Atomic Mass of Silver (Ag)
The relative atomic mass of Silver is 107.87 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 Silver. 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 Silver page is one click away.
Silver by the numbers
Z = 47 fixes the protons; the neutron count can vary between isotopes, which is why the atomic mass is an average (107.87 u) rather than a round number.
| Quantity | Value |
|---|---|
| Atomic number (Z) | 47 |
| Relative atomic mass | 107.87 u |
| Protons | 47 |
| Neutrons (commonest isotope) | 61 |
| Electrons | 47 |
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 (107.87). Exams love this one-mark distinction.
Students also ask
Is the atomic mass of Silver a whole number?
No. 107.87 u is the average of Silver'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 Silver have?
Neutrons = mass number − atomic number. For Silver's commonest isotope that is about 108 − 47 = 61, though the exact count differs between isotopes.