The atomic weight of an element is a number that takes into account the natural distribution of the isotopes of that element.
The atomic mass of an element is the average of its isotopes, weighted by abundance in nature.
The average atomic mass takes into account the different isotopes of an element and their relative abundance, while the mass of an individual atom is specific to that particular isotope. The average atomic mass is a weighted average based on all isotopes present in a sample, providing a more accurate representation of the element's mass in nature.
The atomic mass of an element is the average mass of an element's isotopes, weighted by their natural abundance. It is expressed in atomic mass units (u) and is often close to the mass number of the most abundant isotope of the element.
Isotopes have a different amount of Neutrons. The atomic mass is the sum of Protons and Neutrons. Therefore having a different number of Neutrons makes the atomic mass greater. Or vice versa. Boom. Solved.
The atomic mass of an element is the weighted average of the masses of its isotopes, taking into account their abundance. If the atomic mass of an element is 197.97, it represents the average mass of all naturally occurring isotopes of that element.
the average mass numbers of the isotopes of an element
average atomis mass
the atomic mass
All of the isotopes in an element's atomic masses divided by the amount of isotopes there are is the weighted-average mass of the mixture of an elements isotopes.
The atomic mass of an element is the average of its isotopes, weighted by abundance in nature.
The atomic mass of an element is the average of its isotopes, weighted by abundance in nature.
The average of all the naturally occurring isotopes of a particular element are an element's atomic Mass.
The weighted-average mass of all the known isotopes for an element is called the atomic weight or atomic mass. It is calculated by taking into account the abundance of each isotope and its mass to determine the average mass of all isotopes present in nature for that element.
the Atomic Mass
The average atomic mass takes into account the different isotopes of an element and their relative abundance, while the mass of an individual atom is specific to that particular isotope. The average atomic mass is a weighted average based on all isotopes present in a sample, providing a more accurate representation of the element's mass in nature.
It is called the Relative Atomic Mass.
The atomic mass of an element is the average mass of an element's isotopes, weighted by their natural abundance. It is expressed in atomic mass units (u) and is often close to the mass number of the most abundant isotope of the element.