Turning back the clock, chemists first became curious about (1R)-7,7-Dimethyl-2-Oxobicyclo[2.2.1]Hept-1-Yl Methanesulphonic Acid during mid-20th century explorations into bicyclic systems. The world had already seen norbornanone frameworks show up in natural products and synthetic endeavors. From what I’ve seen in the archives and university research, this compound’s roots trace to early efforts to add functional groups to the norbornanone skeleton, looking to sharpen reactivity and tune solubility. Chemists learned a lot by observing how methanesulphonic acid, a classic sulfonic acid with strong acidity, attaches to these rigid rings. Over decades, synthetic tweaks opened up new research into stereochemistry, giving modern labs a solid foundation to understand both the unique properties and the limitations this structure presents.
Putting a spotlight on the compound, (1R)-7,7-Dimethyl-2-Oxobicyclo[2.2.1]Hept-1-Yl Methanesulphonic Acid shows the classic traits of the norbornanone family. With a methyl group crowning both bridgeheads and a sulfonic acid tacked to the rigid backbone, this molecule walks a fine line between hydrophobic and hydrophilic regions. Recent product catalogues bill it as a specialized acid, catching the attention of researchers who need a strong acid with a sturdy, non-aromatic base. Not a household name, yet its structure brings some unique advantages for catalysis and activation. The compound doesn’t just play a supporting role but can drive key steps in organic transformations, partly thanks to its unbeatable acid strength and stability under harsh conditions.
From the bench to the flask, straight observations shine a light on the compound’s stubborn physical stability. It’s a crystalline solid, white or faintly off-white, and usually comes with a sharp, sour bite if you get a whiff near the flask. The melting point usually sits reliably above 150°C, showing off a robust lattice built from the fused ring and sulfonic acid. Solubility leans heavily toward water and polar solvents—no surprise, given the punch that sulfonic acid brings. That hydrophilic tail lets the molecule easily mix into reaction mixtures looking to keep things moving. Acid dissociation in water produces protons quickly, so the compound doesn’t hang around in its protonated form for long. Chemical resistance stands out—dilute bases barely touch it, and even strong oxidants rarely break up the norbornanone skeleton.
Looking through certificates of analysis and MSDS sheets, this compound comes in technical grades at 95% or higher purity, often measured by titration against standard base or by HPLC. Product labeling, reflective of strict chemical handling policies, notes its (1R)-configuration, since enantiomeric purity can steer particular catalysis outcomes. Storage advice leans towards cool, dry locations—moisture can pull in contaminants and degrade shelf stability over long periods. Every batch gets tracked with a lot number, shelf-life, and CAS number for fast traceability. Labs keep their technical sheets close at hand: melting point range, IR spectral fingerprint, proton NMR peaks, and handling precautions written in plain language by folks who’ve worked with acidic, water-loving compounds before.
Synthesis takes some solid bench skills and patience. Most routes start from camphor, norbornanone, or related ketones. A selective methylation at the bridgehead positions, carried out with strong bases and methyl halides, gets the dimethyl substitution in position. Oxidation steps, often using chromium or permanganate oxidants, install the ketone cleanly. The tricky part comes with introducing methanesulphonic acid—direct sulfonation would wreck the norbornanone skeleton, so most chemists use a two-step approach: convert a suitable leaving group (often a halide or ester) then swap for the sulfonic acid using sodium or potassium methanesulphonate in polar solvents like DMSO. The compound salts out when acidified, letting workers isolate and purify by recrystallization. Not every attempt gives high yield, but careful control over temperature and pH keeps things running on track. What strikes me about this prep is how it brings together the old school—classic norbornene chemistry—and the modern need for functional group tolerance.
Chemists rarely let a compound stand still. (1R)-7,7-Dimethyl-2-Oxobicyclo[2.2.1]Hept-1-Yl Methanesulphonic Acid opens doors for several modifications. Acid chlorides snap on to the acid group, making the compound even more reactive. Amines react under the right conditions to build sulfonamides, which often show up in medicinal chemistry and enzyme inhibitors. The bridgehead methyls show stubborn resistance to oxidation, but careful application of radical chemistry (peroxides, UV) can add oxygen-based substituents. Direct reduction of the ketone gives secondary alcohols, which add to the catalog of derivatives for further study. What sets this compound apart is its ability to withstand harsh conditions and still provide unique handles for later transformations, especially for chemists working on dense, functionalized scaffolds.
Across catalogs, you might run into head-spinning synonyms. Some labels drop in the norbornanone reference, calling it 2-Oxo-norbornyl methanesulfonic acid. Other suppliers abbreviate the functional group, and research papers might mention it as camphor-derived methanesulfonic acid when tracing stereochemistry. Every naming scheme circles back to the same rigid core, but if you’re reading older literature, it helps to keep a cheat sheet of alternate names handy. CAS and EC numbers stand as reliable reference points, especially facing the up-and-down use of systematic vs. trivial naming.
Every time I handle sulfonic acids, the safety glasses go on before anything else. Methanesulphonic acid can burn, as anyone who’s splashed their skin or inhaled the fumes learns quickly. Standard procedure means working in a ventilated hood, gloves up, and running emergency decon as soon as the skin comes in contact. Storage needs real discipline—no open vials, and keep acids away from bases or oxidizers. Eyewash stations and acidic spill kits, not bottles of water, clean up the inevitable accidents. Long experience in the lab taught me how even small leaks can corrode metal and stain benchtop surfaces. Waste disposal matters: local regulations treat sulfonic acids as hazardous, so you don’t just dump residues down drains. Proper paperwork tracks every gram, with training programs for staff before new chemicals touch the shelf.
Let’s talk uses that reach beyond the test tube. In recent years, (1R)-7,7-Dimethyl-2-Oxobicyclo[2.2.1]Hept-1-Yl Methanesulphonic Acid found a niche as a catalyst in stereoselective acylations, especially in fields spinning out high-value chiral pharmaceuticals. Its rigid frame, combined with acid donorship, helps push reactions along where other acids stumble, avoiding side reactions in crowded environments. Polymer scientists tried the compound as a crosslinker for specialty resins, harnessing both the acidity and the shape-persistent skeleton. Some environmental chemists experimented with it as a cleaning agent in formulations where aromatic acids would choke waterways, hoping for a mix of strong action and easy removal. Every application runs up against cost and availability, but where the balance tips, the compound delivers.
University groups and some adventurous pharma firms keep turning over new rocks with this molecule. Students grind through analog syntheses, racing to install new substituents and hand-pick alternate stereocenters. A few years ago, teams published work on its use in asymmetric Diels-Alder catalysis, showing improvement over standard Lewis acids in both speed and selectivity. Development pipelines see it as a platform, a rigid structure primed for late-stage functionalization. Funding cycles and grant agencies always ask for environmental fates; new research tries to map breakdown products in simulated wastewater and biotransformation by soil microbes. Computational chemists use the molecule to calibrate acidity scales for modeling, since it offers a rare mix of strong acidity and well-defined geometry.
On the safety front, the literature points to methanesulphonic acid’s strong corrosiveness. Animal studies flag skin and eye irritation at low exposure. The bicyclic core, by itself, doesn’t raise major toxicological alarms, but sulfonic acids can push systemic acidosis at high doses. Chronic exposure in animal models shows little in the way of bioaccumulation, but nobody wants to get careless. Regulatory databases rank it as a hazardous material, but not classed as mutagenic or carcinogenic at research scale handling levels. Reports on inhalation hazards suggest symptoms like coughing and shortness of breath, which match reports from old-timers who worked full shifts with far less PPE than modern labs demand. Safety protocols, updated every year, aim to keep all incidents to zero, with annual retraining and spot checks by safety officers.
Looking ahead, demand for specialized acids with both acidity and molecular rigidity won’t slow down, especially as chemists push toward greener processes and more selective pathways. The molecule’s strong acid function—combined with a stubborn, hydrophobic core—lines up with trends in solid-phase catalysis and recyclable acid reagents. Industry talks about replacing petroleum-derived acids in certain syntheses with more functionalized, precise tools. If production scales up and price drops, expect to see new uses in fine chemicals and maybe even electronics, where unique acid sites can pattern surfaces without the unpredictability of weaker acids. Further toxicity studies and environmental breakdown research will need to keep pace: companies can’t afford to chase applications unless environmental safety stays front and center. As more researchers find ways to stretch this compound’s range, the story of (1R)-7,7-Dimethyl-2-Oxobicyclo[2.2.1]Hept-1-Yl Methanesulphonic Acid looks far from finished.
No one wakes up thinking about (1R)-7,7-Dimethyl-2-Oxobicyclo[2.2.1]Hept-1-Yl methanesulphonic acid, but this tongue-twister of a molecule plays an interesting role in the chemical and pharmaceutical world. It’s a camphor derivative, and camphor itself has a deep history in traditional medicine, fragrances, and even plastics. Once you attach a methanesulphonic group, the compound gains new chemical behavior. The structure creates a solid backbone for researchers designing drugs because it brings stability and unique reactivity, which often gets overlooked in more general discussions about chemical intermediates.
Drug makers don’t often talk to the public about these building-block molecules, but those small moves in the synthesis lab shape the medicines on pharmacy shelves. This acid variant can step in as a chiral auxiliary. Think of it as a molecular guide, helping chemists assemble complex structures in the right three-dimensional way. Stereochemistry isn't flashy, but it's the difference between a safe treatment and something that does nothing—or worse, causes side effects. For example, when synthesizing antiviral agents, antibiotics, or pain relievers, researchers demand both precision and reliability, and that’s where this molecule really makes a difference.
One of the main draws comes from how the methanesulphonic acid group cranks up polarity. This makes the molecule work well in certain reactions where regular camphor would just sit out. In labs, chemists use it to add, remove, or tweak other groups with both speed and accuracy. I’ve watched researchers reach for this compound when they needed to streamline a reaction or to solve a bottleneck that kept stalling larger projects. Its reactivity often helps reduce chemical waste and shortens the steps needed to arrive at a finished product.
This molecule acts as a stepping stone to craft advanced pharmaceutical compounds. During my time shadowing a pharmaceutical chemist, the search for safer, more effective painkillers always circled back to how these small chemical tweaks made big changes. For instance, its influence on creating optically pure drugs means medications can be made with fewer side effects and more predictable outcomes for patients. By improving purity and control, pharmaceutical companies can bring new therapies to market that actually work better for real patients, not just on paper.
Another less-talked-about benefit involves green chemistry. Companies push to minimize hazardous waste, and efficient reagents like (1R)-7,7-Dimethyl-2-Oxobicyclo[2.2.1]Hept-1-Yl methanesulphonic acid fit that bill. Fewer byproducts in plant-scale synthesis lines mean less strain on cleanup crews and less risk for communities living nearby. Back in university labs, I saw how the shift to smarter, cleaner chemistry became a badge of honor in some research circles—showing that scientists could hit their goals without leaving a mess behind.
The pressure on chemists isn’t just to invent new drugs and processes but to keep it green, safe, and affordable. By taking advantage of molecules like this, the industry inches closer to meeting health needs without raising new environmental risks. Encouraging more research funding, better training in chemical safety, and real collaboration between labs and industry means molecules like these can make an even bigger difference in years to come. With patients and the environment on the line, small chemical upgrades matter more than most people realize.
Stepping into a lab always brings a rush—a mix of curiosity and respect for the tools at hand. Chemical names as long as a bus ride like (1R)-7,7-Dimethyl-2-Oxobicyclo[2.2.1]Hept-1-Yl Methanesulphonic Acid, often called camphorsulfonic acid, hint at layers of complexity. Every time a new substance lands on a workbench, past experience demands a fresh look at its quirks, and no shortcut replaces careful handling.
This sulfonated camphor derivative isn’t the kind you’ll find on the shelves at the neighborhood hardware store. Often found in pharmaceutical research, it works as a catalyst or reagent. The hunt for safety data starts with the material safety data sheet (MSDS), which offers a snapshot of hazards, exposure risks, and best storage practices. The MSDS for camphorsulfonic acid lays out some clear warnings—skin and eye contact can irritate, and inhaling dust creates respiratory woes. Working with acids, even if they seem “mild”, taught me fast that irritation can become a big problem without gloves and goggles.
Some labs stick with this acid for chiral resolution or as a salt-forming agent; the appeal comes from its effectiveness, but few chemists forget the risk tied to concentrated acids. Spills sting, and sometimes the consequences show up hours after the fact. Knowing the acid won’t explode or burst into flames if handled right gives some reassurance, but its corrosive nature rules out casual use.
Watching seasoned chemists handle hazardous reagents shaped how I operate. Fume hoods do the heavy lifting; they keep vapors out of your lungs. I once ignored a fume hood with toluene—not a mistake I repeated. Splash-resistant lab coats, proper gloves, and full goggles become standard, especially with substances that burn or irritate. Common sense takes the front seat—no one eats lunch at a bench or grabs reagents with bare hands. Proximity to an eyewash station and safety shower matters, and so does labeling. More than one scare has unfolded because someone filled a beaker with something “clear” and passed it off as water.
New techs in the lab sometimes feel that safety training drags, but stories from longtime staff reach people. Concrete examples of accidents—close calls with acids, ruined clothes, or emergency doctor runs—stick longer than a long slideshow of rules. After every minor spill or close call, the lesson gets reinforced: anticipate mistakes instead of reacting to them.
Organizations like OSHA and the American Chemical Society push for continuous improvement in lab safety. Regular audits, accessible MSDS repositories, and open communication channels keep labs prepared. In research, pressure to hit results can nudge best safety practices out of sight, but ignoring protocol sets up bigger trouble. The safest researcher isn’t the one with the thickest gloves or the strongest hood—it's the one who pauses to ask, “What could go wrong?” before opening a new bottle.
There’s never comfort in complacency. Training never stops; chemistry moves, and regulations shift as science uncovers new data. Labs keep looking for less hazardous reagents or smarter engineering controls. Alternatives for camphorsulfonic acid exist for some tasks, but swappability depends on the project. Collaborating with safety officers, reporting incidents without blame, and backing a culture that values prevention all bring real improvements.
Looking at the long name, many people might hesitate, but this compound is not just a handful for spelling—it also asks for genuine caution during storage. Chemical stability and personal safety go hand in hand. If engineers and researchers ignore practical storage steps, a workspace can become hazardous overnight. The importance of learning good storage habits has only grown as more labs, both professional and amateur, expand their work with new compounds. One misstep stacks up, leading to potential chemical reactivity, spoilage, or even injury. From spills in school labs to costly damage at companies, improper storage delivers real consequences.
A compound like this one doesn't appreciate swings in temperature or light. Heat can push it toward decomposition. Light sometimes speeds up unwanted side reactions. I’ve seen solvents and acids cook up surprise reactions after a careless hour on a sunlit bench, which proved one important fact: darkness and a cool room never disappoint when handling sensitive molecules. Even for casual users—hobby chemists, teachers, grad students—the best bet has always been a climate-controlled cabinet, preferably well labeled and secure.
Exposure to humid air encourages clumping, hydrolysis, or at worst makes the compound unstable. Sulphonic acids often draw water from the environment, acting almost greedy. I remember losing an entire sample to clumping thanks to a humid afternoon and an uncovered jar. People rarely see this coming, yet sealed containers, especially glass with a tight cap, bring peace of mind. Adding a silica gel pack or using a desiccator can keep the moisture out, and that means longer shelf stability and safer handling, lesson learned.
It never pays to let organic acids mix with strong bases or oxidizers. Labs that skip proper segregation often face avoidable hissing, bubbling, or fumes. Safety depends on placing reactive substances alone or with chemical relatives. Organizing cabinets by hazard class—acid here, base there, oxidizer isolated—cuts down on close calls. Labels help, but clear separation sets the tone for responsible work, giving every user and visitor clear guidance about dangers present.
Chemical suppliers and regulatory agencies offer advice based on years of practical evidence. The European Chemicals Agency points out the need for both physical security and environmental control, given the health risks and the compound’s sensitivity. I’ve adopted these habits: always use the original packaging for storage, avoid metal shelves (some acids corrode metal), and maintain a spill kit nearby. Routine inventory checks minimize unpleasant surprises—old, forgotten chemicals pose greater risks than fresh stock.
I learned quickly that informed workers build safer labs. If you work with chemicals, reading the Safety Data Sheet always beats guessing. Proper gloves, goggles, and protective clothing never disappoint, and accidents rarely wait for the weary or unprepared. Training new workers and students on good storage habits pays forward, building an environment where safety wins out over shortcuts.
Responsibility never fades in the lab. Simple, affordable measures—climate control, sealed glass jars, organized cabinets, and clear labels—keep both people and compounds safe. Teaching and reminding colleagues about these steps anchors a safety-first mindset. Storage, at its core, isn't only about protecting chemicals; it's about protecting the people who use them every day.
For those who’ve handled organic chemistry, the name (1R)-7,7-Dimethyl-2-Oxobicyclo[2.2.1]hept-1-yl methanesulphonic acid triggers immediate recall of the norbornanone core. In plain terms, this compound starts with a norbornane skeleton—bicyclo[2.2.1]heptane—outfitted with two methyl groups at one position (carbon 7), and a keto group perched at position 2. Instead of stopping there, chemists attached a methanesulphonic acid group to what's called the “1-yl” location, with the precise 1R stereochemistry.
For someone in the lab, breaking this down brings value. If you've ever tried to draw it from scratch: you sketch a “house” shape (the canonical norbornane) and stick two methyls onto the rooftop, pop an oxo group onto the bridge, and add a methane sulfonic acid at the exit. That leaves you with a molecule that doesn’t just manage to be sturdy but also quite polar, thanks to the acid side chain and the carbonyl.
One of the main features of this molecular setup is rigidity. Norbornanone derivatives figure often in pharmaceuticals and chemical research because they don’t easily flop around like long-chain compounds. That rigidity can be the difference between a useful inhibitor and a bystander, especially in drug discovery, where shape and function track closely.
Now, layering on the methanesulphonic acid group enhances water solubility. Most bicyclic ketones like norbornanone don’t mix well with water—fine if you're working with oils or organic solvents, but not so helpful in biological systems, which run on water. Methanesulphonic acid groups offset this, allowing chemists to shuttle the compound into solution, test activity, and isolate what works.
From time in the research lab, I remember the challenges. Methanesulphonic acid groups bring their own headaches—low volatility, sticky residues, stubborn cleaning jobs after synthesis. But the payoff is real. These groups can be more gentle to enzymes or living tissues than some other sulfonic acid alternatives. Sulfonic acids also act as excellent leaving groups, so attaching or replacing functional groups in a larger synthesis isn’t such a slog.
It gets interesting if you want to make this structure. The norbornanone framework often comes from a Diels-Alder reaction between cyclopentadiene and a dimethyl-substituted alkene—classic “click” in a flask, bumping up yields and saving days of column chromatography. Installation of the sulfonic acid calls for strong reagents and some nerve, since you want clean attachment without wrecking the sensitive ring.
As research into rigid, water-soluble compounds grows, derivatives like this one matter more. They're not just chemistry puzzles; they give scientists reliable starting points in making drugs more stable, more predictable in action. Water solubility and stability help lower costs, cut waste, and can speed up projects in fields from green chemistry to diagnostics. Drawing on these lessons, today’s synthetic chemists push for cleaner methods that clip on functional groups without harsh waste or tricky cleanup.
Chemistry isn't only about the next novel molecule; it’s about stretching what’s possible with old friends like norbornanone, tailoring reactivity, and learning from each run, spill, or breakthrough along the way.
Anyone working in a chemical lab or an industrial setting knows that new compounds always challenge our day-to-day practices. (1R)-7,7-Dimethyl-2-Oxobicyclo-2.2.1-Hept-1-Yl-Methanesulphonic Acid—let’s just call it a mouthful of a molecule—brings interesting physical and toxicological properties. Terpenoid-based sulfonic acids like this one draw eyes in pharmaceutical and organic synthesis research, yet safety data often remains limited compared to legacy compounds.
This compound builds off natural camphor structure, but modification with a methanesulphonic acid group changes the game. Like other sulfonic acids, risk usually links to corrosivity. I’ve handled methanesulphonic acid in a research lab setting, and accidental contact burned skin fast, even at low concentrations. Add the bicyclic backbone, and you can expect some volatility and increased reactivity with some organic bases.
Toxicity data for this exact molecule is limited, but parent chemicals like camphor sometimes lead to neurotoxic effects if absorbed in substantial amounts. Sulfonic acids do not help here; they boost cell membrane penetration. Eyes and lungs become vulnerable. Many chemists, including myself, rely on conservative approaches: double-gloving, strict fume hood work, and splash-resistant eyewear whenever possible. Safety Data Sheets for similar compounds outline risks including severe burns, respiratory irritation, and delayed tissue damage.
Mixing sulfonic acids with strong bases shoots pH through the roof and produces heat—sometimes violent. Contact with oxidizers or reducing agents often triggers uncontrolled reactions. Most concerning, sulfonic acids can react with alcohols, amines, or even some plastics. Personal experience saw methanesulphonic acid slowly eat through nitrile gloves and react with simple glassware coatings. That’s an important note for folks relying on older equipment in academic labs or start-ups tight on budget.
Camphor derivatives also interact poorly with strong oxidants, producing toxic fumes or side products. This can create real hazards for work with transition metal catalysts or in pharmaceutical development settings.
Solid storage protocol cuts down risk sharply. Keep the container sealed, dry, and away from incompatible chemicals. I always tuck away acids like these in ventilated acid cabinets and double-check labels. A splash of this compound on skin can cause delayed symptoms; one colleague I know discovered a nasty burn several hours after a small splash. Prompt washing and medical consultation become crucial.
Ventilation matters—the compound evaporates more than you’d think, and those fumes attack soft tissues with little warning. Capitalizing on PPE and proper scrubbers in exhaust systems gives workers extra peace of mind. Lab managers do well to keep calcium carbonate handy for neutralizing accidental spills, though I’ve seen cases where even small spills require a full safety shutdown.
The industry’s hunger for new, efficient building blocks keeps pushing compounds like this into regular rotation. Lack of deep toxicity data often trails behind commercialization. Open data sharing and risk communication inside research groups help plug knowledge gaps, but nothing replaces hands-on training. New researchers should learn from veteran chemists about the subtleties of sulfonic acids and their unpredictable reactions.
A culture of respect for chemicals—no matter how routine they seem—boosts safety in ways that regulations alone cannot enforce. This approach keeps hazardous events rare, even as labs move into more innovative chemistry.
![(1R)-[7,7-Dimethyl-2-Oxobicyclo[2.2.1]Hept-1-Yl]Methanesulphonic Acid](/static/81c4c90b-3bfe-4770-bbec-fcbf5e0a3809/images/2d/1r-7-7-dimethyl-2-oxobicyclo-2-2-1-hept-1-yl-methanesulphonic-acid.png)
![(1R)-[7,7-Dimethyl-2-Oxobicyclo[2.2.1]Hept-1-Yl]Methanesulphonic Acid](/static/81c4c90b-3bfe-4770-bbec-fcbf5e0a3809/images/3d/1r-7-7-dimethyl-2-oxobicyclo-2-2-1-hept-1-yl-methanesulphonic-acid.gif)
| Names | |
| Preferred IUPAC name | (1R)-[7,7-dimethyl-2-oxobicyclo[2.2.1]heptan-1-yl]methanesulfonic acid |
| Other names |
Camphorsulfonic acid CSA 10-Camphorsulfonic acid 10-Camphorsulphonic acid [(1R)-exo]-(+)-Camphorsulfonic acid |
| Pronunciation | /ˈwʌnˌɑːr ˈsɛvən ˈsɛvən daɪˈmɛθɪl tuː ˈɒksəʊ baɪˈsaɪkloʊ tuː ˈtuː ˈwʌn ˈhɛpt wʌn ɪl ˈmɛθeɪnˌsʌlˈfɒnɪk ˈæsɪd/ |
| Identifiers | |
| CAS Number | 118276-58-1 |
| Beilstein Reference | 635899 |
| ChEBI | CHEBI:142208 |
| ChEMBL | CHEMBL3029988 |
| ChemSpider | 21530611 |
| DrugBank | DB08798 |
| ECHA InfoCard | 10d4b552-173b-4986-93cc-7d272377ae00 |
| EC Number | 3.1.1.1 |
| Gmelin Reference | 1578317 |
| KEGG | C06267 |
| MeSH | Dronedarone |
| PubChem CID | 11423014 |
| RTECS number | RC9173500 |
| UNII | XA977A1Y1K |
| UN number | UN2811 |
| CompTox Dashboard (EPA) | DTXSID4039237 |
| Properties | |
| Chemical formula | C10H16O4S |
| Molar mass | 236.29 g/mol |
| Appearance | White solid |
| Odor | camphoraceous |
| Density | 1.32 g/cm³ |
| Solubility in water | Slightly soluble |
| log P | 1.018 |
| Vapor pressure | 0.00000000000536 mmHg at 25°C |
| Acidity (pKa) | 2.06 |
| Basicity (pKb) | -3.6 |
| Magnetic susceptibility (χ) | -8.15 × 10⁻⁶ cm³/mol |
| Refractive index (nD) | 1.512 |
| Dipole moment | 2.04 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 389.6 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -586.7 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | -1382.6 kJ/mol |
| Pharmacology | |
| ATC code | M01AE16 |
| Hazards | |
| Main hazards | Causes skin irritation. Causes serious eye irritation. May cause respiratory irritation. |
| GHS labelling | GHS02, GHS07 |
| Pictograms | GHS05 |
| Signal word | Warning |
| Hazard statements | H315, H319, H335 |
| Precautionary statements | Precautionary statements: P260-P280-P305+P351+P338-P301+P312-P304+P340 |
| Flash point | Flash point: 121.1 °C |
| Lethal dose or concentration | LD50 oral rat 384 mg/kg |
| LD50 (median dose) | LD50 (median dose): Rat oral 2600 mg/kg |
| NIOSH | RN 1335-19-5 |
| PEL (Permissible) | No OSHA PEL established. |
| REL (Recommended) | 0.62 mg/m³ |
| Related compounds | |
| Related compounds |
Camphor Borneol Isoborneol Camphor sulfonic acid Menthone Fenchone Norcamphor |
