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The Order of Filling Orbitals. The aufbau principle explains how electrons fill low energy orbitals (closer to the nucleus) before they fill higher energy ones. Where there is a choice between orbitals of equal energy, they fill the orbitals singly as far as possible (Hunds rules).
Hund's rule specifies the order of electron filling within a set of orbitals. Orbital filling diagrams are a way of indicating electron locales in orbitals.
The energy of an orbital is calculated by the sum of the principal and the azimuthal quantum numbers. According to this principle, electrons are filled in the following order: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p…
Although this is the general order of orbital filling according to the Madelung rule, there are exceptions, and the actual electronic energies of each element are also dependent upon additional details of the atoms (see Electron configuration § Atoms: Aufbau principle and Madelung rule).
The filling order simply begins at hydrogen and includes each subshell as you proceed in increasing Z order. For example, after filling the 3 p block up to Ar, we see the orbital will be 4s (K, Ca), followed by the 3 d orbitals.
The filling order simply begins at hydrogen and includes each subshell as you proceed in increasing Z order. For example, after filling the 3 p block up to Ar, we see the orbital will be 4s (K, Ca), followed by the 3 d orbitals.
An electron orbital filling diagram shows the arrangement of electrons within the orbitals of an atom or ion. Each orbital is represented by a box, and the electrons are denoted by arrows with their spin indicated. The diagram follows the Aufbau principle, Pauli exclusion principle, and Hund’s rule.
Electrons are placed into the atomic orbitals filling from bottom to top (like water in a jug) from lowest to highest energy (i.e. most stable to least stable). The Schrodinger equation dictates the energy order of the orbitals: (but they can be readily determined by looking at the periodic table or using a simple mnemonic).
Order of filling electrons in the orbitals and Shells.
The order of filling will place one electron in each before placing two in any one orbital since the mutually repulsive electrons prefer to be further apart. The filling of the 2p orbital places eight electrons in the second shell, a "stable octet". The particularly stable configuration produces the noble gas neon.