Intermediates derived from -terphenyl in the methyltributylammonium bis[(trifluoromethyl)sulfonyl]imide ionic liquid saturated with carbon dioxide: Pulse radiolysis study

Rafał Kocia

Journal & Issue Details

Nukleonika

Journal Details

Format: Journal
eISSN: 1508-5791
First Published: 25 Mar 2014
Publication timeframe: 4 times per year
Languages: English

Ionic liquids (ILs) represent a unique class of solvents. The growing interest in this class of solvents is connected with their interesting physical and chemical properties (e.g., non- or low volatility, thermal stability, and combustion resistance) [1,2,3,4,5,6,7,8,9,10,11,12]. They were proposed as good media for the absorption and reduction of carbon dioxide (CO₂) [13,14,15,16,17,18], which are related to the good solubility of CO₂ gas in ILs [19,20,21,22,23,24,25,26,27,28].

Given the backdrop of the increasing energy consumption leading to increased CO₂ emissions around the world, there is immense interest in, as well as keen demand for, new materials and technology for CO₂ capture. The negative impact of changes in the atmospheric concentration of carbon dioxide on the environment is a matter raised many times while debating the sources of, and sustainable consumption strategies for, energy. Reducing greenhouse gas emissions (carbon dioxide, methane, tropospheric ozone, chlorofluorocarbons, and nitrogen oxides), especially CO₂, is key to the future of global energy policy.

Millions of tons of CO₂ emissions annually are a direct result of the burning of fossil fuels used in electricity production.

The atmospheric concentration of CO₂ has increased by 31% since the beginning of the industrial age in the mid-18th century. This level has been higher than ever in the last 650 000 years (the period for which reliable data from the ice cores were obtained) [29]. It has been estimated that about 75% of the increase in CO₂ concentration over the past 20 years is due to the burning of fossil fuels. The remaining 25% is largely due to land use, in particular deforestation [14]. In 2010, a total of 30.6 GT of CO₂ were released into the atmosphere [30]. The International Energy Agency reported that with regard to fuels, in 2010, 44% of the estimated CO₂ emissions came from coal, 36% from oil, and 20% from natural gas. A further increase in CO₂ concentration is expected due to the increased demand for fossil fuels, and thus their greater combustion and to a lesser extent change in land utilization.

Special Report on Emissions Scenarios states that the range of future CO₂ emissions will increase the concentration from 541 ppm to 970 ppm by 2100 [14]. Producing clean energy from sources of fossil fuels such as coal requires not only huge infrastructure but also efficient technologies for the capture and reduction of CO₂ emissions.

The high efficiency of catalysis involving metal complexes in ILs is a good application prospect of this factor to the radiation and the photochemical conversion of carbon dioxide (CO₂) in chemically useful energy products, and the CO₂ may then be an additional source of renewable energy. The advantage is the ability to synthesize ILs, and increased solubility of CO₂, dedicated for this purpose. ILs provide new perspectives for the development of this direction. They turn out to be an excellent environment for carrying out many chemical syntheses [1, 2]. Systems with high CO₂ solubility can be selected. Studies have appeared in which ILs serve a medium enabling the conversion of CO₂ into complex organic compounds [31, 32].

Not without significance is the value of ILs as alternative and more environmentally safe solvents of great importance for modern applications involving clean technologies. In particular, recycling ILs allows their repeated use, while enhancing the selectivity and efficiency of the products obtained.

The favorability for applications of ILs in the nuclear industry [4, 33] gave rise to the problem of their radiation chemistry.

There are many investigations that have used the pulse radiolysis technique, to investigate elementary processes in ILs, including the reactions of presolvated $(e_{presolv}^{-})$ ( {{\rm{e}}_{{\rm{presolv}}}^ - } ) and solvated $(e_{solv}^{-})$ ( {{\rm{e}}_{{\rm{solv}}}^ - } ) electrons, and charge and H transfer reactions [34,35,36,37,38,39,40,41,42,43,44,45,46,47,48,49,50]. The stability of ILs under ionizing radiation [51,52,53] has also been examined.

In previous studies, the formation of the triplet and singlet excited states of p-terphenyl, TP, and (³TP* and ¹TP*) in [MeBu₃N][NTf₂] IL was observed in the presence and absence of scavenger of electrons $(e_{presolv}^{-}, e_{solv}^{-})$ ( {{\rm{e}}_{{\rm{presolv}}}^ - ,\,{\rm{e}}_{{\rm{solv}}}^ - } ) and excited states of the IL components, i.e., ([MeBu₃N]⁺)* and ([NTf₂]⁻)*, benzophenone (BP). It was found that the energy transfer from the excited states of [MeBu₃N][NTf₂] IL is of negligible significance [54].

Radiolysis of pure [MeBu₃N][NTf₂] IL results in not only excitation but also ionization of its components. As has already been reported elsewhere [36,37,38,39,40,41,42, 44], the basic products of pulse irradiation of [MeBu₃N][NTf₂] IL are presolvated electrons $(e_{presolv}^{-})$ ( {{\rm{e}}_{{\rm{presolv}}}^ - } ) , solvated electrons $(e_{solv}^{-})$ ( {{\rm{e}}_{{\rm{solv}}}^ - } ) , electron-deficient centers (IL^⊕), radical anions (IL^Θ), and excited states (IL*) located on both the anions and cations of IL. Of late, some of the primary intermediates, i.e., $e_{presolv}^{-}$ {\rm{e}}_{{\rm{presolv}}}^ - , $e_{solv}^{-}$ {\rm{e}}_{{\rm{solv}}}^ - and IL^⊕ resulting from the radiolysis of a pure [MeBu₃N][NTf₂] IL, were also studied using TP [55–56]. An initial broad optical absorption spectrum observed in the pulse-irradiated deoxygenated IL [MeBu₃N][NTf₂] was dominated by the absorption band allocated to $e_{solv}^{-}$ {\rm{e}}_{{\rm{solv}}}^ - , as was shown previously [41]. Direct observation of the remaining primary products originated from [MeBu₃N][NTf₂] was not possible. TP was chosen as a probe since the transients originated from TP (radical anions [TP^•−], radical cations [TP^•+], singlet excited states [¹TP*], and triplet excited states [³TP*]) absorb in the available spectral region and are convenient for time-resolved measurements using UV-vis spectrophotometry [54,55,56,57,58,59,60,61,62]. Moreover, TEA was used as an electron donor and an effective scavenger of IL^⊕, ³TP*, and TP^•+.

In this work, pulse radiolysis investigations of several reactions bringing about the formation of intermediates originated from TP were carried out in carbon dioxide solutions of [MeBu₃N][NTf₂] IL. Such an approach should help to defeat, in part, a domination of the $e_{solv}^{-}$ {\rm{e}}_{{\rm{solv}}}^ - absorption band and additionally the overlapping of the absorption bands resulting from the presence of TP^•− and ³TP* in deoxygenated [MeBu₃N] [NTf₂] IL with that resulting from the presence of TP^•+, at short times [56].

Experimental

Pulse radiolysis coupled with the time-resolved UV-vis spectrophotometry was performed using the INCT LAE 10 linear accelerator with typical electron pulses lengths of 7–10 ns. A detailed description of the computer controlled experimental setup has been given elsewhere [44]. The system consists of the 150 W “quiet” xenon lamp (Hamamatsu E7536) with a suitable housing and a power supply, the ORIEL MSH 301 monochromator with two switchable outputs (one for a R955 photomultiplier and the second one for the ANDOR intensified charge coupled device [ICCD] camera), and the LeCroy WaveRunner 6051A oscilloscope with an internal memory of 16 Mb.

The samples placed in quartz cells (with optical path 1 cm) were purged with CO₂ and exposed to a pulse irradiation. All experiments were conducted at room temperature 20 ± 2°C. The data were normalized to a dose of 15 Gy per pulse, which was measured using the dinitrogen monoxide-saturated thiocyanate (KSCN) dosimeter (with G × ɛ = 4.8 × 10⁻⁴ m² · J⁻¹ for ${(SCN)}_{2}^{\cdot -}$ ( {{\rm{SCN}}} )_2^{ \bullet - } at 472 nm) [63]). The dose absorbed by [MeBu₃N][NTf₂] was reckoned using a correction factor that considers the difference between the electron densities of the IL investigated and the value, conforming to the dose of 18 Gy absorbed by [MeBu₃N][NTf₂], ascertained using the KSCN dosimeter [36, 42].

The concentration of [MeBu₃N][NTf₂] is ~2.6 M [55], and those of TP and TEA in [MeBu₃N][NTf₂] are 14 mM and 0.22 mM, respectively.

The IL was synthesized according to the procedure described earlier [41]. All other chemicals and gases, being of the highest and purest grade available, were used as supplied.

Results and discussion

Pulse radiolysis of [MeBu₃N][NTf₂] solution saturated with carbon dioxide containing TP

As a result of ionization of the IL, presolvated electrons $(e_{presolv}^{-})$ ( {{\rm{e}}_{{\rm{presolv}}}^ - } ) , electron-deficient centers (IL^⊕), and excited states of ionic liquids (IL*) are formed (see reaction 1). Presolvated electrons $(e_{presolv}^{-})$ ( {{\rm{e}}_{{\rm{presolv}}}^ - } ) are converted eventually to solvated electrons $(e_{solv}^{-})$ ( {{\rm{e}}_{{\rm{solv}}}^ - } ) (see reaction 2). In CO₂-saturated [MeBu₃N][NTf₂] containing TP, $e_{presolv}^{-}$ {\rm{e}}_{{\rm{presolv}}}^ - and $e_{solv}^{-}$ {\rm{e}}_{{\rm{solv}}}^ - react with CO₂, leading to the formation of carbon dioxide radical anions $({CO}_{2}^{\cdot -})$ ( {{\rm{CO}}_2^{ \bullet - }} ) (see reactions 3 and 4).

(1)

IL \to e_{presolv}^{-}, {IL}^{\oplus}, IL *

{\rm{IL}} \,\to\, {\rm{e}}_{{\rm{presolv}}}^ - ,\,{{\rm{IL}}^ \oplus },\,{\rm{IL}}^*

(2)

e_{presolv}^{-} \to e_{solv}^{-}

{\rm{e}}_{{\rm{presolv}}}^ - \,\to\, {\rm{e}}_{{\rm{solv}}}^ -

(3)

{CO}_{2} + e_{presolv}^{-} \to {CO}_{2}^{\cdot -}

{{\rm{CO}}_2}\,+ \,{\rm{e}}_{{\rm{presolv}}}^ - \,\to\, {\rm{CO}}_2^{ \bullet - }

(4)

{CO}_{2} + e_{solv}^{-} \to {CO}_{2}^{\cdot -}

{{\rm{CO}}_2}\,+ \,{\rm{e}}_{{\rm{solv}}}^ - \,\to\, {\rm{CO}}_2^{ \bullet - }

Thus, reactions 3 and 4 eliminate the direct reaction of TP with the $e_{presolv}^{-}$ {\rm{e}}_{{\rm{presolv}}}^ - and $e_{solv}^{-}$ {\rm{e}}_{{\rm{solv}}}^ - , and the formation of TP^•−. The ${CO}_{2}^{\cdot -}$ {\rm{CO}}_2^{ \bullet - } is characterized by a wide absorption band with low intensity in the UV range with a maximum at λ = 235 nm (ɛ = 3000 M⁻¹ · cm⁻¹) [63], which does not have the absorption spectrum within the experimentally available wavelength range.

The second-order rate constant of the reaction of carbon dioxide with hydrated electrons in aqueous solutions was found to be k = 7.7 × 10⁹ dm³·mol⁻¹·s⁻¹ [63, 64]. ${CO}_{2}^{\cdot -}$ {\rm{CO}}_2^{ \bullet - } has strong reducing properties and the redox pairs ${CO}_{2} / {CO}_{2}^{\cdot -}$ {{\rm{CO}}_{{2}}}/{\rm{CO}}_2^{ \bullet - } is E = −2.21 V vs. saturated calomel electrode (SCE) [65, 66]. The estimated solubility of carbon dioxide in the IL [MeBu₃N][NTf₂] is ~60 mM.

Irradiation of a 14 mM TP solution that is CO₂-saturated results in an absorption band with an intensity at a maximum of λ = 450 nm immediately after a pulse clearly smaller (Fig. 1A) than in an analog saturated argon solution (Fig. 1B) [55] and oxygen solution (Fig. 1C) [56]. The resulting initial broad absorption band with a maximum for λ = 450 nm is the result of the overlap of the absorption derived from the ³TP* and to a lesser extent the TP^•+. TP^•+ is formed in a reaction of the electron-deficient centers originated from ionic liquid (IL^⊕) with TP (see reaction 5) and its absorption bands, as recorded by Liu et al. [59]. Also, the reaction of CO₂ with TP^•+ cannot be excluded (see reaction 6). This is due to the concurrent presence of ³TP* and TP^•+, which absorb in this region as well (vide Table 1 in Kocia's study [56]). CO₂ reacts with a presolvated and solvated electron, thus eliminating the direct reaction of TP with the electron and thus the formation of TP^•−. TP excited states (¹TP* and ³TP*) remain, but the ¹TP* is a short-lived state and was not observed on the available timescale of the pulse radiolysis system. The ³TP* lives longer (see reaction 7), and so it will be one of the individuals responsible for the shape of the absorption band with a maximum for λ = 450 nm. The absorption recorded in Fig. 1 after electron pulse decreases and is characterized by absorption maximum located at λ = 450 nm with a slightly higher intensity. This spectrum can be assigned, with no doubt, mainly to ³TP*, keeping in mind its spectral properties (vide Table 1 in Kocia's study [56]).

(5)

{IL}^{\oplus} + TP \to {TP}^{\cdot +} + IL

{{\rm{IL}}^ \oplus }\,+ \,{\rm{TP}} \,\to\, {{\rm{TP}}^{ \bullet + }}\,+ \,{\rm{IL}}

(6)

{TP}^{\cdot +} + CO \to products

{{\rm{TP}}^{ \bullet + }}\,+ \,{\rm{CO}} \,\to\, {\rm{products}}

(7)

IL * + TP \to^{3} TP *

{\rm{IL}}^*\,+ \,\;{\rm{TP}} \,\to\, {\;^3}{\rm{TP}}^*

Transient absorption spectra registered after pulse irradiation of carbon dioxide (A), argon (B), and oxygen (C) saturated solutions of [MeBu₃N][NTf₂] IL containing 14 mM TP after the following time delays on the spectra shown, respectively. The dose applied was 18 Gy.

Direct reactions involving TP and CO₂ and their anion radicals in both directions are probably too slow for observation under the pulse radiolysis. Perhaps the equilibrium is established according to reaction 8. Since the redox pairs TP/TP^•− E = −2.45 V vs. SCE) [62] is more negative than the redox pairs ${CO}_{2} / {CO}_{2}^{\cdot -}$ {{\rm{CO}}_{{2}}}/{\rm{CO}}_2^{ \bullet - } and CO₂ concentration is several times higher than TP concentration, one can expect that the equilibrium (see reaction 8) will be shifted to the right.

(8)

{CO}_{2} + {TP}^{\cdot -} ⇄ TP + {CO}_{2}^{\cdot -}

\text{C}{{\text{O}}_{2}}+\text{T}{{\text{P}}^{\bullet -}}\rightleftarrows \text{TP}+\text{CO}_{2}^{\bullet -}

CO₂ reduction by TP^•− has been observed only in the presence of intermediate catalysts, transition metal complexes, e.g., iron and cobalt porphyrins, cobalt and iron phthalocyanines, cobalt corrins, or cobalt and iron corroles [67,68,69,70,71,72]. The photochemical activity of TP was particularly investigated in connection with CO₂ reduction [71]. In such systems, the CO₂ bound in the form of an appropriate complex was more easily reduced.

The transient spectra acquired after pulse irradiation of the carbon dioxide (A), argon (B), and oxygen (C) saturated [MeBu₃N][NTf₂] IL containing 14 mM of TP at various time delays are presented in Fig. 1.

The presence of ³TP* at short time domains in the presence of 60 mM CO₂ clearly shows that energy transfer from the excited IL* to TP (reaction 7) can contend to some degree with the quenching of the excited IL* by CO₂ (reaction 9). On the other hand, the lack of ³TP* at longer time scales (which in Ar-saturated and O₂-saturated ³TP* was still present [55, 56]) proves its quenching by CO₂ (see reaction 10).

(9)

IL * + {CO}_{2} \to products

{\rm{IL}}*\,+ \,{{\rm{CO}}_2} \,\to\, {\rm{products}}

(10)

^{3} TP * + {CO}_{2} \to products

^3{\rm TP}^*\,+ \,{{\rm{CO}}_2} \,\to\, {\rm{products}}

The respective absorbances presented at λ = 470 nm as a function of the logarithm of time are not single exponentials (Fig. 2). The decays happening within the time range <1 μs to <10 μs confirm in all probability the reactions of ³TP* (see reaction 10) and TP^•+ (see reaction 6) with CO₂.

The absorbance measured at λ = 470 nm as a function of the logarithm of time after pulse irradiation of carbon dioxide-saturated [MeBu₃N][NTf₂] IL solutions containing 14 mM TP.

Pulse radiolysis of [MeBu₃N][NTf₂] solution saturated with carbon dioxide containing TP and TEA

To further observe the absorption spectra of the corresponding intermediates originated from TP, triethylamine (TEA) was added (concentration up to 0.22 mM) to the [MeBu₃N][NTf₂] IL. TEA is a well-known scavenger of radical cations (see reaction 11) and excited states (see reactions 12 and 13). It is, however, unreactive toward solvated electrons and radical anions [55, 56, 60, 61].

(11)

{TP}^{\cdot +} + TEA \to TP + {TEA}^{\cdot +}

{{\rm{PT}}^{ \bullet + }}\,+ \,{\rm{TEA}} \,\to\, {\rm{TP}}\,+ \,{\rm{TE}}{{\rm{A}}^{ \bullet + }}

(12)

^{1} TP * + TEA \to {TP}^{\cdot -} + {TEA}^{\cdot +}

^{{1}}{\rm{TP^*}}\,+ \,{\rm{TEA}} \,\to\, {{\rm{TP}}^{ \bullet - }}\,+ \,{{\rm{TEA}}^{ \bullet + }}

(13)

^{3} TP * + TEA \to {TP}^{\cdot -} + {TEA}^{\cdot +}

^{{3}}{\rm{TP^*}}\,+ \,{\rm{TEA}} \,\to\, {{\rm{TP}}^{ \bullet - }}\,+ \,{{\rm{TEA}}^{ \bullet + }}

The transient spectra acquired after pulse irradiation of the carbon dioxide-saturated [MeBu₃N] [NTf₂] IL containing 14 mM of TP and 0.22 mM TEA at various time delays are presented in Fig. 3.

Transient absorption spectra registered after pulse irradiation of carbon dioxide-saturated solutions of [MeBu₃N][NTf₂] IL containing 14 mM TP and 0.22 mM TEA after the following time delays: 40 ns (circles), 100 ns (up triangles), 2 μs (squares), 10 μs (down triangles), 25 μs (stars), and 100 μs (diamonds). The dose applied was 18 Gy.

The transient absorption spectra registered from 40 ns to 2 μs after the pulses were characterized by a strong absorption band with λ_max = 470 nm and a weaker absorption band with λ_max = 440 nm indicating formation of TP^•− (Fig. 3) via reaction 13. As in the case of solutions without TEA, carbon dioxide efficiently eliminates presolvated electrons (see reaction 3) and solvated electrons (see reaction 4). Therefore, excited states of TP remain. This is possible because carbon dioxide, unlike oxygen [56], is not a scavenger of excited states. On the other hand, it is known that excited states react with TEA. ¹TP* reacts quickly in solutions, while ³TP* reacts more slowly. However, both give TP^•− in these reactions (see reactions 12 and 13). Thus, ³TP* is visible in the recorded spectra (increased absorption at λ = ~450 nm), and at the same time the disappearance of TP^•− will be slowed down by the formation of TP^•− in reaction 13, which is a slower reaction. On the other hand, ¹TP* present only during the impulse can give TP^•− in reaction 12, while absorption from TP^•+ is substantially reduced due to the elimination of TP^•+ and its precursors in the reaction with TEA (see reaction 11).

The absorbance measured at λ = 450 nm, λ = 470 nm, and λ = 475 nm (Fig. 4) as a function of the logarithm of time after pulse irradiation of carbon dioxide-saturated [MeBu₃N][NTf₂] IL solutions containing 14 mM TP and 0.22 mM TEA show several exponential decays in the observed time scale.

The absorbance measured at λ = 450 nm (black circles), λ = 470 nm (red squares), and λ = 475 nm (blue up triangles) as a function of the logarithm of time after pulse irradiation of carbon dioxide-saturated [MeBu₃N] [NTf₂] IL solutions containing 14 mM TP and 0.22 mM TEA.

In measuring the absorption decay for λ = 450, λ = 470 nm, or λ = 475 nm, the aim is to answer the question of whether ³TP*, as a result of its reaction with TEA, is converted to a TP^•− or to other products. If these three waveforms are compared, the share of the first stage of decay for λ = 450 nm (Fig. 4) is almost twice that of the second stage. For λ = 470 nm (Fig. 4) and λ = 475 nm (Fig. 4), the separation of the decay into individual stages is too complex. Complex absorption decay curves (Fig. 4) show that there are probably at least two individuals, ³TP* and TP^•−. The pseudo first-order rates constant for λ = 450, λ = 470 nm, and λ = 475 nm absorption decay were calculated and are equal to ~1.4 × 10⁵ s⁻¹, ~1.0 × 10⁵ s⁻¹, and ~5.6 × 10⁵ s⁻¹, respectively. Decay for λ = 450 nm (Fig. 4) in the range up to 1 μs is slightly faster than for λ = 470 nm (Fig. 4). A faster decay corresponding to λ = 450 nm (representing the maximum absorption of ³TP*) may also indicate that the reaction of ³TP* with TEA has a role in leading the formation of TP^•− (see reaction 13).

Summary

Measurements conducted of the [MeBu₃N][NTf₂] solutions containing TP and saturated with carbon dioxide, an electron acceptor, showed that the direct reaction of CO₂ with TP^•− is too slow for observation under pulse radiolysis. The wide absorption band obtained immediately after the pulse with a maximum for λ = 450 nm is the result of the overlap of the absorption originating from the triplet excited state of TP and the radical cation of TP.

No presence of TP^•− can be explained by the fact that CO₂ (which exhibits a good solubility in [MeBu₃N][ NTf₂]) reacts effectively with presolvated and solvated electrons, thus eliminating the direct reaction of TP with the electrons and thereby forming TP^•−.

However, in the irradiated TP solution saturated with CO₂ with the addition of TEA, the share of TP^•− in the registered spectrum can be seen. It arises from the conversion of excited states of TP, primarily ¹TP*.

The obtained results confirm that ILs are a suitable medium for the recognition of reaction mechanisms related to CO₂ reduction. The high efficiency of CO₂ absorption makes ILs good candidates for environmental applications, and they could thus be successfully used, among other utilities, in membranes for capturing CO₂ from natural gas before combustion and flue gases after combustion.

The obtained results will contribute to the development of research on CO₂ capture and conversion, and in the future, perhaps to the creation of a CO₂ trading market, which will enable its capture and conversion into commercial products.

Figures & Tables

Transient absorption spectra registered after pulse irradiation of carbon dioxide (A), argon (B), and oxygen (C) saturated solutions of [MeBu3N][NTf2] IL containing 14 mM TP after the following time delays on the spectra shown, respectively. The dose applied was 18 Gy.

The absorbance measured at λ = 470 nm as a function of the logarithm of time after pulse irradiation of carbon dioxide-saturated [MeBu3N][NTf2] IL solutions containing 14 mM TP.

Transient absorption spectra registered after pulse irradiation of carbon dioxide-saturated solutions of [MeBu3N][NTf2] IL containing 14 mM TP and 0.22 mM TEA after the following time delays: 40 ns (circles), 100 ns (up triangles), 2 μs (squares), 10 μs (down triangles), 25 μs (stars), and 100 μs (diamonds). The dose applied was 18 Gy.

References

1 Welton, T. (1999). Room-temperature ionic liquids: solvents for synthesis and catalysis. Chem. Rev., 99(8), 2071–2084. DOI: 10.1021/cr980032t. WeltonT. 1999 Room-temperature ionic liquids: solvents for synthesis and catalysis Chem. Rev. 99 8 2071 2084 10.1021/cr980032t 11849019 Open DOI Search in Google Scholar

2 Wasserscheid, P., & Keim, W. (2000). Ionic liquids – new “solutions” for transition metal catalysis. Angew. Chem. Int. Ed., 39(21), 3772–3789. DOI: 1433-7851/00/3921-3773. WasserscheidP. KeimW. 2000 Ionic liquids – new “solutions” for transition metal catalysis Angew. Chem. Int. Ed. 39 21 3772 3789 1433-7851/00/3921-3773 Open DOI Search in Google Scholar

3 Earle, M. J., & Seddon, K. R. (2000). Ionic liquids. Green solvents for the future. Pure Appl. Chem., 72(7), 1391–1398. DOI: 10.1351/pac200072071391. EarleM. J. SeddonK. R. 2000 Ionic liquids. Green solvents for the future Pure Appl. Chem. 72 7 1391 1398 10.1351/pac200072071391 Open DOI Search in Google Scholar

4 Rogers, R. D., & Seddon, K. R. (2002). Ionic liquids: Industrial applications to green chemistry. Washington, USA: The American Chemical Society. RogersR. D. SeddonK. R. 2002 Ionic liquids: Industrial applications to green chemistry Washington, USA The American Chemical Society 10.1021/bk-2002-0818 Search in Google Scholar

5 Chiappe, C., & Pieraccini, D. (2005). Ionic liquids: Solvent properties and organic reactivity. J. Phys. Org. Chem., 18(4), 275–297. DOI: 10.1002/poc.863. ChiappeC. PieracciniD. 2005 Ionic liquids: Solvent properties and organic reactivity J. Phys. Org. Chem. 18 4 275 297 10.1002/poc.863 Open DOI Search in Google Scholar

6 Jain, N., Kumar, A., Chauhan, S., & Chauhan, S. M. S. (2005). Chemical and biochemical transformations in ionic liquids. Tetrahedron, 61, 1015–1060. DOI: 10.1016/j.tet.2004.10.070. JainN. KumarA. ChauhanS. ChauhanS. M. S. 2005 Chemical and biochemical transformations in ionic liquids Tetrahedron 61 1015 1060 10.1016/j.tet.2004.10.070 Open DOI Search in Google Scholar

7 Zhao, H., Xia, S., & Ma, P. (2005). Use of ionic liquids as ‘green’ solvents for extractions. J. Chem. Technol. Biotechnol., 80(10), 1089–1096. DOI: 10.1002/jctb.1333. ZhaoH. XiaS. MaP. 2005 Use of ionic liquids as ‘green’ solvents for extractions J. Chem. Technol. Biotechnol. 80 10 1089 1096 10.1002/jctb.1333 Open DOI Search in Google Scholar

8 Weyershausen, B., & Lehmann, K. (2005). Industrial application of ionic liquids as performance additives. Green Chem., 7(1), 15–19. DOI: 10.1039/b411357h. WeyershausenB. LehmannK. 2005 Industrial application of ionic liquids as performance additives Green Chem. 7 1 15 19 10.1039/b411357h Open DOI Search in Google Scholar

9 Endres, F., & El Abedin, S. Z. (2006). Air and water stable ionic liquids in physical chemistry. Phys. Chem. Chem. Phys., 8(18), 2101–2116. DOI: 10.1039/b600519p. EndresF. El AbedinS. Z. 2006 Air and water stable ionic liquids in physical chemistry Phys. Chem. Chem. Phys. 8 18 2101 2116 10.1039/b600519p 16751868 Open DOI Search in Google Scholar

10 Hough, W. L., Smiglak, M., Rodríguez, H., Swatloski, R. P., Spear, S. K., Daly, D. T., Pernak, J., Grisel, J. E., Carliss, R. D., Soutullo, M. D., Davis, Jr. J. H., & Rogers, R. D. (2007). The third evolution of ionic liquids: active pharmaceutical ingredients. New J. Chem., 31(8), 1429–1436. DOI: 10.1039/b706677p. HoughW. L. SmiglakM. RodríguezH. SwatloskiR. P. SpearS. K. DalyD. T. PernakJ. GriselJ. E. CarlissR. D. SoutulloM. D. DavisJ. H.Jr. RogersR. D. 2007 The third evolution of ionic liquids: active pharmaceutical ingredients New J. Chem. 31 8 1429 1436 10.1039/b706677p Open DOI Search in Google Scholar

11 Plechkova, N. V., & Seddon, K. R. (2008). Applications of ionic liquids in the chemical industry. Chem. Soc. Rev., 37(1), 123–150. DOI: 10.1039/b006677j. PlechkovaN. V. SeddonK. R. 2008 Applications of ionic liquids in the chemical industry Chem. Soc. Rev. 37 1 123 150 10.1039/b006677j 18197338 Open DOI Search in Google Scholar

12 Armand, M., Endres, F., MacFarlane, D. R., Ohno, H., & Scrosati, B. (2009). Ionic-liquid materials for the electrochemical challenges of the future. Nat. Mater., 8(8), 621–629. DOI: 10.1038/nmat2448. ArmandM. EndresF. MacFarlaneD. R. OhnoH. ScrosatiB. 2009 Ionic-liquid materials for the electrochemical challenges of the future Nat. Mater. 8 8 621 629 10.1038/nmat2448 19629083 Open DOI Search in Google Scholar

13 U.S. Department of Energy National Energy Technology Laboratory. (2013). Program Plan Carbon Capture. Albany: U.S. Department of Energy, Office of Fossil Energy, National Energy Technology Laboratory, Strategic Center for Coal. www.netl.doe.gov/technologies/carbon_seq/core_rd/co2capture.html.2009. U.S. Department of Energy National Energy Technology Laboratory 2013 Program Plan Carbon Capture Albany U.S. Department of Energy, Office of Fossil Energy, National Energy Technology Laboratory, Strategic Center for Coal www.netl.doe.gov/technologies/carbon_seq/core_rd/co2capture.html.2009. Search in Google Scholar

14 Houghton, J. T., Ding, Y., Griggs, D. J., Noguer, M., van der Linden, P. J., Dai, X., Maskell, K., & Johnson, C. A. (2001). Climate change 2001: The scientific basis. Contribution of working group I to the third assessment report of the intergovernmental panel on climate change. Cambridge, UK: Cambridge University Press. HoughtonJ. T. DingY. GriggsD. J. NoguerM. van der LindenP. J. DaiX. MaskellK. JohnsonC. A. 2001 Climate change 2001: The scientific basis. Contribution of working group I to the third assessment report of the intergovernmental panel on climate change Cambridge, UK Cambridge University Press Search in Google Scholar

15 Bates, E. D., Mayton, R. D., Ntai, I., & Davis, Jr. J. H. (2002) CO₂ capture by a task-specific ionic liquid. J. Am. Chem. Soc., 124(6), 926–927. DOI: 10.1021/ja017593d. BatesE. D. MaytonR. D. NtaiI. DavisJ. H.Jr. 2002 CO₂ capture by a task-specific ionic liquid J. Am. Chem. Soc. 124 6 926 927 10.1021/ja017593d 11829599 Open DOI Search in Google Scholar

16 Bara, J. E., Camper, D. E., Gin, D. L., & Noble, R. D. (2010). Room-temperature ionic liquids and composite materials: platform technologies for CO₂ capture. Acc. Chem. Res., 43(1), 152–159. DOI: 10.1021/ar9001747. BaraJ. E. CamperD. E. GinD. L. NobleR. D. 2010 Room-temperature ionic liquids and composite materials: platform technologies for CO₂ capture Acc. Chem. Res. 43 1 152 159 10.1021/ar9001747 19795831 Open DOI Search in Google Scholar

17 Zhang, Z., Hu, S., Song, J., Li, W., Yang, G., & Han, B. (2009). Hydrogenation of CO₂ to formic acid promoted by a diamine-functionalized ionic liquid. ChemSus-Chem., 2(3), 234–238. DOI: 10.1002/cssc.200800252. ZhangZ. HuS. SongJ. LiW. YangG. HanB. 2009 Hydrogenation of CO₂ to formic acid promoted by a diamine-functionalized ionic liquid ChemSus-Chem. 2 3 234 238 10.1002/cssc.200800252 19266516 Open DOI Search in Google Scholar

18 Ghavre, M., Morrissey, S., & Gathergood, N. (2011). Hydrogenation in ionic liquid. In A. Kokorin (Ed.), Ionic liquids: Applications and perspectives (pp. 331–392). Rijeka, Croatia, HR: InTech Open Access Publisher. GhavreM. MorrisseyS. GathergoodN. 2011 Hydrogenation in ionic liquid In KokorinA. (Ed.), Ionic liquids: Applications and perspectives 331 392 Rijeka, Croatia, HR InTech Open Access Publisher 10.5772/14315 Search in Google Scholar

19 Blanchard, L. A., Gu, Z. Y., & Brennecke, J. F. (2001). High-pressure phase behavior of ionic liquid/CO₂ systems. J. Phys. Chem. B, 105(12), 2437–2444. DOI: 10.1021/jp003309d. BlanchardL. A. GuZ. Y. BrenneckeJ. F. 2001 High-pressure phase behavior of ionic liquid/CO₂ systems J. Phys. Chem. B 105 12 2437 2444 10.1021/jp003309d Open DOI Search in Google Scholar

20 Buzzeo, M. C., Klymenko, O. V., Wadhawan, J. D., Hardacre, C., Seddon, K. R., & Compton, R. G. (2004). Kinetic analysis of the reaction between electrogenerated superoxide and carbon dioxide in the room temperature ionic liquids 1-ethyl-3-methylimidazolium bis(trifluoromethylsulfonyl)imide and hexyltriethylammonium bis(trifluoromethyl-sulfonyl) imide. J. Phys. Chem. B, 108(12), 3947–3954. DOI: 10.1021/jp031121z. BuzzeoM. C. KlymenkoO. V. WadhawanJ. D. HardacreC. SeddonK. R. ComptonR. G. 2004 Kinetic analysis of the reaction between electrogenerated superoxide and carbon dioxide in the room temperature ionic liquids 1-ethyl-3-methylimidazolium bis(trifluoromethylsulfonyl)imide and hexyltriethylammonium bis(trifluoromethyl-sulfonyl) imide J. Phys. Chem. B 108 12 3947 3954 10.1021/jp031121z Open DOI Search in Google Scholar

21 Aki, S. N. V. K., Mellein, B. R., Saurer, E. M., & Brennecke, J. F. (2004). High-pressure phase behavior of carbon dioxide with imidazolium-based ionic liquids. J. Phys. Chem. B, 108(52), 20355–20365. DOI: 10.1021/jp046895+. AkiS. N. V. K. MelleinB. R. SaurerE. M. BrenneckeJ. F. 2004 High-pressure phase behavior of carbon dioxide with imidazolium-based ionic liquids J. Phys. Chem. B 108 52 20355 20365 10.1021/jp046895+ Open DOI Search in Google Scholar

22 Anthony, J. L., Anderson, J. L., Maginn, E. J., & Brennecke, J. F. (2005). Anion effects on gas solubility in ionic liquids. J. Phys. Chem. B, 109(13), 6366–6374. DOI: 10.1021/jp046404l. AnthonyJ. L. AndersonJ. L. MaginnE. J. BrenneckeJ. F. 2005 Anion effects on gas solubility in ionic liquids J. Phys. Chem. B 109 13 6366 6374 10.1021/jp046404l 16851709 Open DOI Search in Google Scholar

23 Cadena, C., Anthony, J. L., Shah, J. K., Morrow, T. I., Brennecke, J. F., & Maginn, E. J. (2004). Why is CO₂ so soluble in imidazolium-based ionic liquids? J. Am. Chem. Soc., 126(16), 5300–5308. DOI: 10.1021/ja039615x. CadenaC. AnthonyJ. L. ShahJ. K. MorrowT. I. BrenneckeJ. F. MaginnE. J. 2004 Why is CO₂ so soluble in imidazolium-based ionic liquids? J. Am. Chem. Soc. 126 16 5300 5308 10.1021/ja039615x 15099115 Open DOI Search in Google Scholar

24 Ohlin, C. A., Dyson, P. J., & Laurenczy, G. (2004). Carbon monoxide solubility in ionic liquids: determination, prediction and relevance to hydroformylation. Chem. Commun., 35(9), 1070–1071. DOI: 10.1039/b401537a. OhlinC. A. DysonP. J. LaurenczyG. 2004 Carbon monoxide solubility in ionic liquids: determination, prediction and relevance to hydroformylation Chem. Commun. 35 9 1070 1071 10.1039/b401537a 15116189 Open DOI Search in Google Scholar

25 Husson-Borg, P., Majer, V., & Costa Gomes, M. F. (2003). Solubilities of oxygen and carbon dioxide in butylmethylimidazolium tetrafluoroborate as a function of temperature and at pressures close to atmospheric pressure. J. Chem. Eng. Data, 48(3), 480–485. DOI: 10.1021/je0256277. Husson-BorgP. MajerV. Costa GomesM. F. 2003 Solubilities of oxygen and carbon dioxide in butylmethylimidazolium tetrafluoroborate as a function of temperature and at pressures close to atmospheric pressure J. Chem. Eng. Data 48 3 480 485 10.1021/je0256277 Open DOI Search in Google Scholar

26 Pérez-Salado Kamps, Á., Tuma, D., Xia, J., & Maurer, G. (2003). Solubility of CO₂ in the ionic liquid [bmim][PF₆]. J. Chem. Eng. Data, 48(3), 746–749. DOI: 10.1021/je034023f. Pérez-Salado KampsÁ. TumaD. XiaJ. MaurerG. 2003 Solubility of CO₂ in the ionic liquid [bmim][PF₆] J. Chem. Eng. Data 48 3 746 749 10.1021/je034023f Open DOI Search in Google Scholar

27 Evans, R. G., Klymenko, O. V., Saddoughi, S. A., Hardacre, C., & Compton, R. G. (2004). Electroreduction of oxygen in a series of room temperature ionic liquids composed of group 15-centered cations and anions. J. Phys. Chem. B, 108(23), 7878–7886. DOI: 10.1021/jp031309i. EvansR. G. KlymenkoO. V. SaddoughiS. A. HardacreC. ComptonR. G. 2004 Electroreduction of oxygen in a series of room temperature ionic liquids composed of group 15-centered cations and anions J. Phys. Chem. B 108 23 7878 7886 10.1021/jp031309i Open DOI Search in Google Scholar

28 Dyson, P. J., Laurenczy, G., Ohlin, C. A., Vallance, J., & Welton, T. (2003). Determination of hydrogen concentration in ionic liquids and the effect (or lack of) on rates of hydrogenation. Chem. Commun., 9(19), 2418–2419. DOI: 10.1039/B308309H. DysonP. J. LaurenczyG. OhlinC. A. VallanceJ. WeltonT. 2003 Determination of hydrogen concentration in ionic liquids and the effect (or lack of) on rates of hydrogenation Chem. Commun. 9 19 2418 2419 10.1039/B308309H Open DOI Search in Google Scholar

29 Neftel, A., Moor, E., Oeschger, H., & Stauffer, B. (1985). Evidence from polar ice cores for the increase in atmospheric CO₂ in the past two centuries. Nature, 315(6014), 45–47. DOI: 10.1038/315045a0. NeftelA. MoorE. OeschgerH. StaufferB. 1985 Evidence from polar ice cores for the increase in atmospheric CO₂ in the past two centuries Nature 315 6014 45 47 10.1038/315045a0 Open DOI Search in Google Scholar

30 Harvey, F. (2009, May). The Guardian. Retrieved November 23, 2020, from http://www.guardian.co.uk/environment/2011/may/29/carbon-emissions-nuclearpower. HarveyF. 2009 May The Guardian Retrieved November 23, 2020, from http://www.guardian.co.uk/environment/2011/may/29/carbon-emissions-nuclearpower. Search in Google Scholar

31 Peng, J., & Deng, Y. (2001). Cycloaddition of carbon dioxide to propylene oxide catalyzed by ionic liquids. New J. Chem., 25(4), 639–641. DOI: 10.1039/B008923K. PengJ. DengY. 2001 Cycloaddition of carbon dioxide to propylene oxide catalyzed by ionic liquids New J. Chem. 25 4 639 641 10.1039/B008923K Open DOI Search in Google Scholar

32 Yang, H., Gu, Y., Deng, Y., & Shi, F. (2002). Electrochemical activation of carbon dioxide in ionic liquids: synthesis of cyclic carbonates at mild reaction conditions. Chem. Commun., 33(3), 274–275. DOI: 10.1039/B108451H. YangH. GuY. DengY. ShiF. 2002 Electrochemical activation of carbon dioxide in ionic liquids: synthesis of cyclic carbonates at mild reaction conditions Chem. Commun. 33 3 274 275 10.1039/B108451H Open DOI Search in Google Scholar

33 Harmon, C. D., Smith, W. H., & Costa, D. A. (2001). Criticality calculations for plutonium metal at room temperature in ionic liquid solutions. Radiat. Phys. Chem., 60(3), 157–159. DOI: 10.1016/S0969-806X(00)00336-4. HarmonC. D. SmithW. H. CostaD. A. 2001 Criticality calculations for plutonium metal at room temperature in ionic liquid solutions Radiat. Phys. Chem. 60 3 157 159 10.1016/S0969-806X(00)00336-4 Open DOI Search in Google Scholar

34 Behar, D., Gonzales, C., & Neta, P. (2001). Reaction kinetics in ionic liquids: Pulse radiolysis studies of 1-butyl-3-methylimidazolium salts. J. Phys. Chem. A, 105(32), 7607–7614. DOI: 10.1021/jp011405o. BeharD. GonzalesC. NetaP. 2001 Reaction kinetics in ionic liquids: Pulse radiolysis studies of 1-butyl-3-methylimidazolium salts J. Phys. Chem. A 105 32 7607 7614 10.1021/jp011405o Open DOI Search in Google Scholar

35 Marcinek, A., Zielonka, J., Gębicki, J., Gordon, C. M., & Dunkin, I. R. (2001). Ionic liquids: Novel media for characterization of radical ions. J. Phys. Chem. A, 105(40), 9305–9309. DOI: 10.1021/jp0117718. MarcinekA. ZielonkaJ. GębickiJ. GordonC. M. DunkinI. R. 2001 Ionic liquids: Novel media for characterization of radical ions J. Phys. Chem. A 105 40 9305 9309 10.1021/jp0117718 Open DOI Search in Google Scholar

36 Behar, D., Neta, P., & Schultheisz, C. (2002). Reaction kinetics in ionic liquids as studied by pulse radiolysis: Redox reactions in the solvents methyltributylammonium bis(trifluoromethylsulphonyl)imide and n-butylpyridinium tetrafluoroborate. J. Phys. Chem. A, 106(13), 3139–3147. DOI: 10.1021/jp013808u. BeharD. NetaP. SchultheiszC. 2002 Reaction kinetics in ionic liquids as studied by pulse radiolysis: Redox reactions in the solvents methyltributylammonium bis(trifluoromethylsulphonyl)imide and n-butylpyridinium tetrafluoroborate J. Phys. Chem. A 106 13 3139 3147 10.1021/jp013808u Open DOI Search in Google Scholar

37 Grodkowski, J., & Neta. P. (2002). Reaction kinetics in the ionic liquid methyltributylammonium bis(trifluoromethylsulfonyl)imide. Pulse radiolysis study of ^·CF₃ radical reactions. J. Phys. Chem. A, 106(22), 5468–5473. DOI: 10.1021/jp020165p. GrodkowskiJ. NetaP. 2002 Reaction kinetics in the ionic liquid methyltributylammonium bis(trifluoromethylsulfonyl)imide. Pulse radiolysis study of ^·CF₃ radical reactions J. Phys. Chem. A 106 22 5468 5473 10.1021/jp020165p Open DOI Search in Google Scholar

38 Grodkowski, J., & Neta, P. (2002). Reaction kinetics in the ionic liquid methyltributylammonium bis(trifluoromethylsulfonyl)imide. Pulse radiolysis study of 4-mercaptobenzoic acid. J. Phys. Chem. A, 106(39), 9030–9035. DOI: 10.1021/jp020806g. GrodkowskiJ. NetaP. 2002 Reaction kinetics in the ionic liquid methyltributylammonium bis(trifluoromethylsulfonyl)imide. Pulse radiolysis study of 4-mercaptobenzoic acid J. Phys. Chem. A 106 39 9030 9035 10.1021/jp020806g Open DOI Search in Google Scholar

39 Grodkowski, J., & Neta, P. (2002). Formation and reaction of Br₂^·− radicals in the ionic liquid methyltributylammonium bis(trifluoromethylsulfonyl)imide and in other solvents. J. Phys. Chem. A, 106(46), 11130–11134. DOI: 10.1021/jp021498p. GrodkowskiJ. NetaP. 2002 Formation and reaction of Br₂^·− radicals in the ionic liquid methyltributylammonium bis(trifluoromethylsulfonyl)imide and in other solvents J. Phys. Chem. A 106 46 11130 11134 10.1021/jp021498p Open DOI Search in Google Scholar

40 Grodkowski, J., Neta, P., & Wishart, J. F. (2003). Pulse radiolysis study of the reactions of hydrogen atoms in the ionic liquid methyltributylammonium bis[(trifluoromethyl)sulfonyl]imide. J. Phys. Chem. A, 107(46), 9794–9799. DOI: 10.1021/jp035265p. GrodkowskiJ. NetaP. WishartJ. F. 2003 Pulse radiolysis study of the reactions of hydrogen atoms in the ionic liquid methyltributylammonium bis[(trifluoromethyl)sulfonyl]imide J. Phys. Chem. A 107 46 9794 9799 10.1021/jp035265p Open DOI Search in Google Scholar

41 Wishart, J. F., & Neta, P. (2003). Spectrum and reactivity of the solvated electron in the ionic liquid methyltributylammonium bis(trifluoromethylsulfonyl) imide. J. Phys. Chem. B, 107(30), 7261–7267. DOI: 10.1021/jp027792z. WishartJ. F. NetaP. 2003 Spectrum and reactivity of the solvated electron in the ionic liquid methyltributylammonium bis(trifluoromethylsulfonyl) imide J. Phys. Chem. B 107 30 7261 7267 10.1021/jp027792z Open DOI Search in Google Scholar

42 Skrzypczak, A., & Neta, P. (2003). Diffusion-controlled electron-transfer reactions in ionic liquids. J. Phys. Chem. A, 107(39), 7800–7803. DOI: 10.1021/jp030416+. SkrzypczakA. NetaP. 2003 Diffusion-controlled electron-transfer reactions in ionic liquids J. Phys. Chem. A 107 39 7800 7803 10.1021/jp030416+ Open DOI Search in Google Scholar

43 Skrzypczak, A., & Neta, P. (2004). Rate constants for reaction of 1,2-dimethylimidazole with benzyl bromide in ionic liquids and organic solvents. Int. J. Chem. Kinet., 36(4), 253–258. DOI: 10.1002/kin.10162. SkrzypczakA. NetaP. 2004 Rate constants for reaction of 1,2-dimethylimidazole with benzyl bromide in ionic liquids and organic solvents Int. J. Chem. Kinet. 36 4 253 258 10.1002/kin.10162 Open DOI Search in Google Scholar

44 Grodkowski, J., Nyga, M., & Mirkowski, J. (2005). Formation of Br₂^·−, BrSCN^·− and (SCN)₂^·− intermediates in the ionic liquid methyltributylammonium bis[(trifluoromethyl)sulfonyl]imide. Pulse radiolysis study. Nukleonika, 50(Suppl. 2), S35–S38. GrodkowskiJ. NygaM. MirkowskiJ. 2005 Formation of Br₂^·−, BrSCN^·− and (SCN)₂^·− intermediates in the ionic liquid methyltributylammonium bis[(trifluoromethyl)sulfonyl]imide. Pulse radiolysis study Nukleonika 50 Suppl. 2 S35 S38 Search in Google Scholar

45 Wishart, J. F., Lall-Ramnarine, S. I., Rajub, R., Scumpia, A., Bellevue, S., Ragbir, R., & Engel, R. (2005). Effects of functional group substitution on electron spectra and solvation dynamics in a family of ionic liquids. Radiat. Phys. Chem., 72(2/3), 99–104. DOI: 10.1016/j.radphyschem.2004.09.005. WishartJ. F. Lall-RamnarineS. I. RajubR. ScumpiaA. BellevueS. RagbirR. EngelR. 2005 Effects of functional group substitution on electron spectra and solvation dynamics in a family of ionic liquids Radiat. Phys. Chem. 72 2/3 99 104 10.1016/j.radphyschem.2004.09.005 Open DOI Search in Google Scholar

46 Yang, J., Kondoh, T., Norizawa, K., Nagaishi, R., Taguchi, M., Takahashi, K., Katoh, R., Anishchik, S. V. R., Yoshida, Y., & Tagawa, S. (2008). Picosecond pulse radiolysis: dynamics of solvated electrons in ionic liquid and geminate ion recombination in liquid alkanes. Radiat. Phys. Chem., 77(10/12), 1233–1238. DOI: 10.1016/j.radphyschem.2008.05.031. YangJ. KondohT. NorizawaK. NagaishiR. TaguchiM. TakahashiK. KatohR. AnishchikS. V. R. YoshidaY. TagawaS. 2008 Picosecond pulse radiolysis: dynamics of solvated electrons in ionic liquid and geminate ion recombination in liquid alkanes Radiat. Phys. Chem. 77 10/12 1233 1238 10.1016/j.radphyschem.2008.05.031 Open DOI Search in Google Scholar

47 Takahashi, K., Sato, T., Katsumura, Y., Yang, J., Kondoh, T., Yoshida, Y., & Katoh, R. (2008). Reactions of solvated electrons with imidazolium cations in ionic liquids. Radiat. Phys. Chem., 77(10/12), 1239–1243. DOI: 10.1016/j.radphyschem.2008.05.042. TakahashiK. SatoT. KatsumuraY. YangJ. KondohT. YoshidaY. KatohR. 2008 Reactions of solvated electrons with imidazolium cations in ionic liquids Radiat. Phys. Chem. 77 10/12 1239 1243 10.1016/j.radphyschem.2008.05.042 Open DOI Search in Google Scholar

48 Asano, A., Yang, J., Kondoh, T., Norizawa, K., Nagaishi, R., Takahashi, K., & Yoshida, Y. (2008). Molar absorption coefficient and radiolytic yield of solvated electrons in diethylmethyl(2-methoxy)ammonium bis(trifluoromethanesulfonyl)imide ionic liquid. Radiat. Phys. Chem., 77(10/12), 1244–1247. DOI: 10.1016/j.radphyschem.2008.05.032. AsanoA. YangJ. KondohT. NorizawaK. NagaishiR. TakahashiK. YoshidaY. 2008 Molar absorption coefficient and radiolytic yield of solvated electrons in diethylmethyl(2-methoxy)ammonium bis(trifluoromethanesulfonyl)imide ionic liquid Radiat. Phys. Chem. 77 10/12 1244 1247 10.1016/j.radphyschem.2008.05.032 Open DOI Search in Google Scholar

49 Kimura, A., Taguchi, M., Kondoh, T., Yang, J., Yoshida, Y., & Hirota, K. (2008). Study on the reaction of chlorophenols in room temperature ionic liquids with ionizing radiation. Radiat. Phys. Chem., 77(10/12), 1253–1257. DOI: 10.1016/j.radphyschem.2008.05.020. KimuraA. TaguchiM. KondohT. YangJ. YoshidaY. HirotaK. 2008 Study on the reaction of chlorophenols in room temperature ionic liquids with ionizing radiation Radiat. Phys. Chem. 77 10/12 1253 1257 10.1016/j.radphyschem.2008.05.020 Open DOI Search in Google Scholar

50 Wishart, F., Funston, A. M., & Szreder, T. (2006). Radiation chemistry of ionic liquids. In Molten Salts XIV – Proceedings of the International Symposium, 206th ECS Meeting, 3–8 October 2004 (pp. 802–813). Pennington, New Jersey, USA: The Electrochemical Society. WishartF. FunstonA. M. SzrederT. 2006 Radiation chemistry of ionic liquids In Molten Salts XIV – Proceedings of the International Symposium, 206th ECS Meeting 3–8 October 2004 802 813 Pennington, New Jersey, USA The Electrochemical Society 10.1149/200424.0802PV Search in Google Scholar

51 Allen, D., Baston, G., Bradley, A. E., Gorman, T., Haile, A., Hamblett, I., Hatter, J. E., Healey, M. J. F., Hodgson, B., Lewin, R., Lovell, K. V., Newton, B., Pitner, W. R., Rooney, D. W., Sanders, D., Seddon, K. R., Sims, H. E., & Thied, R. C. (2002). An investigation of the radiochemical stability of ionic liquids. Green Chem., 4(2), 152–158. DOI: 10.1039/b111042j. AllenD. BastonG. BradleyA. E. GormanT. HaileA. HamblettI. HatterJ. E. HealeyM. J. F. HodgsonB. LewinR. LovellK. V. NewtonB. PitnerW. R. RooneyD. W. SandersD. SeddonK. R. SimsH. E. ThiedR. C. 2002 An investigation of the radiochemical stability of ionic liquids Green Chem. 4 2 152 158 10.1039/b111042j Open DOI Search in Google Scholar

52 Shkrob, I. A., Chemerisov, S. D., & Wishart, J. F. (2007). The initial stages of radiation damage in ionic liquids and ionic liquid-based extraction systems. J. Phys. Chem. B, 111(40), 11786–1793. DOI: 10.1021/jp073619x. ShkrobI. A. ChemerisovS. D. WishartJ. F. 2007 The initial stages of radiation damage in ionic liquids and ionic liquid-based extraction systems J. Phys. Chem. B 111 40 11786 1793 10.1021/jp073619x 17877387 Open DOI Search in Google Scholar

53 Qi, M., Wu, G., Li, Q., & Lu, Y. (2008). γ-Radiation effect on ionic liquid [bmim][BF₄]. Radiat. Phys. Chem., 77(7), 877–883. DOI: 10.1016/j.radphyschem.2007.12.007. QiM. WuG. LiQ. LuY. 2008 γ-Radiation effect on ionic liquid [bmim][BF₄] Radiat. Phys. Chem. 77 7 877 883 10.1016/j.radphyschem.2007.12.007 Open DOI Search in Google Scholar

54 Grodkowski, J., Kocia, R., & Mirkowski, J. (2009). Formations of p-terphenyl excited states in the ionic liquid methyltributylammonium bis[(trifluoromethyl) sulfonyl]imide. Pulse radiolysis study. Res. Chem. Intermed., 35, 411–419. DOI: 10.1007/s11164-009-0056-2. GrodkowskiJ. KociaR. MirkowskiJ. 2009 Formations of p-terphenyl excited states in the ionic liquid methyltributylammonium bis[(trifluoromethyl) sulfonyl]imide. Pulse radiolysis study Res. Chem. Intermed. 35 411 419 10.1007/s11164-009-0056-2 Open DOI Search in Google Scholar

55 Kocia, R., Grodkowski, J., & Mirkowski, J. (2015). Pulse radiolysis studies of p-terphenyl in the ionic liquid methyltributylammonium bis[(trifluoromethyl)sulfonyl]imide, [MeBu₃N][NTf₂]. Res. Chem. Intermed., 41, 5079–5093. DOI: 10.1007/s11164-014-1590-0. KociaR. GrodkowskiJ. MirkowskiJ. 2015 Pulse radiolysis studies of p-terphenyl in the ionic liquid methyltributylammonium bis[(trifluoromethyl)sulfonyl]imide, [MeBu₃N][NTf₂] Res. Chem. Intermed. 41 5079 5093 10.1007/s11164-014-1590-0 Open DOI Search in Google Scholar

56 Kocia, R. (2019). Pulse radiolysis studies of intermediates derived from p-terphenyl in the oxygenated methyltributylammonium bis[(trifluoromethyl)sulfonyl]imide ionic liquid. Int. J. Chem. Kinet., 51(12), 958–964. DOI: 10.1002/kin.21323. KociaR. 2019 Pulse radiolysis studies of intermediates derived from p-terphenyl in the oxygenated methyltributylammonium bis[(trifluoromethyl)sulfonyl]imide ionic liquid Int. J. Chem. Kinet. 51 12 958 964 10.1002/kin.21323 Open DOI Search in Google Scholar

57 Carmichael, I., & Hug, G. (1986). Triplet-triplet absorption spectra of organic molecules in condensed phases. J. Phys. Chem. Ref. Data, 15, 1–250. DOI: 10.1063/1.555770. CarmichaelI. HugG. 1986 Triplet-triplet absorption spectra of organic molecules in condensed phases J. Phys. Chem. Ref. Data 15 1 250 10.1063/1.555770 Open DOI Search in Google Scholar

58 Shida, T. (1988). Electronic absorption spectra of radical ions. Amsterdam: Elsevier. ShidaT. 1988 Electronic absorption spectra of radical ions Amsterdam Elsevier Search in Google Scholar

59 Liu, A., Loffredo, D. M., & Trifunac, A. D. (1993). Photoionization and ensuing ion-molecule reactions of polycyclic aromatic hydrocarbons in alkane and alcohol solutions. J. Phys. Chem., 97(15), 3791–3799. DOI: 10.1021/j100117a027. LiuA. LoffredoD. M. TrifunacA. D. 1993 Photoionization and ensuing ion-molecule reactions of polycyclic aromatic hydrocarbons in alkane and alcohol solutions J. Phys. Chem. 97 15 3791 3799 10.1021/j100117a027 Open DOI Search in Google Scholar

60 Fujiwara, H., Kitamura, T., Wada, Y., Yanagida, S., & Kamat, P. V. (1999). Onium salt effects on p-terphenyl-sensitized photoreduction of water to hydrogen. J. Phys. Chem. A, 103(25), 4874–4878. DOI: 10.1021/jp984740u. FujiwaraH. KitamuraT. WadaY. YanagidaS. KamatP. V. 1999 Onium salt effects on p-terphenyl-sensitized photoreduction of water to hydrogen J. Phys. Chem. A 103 25 4874 4878 10.1021/jp984740u Open DOI Search in Google Scholar

61 Matsuoka, S., Kohzuki, T., Pac, C., Ishida, A., Takamuku, S., Kusaba, M., Nobuaki, N., & Yanagida, S. (1992). Photocatalysis of oligo(p-phenylenes). Photochemical reduction of carbon dioxide with triethylamine. J. Phys. Chem., 96(11), 4437–4445. DOI: 10.1021/j100190a057. MatsuokaS. KohzukiT. PacC. IshidaA. TakamukuS. KusabaM. NobuakiN. YanagidaS. 1992 Photocatalysis of oligo(p-phenylenes). Photochemical reduction of carbon dioxide with triethylamine J. Phys. Chem. 96 11 4437 4445 10.1021/j100190a057 Open DOI Search in Google Scholar

62 Schuler, R. H., Patterson, L. K., & Janata, E. (1980). Yield for the scavenging of hydroxyl radicals in the radiolysis of nitrous oxide-saturated aqueous solutions. J. Phys. Chem., 84(16), 2088–2089. DOI: 10.1021/j100453a020. SchulerR. H. PattersonL. K. JanataE. 1980 Yield for the scavenging of hydroxyl radicals in the radiolysis of nitrous oxide-saturated aqueous solutions J. Phys. Chem. 84 16 2088 2089 10.1021/j100453a020 Open DOI Search in Google Scholar

63 Buxton, G. V., Greenstock, C. L., Helman, W. P., & Ross, A. B. (1988). Critical review of rate constants for reactions of hydrated electrons, hydrogen atoms and hydroxyl radicals (^•OH/^•O⁻ in aqueous solution. J. Phys. Chem. Ref. Data, 17, 513–886. DOI: 10.1063/1.555805. BuxtonG. V. GreenstockC. L. HelmanW. P. RossA. B. 1988 Critical review of rate constants for reactions of hydrated electrons, hydrogen atoms and hydroxyl radicals (^•OH/^•O⁻ in aqueous solution J. Phys. Chem. Ref. Data 17 513 886 10.1063/1.555805 Open DOI Search in Google Scholar

64 Gordon, S., Hart, E. J., Matheson, M. S., Rabani, J., & Thomas, J. K. (1963). Reactions of the hydrated electron. Discuss. Faraday Soc., 36, 193–205. DOI: 10.1039/DF9633600193. GordonS. HartE. J. MathesonM. S. RabaniJ. ThomasJ. K. 1963 Reactions of the hydrated electron Discuss. Faraday Soc. 36 193 205 10.1039/DF9633600193 Open DOI Search in Google Scholar

65 Sullivan, B. P., Krist, K., & Guard, H. E. (1993). Electrochemical and electrocatalytic reactions of carbon dioxide. Amsterdam, NL: Elsevier Science Publishers B.V. SullivanB. P. KristK. GuardH. E. 1993 Electrochemical and electrocatalytic reactions of carbon dioxide Amsterdam, NL Elsevier Science Publishers B.V. Search in Google Scholar

66 Lamy, E., Nadjo, L., & Saveant, J. M. (1977). Standard potential and kinetic parameters of the electrochemical reduciton of carbon dioxide in dimethyformamide. J. Electroanal. Chem., 78(2), 403–407. DOI: 10.1016/S0022-0728(77)80143-5. LamyE. NadjoL. SaveantJ. M. 1977 Standard potential and kinetic parameters of the electrochemical reduciton of carbon dioxide in dimethyformamide J. Electroanal. Chem. 78 2 403 407 10.1016/S0022-0728(77)80143-5 Open DOI Search in Google Scholar

67 Dhanasekaran, T., Grodkowski, J., Neta, P., Hambright, P., & Fujita, E. (1999). p-Terphenyl-sensitized photoreduction of CO₂ with cobalt and iron porphyrins. Interaction between CO and reduced metalloporphyrins. J. Phys. Chem. A, 103(38), 7742–7748. DOI: 10.1021/jp991423u. DhanasekaranT. GrodkowskiJ. NetaP. HambrightP. FujitaE. 1999 p-Terphenyl-sensitized photoreduction of CO₂ with cobalt and iron porphyrins. Interaction between CO and reduced metalloporphyrins J. Phys. Chem. A 103 38 7742 7748 10.1021/jp991423u Open DOI Search in Google Scholar

68 Grodkowski, J., Dhanasekaran, T., Neta, P., Hambright, P., Brunschwig, B. S., Shinozaki, K., & Fujita, E. (2000). Reduction of cobalt and iron phthalocyanines and the role of the reduced species in catalyzed photoreduction of CO₂. J. Phys. Chem. A, 104(48), 11332–11339. DOI: 10.1021/jp002709y. GrodkowskiJ. DhanasekaranT. NetaP. HambrightP. BrunschwigB. S. ShinozakiK. FujitaE. 2000 Reduction of cobalt and iron phthalocyanines and the role of the reduced species in catalyzed photoreduction of CO₂ J. Phys. Chem. A 104 48 11332 11339 10.1021/jp002709y Open DOI Search in Google Scholar

69 Grodkowski, J. (2004). Radiolytic and photochemical reduction of carbon dioxide in solution catalyzed by transition metal complexes with some selected macrocycles. Warszawa: Institute of Nuclear Chemistry and Technology. (Raporty IChTJ. Seria A nr 1/2004). GrodkowskiJ. 2004 Radiolytic and photochemical reduction of carbon dioxide in solution catalyzed by transition metal complexes with some selected macrocycles Warszawa Institute of Nuclear Chemistry and Technology (Raporty IChTJ. Seria A nr 1/2004). Search in Google Scholar

70 Grodkowski, J., & Neta, P. (2000). Cobalt corrin catalyzed photoreduction of CO₂. J. Phys. Chem. A, 104(9), 1848–1853. DOI: 10.1021/jp9939569. GrodkowskiJ. NetaP. 2000 Cobalt corrin catalyzed photoreduction of CO₂ J. Phys. Chem. A 104 9 1848 1853 10.1021/jp9939569 Open DOI Search in Google Scholar

71 Grodkowski, J., Neta, P., Fujita, E., Mahammed, A., Simkhovich, L., & Gross, Z. (2002). Reduction of cobalt and iron corroles and catalyzed reduction of CO₂. J. Phys. Chem. A, 106(18), 4772–4778. DOI: 10.1021/jp013668o. GrodkowskiJ. NetaP. FujitaE. MahammedA. SimkhovichL. GrossZ. 2002 Reduction of cobalt and iron corroles and catalyzed reduction of CO₂ J. Phys. Chem. A 106 18 4772 4778 10.1021/jp013668o Open DOI Search in Google Scholar

72 Grodkowski, J., & Neta, P. (2000). Ferrous ions as catalysts for photochemical reduction of CO₂ in homogeneous solutions. J. Phys. Chem. A, 104(19), 4475–4479. DOI: 10.1021/jp993456f. GrodkowskiJ. NetaP. 2000 Ferrous ions as catalysts for photochemical reduction of CO₂ in homogeneous solutions J. Phys. Chem. A 104 19 4475 4479 10.1021/jp993456f Open DOI Search in Google Scholar

Nukleonika

Intermediates derived from p-terphenyl in the methyltributylammonium bis[(trifluoromethyl)sulfonyl]imide ionic liquid saturated with carbon dioxide: Pulse radiolysis study

Rafał Kocia
Rafał Kocia

Published Online: 20 Jan 2023

Volume & Issue: Volume 67 (2022) - Issue 4 (December 2022)

Page range: 73 - 80

Received: 26 Oct 2022

Accepted: 02 Dec 2022

Journal & Issue Details

Nukleonika

PDF Preview

Article

Fig. 1

Fig. 2

Fig. 3

Fig. 4

Figures & Tables

Fig. 1

Fig. 2

Fig. 3

Fig. 4

References

Recent Articles

Nukleonika

Intermediates derived from p-terphenyl in the methyltributylammonium bis[(trifluoromethyl)sulfonyl]imide ionic liquid saturated with carbon dioxide: Pulse radiolysis study

Rafał KociaRafał Kocia

Published Online: 20 Jan 2023

Volume & Issue: Volume 67 (2022) - Issue 4 (December 2022)

Page range: 73 - 80

Received: 26 Oct 2022

Accepted: 02 Dec 2022

Journal & Issue Details

Nukleonika

PDF Preview

Article

Fig. 1

Fig. 2

Fig. 3

Fig. 4

Figures & Tables

Fig. 1

Fig. 2

Fig. 3

Fig. 4

References

Recent Articles

Rafał Kocia
Rafał Kocia