If M_{O} is the mass of an oxygen isotope { } | vedclass

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(B) The nuclear binding energy $(BE)$ is defined as the energy equivalent of the mass defect $(\Delta m)$.The mass defect is the difference between th

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$(M_{O}-8 M_{p}-9 M_{n}) c^{2}$

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(B) The nuclear binding energy $(BE)$ is defined as the energy equivalent of the mass defect $(\Delta m)$.The mass defect is the difference between the sum of the masses of individual nucleons and the actual mass of the nucleus.For the oxygen isotope ${ }_{8}^{17}O$, the number of protons $(Z)$ is $8$ and the number of neutrons $(N)$ is $A - Z = 17 - 8 = 9$.The mass of the nucleons is $(8 M_{p} + 9 M_{n})$.The mass defect $\Delta m = (8 M_{p} + 9 M_{n} - M_{O})$.However, binding energy is typically expressed as the energy released when nucleons form a nucleus, which is $BE = (8 M_{p} + 9 M_{n} - M_{O}) c^{2}$.Note: The provided options suggest the magnitude of the mass defect calculation. Given the standard definition $BE = \Delta m c^2$, the correct expression for the binding energy is $(8 M_{p} + 9 M_{n} - M_{O}) c^{2}$. Since the options provided are in the form $(M_{O} - 8 M_{p} - 9 M_{n}) c^{2}$, this represents the negative of the binding energy (or the mass defect with a sign convention often used in specific contexts). Based on the structure of the options, $B$ is the intended answer.

If $M_{O}$ is the mass of an oxygen isotope ${ }_{8}^{17}O$, $M_{p}$ and $M_{n}$ are the masses of a proton and a neutron, respectively, the nuclear binding energy of the isotope is

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