Final answer:
To determine which species has the smallest particle size, one must evaluate the atomic or ionic radii, which are affected by the number of protons in the nucleus and the number of electron shells in the species. The exact answer depends on the specific options given, which are not provided in this scenario. Generally, smaller atomic or ionic radii are associated with a higher nuclear charge and fewer electron shells.
Step-by-step explanation:
The question concerns the comparison of atomic or ionic size, a concept important in the study of chemistry. To find the species with the smallest particle size, one must consider the number of protons in the nucleus and the number of electronic shells, as these factors directly influence atomic and ionic radii. According to the given options, we're looking for the species with the highest nuclear charge and the fewest number of electron shells. Generally, when comparing atomic radii, an atom with more protons (higher nuclear charge) pulls electrons closer to the nucleus, resulting in a smaller radius. Additionally, removing electrons (forming cations) typically decreases size due to reduced electron-electron repulsion, while adding electrons to form anions increases size.
Without the actual options for the species in question, it's not possible to definitively answer which species is the smallest. However, if you look at periodic trends, generally, as you move across a period from left to right, atomic size decreases due to an increase in nuclear charge, causing stronger attraction of electrons towards the nucleus. Conversely, atomic size typically increases as you move down a group because additional electron shells are added. Thus, a smaller atomic or ionic radii is generally found in elements with a higher effective nuclear charge and fewer electron shells.