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.)
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.)
It depends on their relative abundance in the universe.
Isotopes contain a different number of neutrons.
It is important to use a weighted average because different isotopes of an element have different atomic masses due to the presence of different numbers of neutrons. The abundance of each isotope also varies, meaning some isotopes are more common than others. By using a weighted average, the more abundant isotopes have a greater contribution to the overall average atomic mass of the element, providing a more accurate representation.
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)
The atomic mass of chlorine is a weighted average of the masses of all its naturally occurring isotopes, taking into account their abundance. Chlorine has two main isotopes, chlorine-35 (with an atomic mass of approximately 34.97) and chlorine-37 (with an atomic mass of approximately 36.97). The 0.5 difference in the atomic mass comes from the relative abundance of these isotopes in nature.
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.
Isotopes contain a different number of neutrons.
It is important to use a weighted average because different isotopes of an element have different atomic masses due to the presence of different numbers of neutrons. The abundance of each isotope also varies, meaning some isotopes are more common than others. By using a weighted average, the more abundant isotopes have a greater contribution to the overall average atomic mass of the element, providing a more accurate representation.
Bromine's average eight is 79.904 is the answer in my reference, with more than 20 isotopes.
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)
The atomic mass of chlorine is a weighted average of the masses of all its naturally occurring isotopes, taking into account their abundance. Chlorine has two main isotopes, chlorine-35 (with an atomic mass of approximately 34.97) and chlorine-37 (with an atomic mass of approximately 36.97). The 0.5 difference in the atomic mass comes from the relative abundance of these isotopes in nature.
More important than others.
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.
The underlined word "more heavily" is in the comparative degree. It is comparing the sleeping heaviness of some people to others.
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.
comparative
You have what's known as a weighted average. The 80 score is weighted more heavily than the 91 score, so the weighted average will be closer to 80 than a non-weighted average. 0.85 x 80 = 68 0.15 x 91 = 13.65 68 + 13.65 = 81.65
Some isotypes are more stable than others. Decay occurs because of instability in isotopes, so stable isotopes do not undergo radioactive decay.