
Chemistry: Matter & Change, Student Edition (1st Edition) Edit editionThis problem has been solved:
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An isotope is an atom of an element with an unbalanced number of Protons and Neutrons. This imbalance leads to some characteristic differences in the nature of an element’s isotopes.
For Hydrogen, three common isotopes are found in nature. The most abundant isotope of Hydrogen is Protium. Protium has one Electron and one Proton, but has no Neutron in its nucleus.
The second isotope Deuterium is sometimes called Heavy Hydrogen. It has one Proton, one Neutron, and one electron. It is called Heavy Hydrogen because the atomic weight of the isotope is greater than the average atomic mass of the element Hydrogen.
The last isotope of Hydrogen is called Tritium. The isotope Tritium is radioactive. It is radioactive because the Neutron to Proton ratio is out of the band of stability. The band of stability is the range of ratios between Neutrons and Protons in a nucleus that produce a stable isotope. Tritium has one Proton, two Neutrons, and one Electron.
Corresponding textbook

- Chapter EH
- Chapter 1
- Chapter 2
- Chapter 2.SP
- Chapter 3
- Chapter 3.SP
- Chapter 4
- Chapter 4.SP
- Chapter 5
- Chapter 5.SP
- Chapter 6
- Chapter 6.SP
- Chapter 7
- Chapter 7.SP
- Chapter 8
- Chapter 8.SP
- Chapter 9
- Chapter 9.SP
- Chapter 10
- Chapter 10.SP
- Chapter 11
- Chapter 11.SP
- Chapter 12
- Chapter 12.SP
- Chapter 13
- Chapter 13.SP
- Chapter 14
- Chapter 14.SP
- Chapter 15
- Chapter 15.SP
- Chapter 16
- Chapter 16.SP
- Chapter 17
- Chapter 17.SP
- Chapter 18
- Chapter 18.SP
- Chapter 19
- Chapter 19.SP
- Chapter 20
- Chapter 20.SP
- Chapter 21
- Chapter 21.SP
- Chapter 22
- Chapter 22.SP
- Chapter 23
- Chapter 24
- Chapter 24.SP
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