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Manganese(II) oxalate dihydrate (MnOx) occurs naturally as the mineral Lindbergite.
Manganese(II) oxalate dihydrate (MnOx), is an inorganic compound with the chemical formula MnC₂O₄·2H₂O.
Manganese(II) oxalate dihydrate (MnOx) consists of divalent manganese (Mn²⁺) ions coordinated with oxalate (C₂O₄²⁻) anions and is further stabilized by two molecules of water of crystallization.
CAS Number: 6556-16-7
Molecular Formula: C2H2MnO6
Molecular Weight: 176.97
EINECS Number: 211-367-3
Synonyms:6556-16-7, Manganese(II) Oxalate Dihydrate, Manganese oxalate,dihydrate, manganese, oxalic acid, dihydrate, MFCD00150452, Manganese(II) oxalate dihydrate, Mn 30%, Manganese,diaqua[ethanedioato(2-)-ko1,ko2]-,(t-4)-, MANGANESE OXALATE, DIHYDRATE, MANGANESE(II) OXALATE, MANGANESE(II) OXALATE, DIHYDRATE, MANGANESE(II) OXALATE DIHYDRATE 97+%, Manganese(II) oxalate dihydrate, Mn 30% min, Manganese (II) Oxaltate, Manganous oxalate dihydrate, Oxalic acid manganese(II)·dihydrate
Manganese(II) oxalate dihydrate (MnOx) is an inorganic compound with the chemical formula MnC2O4.
Solid samples are pale pink and insoluble in water.
At least two hydrates have been observed.
Manganese(II) oxalate dihydrate (MnOx) typically appears as a pale pink to light rose-colored crystalline solid, which is characteristic of many manganese(II) salts.
Manganese(II) oxalate dihydrate (MnOx) is only slightly soluble in water but more soluble in acidic solutions, where the oxalate ligand can form stable complexes with manganese ions.
Manganese(II) oxalate dihydrate (MnOx) is primarily synthesized through the precipitation reaction between soluble manganese salts, such as manganese(II) chloride or manganese(II) sulfate, and oxalic acid or soluble oxalates under aqueous conditions.
The resulting precipitate is washed and dried to obtain the crystalline dihydrate form. When heated, this compound undergoes dehydration and thermal decomposition, eventually yielding manganese oxide (MnO) and releasing carbon monoxide (CO) and carbon dioxide (CO₂) gases.
This thermal behavior makes it an important precursor in the synthesis of manganese oxides with various oxidation states, which have applications in catalysis, energy storage, and material science.
From a structural perspective, the oxalate anion acts as a bidentate ligand, coordinating through its two oxygen atoms to the manganese center, forming a chelated structure.
The water molecules in the dihydrate form are usually hydrogen-bonded to the oxalate groups or coordinated to the manganese ion, contributing to the stability of the crystal lattice.
The crystalline structure and bonding environment can be studied through techniques such as X-ray diffraction (XRD), infrared spectroscopy (FT-IR), and thermogravimetric analysis (TGA), which provide insights into its thermal stability, coordination behavior, and phase transitions.
Manganese(II) oxalate dihydrate (MnOx) is of scientific and industrial interest because it can serve as a precursor for producing nanosized manganese oxides, which exhibit excellent catalytic, magnetic, and electrochemical properties.
For example, MnO and Mn₃O₄ derived from the controlled decomposition of this compound are widely investigated for use in lithium-ion battery electrodes, supercapacitors, and environmental catalysts.
Additionally, due to the oxalate component, the compound can participate in redox reactions under thermal or photochemical conditions, making it relevant in studies involving decomposition kinetics and reactive intermediate formation.
In terms of safety, Manganese(II) oxalate dihydrate (MnOx) should be handled with care because manganese compounds can be toxic if inhaled or ingested in large quantities, and oxalates are known to form insoluble calcium oxalate in biological systems, potentially leading to health issues.
Therefore, appropriate personal protective equipment, such as gloves, goggles, and dust masks, is recommended when handling this compound in laboratory or industrial settings.
Manganese(II) oxalate dihydrate (MnOx) is a crystalline coordination compound with intriguing structural, thermal, and chemical properties, widely utilized as a precursor in material synthesis, particularly for applications that exploit the unique properties of manganese-based oxides.
Melting point: 100°C
Density: 2.453
Solubility: soluble in acid solutions
Form: white crystalline powder
Specific Gravity: 2.453
Color: white crystals, crystalline powder
Water Solubility: Soluble in dilute acids. Slightly soluble in water.
Merck: 14,5734
Solubility Product Constant (Ksp): pKsp: 6.77
Exposure limits: ACGIH: TWA 0.02 mg/m3, TWA 0.1 mg/m3
Manganese(II) oxalate dihydrate (MnOx) in shorthand notation in certain contexts, is a coordination compound that belongs to the family of transition metal oxalates.
Manganese(II) oxalate dihydrate (MnOx) features manganese in the +2 oxidation state, which is coordinated by the oxalate anion, a dicarboxylate ligand known for its strong chelating ability.
The presence of two water molecules in its crystalline lattice classifies it as a dihydrate, and these water molecules play an essential role in stabilizing the crystal structure through hydrogen bonding and, in some cases, weak coordination with the manganese center.
Manganese(II) oxalate dihydrate (MnOx) is typically obtained as a fine crystalline powder with a distinct light pink coloration, a hue that arises from the electronic d–d transitions within the Mn²⁺ ion under visible light.
From a crystallographic perspective, Manganese(II) oxalate dihydrate (MnOx) generally crystallizes in a monoclinic structure, where each manganese ion is surrounded by oxygen atoms originating from both oxalate ligands and water molecules, forming an extended three-dimensional network.
The oxalate ions bridge between manganese centers, giving rise to polymeric chains or layers depending on the crystal packing.
The hydrogen-bond network provided by the lattice water further enhances the rigidity and stability of the structure.
Manganese(II) oxalate dihydrate (MnOx) exhibits several physicochemical properties that make it an attractive subject of research.
It is only sparingly soluble in water, yet its solubility increases in acidic environments where the oxalate ligand can be protonated and manganese ions can be released into the solution.
Manganese(II) oxalate dihydrate (MnOx)s decomposition is of particular interest: upon heating, manganese(II) oxalate dihydrate first undergoes a stepwise dehydration, losing its crystallization water at relatively low temperatures (around 150–200 °C).
Subsequently, at higher temperatures, the anhydrous manganese(II) oxalate decomposes to produce manganese(II) oxide (MnO) while evolving carbon monoxide and carbon dioxide gases.
This decomposition process is endothermic and has been extensively studied through thermogravimetric analysis (TGA), differential scanning calorimetry (DSC), and mass spectrometry to understand its kinetics and mechanisms.
The importance of manganese(II) oxalate dihydrate extends far beyond its basic chemical identity.
Manganese(II) oxalate dihydrate (MnOx) serves as a versatile precursor for the preparation of a wide range of manganese oxides, including MnO, Mn₃O₄, and Mn₂O₃, which are valued for their catalytic properties, magnetic behaviors, and electrochemical performance.
For example, nanoscale Mn₃O₄ produced from the thermal decomposition of manganese(II) oxalate has been widely applied as an anode material in lithium-ion batteries, where it offers high specific capacity and cycling stability.
Furthermore, manganese oxides derived from this compound are frequently employed as catalysts in oxidation reactions, gas sensors, and materials for environmental remediation, owing to their high surface area, tunable oxidation states, and robust redox activity.
In research involving material science and nanotechnology, Manganese(II) oxalate dihydrate (MnOx) has been utilized as a template material, allowing researchers to control the morphology of the resulting oxide through modification of synthesis parameters such as pH, temperature, and the use of surfactants or dopants.
This makes it highly relevant in the development of advanced functional materials, particularly in energy storage devices, where morphology plays a crucial role in electrochemical performance.
From an environmental and biological standpoint, manganese is an essential trace element in many organisms, functioning as a cofactor in various enzymes.
However, the oxalate component poses potential health risks because oxalates can chelate calcium and form insoluble calcium oxalate crystals in the body, which are associated with kidney stone formation.
Therefore, despite its usefulness, Manganese(II) oxalate dihydrate (MnOx) must be handled with caution in both laboratory and industrial contexts to minimize exposure.
Manganese(II) oxalate dihydrate (MnOx) forms light pink crystals.
The crystalline hydrates have the composition MnC2O4•n H2O, where n = 2 and 3.
The dihydrate forms light pink crystals of the orthorhombic system, space group P212121, cell parameters a = 0.6262 nm, b = 1.3585 nm, c = 0.6091 nm, Z = 4, melts in its own crystallization water at 100 °C.
Manganese(II) oxalate dihydrate (MnOx) is not only an inorganic salt with an aesthetically pleasing crystalline form but also a material of considerable scientific interest.
Its unique combination of coordination chemistry, thermal behavior, and ability to serve as a precursor for technologically important manganese oxides positions it at the intersection of fundamental research and practical applications in catalysis, energy storage, magnetism, and environmental technology.
Additionally, the compound’s properties have made it a model system in studies of thermal decomposition, coordination chemistry, and solid-state transformations.
Spectroscopic techniques such as infrared (IR) spectroscopy reveal characteristic vibrations of the oxalate ligand, including symmetric and asymmetric stretching of the C=O and C–O bonds, which shift during dehydration and decomposition.
X-ray diffraction (XRD) analysis can track changes in crystal structure as the compound undergoes thermal treatment, while electron microscopy (SEM/TEM) helps in observing the morphological evolution of particles during these transformations.
Uses Of Manganese(II) oxalate dihydrate (MnOx):
Manganese(II) oxalate dihydrate (MnOx) is used as a paint and varnish drier.
Manganese(II) oxalate dihydrate (MnOx) is also used as a chemical reagent as well as to prepare other manganese compounds.
In addition, it is used as a semiconductor photosensitive material.
Manganese(II) oxalate dihydrate (MnOx) (MnC₂O₄·2H₂O) has a variety of uses that stem from its unique structural, chemical, and thermal properties, making it an important material in both industrial and research contexts.
One of its most significant uses is as a precursor for the controlled synthesis of manganese-based oxides, such as MnO, Mn₃O₄, and Mn₂O₃, which are materials with outstanding catalytic, magnetic, and electrochemical properties.
These oxides are widely utilized in energy storage devices, particularly in lithium-ion batteries, where they function as active electrode materials that provide high specific capacity, excellent cycling stability, and improved rate capability due to their ability to undergo reversible redox reactions involving multiple oxidation states of manganese.
Another prominent application is in the preparation of catalysts for various chemical reactions, including oxidation processes, decomposition reactions, and environmental remediation.
Manganese oxides derived from Manganese(II) oxalate dihydrate (MnOx) exhibit a high surface area, abundant active sites, and strong catalytic activity, making them suitable for use in processes such as the catalytic combustion of pollutants, the degradation of organic dyes in wastewater treatment, and the removal of nitrogen oxides from exhaust gases.
Furthermore, because manganese oxides can exist in multiple oxidation states, they facilitate redox reactions efficiently, which is advantageous for catalytic applications in both industrial and environmental fields.
In the field of nanotechnology and advanced materials,Manganese(II) oxalate dihydrate (MnOx) is employed as a template or precursor to create nanostructured manganese oxides with specific morphologies, such as nanorods, nanoflakes, or hollow spheres.
By controlling the synthesis conditions, researchers can tailor the size, shape, and surface properties of these oxides, which in turn enhances their performance in applications like supercapacitors, where fast ion diffusion and large surface area are critical for achieving high energy storage efficiency.
These nanostructured oxides are also being investigated for their use in hybrid energy systems, including lithium–air batteries and other next-generation storage technologies.
Additionally, Manganese(II) oxalate dihydrate (MnOx) finds application in magnetic materials research because manganese oxides derived from its decomposition display interesting magnetic properties, including ferrimagnetism and antiferromagnetism, depending on their crystalline phase and particle size.
These properties make them valuable in the design of magnetic sensors, recording devices, and other magnetic components.
In some cases, these manganese oxides also show potential as microwave absorption materials, which can be applied in electromagnetic interference (EMI) shielding and stealth technologies.
Beyond energy and catalysis, Manganese(II) oxalate dihydrate (MnOx) has been used as a chemical reagent and a model compound in studies of thermal decomposition and solid-state transformations.
Because its decomposition pathway is well-defined and produces identifiable gaseous products (such as CO and CO₂), it is often used to investigate the kinetics and mechanisms of thermal reactions in coordination compounds.
These studies not only expand fundamental knowledge in chemistry but also contribute to optimizing industrial processes where controlled thermal decomposition is essential.
Moreover, manganese oxides produced from Manganese(II) oxalate dihydrate (MnOx) have been incorporated into environmental applications such as the adsorption and oxidation of heavy metal ions and toxic gases.
Their high reactivity allows them to play a role in advanced water purification systems and air-cleaning technologies, helping to mitigate environmental pollution.
The use of these materials in environmental protection is gaining attention as industries move toward more sustainable and green technologies.
In summary, the uses of Manganese(II) oxalate dihydrate (MnOx) extend from serving as a critical precursor for high-performance manganese oxides in energy storage and catalysis to being a valuable compound for fundamental studies in chemistry and material science.
Manganese(II) oxalate dihydrate (MnOx)s ability to transform into various functional manganese oxides under controlled conditions allows researchers and industries to exploit its properties in a wide range of applications, including batteries, supercapacitors, catalytic converters, environmental remediation systems, magnetic devices, and electromagnetic shielding materials.
Manganese(II) oxalate dihydrate (MnOx) (MnC₂O₄·2H₂O) also plays an important role in several niche applications where its chemical reactivity, decomposition behavior, and coordination chemistry can be strategically utilized.
For example, in the field of ceramic and glass manufacturing, manganese oxides derived from this compound are used as additives that modify the optical, mechanical, and electrical properties of the final materials.
The presence of manganese oxides can improve the coloration of glass, impart specific magnetic characteristics, and enhance the dielectric properties of ceramic components, making them more suitable for applications in electronics, telecommunications, and decorative industries.
In electrochemical devices, manganese oxides obtained from the thermal decomposition of Manganese(II) oxalate dihydrate (MnOx) are increasingly applied as low-cost, non-toxic alternatives to noble-metal-based catalysts in fuel cells and metal–air batteries.
These oxides exhibit excellent oxygen reduction reaction (ORR) and oxygen evolution reaction (OER) activities, which are crucial for the efficient operation of such energy conversion systems.
The use of manganese-based materials in these devices reduces costs while maintaining good performance, supporting the ongoing transition toward more sustainable energy technologies.
The compound also finds research use in gas sensing technology, where manganese oxides derived from MnC₂O₄·2H₂O demonstrate high sensitivity and selectivity toward gases such as CO, NOx, and volatile organic compounds (VOCs).
Their large surface area and active catalytic sites allow for rapid detection of these gases at low concentrations, which is critical for industrial safety, environmental monitoring, and the development of smart sensing devices.
In biomedical research, manganese oxides obtained from Manganese(II) oxalate dihydrate (MnOx) have been studied as potential materials for use in drug delivery systems and as contrast agents for magnetic resonance imaging (MRI).
Manganese is known to enhance MRI signals due to its paramagnetic properties, and nanosized manganese oxides prepared from this compound can be engineered to interact with biological tissues in a controlled manner.
Additionally, these materials are being investigated for their role in reactive oxygen species (ROS) scavenging, which can have therapeutic benefits in treating oxidative stress-related diseases.
Another emerging application is in environmental catalysis, where manganese oxides derived from MnC₂O₄·2H₂O are incorporated into photocatalytic and electrocatalytic systems for water splitting, pollutant degradation, and carbon dioxide reduction.
These applications benefit from the ability of manganese oxides to cycle between multiple oxidation states, thereby facilitating electron transfer processes that drive these environmentally significant reactions.
Manganese(II) oxalate dihydrate (MnOx) is sometimes employed in the synthesis of composite materials, where it acts as a source of manganese for hybrid structures combining oxides with carbon-based materials, polymers, or other metal oxides.
For example, when combined with multi-walled carbon nanotubes (MWCNTs), graphene, or polyaniline, the derived manganese oxides form composites with enhanced electrical conductivity, mechanical stability, and electromagnetic wave absorption capabilities.
Such composites are of particular interest in the development of advanced electromagnetic interference (EMI) shielding materials and microwave absorbers, where both dielectric and magnetic losses contribute to effective wave attenuation.
Safety Profile Of Manganese(II) oxalate dihydrate (MnOx):
Manganese(II) oxalate dihydrate (MnOx) presents several hazards that should be carefully considered when handling or storing the compound, as both the manganese and oxalate components can pose health and safety risks under certain conditions.
The primary hazard arises from its toxicity if inhaled, ingested, or absorbed through the skin.
Manganese, although an essential trace element in small quantities, can cause neurological damage when exposure is excessive, leading to a condition known as manganism, which resembles Parkinson’s disease and involves symptoms such as tremors, difficulty walking, and impaired motor coordination.
Long-term or repeated exposure to manganese dusts or fumes may also affect the respiratory system and central nervous system.
The oxalate component of Manganese(II) oxalate dihydrate (MnOx) adds another layer of risk, as oxalates are known to be harmful if ingested.
They can bind to calcium in the body to form insoluble calcium oxalate crystals, which can deposit in the kidneys and potentially lead to kidney stones or even kidney damage in severe cases.
Oxalates may also cause irritation to the gastrointestinal tract, resulting in abdominal pain, nausea, and vomiting upon ingestion.
Furthermore, contact with the eyes or skin can lead to irritation, redness, and discomfort, particularly if proper protective measures are not taken.
From an inhalation perspective, fine dust or powder of Manganese(II) oxalate dihydrate (MnOx) can irritate the respiratory tract and lungs.
Prolonged inhalation of dust particles may contribute to lung diseases or systemic manganese toxicity.
Therefore, working with the compound in a well-ventilated area, preferably under a fume hood, is strongly recommended to prevent dust exposure.
