Chromium ( Cr ) has four naturally occurring stable isotopes \( { }^{50} \mathrm{Cr},{ }^{52} \mathrm{Cr},{ }^{53} \mathrm{Cr} \) and \( { }^{54} \mathrm{Cr} \). Which isotope do you expect to be most abundant isotope? (You should not need to do any calculation for this problem).

To determine which isotope of chromium is expected to be the most abundant, we can consider the stability and the mass numbers of the isotopes. The isotopes of chromium are: - \( {}^{50} \mathrm{Cr} \) - \( {}^{52} \mathrm{Cr} \) - \( {}^{53} \mathrm{Cr} \) - \( {}^{54} \mathrm{Cr} \) Generally, isotopes with mass numbers closer to the average atomic mass of the element tend to be more abundant. The average atomic mass of chromium is approximately 51.9961 amu, which is very close to \( {}^{52} \mathrm{Cr} \). Since \( {}^{52} \mathrm{Cr} \) has a mass number of 52, which is closest to the average atomic mass of chromium, we can expect that \( {}^{52} \mathrm{Cr} \) is the most abundant isotope among the naturally occurring stable isotopes of chromium.