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As an approximate rule, electron configurations are given by the Aufbau principle and the Madelung rule. However there are numerous exceptions; for example the lightest exception is chromium, which would be predicted to have the configuration 1s 2 2s 2 2p 6 3s 2 3p 6 3d 4 4s 2 , written as [Ar] 3d 4 4s 2 , but whose actual configuration given ...
Electron configuration 3s 1: Electrons per shell: 2, 8, 1: ... Sodium is an alkali metal, being in group 1 of the periodic table. Its only stable isotope is 23 Na ...
This would be the case for example to excite a 2p electron of sodium to the 3s level and form the excited 1s 2 2s 2 2p 5 3s 2 configuration. The remainder of this article deals only with the ground-state configuration, often referred to as "the" configuration of an atom or molecule.
Configurations of elements 109 and above are not available. Predictions from reliable sources have been used for these elements. Grayed out electron numbers indicate subshells filled to their maximum. Bracketed noble gas symbols on the left represent inner configurations that are the same in each period. Written out, these are: He, 2, helium : 1s 2
Atomic number (Z): 11: Group: group 1: hydrogen and alkali metals: Period: period 3: Block s-block Electron configuration [] 3sElectrons per shell: 2, 8, 1: Physical properties; Phase at STP
The eleventh electron begins the filling of the third shell by occupying a 3s orbital, giving a configuration of 1s 2 2s 2 2p 6 3s 1 for sodium. This configuration is abbreviated [Ne] 3s 1 , where [Ne] represents neon's configuration.
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By contrast, the second electron resides in the deeper second electron shell, and the second ionization energy required for its removal is much larger: +4562 kJ per mole. [2] Thus sodium will, in most cases, form a compound in which it has lost a single electron and have a full outer shell of eight electrons, or octet.