Reactions of Gaseous Molecule Ions with Gaseous Molecules. II

Schissler, D. O.; Stevenson, D. P.

doi:10.1063/1.1742664

Cited by 109 publications

(24 citation statements)

References 3 publications

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“…In that case, the leading term in the interaction potential scales as r −2 rather than r −4 [11]. Furthermore, several experiments [12][13][14] have shown a departure from the inverse velocity dependence of the classical cross-section in some reactions. Ultimately, the probability of a reaction occurring in the event of a classical interaction is dependent on the combined energy state of the reactants, the available energy states in the final products, and the possible reaction pathways between them [15].…”

Section: +mentioning

confidence: 99%

Charge exchange and chemical reactions with trappedTh3+

2011

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We have measured the reaction rates of trapped, buffer gas cooled Th 3+ and various gases and have analyzed the reaction products using trapped ion mass spectrometry techniques. Ion trap lifetimes are usually limited by reactions with background molecules, and the high electron affinity of multiply charged ions such as Th 3+ make them more prone to loss. Our results show that reactions of Th 3+ with carbon dioxide, methane, and oxygen all occur near the classical Langevin rate, while reaction rates with argon, hydrogen, and nitrogen are orders of magnitude lower. Reactions of Th 3+ with oxygen and methane proceed primarily via charge exchange, while simultaneous charge exchange and chemical reaction occurs between Th 3+ and carbon dioxide. Loss rates of Th 3+ in helium are consistent with reaction with impurities in the gas. Reaction rates of Th 3+ with nitrogen and argon depend on the internal electronic configuration of the Th 3+ .

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Section: +mentioning

confidence: 99%

Charge exchange and chemical reactions with trappedTh3+

2011

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“…The parent ions, HBrf and HC1+, should therefore be the predominate ionic species resulting from ionization in both compounds: [6] i n liquid HC1. occur with roughly equal rate constants (13), and in the liquid phase should be complete within about 10-l3 seconds of formation of the parent ions. Because conventional electrochemical studies (14) have shown that pure liquid HCl undergoes autoprotolysis, it has been inferred ( I ) that neutralization of the H&1+ and Cl-H --C1-ions formed in it by radiation will proceed via the reverse of the autoprotolysis reaction:…”

Section: Resultsmentioning

confidence: 99%

THE RADIOLYSIS OF HCl–HBr MIXTURES

Rumfeldt¹

1963

Can. J. Chem.

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Bromine was the only halogen formed in irradiated mixtures of HC1 and HBr. A study of its effect on the hydrogen yield from HC1 showed that it reacted with the first hydrogenforming species (or its precursor), and indicated the same yield for this species as did the earlier experiments with chlorine. The results were consistent with thermal hydrogen atoms, formed in the reaction as the first hydrogen-forming species, and hot hydrogen atoms, resulting from the dissociation of excited HC1 molecules, as the second species.The hydrogen yield from liquid HBr a t -79' C was a factor of two larger than that from liquid HC1 a t the same temperature, and in mixtures of the two the hydrogen yield increased gradually from a value characteristic of pure HCl ( G H~ = 6.5) t o one characteristic of pure HBr ( G H~ = 12.4). The smaller yield from HC1 cannot be explained by radical combinations:in the radiation tracks and must be attributed either t o differences in the ion-combination reactions in the two liquids or to a genuinely greater yield of ions and/or dissociative excited molecules in HBr. The hydrogen yield from solid HBr a t -196' C was C;HZ = 10.5.X recent publication (1) from this laboratory described a study of the radiolysis of liquid and solid hydrogen chloride. This paper reports the results of a similar study of the radiolysis of hydrogen bromide, and also presents further evidence for the existence of two hydrogen-forming species in irradiated hydrogen chloride. Because the decomposition yield of hydrogen bromide was found to be twice that of hydrogen chloride, hydrogen and halogen yields in mixtures of the two were also studied in the hope that a reason for the difference in radiation sensitivity of the two compounds would become apparent. E X P E R I M E N T A L HaterialsHydrogen chloride and hydrogen bromide were obtained from the Matheson Co. and purified b y the preirradiation procedure already described. Reagent grade bromine was thoroughly dried by treatment with CaC12 and subjected to several bulb-to-bulb distillations. I t was stored over PsOs a t -80" C. ApparatztsThe apparatus and technique used for the preparation of samples and measurement of hydrogen yields were essentially as previously described. In this study a spectroscopic technique was also employed t o observe the halogen production in the irradiated mixtures. Optical cells, which were shielded from the direct Co" beam during irradiations, were attached t o the pyrex irradiation cells. On completion of an irradiation the hydrogen halide -halogen solution was transferred to the optical cell, where its spectrum over the range 3000-5000 A was taken with a Beckman D.U. spectrometer fitted with a cell compartment for use a t -80" C. This consisted of a n aluminum block machined t o receive the optical cell and to permit passage of the light beam. The block was insulated with styrofoain on all sides and attachcd t o two plates, which were bolted to the monochromator and photocell of the D.U. spectrometer. Quartz plates isolated the cell...

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“…Figure 1 shows the ion current for C4H8+ as a function of 1 4 2 and 1 4 0 plotted in the manner of equations [2] and [3]. The zero slope of A (C4H 7+) was intermediate between the appearance potential of C3H 6+ and C3H5+ (or C3H4+), suggesting that both reactions [6] and [7] might be occurring.…”

Section: Ion-~lfolec~ile Reactionsmentioning

confidence: 99%

“…Equations [2] and [3] predict that for a secondary ion arising from two concurrent reactions a plot of I,/I,, against I p , / I p , should lead to a straight line with slope proportional to fZQ:, and intercept proportional to flQ1, while the similar plot of I,/Ip, against I,,/Ip, should be a straight line with slope and intercept proportional to flQl and fZQ2, respectively. \Arith a 1;nowledge of d and [MI the individual cross sections can be determined.…”

Section: Equation [I] May Be Rearranged To Give the Following Two Ecmentioning

confidence: 99%

Concurrent Ion–molecule Reactions Leading to the Same Production

Harrison¹,

Tait²

1962

Can. J. Chem.

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Seven of the major secondary ions in the high-pressure mass spectrunl of cyclopropane have been studied. A method has been developed for studying concurrent ion-molecule reactions and it has been shown that four of the secondary ions are the products of more than one reaction. Cross sections for the separate reactions are reported. The appearance potentials of the major primary ions in the mass spectrum of cyclopropane have been measured:

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Reactions of Gaseous Molecule Ions with Gaseous Molecules. II

Cited by 109 publications

References 3 publications

Charge exchange and chemical reactions with trappedTh3+

Charge exchange and chemical reactions with trappedTh3+

THE RADIOLYSIS OF HCl–HBr MIXTURES

Concurrent Ion–molecule Reactions Leading to the Same Production

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