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How do atoms of nitrogen-14 and nitrogen-15 differ from each other in terms of their atomic numbers, mass numbers and atomic structure?

Last updated date: 29th Feb 2024
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Hint: Isotopes are various types of a component that have a similar number of protons yet the various number of neutrons. Many components, for example, carbon, potassium, and uranium—have various normally occurring isotopes. A neutral atom of \[Carbon - 12\] contains six protons, six neutrons, and six electrons; in this manner, it has a mass number of \[12\] (six protons in addition to six neutrons). Neutral carbon-14 contains six protons, eight neutrons, and six electrons; its mass number is 14 (six protons in addition to eight neutrons). These two substitute types of carbon are isotopes. (e.g., \[carbon - 14\] decaying to \[nitrogen - 14\] )

Complete step by step answer:All things considered, \[^{14}N\] and \[^{15}N\] are two isotopes of nitrogen implying that they have a comparable proportion of protons yet the extraordinary proportion of neutrons.

Thus, the main thing we will see is that they have a similar nuclear number.
We realize that the mass number of an atom is the amount of its proton number and neutron number. Since the two isotopes have different measures of neutrons, they will have various masses, and we reason that their mass numbers are not the same as one another.
Nothing truly changes in their nuclear structure. They will have an alternate measure of neutrons, there are \[7\] neutrons in \[^{14}N\] and \[8\] neutrons in \[^{15}N\] . Besides that, they will have similar measures of electrons.

A few isotopes are stable, yet others can emit, or kick out, subatomic particles to arrive at a more steady, lower-energy, and configuration. Such isotopes are called radioisotopes, and the process where they discharge particles and energy is known as decay. Radioactive decay can cause an adjustment in the quantity of protons in the nucleus; when this occurs, the identity of the atom changes.
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