x=2-8). J. Phys. Chem. A. 116(15), 3802–3815 (2012)CrossRefGoogle Scholar
  13. 13.
    Rodriguez-Cruz, S.E., Jockusch, R.A., Williams, E.R.: Hydration energies of divalent metal ions, Ca2+(H2O)n (n=5-7) and Ni2+(H2O)n (n=6-8), obtained by blackbody infrared radiative dissociation. J. Am. Chem. Soc. 120(23), 5842–5843Google Scholar
  14. 14.
    Rodriguez-Cruz, S.E., Jockusch, R.A., Williams, E.R.: Hydration energies and structures of alkaline earth metal ions, M2+(H2O)n, n=5-7, M=Mg, Ca, Sr, and Ba. J. Am. Chem. Soc. 121(38), 8898–8906 (1999)CrossRefGoogle Scholar
  15. 15.
    Bush, M.F., Saykally, R.J., Williams, E.R.: Infrared action spectra of Ca2+(H2O)11-69 exhibit spectra signatures for condensed-phase structures with increasing cluster size. J. Am. Chem. Soc. 130(46), 15482–15489 (2008)CrossRefGoogle Scholar
  16. 16.
    Bruzzi, E., Stace, A.J.: Experimental measurements of water molecule binding energies for the second and third solvation shells of [ca(H2O)n]2+ complexes. R. Soc. Open Sci. 4(1), 160671 (2017)CrossRefGoogle Scholar
  17. 17.
    Bruzzi, E., Stace, A.J.: Experimental binding energies for the metal complexes [Mg(CH3OH)n]2+, [Ca(CH3OH)n]2+, and [Sr(CH3OH)n]2+ for n in the range 4-20. J. Phys. Chem. A. 118(40), 9357–9363 (2014)CrossRefGoogle Scholar
  18. 18.
    Miliordos, E., Xantheas, S.S.: Unimolecular and hydrolysis channels for the detachment of water from microsolvated alkaline earth dication (Mg2+, Ca2+, Sr2+, Ba2+) clusters. Theor. Chem. Accounts. 133(4), 1450 (2014)CrossRefGoogle Scholar
  19. 19.
    Kohler, M., Leary, J.A.: Gas-phase reactions of doubly charged alkaline earth and transition metal complexes of acetonitrile, pyridine, and methanol generated by electrospray ionization. J. Am. Soc. Mass Spectrom. 8(11), 1124–1133 (1997)CrossRefGoogle Scholar
  20. 20.
    Chen, X., Stace, A.J.: Gas phase measurements on the stabilization and solvation of metal dications in clusters of ammonia and methanol. J. Phys. Chem. A. 117(24), 5015–5022 (2013)CrossRefGoogle Scholar
  21. 21.
    Faralli, C., Pagliai, M., Cardini, G., Schettino, V.: Ab initio dynamics study of Mg2+ and Ca2+ ions in liquid methanol. J. Chem. Theory Comput. 4(1), 156–163 (2008)CrossRefGoogle Scholar
  22. 22.
    Megyes, T., Bálint, S., Bakó, I., Grósz, T., Radnai, T., Pálinkás, G.: Solvation of calcium ion in methanol: comparison of diffraction studies and molecular dynamics simulation. Chem. Phys. 327(2–3), 415–426 (2006)CrossRefGoogle Scholar
  23. 23.
    Palka, K., Hawlicka, E.: Influence of alcohols on Ca2+ hydration. J. Mol. Liq. 122(1–3), 28–31 (2005)CrossRefGoogle Scholar
  24. 24.
    Walker, N.R., Wright, R.R., Stace, A.J.: Stable Ag(II) coordination complexes in the gas phase. J. Am. Chem. Soc. 121(20), 4837–4844 (1999)CrossRefGoogle Scholar
  25. 25.
    Walker, N.R., Dobson, M., Wright, R.R., Barran, P.E., Murrell, J.N., Stace, A.J.: A gas-phase study of the coordination of Mg2+ with oxygen- and nitrogen-containing ligands. J. Am. Chem. Soc. 122(45), 11138–11145 (2000)CrossRefGoogle Scholar
  26. 26.
    Eden, S., Tabet, J., Samraoui, K., Louc, S., Farizon, B., Farizon, M., Ouaskit, S., Märk, T.: Absolute cross sections for the dissociation of hydrogen cluster ions in high-energy collisions with helium atoms. Phys. Rev. A. 73, 023201 (2006)CrossRefGoogle Scholar
  27. 27.
    Woodward, C.A., Dobson, M.P., Stace, A.J.: Chemistry of Mg+ and Mg2+ in association with methanol clusters. J. Phys. Chem. A. 101(12), 2279–2287 (1997)CrossRefGoogle Scholar
  28. 28.
    Woodward, C.A., Dobson, M.P., Stace, A.J.: Intracluster charge-transfer in [Mg.(C3H7OH)n]2+ complexes. J. Phys. Chem. 100(14), 5605–5607 (1996)CrossRefGoogle Scholar
  29. 29.
    Wu, B., Duncombe, B.J., Stace, A.J.: Fragmentation pathways of [Mg(NH3)n]2+ complexes: electron capture verses charge separation. J. Phys. Chem. A. 110(27), 8423–8432 (2006)CrossRefGoogle Scholar
  30. 30.
    Ishii, K., Itoh, A., Okuno, K.: Electron-capture cross sections of multiply charged slow ions of carbon, nitrogen and oxygen in He. Phys. Rev. A. 70(4), 042716 (2004)CrossRefGoogle Scholar
  31. 31.
    Duncombe, B.J., Duale, K., Buchanan-Smith, A., Stace, A.J.: The solvation of Cu2+ in gas-phase clusters of water and ammonia. J. Phys. Chem. A. 111(24), 5158–5165 (2007)CrossRefGoogle Scholar
  32. 32.
    Sanekata, M., Misaizu, F., Fuke, K., Iwata, S., Hashimoto, K.: Reactions of singly-charged alkaline-earth metal-ions with water clusters – characteristic size distribution of product ions. J. Am. Chem. Soc. 117(2), 747–754 (1995)CrossRefGoogle Scholar
  33. 33.
    Chan, K.W., Wu, Y., Liu, Z.-F.: Theoretical study on the intracluster elimination channels of Mg+ (CH3OH), Ca+ (CH3OH), Mg+(NH3) and Ca+(NH3). J. Phys. Chem. 112(37), 8534–8541 (2008)CrossRefGoogle Scholar
  34. 34.
    Chan, K.W., Wu, Y., Liu, Z.-F.: Solvation effects on the intracluster elimination channels in M+(L)n, where M+=Mg+ and Ca+, L=CH3OH, and NH3, and n=2-6. J. Phys. Chem. A. 112(37), 8542–8550 (2008)CrossRefGoogle Scholar
  35. 35.
    Lee, J.I., Qian, J., Sperry, D.C., Midey Jr., A.J., Donnelly, S.G., Farrar, J.M.: Photodissociation spectra for size-selected Sr+(CH3OH)n and Sr+(CD3OD)n clusters. J. Phys. Chem. A. 106(42), 9993–9998 (2002)CrossRefGoogle Scholar
  36. 36.
    Lee, J.I., Farrar, J.M.: Hot and cold clusters: photodissociation of Sr+(CH3OD)n through vibrationally excited intermediates. J. Phys. Chem. A 106(49), 11882–11890 (2002)Google Scholar
  37. 37.
    France, M.R., Pullins, S.H., Duncan, M.A.: Photodissociation of Mg+ (CH3OH)N complexes: evidence for the onset of solvation. Chem. Phys. 239(1–3), 447–457 (1998)CrossRefGoogle Scholar
  38. 38.
    Selegue, T.J., Lisy, J.M.: Intracluster ion-molecule reactions in M+(CH3OH)N where M=Na or Cs. J. Am. Chem. Soc. 116(11), 4874–4880 (1994)CrossRefGoogle Scholar
  39. 39.
    Anderson, A., Muntean, F., Walter, D., Rue, C., Armentrout, P.B.: Collision-induced dissociation and theoretical studies of Mg+ complexes with CO, CO2, NH3, CH4, CH3OH, and C6H6. J. Phys. Chem. A. 104(4), 692–705 (2000)CrossRefGoogle Scholar
  40. 40.
    Tonkyn, R., Wisshaar, J.C.: Reactions of gas-phase dipositive titanium ions with alkanes. J. Am. Chem. Soc. 108(22), 7128–7130 (1986)CrossRefGoogle Scholar
  41. 41.
    El-Nahas, A.M., El-Demerdash, S.H., El-Shereefy, E.E.: Quantum calculations on the structure and stability of Mg2+XH3OH complexes in the gas phase (X=C, Si, and Ge) Int. J. Mass Spectrom. 263(2–3), 267–275 (2007)CrossRefGoogle Scholar
  42. 42.
    Dobson, M.P., Stace, A.J.: The chemistry of Sr2+ in association with propanol clusters. Int. J. Mass Spectrom. 165, 5–12 (1997)CrossRefGoogle Scholar
  43. 43.
    Shukla, A.K., Stace, A.J.: Intermolecular ion molecule reactions in clusters – the reactions of aliphatic-alcohols. J. Phys. Chem. 92(9), 2579–2583 (1988)CrossRefGoogle Scholar
  44. 44.
    Luo, Y.R.: Bond dissociation energies. In: Haynes, W.M. (ed.) CRC Handbook of Chemistry and Physics, 91st ed. CRC Press/Taylor and Francis, Boca Raton (2011)Google Scholar
  45. 45.
    Bruzzi, E., Raggi, G., Parajuli, R., Stace, A.J.: Experimental binding energies for the metal complexes [Mg(NH3)n]2+, [Ca(NH3)n]2+, [Sr(NH3)n]2+ for n=4-20 determined from kinetic energy release measurements. J. Phys. Chem. A. 118(37), 8525–8532 (2014)CrossRefGoogle Scholar

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Authors and Affiliations

  1. 1.School of ChemistryThe University of NottinghamNottinghamUK
  2. 2.School of Biology, Chemistry and Forensic Science, Faculty of Science and Engineering, University of WolverhamptonWolverhamptonUK

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