the mass of some atoms are in decimal
Answers
Answer:
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Explanation:
Why are the atomic masses in decimal form and not as a whole number?
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Atomic mass is never an integer number for several reasons:
The atomic mass reported on a periodic table is the weighted average of all the naturally occuring isotopes. Being an average it would be most unlikely to be a whole number.
The mass of an individual atom in atomic mass units is the mass relative to carbon-12. Only carbon-12 has a mass exactly equal to itself.
Even the mass of a single proton (1.00727661 u), or neutron (1.00866520 u) is not a whole number. These are also the ratio of their masses to carbon-12 (since carbon-12 is the reference standard, its the only atom whose atomic mass
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Why are the atomic masses in decimal form and not as a whole number?
Although atomic weights are not integers due to the averaging of the varying quantities of isotopes constituting each element, this does not explain why the masses of the various isotopes are not, and indeed cannot be expressed as integers. First, a nucleus is comprised of protons and neutrons, which have different masses. More importantly, the binding energy per proton or neutron added to the nucleus. Starting with protium (H-1), energy is released as each nucleon is added until about the nuclear mass of iron and additional energy is required to add each additional nucleon beyond that. According to Einstein’s relationship, this energy change must be expressed as a change in mass.
Protium has a mass of 1.007825 AMU. Adding a neutron (1.008665 AMU) gives a deuterium atom of 2.014102 AMU, not the 2.0015490 obtained by summing the individual masses. Since the mass of a deuteron is not twice the mass of a proton (1.015650 AMU) their mass ratio cannot be expressed as an integer.