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The usual criticism of the electron configuration theory is that it fails to take into account the properties of the oxide film. Uhlig’s idea was that a passive binary alloy would have an electron configuration as close as possible to that of an inert noble gas atom. Uhlig noted that a number of transition metals become passive at certain critical compositions when alloyed with a second metal. The electron configuration theory was proposed by Uhlig and is an extension of the adsorption theory of passivity. In this paper, data on the electron configuration of atoms was used to predict the reactivity of chemical elements belonging to different blocks, S, P, D, F and DF. A fundamental application of electron configurations is in the interpretation of atomic spectra. In effect, electron configurations, along with some simplified form of molecular orbital theory, have become the modern equivalent of the valence concept, describing the number and type of chemical bonds that an atom can be expected to form. The sum of the superscripts is equal to the atomic number. The most widespread application of electron configurations is in the rationalization of chemical properties, in both inorganic and organic chemistry. The electron configuration for every element above Ar has the 1s 2 2s 2 2p 6 orbital configuration. Many of the physical and chemical properties of elements can be correlated to their unique electron configurations. The electron configuration is used to describe the orbitals of an atom in its ground state, but it can also be used to represent an atom that has ionized into a cation or anion by compensating with the loss of or gain of electrons in their subsequent orbitals. Writing the electron configuration of an element, therefore, provides a useful representation of the electrons occupying the specific orbitals in each atom. Electron configurations of the next two elements in the periodic table, for example, could be written as follows. The orbitals themselves are shown on an energy diagram as blanks and we will put in up arrows and down arrows to represent the spin quantum numbers + and. The basis of this prediction is a rule known as the Aufbau principle, which assumes that electrons are added to an atom, one at a time, starting with the lowest energy orbital, until all of the electrons have been placed in an appropriate orbital. By convention, we therefore write abbreviated electron configurations in terms of the number of electrons beyond the previous element with a filled-shell electron configuration. Electrons fill shells according to their energy levels, as dictated by the Aufbau principle and Hund’s rule. The electron configuration of an atom describes the orbitals occupied by electrons on the atom. Electron configuration is also known as electronic configuration and describes the arrangement of electrons in an atom. Corrosionpedia Explains Electron Configuration