Yes; isotopes of the same element have the same atomic number but differ in their atomic masses.
Yes, isotopes of an element do have different Atomic Mass numbers. Isotopes are different atoms of the same element with the same atomic number but different mass numbers.
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 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.
Calculation of the atomic weight of an element having many isotopes:ia - atomic mass of the isotope a x percent concentration of the isotope in the elementib - atomic mass of the isotope b x percent concentration of the isotope in the elementic - atomic mass of the isotope c x percent concentration of the isotope in the element...........................................................................................................................iz - mass of the isotope z x percent concentration of the isotope in the elementMake the sum: I = ia + ib + ic + ..... izThe atomic weight of the element is: I/100 (the term weight is recommended by IUPAC in this case).
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
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)
Each isotope of an element has a different number of neutrons: Atomic mass of the isotope - Atomic number = Number of neutrons
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.
Calculation of the atomic weight of an element having many isotopes:ia - atomic mass of the isotope a x percent concentration of the isotope in the elementib - atomic mass of the isotope b x percent concentration of the isotope in the elementic - atomic mass of the isotope c x percent concentration of the isotope in the element...........................................................................................................................iz - mass of the isotope z x percent concentration of the isotope in the elementMake the sum: I = ia + ib + ic + ..... izThe atomic weight of the element is: I/100 (the term weight is recommended by IUPAC in this case).
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.
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
Yes. The gram atomic mass of each element is the sum of the products of each stable isotope's isotopic fraction multiplied by the mass of that isotope.
If a sample of an element contains atoms of different mass numbers, the name of the element followed by a hyphen and the mass number is the name of an isotope of the element.