Atomic number equals the number of protons, the (atomic) mass number equals the sum of (the number of) protons and neutrons of the same element.
The answer is: they're differing in the number of neutrons
(Mathematically: Where A = p and M = p + n, the difference in A and M is n)
Yes; isotopes of the same element have the same atomic number but differ in their atomic masses.
We can find atomic mass and mass number in chemical elements. Atomic mass is about weight of the atom. Mass number is about total of neutrons and protons.
The masses and relative abundances of all naturally occurring isotopes of the element are required to calculate average atomic mass of the element.
Two isotopes of an element have the same atomic number (number of protons) but have different mass numbers (sum of protons and neutrons). This means that they will differ in the number of neutrons despite being the same element.
Mendeleev's periodic table was based on the atomic masses of elements. However, this was not effective when isotopes were discovered. An isotope of an element is defined as the element having the same atomic number but varying mass numbers. So, mass numbers weren't constant and hence, a better characteristic was chosen -atomic number. Atomic number of any element was a characteristic of a particular element. Hence atomic numbers were taken as the basis of classification instead of atomic masses.
Yes; isotopes of the same element have the same atomic number but differ in their atomic masses.
the Atomic Mass
We can find atomic mass and mass number in chemical elements. Atomic mass is about weight of the atom. Mass number is about total of neutrons and protons.
the atomic mass
The masses and relative abundances of all naturally occurring isotopes of the element are required to calculate average atomic mass of the element.
Its the average of the weight of the different isotopes of that element.
The different mass numbers are due to different numbers of neutrons.
Two isotopes of an element have the same atomic number (number of protons) but have different mass numbers (sum of protons and neutrons). This means that they will differ in the number of neutrons despite being the same element.
Neon is a non meta element. Atomic mass of it is 20 Atomic number of it is1 180.
Mendeleev's periodic table was based on the atomic masses of elements. However, this was not effective when isotopes were discovered. An isotope of an element is defined as the element having the same atomic number but varying mass numbers. So, mass numbers weren't constant and hence, a better characteristic was chosen -atomic number. Atomic number of any element was a characteristic of a particular element. Hence atomic numbers were taken as the basis of classification instead of atomic masses.
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.
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.