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The general representation of an element is:\(_Z^AX\), where \(Z\)is the atomic number of element and A is the mass number.

Atomic number of element is the number of protons and it is equal to the number of electrons in an atom.

Mass number is the total number of protons and neutrons in an atom.

In this case we have isotopes, which are elements with the same number of protons but they have different number of neutrons. That means they will have the same atomic number as main element, but they have different mass number.

For this task we have mass numbers of elements but do not have an atomic number, which we can find in the periodic table.

We have oxygen-14. And if we look at the periodic table we can see that atomic number of \(O\)is \(8.\)

The nuclide form is: \(_8^{14}O\).

The given isotope is copper-70. The atomic number of copper is 29. The nuc

The nuclide form is: \(_{29}^{70}{\rm{Cu}}\).

The given isotope is tantalum-175. The atomic number of \(Ta\)is \(73.\)

The nuclide form is: \(_{73}^{175}{\rm{Ta}}\).

The given isotope is francium-217. The atomic number of \(Fr\)is \(87.\)

The nuclide form is:\(_{87}^{217}{\rm{Fr}}\).