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Isotopes and Their Uses

 
2.4 Isotopes and Their Uses
 
Definition of Isotopes
Atoms of the same element that have the same number of protons but a different number of neutrons. 
 
Isotope Number of Proton Number of Nucleon
Hydrogen
Hydrogen 1 1
Deuterium 1 2
Tritium 1 3
Oxygen
Oxygen-16 8 16
Oxygen-17 8 17
Oxygen-18 8 18
Carbon
Carbon-12 6 12
Carbon-13 6 13
Carbon-14 6 14
 
Relative Atomic Mass of Isotopes
Definition of Natural Abundance
  • The percentage of isotopes present in a natural sample of an element.
Formula for Relative Atomic Mass


\(\color{black}\text{Relative atomic mass}= \dfrac{\Sigma\,(\%\, \text{Isotope } \times \text{Mass of isotope})}{100}\)
 
This image is a diagram illustrating examples of isotopes. At the center, there is a box labeled ‘EXAMPLE OF ISOTOPES.’ Surrounding this central box are eight other boxes, each containing the name of a different isotope: Cobalt-60, Iodine-131, Phosphorus-32, Uranium-235, Carbon-14, Lead-210, Hydrogen-3, and Sodium-24. Red arrows point from the central box to each of the surrounding boxes. The Pandai logo is in the top right corner.
 
Field Isotopes Uses
Medicine Cobalt-60 In radiotherapy to kill cancer cells without surgery.
Iodine-131 Treatment of thyroid disorders such as hyperthyroidism and thyroid cancer.
Agriculture Phosphorus-32 Study of plant metabolism.
Nuclear Uranium-235 Generating electricity through nuclear power generator.
Archaeology Carbon-14 Estimation of artifacts or fossils’ age.
Lead-210 In determining the age of sand and earth layers up to 80 years.
Industry Hydrogen-3 As a detector to study sewage and liquid wastes.
Engineering Sodium-24 In detecting leakage in underground pipes.
 

 

 

 

 

 

The views expressed in the notes here are those of the contributor and don’t necessarily represent the views of Pandai.

Isotopes and Their Uses

 
2.4 Isotopes and Their Uses
 
Definition of Isotopes
Atoms of the same element that have the same number of protons but a different number of neutrons. 
 
Isotope Number of Proton Number of Nucleon
Hydrogen
Hydrogen 1 1
Deuterium 1 2
Tritium 1 3
Oxygen
Oxygen-16 8 16
Oxygen-17 8 17
Oxygen-18 8 18
Carbon
Carbon-12 6 12
Carbon-13 6 13
Carbon-14 6 14
 
Relative Atomic Mass of Isotopes
Definition of Natural Abundance
  • The percentage of isotopes present in a natural sample of an element.
Formula for Relative Atomic Mass


\(\color{black}\text{Relative atomic mass}= \dfrac{\Sigma\,(\%\, \text{Isotope } \times \text{Mass of isotope})}{100}\)
 
This image is a diagram illustrating examples of isotopes. At the center, there is a box labeled ‘EXAMPLE OF ISOTOPES.’ Surrounding this central box are eight other boxes, each containing the name of a different isotope: Cobalt-60, Iodine-131, Phosphorus-32, Uranium-235, Carbon-14, Lead-210, Hydrogen-3, and Sodium-24. Red arrows point from the central box to each of the surrounding boxes. The Pandai logo is in the top right corner.
 
Field Isotopes Uses
Medicine Cobalt-60 In radiotherapy to kill cancer cells without surgery.
Iodine-131 Treatment of thyroid disorders such as hyperthyroidism and thyroid cancer.
Agriculture Phosphorus-32 Study of plant metabolism.
Nuclear Uranium-235 Generating electricity through nuclear power generator.
Archaeology Carbon-14 Estimation of artifacts or fossils’ age.
Lead-210 In determining the age of sand and earth layers up to 80 years.
Industry Hydrogen-3 As a detector to study sewage and liquid wastes.
Engineering Sodium-24 In detecting leakage in underground pipes.
 

 

 

 

 

 

The views expressed in the notes here are those of the contributor and don’t necessarily represent the views of Pandai.
Chapter : Matter and Atomic Structure
Topic : Justifying the uses of isotopes in various fields
Form 4 Chemistry
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