In each of the following pairs, choose the species with the larger radius.
1) S^4+ or S^2+
2) S or S^2-
I answered this below.
So it's S^2+ and S^2-, right?
To determine which species in each pair has the larger radius, we need to compare their electronic configurations, specifically looking at the number of electrons and their arrangement in different orbitals.
1) S^4+ or S^2+
To compare the radii of S^4+ and S^2+, we need to consider their electron configurations.
Sulfur (S) has an atomic number of 16, and its ground state electron configuration is 1s^2 2s^2 2p^6 3s^2 3p^4.
S^2+ means that two electrons have been removed from the 3p^4 subshell. So, the electron configuration of S^2+ would be 1s^2 2s^2 2p^6 3s^2.
S^4+ means that four electrons have been removed from the 3p^4 subshell. So, the electron configuration of S^4+ would be 1s^2 2s^2 2p^6.
By comparing the electron configurations, we can see that S^2+ has more electrons than S^4+. Electrons occupy different energy levels and subshells, contributing to the size of the atom. Therefore, S^2+ will have a larger radius compared to S^4+.
2) S or S^2-
To compare the radii of S and S^2-, we need to consider their electron configurations.
Again, sulfur (S) has an atomic number of 16, and its ground state electron configuration is 1s^2 2s^2 2p^6 3s^2 3p^4.
S^2- means that two additional electrons have been added to the 3p subshell. So, the electron configuration of S^2- would be 1s^2 2s^2 2p^6 3s^2 3p^6.
By comparing the electron configurations, we can see that S^2- has more electrons than S. Again, more electrons typically result in a larger atomic radius. Therefore, S^2- will have a larger radius compared to S.