That would be Carbon (C).
Which has a designated mass of 12.
The total number of neutrons in an atom is known as its atomic mass. The sum of all the atomic weights of isotopes of a particular element is known as an element's atomic weight. Atomic weights are decimal numbers for this reason.
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.
No they are all different and even some atoms of the same element have different weights
Yes, the atomic mass of an element takes into account the relative abundance of each isotope of that element. This is because atomic mass is the weighted average of the masses of all isotopes of an element based on their natural abundance.
Atoms with the same atomic number are all atoms of the same element. However, if the atoms have different molecular weights, they are isotopes of the same element.
The relative abundance of each isotope of an element is used to determine its atomic mass. This is the weighted average of all naturally occurring isotopes.
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.
Atomic weight or atomic mass used in stoichiometric calculations.
The weighted average of all of the natural occuring isotopes for a particular element is called its Atomic Weight (or Relative Atomic Mass)
The weighted average of all of the natural occuring isotopes for a particular element is called its Atomic Weight (or Relative Atomic Mass)
The Atomic Mass number of an element is the sum of the protons and neutrons in the nucleus of an atom of that element.The relative atomic mass is the average atomic mass number of all the known isotopes of an element.
the average atomic mass is computed by summing all isotopic weights of the isotopes of that element and then dividing this by the the total number of isotopes of that element (note that isotopic mass is exactly the same as atomic weight, except for isotopes).