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This page shows the electron configurations of the neutral gaseous atoms in their ground states. For each atom the subshells are given first in concise form, then with all subshells written out, followed by the number of electrons per shell. For phosphorus (element 15) as an example, the concise form is [Ne] 3s 2 3p 3.
Mo 1 5 - 43 Tc 2 5 - 44 Ru 1 7 - 45 Rh 1 8 - 46 Pd-10 - 47 Ag 1 10 - 48 Cd 2 10 - 49 In 2 10 1 50 Sn 2 10 2 51 Sb 2 10 ... Note that these electron configurations are ...
Electron configuration 4d 5 5s 1: ... In its pure form, molybdenum is a silvery-grey metal with a Mohs hardness of 5.5 and a standard atomic ... for long periods of ...
For example, the electron configuration of the neon atom is 1s 2 2s 2 2p 6, meaning that the 1s, 2s, and 2p subshells are occupied by two, two, and six electrons, respectively. Electronic configurations describe each electron as moving independently in an orbital, in an average field created by the nuclei and all the other
A molecular orbital can specify the electron configuration of a molecule: the spatial distribution and energy of one (or one pair of) electron(s). Most commonly a MO is represented as a linear combination of atomic orbitals (the LCAO-MO method), especially in qualitative or very approximate usage.
Application of MO theory for dihydrogen results in having both electrons in the bonding MO with electron configuration 1σ g 2. The bond order for dihydrogen is (2-0)/2 = 1. The photoelectron spectrum of dihydrogen shows a single set of multiplets between 16 and 18 eV (electron volts). [14] The dihydrogen MO diagram helps explain how a bond breaks.
In MO theory, any electron in a molecule may be found anywhere in the molecule, since quantum conditions allow electrons to travel under the influence of an arbitrarily large number of nuclei, as long as they are in eigenstates permitted by certain quantum rules. Thus, when excited with the requisite amount of energy through high-frequency ...
The elements in the group, like those of groups 7–11, have high melting points, and form volatile compounds in higher oxidation states. All the elements of the group are relatively nonreactive metals with a high melting points (1907 °C, 2477 °C, 3422 °C); that of tungsten is the highest of all metals.