Magnesium fluoride - ≥98% , CAS No.7783-40-6

CAS: 7783-40-6 Cat. No.: M292542 Formule: MgF₂ Poids moléculaire: 62.3 Numéro CE: 231-995-1

GRADE & PURITY ≥98%

Synonyms

Magnesium flux | Afluon | Sellaite

Storage

Room temperature

Shipped In

Normal

Vue d’ensemble

In the light of purple fluorescence, slightly soluble in dilute acid, almost insoluble in water. Rutile crystal lattice shows weak purple fluorescence when heated under electric light, and its crystal has good polarization, especially suitable for ultraviolet and infrared spectrum. Very slightly soluble in water (18 ℃, 87mg / L), slightly soluble in dilute acid (especially nitric acid). The lethal dose (guinea pig, oral) was 1.0 g / kg. It's stimulating.

Specifications

Synonymes

Magnesium flux | Afluon | Sellaite

Spécifications et pureté

≥98%

Conditions de stockage de stockage

Room temperature

Expédié en

Normal

Pureté

≥98%

Noms et identifiants

WGK Allemagne

3

RTECS

OM3325000

Poids moléculaire

62.3

Propriétés chimiques et physiques

• Solubilité: Sparingly soluble in water. Slightly soluble in dilute HNO3.
• Sensibilité: Moisture sensitive.
• Point d'ébullition (°C): 2260°C
• Point de fusion (°C): 1248°C

Application Protocols

No standardized bioassay or immunoassay protocols are associated with this inorganic salt. For materials/catalysis applications, users typically develop process-specific protocols. General starting points (literature/good practice):

• Fluoride scavenging from organic solutions

  • Add MgF2 or a magnesium source capable of forming MgF2 in situ under agitation.
  • Stir at ambient temperature; periodically sample the supernatant and quantify fluoride (ISE/IC).
  • Filter, wash the solid with compatible solvent, and re-check fluoride in the filtrate.

• Catalyst support preparation

  • Pre-calcine MgF2 to target surface area.
  • Deposit metal (e.g., incipient wetness impregnation), dry, and activate under inert/reductive atmospheres as needed.

These are illustrative, literature-style outlines only. Item-specific tested applications and recommended dilutions: Not specified for this item; refer to CoA/Spec Sheet and SDS for detailed handling.

Biological Roles

This product is supplied for research use only. The following notes summarize general biochemical context of its constituent ions (literature), not product claims.

• Magnesium ion (Mg2+)

  • Essential cofactor for numerous enzymes (e.g., kinases, ATP-dependent processes) and stabilizes nucleic acid structures through charge screening.
  • Cellular Mg2+ homeostasis is tightly regulated; however, MgF2 as a bulk solid is not a bioavailable magnesium source due to negligible solubility in physiological media.

• Fluoride ion (F−)

  • Interacts with metal centers and can modulate enzyme activities in vitro; commonly used to inhibit certain phosphatases by forming metal–fluoride complexes that mimic transition states.
  • Bioavailability from MgF2 is expected to be minimal under neutral conditions; acidic conditions increase fluoride availability (safety concern rather than a biological role).

• Practical implications for lab biology

  • MgF2 is typically inert in aqueous buffers and cell culture media because of its extremely low solubility; it is not used to deliver Mg2+ or F− to biological systems.
  • For enzymology requiring fluoride, soluble salts (e.g., NaF, KF) are used to achieve defined concentrations.

• Caution

  • Avoid introducing particulate MgF2 into biological assays unless the experiment explicitly investigates solid–liquid interfacial effects; particles can adsorb proteins nonspecifically and interfere with optical measurements.

Buffer Applications

Magnesium fluoride is not a buffering agent and is not used to prepare defined pH buffer systems. Because it is sparingly soluble, it does not provide meaningful acid/base capacity in aqueous solutions.

• If fluoride is required in buffered systems (e.g., as an enzyme inhibitor in vitro), use soluble fluoride salts (e.g., NaF, KF) prepared in standard biological buffers (e.g., Tris, HEPES, phosphate), and adjust pH after addition.

• For experiments involving MgF2 solids in contact with buffers (e.g., surface interactions), maintain good agitation and consider ionic strength, as adsorption of buffer components to inorganic surfaces can occur and impact assay results.

Green Alternatives

Choosing a fluoride material impacts safety, environmental fate, and waste handling. Considerations (literature/general):

• Comparison of fluoride options (general, not item-specific)

  • MgF2

    • Pros: Insoluble, chemically robust; low dusting when granulated; minimal fluoride leaching in neutral media; reusable as heterogeneous phase; low volatility.
    • Cons: Not a soluble nucleophilic fluoride; limited utility as a direct fluorinating reagent; disposal still requires fluoride controls.

  • KF or CsF

    • Pros: Readily available, higher basicity/nucleophilicity in polar aprotic solvents; widely used in Halex, desilylation, and SNAr.
    • Cons: Hygroscopic (especially CsF), can generate corrosive fluoride solutions; greater acute exposure risks due to solubility.

  • TBAF (tetra-n-butylammonium fluoride)

    • Pros: Highly soluble in organics; powerful fluoride donor.
    • Cons: Corrosive, can contain HF; generates quaternary ammonium waste; thermal instability.

  • CaF2 (fluorite)

    • Pros: Very low solubility; abundant mineral; similar inertness to MgF2; often considered benign as a fluoride immobilization matrix.
    • Cons: Even less reactive/soluble; limited catalytic interest.

Sustainability notes

• Prefer heterogeneous, recyclable fluoride phases (MgF2, CaF2) as scavengers or supports when soluble fluoride is not essential.
• Minimize HF-containing workflows; use closed systems and fluoride waste treatment (e.g., Ca2+ precipitation to CaF2).

Pharmaceutical Uses

No pharmaceutical or clinical applications are claimed for this product. The following notes are general materials-science considerations (literature) and not product specifications.

• Excipient/formulation role: Magnesium fluoride is not commonly used as a pharmaceutical excipient due to its low solubility and lack of traditional excipient functionality (e.g., binder, disintegrant). It may appear in materials science contexts where chemically durable, low-refractive-index coatings are needed on devices or analytical optics.

• Regulatory compendia: There is no general pharmacopeial monograph on MgF2 as an excipient comparable to common salts; any use in regulated environments would need specific qualification and material controls.

• Process/analytical considerations: As a hard, chemically stable fluoride, MgF2 can be produced in situ during processes handling HF or fluoride-containing reagents; understanding its formation and removal (filtration) can be relevant to process development.

For drug substance/drug product development, select materials with established pharmacopeial status unless a compelling materials property (e.g., optical) requires MgF2; in such cases, implement appropriate extractables/leachables assessments. This product is for research use only.

Physical Properties

Note: Values below are general literature values for magnesium fluoride and are not item-specific specifications.

• Phase/appearance (literature): Colorless to white crystalline solid; hard, dense; often encountered as a fine powder or as transparent optical-grade crystals.
• Melting point: ~1261 °C (literature)
• Boiling/sublimation/decomposition: ~2260 °C (reported high-temperature volatilization; literature). Practical handling rarely approaches this regime.
• Density: ~3.15 g/cm³ at ambient temperature (literature)
• Solubility (literature):
  • Water: Very slightly soluble (commonly described as practically insoluble); dissolution increases marginally at elevated temperatures.
  • Alcohols/ketones/hydrocarbons: Insoluble.
  • Strong acids containing complexing anions or HF: Reactions/complexation can occur; fluoride activity increases in presence of complexing media.
• Refractive index (bulk crystal, literature): n ~1.377 at 589 nm; exhibits very wide optical transmission from deep UV to IR, a reason for its optical-coating applications.
• pKa/logP: Not applicable (inorganic salt; no acid–base equilibria in molecular sense; partitioning into organic media is negligible).
• Thermal/chemical stability (literature): Excellent stability toward most ambient reagents; resistant to moisture and many acids/bases; fluoride chemistry becomes relevant in strongly acidic fluoride-generating media (e.g., HF).

Item-specific property fields such as precise assay, particle size, trace metals, moisture, or optical homogeneity: Not specified for this item; refer to CoA/Spec Sheet.

Quality and Grades

• Item-specific grade/purity, stabilizers, appearance: Not specified for this item; refer to CoA/Spec Sheet.

• Interpreting grades for MgF2 (general guidance)

  • Reagent grade: Suitable for routine laboratory use where trace metal and optical homogeneity are not critical; may have broader particle-size distribution.
  • High-purity/trace-metal grade: Tight limits on alkali/alkaline earth contaminants, heavy metals, and silica; important for catalysis studies, electronics, or where background metals affect results.
  • Optical grade: Emphasizes low scatter/absorption in UV–IR, low water/impurity content, controlled crystallinity/defect density, and specific surface finish for windows or AR coatings. Not implied for this item unless specified on the CoA.

• Stabilizers: MgF2 typically requires no stabilizer. If moisture or carbonate limits, particle size, or loss on ignition are reported, those will appear on the item CoA/specification; otherwise assume none added.

• Recommended verification for critical work

  • Confirm assay and trace metals by ICP-OES/MS if needed for catalysis or materials applications.
  • Verify particle size/surface area (e.g., BET) for heterogeneous catalysis or support use.
  • For optical applications, verify refractive index homogeneity, transmission, and scatter on the supplied lot (if applicable).

Reaction and Applications

The primary laboratory relevance of magnesium fluoride stems from its robustness as an inorganic fluoride and as an inert/fluoride-bearing heterogeneous phase (literature). Key use areas:

• Heterogeneous catalysis and supports (literature)

  • MgF2 has been studied as a catalyst or catalyst support in transformations sensitive to acid/base properties, including isomerizations, dehydrofluorination, and certain oxidation processes. Fluorinated supports can modify metal dispersion and electronic properties.
  • Fluorination of metal oxides (e.g., MgO → MgF2) is used to tune surface acidity/basicity and hydrophobicity in catalytic systems.

• Fluoride source/fluoride scavenging (literature)

  • While poorly soluble, MgF2 formation often serves as a thermodynamic driving force to scavenge fluoride released during reactions (e.g., Si–F bond formation or HF neutralization with Mg salts). Conversely, MgF2 is not commonly chosen as a soluble nucleophilic fluoride for organic substitution; KF/CsF/TBAF are typical.

• Materials and coatings (literature)

  • Widely used in optical thin films as a durable, low-index anti-reflection (AR) material across UV–IR due to its low refractive index and wide band gap.
  • As a chemically durable window/substrate for UV spectroscopy and high-vacuum optics.

• Practical lab tips

  • For catalytic studies, pre-treat (calcine) MgF2 to define surface area and remove adventitious moisture/carbonates; characterize by BET/XRD.
  • When used as a fluoride sink, ensure adequate mixing/contact; product will remain as a solid and may require filtration and thorough washing.

Reaction Conditions

Because MgF2 is typically a heterogeneous, sparingly soluble solid, conditions depend on whether it is used as a support/scavenger or as a reactive phase (literature/general guidance):

• As a fluoride scavenger

  • Medium: The reaction’s native solvent (e.g., polar aprotics like MeCN, DMF, DCM, or alcohols). MgF2 remains as a suspended solid.
  • Temperature: Ambient to ~80 °C typical for liquid-phase organics; ensure good stirring for mass transfer.
  • Stoichiometry: Empirically determined; monitor residual fluoride (ISE or ion chromatography) and add incrementally until below target limits.

• As a catalyst/support

  • Pre-treatment: Calcination (e.g., 300–500 °C in air or inert) to set surface area and remove adsorbates (specific programs vary by study).
  • Reaction regimes: Gas-phase or liquid-phase; temperatures from 100–400+ °C are reported depending on transformation (e.g., isomerizations, dehydrofluorinations). Use fixed-bed reactors with controlled space velocity for gas-phase studies.
  • Solvents (liquid-phase): Non-coordinating or moderately polar solvents; avoid strong acids that alter the fluoride surface.

• As a fluoride donor (rare)

  • Forcing conditions such as molten salts, mechanochemistry, or high-temperature solid–solid reactions may be required; not common in bench-top organic synthesis.

Expected outcomes: Highly system-dependent; consult primary literature for the specific transformation. These are general guidelines, not item specifications.

Safety and Handling

Always consult the SDS for authoritative, product-specific guidance.

• GHS classification, signal word, hazard statements, pictograms: Not specified for this item; refer to SDS.

• General safety considerations (literature/good practice for fluoride salts)

  • Avoid inhalation of dust and contact with eyes/skin. Use appropriate PPE: safety glasses or goggles, lab coat, and chemical-resistant gloves (e.g., nitrile). Handle powders in a fume hood to minimize dust exposure.
  • Fluoride content: While MgF2 is sparingly soluble, fluoride toxicity is a consideration upon ingestion or exposure to acidic conditions liberating HF or bioavailable fluoride. Prevent ingestion and avoid contact with acids that can increase fluoride availability.
  • Incompatibilities: Strong acids (especially HF and strongly acidic fluoride media), strong complexing agents for Mg2+, and strong dehydrating agents that may promote surface reactions. Avoid contact with glass etchants (HF) and store away from acids to reduce risk.
  • Thermal stability: Chemically robust; avoid generating dust at elevated temperatures and use appropriate ventilation for any high-temperature processing.

• First-aid overview (general)

  • Inhalation: Move to fresh air; seek medical attention if symptoms persist.
  • Skin/eye contact: Rinse with water for several minutes; remove contaminated clothing; obtain medical advice for persistent irritation.
  • Ingestion: Rinse mouth; do not induce vomiting; seek medical attention.

• Waste: Dispose of in accordance with institutional and local regulations for inorganic fluoride-containing solids.

Solvent Selection

This product is a sparingly soluble inorganic solid, not a solvent. Solvent selection is relevant only insofar as dispersion, washing, or reaction media are concerned.

• General miscibility/solubility profile (literature)

  • Water: Very low solubility; behaves largely as an inert solid.
  • Organic solvents (alcohols, ethers, hydrocarbons, chlorinated): Insoluble; can be suspended as a solid.
  • Acidic fluoride media (e.g., HF) or complexing acids: Interaction/complexation possible; dissolution may occur with fluoride-containing strong acids.

• Practical selection for lab use

  • For slurry reactions or solid–liquid contact studies: Choose polar aprotic solvents (e.g., MeCN, DMF, DMSO) or alcohols if compatibility with other components is needed; MgF2 will remain as a heterogeneous phase.
  • For washing and separations: Water or alcohols effectively remove soluble impurities without dissolving MgF2.
  • For etching/generation of soluble fluoride species: Specialized HF-containing systems are used under controlled, high-safety conditions (not routine bench work).

• When to choose alternatives

  • If a soluble fluoride source is required, consider KF, CsF, or TBAF (with due safety considerations) instead of MgF2.
  • If an inert, high-surface-area support is needed, alumina or silica may be preferred unless fluoride character is functionally desired.

Storage and Reconstitution

• Storage (item-specific from Product Data)

  • Store at room temperature.
  • Shipped under normal conditions.

• General handling (good practice)

  • Keep container tightly closed and store in a dry location to prevent adventitious moisture uptake and contamination.
  • Segregate from strong acids and fluoride-generating corrosives (e.g., HF) to minimize risk of corrosive interactions.
  • Avoid creating or breathing dust; use in a fume hood when handling powders.

• Reconstitution

  • Solid inorganic salt; no reconstitution is required. If a slurry is desired, disperse in a compatible solvent (water or organic) using mechanical stirring or brief sonication; MgF2 will remain as an undissolved solid under most conditions.

• Shelf life/retaining quality

  • Magnesium fluoride is chemically robust; under proper storage it remains stable for extended periods. For critical work, verify key attributes (e.g., particle size, surface area, or impurity profile) on receipt and after prolonged storage.

Any item-specific specifications (assay, moisture, particle size, trace metals): Not specified for this item; refer to CoA/Spec Sheet.

Structure and Identity

Brief overview: Magnesium fluoride is an inorganic binary salt composed of magnesium(II) and fluoride anions, widely recognized for its exceptional chemical and optical robustness (literature).

• Item-specific facts (from Product Data)

  • SKU: M292542
  • Product Name: Magnesium fluoride
  • CAS: 7783-40-6
  • Storage Conditions: Room temperature
  • Shipped In: Normal
  • Research Use Note: For research use only
  • Any further identifiers (InChIKey, SMILES, grade/purity, appearance): Not specified for this item; refer to CoA/Spec Sheet.

• Literature/computed identity (general reference, not item specification)

  • Molecular formula: MgF2 (literature)
  • Formula weight (FW): ~62.30 g/mol (literature)
  • Common SMILES: [Mg+2].[F-].[F-] (literature)
  • InChI (key not provided here): Not specified for this item; refer to CoA/Spec Sheet.

• Structural features (descriptive, literature)

  • Composition: Dicationic Mg2+ coordinated by two F− in the simplest stoichiometry; in the solid state, each Mg is octahedrally coordinated to six F in an extended lattice (rutile-type structure).
  • Crystal structure: Tetragonal, rutile-type (space group P42/mnm; literature), forming an infinite 3D ionic network.
  • Functional groups: Inorganic salt; no covalent functional groups; strong ionic Mg–F interactions impart high lattice energy and thermal/chemical stability.
  • 2D depiction (verbal): A central Mg2+ species charge-balanced by two fluoride anions; as a bulk solid the repeating MgF6 octahedra share edges/corners in a tetragonal array (literature).

Synthetic Utility

Magnesium fluoride’s value in synthesis is rooted in its role as a robust, heterogeneous fluoride phase and as a component in catalyst systems (literature):

• Fluoride scavenger/drive reactions

  • Formation of MgF2 is highly favorable; adding Mg2+ sources (e.g., MgO, Mg salts) in processes that release HF or F− can sequester fluoride as MgF2, simplifying workup and mitigating corrosion.

• Heterogeneous catalysis/support effects

  • Fluorination of oxide supports (generating MgF2 surfaces) modifies acidity/basicity and hydrophobicity, tuning selectivity in isomerizations, hydrocarbon transformations, and partial oxidations.
  • Metal catalysts (e.g., Pt, Pd, Ni) on MgF2 have been explored for hydrogenation/dehydrofluorination where suppression of strong Brønsted acidity is desired.

• Fluoride transfer chemistry

  • Due to limited solubility and low nucleophilicity, MgF2 is rarely the reagent of choice for nucleophilic fluorination of organics; CsF/KF/TBAF dominate. Nonetheless, MgF2 can participate under forcing conditions or in molten salt/solid-state protocols.

• Surface and materials synthesis

  • Controlled conversion of Mg(OH)2 or MgO to MgF2 enables fabrication of fluoride-rich surfaces and thin films with distinctive optical and chemical properties.

Practical notes

• For scavenging, add Mg2+ base or oxide under agitation and verify fluoride removal by ion-selective electrode or IC.
• For catalytic use, pre-treat MgF2 (e.g., calcination) to define surface area and remove adventitious carbonates; characterize by XRD/BET/TPD to correlate surface properties with reactivity.

Target Specificity

Not applicable. This product is an inorganic salt, not a biological affinity reagent or antibody. No target specificity claims are associated with this item.

Foire aux questions

What is the purity of this product?

This product is supplied at ≥98% purity (chemical assay). Lot-specific values are stated on the Certificate of Analysis.

How should this product be stored?

Store at room temperature.

How is this product shipped?

This product ships under standard ambient conditions. No temperature-controlled packaging is required.

What are the CAS number, molecular formula and molecular weight?

The CAS Number is 7783-40-6, the molecular formula is MgF2, and the molecular weight is 62.3 g/mol.

What documentation is provided?

Available product documentation, including Certificates of Analysis (COA), Safety Data Sheets (SDS), and specification sheets, is shown in the product document area. Document availability and access follow the current site policy.