The atomic number (denoted by ‘Z’) uniquely identifies each element and determines its chemical properties. Elements are defined by the number of protons they possess, which is reflected in their atomic number.
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The mass number contributes to an atom’s stability, with isotopes having different mass numbers due to varying numbers of neutrons. Some isotopes may be more stable than others, depending on the balance between protons and neutrons in the nucleus.
The notation for an atom includes its atomic number (number of protons), mass number (sum of protons and neutrons), and the symbol of the element. For example, carbon-12 is represented as 12/6 C, where 6 is the atomic number, 12 ...
The mass number of an atom with 6 protons and 6 neutrons is 12.
The mass number (denoted by ‘A’) is calculated as the sum of the total number of protons and neutrons present in the nucleus of an atom. It represents the atom’s total mass.