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Related Concept Videos

Isotopes and Radioisotopes01:28

Isotopes and Radioisotopes

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In the early 1900s, English chemist Frederick Soddy realized that an element could have atoms with different masses that were chemically indistinguishable. These different types are called isotopes — atoms of the same element that differ in mass. Isotopes differ in mass because they have different numbers of neutrons but are chemically identical because they have the same number of protons. Soddy was awarded the Nobel Prize in Chemistry in 1921 for this discovery.
An isotope containing...
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Nuclear Stability03:18

Nuclear Stability

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Protons and neutrons, collectively called nucleons, are packed together tightly in a nucleus. With a radius of about 10−15 meters, a nucleus is quite small compared to the radius of the entire atom, which is about 10−10 meters. Nuclei are extremely dense compared to bulk matter, averaging 1.8 × 1014 grams per cubic centimeter. If the earth’s density were equal to the average nuclear density, the earth’s radius would be only about 200 meters.
To hold positively charged protons together...
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Isotopes01:12

Isotopes

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Elements have a set number of protons that determines their atomic number (Z). For example, all atoms with eight protons are oxygen; however, the number of neutrons can vary for atoms of the same element. The sum of the number of protons and the number of neutrons is the mass number (A). Atoms with the same atomic number but different mass numbers are called isotopes. Elements can have multiple isotopes, for example, carbon-12, carbon-13, and carbon-14.
An element's atomic mass, or weight,...
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Radioactivity and Nuclear Equations03:18

Radioactivity and Nuclear Equations

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Nuclear chemistry is the study of reactions that involve changes in nuclear structure. The nucleus of an atom is composed of protons and, except for hydrogen, neutrons. The number of protons in the nucleus is called the atomic number (Z) of the element, and the sum of the number of protons and the number of neutrons is the mass number (A). Atoms with the same atomic number but different mass numbers are isotopes of the same element.
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Nuclear Transmutation03:20

Nuclear Transmutation

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Nuclear transmutation is the conversion of one nuclide into another. It can occur by the radioactive decay of a nucleus, or the reaction of a nucleus with another particle. The first manmade nucleus was produced in Ernest Rutherford’s laboratory in 1919 by a transmutation reaction, the bombardment of one type of nuclei with other nuclei or with neutrons. Rutherford bombarded nitrogen-14 atoms with high-speed α particles from a natural radioactive isotope of radium and observed...
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Mass Spectrometry: Isotope Effect01:13

Mass Spectrometry: Isotope Effect

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Most elements exist in nature as a mixture of isotopes. The isotopes differ in weight due to their respective number of neutrons. The molecular weight of a molecule is different depending on the specific isotope of its elements involved. As a result, the mass spectrum of the molecule exhibits peaks from the same fragment at multiple positions. The positions of these mass signals depend on the difference between the molecular mass. Furthermore, the intensity of these signals is dependent on the...
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Preparing an Isotopically Pure 229Th Ion Beam for Studies of 229mTh
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The isotope distribution: A rose with thorns.

Jürgen Claesen1,2, Alan Rockwood3, Mikhail Gorshkov4

  • 1Department of Epidemiology and Data Science, Amsterdam UMC, Vrije Universiteit Amsterdam, Epidemiology and Data Science, Amsterdam, The Netherlands.

Mass Spectrometry Reviews
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Summary

Observed isotope distribution in mass spectrometry can differ from theoretical calculations due to various factors. Understanding these deviations is crucial for accurate molecular identification and analysis in complex mixtures.

Keywords:
(ultra)‐high‐resolution mass spectrometrycoalescencedata processingion trapisotope distribution

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Area of Science:

  • Analytical Chemistry
  • Spectroscopy
  • Computational Chemistry

Background:

  • Isotope distributions, reflecting isotopologue probabilities, are theoretically calculable.
  • Modern mass spectrometry allows high-sensitivity measurement of molecular isotope distributions.
  • Discrepancies between observed and expected isotope distributions are common.

Purpose of the Study:

  • To review factors influencing observed isotope distributions in mass spectrometry.
  • To highlight the utility of isotope distribution analysis in various scientific applications.
  • To provide a comprehensive overview of experimental and processing-related influences.

Main Methods:

  • Literature review of factors affecting isotope distribution measurement.
  • Discussion of theoretical calculations versus experimental observations.
  • Analysis of mass spectrometry stages influencing data acquisition and processing.

Main Results:

  • Identified key factors impacting observed isotope distribution: elemental isotope variations, ion sampling, ion interactions, electronic noise, centroiding, and apodization.
  • Demonstrated that deviations from theoretical distributions are not merely artifacts but offer analytical value.
  • Outlined the occurrence of these factors across the entire mass spectrometry workflow.

Conclusions:

  • Deviations in observed isotope distributions from theoretical values are influenced by multiple factors throughout the mass spectrometry process.
  • Despite complicating analysis, these deviations are valuable for applications like proteomics and elemental composition determination.
  • A thorough understanding of these factors is essential for accurate interpretation of mass spectral data.