I.E. and e config. 2023 Chemistry PDF

Chem. 11 Relationship between electron arrangement and ionization energy A graph of 1^st^ I.E. (kJ/mol) vs. Atomic number of atom 12.1 Electron Behavior - The!Mad!Scientist!  I.E.1 = Energy required to remove the 1^st^ elec...

Chem. 11 Relationship between electron arrangement and ionization energy A graph of 1^st^ I.E. (kJ/mol) vs. Atomic number of atom 12.1 Electron Behavior - The!Mad!Scientist!  I.E.1 = Energy required to remove the 1^st^ electron I.E.2 = Energy required to remove the 2^nd^ electron I.E.3 = Energy required to remove the 3^rd^ electron Electron configurations for period 3 elements ^11^Na **1s^2^ 2s^2^ 2p^6^ 3s^1^ \[Ne^10^\]**­­­­ [↑\_] 3s ^12^Mg **1s^2^ 2s^2^ 2p^6^ 3s^2^ \[Ne^10^\]**­­­­ [↑↓] 3s ^13^Al **1s^2^ 2s^2^ 2p^6^ 3s^2^ 3p^1^ \[Ne^10^\]**­­­­ [↑↓] [↑\_] \_\_\_ \_\_\_ 3s 3p ^14^Si **1s^2^ 2s^2^ 2p^6^ 3s^2^ 3p^2^ \[Ne^10^\]**­­­­ [↑↓] [↑\_\_] [↑] [\_\_\_] 3s 3p ^15^P **1s^2^ 2s^2^ 2p^6^ 3s^2^ 3p^3^ \[Ne^10^\]**­­­­ [↑↓] [↑\_\_] [↑\_\_] [↑\_\_] 3s 3p ^16^S **1s^2^ 2s^2^ 2p^6^ 3s^2^ 3p^4^ \[Ne^10^\]**­­­­ [↑↓] [↑↓] [↑\_\_] [↑\_\_] 3s 3p ^17^Cl **1s^2^ 2s^2^ 2p^6^ 3s^2^ 3p^5^ \[Ne^10^\]**­­­­ [↑↓] [↑↓] [↑↓] [↑\_\_] 3s 3p ^18^Ar **1s^2^ 2s^2^ 2p^6^ 3s^2^ 3p^6^ \[Ne^10^\]**­­­­ [↑↓] [↑↓] [↑↓] [↑↓] 3s 3p The Ionization energy gives an indication of how tightly held the electron is to an atom. Things to consider: Stable electron configurations (in decreasing order) \#1. Noble gas (full valence orbital system) Remember as you move across a period (Na to Ar), the effective nuclear charge exhibited by the protons in the nucleus increases (+ 1 proton per element) resulting in a smaller radius and increased energy required to completely remove an electron from an atom (aka Ionization energy). This trend however, is not uniform as is dependent on the orientation of the electrons in orbitals (and axes) and their proximity to each other. I.E.\#2 for Period 3 cations (+1 charge) Na^+^ \[He^2^\] [ ↑↓] [↑↓] [↑↓] [↑↓] 2s 2p Mg^+^ **\[Ne^10^\]**­­­­ [↑\_] 3s **Al^+^ \[Ne^10^\]**­­­­ [↑↓] 3s Si^+^ **\[Ne^10^\]**­­­­ [↑↓] [↑\_] \_\_\_ \_\_\_ 3s 3p P^+^ **\[Ne^10^\]**­­­­ [↑↓] [↑\_\_] [↑] [\_\_\_] 3s 3p S^+^ **\[Ne^10^\]**­­­­ [↑↓] [↑\_\_] [↑\_\_] [↑\_\_] 3s 3p Cl^+^ **\[Ne^10^\]**­­­­ [↑↓] [↑↓] [↑\_\_] [↑\_\_] 3s 3p Ar^+^ **\[Ne^10^\]**­­­­ [↑↓] [↑↓] [↑↓] [↑\_\_] 3s 3p