The difference between the mass number of an isotope and its atomic number is number of neutrons.
<h3>What is atomic mass? </h3>
Atomic mass is defined as the sum of number of protons and number of neutrons of an element.
Atomic mass is represented by A.
<h3>What is Atomic number?</h3>
Atomic number is defined as the number of electron in an element.
Atomic number is represented by Z.
<h3>What is Isotopes? </h3>
Isotopes are the element which have same atomic number but have different atomic mass.
Number of proton is equal to number of electrons.
Proton is positively charged, electrons are negativity charge while neutrons are neutral in nature.
Proton and neutrons are present in the nucleus of an element. On the other hand, electron revolves around the nucleus.
For example:
The atomic mass of¹⁶₈O is 16, while of ¹⁷₈O is 17.
Neutrons = atomic mass - atomic number
Neutrons of ¹⁶₈O = 16-8 = 8
Neutrons of ¹⁷₈O = 17-8 = 9
So, they have different atomic mass and number of neutrons.
Thus, we concluded that the difference between the mass number of an isotope and its atomic number is number of neutrons.
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