Atomic Mass of Nitrogen (N)
The relative atomic mass of Nitrogen is 14.007 u — the weighted average of its naturally occurring isotopes, on the carbon-12 scale.
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Nitrogen by the numbers
Z = 7 fixes the protons; the neutron count can vary between isotopes, which is why the atomic mass is an average (14.007 u) rather than a round number.
| Quantity | Value |
|---|---|
| Atomic number (Z) | 7 |
| Relative atomic mass | 14.007 u |
| Protons | 7 |
| Neutrons (commonest isotope) | 7 |
| Electrons | 7 |
Atomic mass vs mass number
Mass number (A) counts particles — protons + neutrons in one specific atom, always a whole number. Relative atomic mass is the experimentally measured average over all natural isotopes, so it comes out fractional (14.007). Exams love this one-mark distinction.
Students also ask
Is the atomic mass of Nitrogen a whole number?
No. 14.007 u is the average of Nitrogen's natural isotopes, which is why it lands between whole numbers. The mass number of a single isotope, though, is always whole.
How many neutrons does Nitrogen have?
Neutrons = mass number − atomic number. For Nitrogen's commonest isotope that is about 14 − 7 = 7, though the exact count differs between isotopes.