nothing at all. It is just a way of filing them
the mass of an atom of a chemical element expressed in atomic mass units. 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.
There is no good correlation lies between the element reactivity and the atomic mass.
An isotope is identified by atomic number (element number or name), by mass number, and by atomic weight. The mass numberfor an isotope is listed as a leading superscript such as 29Si, which in this example is silicon containing 14 protons and 15 neutrons (a rarer but stable isotope of the element). Similarly the atomic weight is indicated by a superscript such as U235 , an isotope of uranium having 92 protons and 143 neutrons.The actual atomic weight is often expressed as a decimal number corresponding to the mass of the atom in "atomic units", where a proton is about 1.0072, a neutron 1.0086, and an electron about .00055 atomic units.
Atomic number= number of protons. Hydrogen atomic number=1
The atomic number of fluorine is 9.The atomic number of sodium is 11.
Atomic number.
A subscript number after each atomic symbol in a formula for the compound.
Experimentally, I'm not sure, but I know you can look at your periodic chart, the large number over the symbol of each element is teh number of protons in that element.
the mass of an atom of a chemical element expressed in atomic mass units. 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.
12, the same as the number of protons indicated by magnesium having an atomic number of 12.
the answer is that it is called a atomic number.
There is no good correlation lies between the element reactivity and the atomic mass.
The atomic number is equal to the number of the protons in the atomic nucleus.
Atomic weight in atomic mass units = the number of protons + the number of neutrons. The number of protons is your atomic number. Subtract that from the atomic weight for the number of neutrons.
this elemnt has an atomic number that is double the atomic number of silicon?
An isotope is identified by atomic number (element number or name), by mass number, and by atomic weight. The mass numberfor an isotope is listed as a leading superscript such as 29Si, which in this example is silicon containing 14 protons and 15 neutrons (a rarer but stable isotope of the element). Similarly the atomic weight is indicated by a superscript such as U235 , an isotope of uranium having 92 protons and 143 neutrons.The actual atomic weight is often expressed as a decimal number corresponding to the mass of the atom in "atomic units", where a proton is about 1.0072, a neutron 1.0086, and an electron about .00055 atomic units.
Subtract the atomic number from the atomic weight.