Question

how do these isotopes differ in the subatomic particles present in them​

Answer 1

Answer:

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Explanation:

As mentioned above, all atoms of a given element have the same number of protons (atomic number), however, different atoms of a given element may have different numbers of neutrons. ... These isotopes differ in the number of neutrons in their nuclei, but all three have one proton and one electron.

Answer 2

Since the mass number is the number of protons plus the number of neutrons and the atomic number is the number of protons, you can find the number of neutrons by simply subtracting the atomic number from the mass number. As an example, suppose we have an element with an atomic number of 8 and a mass number of 17. From this information you can deduce that this element has 8 protons, 8 electrons and 9 neutrons (17-8=9). Now let me throw you a curve ball. As mentioned above, all atoms of a given element have the same number of protons (atomic number), however, different atoms of a given element may have different numbers of neutrons. We say that these are different isotopes of the element. For example, there are three isotopes of hydrogen. The most common isotope comprising 99.98% of all hydrogen atoms has a mass number of 1. It therefore is composed of 1 proton, no neutrons, and one electron. The other less abundant isotopes of hydrogen have mass numbers of 2 and 3, respectively. These isotopes differ in the number of neutrons in their nuclei, but all three have one proton and one electron. In reality there are naturally occurring isotopes of every element, each having its own unique mass number. In chemical notation the mass number for a given isotope is expressed as a superscript preceding the symbol for the element. The three isotopes for hydrogen would be expressed as 1H, 2H, and 3H.