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Nickel Fluoride: In-Depth Commentary
Historical Development
Nickel fluoride cropped up in the early days of transition metal chemistry when scientists needed stable compounds to study bonding between metals and halogens. The research started before World War II, during a push to better understand elements with magnetic and catalytic punch. Nickel, known for its industrial strength and handy electronic structure, naturally invited curiosity about its halides. Early reports pointed to unpredictable reactivity, sparking deeper quest for proper isolation and repeatable synthesis. Tubes packed with fluorine gas and nickel powder did the hard work, under rigorous containment, and paved the way for a compound that helped shape the backbone of electrochemistry, catalysis, and high-energy materials research. Academic work in the 1940s and 50s ironed out the basic forms: nickel(II) fluoride, a stable pale green powder, and the rare nickel(III) and nickel(IV) fluorides, which only show up under tough synthetic conditions. Laboratory traditions, careful handling, and evolving analytical tools kept interest running as applications became clearer over decades.
Product Overview
Nickel fluoride sits in catalogs as a pale or greenish crystalline solid, drawing attention from researchers who work with advanced materials, catalysts, and battery components. Common forms include nickel(II) fluoride (NiF2), both anhydrous and hydrated, while some labs experiment with higher oxidation state fluoro-nickels for niche reactions. Purity stands as a hallmark, since traces of water or other halides cause serious headaches in chemical transformations. For suppliers, measuring out powder with exacting precision and storing it in sealed containers isn’t just a necessity—it determines whether nickel fluoride ends up working as intended in a cleanroom or a glovebox. Product granularity matters, since fine powders react faster but pose dust inhalation risks, and larger crystals invite safer handling during scale-up. Packaging often comes in glass or fluoropolymer bottles, clearly marked for immediate recognition in busy storerooms.
Physical & Chemical Properties
Nickel(II) fluoride appears as a greenish solid—sometimes blue-green, depending on the level of hydration. It’s not your typical table salt: the crystals resist dissolving in organic solvents and only slowly break down in water, with the process managed by the hydration state. Beneath the surface, NiF2 holds together with strong ionic bonds, giving it high thermal stability and a melting point in the neighborhood of 1,475°C. Thermal decomposition unleashes toxic fumes, making direct heating a risky proposition outside of tightly controlled lab conditions. In its crystal lattice, nickel adopts an octahedral geometry, connected to six fluorides, offering magnetic behavior that’s still discussed in solid-state physics classes. The anhydrous version keeps its form under dry air, but will grab water molecules from humid air, so humidity control must stay tight. It's not volatile but can turn into aerosols. Chemical reactions often start slow but pick up speed given a source of heat or a strong fluoride donor.
Technical Specifications & Labeling
Each drum or bottle of nickel fluoride needs legible, chemical-resistant labeling, showing not only its chemical formula but also batch number, date of synthesis, and a warning panel highlighting toxicity and severe irritant properties. Specifications demanded by industry and research include purity—often at 99.9% or higher for sensitive work—and well-documented hydration state. Common quality checks pull from X-ray diffraction, infrared spectroscopy, and titrimetric analysis to confirm phase and moisture levels. Labs insist on knowing the fine print: trace metal impurities, residual halides, particle size distribution, and whether the product qualifies as hazardous under various transport regulations. Standards bodies like Sigma-Aldrich, Merck, and others keep a list of product IDs and synonyms for clarity, while shipping documents flag the compound under UN 3288, packing group III for toxic solids.
Preparation Method
Making nickel fluoride is a process that demands patience and an eye for safety. One common route starts by reacting nickel metal directly with fluorine gas at elevated temperatures, a method not for the faint-hearted due to the violence of elemental fluorine. Alternatively, nickel(II) chloride can be treated with hydrofluoric acid, producing nickel fluoride and hydrochloric acid as a byproduct. Both methods require non-reactive equipment—nickel or Monel vessels, PTFE tubing—since fluorides chew through glass and steel given enough time or heat. Crystallization follows, with filtration and drying under vacuum or inert gas to keep out moisture. Each step runs under an exhaust hood, and workers wear face shields, chemical-resistant gloves, and sometimes full-body suits to block splashes and fumes. Waste neutralization involves CaCO3 or other fluoride binders, followed by compliance checks on effluent before discharge.
Chemical Reactions & Modifications
Nickel fluoride proves useful as a fluorinating agent, especially in organic chemistry where introducing fluorine atoms to molecules can radically alter their properties. NiF2 oxidizes organic substrates, sometimes acting as a catalyst in halogen exchange or oxidative addition reactions. It swaps ligands easily to form complex fluoronickel species, and under the right conditions, chemists coax nickel into higher oxidation states, synthesizing NiF3 or NiF4. These powerful oxidizers participate in fluorocarbon synthesis, rare-earth extraction, and specialty inorganic chemistry. Reactions with concentrated acids produce hexafluoronickelate complexes—salts used to separate nickel from other metals or to study lattice energies. Thermal decomposition reverses the synthesis, releasing nickel oxide and fluoride gas, underscoring the need for closed systems. In research settings, slow diffusion techniques build single crystals suitable for X-ray analysis, revealing subtle aspects of nickel-fluorine bonding that spark debates about electronic structure.
Synonyms & Product Names
Nickel fluoride circles through chemical supply catalogs under various names: nickel(II) fluoride, nickel difluoride, and simply NiF2. Hydrated forms include nickel(II) fluoride tetrahydrate. In technical literature, compounds might show up as nickelous fluoride or, for higher oxidation states, nickel(III) fluoride and nickel(IV) fluoride. International shipment and regulatory databases stick with the CAS Number 10028-18-9, ensuring traceability. Brands assign catalog codes and labels, and some regional guides translate names into German (Nickelfluorid), French (fluorure de nickel), or Japanese (ニッケルフッ化物).
Safety & Operational Standards
Direct experience with nickel fluoride shows just how much training and preparation count for safe handling. Even small doses of inhaled dust can harm respiratory health, while skin contact causes burns and serious allergic reactions for some workers. Hydrofluoric acid, produced through hydrolysis or reaction with acids, leaches calcium from tissues and triggers painful, sometimes deadly poisoning. Labs enforce double-layer nitrile or neoprene gloves, splash goggles, and sometimes air-supplied respirators in areas where powders or vapors might escape. Any spills need immediate neutralization and cleanup—standard practice calls for special spill kits with calcium gluconate and chelating absorbents. Air monitoring equipment and regular health screenings keep longer-term risks in check for those working with nickel compounds. Workplace controls—ventilation hoods, negative-pressure rooms, and strict hygiene routines—are nonnegotiable, and every facility using nickel fluoride posts safety data sheets, guides on first aid, and emergency response instructions.
Application Area
Nickel fluoride shows up where strong oxidizing and fluorinating power make a difference. Electroplating industries turn to nickel(II) fluoride as a source of nickel in specialized baths, while battery researchers examine its behavior as a cathode material offering higher voltages and better cycle stability in test cells, especially for next-generation lithium-ion systems. In organofluorine synthesis, NiF2 acts as a catalytic or stoichiometric fluorine source, delivering C–F bond formation crucial for pharmaceutical and agrochemical development. Some applications rely less on bulk use and more on its unique chemistry, such as in the production of optically active, magnetically sensitive ceramics or superalloy components. Water treatment programs use hexafluoronickelate salts for selective transition metal removal from waste streams, drawing on the strong affinity between nickel, fluoride, and contaminant ions. Academic groups keep exploring new reactions with nickel fluorides, chasing breakthroughs in catalysis, inorganic materials, and surface engineering.
Research & Development
Exploratory work on nickel fluoride pushes into new territory each year. Researchers investigate how doping NiF2 with rare earth elements tunes magnetic and electronic properties, opening paths to quantum materials and memory storage applications. The complex interplay between nickel’s d-orbitals and fluoride ligands continues to intrigue solid-state chemists, who study lattice distortions, electron transfer rates, and the emergence of antiferromagnetic or metamagnetic behavior under applied fields. On the catalysis front, teams combine experimental and computational methods to model how NiF2 mediates fluorination of bioactive molecules, aiming to streamline drug discovery and agrochemical production. Battery technology enjoys deeper dives into how nanostructured nickel fluoride improves charge retention, cycling stability, or suppresses unwanted side reactions. Advances in synthesis—controlling particle sizes to nanometers, templating crystal habits, supporting NiF2 on conductive substrates—broaden its use in both fundamental and applied research.
Toxicity Research
Experience shows that health effects of nickel fluoride demand vigilant study, not just compliance. Chronic exposure links to lung and nasal cancers, fibrotic lung disease, and skin sensitization; short-term contact brings severe burns and flu-like symptoms. Fluorides present additional risk due to their ability to bind calcium, with accidental exposures requiring rapid antidote administration and careful monitoring in emergency departments. Toxicological studies in animals document dose-dependent damage to bone, kidney, and nervous systems, while occupational health surveys track cancer and allergy clusters around nickel compound production sites. Regulations take these findings seriously, prompting low permissible exposure limits and mandatory dust controls, while environmental monitoring keeps an eye on nickel release into soil and waterways. Researchers continue probing mechanisms of toxicity, the role of individual susceptibility, and routes for safer handling or substitution in less hazardous applications.
Future Prospects
Industry and academia keep asking whether nickel fluoride can anchor the next leap in technology. Battery demands push for safer, more robust fluoride-based cathodes, aiming for higher energy density without compromising stability or worker safety. Synthetic chemists want more selective, lower-temperature fluorination agents that avoid HF’s dangers and tough waste handling—research into ligand tuning, combinatorial synthesis, and heterogeneous catalysis shows promise. Environmental science looks to advanced nickel fluoride compounds that absorb contaminants from water and soil, bringing regeneration and low-impact disposal into sharper focus. The challenge for future development comes from balancing breakthrough performance with toxicity and lifecycle cost, but improvements in process design, exposure detection, and personal protection lay the groundwork for broader, safer use of nickel fluoride in tomorrow’s materials and energy sectors.
Unlocking Some Uses of Nickel Fluoride
Nickel fluoride doesn’t find its way into headlines like lithium or cobalt. Yet, in fields that deal in advanced materials and technology, this compound quietly plays a crucial role. I’ve worked in environments where chemicals like nickel fluoride bring lab-scale innovations to life—solid-state batteries, specialized coatings, and even chemical analysis. For something that sounds as obscure as nickel fluoride, its impact stretches across several highly technical arenas.
Fuel Cells and High-Tech Batteries
The best-known use for nickel fluoride crops up in fuel cells and emerging battery technology. Engineers use it to improve the electrolytes in battery cells, with the goal of helping energy move more efficiently between the battery’s layers. This matters for electric vehicles and grid storage systems—places where better energy density and longer life cycles mean real-world improvements. According to research published by the Journal of Power Sources, nickel fluoride can help enhance ionic conductivity in certain electrolytes. This translates into batteries that hold up longer under harsh conditions, so consumer devices and electric cars can run further on a single charge.
Chemical Catalysis
Nickel fluoride helps to drive chemical transformations that wouldn’t happen otherwise. In the specialty world of catalysts, this material can spur or speed up particular reactions, making it easier to produce important compounds. Chemical plants around the world look for ways to cut costs, cut waste, and improve yields in everything from petrochemical refining to making pharmaceuticals. A versatile catalyst often makes all the difference between a process that’s sustainable and one that’s only marginally profitable.
Material Science and Electronics
Modern electronics owe a debt to compounds like nickel fluoride. At high temperatures, it can create thin films through a process called chemical vapor deposition. These coatings provide resistance against wear and corrosion, a difference-maker for high-performance devices and manufacturing tools. In my own work, I’ve seen how companies demand cleaner surfaces and finer controls in the microchips that fill our cars, phones, and medical equipment. Special coatings using compounds like nickel fluoride can boost precision, reliability, and lifespan—qualities demanded by every tech company chasing the next leap in design.
Lab-Scale Applications and Research
Academic research teams use nickel fluoride as a fluorinating agent. The lab work often looks like the backstage crew of a big concert: not glamorous, but essential. Creating new fluorinated compounds can mean breakthroughs in medicine or industrial chemistry. Many of the latest cancer drugs and agricultural chemicals rely on precise fluorine chemistry, and nickel fluoride enables some of those tricky steps to happen with fewer byproducts and cleaner outcomes.
Safety and Environmental Questions
Handling nickel fluoride calls for tough precautions. This material isn’t something workers can treat casually; its toxicity means chemical burns and respiratory problems are real risks. Regulators have set strict limits for exposure, and anyone in a lab or plant has to know emergency procedures inside and out. Safe handling isn’t just a legal box to check—it’s the difference between a healthy workday and a long hospital visit. Researchers continue to explore safer alternatives, and firms investing in green chemistry look for ways to recover, recycle, or replace hazardous compounds in their operations.
Looking Ahead: The Push for Responsible Use
With the global push toward safer, more reliable technology—from car batteries to smart sensors—compounds like nickel fluoride find new jobs every year. The emerging trend is clear: industries want high performance, but they won’t accept major health or environmental risks. The ongoing challenge lies in balancing curiosity and progress with respect for the people handling these materials. Investment in advanced safety tools, stronger regulations, and deeper training helps close that gap. Researchers keeping up with the latest studies can help spot safer approaches before they become industry standards.
Nickel Fluoride and Practical Risks
Nickel fluoride pops up in chemical labs and some specialized industrial setups. Most folks don’t see it unless they're around nickel extraction, battery production, or certain types of research. This stuff builds on nickel and fluorine, both of which raise red flags for safety teams. Just thinking about my days in a college chemistry lab, we always treated anything labeled as a nickel salt with caution. That gut-check feeling carries over here.
Health Hazards: More Than Just a Caution Sticker
Touching or breathing nickel compounds often leads to trouble. For nickel fluoride, that’s an understatement. Skin contact can spark rashes or eczema, especially if you have sensitive skin or a nickel allergy—something that affects a surprising portion of the population. Inhalation exposure can irritate the lungs, leading to coughing, shortness of breath, and in the long run, a bump in cancer risk. I remember reading a review from the International Agency for Research on Cancer, and plain as day, it put nickel compounds in the "carcinogenic to humans" category.
Swallowing nickel fluoride isn’t likely unless safety barriers completely break down, but the risk matters. Swallowing even a small amount may cause stomach pain, nausea, and more systemic problems as it moves through your body. Fluoride can disrupt calcium balance, and that gets hazardous fast. I once heard from a friend who brushed up against nickel fluoride dust—he spent hours in the ER with lung irritation booming like a bad cold.
Ways Nickel Fluoride Travels
In workspaces, airborne dust stands out as the sneakiest danger. It clings to clothing and skin, sneaks into noses and throats, and won’t hesitate to ride home on shoes. Routine spills or leaks aren’t rare in chemical plants and can coat surfaces for a shift or more. From experience, even rigorous housekeeping and showers don’t catch every speck—especially during busy periods. Without strong airflow and proper masks, staff bring problems home without knowing it.
Preventing Harm: What Works?
Good equipment keeps risk in check. Fume hoods, local exhausts, chemical-resistant gloves, and respirators aren’t just for show. Old coworkers of mine used to sigh about donning gear, then one learned the hard way after handling a broken flask. He missed a tiny tear in his gloves and needed skin treatment for weeks.
Training matters, too. Nobody wants a rushed, all-text safety manual; hands-on demos stick with people longer. Workers respond well to stories—like “Jim got sick after skipping the mask, don’t be Jim.” Leadership needs to invest in training, pay attention to ventilation upgrades, and test air regularly. Point-blank, it costs more to manage medical leave than to address hazards up front.
Moving Forward: Room for Better Tactics
Switching to safer alternatives, where possible, makes sense. Manufacturers keep searching for substitutes, sometimes swapping out dangerous nickel compounds for other materials in batteries or industrial processes. Regulators have started requiring tighter reporting and labeling standards, pushing firms to boost safety or risk heavy penalties.
Nickel fluoride won’t disappear soon, but folks can shrink risk using common sense, strong education, and equipment that works every time. If my own experience around reactive chemicals has taught me anything, it’s this: respect what’s on the label, not just what’s inside the jar.
Nickel Fluoride: The Basics
Nickel fluoride carries a chemical formula most often seen as NiF2. With nickel sitting in group 10 on the periodic table, it commonly shows up in a +2 oxidation state, pairing up with two fluoride ions per nickel ion. This compound appears as a green, crystalline material and usually lands in laboratory settings or specialized industrial processes.
Everyday Relevance in Industry and Science
This chemical may not turn heads at the grocery store, but it plays a quiet role in technology and industry. Nickel, with its own legacy in batteries and alloys, teams up with fluoride, a strong oxidizer, to produce materials in electronics and catalysts. NiF2 acts as a fluorinating agent, meaning it shares its fluorine for making other chemicals, some of which end up in pharmaceuticals or specialty chemicals.
In electrochemistry, nickel fluoride helps deposit nickel coatings through processes like electroplating. That coating protects machine parts against corrosion. Anyone who has dealt with rusty tools or worn machine gears knows why this matters to manufacturers.
Why Clarity on Nickel Fluoride Matters
Mistakes in chemistry often have real-world consequences. Handling the formula the wrong way—even just mixing up a subscript—can invite confusion, safety hazards, or lost time. Take, for example, someone who thinks they’re buying or selling NiF3 (nickel with a +3 oxidation state), which behaves differently and is tougher to come by. These errors don’t just stay in textbooks. They might show up in purchasing contracts, regulatory filings, or safety procedures.
Nickel fluoride isn’t a household name, but exposure to it should be handled with care. Breathing in nickel-containing dust can cause long-term health problems, and fluorides tend to be toxic if inhaled or ingested. Clear labeling and careful handling instructions use the precise formula for a reason. When training new technicians or labeling stock in a warehouse, these details keep people safe.
Checking the Facts: Reliable Sourcing
Reliable information on nickel fluoride comes from standard chemical databases, peer-reviewed publications, and regulatory agencies such as the NIOSH Pocket Guide. The formula NiF2 appears across major references. Reputable chemical suppliers, like Sigma-Aldrich or Fisher Scientific, use the same notation, matching regulatory filings and international safety standards. These details earn trust in the lab, on the shop floor, and in policy discussions.
Building Knowledge and Safe Practice
Chemistry can seem impenetrable with its formulas and jargon. The habit of double-checking every formula, especially for compounds like NiF2, saves headaches and sometimes protects health or investment. The details may seem small, but they shape the outcome in quality control, product development, and environmental safety. Nickel fluoride, with its simple but essential formula, gives one more reason to slow down and get the details right.
Moving Forward: Precision in a Fast-Moving World
Anyone involved with nickel fluoride—from students to engineers to regulators—benefits from remembering that the formula NiF2 stands for both precision and preparation. Good science and safe industry both depend on that kind of attention, not just for nickel fluoride but for every chemical handled in any field.
Building Safety From The Ground Up
Nickel fluoride doesn’t show up in every workplace. Where it does, folks handling it ought to keep safety at the top of the list. Forget careful storage for a moment—just taking a breath of its dust or getting it on your skin can leave you with nasty burns or worse. It can eat through metal, skin, and the lining of your lungs. Personal protective gear is far more than a box to check. From boots to gloves to a solid face shield, you want barriers that actually work. No shortcuts.
Storage: Less Drama, More Caution
Nickel fluoride likes to grab water from the air and reacts badly with most metals. Stick it in a dry, cool spot with solid ventilation. Use containers made of materials like plastic or glass, since metal can go south pretty quickly. Never put it on the bottom shelf where leaks can pool. Keep it off the floor, somewhere easy to check but tough for curious hands to reach. Signs warning of the danger aren’t for decoration—they protect everyone in the building.
Clean Work Habits, Cleaner Results
Anyone working around nickel fluoride needs real training. Folks must know what it does and what happens if you let your guard down. Washing your face and hands before a meal or a smoke isn’t just advice. You do what you can to keep the stuff out of your mouth, off your clothes, and away from anything you care about. Keep the eating and drinking far from the work zone. Use a vacuum with a HEPA filter instead of a broom for cleanup, so you don’t kick up dust for others to breathe in.
Emergencies Are No Joke
Spills don’t wait for a slow day. Plan for accidents, because the mess travels fast. Keep an eye wash and shower station close by. Spilled nickel fluoride calls for more than just a mop. Get a proper spill kit—one with calcium compounds to neutralize fluoride, along with the gear to keep it from burning skin. Make sure everyone knows where to find first-aid supplies and how to call in a hazmat team if needed.
Waste Tells Its Own Story
Pitching waste in the regular trash leads straight to environmental problems. Local and federal laws draw a hard line on how to dispose of toxic stuff like nickel fluoride. Work with a disposal company that knows the law and the science. Nobody wants this leaking into water or air, so lock up waste in sealed containers that won’t corrode and clearly label every drum.
Trust—But Verify—Your Processes
It’s easy for routines to slide, so check procedures every so often. Update your training when folks join or equipment changes. Pull out the records and see who’s handling and moving the chemical. It makes a difference if supervisors walk the floor and talk with the crew. Nobody learns safety from a poster alone.
Clear Communication Pays Dividends
Years in labs and warehouses teach one lesson: talk about mistakes and near misses. Break down the flow of tasks and point out trouble spots. Listen to the folks who actually use nickel fluoride day in and day out—they know what works and what doesn’t.
Respecting the Risk, Protecting Lives
Nickel fluoride is hard on anything living. Careful storage and strong habits help keep dangerous mistakes from turning into lasting harm. Tools, training, and real conversations set up a safer job and a cleaner environment for everyone.
Recognizing Nickel Fluoride
Nickel fluoride, a chemical compound pairing nickel with fluorine, offers up an appearance that reminds you science isn’t always about clear liquids or white powders. If you hold up a sample, you’re looking at green crystals—sometimes tending toward a bluish shade. That color doesn’t just bring visual interest to a chemist’s bench. It tells you something about the way nickel ions interact with light, and that little detail flows right into how it’s used, stored, and handled in labs and industry alike.
Physical Traits You Won’t Ignore
Those crystals don’t dissolve in water easily. Drop a bit in a beaker of room temperature water and you might stare at it for a long time before it goes away. It holds together better than many salts, resisting that urge to break apart in a watery environment. That helps with certain industrial processes where you don’t want unwanted reactions coming from something dissolving too quickly. The melting point sits up above 800°C, so it laughs off normal flame or heat sources. Bring a torch or a technical furnace, or you’re not transforming it to its liquid phase any time soon.
Sensitivity and Reactivity
Nickel fluoride looks peaceful sitting in its jar, but keep it dry. Once moisture enters the picture, things can get lively. Water and humidity help it break down, which means any open-air storage starts a slow conversion into other forms that can corrode metal containers and taint neighboring chemicals. Also, mixing it with other reactants—especially something as simple as acids—brings out its true chemical nature, releasing hydrogen fluoride gas, a highly toxic substance that you do not want anywhere near your skin or lungs.
The Real-World Importance
So why should anyone care about what nickel fluoride looks like or how it behaves? In my research past, safety always comes first. If someone mistakes nickel fluoride’s green crystals for a less hazardous compound, that could spell danger. It demands respect because it’s not just toxic on its own, but involved in processes that can turn a simple lab accident into a real emergency. Early in my lab training, one careless approach around fluorides led to a near-evacuation—not due to the material’s looks, but its overlooked tendency to react and release harmful gas. People who work with it, day in and day out, wear full gear, follow procedures, and keep rigorous logs so nothing gets out of hand.
Managing Risks and Moving Forward
Better packaging fixes half the trouble. Nickel fluoride should always stay in moisture-proof containers, preferably with clear hazard labels. Modern chemical storage focuses on segregation—keeping it far away from acids or anything that could trigger a reaction. Improved training—walking every new staff member through the risks of handling nickel compounds—helps avoid mishaps. Engineering controls, like sealed gloveboxes and reliable fume hoods, keep accidents rare. Knowing its look and its quirks doesn’t just check a box—it helps make sure everyone, from the shift chemist to the curious student, stays safe in the workplace.
Industry Uses and Future Outlook
In the big picture, nickel fluoride earns its place in producing special alloys, catalysis, and as a starting point for more elaborate nickel chemistry. Its unique green color isn’t just a curiosity—it’s a visible flag marking one of the many stops on the roadmap of modern material science. As more industries chase performance and efficiency, understanding both the physical side and the hidden risks that come with nickel fluoride keeps teams ready and products safer. Anyone working close to such compounds should remember: what you see in the beaker can matter just as much as what you measure in a test.
| Names | |
| Preferred IUPAC name | nickel difluoride |
| Other names |
Nickel difluoride
Nickel(II) fluoride |
| Pronunciation | /ˈnɪk.əl ˈfluː.raɪd/ |
| Identifiers | |
| CAS Number | 10028-18-9 |
| Beilstein Reference | 3587547 |
| ChEBI | CHEBI:78029 |
| ChEMBL | CHEMBL510879 |
| ChemSpider | 16389 |
| DrugBank | DB15325 |
| ECHA InfoCard | echa.europa.eu/substance-information/-/substanceinfo/100.028.883 |
| EC Number | 215-146-2 |
| Gmelin Reference | Gmelin Reference: 14128 |
| KEGG | C18655 |
| MeSH | D009538 |
| PubChem CID | 24558 |
| RTECS number | QR6300000 |
| UNII | 9Q2D17DJ0S |
| UN number | UN2725 |
| CompTox Dashboard (EPA) | CompTox Dashboard (EPA)": "DTXSID3077856 |
| Properties | |
| Chemical formula | NiF2 |
| Molar mass | 96.688 g/mol |
| Appearance | Green deliquescent crystals |
| Odor | Odorless |
| Density | 4.72 g/cm³ |
| Solubility in water | Slightly soluble |
| log P | -0.06 |
| Vapor pressure | Negligible |
| Basicity (pKb) | 6.15 |
| Magnetic susceptibility (χ) | +10800·10⁻⁶ cm³/mol |
| Refractive index (nD) | 1.435 |
| Dipole moment | 3.92 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 56.5 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -252.7 kJ/mol |
| Pharmacology | |
| ATC code | V03AB43 |
| Hazards | |
| Main hazards | Toxic by inhalation, ingestion, and skin absorption; causes burns; may cause allergic skin reactions; corrosive to eyes, skin, and respiratory tract. |
| GHS labelling | GHS02, GHS06, GHS08 |
| Pictograms | GHS03,GHS06 |
| Signal word | Danger |
| Hazard statements | H301 + H331: Toxic if swallowed or inhaled. H314: Causes severe skin burns and eye damage. H317: May cause an allergic skin reaction. H350i: May cause cancer by inhalation. H372: Causes damage to organs through prolonged or repeated exposure. |
| Precautionary statements | P260, P264, P270, P271, P273, P280, P284, P302+P352, P304+P340, P304+P341, P305+P351+P338, P310, P312, P314, P321, P332+P313, P362+P364, P403+P233, P405, P501 |
| NFPA 704 (fire diamond) | 3-1-3-OX |
| Lethal dose or concentration | LDLo (oral, rat): 50 mg/kg |
| LD50 (median dose) | LD50 (median dose): 175 mg/kg (rat, oral) |
| NIOSH | WF4725000 |
| PEL (Permissible) | 0.1 mg/m3 |
| REL (Recommended) | REL (Recommended): 0.015 mg Ni/m³ |
| IDLH (Immediate danger) | 10 mg/m3 |
| Related compounds | |
| Related compounds |
Nickel(II) chloride
Nickel(II) bromide Nickel(II) iodide Nickel(II) oxide Iron(II) fluoride |
