isotope with advantage and disadvantage
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It will help the 1st year medical student to understand isotope with their advantage and disadvantage. Also, help to know about the different type and basic structure of isotope.
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Radioactive decay and nuclear radiation involve the spontaneous disintegration of an unstable nucleus, emitting particles or electromagnetic radiation. There are different types of radioactive decay that affect the nucleus, changing the number of protons or neutrons. Half-life is the time for half of a radioactive sample to decay and relates to a nucleus's stability, with more stable nuclei having longer half-lives. A decay series involves successive decays from a parent nuclide to daughter nuclides until a stable nuclide is reached. Artificial radioactive nuclides are made through artificial transmutations like bombarding nuclei, and are significant for producing transuranium elements.
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Radioactivity is the spontaneous disintegration of atomic nuclei to reach stability, which involves the emission of ionizing radiation or particles. This process is known as radioactive decay, nuclear decay, or radioactive disintegration. Radionuclides, which are atoms that undergo this process, can be naturally occurring or artificially produced in particle accelerators or nuclear reactors. The half-life of a radioisotope is the amount of time it takes for half of the radioactive atoms in a sample to decay. There are three types of half-lives: physical, biological, and effective.
Half Life
1) The document discusses radioactive decay and half-life, which is the time it takes for half of the atoms in a radioactive sample to decay.
2) Different elements have different decay rates and half-lives, which are properties of the element that cannot be changed.
3) While the decay of individual atoms is random, the decay of a large group of atoms can be predicted and represented through a half-life curve showing the decrease in radioactivity over time.
Quantum Numbers
1) Erwin Schrodinger developed quantum mechanics and formulated the Schrodinger equation in 1926, which treats electrons as waves rather than particles.
2) The Schrodinger equation led to the discovery of quantum numbers that describe electron behavior and allowed for a more accurate model of atomic structure.
3) There are four quantum numbers - the principal quantum number (n) describes the electron shell or energy level, the azimuthal quantum number (l) describes the subshell shape, the magnetic quantum number (m) describes spatial orientation, and the spin quantum number (s) describes electron spin.
Radioactive decay, kinetics and equilibrium
This document discusses radioactive decay, kinetics, and equilibrium. It begins by defining radioactive decay as the spontaneous emission of particles or radiation from atomic nuclei. It describes the three main types of radioactive decay and their effects on atomic and mass numbers. The document then discusses radioactive kinetics, including the concepts of half-life, mean life, and first-order decay. Finally, it covers radioactive equilibrium and the different types including transient, secular, and no equilibrium. Diagrams of activity profiles over time are provided to illustrate the different equilibrium conditions.
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introduction
what is isotopes
defination
main types
srtable and unstable isotopes
application of isotopes
agriculture
Radioactive isotopes
Radioactive isotopes emit radiation through radioactive decay as their unstable nuclei break down. There are three main types of radiation emitted: alpha particles, beta particles, and gamma rays. Radioactive isotopes are used in scientific research, analytical applications like radioimmunoassays, and medical diagnostic procedures and therapies. Some key radioactive isotopes used include iodine-131 for thyroid imaging and cancer treatment, technetium-99m for thyroid scans, and strontium-89 or samarium-153 to treat bone metastases.
Basic Radiation Physics - Mr. D.S. Patkulkar.pdf
This document provides an overview of basic radiation physics for radiation safety officer (RSO) certification. It defines ionizing radiation and different types including alpha, beta, gamma, x-rays and neutron radiation. It describes the composition of atoms and isotopes. Unstable nuclei undergo radioactive decay through emission of particles or photons. Radiation has sufficient energy to ionize atoms. The document covers radiation quantities, units of measurement, radiation interactions with matter and shielding. Understanding basic radiation physics is essential for RSOs to safely control and use radioactive sources.
Atomic structure
1) Atoms are composed of a small, dense, positively charged nucleus surrounded by negatively charged electrons.
2) Rutherford's gold foil experiment showed that atoms are mostly empty space, with a small, dense nucleus accounting for most of an atom's mass.
3) The atomic number of an element is the number of protons in its nucleus, while the mass number includes both protons and neutrons. Isotopes of the same element have different numbers of neutrons.
Radio isotopes
This document discusses radioactivity and radioactive decay. It defines key terms like isotopes, half-life, and units of radioactivity. It describes different types of radioactive decay including alpha, beta, gamma emission and electron capture. Detection methods like autoradiography, gas detectors, and scintillation counting are summarized. Applications of radioisotopes in areas like tracing metabolic pathways, enzyme assays, and diagnostic tests are briefly mentioned. Some therapeutic uses and health hazards of radiation are also noted.
Radioactivity & Radiopharmaceuticals Manik
This document discusses radioactivity and radiopharmaceuticals used in nuclear medicine for diagnosis and treatment. It defines isotopes, radioactive isotopes, and radioactivity. The major types of radioactive decay are described, including alpha particles, beta particles, gamma rays, and electron capture. The properties and effects of each type of radiation are summarized. The kinetics of radioactive decay are explained using decay constant and half-life. Radiation dosimetry is introduced as the calculation of radiation dose exposed to and absorbed by objects.
introduction to nuclear chemistry for advanced students by igori wallace
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This document provides an overview of atomic structure and the periodic table. It discusses key topics including:
- Atoms have existed since the beginning of the universe and are mostly empty space.
- Elements are made of only one type of atom. The periodic table organizes all known elements.
- Atoms contain protons, neutrons, and electrons. The number of protons determines an element's identity.
- Isotopes are atoms of the same element with different numbers of neutrons.
- Electrons can have distinct energy levels, emitting light of specific frequencies when changing levels.
- The periodic table arranges elements by proton number and electron configuration in shells.
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Radiometric dating determines the age of objects by measuring the decay of radioactive isotopes into stable daughter isotopes. There are four main types of radiometric dating: 1) potassium-argon dating works on rocks over 100,000 years old, 2) uranium-lead dating dates rocks over 10 million years using uranium-238 decay, 3) rubidium-strontium dating also dates rocks over 10 million years, and 4) carbon-14 dating is used on objects under 50,000 years old by measuring carbon-14 decay. The rate of radioactive decay remains constant, allowing scientists to determine a sample's age based on the ratio of parent and daughter isotopes.
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isotope with advantage and disadvantage
- 1. Dangerous
- 2. Definition Atoms with same atomic number/number of proton but different atomic weight (number of protons+neutrons). So atoms may be different atomic weight due to different neutron number.
- 3. Isotopes are variants of a particular chemical element which differ in neutron number. All isotopes of a given element have the same number of protons but different numbers of neutrons in each atom.
- 4. The term isotope is formed from the Greek roots isos ("equal") and topos ("place"), meaning "the same place“. So the meaning behind the name is that different isotopes of a single element occupy the same position on the periodic table.
- 7. The number of protons within the atom's nucleus is called atomic number and is equal to the number of electrons in the neutral (non-ionized) atom. Each atomic number identifies a specific element, but not the isotope; an atom of a given element may have a wide range in its number of neutrons.
- 8. The number of (both protons and neutrons) in the nucleus is the atom's mass number, and each isotope of a given element has a different mass number.
- 9. Types of isotope Stable isotope/ non radioactive Unstable isotope/ radioactive isotope
- 10. Stable isotope The first evidence for multiple isotopes of a stable (non- radioactive) element was found by J. J. Thomsonin 1913 as part of his exploration into the composition of canal rays (positive ions)
- 11. Stability of an isotope depends on the definite neutron to proton ratio which is specific for a specific atom. In low atomic weight atoms stability achieved with neutron to proton ratio around one
- 12. In case high molecular weight stability usually achieved by more neutron than proton and the ratio more than one (>1). Naturally occurring isotopes are predominantly stable isotope.
- 13. Examples of stable isotopes
- 14. Unstable isotope (raidoactive) The existence of isotopes was first suggested in 1913 by the radiochemist Frederick Soddy based on studies of radioactive decay chains that indicated about 40 different species referred to as radioelements (i.e. radioactive elements) between uranium and lead
- 15. Unstable isotope (raidoactive) Have the capacity to emit radiation These isotopes neutron and proton ratio far from stability ratio Isotopes of heavy elements are usually unstable example: radium, urenium Aim of radioactivity is to become stable
- 16. Example
- 18. Radioactive decay It is the spontaneous decomposition or disintegration of an unstable isotope of a definite element in an attempt to become a stable isotope with simultaneous emission of radiation (α,β,γ) and formation of new element.
- 19. Radioactivity It is the spontaneous emission of accelerated particles (radiation) from an unstable isotope by radio active decay.
- 20. Mechanisms of radio active decay Alpha decay: heavy atoms (atomic number >70) may emit alpha particles from radio active nucleus. beta decay: atomic number <60 may emit beta particles. Positive beta decay: in case of artificial isotope positive beta particles (positron) emit.
- 21. Half life of radioactive isotope Radioactive isotope Half life 14Carbon 5760 yrs 3Hydrogen 12 yrs 60Cobalt 5.3yrs 51Chromium 28days 32Phosphrus 14days 131Iodine 8days 99Technetium 8hrs It is the time required for a radioactive isotope to reduce its radioactivity half of its initial value
- 22. Clinical use/importance of radio- active isotope Diagnostic use- to diagnosis diseases Therapeutic use- radiotherapy treatment for malignancy Use in tracer technique- to study of metabolic pathway Measurement of volume & spaces- ECF volume, blood volume Measurement of regional blood flow Sterilization of medical instrument
- 23. Diagnostic use Iodine uptake test for thyroid disorder Radio immune assay for hormonal disorder Organ scanning- bone, brain, thyroid Absorption test- iron, Vit B12 RBC half life measurement Isotope renogram for measurement of GFR, renal clearance
- 24. Radiation hazards/disadvantage of radio isotope Immediate hazard: 1. Bone marrow depression and immune suppression 2. Damage to intestinal mucosa causing diarrhoea & malabsorption 3. Baldness, rough scaly skin 4. In pregnancy: fetal growth retardation, congenital malformation fetal or neonatal death
- 25. Delayed hazards: carcinogenesis, sterility, neonatal death Genetic effect: DNA damage, mutation
- 26. Radiosensitive tissue These are most rapidly dividing tissue. Such as Bone marrow Gonads Lymph node Skin Intestine
Editor's Notes
- It is the time required for a radioactive isotope to reduce its radioactivity half of its initial value