Mass spectrometer. (and centrifuges)
The mass number for a particular isotope of an element is a precise value. The average atomic mass for an element is the value you would measure for that element given all the isotopes it has and their abundance in the sample.
The average atomic mass of an element would be closer to a whole number if there were few to no electrons. This means having little to no electrons in the element's isotopes.
Isotopes of an element are the same in that they are both forms of the same element. All carbon isotopes, for example, are forms of the carbon atom. Each isotope will possess the same number of protons and electrons (equivalent to the element's atomic number). However, isotopes of an element possess different numbers of neutrons, altering their atomic mass. As such, if you know the atomic mass (or weight) of a given isotope, you already know the number of protons and electrons. Using the measured mass of the proton (around 1.007 amu) and the measured mass of the electron (around 0.00055 amu), you can determine the remaining mass from the neutrons and, consequently, the number of neutrons.
mass number = number of protons + number of neutrons DIFFERENT FROM ATOMIC MASS atomic mass = weighted average of all the isotopes of that element
The atomic number is the number of protons in an atom. This number is fixed and determines what element that atom is. The Atomic Mass is the mass of an atom and is roughly equivalent to the number of protons plus the average number of neutrons that atoms of that particular element.
The element's average atomic mass.
The atomic mass of an element is the average of all the isotopes of that element that exist on this earth, either naturally or artificially. An isotope is an atom that differs in the number of neutrons that it would normally have (which is usually the same as the number of protons it has, except in the case of hydrogen).
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.
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.
the average mass numbers of the isotopes of an element