If the relative molecular mass of an element is not a whole number, it can be deduced that the element is
naturally radioactive
abundant in nature
a transition metal
an isotopic mixture
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If the relative mass is a whole number (or very close to one), it usually means one of two things:
Mono-isotopic: The element has only one stable, naturally occurring isotope (e.g., Fluorine-19 or Sodium-23). Since there’s nothing else to mix in, the average mass stays a whole number.
Dominant Isotope: One isotope is so incredibly abundant (like Carbon-12 at 98.9%) that the traces of others don't shift the average far enough to move it off the whole number in a basic calculation.
It’s worth noting that even "whole" masses are rarely exactly integers due to the tiny mass of electrons and "binding energy," but for most chemistry problems, we treat them as whole numbers.
@merit zeal
If the relative molecular mass (or more commonly, the relative atomic mass) of an element is not a whole number, it can be deduced that the element is an isotopic mixture (i.e., it exists as a mixture of different isotopes).
