To determine the correct order of atoms from highest to lowest ionization energy, we need to understand the periodic trends of ionization energy in the periodic table. Ionization energy generally increases across a period (from left to right) and decreases down a group (from top to bottom).
Let's analyze the given options:
Option A: [tex]$Mg > Al > S > Cl$[/tex]
In a period, ionization energy increases from left to right. Given that Mg, Al, S, and Cl are all in the same period (Period 3), we expect their ionization energies to increase from Mg to Cl. Therefore, Mg should have the lowest ionization energy and Cl the highest. This option doesn’t follow the trend as it incorrectly places Mg and Al before S and Cl.
Option B: [tex]$Cl > Al > S > Mg$[/tex]
According to the periodic table, Cl is to the right of S, Al, and Mg, so it should have the highest ionization energy. However, between S and Al, S should have a higher ionization energy than Al since S is further right in the period. This option incorrectly places Al before S.
Option C: [tex]$Cl > S > Al > Mg$[/tex]
This option correctly places Cl (furthest right in the period) with the highest ionization energy, followed by S, then Al, and finally Mg. This follows the expected trend across a period: ionization energy increases from Mg to Cl.
Option D: [tex]$Mg > S > Al > Cl$[/tex]
This option is not correct because Mg should have the lowest ionization energy, not the highest. Additionally, Al should be placed before S, not after.
Therefore, considering the trends in ionization energy across the period, the correct option is:
Option C: [tex]$Cl > S > Al > Mg$[/tex]
In conclusion, the correct order from highest to lowest ionization energy for the given atoms is: Cl > S > Al > Mg, which corresponds to Option C.
