Manganese

Manganese — Material Page

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Manganese (Mn, atomic number 25) is a hard, brittle, silvery-gray Group 7 transition metal that is the twelfth most abundant element in Earth's crust (~950 ppm) and the fourth most consumed metal globally after iron, aluminum, and copper — consumed almost entirely as an alloying addition to steel. Pure manganese adopts a complex cubic crystal structure (α-Mn, body-centered cubic with 58 atoms per unit cell) at room temperature, transforming through β, γ, and δ allotropes at progressively higher temperatures before melting at 1,246 °C. It is monoisotopic — ⁵⁵Mn is the only stable isotope, a rarity among Period 4 transition metals — and has an unusually wide range of stable oxidation states in compounds: +2, +3, +4, +6, and +7, each with distinct and useful chemistry. Despite the metal's brittleness in pure form (it cannot be worked cold and must be used as a powder or as an alloying addition), manganese compounds and alloys are indispensable across steelmaking, electrochemistry, catalysis, and biology. Manganese is an essential trace micronutrient — the active metal in manganese superoxide dismutase (MnSOD), the mitochondrial antioxidant enzyme, and in the Mn₄CaO₅ oxygen-evolving complex (OEC) of photosystem II that performs the biological water oxidation reaction underpinning all oxygenic photosynthesis.

Manganese's overwhelmingly dominant application — consuming approximately 90% of global production (~20 million tonnes/year of manganese ore) — is as an alloying addition to steel, where it serves two distinct roles: deoxidation/desulfurization during steelmaking, and solid-solution and microstructural strengthening in the finished steel. In steelmaking, manganese reacts preferentially with dissolved oxygen and sulfur in the steel melt (forming MnO and MnS inclusions that are removed in the slag), preventing sulfur embrittlement (hot shortness) that plagued early steels — Robert Forester Mushet's discovery of spiegeleisen (Mn-Fe-C alloy) addition to Bessemer steel in 1856 was the pivotal metallurgical breakthrough that made Bessemer steel commercially viable. In the finished steel, manganese stabilizes austenite, refines the pearlitic microstructure, increases hardenability (allowing through-hardening of thicker sections), and enables solid-solution strengthening at 0.5–2 wt% additions present in virtually all structural steels. High-manganese steels (Hadfield steel: 11–14 wt% Mn) are fully austenitic and undergo work-hardening during impact — achieving surface hardness of 500–800 HV while retaining high toughness — making them the material of choice for rock-crushing equipment, railroad crossings, and armored vehicle tracks. Advanced high-strength steels (AHSS) for automotive light-weighting — including TWIP (twinning-induced plasticity) steels with 15–30 wt% Mn achieving 800–1,000 MPa tensile strength with 40–80% elongation — represent one of the most active steel research frontiers.

Manganese's electrochemical versatility — spanning five oxidation states with accessible redox transitions — makes it central to battery technologies, water oxidation catalysis, and environmental remediation. MnO₂ (pyrolusite, Mn⁴⁺) is the cathode in alkaline and zinc-carbon primary batteries (Leclanché cells), with global consumption of ~400,000 tonnes/year of electrolytic manganese dioxide (EMD) — the largest single application of high-purity Mn. Lithium manganese oxide (LiMn₂O₄, LMO spinel) and lithium nickel manganese cobalt oxide (NMC: LiNiₓMnᵧCoᵤO₂) cathodes in lithium-ion batteries consume rapidly growing quantities of manganese, positioning Mn as a critical battery material as EV deployment scales. The Mn⁴⁺ → Mn²⁺ reduction in permanganate (MnO₄⁻, Mn⁷⁺) is one of the most widely used oxidimetric reactions in analytical chemistry and water treatment; potassium permanganate (KMnO₄) is a ubiquitous laboratory oxidant, disinfectant, and industrial water purification agent. Mn-based molecular catalysts for water oxidation — mimicking the biological Mn₄CaO₅ OEC — are an active area of artificial photosynthesis research.

General Properties

Property	Value	Notes
Atomic Number	25	Group 7, Period 4; transition metal; 3d⁵4s² electron configuration — a half-filled d shell, giving the highest number of unpaired electrons (5) of any element and contributing to paramagnetism in Mn²⁺; sits between chromium (24) and iron (26); monoisotopic (⁵⁵Mn, 100%), one of only 22 monoisotopic elements
Atomic Mass	54.938 u	Monoisotopic — ⁵⁵Mn is the only stable isotope; the monoisotopic nature simplifies mass spectrometric analysis of Mn but eliminates isotopic dilution options for IDMS concentration measurements; ⁵⁴Mn (t½ = 312 days) is the principal radioactive isotope, produced by cosmic ray spallation on iron and used as a gamma-ray calibration source (834.8 keV line)
Density (20 °C, α-Mn)	7.21 g/cm³	Moderate density, slightly less than iron (7.87 g/cm³); the complex α-Mn crystal structure (cubic, 58 atoms/unit cell, space group I–43m) with four distinct Mn site geometries gives it anomalously low density and high brittleness compared to neighboring transition metals; γ-Mn (FCC, above 1,095 °C) and δ-Mn (BCC, above 1,134 °C) are denser and less brittle but inaccessible at room temperature
Melting Point	1,246 °C (1,519 K)	Lower melting point than its Period 4 neighbors iron (1,538 °C) and chromium (1,907 °C); passes through four allotropic forms (α→β at 727 °C, β→γ at 1,095 °C, γ→δ at 1,134 °C) before melting; the low melting point relative to iron is relevant to steelmaking: Mn-Fe alloys (ferromanganese, silicomanganese) melt at lower temperatures than pure Mn, facilitating addition to steel melts
Boiling Point	2,061 °C (2,334 K)	Mn has relatively high vapor pressure at steelmaking temperatures — above ~1,600 °C in electric arc furnaces, significant Mn evaporation occurs from molten steel, requiring compositional adjustment and generating Mn-rich fume that requires careful occupational exposure control (OSHA PEL 1 mg/m³ as Mn fume); inhalation of Mn fume causes manganism (Parkinson's-like neurological disorder)
Thermal Conductivity	7.8 W/m·K	Very low thermal conductivity for a transition metal — lower than stainless steel (~15 W/m·K) and much lower than iron (80 W/m·K); reflects the complex α-Mn crystal structure with its large unit cell and multiple atom environments that strongly scatter phonons; Mn additions to steel reduce thermal conductivity, relevant to thermal management in high-Mn structural steels
Electrical Resistivity	1,440 nΩ·m (α-Mn, 20 °C)	Extraordinarily high electrical resistivity for a metal — approximately 85× that of iron; one of the highest resistivities of any pure metal, comparable to some stainless steels; reflects spin-disorder scattering from the complex antiferromagnetic structure of α-Mn; the resistivity decreases dramatically through the allotropic transitions (γ-Mn has resistivity ~185 nΩ·m — nearly 8× lower than α-Mn)
Crystal Structure	α-Mn: BCC-derived cubic (58 atoms/cell, Im–3m); β: 20 atoms/cell; γ: FCC; δ: BCC	α-Mn has one of the most complex crystal structures of any pure element — 58 atoms in the unit cell with four distinct coordination environments (Mn-I to Mn-IV sites); this complexity causes brittleness and low thermal conductivity; α-Mn is antiferromagnetic (TN = –173 °C, 100 K) with a complex non-collinear spin structure; the γ-Mn phase (FCC, paramagnetic) is stabilized at room temperature by alloying with Cu, Fe, or Ni to give Mn-based antiferromagnets and shape memory alloys

Mechanical Properties

Property	Value	Notes
Hardness	Mohs ~6; ~196 HV Vickers (α-Mn)	Hard but extremely brittle — pure manganese cannot be rolled, drawn, or forged; it fractures without plastic deformation at room temperature due to the complex α-Mn crystal structure with limited slip systems; the high hardness of Mn additions to steel (precipitation of MnC, Mn-rich austenite) contributes to the wear resistance of Hadfield steel and tool steels; Mn cannot be used as a structural metal in elemental form
Elastic (Young's) Modulus	198 GPa	Comparable to iron (211 GPa) despite the complex crystal structure; the high modulus combined with extreme brittleness means pure Mn has essentially no practical mechanical applications — it is used as a powder, flake, or alloying addition rather than as a structural metal; Mn additions to steel nominally increase the elastic modulus slightly through solid-solution effects
Brittleness	Completely brittle at room temperature; no measurable elongation	Pure α-Mn has zero ductility at room temperature — it is one of the few transition metals that cannot be mechanically worked in any form; this brittleness is a direct consequence of the complex crystal structure limiting dislocation motion; industrial Mn is supplied as electrolytic flake, broken pieces, or powder rather than rod or foil; the γ-Mn allotrope (FCC) is ductile but inaccessible at ambient conditions without alloying stabilization

Chemical Properties

Property	Value / Behavior	Notes
Oxidation States	+2 (MnO), +3 (Mn₂O₃), +4 (MnO₂), +6 (MnO₄²⁻), +7 (MnO₄⁻)	Manganese has the widest range of stable oxidation states of any transition metal in common use; Mn²⁺ is the most stable aqueous ion (pale pink, d⁵ high-spin), used as a Lewis acid catalyst and MRI contrast agent (MnCl₂); MnO₂ (Mn⁴⁺) is the cathode in alkaline batteries and a strong oxidant; MnO₄⁻ (permanganate, Mn⁷⁺) is an intense purple oxidant used in titrimetry, water treatment, and organic oxidation reactions; the Mn²⁺/MnO₄⁻ span of 1.51 V enables the full range of oxidimetric chemistry
Corrosion in Air	Oxidizes slowly; forms mixed MnO/Mn₂O₃/Mn₃O₄ scale	Manganese tarnishes in moist air at room temperature, forming a dull brown oxide layer; the oxide is not self-passivating in the way chromium or aluminum oxides are — the scale is porous and not protective over extended periods; dissolves readily in dilute mineral acids; Mn powder and fine flake present a dust explosion hazard (Class St 1)
Role in Steelmaking Chemistry	Deoxidizer (MnO), desulfurizer (MnS), austenite stabilizer	Mn preferentially reacts with dissolved O and S in steel melts: Mn + O → MnO (floats to slag), Mn + S → MnS (forms benign globular inclusions vs. iron sulfide films that cause hot shortness); the MnS/FeS ratio critically determines hot workability — minimum 3:1 Mn:S ratio is the standard requirement in structural steels; Mn²⁺ strongly stabilizes austenite (it sits right of Fe on the austenite-forming element diagram, similar effect per atom to Ni)
Biological Role	Essential trace element; Mn₄CaO₅ OEC in Photosystem II; MnSOD mitochondrial antioxidant	Manganese is essential for oxygenic photosynthesis — the Mn₄CaO₅ oxygen-evolving complex (OEC) in Photosystem II is the only biological catalyst capable of oxidizing water to O₂ (2H₂O → O₂ + 4H⁺ + 4e⁻, E° = +0.82 V), the ultimate source of all atmospheric oxygen and the primary energy input to the biosphere; MnSOD (Mn superoxide dismutase) in mitochondria dismutates superoxide radicals (O₂•⁻) to H₂O₂; Mn is a cofactor in arginase (urea cycle) and several carboxylases; daily dietary requirement ~2–5 mg/day

Identifier	Value
Symbol	Mn
Atomic Number	25
CAS Number	7439-96-5
UN Number	UN3089 (powder, flake)
EINECS Number	231-105-1

Isotope	Type	Notes
⁵⁵Mn	Stable	100% natural abundance — manganese is monoisotopic, one of only 22 monoisotopic elements; I = 5/2, NMR-active (large quadrupole moment giving broad lines in most chemical environments, but ⁵⁵Mn NMR is used to probe Mn coordination in catalysts, battery materials, and enzymes); the half-filled d⁵ configuration of Mn²⁺ (high spin) is the ground state for aqueous Mn and accounts for the pale pink color of Mn²⁺ solutions (very weak spin-forbidden d-d transitions); ⁵⁵Mn(n,γ)⁵⁶Mn reaction (t½ = 2.58 hr, β⁻/γ) is used in neutron activation analysis as a thermal neutron flux monitor
⁵⁴Mn	Radioactive	t½ = 312.1 days (electron capture); emits 834.8 keV gamma ray (99.98% intensity) — the standard gamma-ray calibration line for HPGe detectors in the 0.5–1.5 MeV range; produced by cosmic ray spallation on iron (⁵⁶Fe + p → ⁵⁴Mn + 3p) and by proton bombardment of chromium in cyclotrons; used as a standard gamma source in nuclear medicine physics, environmental radioactivity monitoring, and detector efficiency calibration; also an activated corrosion product in nuclear reactor primary circuits (⁵⁴Fe activation pathway)
⁵²Mn	Radioactive	t½ = 5.59 days (β⁺/EC); emits 1.434 MeV gamma and 511 keV annihilation photons; produced by proton bombardment of chromium (⁵²Cr(p,n)⁵²Mn) or vanadium (⁵¹V(d,n)⁵²Mn) in cyclotrons; used as a PET radiotracer for manganese biodistribution and transport studies — ⁵²Mn PET provides unique quantitative imaging of Mn uptake in brain (relevant to manganism neurotoxicity research), liver, and gastrointestinal tract; also used to trace Mn fate in battery materials and to study plant Mn uptake and translocation

Scientific & Research Applications

Use Case	Form Typically Used	Description
Water Oxidation Catalysis (Artificial Photosynthesis)	Mn oxide clusters (MnO₂, Mn₃O₄), molecular Mn complexes, Mn-based MOFs	Inspired by the biological Mn₄CaO₅ oxygen-evolving complex (OEC) in Photosystem II, researchers are developing Mn-based molecular and heterogeneous catalysts for water oxidation (2H₂O → O₂ + 4H⁺ + 4e⁻) as the oxidative half-reaction of artificial photosynthesis for solar fuel production. Birnessite-type MnO₂ and cubane-like Mn₄O₄ clusters show activity at modest overpotentials; the key challenge is achieving the four-electron, four-proton water oxidation at biologically relevant potentials without expensive noble metals. Research interfaces with photocatalysis, photoelectrochemical cells, and direct CO₂ reduction for solar fuels.
LiMn₂O₄ & NMC Battery Cathode Research	MnO₂ (EMD), Mn₂O₃, Mn₃O₄ cathode precursors; Mn metal for alloy synthesis	Lithium manganese spinel (LiMn₂O₄, LMO) cathodes operate at 4 V vs. Li/Li⁺ and offer high power capability, safety (no phase transitions triggering thermal runaway), and lower cost than LCO — but suffer capacity fade from Jahn-Teller distortion of Mn³⁺ and Mn dissolution into electrolyte. Research focuses on Li-rich layered Mn oxides (Li₁.₂Ni₀.₁₃Mn₀.₅₄Co₀.₁₃O₂), LNMO spinel (high-voltage 4.7 V), and Mn-rich NMC compositions (NMC 811, 9-0.5-0.5) for high-energy automotive batteries. Mn-rich cathode chemistries are favored for reducing Co content and cost in next-generation LIBs.
Magnetic Materials Research	Mn thin films (MBE/sputtering), Mn₃Sn, MnBi, Ga-Mn-As epitaxial layers	Manganese is central to several technically important magnetic and spintronic systems. MnBi is one of the few room-temperature hard magnets with positive magnetocrystalline anisotropy temperature coefficient (useful for high-temperature permanent magnets). Mn₃Sn (antiferromagnet) generates anomalous Hall effect without net magnetization — enabling "antiferromagnetic spintronics" for ultrafast magnetic memory. Ga-Mn-As and In-Mn-As dilute magnetic semiconductors (DMS) exhibit carrier-mediated ferromagnetism and are model systems for spin-polarized carrier physics. γ-MnGa alloys (FCC phase stabilized by Ga) have extremely high magnetocrystalline anisotropy.
Semiconductor Doping Research	MnCl₂ or Mn metal for MOCVD/MBE doping; Mn-doped ZnO, GaN, GaAs	Mn²⁺ doped into wide-bandgap semiconductors (ZnO, GaN, ZnS, ZnSe) produces dilute magnetic semiconductors (DMS) with room-temperature ferromagnetism and spin-polarized photoluminescence — studied for spintronic devices and magneto-optical applications. Mn²⁺ doping of II-VI semiconductors (CdS:Mn, ZnS:Mn) produces efficient orange-yellow photoluminescence (⁴T₁→⁶A₁ Mn²⁺ d-d transition) used in electroluminescent displays. Mn:ZnSe quantum dots and Mn:perovskite nanocrystals are studied for luminescent solar concentrators and displays.
MRI Contrast Agent Research	MnCl₂, Mn-porphyrin complexes, Mn oxide nanoparticles	Mn²⁺ (d⁵, S = 5/2, 5 unpaired electrons) has large magnetic moment and fast water exchange kinetics, making it an effective T₁ MRI contrast agent — mangafodipir (Mn-DPDP) was FDA-approved for liver MRI imaging. Research focuses on Mn-based alternatives to Gd-based contrast agents (GBCAs) given concerns about Gd tissue retention; Mn-porphyrin complexes, Mn-albumin, and MnO nanoparticles are studied for liver, cardiac, and tumor-targeted T₁ contrast enhancement. Mn²⁺ is also a natural T₁ contrast agent for neurological imaging (MEMRI — manganese-enhanced MRI) tracking neural tract connectivity.
Nuclear Studies (⁵⁴Mn Gamma Source)	⁵⁴Mn-labeled compounds (carrier-free), ⁵⁴MnCl₂ standard solutions	⁵⁴Mn (t½ = 312 days, 834.8 keV gamma, 99.98%) is a standard gamma-ray energy calibration source for HPGe detector efficiency measurements and nuclear instrument calibration across medical physics, environmental radioactivity monitoring, and nuclear safeguards laboratories. ⁵⁴Mn is produced in nuclear reactors (⁵⁴Fe activation) and by proton bombardment of Cr; environmental ⁵⁴Mn monitoring tracks reactor-derived radionuclide releases in cooling water discharges. ⁵⁴Mn is also used to trace Mn fate in ecological systems (plant uptake, marine sediments, groundwater transport).

Industrial & Commercial Applications

Sector	Form / Grade Used	Description
Steel Production (Ferromanganese & Silicomanganese)	Ferromanganese (65–80% Mn), silicomanganese (60–70% Mn, 14–20% Si), electrolytic Mn metal (EMM, 99.7%+)	Manganese is added to virtually all commercial steel — typically 0.3–1.5 wt% in carbon and low-alloy steels, up to 14 wt% in Hadfield manganese steel. Ferromanganese (from smelting MnO₂ ore with coke and limestone) and silicomanganese are the primary forms for bulk steel additions — the silica in silicomanganese assists deoxidation. Electrolytic manganese metal (EMM, ≥99.7%) is used for additions requiring low carbon content (stainless steels, special alloys, battery precursors). Annual Mn ore consumption for steelmaking is ~17 million tonnes (~90% of all Mn ore mined).
Alkaline & Zinc-Carbon Battery Cathodes	Electrolytic manganese dioxide (EMD, γ-MnO₂, ≥91% MnO₂)	Electrolytic manganese dioxide (EMD, produced by electrochemical oxidation of MnSO₄ solution at the anode) is the cathode active material in alkaline batteries (AA, AAA, C, D cells) — the most widely sold primary battery chemistry globally. EMD (γ-MnO₂) has higher electroactivity and surface area than chemical MnO₂ (CMD), giving higher battery capacity. Approximately 400,000 tonnes/year of EMD are consumed globally in alkaline battery manufacturing. The Mn²⁺/MnO₂ electrochemistry in the Zn-MnO₂ alkaline cell achieves 1.5 V open-circuit voltage and ~70–80 Wh/kg practical energy density.
Aluminum Alloy Addition	Electrolytic Mn metal or Al-Mn master alloy; 0.3–1.5 wt% Mn in Al	Manganese additions to aluminum alloys (3xxx series: Al-Mn; 5xxx series: Al-Mg-Mn) improve corrosion resistance by scavenging Fe and Si into dispersoid particles (Al₆Mn, Al₁₂Mn₃Si), improve strength through solid-solution hardening, and control recrystallization texture in rolled sheet. 3003 (Al-1.2Mn) is the most widely used non-heat-treatable Al alloy, used in cookware, building products, and chemical equipment; 3105 and 3004 (Al-Mn-Mg) in beverage can bodies. Mn additions (0.2–0.4%) in 5xxx and 7xxx alloys stabilize grain structure and reduce sensitization.
Potassium Permanganate (Water Treatment & Chemical Synthesis)	KMnO₄ (industrial grade, 99%); MnO₂ catalyst for KMnO₄ synthesis	Potassium permanganate (KMnO₄, 0.01–1% solutions) is one of the most widely used industrial and laboratory oxidizing agents — used for municipal water treatment (oxidizing Fe²⁺, Mn²⁺, and H₂S; controlling taste and odor compounds; Cryptosporidium oocyst inactivation), wastewater treatment, swimming pool sanitation, medical antiseptic/antifungal (topical KMnO₄ solutions for dermatology), and industrial organic oxidations (alcohol → aldehyde → carboxylic acid synthesis, glycol diol formation). KMnO₄ decontamination of chlorinated solvent (TCE, PCE) plumes in contaminated groundwater uses in situ chemical oxidation (ISCO) injection.
Fertilizers & Agricultural Micronutrients	MnSO₄ (37% Mn), MnO (foliar spray), chelated Mn-EDTA	Manganese is an essential plant micronutrient (required for chlorophyll synthesis, Photosystem II function, and multiple enzyme systems) — deficiency causes interveinal chlorosis and reduced crop yields, particularly in alkaline, sandy, or organic soils with high pH. MnSO₄ soil amendments and MnO foliar sprays correct Mn deficiency in soybean, wheat, oats, and citrus crops. Chelated Mn-EDTA provides Mn in plant-available form across a wider soil pH range. Annual global consumption of Mn in agricultural applications is ~100,000 tonnes.
Glass & Ceramics Colorant	MnO₂ (ceramics), MnCO₃ (glass batch), MnO (reducing atmosphere)	Manganese has been used to colorize and decolorize glass since antiquity. Mn³⁺ in glass produces a purple-amethyst color (historic "glass of antimony"); Mn²⁺ in reducing atmospheres is colorless; MnO₂ addition acts as a "glassmaker's soap," oxidizing colorizing Fe²⁺ to less-colorful Fe³⁺. Ancient Roman glasses frequently contain Mn as a fining/decoloring agent. In ceramics, MnO₂ produces browns (with Al), purples (with TiO₂), and blacks (with Co, Fe, Cr) — widely used in ceramic colorant stains and underglaze pigments.

Purity	Main Use
98.7%	Standard-grade manganese for alloying, general metallurgical processes, and non-critical applications — suitable for ferroalloy production, aluminum alloy master alloy additions, and industrial chemical synthesis where sub-1.3% impurities (primarily Fe, C, Si, S) are acceptable
99.5%	High-purity manganese for advanced industrial uses including battery precursor production (NMC/LMO cathode synthesis), specialized stainless steel and superalloy additions requiring low Fe and C content, and EMD precursor electrolyte preparation where iron contamination would degrade battery performance
99.95%	Ultra-high-purity manganese for semiconductor processing (Mn-doped DMS growth by MBE/MOCVD), research-grade catalyst synthesis (Mn-oxide water oxidation catalysts, Mn-porphyrin MRI contrast agents), and precision applications where sub-500 ppm metallic impurities are required for reproducible electronic or magnetic properties

Synonym / Alternative Name	Context
Mn	Chemical symbol; from Latin manganum, itself derived from the Greek Magnesia (Μαγνησία) — the same Thessalian region that gave its name to magnesium, reflecting the historical confusion between pyrolusite (MnO₂) and magnesia alba (MgCO₃) before these compounds were chemically distinguished; manganese was first isolated by Johan Gottlieb Gahn in 1774 by reduction of pyrolusite with charcoal
Manganese metal	Standard commercial designation for the elemental form, specifically electrolytic manganese metal (EMM) — the standard commodity form produced by electrolysis of MnSO₄ solution (99.7–99.9% Mn); distinguished from manganese ore, ferromanganese, and manganese compounds in trade documentation and supply chain reporting
Elemental manganese	Scientific term distinguishing the pure metal from manganese compounds (MnO₂, KMnO₄, MnSO₄, MnCl₂, LiMn₂O₄, etc.) in chemistry and materials literature; rarely used commercially since virtually all industrial Mn is consumed as ferromanganese, EMD, or EMM rather than as elemental research-grade metal
Manganese (EMM)	Trade designation for electrolytic manganese metal — the standard primary manganese product (≥99.7% Mn, low C) produced by electrodeposition from acidic MnSO₄ electrolyte; the dominant commodity form of high-purity manganese in global trade, primarily produced in China; distinguished from electrolytic manganese dioxide (EMD), which is the battery cathode product
Ferromanganese	Fe-Mn alloys (65–80% Mn) produced by smelting manganese ore with coke; the principal form in which Mn is added to steel — high-carbon ferromanganese (7–8% C), medium-carbon (1–1.5% C), and low-carbon (<0.5% C) grades for different steel applications; not pure Mn but listed here as the most commonly encountered commercial Mn-bearing material in steelmaking

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