Yes, isotopes of an element have the same number of protons but different numbers of neutrons, leading to variations in Atomic Mass. This is why the atomic mass on the Periodic Table is often listed as a range for an element.
Number of neutrons = Atomic mass of an isotope - Atomic number of the element The atomic number of hassium is 108; each isotope of an element has a different number of neutrons and a different atomic mass.
average atomic massof an element=(Atomic mass of first isotope X % of that isotope) + (Atomic mass of second isotope X % of the second isotope)
The two main factors in determining the average atomic mass of an element are:the isotopic composition of the element (the fraction of each isotope)the atomic mass of each isotope
An isotope is a variant of an element with a different number of neutrons in its nucleus. The mass number of an isotope is the sum of its protons and neutrons in the nucleus. Therefore, the mass number is specific to each isotope of an element.
The mass number for a particular isotope of an element is a precise value. The average atomic mass for an element is the value you would measure for that element given all the isotopes it has and their abundance in the sample.
Because each isotope of an element has a mass different from any other isotope of the same element, and the atomic mass of an element is an average, weighted by the proportion of each isotope, in the naturally occurring element.
isotope
Number of neutrons = Atomic mass of an isotope - Atomic number of the element The atomic number of hassium is 108; each isotope of an element has a different number of neutrons and a different atomic mass.
average atomic massof an element=(Atomic mass of first isotope X % of that isotope) + (Atomic mass of second isotope X % of the second isotope)
The two main factors in determining the average atomic mass of an element are:the isotopic composition of the element (the fraction of each isotope)the atomic mass of each isotope
Each isotope of an element has a different number of neutrons: Atomic mass of the isotope - Atomic number = Number of neutrons
An isotope is a variant of an element with a different number of neutrons in its nucleus. The mass number of an isotope is the sum of its protons and neutrons in the nucleus. Therefore, the mass number is specific to each isotope of an element.
The mass number for a particular isotope of an element is a precise value. The average atomic mass for an element is the value you would measure for that element given all the isotopes it has and their abundance in the sample.
The number of neutrons in the nucleus is different in each isotope of an element. Isotopes of an element have the same number of protons (atomic number) but different numbers of neutrons, leading to variations in atomic mass.
The atomic mass number of oxygen is 16.0. --------- The mass number is the sum of neutrons and protons in the atomic nucleus and is different for each isotope of any element. For example the isotope oxygen-16 has the mass number 16. After IUPAC Tables from 2009 the atomic weight of oxygen is [15,99903; 15,99977]. The conventional (abridged) atomic weight is 15.999 amu.
The mass number is the sum of neutrons and protons in the atomic nucleus and is different for each isotope of any element. For example the isotope oxygen-16 has the mass number 16.
Yes, the atomic mass of an element takes into account the relative abundance of each isotope of that element. This is because atomic mass is the weighted average of the masses of all isotopes of an element based on their natural abundance.