110 Examples of Isotopes

Isotopes are atoms of the same element with different numbers of neutrons in their nucleus. As they differ in the number of neutrons in the nucleus, they have a different mass number.

The atoms that are isotopes to each other, have the same atomic number, but different mass number. The atomic number is the number of protons in the nucleus, and the mass number is the sum of the number of neutrons and protons found in the nucleus.

Examples of isotopes The three examples of hydrogen isotopes.

If the isotopes are of different elements, then the number of neutrons will also be different. Chemical elements usually have more than one isotope.

There are only 21 elements of the periodic table that only have a natural isotope for its element, such as beryllium or sodium. And on the other hand, there are elements that can reach the 10 stable isotopes such as tin.

There are also elements such as uranium, in which their isotopes can be transformed into stable or less stable isotopes, where they emit radiation, so we call them unstable.

Unstable isotopes are used to estimate the age of natural samples, such as carbon 13, since knowing the rate of disintegration of the isotope in relation to those that have already declined can be known a very accurate age dating. In this way the age of the Earth is known.

We can distinguish between two types of isotopes, natural or artificial. Natural isotopes are found in nature and artificial ones are created in a laboratory by bombardment of subatomic particles.

Leading examples of isotopes

1-Carbon 14: is a carbon isotope with a half-life of 5,730 years that is used in archeology to determine the age of rocks and organic matter.

2-Uranium 235: This uranium isotope is used in nuclear power plants to provide nuclear power, just as it is used to build atomic bombs.

3-Iridium 192: this isotope is an artificial isotope used to check the tightness of the tubes.

4-Uranium 233: This isotope is artificial and not found in nature, and is used in nuclear power plants.

5-Cobalt 60: used for cancer because it emits radiation more powerful than radium and is cheaper.

6-Technetium 99: this isotope is used in medicine to look for clogged blood vessels

7-Radio 226: this isotope is used for the treatment of skin cancer

8-Bromo 82: this is used to perform hydrographic surveys of water flows or the dynamics of lakes.

9-Tritium: This isotope is an isotope of hydrogen used in medicine as a tracer. The well-known hydrogen bomb really is a tritium pump.

10-Iodine 131: is a radionuclide that was used in the nuclear tests carried out in 1945. This isotope increases the risk of cancer in addition to diseases like the thyroid.

11-Arsenic 73: serves to determine the amount of arsenic that has been absorbed by the body

12-Arsenic 74: this is used for the determination and location of brain tumors.

13-Nitrogen 15: is used in scientific research to perform the nuclear magnetic resonance spectroscopy test. It is also used in agriculture.

14-Gold 198: this one is used for the drilling of oil wells

15-Mercury 147: this is used for the realization of electrolytic cells

16-Lanthanum 140: used in boilers and industrial furnaces

17-Phosphorus 32: used in bone medical tests, bones in addition to bone marrow

18-Phosphorus 33: is used to recognize nuclei of DNA or nucleotides.

19-Scandium 46: this isotope is used in soil and sediment analyzes

20-Fluorine 18: also known as Fludesoxyglucose, and is used to make studies of body tissues.

Other examples of isotopes

  1. Antimony 121
  2. Argon 40
  3. Sulfur 32
  4. Barium 135
  5. Beryllium 8
  6. Boro 11
  7. Bromine 79
  8. Cadmium 106
  9. Cadmium 108
  10. Cadmium 116
  11. Calcium 40
  12. Calcium 42
  13. Calcium 46
  14. Calcium 48
  15. Carbon 12
  16. Cerium 142
  17. Zirconium 90
  18. Chlorine 35
  19. Copper 65
  20. Chrome 50
  21. Dystrosy 161
  22. Dysprosium 163
  23. Dysprosium 170
  24. Erbium 166
  25. Tin 112
  26. Tin 115
  27. Tin 120
  28. Tin 122
  29. Strontium 87
  30. Europio 153
  31. Gadolinium 158
  32. Gallium 69
  33. Germanium 74
  34. Hafnium 177
  35. Helio 3
  36. Helio 4
  37. Hydrogen 1
  38. Hydrogen 2
  39. Iron 54
  40. Indio 115
  41. Iridio 191
  42. Iterbio 173
  43. Krypton 80
  44. Krypton 84
  45. Lithium 6
  46. Magnesium 24
  47. Mercury 200
  48. Mercury 202
  49. Molybdenum 98
  50. Neodymium 144
  51. Neon 20
  52. Nickel 60
  53. Nitrogen 15
  54. Osmio 188
  55. Osmium 190
  56. Oxygen 16
  57. Oxygen 17
  58. Oxygen 18
  59. Palladium 102
  60. Palladium 106
  61. Silver 107
  62. Platinum 192
  63. Lead 203
  64. Lead 206
  65. Lead 208
  66. Potassium 39
  67. Potassium 41
  68. Renius 187
  69. Rubidio 87
  70. Ruthenium 101
  71. Ruthenium 98
  72. Samarium 144
  73. Samarium 150
  74. Selenium 74
  75. Selenium 82
  76. Silicon 28
  77. Silicon 30
  78. Thallium 203
  79. Thallium 205
  80. Teluro 125
  81. Teluro 127
  82. Titanium 46
  83. Titanium 49
  84. Uranium 238
  85. Wolframio 183
  86. Xenon 124
  87. Xenon 130
  88. Zinc 64
  89. Zinc 66
  90. Zinc 67

References

  1. COTTON, F. Albert Wilkinson, et al. Basic inorganic chemistry . Limusa, 1996.
  2. RODGERS, Glen E. Inorganic chemistry: Introduction to coordination chemistry, solid state and descriptive . McGraw-Hill Interamericana, 1995.
  3. RAYNER-CANHAM, GeoffScalona García, et al. Descriptive inorganic chemistry . Pearson Education, 2000.
  4. HUHEEY, James E. KEITER, et al. Inorganic chemistry: principles of structure and reactivity . Oxford:, 2005.
  5. GUTIÉRREZ RÍOS, Enrique. Inorganic chemistry . 1994.
  6. HOUSECROFT, Catherine E., et al. Inorganic chemistry . 2006.
  7. COTTON, F. Albert; WILKINSON, Geoffrey. Basic inorganic chemistry . 1987.


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