Editing Nonmetal (section)

=== Chemical properties by element type ===
{{hatnote|See also {{slink||Chemical}}}}

[[Chemical properties]] are listed from general characteristics to more specific details.

{|class="wikitable" style="font-size:95%"
|-
!rowspan="2" style="horizontal=align:center; font-size:105%""|Property
!colspan="5" style="horizontal=align:center; font-size:105%""|Element type
|-
! scope="col" style="width:17%; text-align:left"|Metals
! scope="col" style="width:17%; text-align:left; border-right:2px dashed #CDCDCD; border-left:2px dashed #CDCDCD; border-top:2px dashed #CDCDCD"|Metalloids
! scope="col" style="width:17%; text-align:left" | Unc. nonmetals
! scope="col" style="width:17%; text-align:left"|Halogen nonmetals
! scope="col" style="width:17%; text-align:left"|Noble gases
|- style="vertical-align:top"
| scope="row" |General chemical behavior
| {{indented plainlist|indent=0.9em|
* ◇ strong to weakly metallic<ref>[[#Kneen|Kneen, Rogers & Simpson 1972, p. 264]]</ref>
* ◇ [[noble metal]]s are relatively inert<ref>[[#Rayner|Rayner-Canham 2018, p. 203]]</ref>
  }}
| style="border-right:2px dashed #CDCDCD; border-left:2px dashed #CDCDCD|weakly nonmetallic{{efn|Metalloids always give "compounds less acidic in character than the corresponding compounds of the [typical] nonmetals."<ref name="Rochow 1966, p. 4" />}}
| moderately nonmetallic<ref name="W2009">[[#Welcher|Welcher 2009, p. 3–32]]: "The elements change from{{nbsp}}... metalloids, to moderately active nonmetals, to very active nonmetals, and to a noble gas."</ref>
| strongly nonmetallic<ref>[[#Mackin|Mackin 2014, p. 80]]</ref>
| {{indented plainlist|indent=0.9em|
* ◇ inert to nonmetallic<ref>[[#Johnson1966|Johnson 1966, pp. 105–108]]</ref>
* ◇ radon shows some cationic behavior<ref>[[#Stein1969|Stein 1969, pp. 5396‒5397]]; [[#Pitzer|Pitzer 1975, pp. 760‒761]]</ref>
  }}
|- style="vertical-align:top"
| scope="row" rowspan=3|[[Oxide]]s
|basic; some [[amphoteric]] or acidic<ref name="Porterfield">[[#Porter|Porterfield 1993, p. 336]]</ref>
| style="border-right:2px dashed #CDCDCD; border-left:2px dashed #CDCDCD"|amphoteric or weakly acidic<ref>[[#Rochow1966|Rochow 1966, p. 4]]; [[#Atkins2006|Atkins et al. 2006, pp. 8, 122–123]]</ref>{{efn|Arsenic trioxide reacts with sulfur trioxide, forming [[arsenic sulfate|arsenic "sulfate"]] As<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub>.<ref>[[#Wiberg|Wiberg 2001, p. 750]].</ref> This substance is covalent in nature rather than ionic;<ref>[[#Douglade|Douglade & Mercier 1982, p. 723]]</ref> it is also given as As<sub>2</sub>O<sub>3</sub>·3SO<sub>3</sub>.<ref>[[#Gillespie|Gillespie & Robinson 1959, p. 418]]</ref>}}
|acidic{{efn|{{chem|||NO|2}}, {{chem|||N|2||O|5}}, {{chem|||SO|3}}, {{chem|||SeO|3}} are strongly acidic.<ref>[[#Sanderson1967|Sanderson 1967, p. 172]]; [[#Mingos2019|Mingos 2019, p. 27]]</ref>}} or neutral{{efn|H<sub>2</sub>O, CO, NO, N<sub>2</sub>O are neutral oxides; CO and N<sub>2</sub>O are "formally the [[anhydride]]s of [[formic acid|formic]] and [[hyponitrous acid]], respectively viz. CO + H<sub>2</sub>O → H<sub>2</sub>CO<sub>2</sub> (HCOOH, formic acid); N<sub>2</sub>O + H<sub>2</sub>O → H<sub>2</sub>N<sub>2</sub>O<sub>2</sub> (hyponitrous acid)."<ref>[[#House|House 2008, p. 441]]</ref>}}

|acidic{{efn|{{chem|||ClO|2}}, {{chem|||Cl|2||O|7}}, {{chem|||I|2||O|5}} are strongly acidic.<ref>[[#Mingos2019|Mingos 2019, p. 27]]; [[#Sanderson1967|Sanderson 1967, p. 172]]</ref>}}

|metastable XeO<sub>3</sub> is acidic;<ref>[[#Wiberg|Wiberg 2001, p. 399]]</ref> stable XeO<sub>4</sub> strongly so<ref>[[#Klae|Kläning & Appelman 1988, p. 3760]]</ref>
|- style="vertical-align:top"
| few glass formers{{efn|Metals that form glasses are: vanadium; molybdenum, tungsten; alumnium, indium, thallium; tin, lead; and bismuth.<ref name="Rao 2002, p. 22">[[#Rao2002|Rao 2002, p. 22]]</ref>}}
|style="border-right:2px dashed #CDCDCD; border-left:2px dashed #CDCDCD"|all glass formers<ref>[[#Sidorov|Sidorov 1960, pp. 599–603]]</ref>
|some glass formers{{efn|Unclassified nonmetals that form glasses are phosphorus, sulfur, selenium;<ref name="Rao 2002, p. 22"/> [[carbon dioxide|CO<sub>2</sub>]] forms a glass at 40&nbsp;GPa.<ref>[[#McMillan|McMillan 2006, p. 823]]</ref>}}
|no glass formers reported
|no glass formers reported
|- style="vertical-align:top"
|ionic, polymeric, layer, chain, and molecular structures<ref>[[#Wells|Wells 1984, p. 534]]</ref>
|style="border-right:2px dashed #CDCDCD; border-left:2px dashed #CDCDCD"|polymeric in structure<ref name="Pudd">[[#Puddephatt|Puddephatt & Monaghan 1989, p. 59]]</ref>
|{{indented plainlist|indent=0.9em|
* ◇ mostly molecular<ref name="Pudd"/>
* ◇ carbon, phosphorus, sulfur, selenium have 1+ polymeric forms}}

|{{indented plainlist|indent=0.9em|
* ◇ mostly molecular
* ◇ iodine has a polymeric form, [[Iodine pentoxide|I<sub>2</sub>O<sub>5</sub>]]<ref>[[#King1995|King 1995, p. 182]]</ref>}}

|{{indented plainlist|indent=0.9em|
* ◇ mostly molecular
* ◇ [[xenon dioxide|XeO<sub>2</sub>]] is polymeric<ref>[[#Ritter|Ritter 2011, p. 10]]</ref>}}
|- style="vertical-align:top"
| scope="row" |Compounds with metals
| alloys<ref name="Kneen"/> or [[intermetallic compound]]s<ref>[[#Yama|Yamaguchi & Shirai 1996, p. 3]]</ref>
| style="border-right:2px dashed #CDCDCD; border-left:2px dashed #CDCDCD"|tend to form alloys or intermetallic compounds<ref>[[#Vernon2020|Vernon 2020, p. 223]]</ref>
| {{indented plainlist|indent=0.9em|
* ◇ salt-like to covalent or metallic: hydrogen†, carbon, nitrogen, phosphorus, sulfur, selenium<ref name="Vernon2020p220"/>
* ◇ mainly ionic: oxygen<ref>[[#Woodward|Woodward et al. 1999, p. 134]]</ref>
  }}
| mainly ionic<ref name="Cotton"/>
| simple compounds at STP not known{{efn|[[Disodium helide]] (Na<sub>2</sub>He) is a compound of helium and sodium that is stable at high pressures above 113&nbsp;GPa. Argon forms an alloy with nickel, at 140&nbsp;GPa and close to 1,500 K, however at this pressure argon is no longer a noble gas.<ref>[[#Dalton|Dalton 2019]]</ref>}}
|- style="vertical-align:top"
| scope="row" rowspan=3|[[Ionization energy]] (kJ mol<sup>−1</sup>)<ref name="AylwardIE">[[#Aylward|Aylward & Findlay 2008, p. 132]]</ref>&thinsp;‡
| low to high
| style="border-right:2px dashed #CDCDCD; border-left:2px dashed #CDCDCD"|moderate
| moderate to high
| high
| high to very high
|- style="vertical-align:top"
| style="border-right:2px dashed #CDCDCD; border-left:2px dashed #CDCDCD"| 376 to 1,007
| style="border-right:2px dashed #CDCDCD; border-left:2px dashed #CDCDCD"| 762 to 947
| 941 to 1,402
| 1,008 to 1,681
| 1,037 to 2,372
|- style="vertical-align:top"
| style="border-right:2px dashed #CDCDCD; border-left:2px dashed #CDCDCD"| average 643
| style="border-right:2px dashed #CDCDCD; border-left:2px dashed #CDCDCD"| average 833
| average 1,152
| average 1,270
| average 1,589
|- style="vertical-align:top"
| scope="row" rowspan=3|[[Electronegativity]] (Pauling){{efn|Values for the noble gases are from Rahm, Zeng and Hoffmann.<ref name="Rahm">[[#Rahm|Rahm, Zeng & Hoffmann 2019, p. 345]]</ref>}}<ref name="AylwardEN">[[#Aylward|Aylward & Findlay 2008, p. 126]]</ref>&thinsp;‡
| low to high
| style="border-right:2px dashed #CDCDCD; border-left:2px dashed #CDCDCD"| moderate
| moderate to high
| high
| high (radon) to very high
|- style="vertical-align:top"
| 0.7 to 2.54
| style="border-right:2px dashed #CDCDCD; border-left:2px dashed #CDCDCD"| 1.9 to 2.18
| 2.19 to 3.44
| 2.66 to 3.98
| ca. 2.43 to 4.7
|- style="vertical-align:top"
| average 1.5
| style="border-right:2px dashed #CDCDCD; border-left:2px dashed #CDCDCD; border-bottom:2px dashed #CDCDCD;"| average 2.05
| average 2.65
| average 3.19
| average 3.3
|}
<span style="font-size:95%">
† Hydrogen can also form alloy-like hydrides<ref name="Cao4"/><br />
‡ The labels ''low'', ''moderate'', ''high'', and ''very high'' are arbitrarily based on the value spans listed in the table</span>