Which of the following has the smallest radius?

Question

BlackTom AI · Accepted Answer

We need to compare the ionic radii of species that all contain 36 electrons, so we should focus on their nuclear charges to determine which is smallest.
Option Br–: bromide ion has 36 electrons (Z = 35). Its nuclear charge is relatively low for a 36-electron species, so its electron cloud is not pulled in very tightly, yielding a larger radius than species with higher effective nuclear charge.
Option As3–: arsenide 3− ion also has 36 electrons, but its nucleus has Z = 33. With a lower nuclear charge, the electrons aren’t pulled in as tightly, leading to a relatively larger radius.
Option Se2–: selenide 2− ion similarly has 36 electrons, and Z = 34. This gives it a somewhat stronger pull than Br– and As3–, but still less than species with a higher Z, so its radius is not the smallest among these.
Option Sr2+: strontium 2+ ion has 36 electrons with Z = 38. The greater nuclear charge exerts a stronger attractive force on the same number of electrons, pulling them closer and producing the smallest radius among the listed species.
Option Rb+: rubidium ion Rb+ has 36 electrons as well, with Z = 37. Its nuclear charge is less than that of Sr2+, so its electrons are not pulled in as tightly, resulting in a larger radius than Sr2+.
In summary, for isoelectronic 36-electron species, the one with the highest nuclear charge (Sr2+) will have the smallest radius, making Sr2+ the smallest among the options.

Which of the following has the smallest radius?

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