Editing Reactivity series (section)

==Table==
{| class = "Wikitable"

! Metal !! Ion !! Reactivity !! Extraction
|-
| style="background: #ffebd2" | [[Caesium]]&nbsp;Cs<!--Please don't add francium. Francium is very heavy, and so its electrons move fast enough that relativity must be considered. The end result is that the 7s electrons are stabilized, enough that Fr is probably actually LESS reactive than Cs! But nothing is known for sure.-->
| style="background: #ffebd2" | Cs<sup>+</sup>
| rowspan=8 style="background: #ffebd2" align=center | reacts with cold water
| rowspan=11 style="background: #ffebd2" align=center| [[Electrolysis]] (a.k.a. electrolytic refining)
|-
| style="background: #ffebd2" | [[Rubidium]]&nbsp;Rb
| style="background: #ffebd2" | Rb<sup>+</sup>
|-
| style="background: #ffebd2" | [[Potassium]]&nbsp;K
| style="background: #ffebd2" | K<sup>+</sup>
|-
| style="background: #ffebd2" | [[Sodium]]&nbsp;Na
| style="background: #ffebd2" | Na<sup>+</sup>
|-
| style="background: #ffebd2" | [[Lithium]]&nbsp;Li
| style="background: #ffebd2" | Li<sup>+</sup>
|-
| style="background: #ffebd2" | [[Barium]]&nbsp;Ba
| style="background: #ffebd2" | Ba<sup>2+</sup>
|-
| style="background: #ffebd2" | [[Strontium]]&nbsp;Sr
| style="background: #ffebd2" | Sr<sup>2+</sup>
|-
| style="background: #ffebd2" | [[Calcium]]&nbsp;Ca
| style="background: #ffebd2" | Ca<sup>2+</sup>
|-
| style="background: #ffeeff" | [[Magnesium]]&nbsp;Mg
| style="background: #ffeeff" | Mg<sup>2+</sup>
| rowspan=1 style="background: #ffeeff" align=center | reacts very slowly with cold water, but rapidly<br />in boiling water, and very vigorously with [[acid]]s
|-
| style="background: #ffffe6" | [[Beryllium]]&nbsp;Be
| style="background: #ffffe6" | Be<sup>2+</sup>
| rowspan=2 style="background: #ffffe6" align=center | reacts with acids and steam
|-
| style="background: #ffffe6" | [[Aluminium]]&nbsp;Al
| style="background: #ffffe6" | Al<sup>3+</sup>
|-

| style="background: #ffffe6" | [[Manganese]]&nbsp;Mn
| style="background: #ffffe6" | Mn<sup>2+</sup>
| rowspan=9 style="background: #ffffe6" align=center | reacts with [[acid]]s; very poor reaction with steam
| rowspan=2 style="background: #ffffe6" align=center | [[smelting]] with [[coke (fuel)|coke]]
|-
| style="background: #ffffe6" | [[Zinc]]&nbsp;Zn
| style="background: #ffffe6" | Zn<sup>2+</sup>
|-
| style="background: #ffffe6" | [[Chromium]]&nbsp;Cr
| style="background: #ffffe6" | Cr<sup>3+</sup> 
| rowspan=1 style="background: #ffeeff" align=center | [[aluminothermic reaction]]
|-
| style="background: #ffffe6" | [[Iron]]&nbsp;Fe
| style="background: #ffffe6" | Fe<sup>2+</sup>
| rowspan=6 style="background: #ffffe6" align=center | [[smelting]] with [[coke (fuel)|coke]]
|-
| style="background: #ffffe6" | [[Cadmium]]&nbsp;Cd
| style="background: #ffffe6" | Cd<sup>2+</sup>
|-
| style="background: #ffffe6" | [[Cobalt]]&nbsp;Co
| style="background: #ffffe6" | Co<sup>2+</sup>
|-
| style="background: #ffffe6" | [[Nickel]]&nbsp;Ni
| style="background: #ffffe6" | Ni<sup>2+</sup>
|-
| style="background: #ffffe6" | [[Tin]]&nbsp;Sn
| style="background: #ffffe6" | Sn<sup>2+</sup>
|-
| style="background: #ffffe6" | [[Lead]]&nbsp;Pb
| style="background: #ffffe6" | Pb<sup>2+</sup>
|-
| style="background: #cdcdcd" | [[Antimony]]&nbsp;Sb
| style="background: #cdcdcd" | Sb<sup>3+</sup>
| rowspan=2 style="background: #cdcdcd" align=center | may react with some strong [[oxidizing acid]]s
| rowspan=10 style="background: #cdcdcd" align=center | heat or physical extraction
|-
| style="background: #cdcdcd" | [[Bismuth]]&nbsp;Bi
| style="background: #cdcdcd" | Bi<sup>3+</sup>
|-
| style="background: #cdcdcd" | [[Copper]]&nbsp;Cu
| style="background: #cdcdcd" | Cu<sup>2+</sup>
| style="background: #ffffe6" align=center | reacts slowly with air
|-
| style="background: #cdcdcd"  | [[Tungsten]]&nbsp;W
| style="background: #cdcdcd" | W<sup>3+</sup>{{Citation needed|date=November 2024}}
| rowspan=7 style="background: #cdcdcd" align=center | may react with some strong [[oxidizing acid]]s
|-
| style="background: #cdcdcd" | [[Mercury (element)|Mercury]]&nbsp;Hg
| style="background: #cdcdcd" | Hg<sup>2+</sup>
|-
| style="background: #cdcdcd" | [[Silver]]&nbsp;Ag
| style="background: #cdcdcd" | Ag<sup>+</sup>
|- 
| style="background: #cdcdcd" | [[Gold]]&nbsp;Au
| style="background: #cdcdcd" | Au<sup>3+</sup><ref
name=":0">{{Webarchive|url=https://web.archive.org/web/20190507084512/http://www.cod.edu/people/faculty/jarman/richenda/1551_hons_materials/Activity%20series.htm|date=May 7 2019|title=Activity series}}</ref><ref>{{cite book|last=Wulsberg|first=Gary|year=2000|title=Inorganic Chemistry|url=https://books.google.com/books?id=hpWzxTnQH14C&pg=PA249|page=294|isbn=9781891389016}}</ref>
|- 
| style="background: #cdcdcd" | [[Platinum]]&nbsp;Pt

| style="background: #cdcdcd" | Pt<sup>4+</sup>
|}
<!--This is not the electrochemical series, but Gold's oxidation potential is more than half a volt higher than Platinum's. It is thermodynamicaly favourable for Pt to form PtO in air, and then PtO2; but Au won't form oxides spontaneously. Pt is used in crucibles etc, but this is due to its better mp/mechanical properties!-->

Going from the bottom to the top of the table the metals:
* increase in reactivity;
* lose electrons ([[Redox|oxidize]]) more readily to form positive ions;
* corrode or tarnish more readily;
* require more energy (and different methods) to be isolated from their compounds;
* become stronger [[reducing agent]]s ([[electron]] donors).