W jaki sposób można otrzymać ten związek Bo z tego co wiem to kwas manganowy (VII) jest silnym utleniaczem i reakcja glinu z nim nie zajdzie (pasywacja)

pewnie tak jak większość soli
a tu przykładzik

MANUFACTURE OF TRANSITIONS METAL PERMANGANATES.
HU90-2426


Transition metal permanganates used as oxidant and catalyst are prepd. by successive reactions of KMnO4 with Al2(SO4)3 to form Al(MnO4)3, Al(MnO4)3 with Ba(OH)2 to form Ba(MnO4)2, and Ba(MnO4)2 with metal sulfate (MeSo4) to form Me(MnO4)2. The conversion of the KMnO4 is increased from 80 to 95% by using 10-100% (preferably 33%) excess of Al2(SO4)3 as compared to stoichiometric amt. The unreacted KMnO4 is removed from the reaction mixt. by slow crystn. of K2Al8(MnO4)2(SO4)12×17H2O. The Me(MnO4)2 yield is increased to
>95% and the purity of the product is improved.

Czy tutaj chdzi o taką reakcję ( wydaje mi się, że nie bo powstanie jak to ktoś na forum kiedyś określił - zupa jonów )

6KMnO4 + Al2(SO4)3 ----> 2Al(MnO4)3 + 3K2SO4

( Jeśli to jednak taka reakcja jak potem oddzielić od siebie te substancje, bo obie są rozpuszczalne w wodzie )

A czy są jakieś inne sposoby np przy użyciu MnO2 [ jest temat odnośnie tlenku manganu (IV) i ktoś tam napisał, że w reakcji tlenku manganu (IV) z kwasem siarkowym (VI) powstają jony MnO4 2- albo MnO4 - w zależności od odczynu roztworu ( czy to prawda , bo wydaje mi się, że powinny powstać jony Mn 2+)]??

to nie jest przepis na Al(MNO4)3
Jak wspominalem mozna sprobowac metod typowych dla wszystkich soli (np analizujac przepiy na nadmanganiany z preparatyk i biorac pod uwage wlasciwosci tego co chcesz otrzymac. Natomiast to streszczenie podalem jako przyklad gdzie o ile dobrze zrozumialem i odebralem intencje streszczenia to nei jest taka zwykla zupa jonowa ale jak wynika (przynajmniej wg mnie) mozemy mowic o obecnosci Al(MNO4)3 a nei mieszaniny jonow na co wskazuje tresc - inaczejmowiono by o katalitycznych wlasciwosciach Al a nie o tworzeniu Al(MNO4)3 i jego dalszej reakcji. Moze nadintepretowalem ale sugerujac sie stylem publikacji tak interpretowalem a nei inaczej

Zreszta jak widac wychwyciles to co potrzeba i zamiast narzekac na zupe to za tablice z wlasciwosciami i wymyslic metode rozdzialu (biorac pod uwage moje wczesniejsze domneimania)

Nie zawsze jest tak ze cos sie od razu wytraci czasami trzeba popracowac i glowa i lapkami A przegladu danych w swieta mi sie za bardzo neichce robic.
Sprawdzilem kilka preparatyki po spisie i na gotowca dla teojego Al(MNO4)3 nei natrafilem

Co do uzycia MnO2 to mozna poprobowac analogicznie jak dla otrzymywania KMNO4 ale czywyjdzie trzeba sprawdzic

Co do tego co ktos napisal to podaj do tego linka to pogadamy
przypuszczam iz chodzi o utlenainei MnO2 w srodowiksu kwasnym (?) gdzie zaczyna sie pojawiac koeljna reakcja Mn(VI) - - Mn(VII)
Zycie intymne Mn i jego dziwne zachowania nie sa dla mnie najciekawsza rzecza a to taki kmaly zbiorek reakcji
http://www.gdynia.mm.pl/~drake87/drake8 ... 207003.htm

http://malutki.vitnet.pl/viewtopic.php? ... c&start=25

To link do tego posta (o ile nie został usunięty). A z rozdzielaniem będę musiał się pogłowić, bo o ile mi wiadomo to sole potasu i manganiany (VII) są rozpuszczalne w wodzie. Dostałem na gwiazdkę książkę z tablicami, to się pogłowię . Niestety nie mam tabeli rozpuszczalności manganianów (VI) czy wie ktoś gdzie można znaleźć

wprawdzie w tym wyciągu z artykułu produktem docelowym jest Ba(MnO4)2 to po dordze widać że może otrzymać Al(MnO4)3 z reakcji o któej mówił CU. Artykuł jest w czaopismie do ktrórego dostępu nie mam[ostatni numer do jakiego mam dostęp to 1980 nr 6] bo bym zeskanował i wrzucił...

Szanowny Kryształoman namieszałeś na forumnieźle.
Ale wydaje mi się iż o ile dobrze odszyfrowalem ta kacza zupe do kwadratu to jest tak :
1. dopadles zuzyta bateryjke ktora wg twoich wiadomosci zawiera MnO2 lub cos co z niego powstalo _ cala masa syfu
2. Sluchajac RadiaZRyjkiem doznales natchnienia i zachcialo ci sie otrzymac czyst mangan w celach ktoych wole sie nei domyslac bo juz sie wlos ze strachu jezy (kolejne 100 postow jak nic)
3. Zasugerowany odpowiedziami rozpoczoles robic doktorat o temacie "Synteza acetonu z kapcia skarpetki i starej bateryjki"

Biorac pod uwage to co pisales (odczynniki : elektrolit, bateryjka , NaOH) i zakladajac w domniemaniu ze sprzet jest zblizony sugerowalbym bateryjke oddac do punktu odbioru bateryjek a elektrolit opchnac.

Jednakze biorac pod uwge fakt iz jakos lyknoles angielskie streszczenie to moja sugestja jest taka :
- sprecyzuj problem co naco poco czy to badania podstawowe z zakresu recyclingu bateryjek i dla jaj otrzymywanie Mn czy tez masz konkretny cel.

W przypadku konkretnnego celu pogadamy dokladniej.

Jesli natomiast prowadzisz badania podstawowe w zakresie chemii manganu i jego zwiazkow to sugerowalbym jednak troche poczytac :
1. Supniewski
2. Google
informacja ulatwiajaca :
Techniczny mangan otrzymuje się poprzez prażenie jego rud i redukowanie glinem powstałego tlenku (Mn3O4) do wolnego manganu. Czysty mangan otrzymuje się w wyniku elektroredukcji (elektroliza + redukcja z materiałem elektrody) soli manganu (II) na katodzie rtęciowej.
Czy Al-termia zadziala ?

co do robactwa:
http://hmx.p2a.pl/viewtopic.php?pid=115

3. porcyjka i np Handbook of Inorganic Chemicals

MANGANESE(II) OXIDE
[1344-43-0]
Formula: MnO; MW 70.94
Synonyms: manganous oxide; manganese monoxide; green manganese oxide;
manganosite [1313-12-8]
Occurrence and Uses
Manganese(II) oxide occurs naturally as manganosite [1313-12-8]. The
mineral is found very rarely in nature. Manganese(II) oxide is used in the fertilizer
industry as a source of manganese in fertilizers; in feedstuff formulations;
and as an intermediate in the production of several manganese compounds.
Physical Properties
Green cubic crystal; refractive index 2.16; density 5.37 g/cm3 at 23°C; Moh’s
hardness 5.5; melts at 1945°C; insoluble in water.
Thermochemical Properties
ΔHƒ° –92.07 kcal/mol
ΔGƒ° –86.74 kcal/mol
S° 14.27 cal/degree mol
Cρ 10.86 cal/degree mol
Production
Manganese(II) oxide is obtained commercially from manganese(IV) oxide
(manganese dioxide) by the reduction with hydrogen, carbon monoxide or
methane at elevated temperatures (>800°C):
MnO2 + CO → MnO + CO2
MnO2 + H2 → MnO + H2O
The oxide also can be made by thermal decomposition of manganese(II) carbonate
or manganese(II) oxalate in the absence of air:
MnCO3 → MnO + CO2
Also, careful dehydration of manganese(II) hydroxide, Mn(OH)2, under controlled
conditions in the absence of air yields MnO.
MANGANESE(II) OXIDE 549
Reactions
Manganese(II) oxide is the lowest oxide of manganese and it is purely a
basic oxide. It reacts with acids to form their manganese(II) salts:
MnO + H2SO4 → MnSO4 + H2O
MnO + 2HCl → MnCl2 + H2O
The compound also is oxidized by air or oxygen to higher oxides of manganese.
When heated cautiously in air, the product is manganese sesquioxide
or manganese(III) oxide:
4MnO + O2 → 2Mn2O3
Analysis
Elemental composition: Mn 77.44%, O 22.55%. The oxide can be characterized
nondestructively by x-ray methods. Also, manganese may be analyzed
by AA or ICP technique following acid digestion with nitric acid and diluting
the acid extract appropriately (see Manganese).
MANGANESE(III) OXIDE
[1317-34-6]
Formula: Mn2O3; MW 157.87
Synonyms: manganese sesquioxide; dimanganese trioxide
Occurrence and Uses
Manganese(III) oxide occurs in nature as the mineral braunite. The oxide
is used in the production of ferrites and thermistors.
Physical Properties
Black cubic (or rhombic) crystals; density 4.50 g/cm3; Moh’s hardness 6–6.5
(for braunite); decomposes at about 875°C; insoluble in water; insoluble in
alcohol and acetone; soluble in acids.
Thermochemical Properties
ΔHƒ° –229.2 kcal/mol
ΔGƒ° –210.6 kcal/mol
S° 26.40 cal/degree mol
Cρ 25.73 cal/degree mol
Preparation
Manganese(III) oxide is obtained by heating manganese(II) oxide in air at
600 to 850°C. It also may be prepared by igniting manganese(II) salts in air
550 MANGANESE(III) OXIDE
or oxygen. The oxide also is produced by cautious heating of manganese(II)
oxide in oxygen. Manganese(III) oxide also can be made by dehydrating manganese(
III) metahydroxide, MnO(OH), in a vacuum at 250°C. In such preparation,
an unstable tetragonal modification, beta-Mn2O3, is first obtained
which on prolonged heating converts to the stable cubic modification, alpha-
Mn2O3.
Analysis
Elemental composition: Mn 69.59%, O 30.41%. The oxide can be characterized
by x-ray methods and analyzed for manganese by AA or ICP following
acid extraction.
MANGANESE(II,III) OXIDE
[1317-35-7]
Formula: Mn3O4; MW 228.81
Synonyms: trimanganese tetraoxide; manganomanganic oxide; red oxide of
manganese
Occurrence and Use
Manganese(II,III) oxide occurs in nature as the mineral hausmannite
[1309-55-3]. It is used to make ferrites and thermistors. The oxide also is used
in the thermite process for producing manganese.
Physical Properties
Black tetragonal crystal; exhibits two allotropic modifications—a stable
alpha phase, occurring in tetragonal crystalline form (as hausmannite) and an
unstable beta modification; density 4.85 g/cm3; Moh’s hardness 5.5; melts at
1,567°C; insoluble in water; soluble in hydrochloric acid.
Thermochemical Properties
ΔHƒ° –331.7 kcal/mol
ΔGƒ° –306.7 kcal/mol
S° 37.2 cal/degree mol
Cρ 33.4 cal/degree mol
Preparation
Manganese(II,III) oxide is made by heating manganese(IV) oxide, MnO2, or
manganese(III) oxide, Mn2O3, above 950°C. When Mn2O3 is heated in air, the
temperature should be above 940°C, but if heated in oxygen, the temperature
should be above 1,090°C. Also, heating manganese(III) oxide at 230°C in
hydrogen yields Mn3O4. However, further heating above 300°C converts
Mn3O4 formed to green manganese(II) oxide, MnO.
Manganese(II,III) oxide also is obtained by heating the dioxide, MnO2, with
carbon at 600 to 700°C.
MANGANESE(II,III) OXIDE 551
Reactions
Manganese(II,III) oxide reacts with dilute acids forming the corresponding
manganous salt and manganese(IV) oxide, MnO2:
Mn3O4 + 2H2SO4 → 2MnSO4 + MnO2 + 2H2O
The oxide, however, dissolves slowly in cold sulfuric acid forming a red
solution that also contains manganic sulfate, Mn2(SO4)3:
Mn3O4 + 4H2SO4 → MnSO4 + Mn2(SO4)3 + 4H2O
Reaction with acetic acid yields manganese(II) acetate and manganese(III)
oxide:
Mn3O4 + 2CH3COOH → Mn(CH3COO)2 + Mn2O3 + H2O
Manganese(II,III) oxide is reduced to manganese metal when heated with
powdered aluminum (the Thermite process). The reaction is vigorous and
exothermic:
3Mn3O4 + 8Al → 4Al2O3 + 9Mn
Analysis
Elemental composition: Mn 72.03%, O 27.98%. The oxide can be characterized
by x-ray methods. Manganese in the oxide can be analyzed by AA or ICP
method after digesting the oxide in nitric acid.
MANGANESE(IV) OXIDE
[1313-13-9]
Formula: MnO2; MW 86.937
Synonyms: manganese dioxide; manganese peroxide; black manganese oxide
Occurrence and Uses
Manganese(IV) oxide is the most important ore of manganese from which
the metal is mostly manufactured. The oxide occurs in nature as the mineral
pyrolusite as heavy gray lumps, or black when powdered.
The mineral is used to produce manganese metal, most manganese salts,
and also manganese steel and other alloys. The metallurgical applications of
manganese(IV) oxide mainly involve making ferromanganese and special
manganese alloys. Another important application of manganese(IV) oxide is
in manufacturing dry-cell batteries and alkaline cells. The oxide also is a colorant
in brick, tile, porcelain and glass; a drier for paints and varnishes; a
552 MANGANESE(IV) OXIDE
preparation for printing and dyeing textiles; a curing agent for polysulfide
rubbers; an adsorbent for hydrogen sulfide and sulfur dioxide; an oxidizing
agent in many organic syntheses such as quinone and hydroquinone; and a
catalyst in laboratory preparation of oxygen from potassium chlorate.
Manganese(IV) oxide also is used to make welding rods and fluxes, and
ceramic magnets (ferrites); and is an additive to fertilizers.
Physical Properties
Black tetragonal crystals; density 5.08 g/cm3; Moh’s hardness 6.3; decomposes
at 535°C; insoluble in water.
Thermochemical Properties
ΔHƒ° –124.3 kcal/mol
ΔGƒ° –111.2 kcal/mol
S° 12.69 cal/degree mol
Cρ 12.93 cal/degree mol
Preparation
Pure manganese(IV) oxide (precipitate form) may be prepared by reducing
permanganate ion with a manganous salt:
2KMnO4 + 3MnSO4 + 2H2O → 5MnO2 + K2SO4 + 2H2SO4
Manganese(IV) oxide can also be precipitated by oxidation of a manganese(
II) salt using an oxidizing agent such as hypochlorite or peroxydisulphate:
Mn2+ + S2O82– + 2H2O → MnO2 + 2SO42– + 4H+
Manganese(IV) oxide may also be made by thermal decomposition of manganese(
II) nitrate; or from roasting manganese(II) carbonate in air:
Mn(NO3)2 → MnO2 + 2NO2
MnCO3 + ½ O2 → MnO2 + CO2
A highly active gamma-MnO2 can be produced by treating manganese(III)
oxide with hot sulfuric acid:
Mn2O3 + H2SO4 → MnO2 + MnSO4 + H2O
Mn2O3 is derived from pyrolusite by heating the mineral at 600–800°C or
reducing with powdered coal at 300°C.
Reactions
Thermal decomposition of manganese(IV) oxide at 600 to 800°C yields manganese(
III) oxide:
MANGANESE(IV) OXIDE 553
4MnO2 → 2Mn2O3 + O2
MnO2 also is reduced to Mn2O3 at 300°C in the presence of a reducing agent
such as hydrogen, methane or carbon.
Treatment with concentrated hydrochloric acid forms manganese(IV) chloride
which readily decomposes to manganese(III) chloride and manganese(II)
chloride, successively liberating chlorine:
MnO2 + 4HCl → MnCl4 + 2H2O
MnCl4 → MnCl3 + ½ Cl2
MnCl3 → MnCl2 + ½ Cl2
When heated with concentrated sulfuric acid, manganese(IV) oxide yields
manganese(II) sulfate, evolving oxygen:
MnO2 + H2SO4 → MnSO4 + H2O + ½ O2
When the solution is heated at 135°C, MnSO4 is oxidized to Mn2(SO4)3.
Reaction with sulfuric acid in the presence of oxalic acid yields manganese(II)
sulfate and carbon dioxide:
MnSO2 + (COOH)2 + H2SO4 → MnSO4 + 2CO2 + 2H2O
While the reaction with sulfuric acid in the presence of sodium chloride
evolves chlorine:
MnO2 + 2NaCl + 2H2SO4 → MnSO4 + Na2SO4 + 2H2O + Cl2
When heated with potassium hydroxide, manganese(IV) oxide partially
decomposes to manganese(III) oxide and potassium manganate:
3MnO2 + 2KOH → Mn2O3 + K2MnO4 + H2O
However, in the presence of oxygen or other oxidizing agents, all manganese
is oxidized to manganate:
MnO2 + 2KOH + ½ O2 → K2MnO4 + H2O
Manganate(VI) can further oxidize to manganate(VII) (or permanganate)
in alkaline solution with a strong oxidizing agent such as hypochlorite, chlorine
or perchlorate, or under anodic oxidation. Alternatively, in less alkaline
media (where the KOH concentration is less than about 15%), the manganate
ion MnO42– hydrolyzes, disproportionating to permanganate MnO4¯ and forming
back manganese(IV) oxide:
554 MANGANESE(IV) OXIDE
3MnO42– + 2H2O → 2MnO4¯ + MnO2 + 4OH¯
The green color of manganate solution turns purple due to the permanganate
formed.
Manganese(IV) oxide is an oxidizing agent. In acid medium, it oxidizes iodide
to iodine:
MnO2 + 2I¯ + 4H+ → Mn2+ + 2H2O + I2
Thus, in the presence of dilute acids, MnO2 is readily attacked by strong
reducing agents. Similarly, reaction with sulfurous acid forms manganese(II)
dithionate:
MnO2 + 2H2SO3 → MnS2O6 + 2H2O
Or with nitrous acid in the presence of nitric acid, manganese(II) nitrate is
formed:
MnO2 + HNO2 + HNO3 → Mn(NO3)2 + H2O
Reaction with potassium bifluoride in the presence of hydrofluoric acid creates
a stable complex fluoride, K2MnF6 in which Mn is in +4 oxidation state:
MnO2 + 2KHF2 + 2HF → K2MnF6 + 2H2O
When fused with basic oxides such as calcium oxide, manganites or manganate(
IV) salts such as CaO•MnO2, 2CaO•MnO2, CaO•3MnO2 are formed.
The stoichiometric compositions of these manganites vary.
Manganese(IV) oxide reacts with aniline in the presence of sulfuric acid
forming quinone, an intermediate product in the manufacture of hydroquinone:
4MnO2 + 2C6H5NH2 + 5H2SO4 → 2C6H4O2 + 4MnSO4 + (NH4)2SO4 + 4H2O
Analysis
Elemental composition: Mn 63.19%, O 36.81%. The pure oxide may be characterized
by x-ray crystallography. The MnO2 content in pyrolusite may be
measured by titration. An excess of a standard solution of oxalic acid is added
to a solution of MnO2 in sulfuric acid. After all solid MnO2 dissolves, the
excess oxalic acid is measured by titrating against a standard solution of
potassium permanganate (see Reactions).
Alternatively, pyrolusite is heated with concentrated hydrochloric acid and
MANGANESE(IV) OXIDE 555
the chlorine evolved is passed through a solution of potassium iodide. The
iodine liberated is titrated against a standard solution of sodium thiosulfate
using starch indicator. One mol MnO2 is equivalent to two mol thiosulfate.
Also, acid extracts of MnO2 may be diluted and measured by AA or ICP techniques
(See Manganese).




MANGANESE
[7439-96-5]
Symbol: Mn; atomic number 25; atomic weight 54.938; a Group VIIB
(Group 7) transition metal; electron configuration [Ar]4s23d7; atomic radius
1.27Å; valence 0, +1, +2, +3, +4, +5, +6, +7; most common oxidation states
+2, +4 and +7; stable natural isotope Mn-55 (100%)
History, Occurrence, and Uses
Manganese was recognized as an element by Scheele, Bergman and others
in 1774 and isolated by Gahn in the same year. Gahn obtained the metal by
thermal reduction of pyrolusite with carbon. The element derived its name
from the Latin word, magnes which means magnet, referring to the magnetic
properties of its ore pyrolusite.
Manganese is distributed widely in nature, mostly as oxide, silicate, and
carbonate ores. Manganese ores often are found in association with iron ores
in small quantities. The element, however, does not occur naturally in native
form. Manganese is the twelfth most abundant element in the earth’s crust.
538 MANGANESE
Its concentration in the earth’s crust is estimated to be 0.095%. Its average
concentration in seawater is 2μg/L. Manganese also is found in large quantities
in deep-sea nodules over the ocean floor at depths of 2.5 to 4 miles. The
composition of some common manganese minerals is tabulated below:
Mineral CAS Registry Number Composition
Pyrolusite [14854-26-3] MnO2
Manganite [52019-58-6] Mn2O3•H2O
Hausmannite [1309-55-3] Mn3O4
Rhodochrosite [598-62-9] MnCO3
Rhodonite [14567-57-8] MnSiO3
Bementite [66733-93-5] Mn8Si6O15(OH)10
Braunite — — — 3Mn2O3•MnSiO3
Psilomelane [12322-95-1] BaMnIIMnIV8O16(OH)4
Manganese is used widely in industry: the most important use is in ferrous
metallurgy. It also is used in chemical, electrochemical, food and pharmaceutical
applications. Ferromanganese alloys are used in steel manufacturing.
Manganese serves as a deoxidizer of molten steel and controls its sulfur content.
Manganese metal also enhances strength and hardness of the alloy, and
its resistance to corrosion. Manganese is used in high-temperature steels,
stainless steels, manganese steel and various nickel-chromium and manganese-
aluminum alloys. Practically all aluminum and magnesium alloys
contain manganese.
Manganese is an essential element for plants and animals. Its shortage in
soil can cause chlorosis or lack of chlorophyll in plants—manifested by the
appearance of yellow or grey streaks on the leaves or mottling. It activates
certain plant enzymes, such as oxalosuccinic decacarboxylase in the oxidation
of carbohydrates. Manganese deficiency can cause deformity of bones in animals.
In chemical industries, manganese is used to prepare several compounds.
It also is used as a catalyst. Its salts have numerous applications in oxidation,
catalysis, and medicine.
Physical Properties
Reddish-gray metal; exists in four allotropic modifications: alpha-, beta-,
gamma- and delta forms. Alpha form has cubic crystal structure; 58 atoms per
unit cell; density 7.43 g/cm3; brittle; transforms to beta form at 720°C. Betamanganese
is brittle and has a cubic lattice structure; containing 20 atoms
per unit cube; transforms to gamma form at 1,100°C or back to alpha form on
cooling; density 7.29 g/cm3. The gamma form exists as face-centered cubic
crystal containing 4 atoms per unit cell; density 7.18 g/cm3; converts to delta
form at 1,136°C. Delta-manganese consists of body-centered cubic crystals
containing 2 atoms per unit cube; density 6.30 g/cm3; stable up to 1,244°C
above which it melts to liquid.
Manganese vaporizes at 2,097°C; vapor pressure 0.9 torr at 1,244°C; hardness
5.0 (Mohs scale); magnetic susceptibility 9.9 cgs units at 18°C; electrical
MANGANESE 539
resistivities 185, 44, and 60 microhm–cm at 20°C for alpha-, beta- and gamma
allotropes respectively; thermal neutron absorption 13.2 barns.
Thermochemical Properties
ΔHƒ° (Mn-alpha) 0.0 kcal/mol
ΔHƒ° (Mn-gamma) 0.37 kcal/mol
ΔHƒ° (Mn-gas) 67.1 kcal/mol
ΔGƒ° ( Mn-alpha) 0.0 kcal/mol
ΔGƒ° ( Mn-gamma) 0.34 kcal/mol
ΔGƒ° ( Mn-gas) 57.0 kcal/mol
S° ( Mn-alpha) 7.65 cal/degree mol
S° (Mn-beta) 8.22 cal/degree mol
S° ( Mn-gamma) 7.75 cal/degree mol
S° (Mn-gas) 41.49 cal/degree mol
Cρ (Mn-alpha) 6.29 cal/degree mol
Cρ (Mn-beta) 6.34 cal/degree mol
Cρ (Mn-gamma) 6.59 cal/degree mol
Cρ (Mn-gas) 4.97 cal/degree mol
ΔHfus 3.516 kcal/mol
Coefficeint of linear expansion (at 25°C) 22x10–6/°C
Production
Manganese is recovered primarily from its oxide ores, the most important
being pyrolusite, MnO2. The basic method of producing the metal has not
changed much since Gahn first isolated it by reducing manganese dioxide
with carbon. Several processes to produce manganese meet its high demand
in ferrous metallurgy. The oxides are reduced thermally in an electric furnace
or a blast furnace. The ore is smelted at high temperatures in the presence of
carbon, which reduces higher oxides of manganese, MnO2, Mn2O3, and Mn3O4
into MnO, and then forms metallic manganese which has a relatively high
vapor pressure:
MnO2 + C → MnO + CO
Mn3O4 + C → 3MnO + CO
MnO + C → Mn + CO
Selection of the process depends on the requirement of the product, such as
high-carbon or low-carbon ferromanganese or silicomanganese of varying carbon
contents. Usually coke is used as a reducing agent for high-carbon ferromanganese
for the steel industry. Low-carbon ferromanganese, silicomanganese,
or refined ferromanganese that has low carbon content ranging from
0.1 to 1.5% maximum carbon, may be obtained by using silicon as a reducing
agent:
MnO2 + Si → Mn + SiO2
540 MANGANESE
Mn3O4 + 2Si → 3Mn + SiO2
2MnO + Si → 2Mn + SiO2
Often, the manganese ores contain several other naturally occurring metal
oxides such as alumina, silica, magnesia, and lime. Some of these oxides may
be blended into manganese ore as fluxes to the furnace charge.
Manganese may be produced by electrolytic processes. Aqueous solutions of
manganese(II) sulfate are used as the electrolyte. Mn ore is roasted and
reduced with carbon or silicon to convert the higher oxides of manganese into
MnO. The products are then leached with dilute sulfuric acid at pH 3. MnO
dissolves in the acid forming manganese(II) sulfate. The solution is filtered
and separated from insoluble residues. It then is neturalized with ammonia
to pH 6–7.
Iron and aluminum precipitate out when treated with ammonia and are
removed by filtration. Other metals, such as copper, zinc, lead and arsenic are
precipitated and removed as sulfides upon passing hydrogen sufide through
the solution. Colloidal particles of metallic sulfides and sulfur are removed by
treatment with iron(II) sulfide. The purified solution of manganese(II) sulfate
is then electrolyzed in an electrolytic cell using lead anode and Hastelloy or
Type 316 stainless steel cathode, both of which are resistant to acid.
Manganese is deposited on the cathode as a thin film.
Manganese also is produced by electrolysis of fused salt. In one such
process, the reduced MnO is blended to molten calcium fluoride and lime. The
latter is used to neutralize silica in the ore. The fused composition of these
salts is electrolyzed at 1,300°C in an electrolytic cell made up of high temperature
ceramic material, using a carbon anode and a cathode consisting of iron
bars internally cooled by water.
Reactions
Manganese forms compounds in several valence states: 0, +1, +2, +3, +4,
+5, +6, and + 7. Of these, the valences 0, +1, and +5 are very uncommon. The
divalent salts are the most stable. While in the divalent state, the metal is a
reducing agent; in tetravalent state it is an oxidizing agent. Heptavalent manganese
(Mn7+) is a powerful oxidizing agent. Some examples of Mn compounds
in all these oxidation states are tabulated below:
Oxidation State Example
Mn(O) Mn2(CO)10
Mn(I) C9H7Mn(CO)3
Mn(II) MnCl2; MnSO4; MnO
Mn(III) MnF3; Mn2O3
Mn(IV) MnO2; K2MnO3
Mn(V) K3MnO4
Mn(VI) K2MnO4; BaMnO4
Mn(VII) KMnO4; Mn2O7
MANGANESE 541
Many chemical properties of manganese are similar to iron. Manganese
burns in air or oxygen at elevated temperatures forming trimanganese tetroxide:
3Mn + 2O2 → Mn3O4
The metal reacts slowly with water in cold, forming manganous hydroxide
with the evolution of hydrogen:
Mn + 2H2O → Mn(OH)2 + H2
The reaction is usually slow below 100°C, but proceeds rapidly upon heating.
Manganese reacts readily with dilute mineral acids forming their divalent
salts and liberating hydrogen:
Mn + 2HCl → MnCl2 + H2
Mn + H2SO4 → MnSO4 + H2
Manganese forms manganese(II) halides when heated with halogens. With
fluorine, reaction is very vigorous and the products are MnF2 and MnF3:
Mn + Cl2 → MnCl2
Mn + F2 → MnF2
2Mn + 3F2 → 2MnF3
When heated with sulfur, the product is manganese(II) sulfide, MnS2.
Manganese combines with carbon or silicon at elevated temperatures forming
a series of carbides or silicides having compositions such as Mn2C7, Mn3C,
Mn7C3 and Mn15C4 or MnSi, Mn3Si and Mn5Si3. Manganese reacts with nitrogen
above 750°C forming various nitrides, such as Mn3N2, Mn5N2 and Mn4N.
The metal ignites in nitrogen at 1,200°C, then burns with a heavy, smoky
flame forming the above nitrides. The principal product is Mn3N2. Also reaction
with anhydrous ammonia above 350°C yields several nitrides of varying
composition.
Manganese dissolves in concentrated alkali in boiling solutions forming
manganese(II) hydroxide and hydrogen. However, in the presence of excess
oxygen or under oxygen pressure, the product is a manganate:
2Mn + 4KOH + 3O2 → 2K2MnO4 + 2H2O
Reactions with concentrated acids are slow at room temperature, but rapid
when heated. No hydrogen forms in concentrated acids. With concentrated
sulfuric and nitric acids, sulfur dioxide and nitric oxide form:
Mn + 2H2SO4 → MnSO4 + SO2 + 2H2O
542 MANGANESE
Mn + 2HNO3 → MnNO3 + NO + 2H2O
Manganese combines with several metals at elevated temperatures forming
binary compounds in varying compositions. Such metals include Al, Zn, Ni,
Sn, As, Sb, Be, Pd, and Au.
Analysis
Manganese in aqueous solution may be analyzed by several instrumental
techniques including flame and furnace AA, ICP, ICP-MS, x-ray fluorescence
and neutron activation. For atomic absorption and emission spectrometric
determination the measurement may be done at the wavelengths 279.5,
257.61 or 294.92 nm respectively. The metal or its insoluble compounds must
be digested with nitric acid alone or in combination with another acid. Soluble
salts may be dissolved in water and the aqueous solution analyzed. X-ray
methods may be applied for non-destructive determination of the metal. The
detection limits in these methods are higher than those obtained by the AA or
ICP methods. ICP-MS is the most sensitive technique. Several colorimetric
methods also are known, but such measurements require that the manganese
salts be aqueous. These methods are susceptible to interference.
Manganese produces violet color in an oxidizing flame on a microcosmic or
borax bead. The color disappears in a reducing flame.
Toxicity
Although trace amounts of manganese are essential for animals, in large
quantities the metal can cause acute and chronic poisoning. Chronic inhalation
of metal dust or fumes can cause manganism, a nonfatal disease affecting
the central nervous system. The symptoms are mental disorder and disturbance
in speech.


Wydaje mi się iz masz tu wszystkie wstepnie neizbedne informacje aby rozpoczac intymne spotkanie z flakami bateryjki.
Milej lektory i owocnej syntezy.

Dzięki crazyuserze Teraz mogę spokojnie wejść w życie intymne manganu i jego związków

W niektórych miejscach, zamiast liter pojawiają się pewne dziwne znaki np. :
MnO2 + 2KOH + ½ O2 → K2MnO4 + H2O

3MnO42– + 2H2O → 2MnO4¯ + MnO2 + 4OH¯

i moja ostatnia prośba : Czy mógłbyś mi odsłonić tajniki tego szyfru

to takie brzydkie słowo na h.... html
na PW cos ci wysylam
nie wiem czy dopelznie

Nie chce zakładać kolejnego tematu, a moje pytanie ma związek z manganem. Na pewno wielokrotnie już mieliście doczynienia z Mn(OH)2, jak wiadomo szybko utlenia sie, pozostawiamy probówkę z osadem na pare minut i obserwujemy jego ciemnienie. Oczywiście można osad potraktować H2O2 i teraz moje pytanie.. Czy moją odpowiedź że w wyniku utleniana osadu powstaje tam Mn2O3 można uznać za prawidłową?

YES YES YES

mo dobra teraaz snopeczek sianka :

MANGANESE(II) HYDROXIDE
[18933-05-6]
Formula: Mn(OH)2; MW 88.953
Synonyms: manganous hydroxide; pyrochroite
Occurrence: Manganese(II) hydroxide occurs naturally as the mineral
pyrochroite
Physical Properties
Pink hexagonal crystal; density 3.26 g/cm3; refractive index 1.68; Mohs
hardness 2.5; decomposes at 140°C; insoluble in water; KSP 5.61x10–12; soluble
in acid; dissolves in alkaline solution on heating.
Thermochemical Properties
ΔHƒ° –167.0 kcal/mol
ΔGƒ° –148.0 kcal/mol
S° 23.0 cal/degree mol
Preparation
Manganese(II) hydroxide is obtained as a white precipitate by adding a
solution of sodium or potassium hydroxide to a solution of manganese(II) salt,
such as manganese(II) chloride:
Mn2+ + 2OH¯ → Mn(OH)2
The white precipitate rapidly turns brownish-pink in air. The reaction does
not occur with ammonia in the presence of ammonium salt.
The hydroxide also is found in nature as mineral pyrochroite in the form of
white transparent leaflets. The white leaflets turn pink on exposure to air.
Reactions
Manganese(II) hydroxide is a base exhibiting weak amphoteric behavior. It
reacts with acids forming the corresponding manganese(II) salt:
Mn(OH)2 + 2KOH → K2Mn(OH)4
The hydroxide is rapidly oxidized in air forming manganese(III) oxide, Mn2O3.
548 MANGANESE(II) HYDROXIDE
Analysis
Elemental composition: Mn 61.76%, H 2.27%, O 35.97%. The compound is
digested in nitric acid and analyzed for manganese by AA, ICP or other instrumental
technique.

Mój pierwszy głupi pomysł otrzymania Al(MnO4)3

W książce, która wpadła w moje ręce dzięki crazyuserowi ( jeszcze raz dzięki Ci za to crazyuserze ) jest taka reakcja :

MnO2 + 2KOH + 0,5 O2---->K2MnO4 + H2O

Po moim przekombinowaniu

12MnO2 + 4Al(OH)3 + 9O2 ----> 4Al(MnO4)3 + 6H2O

Jak źle wyrównałem to wybaczcie

Jest tam również napisane, że zamiast tlenu może być inny związek utleniający, więc np H2O2

Co o tym sądzicie ( w pierszym jest Mn 6+, bo jest zasadowy, a w drugim Mn7+, bo odczyn nie jest zasadowy )

H2O2 nie będzie, nie pamiętam teraz całej tabeli ale H2O2 nie utleni Ci MnO2. Proponuje KClO3 Pomijam, że ta reakcja z Al(OH)3 wydaje mi się..hmm...nieco dziwna.

No raczej... za słaba zasada.

Trudno nawet mówić o zasadzie bo wodorotlenek glinu jakoś szczególnie to się w wodzie nie rozpuszcza

H2O2 to nie jedyny utlenaicz na swiecie, poza tym warto zapytac co to jest H2O2 ?
widze ze do supniewskiego sie nawe nei zajrzalo
warto zwrocic uwage iz generalnie wszedzie wspomina sie o metalach alkalicznych a wyglad iz pozostale moga sie zachowywac raczej inaczej, choc ten artykl daje do myslenai dlaczego wlasnei jako produkt przejsciowy uzywano Al-pm

Proponowwane do obejrzenia linki :
http://www.sciencemadness.org/talk/view ... =8480&page
(całość a nie tylko poczatek )
http://www.freshpatents.com/Electrochem ... 012570.php

Właśnie tak się zastanawiam, że jeżeli koniecznie musi być metal alkaliczny, to można użyć litu ( węglan litu jest substancją trudno rozpuszczalną w wodzie), a jeżeli nie musi być metalem alkalicznym, to można użyć wapnia ( kilka soli wapnia jest trudno rozpuszczalnych w wodzie).

Na stronce, którą podał crazyuser jako utleniacze są używane chlorany (I). Czy można zamiast nich używać azotanów (V) ( saletry chyba też są dość dobrymi utleniaczami ) Jeżeli zamiast potasu użyć wapnia, to taka reakcja :


2MnO2 + Ca(ClO)2 + 2Ca(OH)2 --> 2CaMnO4 + CaCl2 + 2H2O

3MnO4 2- + 2H2O ----> 2 MnO4 - + MnO2 + 4OH -

po tej reakcji powinien już być manganian (VII) wapnia

3Ca(MnO4)2 + Al2(SO4)3 ----> 2Al(MnO4)3 + 3CaSO4

Miałbym po pierwszej reakcji problem jak oddzielić CaCl2 i Ca(MnO4)2, więc czy mógłby mi ktoś napisać reakcję, w której zamiast Ca(ClO)2 byłby Ca(NO3)2 ( Jeśli Ca(NO3)2 nie jest za słabym utleniaczem )

moze byc cos takiego ?

MnO2 + Ca(NO3)2 = CaMnO4 + 2 NO2

Widze ze to jednak badania podstawowe i to ostre

robi sie z tego pomieszanie z poplataniem , hipotetyczne reakcje z prawdziwymi, reakcje w roztworach z reakcjami soli stopionych i elektrochemicznymi ...
pora aby pan docent Kryształoman wniosl cos wiecej do tematu oprocz zamawiania artow, danych i rownan reakcji.

/me oglasza straik - pan docent Kryształoman powinien choc czytac dokladniej