Radioactivity: Difference between revisions
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'''Radioactivity''' is the | '''Radioactivity''' is the phenomenon of emission—i.e., radiation—of electromagnetic energy and subatomic particles by the atomic nuclei of some of Earth's naturally occurring [[chemical element]]s, and all those 'artificial' chemical elements made by scientists in the laboratory. Atoms whose nuclei exhibit the phenomenon of radioactivity are referred to as being 'radioactive'. Nuclei can radiate spontaneously or can be induced to do so by [[nuclear fission]] (splitting of the nucleus) or [[nuclear fusion]] (merging of nuclei). Energy release is in the [[X-ray]], [[gamma radiation]] and [[cosmic radiation]] ranges of the [[electromagnetic spectrum]], and as [[kinetic energy]] of particles such as [[neutron]]s, [[alpha particle]]s, [[beta particle]]s, and [[neutrino]]s.<ref name=closeparphys2004>Close FE. (2004) ''Particle Physics: A Very Short Introduction''. Oxford: Oxford University Press. ISBN 0192804340. | [http://bit.ly/ekiYEP Google Books preview].</ref> <ref name=brownchem11>"Nuclear Chemistry". Chapter 21. In: Brown TL, Eugene Lemay H, Bursten BE, Murphy CJ. (2009) ''Chemistry: The Central Science''. 11th edition. Upper Saddle River, NJ: Pearson Education, Inc. ISBN 9780136006176.</ref> | ||
Not all | ==Overview== | ||
Not all chemical elements exhibit radioactivity: specific elements may have stable (i.e., non-radioactive) and radioactive (unstable) [[isotope]]s—all the isotopes of a given chemical element have the same number of protons but differing number of neutrons. | |||
All of the elements with atomic numbers Z=84 and greater—i.e., elements that have 84 or more protons—are radioactive, having either no stable naturally occurring isotope, or if an artificial (man-made) element, having no stable isotope. Of the elements with atomic numbers less than Z=84, only technetium (Tc, Z=43) and promethium (Pm, Z=61) have no stable isotopes. | |||
The nucleus of an isotope with a specified number of protons and neutrons is referred to as a [[nuclide]]. Radioactive nuclei are referred to as [[radionuclide]]s and their atoms are referred to as [[radioisotope]]s. | |||
Nuclei are composed of positively charged particles, [[proton]]s and—with the exception of the hydrogen nucleus—one or more electrically neutral particles, [[neutron]]s. The number of protons defines the [[atomic number]], and the total number of protons and neutrons defines the [[atomic mass]]. Counteracting the repulsive electromagnetic force between the positively charged protons, another fundamental force of nature, an attractive force, called the [[strong nuclear force]], comes into play when protons become closely packed, close enough (<10<sup>−15</sup> meters apart) to essentially touch each other. That strong attractive force helps keep the protons from flying apart. | |||
Uranium's 235 isotope, which occurs in nature with an abundance of about | Neutrons, nearly the same size and mass as protons but carrying no electrical charge, also feel the strong nuclear force. The presence of neutrons, interposed among the protons, adds to the mass of the nucleus, and also to its overall strong attractive force, thus helping stabilize the nucleus. A radioactive isotope lacks some number of neutrons needed to stabilize the nucleus. In general an unstable nucleus will, in the process of radiation, 'decay' to a more stable one. | ||
[[Quantum mechanics]] postulates that it is impossible to predict at which point in time a given nucleus will emit particles or γ rays, but statistics may be applied to a sufficiently large number of nuclei and it becomes possible to speak of the [[half-life]], which is the time-period in which half the nuclei have undergone radioactive decay. | |||
For example, [[uranium]], with an atomic number of 92, has the relatively stable isotope <sup>238</sup>U with a half-life of 4.46 × 10<sup>9</sup> years. Although this is a very long period, a sufficiently large collection of <sup>238</sup>U nuclei emits detectable amounts of [[alpha particle|α particles]] and even its decay product, the 234 isotope of [[thorium]], emits detectable amounts of β particles. | |||
==Units of radioactivity== | |||
[[Image:RadiationUnitRelations.png|left|450px|thumb|Overview of phenomena and units]] | |||
A variety of [[units of radioactivity]] characterize the energy of a radioactive source, as well as its absorption by different materials. | |||
==History of radioactivity== | |||
To fully appreciate the history of radioactivity requires appreciating the history of the studies of the nature and uses of [[electricity]] that led to the discovery of [[X-ray]]s.... | |||
Radioactivity was first discovered in uranium salts. [[Henri Becquerel]] noted on 1 March 1896 that the uranyl salt K<sub>2</sub>UO<sub>2</sub>(SO<sub>2</sub>)<sub>2</sub>•(H<sub>2</sub>O)<sub>2</sub> blackens photographic film after several days of contact. It is now believed that the blackening observed by Becquerel was caused by the β radiation from uranium's "daughter" thorium. In 1898 [[Marie Curie]] and her husband [[Pierre Curie|Pierre]] coined the name "radioactive substance" and afterwards it was a small step to the term radioactivity. | |||
Uranium's 235 isotope, which occurs in nature with an abundance of about 0.7%, is only slightly less stable than the 238 isotope, with a half-life of 7.13 × 10<sup>8</sup> years. It will fission into two almost equal parts when it is struck by a neutron and then it releases enormous amounts of energy, which makes the 235 isotope suitable as fuel for [[nuclear reactor]]s and as explosive in nuclear weapons. | |||
==References== | |||
{{reflist}} | |||
Revision as of 16:02, 22 March 2024
Radioactivity is the phenomenon of emission—i.e., radiation—of electromagnetic energy and subatomic particles by the atomic nuclei of some of Earth's naturally occurring chemical elements, and all those 'artificial' chemical elements made by scientists in the laboratory. Atoms whose nuclei exhibit the phenomenon of radioactivity are referred to as being 'radioactive'. Nuclei can radiate spontaneously or can be induced to do so by nuclear fission (splitting of the nucleus) or nuclear fusion (merging of nuclei). Energy release is in the X-ray, gamma radiation and cosmic radiation ranges of the electromagnetic spectrum, and as kinetic energy of particles such as neutrons, alpha particles, beta particles, and neutrinos.[1] [2]
Overview
Not all chemical elements exhibit radioactivity: specific elements may have stable (i.e., non-radioactive) and radioactive (unstable) isotopes—all the isotopes of a given chemical element have the same number of protons but differing number of neutrons.
All of the elements with atomic numbers Z=84 and greater—i.e., elements that have 84 or more protons—are radioactive, having either no stable naturally occurring isotope, or if an artificial (man-made) element, having no stable isotope. Of the elements with atomic numbers less than Z=84, only technetium (Tc, Z=43) and promethium (Pm, Z=61) have no stable isotopes.
The nucleus of an isotope with a specified number of protons and neutrons is referred to as a nuclide. Radioactive nuclei are referred to as radionuclides and their atoms are referred to as radioisotopes.
Nuclei are composed of positively charged particles, protons and—with the exception of the hydrogen nucleus—one or more electrically neutral particles, neutrons. The number of protons defines the atomic number, and the total number of protons and neutrons defines the atomic mass. Counteracting the repulsive electromagnetic force between the positively charged protons, another fundamental force of nature, an attractive force, called the strong nuclear force, comes into play when protons become closely packed, close enough (<10−15 meters apart) to essentially touch each other. That strong attractive force helps keep the protons from flying apart.
Neutrons, nearly the same size and mass as protons but carrying no electrical charge, also feel the strong nuclear force. The presence of neutrons, interposed among the protons, adds to the mass of the nucleus, and also to its overall strong attractive force, thus helping stabilize the nucleus. A radioactive isotope lacks some number of neutrons needed to stabilize the nucleus. In general an unstable nucleus will, in the process of radiation, 'decay' to a more stable one.
Quantum mechanics postulates that it is impossible to predict at which point in time a given nucleus will emit particles or γ rays, but statistics may be applied to a sufficiently large number of nuclei and it becomes possible to speak of the half-life, which is the time-period in which half the nuclei have undergone radioactive decay.
For example, uranium, with an atomic number of 92, has the relatively stable isotope 238U with a half-life of 4.46 × 109 years. Although this is a very long period, a sufficiently large collection of 238U nuclei emits detectable amounts of α particles and even its decay product, the 234 isotope of thorium, emits detectable amounts of β particles.
Units of radioactivity
A variety of units of radioactivity characterize the energy of a radioactive source, as well as its absorption by different materials.
History of radioactivity
To fully appreciate the history of radioactivity requires appreciating the history of the studies of the nature and uses of electricity that led to the discovery of X-rays....
Radioactivity was first discovered in uranium salts. Henri Becquerel noted on 1 March 1896 that the uranyl salt K2UO2(SO2)2•(H2O)2 blackens photographic film after several days of contact. It is now believed that the blackening observed by Becquerel was caused by the β radiation from uranium's "daughter" thorium. In 1898 Marie Curie and her husband Pierre coined the name "radioactive substance" and afterwards it was a small step to the term radioactivity.
Uranium's 235 isotope, which occurs in nature with an abundance of about 0.7%, is only slightly less stable than the 238 isotope, with a half-life of 7.13 × 108 years. It will fission into two almost equal parts when it is struck by a neutron and then it releases enormous amounts of energy, which makes the 235 isotope suitable as fuel for nuclear reactors and as explosive in nuclear weapons.
References
- ↑ Close FE. (2004) Particle Physics: A Very Short Introduction. Oxford: Oxford University Press. ISBN 0192804340. | Google Books preview.
- ↑ "Nuclear Chemistry". Chapter 21. In: Brown TL, Eugene Lemay H, Bursten BE, Murphy CJ. (2009) Chemistry: The Central Science. 11th edition. Upper Saddle River, NJ: Pearson Education, Inc. ISBN 9780136006176.