Manganese dioxide

Template:Chembox Manganese dioxide is the inorganic compound with the formula Template:Chem/link. This blackish or brown solid occurs naturally as the mineral pyrolusite, which is the main ore of manganese and a component of manganese nodules. The principal use for Template:Chem/link is for dry-cell batteries, such as the alkaline battery and the zinc–carbon battery, although it is also used for other battery chemistries such as aqueous zinc-ion batteries. Template:Chem/link is also used as a pigment and as a precursor to other manganese compounds, such as potassium permanganate (Template:Chem2). It is used as a reagent in organic synthesis, for example, for the oxidation of allylic alcohols. Template:Chem/link has an α-polymorph that can incorporate a variety of atoms (as well as water molecules) in the "tunnels" or "channels" between the manganese oxide octahedra. There is considerable interest in Template:Chem/link as a possible cathode for lithium-ion batteries.

Structure

Several polymorphs of Template:Chem/link are claimed, as well as a hydrated form. Like many other dioxides, Template:Chem/link crystallizes in the rutile crystal structure (this polymorph is called pyrolusite or Template:Chem/link)

, with three-coordinate oxide anions and octahedral metal centres. Template:Chem/link is characteristically nonstoichiometric, being deficient in oxygen. The complicated solid-state chemistry of this material is relevant to the lore of "freshly prepared" Template:Chem/link in organic synthesis. The α-polymorph of Template:Chem/link has a very open structure with "channels", which can accommodate metal ions such as silver or barium. Template:Chem/link is often called hollandite, after a closely related mineral. Two other polymorphs, Todorokite and Romanechite Template:Chem/link, have a similar structure to Template:Chem/link but with larger channels. Template:Chem/link exhibits a layered structure more akin to that of graphite.

Production

Naturally occurring manganese dioxide contains impurities and a considerable amount of manganese(III) oxide. Production of batteries and ferrite (two of the primary uses of manganese dioxide) requires high purity manganese dioxide. Batteries require "electrolytic manganese dioxide" while ferrites require "chemical manganese dioxide".

Chemical manganese dioxide

One method starts with natural manganese dioxide and converts it using dinitrogen tetroxide and water to a manganese(II) nitrate solution. Evaporation of the water leaves the crystalline nitrate salt. At temperatures of 400 °C, the salt decomposes, releasing Template:Chem/link and leaving a residue of purified manganese dioxide. These two steps can be summarized as:

Template:Chem/link + Template:Chem/link Template:Eqm Template:Chem/link

In another process, manganese dioxide is carbothermically reduced to manganese(II) oxide which is dissolved in sulfuric acid. The filtered solution is treated with ammonium carbonate to precipitate Template:Chem/link. The carbonate is calcined in air to give a mixture of manganese(II) and manganese(IV) oxides. To complete the process, a suspension of this material in sulfuric acid is treated with sodium chlorate. Chloric acid, which forms in situ, converts any Mn(III) and Mn(II) oxides to the dioxide, releasing chlorine as a by-product.

Lastly, the action of potassium permanganate over manganese sulfate crystals produces the desired oxide.

2 Template:Chem/link + 3 Template:Chem/link + 2 Template:Chem/link→ 5 Template:Chem/link + Template:Chem/link + 2 Template:Chem/link

Electrolytic manganese dioxide

Electrolytic manganese dioxide (EMD) is used in zinc–carbon batteries together with zinc chloride and ammonium chloride. EMD is commonly used in zinc manganese dioxide rechargeable alkaline (Zn RAM) cells also. For these applications, purity is extremely important. EMD is produced in a similar fashion as electrolytic tough pitch (ETP) copper: The manganese dioxide is dissolved in sulfuric acid (sometimes mixed with manganese sulfate) and subjected to a current between two electrodes. The MnO₂ dissolves, enters solution as the sulfate, and is deposited on the anode.

Reactions

The important reactions of Template:Chem/link are associated with its redox, both oxidation and reduction.

Reduction

Template:Chem/link is the principal precursor to ferromanganese and related alloys, which are widely used in the steel industry. The conversions involve carbothermal reduction using coke:

Template:Chem/link + 2 C → Mn + 2 CO

The key redox reactions of Template:Chem/link in batteries is the one-electron reduction:

Template:Chem/link + e⁻ + Template:Chem/link → MnO(OH)

Template:Chem/link catalyses several reactions that form Template:Chem/link. In a classical laboratory demonstration, heating a mixture of potassium chlorate and manganese dioxide produces oxygen gas. Manganese dioxide also catalyses the decomposition of hydrogen peroxide to oxygen and water:

2 Template:Chem/link → 2 Template:Chem/link + Template:Chem/link

Manganese dioxide decomposes above about 530 °C to manganese(III) oxide and oxygen. At temperatures close to 1000 °C, the mixed-valence compound Template:Chem/link forms. Higher temperatures give MnO, which is reduced only with difficulty.

File:Beta-MnO2.png

Crystal structure of $\mathrm{\beta }\text{-}\mathrm{M}\mathrm{n}\mathrm{O}{\phantom{A}}_2$ (pyrolusite type). $\mathrm{M}\mathrm{n}\mathrm{O}{\phantom{A}}_6$ octahedra share corners forming 1D chains along [001].

Hot concentrated sulfuric acid reduces Template:Chem/link to manganese(II) sulfate:

2 Template:Chem/link + 2 Template:Chem/link → 2 Template:Chem/link + Template:Chem/link + 2 Template:Chem/link

The reaction of hydrogen chloride with Template:Chem/link was used by Carl Wilhelm Scheele in the original isolation of chlorine gas in 1774. Scheele treated sodium chloride with concentrated sulfuric acid:

Template:Chem/link + 4 HCl → Template:Chem/link + Template:Chem/link + 2 Template:Chem/link

Standard electrode potentials suggest that the reaction would not proceed...

E^o (Template:Chem/link(s) + 4 Template:Chem/link + 2 e⁻ Template:Eqm Mn²⁺ + 2 Template:Chem/link) = +1.23 V

E^o (Template:Chem/link(g) + 2 e⁻ Template:Eqm 2 Cl⁻) = +1.36 V

...but it is favoured by the extremely high acidity and the evolution (and removal) of gaseous chlorine.

This reaction is also a convenient way to remove the manganese dioxide precipitate from the ground glass joints after running a reaction (for example, an oxidation with potassium permanganate).

Oxidation

Heating a mixture of KOH and Template:Chem/link in air gives green potassium manganate:

2 Template:Chem/link + 4 KOH + Template:Chem/link → 2 Template:Chem/link + 2 Template:Chem/link

Potassium manganate is the precursor to potassium permanganate, a common oxidant.

Occurrence and applications

Prehistory

Excavations at the Pech-de-l'Azé cave site in southwestern France have yielded blocks of manganese dioxide writing tools, which date back 50,000 years and have been attributed to Neanderthals . Scientists have conjectured that Neanderthals used this mineral for body decoration, but there are many other readily available minerals that are more suitable for that purpose. Heyes et al. (in 2016) determined that the manganese dioxide lowers the combustion temperatures for wood from above 350°C (662°F) to 250°C (482°F), making fire making much easier and this is likely to be the purpose of the blocks.

Batteries

The predominant application of Template:Chem/link is as a component of dry cell batteries: alkaline batteries and so called Leclanché cell, or zinc–carbon batteries. Approximately 500,000 tonnes are consumed for this application annually.

δ-Template:Chem/link has also been researched as the primary cathode material for aqueous zinc-ion battery systems. Such cathodes often contain additives to address structural, kinetic, and conductivity-based issues. These carbon additives can include reduced graphene oxide (rGO) and carbon nanotubes, among others.

Organic synthesis

A specialized use of manganese dioxide is as oxidant in organic synthesis. The effectiveness of the reagent depends on the method of preparation, a problem that is typical for other heterogeneous reagents where surface area, among other variables, is a significant factor. The mineral pyrolusite makes a poor reagent. Usually, however, the reagent is generated in situ by treatment of an aqueous solution Template:Chem/link with a Mn(II) salt, typically the sulfate. Template:Chem/link oxidizes allylic alcohols to the corresponding aldehydes or ketones:

cis-RCH=Template:Chem/link + Template:Chem/link → cis-RCH=CHCHO + MnO + Template:Chem/link

The configuration of the double bond is conserved in the reaction. The corresponding acetylenic alcohols are also suitable substrates, although the resulting propargylic aldehydes can be quite reactive. Benzylic and even unactivated alcohols are also good substrates. 1,2-Diols are cleaved by Template:Chem/link to dialdehydes or diketones. Otherwise, the applications of Template:Chem/link are numerous, being applicable to many kinds of reactions including amine oxidation, aromatization, oxidative coupling, and thiol oxidation.

Other potential applications

In Geobacteraceae sp., MnO₂ functions as an electron acceptor coupled to the oxidation of organic compounds. This theme has possible implications for bioremediation within the field of microbiology.

Template:Chem/link is used as an inorganic pigment in ceramics and in glassmaking.

See also

• List of inorganic pigments

Cited sources

• Template:RubberBible99th

External links

• Index of Organic Synthesis procedures utilizing Template:Chem/link
• Example Reactions with Mn(IV) oxide
• National Pollutant Inventory – Manganese and compounds Fact Sheet
• PubChem summary of Template:Chem/link
• International Chemical Safety Card 0175
• Potters Manganese Toxicity by Elke Blodgett
• The reaction between manganese dioxide and potassium permanganate (1893) by A. J. Hopkins