Tuesday, December 4, 2018

ACTIVITY SERIES OF METALS : Predicting Reactivity - The activity series of metals is an empirical tool used to predict products in displacement reactions and reactivity of metals with water and acids in replacement reactions and ore extraction. It can be used to predict the products in similar reactions involving a different metal.

A close-up view of the periodic table focused on the chemical element Lithium.

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Activity Series
Activity Series of Metals: Predicting Reactivity
by Todd Helmenstine

The activity series of metals is an empirical tool used to predict products in displacement reactions and reactivity of metals with water and acids in replacement reactions and ore extraction.
It can be used to predict the products in similar reactions involving a different metal.
Exploring the Activity Series Chart
The activity series is a chart of metals listed in order of declining relative reactivity.
The top metals are more reactive than the metals on the bottom.
For example, both magnesium and zinc can react with hydrogen ions to displace H2 from a solution by the reactions:
Mg(s) + 2 H+(aq) H2(g) + Mg2+(aq)
Zn(s) + 2 H+(aq) H2(g) + Zn2+(aq)
Both metals react with the hydrogen ions, but magnesium metal can also displace zinc ions in solution by the reaction:
Mg(s) + Zn2+  Zn(s) + Mg2+
This shows magnesium is more reactive than zinc and both metals are more reactive than hydrogen.
This third displacement reaction can be used for any metal that appears lower than itself on the table.
The further apart the two metals appear, the more vigorous the reaction.
Adding a metal like copper to zinc ions will not displace the zinc since copper appears lower than zinc on the table.
The first five elements are highly reactive metals that will react with cold water, hot water, and steam to form hydrogen gas and hydroxides.
The next four metals (magnesium through chromium) are active metals that will react with hot water or steam to form their oxides and hydrogen gas.
All the oxides of these two groups of metals will resist reduction by H2 gas.
The six metals from iron to lead will replace hydrogen from hydrochloric, sulfuric and nitric acids.
Their oxides can be reduced by heating with hydrogen gas, carbon, and carbon monoxide.
All the metals from lithium to copper will combine readily with oxygen to form their oxides.
The last five metals are found free in nature with little oxides. Their oxides form through alternate pathways and will readily decompose with heat.
The series chart below works remarkably well for reactions that occur at or near room temperatures and in aqueous solutions.
Activity Series of Metals
Metal
Symbol
Reactivity
Lithium
Li
displaces H2 gas from water, steam and acids and forms hydroxides
Potassium
K
Strontium
Sr
Calcium
Ca
Sodium
Na
Magnesium
Mg
displaces H2 gas from steam and acids and forms hydroxides
Aluminum
Al
Zinc
Zn
Chromium
Cr
Iron
Fe
displaces H2 gas from acids only and forms hydroxides
Cadmium
Cd
Cobalt
Co
Nickel
Ni
Tin
Sn
Lead
Pb
Hydrogen gas
H2
included for comparison
Antimony
Sb
combines with O2 to form oxides and cannot displace H2
Arsenic
As
Bismuth
Bi
Copper
Cu
Mercury
Hg
found free in nature, oxides decompose with heating
Silver
Ag
Palladium
Pd
Platinum
Pt
Gold
Au

 

Todd Helmenstine Biography
Todd Helmenstine is a science writer, graphic artist, and IT professional.
Mr. Helmenstine has bachelor of art degrees in physics and mathematics from Hastings College in Hastings, Nebraska.
Todd is best known for his popular printable periodic tables and periodic table wallpapers. His work has been featured on About.com, ThoughtCo.com, and showcased here on Science Notes. The tables have appeared, by permission, in numerous textbooks, journals, and videos.
How Todd Helmenstine Makes Periodic Tables
Most of the printable periodic tables and other illustrations are made using Adobe Illustrator and Adobe Photo Shop. In some cases, 3-D renders are made, using Incendia or Bryce.


A close-up view of the periodic table focused on the chemical element Lithium.

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