Final answer:
An isotope with 23 protons and 33 neutrons is expected to exist as a stable isotope of vanadium, given its neutron-to-proton ratio which falls within the typical range of stability for elements with that atomic mass.
Step-by-step explanation:
Yes, you would expect to find an isotope with 23 protons and 33 neutrons. This isotope would be an isotope of vanadium (V), which has an atomic number of 23 and, with 33 neutrons, it would have a mass number of 56 (23 protons + 33 neutrons = 56). The stability of an isotope is determined by its neutron-to-proton ratio and whether it falls within the band of stability. For lighter elements, such as vanadium, a neutron-to-proton ratio close to 1:1 is usually stable, whereas heavier elements require a higher ratio for stability. With 33 neutrons for 23 protons, this isotope of vanadium has a ratio of about 1.43, which is within the range that can be stable for elements of this atomic mass.