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

 

\(\text{Relative atomic mass}= \dfrac{\Sigma(\% \text{Isotope } \times \text{Mass of isotope})}{100}\)

 
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
 

 

 

 

 

 

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

 

\(\text{Relative atomic mass}= \dfrac{\Sigma(\% \text{Isotope } \times \text{Mass of isotope})}{100}\)

 
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