Question

For each atom in the table below, write down the subshell from which an electron would have to be removed to make a + 1 cation, and the subshell to which an electron would have to be added to make a - 1 anion.

Answer 1

Answer is in attachment :)

Step-by-step explanation:

A +1 cation is formed when an electron is removed from an atom, usually from the valence shell or outermost energy level.

Conversely, a -1 anion is formed when an electron is added to an atom, typically to the outermost valence shell.

Hydrogen (H) has only one electron in the 1s subshell. Removing this electron forms a +1 cation (H+). Adding an electron to this subshell forms a -1 anion (H-).

Tin (Sn) is a part of the p-block of the periodic table, and its valence electron is in the 5p subshell. So, to form a +1 cation (Sn+), an electron would be removed from the 5p subshell. To form a -1 anion (Sn-), an electron would be added to the 5p subshell.

Strontium (Sr) is an alkaline earth metal, and its valence electrons occupy the 5s subshell. Therefore, to form a +1 cation (Sr+), an electron would be removed from the 5s subshell. To form a -1 anion (Sr-), an electron would be added to the 5s subshell.

Argon (Ar) is a noble gas with a stable electron configuration. Its outermost electrons are in the 3p subshell, so that's where an electron would be removed to form a +1 cation (Ar+). However, noble gases are less likely to form cations because they already have a full valence shell. If an electron were to be added to form a -1 anion (Ar-), it would go into the next available subshell, which is the 4s subshell.

Hope this helps you out! :)