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(C) Isotopes are atoms of the same element that have the same number of protons and electrons but a different number of neutrons.For Uranium $(U)$,the

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Contain same number of protons and electrons,but $^{238}U$ contains $3$ more neutrons than $^{235}U$.

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(C) Isotopes are atoms of the same element that have the same number of protons and electrons but a different number of neutrons.For Uranium $(U)$,the atomic number $(Z)$ is $92$,which means both $^{235}U$ and $^{238}U$ have $92$ protons and $92$ electrons.The number of neutrons $(N)$ is calculated as $N = A - Z$,where $A$ is the mass number.For $^{238}U$: $N = 238 - 92 = 146$ neutrons.For $^{235}U$: $N = 235 - 92 = 143$ neutrons.Comparing the two,$^{238}U$ has $146 - 143 = 3$ more neutrons than $^{235}U$.

Which of the following is true for a sample of isotopes containing $^{235}U$ and $^{238}U$?

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