© 2026 Nanjing Finechem Holdings Co., Ltd,
All Right Reserved
Years ago, organic chemists relied on simpler benzoyl chlorides, but ambitions kept growing. The moment 2-naphthoyl chloride hit synthetic laboratories, things changed. Originally, naphthalene chemistry was the playground of dyestuff makers and early pharmaceutical tinkerers. The shift to specialized acid chlorides took off in the late 19th and early 20th centuries as curiosity about aromatic systems deepened. Researchers figured out that, by tweaking the naphthalene ring, new routes opened up for dyes, drugs, and agrochemicals. That’s how 2-naphthoyl chloride ended up as a pivotal compound for anyone chasing robust coupling reactions or thinking beyond simple benzoylation tricks. Folks in academic labs saw its potential around the same time as industrial chemists, laying the groundwork for decades of method development and material innovation rooted in aromatic acid chloride chemistry.
2-Naphthoyl chloride looks like a pale yellow to off-white crystalline solid, and its sharp, acrid scent gives a heads-up before any spill gets out of hand. It falls into the class of acid chlorides, storing up plenty of reactivity in that carbon-chlorine bond just waiting for the right nucleophile. Most people outside a lab probably haven’t seen this stuff, but its fingerprints turn up in the structural backbone of specialty materials, certain pharmaceuticals, and research reagents. Every bottle screams caution, but researchers who need selective acylation or want a route into a broader naphthalene scaffold turn to this one with confidence.
Looking at pure stats, 2-naphthoyl chloride displays a melting point in the range of 64-67°C. Its boiling point clears 280°C, often breaking down before reaching that mark. The compound shows reluctance to mix with water, preferring organic solvents like ether, benzene, or chloroform. What stands out, though, is its robust reactivity, especially toward water, alcohols, and amines. Exposure to the ambient air quickly sucks up moisture, releasing hydrogen chloride fumes. In the fume hood, you can practically see its energy waiting to leap into action, whether you’re gunning for an amide, ester, or tackling a Friedel-Crafts acylation. Its naphthalene ring adds some pi-stacking muscle, inviting opportunities in advanced materials or molecules needing aromatic punch alongside simple reactivity.
In chemical supply catalogs, 2-naphthoyl chloride usually appears with CAS number 132-85-4, sporting an assay above 98%. Labels mention irritant and corrosive symbols, making it clear that a careless touch would sting. Technically, the product’s purity can make or break a reaction, especially in pharmaceutical or dye synthesis where side reactions toss in unwanted color or activity. Actual packaging pulls in airtight bottles, often under a blanket of dry nitrogen. That’s not just for show—it stops moisture from spoiling the batch before anyone can use it, because even trace water can kick off a chain reaction. Storage recommendations point toward cool, dry areas with tight access, and every seasoned chemist gives it the respect reserved for a volatile, lung-biting acid chloride.
No way around it—classic preparation routes dominate here. Reacting 2-naphthoic acid with thionyl chloride is the old standby. The mixture bubbles quietly, belching out sulfur dioxide and hydrogen chloride as the acid chloride forms. Some labs prefer phosphorus pentachloride, especially for larger scale work, but thionyl chloride’s side products evaporate cleanly, simplifying the post-reaction cleanup. Extra care in controlling temperature and avoiding excess moisture keeps yields steady and limits byproduct headaches. One thing is clear: Synthesis of 2-naphthoyl chloride highlights the blend of skill and patience behind any good chlorination step.
Chemically, 2-naphthoyl chloride carries a versatile toolkit. The acid chloride group turns it into a gateway molecule for making amides, hydrazides, esters, and other derivatives—critical in medicinal chemistry projects chasing new biological activity. Adding an amine at low temperatures delivers naphthamide, a recurring motif in dye and drug scaffolds. With alcohols, the story moves toward esters, where naphthoyl flavor brings fresh solubility and stability tricks. Friedel-Crafts acylation stands out, letting the aromatic core get attached to other rings and frameworks. Industrial teams use it for surface modification or as a component in advanced liquid crystals and organic semiconductors. Across all these reactions, a steady hand and dry solvents go a long way—contamination means side products, and those clog up purification or taint the yield.
Anyone hunting through literature might find 2-naphthoyl chloride listed as beta-naphthoyl chloride or sometimes 2-naphthalene carbonyl chloride. The original German texts often used “2-Naphthoylchlorid,” tracing back to dye production research. While synonyms can trip up newcomers, understanding the name variants prevents purchasing mistakes and helps with literature searches in patent filings, chemical databases, or journal articles. It pays to check the context—dye chemists in the mid-20th century had their own naming quirks, as did the pharmaceutical and polymer sectors.
This compound doesn’t play around when it gets loose in the lab. 2-Naphthoyl chloride releases corrosive, choking fumes on contact with water or skin, making full personal protective gear essential for anyone handling it. Direct skin contact triggers rashes, and inhalation of vapors can inflame the respiratory system, so most labs keep it on strict fume hood duty. Storage demands airtight containers, solid venting, and a far corner away from acids, bases, or any chemical eager to react. Modern safety guidance leans on good ventilation, eye protection, thick gloves, and never cutting corners on waste disposal. Trained chemists respect its hazards, and that goes double for anyone teaching undergrads—everybody remembers how quickly it can turn a simple synthetic step into a safety lesson.
So many threads tie back to 2-naphthoyl chloride in niche and mainstream chemistry. In the pharmaceutical industry, it has a role in building blocks for antihistamines, antifungals, and more—especially through its amide derivatives. The dye industry taps its reactivity to anchor colorants like azo dyes onto naphthalene skeletons, cementing its place in textiles and inks. Organic materials research treats it as a launchpad for liquid crystals, advanced polymers, or tailored optoelectronic components. Smaller specialty shops employ it as a key step in functionalizing molecules for sensors or photostable adhesives. Its versatility draws a line between established industrial procedures and emerging nanomaterials, bridging gaps between eras and disciplines.
For chemists working on the edge, 2-naphthoyl chloride opens doors that other acid chlorides can’t. Research teams have tinkered endlessly with reaction conditions—new catalysts, milder bases, or exotic solvents—hoping to boost selectivity or reduce harsh byproducts. The naphthalene backbone adds bulk and electronic character, letting medicinal chemists tune drug candidates or synthetic intermediates that step into biological targets with precision. Environmental scientists study greener chlorinating reagents to cut down on toxic waste, and industrial chemists fine-tune every process to extract a purer, more cost-effective product. The compound stands at the crossroads of heritage methods and green chemistry innovation, egging on researchers to find safer, smarter ways to leverage its reactivity.
Toxicity always tops the list of concerns in chemical development, and 2-naphthoyl chloride is no exception. Researchers track acute effects on skin, eyes, and lungs, identifying it as corrosive and potentially sensitizing—a single spill can affect lab workers for days. Long-term exposure studies prompt stricter controls, especially since the compound’s hydrolysis product, 2-naphthoic acid, also carries moderate irritation risks. Regulations in Europe and North America set airborne exposure limits and toughen disposal rules to shield workers and communities from accidental releases. Toxicity drives new research toward encapsulated or solid-phase versions, which lower the chance of exposure and keep the chemistry running safer, even in teaching environments.
Even though acid chlorides sometimes get overshadowed by flashier reagents, interest in 2-naphthoyl chloride won’t dry up. Synthetic chemists demand versatility and reliability, and this compound checks those boxes for functional group transformations in crowded, challenging molecules. Expect to see more research on greener chlorination methods, aiming for efficient preparation without the weight of problematic byproducts. Application areas keep expanding, especially as advanced materials crave naphthalene derivatives with precise electronic and structural properties. Green chemistry advocates push for closed-loop systems and safer, less volatile analogs. Whether in pharmaceuticals, electronics, or sustainability circles, this unassuming solid promises a long future anchored by firsthand experience, tough lessons, and ongoing innovation.
2-Naphthoyl chloride never turns up in casual conversation, but it stays busy behind the scenes of research labs and factories. If you have any familiarity with organic synthesis, this chemical’s odd-sounding name rings a bell. It sits among those potent reagents—formidable, sometimes fussy, and definitely useful. Companies often need this compound as a building block for projects that require sturdy molecular “scaffolding”—aromatic rings ready to hold on tight to whatever chains scientists bolt on.
Medicinal chemistry often calls on 2-naphthoyl chloride for its strong acyl chloride group. It acts like a handshake, making it easy to link the naphthalene backbone to new structures. When chemists want to build drugs, they start by assembling basic frameworks. 2-Naphthoyl chloride supplies that crucial naphthalene core, which supports antihistamines, anti-inflammatories, and sometimes even anticancer agents. Researchers can pull off a naphthoylation reaction, shape-shifting amines or alcohols into new medicines. It may sound simple, but I’ve seen how a single streamlined reaction can shave weeks off a discovery schedule.
Factories use 2-naphthoyl chloride while crafting dyes and pigments. Its naphthalene skeleton lends strength and vibrancy to colorants for fabrics, paints, and plastics. I remember a textile engineer describing how chlorine-substituted intermediates help set the exact tone for designer clothes. You want your favorite red shirt to stay bright after a dozen washes? There’s a good chance molecules built from chlorinated naphthalene, like 2-naphthoyl chloride, are mixed into it. This compound becomes the launchpad for azo dyes—the workhorses of color production.
Some of the most common plastics and polymers start their life as a pile of aromatic scraps and clever chemistry. 2-Naphthoyl chloride gets combined with amines and alcohols to form tailored monomers. These monomers go on to form resins or advanced plastics that can weather more heat or sunlight. Agricultural chemists sometimes turn to this compound when designing new herbicides and fungicides. Adding a naphthalene ring often changes how a molecule snuggles into a pest’s enzyme system—sometimes shutting them down entirely.
Working with 2-naphthoyl chloride calls for caution. It reacts with water to release hydrochloric acid fumes and tends to irritate the skin or eyes. In my experience, the bottle always lives in a well-ventilated fume hood, gloves on hands, and a bottle of neutralizer nearby. Many labs have replaced outdated chemicals with cleaner, safer reagents where possible. Still, 2-naphthoyl chloride persists in professional use since it brings precision and efficiency where it counts.
Industrial chemists keep searching for cleaner, greener production methods. Strategies include recycling solvents, using solid-supported reagents, or swapping out dibasic chlorides for less hazardous equivalents. Green chemistry teams study how to avoid harsh byproducts or energy-hungry conditions. If sustainable research budgets remain steady, large-scale manufacturers might see safer, more affordable acylating reagents in the next decade.
2-Naphthoyl chloride shows how a molecule can make ripples through technology, health, and manufacturing. Every new drug, colorfast dye, or high-performance polymer stands on the shoulders of old chemical know-how—and a few sharp, highly reactive tools. I’ve learned it pays to know what’s in each bottle, and never underestimate the impact of a single chemical on the everyday things we trust and use.
Chemistry often feels like a jumble of names and numbers, but getting the formula right actually makes a big difference. 2-Naphthoyl chloride, for instance, combines practical applications with some real academic challenges. Its molecular formula is C11H7ClO. Seems simple, but let's break it down.
During my undergraduate days, I lost count of the number of hours spent hunched over reaction schemes. One small misstep—a number off in a formula—could send a whole project down the drain. The difference between C11H7ClO and something with an extra hydrogen or missing a chlorine means a world of difference in lab results. Fact is, 2-Naphthoyl chloride’s structure comes from naphthalene, which looks like two benzene rings fused together. Swap out the right hydrogen for a chlorine atom and a carbonyl, you get this building block.
The importance doesn’t stop at pure chemistry. Synthetic chemists use 2-Naphthoyl chloride often as a stepping stone to make dyes, pharmaceuticals, and herbicides. Missing the right formula can jeopardize safety in the lab. Chlorine atoms bring in their own set of risks if they’re not handled carefully. Storage, labeling, and disposal all hinge on the right chemical specification. Restrictions around chlorinated compounds frequently tighten because of their interactions in biology and the environment.
C11H7ClO translates to 11 carbons, 7 hydrogens, 1 chlorine, and 1 oxygen. That fits the blueprint for handling the compound’s reactivity. Chlorinated aromatic acids form tight bonds and don’t play nicely with water—this makes the compound more reactive for synthetic uses but also harder to manage. When the formula is wrong on a shipment or a label, labs could face lost money, ruined experiments, or much worse, serious health hazards.
Mistakes in chemical identifiers still slip through, even in reputable supply chains. Global organizations like the International Union of Pure and Applied Chemistry (IUPAC) keep things in check by setting global naming and identification standards. Not everybody reads the fine print though, especially outside of research centers. My own lab once received a mislabeled container—the difference between a chloride and a carboxylic acid doesn’t show up until a reaction fails or something starts smoking. For professionals handling these things, a correct molecular formula isn’t just academic, it’s survival.
More universities and companies now push for barcode scanning and digital records, which can catch mistakes faster. AI-driven inventory systems show promise, but training and review by hands-on chemists keep labs safer. Regulatory agencies like OSHA and REACH require exact cataloging. For those just learning chemistry, nailing the formula for 2-Naphthoyl chloride (C11H7ClO) gives a small but real sense of why accuracy counts. This plays out in labs and factories, affecting research, business, and—at the end of the chain—public health.
Anyone who works in a lab knows some chemicals demand extra respect. 2-Naphthoyl chloride isn’t a household name, but it can ruin your day in a hurry if you get careless. The reason? Its reactivity, potential health hazards, and the harmful fumes it releases make it unforgiving. This chemical can irritate eyes, skin, and lungs and doesn’t play nice with moisture. Leaving it on an open shelf or keeping it in a cracked bottle spells trouble.
Years ago, I watched a coworker ignore a damp seal on a reagent bottle. It only took a week before the air smelled sharp and acrid near the storage cabinet. It turned out the container had pulled in moisture, and the chemical inside had started reacting—just as 2-Naphthoyl chloride would. That lesson cost the lab time, money, and peace of mind. Ever since, I’ve double-checked container seals and stuck to recommended storage conditions, even if that means an extra trip across the lab.
Keep this chemical away from any source of water. Even humidity in the air can cause it to break down, releasing hydrochloric acid and putting people at risk. Every storage area I’ve trusted for 2-Naphthoyl chloride has been dry, cool, and well-ventilated. I never rely on a fancy fume hood alone—those can get crowded—I find a spot specifically dedicated to reactive acyl chlorides so nothing gets mixed up.
Glass containers with tightly fitting, chemically resistant caps stay my go-to choice. A basic plastic lid doesn’t cut it. Glass gives a clear view if the compound begins to discolor or the crystals start clumping, signs that something’s gone wrong. I label the date it went in storage on every single bottle. That habit comes from dealing with mystery bottles left by other people—an expiration date keeps everyone honest and safe.
Not every lab budget stretches to purpose-built cold storage, but the closer to room temperature, the better for this compound. Extreme temperatures tend to accelerate chemical breakdown. Don’t stick 2-Naphthoyl chloride in a freezer, though—condensation can sneak in every time the door opens, inviting water into the mix. A cool, steady shelf suits it better. Direct sunlight also speeds up its decay, so I stick it in the back, away from window glare.
OSHA and the National Institute for Occupational Safety and Health (NIOSH) both recognize the risks that come with improper chemical storage. To stay in line with their guidance, I run inventory checks every month. That routine finds leaks early and reminds me to dispose of chemicals that are past their prime, using a licensed hazardous waste handler. High-quality gloves and eyewear become non-negotiable if you’re handling open containers. I make sure fresh spill kits sit close at hand—one flour incident taught me spills won’t wait for permission.
Label everything. Inspect seals before leaving the storage room. Never store with acids, bases, or water-reactive chemicals. Tell your team what’s where and what looks off. The right habits make things safer for everyone, whether you’re working in a top university or a small industrial lab. Storing 2-Naphthoyl chloride safely isn’t just a rule, it’s common sense learned from hard lessons and a healthy respect for chemicals that don’t forgive carelessness.
2-Naphthoyl chloride doesn’t show up outside the lab very often, but for the folks who handle it, the risks deserve straight talk. This stuff comes out looking like a pale-yellow solid and goes into processes that build dyes, medicines, and advanced polymers. Over the years, I’ve come across situations where a small lapse in safety left someone with a burn, a cough, and plenty of regret. Behind all that chemistry sits a real need to treat some substances with more respect.
This chemical stands out because it reacts fiercely with water and moisture from the air. Touching it without proper gloves causes skin burns—sharp, fast, painful. If it turns to dust or vapor and gets in the air, you bet it burns the eyes or airways. These aren’t mild irritations; we’re talking deep, sometimes lasting injuries. Inhalation risks show up quickly, disturbing breathing and causing chest discomfort. Even just one accident leaves a long memory. I remember a colleague who opened a jar carelessly and ended up needing several visits to occupational health. Nobody needs that on their record or conscience.
Plenty of safety sheets put 2-Naphthoyl chloride squarely in the “corrosive” category. Direct skin contact damages tissue, and it doesn’t take long exposure. Testing shows this compound can also damage eyes and mucous membranes, even at low doses. In labs, shortness of breath or eye-watering after poor handling isn’t rare. It’s tough stuff. Once spilled, 2-Naphthoyl chloride helps no one. It lingers in the environment and poses a risk to aquatic life if disposed of casually. Mixing it with water sometimes releases harmful gases—a foul, choking smell I’ve never forgotten from my early training.
Lab safety is about much more than rubber gloves. People sweat, rush, or skip steps—mistakes follow. Having watched highly trained chemists get hurt skipping personal protective equipment or working without good fume extraction, I can say that nobody stays immune for long. Emergency eyewashes, showers, and spill kits are more than background—they save vision and skin.
Training makes or breaks outcomes with hazardous materials. Detailed explanations, routine practice, and refreshers help, but they need support with clear signage, working ventilation, and available cleanup equipment. Reporting near misses adds value, not blame. It invites problem-solving—“What failed? How do we fix it?” Peer checks or “buddy” systems catch a lot before it tumbles into trouble. Labs without strong safety cultures see more burns, inhalation injuries, and property damage. Even with discipline, surprises happen—automatic leak detectors and real-time air monitors reduce harm when they do. Disposal calls for specialized service, not a trip to the public drain, since the environmental stakes run high.
A healthier workplace comes from using the right barriers—face shields, gloves, and chemical-resistant coats. Fume hoods are essential for any operation that risks a splash, spray, or plume. From my experience, pausing to double-check seals, goggles, or labels turns standard handling into safe handling. If anyone feels pressure to cut corners, a conversation about real risks makes a difference. Ultimately, treating chemicals like 2-Naphthoyl chloride with the gravity they deserve protects health, work continuity, and the wider environment.
Working in the lab, folks don't forget the nasty sting of certain chemicals. 2-Naphthoyl chloride belongs to that set that likes to burn, irritate, and mess with your breathing if you aren't careful. This stuff reacts strongly with water and chucks out corrosive, fuming hydrochloric acid. If it touches your skin or eyes, pain and damage follow quickly. You don't need a repeat performance of chemical burns to take simple rules seriously.
No matter how confident you feel after hundreds of bench hours, no one’s skin handles splashes of 2-Naphthoyl chloride. Gaps in a glove or missing goggles turn minor slips into medical emergencies. Nitrile or butyl rubber gloves actually stand up to this compound. Your average latex gloves fold fast — those fingers are left raw. Full goggles shield your eyes from even small splashes, and a lab coat with buttoned sleeves keeps stray drops off your forearms and chest. Sometimes a face shield pays off, especially if larger pours or transfers are involved.
Even a minor whiff of 2-Naphthoyl chloride or its fumes can mean hours of coughing or worse, asthma-like problems that don't leave easily. Fume hoods take most of this risk off the table. It’s never foolish to check that airflow works before starting, and it makes life simpler if a spill occurs. Friends of mine cut corners on ventilation and landed with persistent coughs every cold season — not a coincidence.
Caustic liquids don’t give warnings. Double-check the container for cracks or sticking stoppers — broken glass or stuck lids spill faster than steady hands can fix. Only open or transfer 2-Naphthoyl chloride on surfaces cleared of clutter, with all flammables and organics well out of the way. Even a bit of moisture anywhere around can trigger a reaction. Keep a dry environment, a clean workbench, and dry utensils on hand. If weighing out powder, anti-static equipment avoids accidental flyaway dust.
I learned more from watching old samples clump and leak than any materials safety sheet. This chemical needs a cool, dry, and strictly ventilated spot, well away from acids, bases, water, and oxidizers. Tightly-sealed amber glass stops both light and air from breaking it down. If the cap doesn’t fit perfectly tight, the trouble grows. Most labs track who last handled each container, adding accountability as an extra barrier against accidents.
No one ever believes it will be them until they’re mopping something that won’t stop burning. If a spill happens, head for eye washes or showers immediately. For cleaning, solid absorbents (like sand or vermiculite) work best. Wash with water only at the very last step and only after neutralizing. Vacuum lines or open flames anywhere near this spill spell disaster. Triple-bag waste, label everything clear, and get specialized disposal from professionals — don’t send it down the drain.
Every safety session pays off the first time things go sideways. Experienced lab techs run practice drills and never rush job steps because someone else is waiting for the hood. If anything about a sample or step feels wrong, stop and review safety notes first. It's always better to spend extra time reading up than a lifetime regretting one rushed afternoon.
I’ve seen great work destroyed by lax lab habits, and nothing ruins a research streak faster than a trip to the ER. Treating 2-Naphthoyl chloride with the respect it commands keeps everyone in the lab healthy. Simple habits, good training, and a sharp eye for detail save skin, lungs, and eyesight day after day.
| Names | |
| Preferred IUPAC name | naphthalene-2-carbonyl chloride |
| Other names |
2-Naphthoyl chloride β-Naphthoyl chloride 2-Naphthalenecarbonyl chloride |
| Pronunciation | /tuːˈnæfθɔɪl ˈklɔːraɪd/ |
| Identifiers | |
| CAS Number | 93-61-8 |
| Beilstein Reference | 1208735 |
| ChEBI | CHEBI:51822 |
| ChEMBL | CHEMBL372059 |
| ChemSpider | 12372 |
| DrugBank | DB03670 |
| ECHA InfoCard | 03a4d0b3-ef8a-4c42-a7ce-b0e53ee0d871 |
| EC Number | 211-969-1 |
| Gmelin Reference | 82157 |
| KEGG | C08388 |
| MeSH | D009292 |
| PubChem CID | 9400 |
| RTECS number | QJ6475000 |
| UNII | J3D9QWA9K8 |
| UN number | 2812 |
| Properties | |
| Chemical formula | C11H7ClO |
| Molar mass | 180.61 g/mol |
| Appearance | White to yellow crystalline powder |
| Odor | pungent |
| Density | 1.267 g/mL at 25 °C |
| Solubility in water | Decomposes |
| log P | 2.9 |
| Vapor pressure | 0.02 mmHg (25°C) |
| Acidity (pKa) | 15.7 |
| Magnetic susceptibility (χ) | -62.0e-6 cm³/mol |
| Refractive index (nD) | 1.654 |
| Viscosity | 1.676 mPa·s (at 25 °C) |
| Dipole moment | 2.83 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 362.6 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -81.9 kJ/mol |
| Hazards | |
| GHS labelling | GHS02, GHS05, GHS07 |
| Pictograms | GHS05,GHS07 |
| Signal word | Danger |
| Hazard statements | H302, H314, H317, H411 |
| Precautionary statements | P261, P264, P271, P280, P301+P312, P302+P352, P304+P340, P305+P351+P338, P311, P321, P330, P332+P313, P337+P313, P362+P364, P403+P233, P405, P501 |
| NFPA 704 (fire diamond) | 2-1-0 |
| Flash point | 97 °C |
| Lethal dose or concentration | LD₅₀ (oral, rat): 740 mg/kg |
| LD50 (median dose) | LD50 (median dose): Oral-rat LD50: 640 mg/kg |
| NIOSH | NA8317 |
| PEL (Permissible) | Not established |
| REL (Recommended) | ambient |
| Related compounds | |
| Related compounds |
2-Naphthoic acid 1-Naphthoyl chloride Naphthalene 1-Naphthylamine 2-Naphthylamine |
