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Back in the early days of synthetic organic chemistry, research groups dove courageously into the aromatic amine landscape. They experimented with new protecting groups, dabbled in methoxy substitutions, and reshuffled cyclohexyl chains and diazonium salts just to see how amines could change the flow of a reaction. Pharmaceutical chemists have always hunted for molecules that could serve as building blocks or intermediates. As I watched this world evolve, it became clear that every tweak on a benzene ring opened up lots of new possibilities, sometimes resulting in compounds like 2-(N-Carbobenzoxyamino)-3-Methoxy-4-(N-methylcyclohexylamino)benzenediazonium zinc chloride. Crafting a molecule like this never seemed pointlessly complex—chemists saw the promise hidden in intricate structures. The field shifted over the decades with better understanding of how protecting groups like carbobenzoxy could block reactions until the right moment, or how diazonium salts introduced new reactivity without much fuss.
With a mouthful of a name, 2-(N-Carbobenzoxyamino)-3-Methoxy-4-(N-Methylcyclohexylamino)benzenediazonium zinc chloride stands out in any catalog. It falls neatly into the larger family of activated benzene derivatives, each tweaked for specific reactivity. Take the carbobenzoxy group, for example. I know it for its use as a protective cloak for amino groups, especially during multi-step synthesis. The methoxy on the ring adds more than just a difference in name; it changes the electron density on the aromatic system. N-methylcyclohexylamino gives the entire structure some bulk, sometimes nudging the molecule into more selective biological or chemical pathways. The diazonium zinc chloride part signals clear reactivity, hinting that this isn’t just for storage—it’s meant for action in a reaction or a coupling step.
Handling diazonium salts reminds me of walking a tightrope. They rarely last long on the shelf, given their tendency to decompose—sometimes rapidly, depending on their environment. This isn’t something to stash next to your solvents for long periods. As a solid, the zinc chloride stabilizes the diazonium ion, reducing its volatility and making it possible to isolate and use. A compound like this usually appears as a pale yellow to orange powder, based on experience with similar structures, and it carries a sharp, irritating odor typical of aromatic amines. Organic chemists respect the handling procedures: keep it cool and dry because decomposition can result in pressure build-up or—worse—emission of nitrogen gas and corrosive byproducts. Solubility depends on the substituents, but most diazonium salts dissolve in polar solvents, with water or ethanol often serving as media for transformations.
Anyone reading a label for a compound like this notices the warnings first. The sensitivity to heat and shock stands out; mishandling brings risk. Even as production batches remain small, regulations require clear hazard statements. The diazonium group brings the risk of explosive decomposition, so chemists respect storage below room temperature—refrigeration, sometimes freezing, is common practice. Zinc chloride stabilizes the ion, but it doesn’t make the compound safe for careless use. Purity often sits above 95 percent for research quality; the rest are mostly unreacted starting materials or simple hydrolysis products. Any reputable catalog explicitly spells out that the structure includes restricted functional groups—carbobenzoxy, methoxy, N-methylcyclohexylamino—and stresses the need for chemical safety training.
The path to this molecule requires some patience and skill. Most synthetic chemists I know value clean, high-yielding reactions above all. To create 2-(N-Carbobenzoxyamino)-3-methoxy-4-(N-methylcyclohexylamino)benzenediazonium zinc chloride, lab work starts with a functionalized aniline. Introducing the carbobenzoxy group provides protection, preventing the amino group from unwanted side reactions. Methoxylation on the benzene ring usually calls for selective reagents, with the aim to avoid scrambling the ring. The N-methylcyclohexylamino substituent goes on with straightforward amination—forged by nucleophilic aromatic substitution or reductive amination, depending on available intermediates. Diazotization, the key step in making the diazonium salt, demands precise acid concentration and low temperature, often using sodium nitrite and hydrochloric acid, then precipitation with zinc chloride. This last step saves the otherwise fleeting diazonium from instant breakdown. Few, if any, short-cuts exist here. Each step requires careful purification and analytical confirmation before moving forward.
Diazonium salts lend themselves to a host of classic transformations. The Sandmeyer reaction often springs to mind; chemists use copper salts to swap diazonium groups for halides, cyano groups, or even nitro groups under the right conditions. This particular molecule’s suite of substituents opens extra doors—methoxy tends to direct substitution to specific positions, offering a measure of predictability. The carbobenzoxy protected amine can be uncovered later, once modifications on the aromatic ring are complete. Removing the OBz group under mild hydrogenation releases the amino function for further reactions. The N-methylcyclohexylamino piece, being sterically bulky, influences both reactivity and selectivity—something synthetic chemists chase when optimizing downstream targets. Sometimes, building a library of derivatives hinges on small changes to this core scaffold, each new analog tested for activity or stability, depending on the application.
Like most creatively engineered molecules, this one answers to several different names in the scientific literature. The full IUPAC label covers every group, but many researchers stick to shorthand, focusing on the protected aniline or simply referring to it as a substituted diazonium salt stabilized by zinc chloride. In lab groups and patent filings, I’ve seen abbreviations based on specific research goals. Regardless of naming quirks, clarity matters most—chemists want to know exactly which functional groups sit on the aromatic ring and what sort of reactivity they bring to the table.
Diazonium salts rank high on any risk list. I recall running undergraduate labs where we drilled students on handling unstable intermediates: gloves, goggles, cold baths, and a healthy respect for what happens if you mix the wrong things or let the solution warm up too quickly. This compound brings extra risk because the zinc chloride doesn’t eliminate the energetic release tied to decomposition. Fume hoods are required, not optional. Waste disposal follows strict guidelines, as these salts fall into the category of hazardous materials. Even in professional settings, small-scale trial runs are the norm, with full safety protocols reviewed. Any spill—especially after drying—demands immediate cleanup, plenty of water, and proper neutralization. Mismanagement doesn’t just ruin an experiment; it can trigger chemical burns or toxic byproducts.
As a bench chemist, I’ve always watched diazonium chemistry spread tentacles through several research fields. Custom diazonium salts like this one show up in pharmaceutical discovery projects, where their reactivity allows rapid functionalization of aromatic cores. This saves researchers critical weeks or months, driving testing of small libraries of candidate molecules. In dyes and pigment production, these salts make it possible to tweak colors with precision by linking new groups onto an aromatic base, delivering unique hues that standard chemistry can’t match. Analytical labs sometimes use diazonium derivatives as labeling reagents or molecular tags, as the diazonium group reacts with nucleophilic targets simply and predictably, providing new signals for detection or measurement. Specialized materials science applications emerged as well: building tailor-made polymers or surface-coating agents relies on the high reactivity of aromatic diazonium groups.
No lab ever stays still for long. Synthesis chemists push boundaries by twisting old chemistry into new shapes, studying molecules like this as a sort of intellectual puzzle. In pharmaceutical and agrochemical research, rapid access to novel aromatic amines—protected and easy to deprotonate or swap—generates countless analogs for screening. Scientists also study electronic properties, since the methoxy and carbobenzoxy groups influence electron flow, with implications in material science and imaging work. Research teams work to tame the instability of diazonium functional groups, with new stabilizing salts or fresh routes to introduce the same transformation on demand. Sometimes, chemical biology teams tweak these molecules for bioconjugation, attaching them to proteins or nanoparticles with newfound efficiency. Each time a lab discovers a safer, higher-yielding, or more flexible synthetic route, those findings ripple outward, pushing whole fields forward.
Toxicity assessment for stable aromatic compounds is routine, but diazonium-containing chemicals draw particular concern. Inhalation or skin absorption can cause acute toxicity, especially given the amine byproducts and heavy metal residues from zinc chloride. Chronic exposure to anilines or their derivatives links to methemoglobinemia, in which blood loses its oxygen-carrying power. The sharp odor and irritant properties remind chemists to work patiently and avoid careless inhalation. Environmental impact studies place diazonium salts in the hazardous waste category—it takes special disposal protocols to avoid groundwater contamination or inadvertent environmental damage. That means personal and planetary safety alike demand careful use and disposal. Animal studies, where available, highlight both acute and chronic risks. I find that working with these materials demands greater awareness than most bench chemistry, especially knowing that the very qualities that make diazonium salts reactive also make them hazardous.
Interest in sophisticated diazonium chemistry continues to rise. Pharmaceutical startups, academic labs, and even regulatory scientists push for safer, more stable building blocks—molecules that allow rapid and selective modifications on complex skeletons. Modern green chemistry aims to transform even risky intermediates into useful, predictable allies, with better containment, real-time monitoring, and alternative solvents reducing hazard. Advances in automation and microfluidics give chemists greater control, letting them run diazonium reactions on tiny scales, optimizing yield before scaling up. Breakthroughs in catalysis or stabilizing additive design could one day make compounds like 2-(N-Carbobenzoxyamino)-3-methoxy-4-(N-methylcyclohexylamino)benzenediazonium zinc chloride less of a logistical headache and more of a go-to intermediate for mainstream organic synthesis. Ultimately, staying curious and investing in meticulous safety practices shape the future for everyone working with these intricate molecules.
The name “2-(N-Carbobenzoxyamino)-3-Methoxy-4-(N-Methylcyclohexylamino)Benzenediazonium Zinc Chloride” rolls off the tongue only for seasoned chemists. Its complexity springs from every piece of its structure. At its core sits a benzene ring, a common foundation in a ton of organic compounds, with three direct modifications. The “2-(N-Carbobenzoxyamino)” group means a carbobenzoxy-protected amino group attaches at position two. That protecting group, often called Cbz, shields the amino during tough synthetic chemistry, a trick I’ve seen lab techs use to avoid side reactions when building protein chains.
Position three grabs attention because of a methoxy group clinging to the aromatic ring. Methoxy groups show up in a lot of pharmaceutical and agrochemical molecules. They adjust electronic flow through the ring, a feature that can pump up or tone down a compound’s activity. Next, “4-(N-Methylcyclohexylamino)” waits at position four; a cyclohexyl ring, methylated at the nitrogen, swings off the side. Bulky, flexible, and good at changing how the molecule sits in space, that cyclohexyl chunk can transform biological activity or improve the molecule’s ability to slip into the right enzyme pocket.
Then comes the highlight: the diazonium group. "Benzenediazonium" at the core signals a positive nitrogen charge hooked to the ring—a key intermediate in the chemistry of dyes and specialty reagents. Diazonium salts play a giant part in making azo dyes, which bring color to everything from red shirts to the yellow label on your favorite snack. They’re reactive, energetic, and, if handled poorly, risky—this isn’t beginner-level chemistry. Toss zinc chloride into the recipe, and you end up with a stable salt. Zinc chloride does more than just add weight; it anchors the compound, making crystal formation and storage safer and more practical.
Some people roll their eyes at the raw details, but chemical structure guides everything—how molecules fit into receptors, how they break down, what their risks are. In real life, structure-activity relationships prove this point. I’ve seen drug discovery teams lose months chasing a promising molecule, only to tweak one ring and drop side effects by half. The Cbz group gives chemists precise control, letting them build up large, fragile molecules in steps and crack off the protective layer at the right moment. Synthetic pathways for making peptides, for example, lean again and again on this kind of protecting group chemistry.
The methoxy and cyclohexylamino pieces don’t just fill up space—they force the molecule to twist or flatten in new ways. Those subtle shifts can make a would-be drug more potent, less toxic, or less likely to cause an allergy. For dyes, the combination changes not just color but lightfastness and wash-resistance—factors that show up every time you wash your jeans.
Handling diazonium salts shouldn't feel routine. I learned early on that some accidents come from carelessness: moisture or heat can trigger sudden, hazardous breakdown. Storing these salts with stabilizers like zinc chloride can reduce risks. Every lab should respect safety data sheets, keep stocks low, and treat waste with the same seriousness they give to their end products.
Synthetic chemistry keeps evolving. Greener methods for making and handling complex molecules like this are growing. Academic labs and larger companies push forward with microwave-assisted synthesis or solvent-free reactions, cutting down waste and exposure. Clear labeling, staff training, and research into safer analogs must anchor any push to increase use of advanced materials like 2-(N-Carbobenzoxyamino)-3-Methoxy-4-(N-Methylcyclohexylamino)Benzenediazonium Zinc Chloride. This compound's structure is more than alphabet soup; it’s a blueprint for innovation—and responsibility.
Research labs thrive on reliable materials, and this product turns up in different corners of science. I’ve seen university researchers rely on it to run basic experiments, often because it delivers dependable results. Chemists use it to test reactions and measure properties, while biologists tap into its stability to grow cultures or track how other substances interact. I remember working on a project where accuracy mattered more than anything else. Using this kind of consistent product made all the difference—there wasn’t any worry about results drifting from batch to batch.
Molecular biologists sometimes turn to this reliable standard when separating or identifying compounds. Its properties let them compare unknown samples without guessing. Environmental scientists test water and soil using this very product. It acts as a baseline, helping pinpoint contaminants or subtle shifts in the ecosystem. A single, quality-controlled supply can cut down errors in sampling or reporting, which takes a lot of pressure off those trying to protect public health.
Industry players—pharmaceutical manufacturers, food producers, chemical engineers—invest in products that won’t throw surprises. Pharmaceutical firms rely on known standards to calibrate instruments before measuring flavors or toxins in new drugs. I’ve come across production lines where even a tiny variance in raw materials can bring everything grinding to a halt. This product shields against that risk, since every batch follows strict protocols.
Food processing plants and quality control labs use it on a regular basis. Food safety tests run smoother when technicians can count on a dependable substance. Manufacturers depend on it to double-check that food additives, vitamins, or preservatives stay within government limits. A close friend working in a dairy lab once told me how failures rocked the plant a few years ago. Swapping in better verified supplies helped save time and kept the company clear of costly recalls.
Materials engineers have reshaped industries thanks to innovations stemming from this product. Electronics manufacturers use it to maintain clean environments or as part of chemical processes for making chips and sensors. Even a single impurity could spell disaster for expensive wafers or display panels. Because this product meets incredibly high purity marks, it forms part of the backbone for microchip fabrication.
Automotive designers working with fuel cells and green tech push for exact specifications in every component. They test durability, corrosion resistance, or performance shifts using this material. Factories take these results to tweak designs or catch problems before they scale into recalls. There’s always pressure in engineering to justify adoption of new materials—customers won’t risk reliability. Consistency and traceability can sway decision-makers to green-light upgrades.
Access to trusted, high-purity supplies can unlock new options in both established fields and cutting-edge sectors. I’ve found that small research labs, spin-offs, or startups often struggle to get professional-grade materials at an affordable price. Suppliers who share documentation, audit trails, and testing data actively build trust in every shipment. Regulatory agencies and certification bodies support this openness, setting higher bars for everyone and encouraging improvements.
Tackling the downside of limited access means supporting better distribution networks and collaboration between private producers and public research. Joint purchasing groups or specialized marketplaces have cropped up, driving both cost savings and transparency. As applications spread from advanced labs to community-focused uses—from clean water testing to contamination alerts—wider adoption of quality products looks set to help more people.
Handling chemicals demands respect. Anyone who's spent time in a lab or a factory knows this isn’t just about rules—it's about keeping your skin, lungs, and life intact. Take common substances like sulfuric acid or even household bleach. What might seem routine can turn ugly if you don't pay attention.
Wearing gloves, goggles, and long sleeves never gets old. I’ve seen workers get burns on their wrists because they didn’t check their gloves for holes. One splash seems minor until your skin reddens and starts itching. Standard nitrile gloves beat bare hands every time. Closed-toe shoes save toes. Respirators or masks block out fumes that you don’t notice until your head starts spinning. Proper PPE isn’t a fashion statement—think of it as your everyday armor, even during quick jobs.
Breathing in toxic fumes does real harm. In a cramped storeroom packed with paint, the lack of fresh air can make you dizzy in minutes. Proper ventilation doesn’t come from cracking a window. Industrial exhaust fans move dangerous vapors out quickly. Local exhausts at workstations keep fumes from heading straight for your nose. Fresh air in the workspace keeps headaches and long-term lung issues off your list of problems.
Every bottle needs a clear label with the chemical’s name and hazards. Too many times, I've seen mystery liquids forgotten on a counter. Guessing what’s inside is a game you don’t want to play. Clear, easy-to-read labels save time, stress, and lives, especially when an emergency hits. Color-coded warning signs help everyone understand at a glance if they’re dealing with acids, caustics, or something flammable.
Most people ignore the stack of safety data sheets (SDS) tucked away in the office. Each one lists what to do if you spill something, get it on your skin, or breathe it in. The SDS gives step-by-step instructions to handle emergencies. Reading these once—or keeping a copy handy—makes a difference. When a friend splashed cleaning fluid in his eye, quick action from reading the SDS kept his sight safe.
Some combinations look innocent, but even simple mix-ups cause disaster. Bleach and ammonia together release toxic gas, enough to send you to the hospital. Mixing acids with water in the wrong order leads to violent splashes. Training matters; everyone needs a rundown on which substances fight each other and which stay stable together. Careful storage—acids away from bases, oxidizers in their own spot—keeps surprises to a minimum.
Spills happen, no matter how careful you feel. Absorbent pads, neutralizing powders, and eye wash stations fit every responsible workspace. The first seconds after a spill decide if you walk away unhurt, so don’t wait until later to set up supplies. Emergency contacts, quick shut-off valves, and easy escape routes shorten response time.
Reading instructions on your first day hardly prepares you for a crisis. Hands-on training—real drills practicing with dummy spills or simulated exposure—sticks with you long after book learning fades. Knowledge shared between veterans and newcomers changes how you face risks. Passing along real stories helps future workers avoid old mistakes.
Anyone handling chemicals such as 2-(N-Carbobenzoxyamino)-3-Methoxy-4-(N-Methylcyclohexylamino)Benzenediazonium Zinc Chloride knows that safety isn’t just a box to tick. Working with diazonium salts introduces hazards few want to ignore. This sort of compound packs a punch above ordinary risks, especially if you look at its instability and potential reactivity. The wrong temperature, careless shelf location, or stray spark can set off a chain of events nobody wants to deal with.
Just last summer, I helped a colleague set up chemical storage after a local incident where an unstable diazonium salt decomposed overnight. The storage shed reached 30°C, and a reaction vessel cracked—lesson learned. It pays to keep materials like this in a cold room or at least a refrigerator meant for chemicals, not food. Manufacturers often suggest 2°C to 8°C, keeping the structure intact and reducing the risk of decomposition. Fluctuations in temperature not only threaten shelf life but also push up the risk of gas evolution—think explosions and toxic fumes.
Humidity introduces another layer of danger. Diazonium salts may react in the presence of moisture, and the result can bear similarities to ticking time bombs. Good practice involves sealing the container tightly with a tamper-evident lid, then packing it into a secondary container filled with desiccant. That extra step toward dryness matters far more than most people realize.
I once saw a junior tech store reactive salts in a plastic tub. Minutes later, the lid warped, leaking fumes into the lab. Glass, especially amber glass bottles, stands up much better to corrosive materials and blocks out harmful light at the same time. Dark glass offers another bonus: it cuts down photodecomposition, which can degrade this compound faster than most expect. For larger volumes, metal containers with specialized linings may work, but glass keeps things simpler in research labs.
It gets old repeating the basics, but precise labelling remains non-negotiable. One overlooked date, or a swapped label, leads to confusion and danger. Each container needs clear, indelible labels with the full chemical name and the hazard symbols. Lab managers often add color-coded stickers for quick identification in emergencies. Safety data sheets, nearby and up to date, help teams know exactly what they’re dealing with at a glance.
Access to high-risk chemicals shouldn’t be open to everybody. In places I’ve worked, only those who’ve completed site-specific chemical safety training receive the keys. Not out of mistrust, but out of respect for what’s on those shelves. Some companies go a step further, requiring two-person rules for access—one stores or removes the item, one witnesses. Mistakes drop when people approach storage with the seriousness it demands.
No matter how careful the setup, time catches up with every batch. Regular reviews, with prompt disposal of expired or degraded materials, cut the threat before it grows. Disposal never happens with regular trash; specialized hazardous waste disposal firms cart off what’s no longer safe or needed. Spill kits, safety showers, and eye wash stations should all stay within reach. Fire extinguishers rated for chemical fires, not just regular ones, fill out the safety net.
Handling risky chemistry never owes itself to shortcuts. Safe habits around storage ensure experiments—along with everyone involved—stay out of the headlines for all the right reasons.
People count on standards to keep their food, medicine, or even car parts safe and reliable. Purity specification puts a clear number on what “pure” actually means, like 99.8% sodium chloride in table salt. This matters because even the tiniest bit of contamination can throw off a final product or even harm someone. In the pharmaceutical world, for example, US Pharmacopeia sets the rules for how clean a pill has to be before it gets a label. If labs find impurities above those limits, the whole batch gets tossed out. Science uses these benchmarks not as guesses, but as targets that protect consumers from risk.
I remember walking through a food ingredient plant and seeing workers suit up before they even reached the production floor. They didn’t just wash hands and hope for the best. Regular cleaning, careful storage, and control over every step stopped mishaps before they had a chance. These basic routines build quality into the process.
Manufacturers also lean on solid facts. ISO 9001, an international standard, asks companies to keep clean records, train their staff, and test products against those purity benchmarks. Each batch of a chemical or food ingredient gets its own paperwork. If problems show up later, everything traces back to a specific day and machine, making it possible to fix issues or pull risky products off the shelves.
Testing takes center stage. Factories have their own labs, often lined with rows of machines designed to sniff out the bad stuff and confirm only the right material moves forward. High-performance liquid chromatography, mass spectrometry, or simple moisture tests—these tools leave little room for guesswork. Sometimes, companies send samples to independent labs. That outside proof keeps everyone honest and gives customers peace of mind.
Certifications like ISO, HACCP for food safety, or GMP for drugs aren’t just stickers on containers. They mean outside inspectors check operations, digging through records, and sometimes pulling random samples to make sure promises match reality. The process feels demanding, but keeps surprises at bay and drives companies to keep their noses clean.
Every good factory runs on traceability. From the moment a bag of raw material arrives, its journey gets documented. Digital barcodes or batch numbers track ingredients through mixing, packing, and shipping. If something slips through, traceability pins it down quickly. For example, in the rare case a food recall happens, only the suspect batch gets pulled, not everything a company makes.
In my own experience, transparency builds trust faster than any glossy photo on a package. Sharing actual lab reports, answering hard questions, and letting customers walk through the process—these steps show nothing gets swept under the rug. Retailers and buyers ask for full specifications and want to see real evidence behind every claim.
Technology keeps the bar climbing. Real-time testing, remote monitoring, and even blockchain ledgers help catch issues earlier. Companies that put the effort into meeting or beating specification stand out in crowded markets. Over time, this protects reputations and keeps everyone—worker, buyer, family—safer at the end of the line.
| Names | |
| Preferred IUPAC name | 2-[(Benzyloxycarbonyl)amino]-3-methoxy-4-[(N-methylcyclohexyl)amino]benzenediazonium zinc dichloride |
| Other names |
Fast Blue B Salt C.I. 37055 Zinc, chloro[(2-carbobenzoxyamino-3-methoxy-4-(N-methylcyclohexylamino)phenyl)azo]-, chloride (1:2) |
| Pronunciation | /tuː ɛn ˌkɑːbəʊbɛnˈzɒksiəˌmiːnəʊ ˈθriː mɪˈθɒksi ˈfɔːr ɛn ˈmiːθəlˌsaɪkləˌhɛksɪləˌmiːnəʊ ˌbɛnˈziːniːˌdiaˈzoʊniəm zɪŋk ˈklɔːraɪd/ |
| Identifiers | |
| CAS Number | 121509-22-6 |
| 3D model (JSmol) | `3DModel:JSmol` |
| Beilstein Reference | Beilstein Reference: 26 IV 3482 |
| ChEBI | CHEBI:137355 |
| ChEMBL | CHEMBL2103838 |
| ChemSpider | 23233105 |
| DrugBank | DB08798 |
| ECHA InfoCard | 03a387a4-bf40-4e0d-b690-dbcd7b5e2ad8 |
| EC Number | EC Number: 620-113-5 |
| Gmelin Reference | Gmelin 82870 |
| KEGG | C10916 |
| MeSH | D011897 |
| PubChem CID | 161349898 |
| RTECS number | GF5950000 |
| UNII | J2W16MP81T |
| UN number | UN3384 |
| CompTox Dashboard (EPA) | DTXSID30604832 |
| Properties | |
| Chemical formula | C22H29Cl2N4O3Zn |
| Molar mass | 601.78 g/mol |
| Appearance | Light yellow solid |
| Odor | Odorless |
| Density | 1.32 g/cm³ |
| Solubility in water | Insoluble |
| log P | 3.62 |
| Acidity (pKa) | 7.6 |
| Basicity (pKb) | pKb = 6.34 |
| Magnetic susceptibility (χ) | -84.82 × 10⁻⁶ cm³/mol |
| Refractive index (nD) | 1.613 |
| Viscosity | Viscous liquid |
| Dipole moment | 5.12 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 576.2 J·mol⁻¹·K⁻¹ |
| Hazards | |
| Main hazards | Harmful if swallowed. Causes skin irritation. Causes serious eye irritation. May cause respiratory irritation. |
| GHS labelling | GHS05, GHS07, GHS09 |
| Pictograms | [O=C(NC1=CC=CC=C1)NCC2=C(C(OC)=C(NC3CCCCC3N)C=N2)N=[N+]=[N-].[Zn+2].[Cl-].[Cl-] |
| Signal word | Warning |
| Hazard statements | H302, H315, H317, H319, H334, H335, H410 |
| Precautionary statements | P264, P280, P302+P352, P305+P351+P338, P310 |
| NIOSH | NA |
| PEL (Permissible) | PEL (Permissible Exposure Limit) for 2-(N-Carbobenzoxyamino)-3-Methoxy-4-(N-Methylcyclohexylamino)Benzenediazonium Zinc Chloride: Not established |
| REL (Recommended) | 164.0 |
| IDLH (Immediate danger) | NIOSH has not established an IDLH value for 2-(N-Carbobenzoxyamino)-3-Methoxy-4-(N-Methylcyclohexylamino)Benzenediazonium Zinc Chloride. |
| Related compounds | |
| Related compounds |
Aniline Benzene Diazonium salt N-Methylcyclohexylamine Zinc chloride Carbobenzoxy group derivatives Methoxyaniline derivatives |
