Electronic - Positronic Configurations

The Periodic Table of Matter & Antimatter Elements is divided into sections devoted to filling in the various kinds of subshells as shown below:

Each column represents electrons or positrons being added to the same type of orbital.  The electron and positron order of filling is shown above.  Although most atoms are in the ground state, excited states are possible by pumping electrons up to higher energy.  The ground state of hydrogen is 1s¹. By adding the right amount of energy, the electron can be pumped up to 1s⁰ 2s¹, or even 1s⁰ 2s⁰ 2p¹, etc.. Such transitions produce the spectrum of hydrogen atom.

Because of the Pauli Exclusion Principle, each orbital, sublevel and primary level can only hold a certain number of electrons. The electrons and positrons must go into a distinct set of orbitals. In the ground state of the atom, electrons will occupy the lowest energy orbitals first, and only fill the higher energy orbitals when no lower energy orbitals are left. The arrangement of electrons in an atom is known as its electronic and positronic configurations.

The configurations describes the energy levels that are occupied by electrons & positions within matter & antimatter atoms. The total electronic energy of an atom is minimized by placing the electrons or positrons in the lowest possible energy levels.  

E n e r g y o f E l e c t r o n s	Elements       120 8s2               8s   118 7p6             7p     112 6d10           6d       102 5f14         5f         88 7s2             7s   Radon 86 6p6           6p       80 5d10         5d         70 4f14       4f           56 6s2           6s     Xenon 54 5p6         5p         48 4d10       4d           38 5s2         5s       Krypton 36 4p6       4p           30 3d10     3d             20 4s2       4s         Argon 18 3p6     3p             12 3s2     3s           Neon 10 2p6   2p             Helium 4 2s2   2s               2 1s2 1s               Matter Atomic Nos Sub shells 2 8 18 32 32 18 8 2
	Periods 1 2 3 4 5 6 7 8
E n e r g y o f P o s i t r o n s	Anti Matter Atomic Nos Sub shells 2 8 18 32 32 18 8 2 2 1s2 1s AHelium 4 2s2 2s ANeon 10 2p6 2p 12 3s2 3s AArgon 18 3p6 3p 20 4s2 4s 30 3d10 3d AKrypton 36 4p6 4p 38 5s2 5s 48 4d10 4d AXenon 54 5p6 5p 56 6s2 6s 70 4f14 4f 80 5d10 5d ARadon 86 6p6 6p 88 7s2 7s 102 5f14 5f AUnk 112 6d10 6d 118 7p6 7p 120 8s2 8s Elements

Writing the configurations can be tedious for an atom like uranium with 92 electrons. It is common to abbreviate the electron configuration with the preceding noble gas. For Mg, this is neon, which has an electron configuration of 1s²2s²2p⁶, so we can write the the electron configuration of the Mg atom as Mg: [Ne]3s².  Deciding how electrons distribute themselves in a given set of orbitals is the function of Hund's rule

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