This is because of the existence of isotopes. What's an isotope? It's an element that has a specific number of neutrons. I'll give an example. Carbon has 6 Neutrons, 6 Protons, 6 Electrons.
That's the most common form of Carbon. But 1% of all Carbon is an isotope that has 1 extra Neutron. So it weighs 1 more, also. So this isotope weighs 13 instead of 12. We call it Carbon 13, or 13C.
There's also a 14C and so on....but in far smaller amounts.
So anyhow, since we have 99% Carbon weighing 12 and 1% Carbon weighing 13, what weight do we put on our Periodic Table?
Well, I guess we could put the most common.
But what about Bromine? That has 2 major isotopes. One weighs 79 and the other 81, they are 51% and 49% (very roughly) abundant respectively.
That's almost an exact split...it'd be pretty ridiculous to only put the weight of one.
So instead we say it's weight is 79.9...which is it's weight averaged over all of it's isotopes, with respect to their abundance.
It doesn't seem right to average it on an atom-to-atom basis. But if I'm weighing 2grams of my sample, there are HUGE numbers of molecules there. And the only way I can do an accurate calculation is to know an averaged mass, because my sample WILL contain all of the isotopes.
If I calculate for only 1 isotopic weight, my calculations will be wrong. That's why we average them.
Basically for convenience, to avoid using powers of 10 as part of numbers more often than necessary; there is no commonly accepted prefix for the basic mass unit "gram" to make the mass of a single atom greater than a small fraction of such a unit.
Subatomic particles are not measured by their weight in a scientific situation; they are measured by their rest masses in most cases or by their relativistic mass if they are interacting in a collision.
The average atomic weight of a chemical element take into account the isotopic composition and the atomic masses of these isotopes.
The atomic weights (not mass !) of chemical elements are related to 1/12 of the mass of the isotope carbon-12 in the ground state (the Atomic Mass unit).
They are calculated the ratio of the average mass of one atom of an element to one twelfth of the mass of an atom of carbon-12.
Both have a basis of carbon-12
The mass number of an isotope of an element is equal to its atomic mass number. However, the atomic weight of an element is a weighted average of the isotopes that occur in the element in nature. Because almost all elements have more than one naturally occurring isotope (if they have any), the atomic weights of most elements are not integers, as mass numbers always are.
Average :]
The relative atomic mass is 180.948
In increasing order of atomic weights.
If they have the same atomic number but different mass, then they have a different number of neutrons, and they are called ISOTOPES.
That would be Carbon (C). Which has a designated mass of 12.
True. The unit for the atomic weights of chemical elements is the relative atomic mass unit (1/12 from the atomic mass of the isotope 12C). Note that atomic weights is used for elements and atomic mass for isotopes.
True
Because atomic weights must be measured in fractions.
relative Atomic Mass
relative atomic mass
Actually weights are too small and are hard to work with.
It is approximately equivalent to the number of protons and neutrons in the atom (the mass number) or to the average number allowing for the relative abundances of different isotopes.
the relative atomic mass for the element potassium is 39.0983
The mass number of an isotope of an element is equal to its atomic mass number. However, the atomic weight of an element is a weighted average of the isotopes that occur in the element in nature. Because almost all elements have more than one naturally occurring isotope (if they have any), the atomic weights of most elements are not integers, as mass numbers always are.
Average :]
Atomic Mass Number