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[[File:Periodic table (metals–metalloids–nonmetals, 32 columns).png|upright=1.36|rightleft|thumb

[[File:First Ionization Energy.svg|thumb|upright=2.27|rightleft|Ionization energy: each period begins at a minimum for the alkali metals, and ends at a maximum for the noble gases]]

[[Image:Periodic variation of Pauling electronegativities.png|thumb|rightleft|upright=1.35|Graph showing increasing electronegativity with growing number of selected groups]]

[[File:Electron affinity of the elements.svg|thumb|upright=1.8|rightleft|Dependence of electron affinity on atomic number.<ref>Huheey, Keiter & Keiter, p. 42</ref> 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.<ref>{{cite book |last1=Siekierski|first1=S.|last2=Burgess|first2=J.|title=Concise chemistry of the elements|publisher=Horwood Publishing|location=Chichester|year=2002|isbn=1-898563-71-3|pages=35‒36}}</ref>]]