Detection of the Gasoline Components Methyltert-Butyl Ether, Benzene, Toluene, andm-Xylene Using Ion Mobility Spectrometers with a Radioactive and UV Ionization Source

2003 ◽  
Vol 75 (6) ◽  
pp. 1483-1490 ◽  
Author(s):  
Jörg Ingo Baumbach ◽  
Stefanie Sielemann ◽  
Zhiyong Xie ◽  
Hartwig Schmidt
Keyword(s):  
Ion Mobility ◽  
Butyl Ether ◽  
Ionization Source ◽  
Benzene Toluene

Effect of Work Parameters for Surface Ionization Source on Ion Mobility Spectrum

2012 ◽  
Vol 39 (10) ◽  
pp. 1491-1495
Author(s):  
De-Xin ZHANG ◽  
Xiao-Guang GAO ◽  
Jian JIA ◽  
Xiu-Li HE ◽  
Jian-Ping LI
Keyword(s):  
Ion Mobility ◽  
Surface Ionization ◽  
Ionization Source ◽  
Mobility Spectrum

scholarly journals Fast Sensing of Hydrogen Cyanide (HCN) Vapors Using a Hand-Held Ion Mobility Spectrometer with Nonradioactive Ionization Source

Sensors ◽  
2021 ◽  
Vol 21 (15) ◽  
pp. 5045
Author(s):  
Victor Bocos-Bintintan ◽  
Ileana Andreea Ratiu
Keyword(s):  
Ion Mobility ◽  
Hydrogen Cyanide ◽  
Limit Of Detection ◽  
Chemical Warfare Agent ◽  
Source Model ◽  
Negative Ion ◽  
Industrial Chemicals ◽  
Ionization Source ◽  
Toxic Industrial Chemicals ◽  
Negative Ion Mode

Sensitive real-time detection of vapors produced by toxic industrial chemicals (TICs) always represents a stringent priority. Hydrogen cyanide (HCN) is definitely a TIC, being widely used in various industries and as an insecticide; it is a reactive, very flammable, and highly toxic compound that affects the central nervous system, cardiovascular system, eyes, nose, throat, and also has systemic effects. Moreover, HCN is considered a blood chemical warfare agent. This study was focused toward quick detection and quantification of HCN in air using time-of-flight ion mobility spectrometry (ToF IMS). Results obtained clearly indicate that IMS can rapidly detect HCN at sub-ppmv levels in air. Ion mobility spectrometric response was obtained in the negative ion mode and presented one single distinct product ion, at reduced ion mobility K0 of 2.38 cm2 V−1 s−1. Our study demonstrated that by using a miniaturized commercial IMS system with nonradioactive ionization source model LCD-3.2E (Smiths Detection Ltd., London, UK), one can easily measure HCN at concentrations of 0.1 ppmv (0.11 mg m−3) in negative ion mode, which is far below the OSHA PEL-TWA value of 10 ppmv. Measurement range was from 0.1 to 10 ppmv and the estimated limit of detection LoD was ca. 20 ppbv (0.02 mg m−3).

Stepwise optimization of a Flexible Microtube Plasma (FµTP) as an ionization source for Ion Mobility Spectrometry

2020 ◽  
Vol 1127 ◽  
pp. 89-97 ◽  
Author(s):  
Carolin Drees ◽  
Alexander Schütz ◽  
Guanghui Niu ◽  
Joachim Franzke ◽  
Wolfgang Vautz ◽  
...  
Keyword(s):  
Ion Mobility Spectrometry ◽  
Ion Mobility ◽  
Ionization Source

Enthalpies of interaction of nitrogen base solutes with organic solvents

1985 ◽  
Vol 63 (9) ◽  
pp. 2540-2544 ◽  
Author(s):  
W. Kirk Stephenson ◽  
Richard Fuchs
Keyword(s):  
Hydrogen Bond ◽  
Organic Solvents ◽  
Butyl Alcohol ◽  
Hydrogen Bond Donor ◽  
Butyl Ether ◽  
Hydrogen Bond Acceptor ◽  
Nitrogen Base ◽  
Benzene Toluene ◽  
Polar Interactions ◽  
S Model

Heats of solution of triethylamine, aniline, pyridine, and model compounds (3-ethylpentane, benzene) in 17 organic solvents (n-heptane, cyclohexane, carbon tetrachloride, 1,2-dichloroethane, α,α,α-trifluorotoluene, triethylamine, butyl ether, ethyl acetate, dimethylformamide, dimethyl sulfoxide, benzene, toluene, mesitylene, t-butyl alcohol, 1-octanol, methanol, 2,2,2-trifluoroethanol) have been combined with solute heats of vaporization to give enthalpies of transfer from vapor to solvent (ΔH(v → s)). Differences between solute and model values (ΔΔH(v → s) = ΔH(v → s) (solute) – ΔH(v → s) (model)) were used to evaluate nitrogen base solute–solvent polar interactions. Correlations of ΔΔH(v → s) with Taft–Kamlet solvatochromic parameters (π*, α, β) have been determined.Aniline was found to be a better hydrogen bond donor acid than hydrogen bond acceptor base. Nevertheless, alcohols donate H-bonds to aniline. Triethylamine and pyridine are stronger HBA bases than aniline. The π* (dipolarity–polarizability) parameter of aniline (as a solute) is calculated to be 1.10.

Ion Mobility Spectrometry for Monitoring Chemical Warfare Agents

2012 ◽  
Vol 241-244 ◽  
pp. 980-983 ◽  
Author(s):  
Jian Zheng ◽  
Tian Min Shu ◽  
Jie Jin
Keyword(s):  
Ion Mobility Spectrometry ◽  
Ion Mobility ◽  
Cluster Formation ◽  
Chemical Warfare Agents ◽  
Chemical Warfare ◽  
Ambient Conditions ◽  
Ionization Source ◽  
Warfare Agents ◽  
Positive Mode ◽  
Detecting Method

The technique of ion mobility spectrometry (IMS) offers a practical and fast detecting method in ambient conditions to estimate whether there may presence contrabands or even chemical warfare agents (CWAs). In this work we have investigated a self-made radioactive 63Ni (β emission) ionization source for ion mobility spectrometry employed with an atmospheric pressure to detect real CWAs, such as GB, GD, HD, VX from aerosol samples. Furthermore, we have experimentally studied the influence of drift tube temperature not only in ion cluster formation in the positive mode, but also the detection limitation of CWAs.

Enthalpies of hydrogen bond formation of 1-octanol with aprotic organic solvents. A comparison of the solvation enthalpy, pure base, and non-hydrogen-bonding baseline methods

1985 ◽  
Vol 63 (2) ◽  
pp. 342-348 ◽  
Author(s):  
W. Kirk Stephenson ◽  
Richard Fuchs
Keyword(s):  
Hydrogen Bond ◽  
Hydrogen Bonding ◽  
Bond Formation ◽  
Enthalpies Of Solution ◽  
Dispersion Interactions ◽  
Butyl Ether ◽  
Hydrogen Bond Formation ◽  
Solvation Enthalpy ◽  
Benzene Toluene ◽  
Good Agreement

Enthalpies of solution (ΔHs) of 1-octanol and five model compounds (di-n-butyl ether, n-heptyl methyl ether, 1-fluoro-octane, 1-chlorooctane, and n-octane) have been determined in 13 solvents (heptane, cyclohexane, CCl4, 1,1,1-trichloro-ethane, 1,2-dichloroethane, triethylamine, butyl ether, ethyl acetate, DMF, DMSO, benzene, toluene, mesitylene), and combined with heats of vaporization to give enthalpies of transfer from vapor to solvent (ΔH(v → S)). These values have been used to calculate the enthalpy of hydrogen bond formation (ΔHh) of 1-octanol with each solvent, using the pure base (PB), solvation enthalpy (SE), and non-hydrogen-bonding baseline (NHBB) methods. Evidence is presented suggesting that (a) the SE method is susceptible to mismatches of the 1-octanol vs. model polar and dispersion interactions, (b) the PB method is sensitive to polar interaction mismatches, whereas (c) the NHBB method compensates for both polar and dispersion interactions mismatches. The (apparent) ΔHh values determined by the SE and PB methods may be as much as several kcal/mol (nearly 50%) too large, because of the inclusion of other polar and dispersion interactions. The NHBB method is therefore preferred for determining enthalpies of H-bond formation from calorimetric data. However, apparent ΔHh values from the SE and PB methods can be incorporated into total solvatochromic equations using Taft–Kamiet π*, β, and ξ parameters, to provide enthalpies of H-bond formation in good agreement with ΔHh (NHBB).

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