I don't understand electron configuration can some explain to meI have a test tomorrow on it[Rn] 7s2 5f12 i have a chart off this to do but i dont understand electron configuration! what about when there is 3??? like: 4s2 3d10 4p6? its confusing and i dont understand how the element name for that is aluminumi need an explanation pleaseblock? period ? group ? element name? element type? atomic ? p-? n?
For purposes of simplicity, the electron configuration of an atom is often written with the symbol of a noble gas in brackets, such as [Rn], followed by the symbols for the distribution of the remaining electronsFor example, sodium would be written [Ne] 3s?, meaning that if the single 3s electron were removed the remaining electron arrangement would be that of neonThe number to the left of the s information, as in 3s?, shows what period the element is inThe 3 in the 3s? of sodium means that sodium is a period-3 elementThe s, p, d, and f parts refer to the different kinds of orbitals, or sub-shells, that the electrons are found inS orbitals are the simplest and innermost in any given shellOnly two electrons can fit there, so you'll see such things as 2s? or 4s?, but not 3s? or anything elseP orbitals can hold 6 electrons; d orbitals can hold 10 electrons; f orbitals can hold 14 electrons[Rn] 7s? 5f??, also written as [Rn] 5f?? 7s?, means that the atom has 2 s electrons and 12 f electrons beyond the arrangement for radonThese 14 other electrons show that this atom has 14 more protons than radon; 86 + 14 100, the atomic number of fermiumAluminum is a period-3 element, so its configuration will also begin with [Ne]; the complete expression is [Ne] 3s? 3p?Your example of 4s2 3d10 4p6 would be krypton, though you need [Ar] in front of itSee the Wikipedia articles linked below for discussions of s-block, p-block, d-block, and f-block elements and their electron arrangements.
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