Related Experiment Video
Updated: Jun 16, 2026

10:42
Preparing an Isotopically Pure 229Th Ion Beam for Studies of 229mTh
Published on: May 3, 2019
Decay scheme study of 126Sn and 126Sb
1CEA, LIST, Laboratoire National Henri Becquerel (LNE-LNHB), Gif-sur-Yvette, France. laurent.ferreux@cea.fr
Summary
This study investigated the decay of tin-126 (¹²⁶Sn) using gamma-ray spectrometry. New experimental data refined the understanding of its decay scheme and the branching ratio of antimony-126m (¹²⁶Sb(m)).
Area of Science:
- Nuclear Physics
- Radiochemistry
Background:
- Understanding the decay scheme of radioactive isotopes is crucial for nuclear structure studies.
- Tin-126 (¹²⁶Sn) is a neutron-rich isotope whose decay properties require precise experimental determination.
Purpose of the Study:
- To accurately determine the decay scheme of tin-126 (¹²⁶Sn).
- To measure key parameters including the isomeric branching ratio of antimony-126m (¹²⁶Sb(m)) and the maximum beta energy.
- To re-examine and refine the decay scheme of ¹²⁶Sn and its daughter products based on new experimental findings.
Main Methods:
- Utilized gamma-ray spectrometry to measure relative photon emission intensities from purified ¹²⁶Sn samples.
- Employed liquid scintillation to determine the maximum beta energy associated with the ¹²⁶Sn decay.
- Calculated the isomeric branching ratio for ¹²⁶Sb(m) and the Kbeta/Kalpha intensity ratio for Sb.
Main Results:
- The isomeric branching ratio of antimony-126m (¹²⁶Sb(m)) was determined to be 18.6 (6) %.
- The Kbeta/Kalpha intensity ratio of Sb was found to be 0.226 (11).
- New experimental data provided a basis for re-evaluating the decay scheme of ¹²⁶Sn.
Conclusions:
- The experimental results provide critical data for nuclear structure models.
- The refined decay scheme of ¹²⁶Sn enhances our understanding of nuclear processes.
- Accurate decay data are essential for applications in nuclear science and technology.
Related Concept Videos
Nuclear Stability
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 in the...
To hold positively charged protons together in the...
Radioactivity and Nuclear Equations
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.
A nuclide of an element has a specific number of protons and...
A nuclide of an element has a specific number of protons and...
Types of Radioactivity
The most common types of radioactivity are α decay, β decay, γ decay, neutron emission, and electron capture.
Alpha (α) decay is the emission of an α particle from the nucleus. For example, polonium-210 undergoes α decay:
Alpha (α) decay is the emission of an α particle from the nucleus. For example, polonium-210 undergoes α decay:
Nuclear Transmutation
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 protons being...
Atomic Number and Mass Number
The number of protons in the nucleus of an atom is its atomic number (Z). This is the defining trait of an element. Its value determines the identity of the atom. For example, any atom that contains six protons is the element carbon and has the atomic number 6, regardless of how many neutrons or electrons it may have. A neutral atom must contain the same number of positive and negative charges, so the number of protons equals the number of electrons. This means that the atomic number also...
Isotopes and Radioisotopes
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 more...
An isotope containing more...

