0
What is weighted average atomic number
Wiki User
∙ 9y ago
Add your answer:
Earn +20 pts
The average atomic mass of an element is the average of the atomic masses of its?
The average atomic mass of an element is the average of the atomic masses of its isotopes (that is a weighted average). You have to take into account the abundance of each isotope when they do your averaging.
How do the decimal places on the atomic masses of elements realate to isotopes?
The atomic mass of an element is the weighted average of masses of the isotopes of the element, weighted in proportion to their abundance.
Why atomic mass of an atom is defined as relative atomic mass?
It is calculated as the ratio of the mass of one atom of an element to one twelfth of the mass of an atom of carbon-12. In fact, the weighted average of the mass of an atom of an element - weighted according to its isotopic abundance.
Atomic mass used in a sentence?
The atomic mass of an element is the weighted average of the masses of all the stable isotopes of the element (if it has any), weighted by the natural occurrence levels of the isotopes in the elements as found on earth or in the atmosphere.
Atomic mass is equivalent to the number of?
The atomic mass is the mass of an atom of that element in AMUs. (Atomic Mass Units)The atomic number, however, is equivalent to the number of protons in an atom of that element.The mass number of an atom is the total number of protons and neutrons in the nucleus of an atom. This is therefore always a whole number. The relative atomic mass of an element is the weighted average of the masses of the isotopes relative to 1/12 of the mass of a carbon-12 atom.It is a weighted average as it takes into account the relative abundances of the different isotopes (atoms of the same element but with different numbers of neutrons) of an element. This number is found in the periodic table.For example chlorine has two isotopes, 35Cl and 37Cl, in the approximate ratio of 3 atoms of 35Cl to 1 atom of 37Cl.The number of protons and neutrons in a 35Cl atom must add up to 35, the mass number. The relative atomic mass of chlorine takes into account both isotopes and is therefore 35.5.
Weighted average mass of the mixture of its isotopes?
Average atomic mass I think.
What is the weighted average atomic mass of bromine?
79.9173125
What is the average atomic mass compared to atomic mass?
Atomic mass is the number of protons and neutrons in an atom.
Is the mass and atomic mass the same?
No. The atomic weight is the number on the Periodic Table and is a weighted average of the atomic masses.
An average of the masses of all the naturallly occurring isotopes of an element?
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 atomic mass of an element is defined as the weighted average mass of that element's?
For the chemical elements the correct expression is atomic weight.This value is the weighted average mass of the natural isotopes of this element.
What is the weighted average mass of all the know isotopes for an element?
It is its Atomic Mass and why atomic mass is frequently not a whole number.
The average atomic mass of an element is the average of the atomic masses of its?
The average atomic mass of an element is the average of the atomic masses of its isotopes (that is a weighted average). You have to take into account the abundance of each isotope when they do your averaging.
The weighted average of the masses of all the naturally occurring isotopes of an element is the what?
Atomic weight or atomic mass used in stoichiometric calculations.
Why is the atomic mass of sulfur listed on the periodic table not a whole number?
The atomic mass given on the periodic table is a weighted average of all the isotopes, weighted by abundance of each isotope
Why is a weighted average required for calculating atomic mass?
Isotopes - that same element with a different atomic weight.
How is the atomic mass for chlorine related to isotopes for that atom?
The average atomic mass is weighted by the most common isotopes and their relative abundance.
