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The type of element is decided by the number of protons in it's nucleus. Number of neutrons are either equal or more than number of protons. Mass of proton and neutron is almost equal and that of electron is almost negligible as compared to both of others. As number of neutrons differ, mass of the elements also differ. Though they have 'same' chemical properties. Such atoms with different mass are called Isotopes. If the number of neutron is more, then such Isotopes are having more mass (or weight.)
What else can I help you with?
What are some isotopes more heavily weighted than other?
Isotopes contain a different number of neutrons.
Why is it important to use a weighted average when determining the average atomic mass of your element?
The majority of chemical elements have one or more natural isotopes; each isotope has a different mass and concentration. A weighted average atomic weight is unavoidable for a correct evaluation.Don't use the expression atomic maas - this in only for isotopes. For chemical elements IUPAC recommend atomic weight.
Weighted average mass of the mixture of its isotopes?
The weighted average mass of a mixture of isotopes is calculated by multiplying the mass of each isotope by its natural abundance, and then summing these values together. This gives a more accurate representation of the overall mass of the isotopes in the mixture, taking into account their relative abundances.
Why do elements which exists as isotopes have fractional atomic mass?
Each isotope of an element has a different Atomic Mass, so an average is taken of all the isotopes, but the average is weighted because the natural abundance (%) of each isotope is factored in. If hydrogen-1 is much more abundant than deuterium and tritium, then the weighted average will be closer to 1 than 2 or 3 but not a whole number. The following equation shows how percent abundance factors into the weighted average. (atomic mass A)(X% abundance) + (atomic mass B)(Y% abundance)...=(weighted average of all isotopes of the element)(100% abundance)
Is the atomic mass used for the mass of an element which has isotopes?
Yes, it must be used as all elements have one or more isotopes and all elements have an atomic mass.
What are some isotopes more heavily weighted than other?
Isotopes contain a different number of neutrons.
Why is it important to use a weighted average when determining the average atomic mass of your element?
The majority of chemical elements have one or more natural isotopes; each isotope has a different mass and concentration. A weighted average atomic weight is unavoidable for a correct evaluation.Don't use the expression atomic maas - this in only for isotopes. For chemical elements IUPAC recommend atomic weight.
Weighted average mass of the mixture of its isotopes?
The weighted average mass of a mixture of isotopes is calculated by multiplying the mass of each isotope by its natural abundance, and then summing these values together. This gives a more accurate representation of the overall mass of the isotopes in the mixture, taking into account their relative abundances.
Why do elements which exists as isotopes have fractional atomic mass?
Each isotope of an element has a different Atomic Mass, so an average is taken of all the isotopes, but the average is weighted because the natural abundance (%) of each isotope is factored in. If hydrogen-1 is much more abundant than deuterium and tritium, then the weighted average will be closer to 1 than 2 or 3 but not a whole number. The following equation shows how percent abundance factors into the weighted average. (atomic mass A)(X% abundance) + (atomic mass B)(Y% abundance)...=(weighted average of all isotopes of the element)(100% abundance)
What is the degree of comprison for the underlined words some people sleep more heavily than others?
"More heavily" is a comparative. "Most heavily" would be a superlative.
Is the atomic mass used for the mass of an element which has isotopes?
Yes, it must be used as all elements have one or more isotopes and all elements have an atomic mass.
Where does the 0.5 in chlorine's atomic mass come from?
There are different isotopes of the element. Isotopes are atoms of an element that have different amounts of protons, so the isotopes with more protons weigh more because there is more mass in the atom. Some isotopes are more common than others, and the atomic mass is a weighted AVERAGE of all the isotopes of that element. On most elements there is a large difference between the most common and lesser common isotopes, but chlorine has 2 isotopes that are very close. So the average ends up between the two numbers. The actual weight of 1 atom will never be something.5 because protons and neutrons weigh 1amu and electrons weigh 0. But in most cases the sample of a chemical you use will be a mixture of the isotopes, so the .5 weight will be correct.
When a weighted average is taken this means that some numbers are what?
More important than others.
What is the average atomic mass compared to atomic mass?
The average atomic mass is a weighted average of the masses of all isotopes of an element, taking into account their abundance. The atomic mass listed on the periodic table is the weighted average of all naturally occurring isotopes of the element. So, they are essentially the same thing, with the average atomic mass being a more specific term.
How do you get weighted mean?
A weighted mean is when some values contribute more than others. In order to calculate weighted mean multiply each weight by its value, add those and then divide by the sum of the weights.
What is an isotope and why are atomic masses usually in decimal form?
An isotope is a variant of the atom with the same number of protons but more or fewer neutrons. The atomic mass is an average of the isotopes of the element. The average is weighted according to the relative abundance of such isotopes.
The relative abundance of each isotope of an element determines its?
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.
