Copper isotopes are not always whole numbers because the Atomic Mass of an isotope is determined by the total number of protons and neutrons in its nucleus, which can vary. Copper has two stable isotopes, copper-63 and copper-65, with atomic masses that reflect the different neutron counts. The atomic mass of naturally occurring copper is a weighted average of these isotopes, leading to a non-integer value (approximately 63.55). This average accounts for the relative abundance of each isotope in nature.
The isotopes of copper have the relative atomic masses of 63 and 65 and these are approximations. The exact values contain decimal figures.
Few elements have isotopes. their atomic mass is not a whole number.
Elements exist as isotopes in nature. So their atomic weight is not a whole number.
The average atomic mass of an element is close to a whole number when the element has nearly equal amounts of its isotopes, with atomic masses that are close to whole numbers themselves. This occurs in elements with only one stable isotope or with stable isotopes that have similar abundances.
The atomic mass of nobelium reported as a whole number is usually the average atomic mass of its isotopes, taking into account the natural abundance of each isotope. Since this average is calculated from the weighted average of the isotopes' masses, the result often appears as a whole number.
The short answer is yes. The long answer is that isotopes have different numbers of neutrons than other isotopes of the same element, so when expressing the mass of an isotope, you don't take an average; you just add the number of neutrons and the number of protons. However, that number is not entirely accurate since the mass of a proton and a neutron are very slightly different. So, if you want to be very exact, then no, the mass of an isotope is not a whole number, but it is very, very close.
The isotopes of copper have the relative atomic masses of 63 and 65 and these are approximations. The exact values contain decimal figures.
Atomic mass is the total mass of protons and neutrons in an atom, which are whole numbers. Atomic weight, on the other hand, takes into account the abundance of different isotopes of an element, which can result in a weighted average that may be a decimal number.
Mass number is the average of all the naturally occurring isotopes of that element. When calculated, this average is not a whole number.
Few elements have isotopes. their atomic mass is not a whole number.
what whole number will 8 always divide by?
Elements exist as isotopes in nature. So their atomic weight is not a whole number.
Yes, the difference of two whole numbers is always a whole number.
The average atomic mass of an element is close to a whole number when the element has nearly equal amounts of its isotopes, with atomic masses that are close to whole numbers themselves. This occurs in elements with only one stable isotope or with stable isotopes that have similar abundances.
Approximately, yes. But the mass number is an average of the masses of the isotopes of the element, weighted together according to their abundance. This averaging of different whole numbers results in the mass number not being a whole number.
yes,because in isotopes neutrons differ from normal element.
Isotopes differ from each other by having different numbers of neutrons but the same number of protons since they are only the same element if they have the same number of protons. Atomic numbers aren't whole because their mass is based of the mass of hydrogen and amu's (atomic mass units) and due to how elements are formed, minute amounts of mass are lost in order to form the nuclear bonds resulting in not whole numbers.