The atomic weight that is listed on the Periodic Table for each element is the weighted average of the atomic masses of an element's naturally occurring isotopes. So you are describing atomic weight as it is used on the periodic table.
The weighted average for all isotopes that occur in nature for an element is its atomic weight listed on the Periodic Table of the elements.
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 two notations represent atoms that are isotopes of the same element is 121 Sn and 119 Sn. The atomic mass of an element is defined as the weighted average mass of that elements naturally occurring isotopes.
Yes, weighted by how often the isotopes are found in nature.
Silver has 2 different naturally occurring isotopes:Silver-107 (51.35%) - 60 neutrons - mass 106.9389 amuSilver-109 (48.65%) - 62 neutrons - mass 108.9393 amuThe masses in amu differ from the mass number of the isotope because of the "mass defect, which in silver is slightly negative as is typical of elements in the middle of the binding energy curve. Also the mass of Silver on the periodic table of 107.912 amu is a weighted average the two isotopes masses. This is the number the chemist wants as he rarely cares about isotopes. If you want to count neutrons, you need a table of the isotopes of the elements, not just a periodic table. This is available in nuclear engineering, health physics, etc. texts.
The known weighted-averagemass of all the naturally occurring* isotopes for an element is the atomic mass of the element.____________________*This is not the same as "all the known isotopes", becausemost elements have known isotopes that are not naturally occurring.
The known weighted-averagemass of all the naturally occurring* isotopes for an element is the atomic mass of the element.____________________*This is not the same as "all the known isotopes", becausemost elements have known isotopes that are not naturally occurring.
The known weighted-averagemass of all the naturally occurring* isotopes for an element is the atomic mass of the element.____________________*This is not the same as "all the known isotopes", becausemost elements have known isotopes that are not naturally occurring.
For the chemical elements the correct expression is atomic weight.This value is the weighted average mass of the natural isotopes of this element.
The mean 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 weighted average of all of the natural occuring isotopes for a particular element is called its Atomic Weight (or Relative Atomic Mass)
The atomic weight of the element (syn.: mass number).
The answer is the atomic weight of the original element: It's the number on the top left of each element square of the Periodic Table.
Atomic masses are a weighted average of the naturally occurring isotopes.
This is the weighted average neutron number for the naturally occurring isotopes of nickel, which has the atomic number 28 and the gram-atomic mass of 58.69. In an individual isotope, the neutron number is always the isotopic atomic mass number minus the atomic number, and the same principle applies to the weighted average neutron number for the naturally occurring isotopes of an element.
The atomic weight for each element on the periodic table represents a weighted average of the masses of all naturally occurring isotopes of an element. Because of this, the elements do not have whole-number atomic weights. An exception is the atomic weight for some elements written inside parentheses. These elements do not have stable isotopes and the atomic weight listed is the atomic weight for the longest lived isotope.