Approximate order in which shells and subshells are arranged by increasing energy according to the Madelung rulePeriodic table trends (arrows show an increase)
Dependence of electron affinity on atomic number.[۱] Values generally increase across each period, culminating with the halogens before decreasing precipitously with the noble gases. Examples of localized peaks seen in hydrogen, the alkali metals and the group 11 elements are caused by a tendency to complete the s-shell (with the 6s shell of gold being further stabilized by relativistic effects and the presence of a filled 4f sub shell). Examples of localized troughs seen in the alkaline earth metals, and nitrogen, phosphorus, manganese and rhenium are caused by filled s-shells, or half-filled p- or d-shells.[۲]
The discovery of the elements mapped to significant periodic table development dates (pre-, per- and post-)Newlands' periodic table, as presented to the Chemical Society in 1866, and based on the law of octaves
Mendeleev's periodic table from his book An Attempt Towards a Chemical Conception of the Ether
A version of Mendeleev's 1869 periodic table: An experiment on a system of elements based on their atomic weights and chemical similarities. This early arrangement presents the periods vertically, and the groups horizontally.
Mendeleev's 1871 periodic table with eight groups of elements. Dashes represented elements unknown in 1871.Eight-column form of periodic table, updated with all elements discovered to 2016
↑Siekierski, S.; Burgess, J. (2002). Concise chemistry of the elements. Chichester: Horwood Publishing. د کتاب پاڼي 35‒36. د کتاب نړيواله کره شمېره1-898563-71-3. الوسيط |CitationClass= تم تجاهله (مساعدة)
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