Atomic Mass of Vanadium (V)
The relative atomic mass of Vanadium is 50.942 u — the weighted average of its naturally occurring isotopes, on the carbon-12 scale.
Teachers call it "one fact, fully handled" — exactly what this page does for Vanadium. The answer sits at the top in bold; scroll for the working, the shell-by-shell breakdown and the two questions students ask most. Need the whole picture instead — history, characteristics, uses, exam questions? The full Vanadium page is one click away.
Vanadium by the numbers
Z = 23 fixes the protons; the neutron count can vary between isotopes, which is why the atomic mass is an average (50.942 u) rather than a round number.
| Quantity | Value |
|---|---|
| Atomic number (Z) | 23 |
| Relative atomic mass | 50.942 u |
| Protons | 23 |
| Neutrons (commonest isotope) | 28 |
| Electrons | 23 |
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 (50.942). Exams love this one-mark distinction.
Students also ask
Is the atomic mass of Vanadium a whole number?
No. 50.942 u is the average of Vanadium'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 Vanadium have?
Neutrons = mass number − atomic number. For Vanadium's commonest isotope that is about 51 − 23 = 28, though the exact count differs between isotopes.