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Chemistry often builds on legacies that young researchers walk right past in a rush to find new materials. Few recall that the diazonium salts, including 4-dimethylaminobenzenediazonium trichlorozincate, have roots reaching back to 1858 with Peter Griess’s discovery of diazonium chemistry. Before today’s focus on safety, researchers faced unpredictable explosions just from drying out these salts. Over time, pairing diazonium ions with metal complex anions such as trichlorozincate allowed for more manageable handling. Early dyes and the color photography industry seized this twist—the salts offered bright, long-lasting colors, an effect that couldn't come from organic compounds alone. These historic roots color the current use and study of 4-dimethylaminobenzenediazonium trichlorozincate. It’s never just a reagent; it’s an artifact sitting right between the past and present of organic synthesis.
When I see a jar of this compound in a research lab, what jumps out is the contrast between its delicate utility and the risks it can pose. This salt takes the slightly fishy smell and yellowish tint associated with diazonium compounds, but stabilization from the trichlorozincate brings a crystalline, pale yellow powder, less likely to decompose or detonate out of the blue. Structurally, 4-dimethylaminobenzenediazonium trichlorozincate pairs the aromatic diazonium cation, aromatic and highly reactive, with the zinc trichloride anion, forming an ionic lattice that holds together far more stably than free diazonium salts. In a world populated by fleeting intermediates, this complex can actually see the inside of a shipping box on its way to a teaching lab, although storage guidelines still warn against temperature swings, moisture, or sunlight.
Compared with many organic intermediates, this compound stands out for both its solid form and its stability if stored in the dark at low temperature. The solid's color and modest solubility in water give chemists control over transfer and measurement. Beyond physical properties, the chemical behavior really stirs a synthetic chemist’s imagination. As with its relatives, the diazonium group offers a rich reactivity profile—capable of forming azo dyes, engaging in Sandmeyer-type substitutions, and even acting as a bridge to create biaryl linkages. The dimethylamino group on the benzene ring pushes more electron density into the system, making this compound more reactive in electrophilic substitution reactions than less-substituted diazonium salts. All this explains its starring role in library syntheses and combinatorial chemistry, not just academic curiosity.
Labels for 4-dimethylaminobenzenediazonium trichlorozincate need to do more than check boxes for hazard pictograms. Serious research organizations lay out data-pointed hazard communication, the need for chemical fume hoods, limits on handling quantity, and explicit disposal protocols. Crystalized diazonium complexes demand respect; accidents from mishandling come not just from explosions but from chronic exposure to decomposition products known for their toxicity. Regulatory guidelines direct the shipment and storage, echoing what research chemists share one-on-one: keep quantities small, avoid heating, and keep an inert atmosphere or desiccator for long-term shelf life. Unambiguous risk phrases serve as constant reminders, cutting down on avoidable mistakes in busy labs.
Producing 4-dimethylaminobenzenediazonium trichlorozincate is a real-world lesson in balancing high yields with safety. Diazotization runs through cold aqueous solutions—4-dimethylaminobenzenamine (the precursor) meets sodium nitrite in acid, forming the diazonium cation in situ. Gradually, this solution combines with zinc chloride, sometimes present as a concentrated aqueous solution, which helps shift precipitation toward the desired salt. Careful temperature control, usually below 5°C, prevents disastrous side reactions or runaway decomposition. Filtration under cold conditions, washing with chilled solvents, and fast drying with desiccants sidestep the hazards of handling and storing a dry powder that might otherwise go unstable.
On a bench covered with glassware and TLC plates, the reactivity of this compound takes center stage. A diazonium group sitting next to a dimethylamino substituent gives more than pretty dyes—it leaves the door open for nucleophilic substitutions, azo coupling, and useful arylations. The convenience of the zinc complex comes into play here, too; it can participate in transition metal-catalyzed reactions, one of the many keys to constructing complex organic molecules. The salt can serve as a drop-in partner for C–N or C–C coupling reactions, expanding the limits of what’s practical in both pharmaceutical research and materials science. That’s the promise—and headache—of these compounds: nearly limitless reaction routes, tangled with the ever-present risks of unstable diazonium intermediates cracking apart in a warm flask.
Not everything in the chemical world goes by a single name. 4-dimethylaminobenzenediazonium trichlorozincate crops up as N,N-dimethyl-4-benzenediazonium trichlorozincate in European literature, or simply DMABDTZ in shorthand on synthetic schemes. Researchers new to the game need to double-check that catalog entry to avoid the classic mistake of mixing up the chloride salt, nitrate, or the trichlorozincate version. Such nuances have sent more than one student rifling through sample drawers after realizing that the “same” salt dissolves too quickly or doesn’t react at all, all because of a missing zinc.
No experienced chemist shrugs off the risks carried by diazonium complexes, especially trichlorozincate salts. National chemical safety boards register multiple accidents tied to careless heating, hasty weighing, or failing to label a flask. Having worked in labs where these compounds made weekly appearances, I’ve seen everything from minor skin burns to near-misses with glassware explosions from dry powders. Today, many research-intensive departments build training programs around hands-on hazard assessments for diazonium handling, targeting both graduate students and lab technicians. PPE means more than goggles—face shields and full-length gloves answer the problems presented by splashing liquid or airborne particulates. The culture grows stronger when everyone from postdocs to undergraduates calls out unsafe practices without hesitation.
The journey from academic curiosity to widespread utility changed 4-dimethylaminobenzenediazonium trichlorozincate from a niche chemical to an essential tool. Synthetic chemists looking to build azo dyes lean heavily on this salt, using its reliable reactivity profile for vibrant, persistent colors that stick in textiles and inks. Polymer surface modification teams deploy it for high-contrast photoresists in microfabrication. Pharmaceutical explorers see it as a trackable intermediate, a way to swap in aryl groups using Sandmeyer chemistry or design small molecules for screening libraries. With the expansion of “click” chemistry and new coupling strategies, the compound moves beyond traditional reactions, appearing in cross-coupling and radical-initiated synthesis. These applications grow each year as automation and combinatorial synthesis fuel the search for new materials and drug candidates.
Modern research never accepts “close enough.” Here, structural and reactivity studies dig into the complex’s crystallography, kinetics, and decomposition pathways. Research groups dissect the compound’s behavior under photolysis, pushing into fields like photo-switchable materials and light-triggered drug delivery. Chemoinformatics approaches piece together libraries of new derivatives by tweaking the dimethylamino position or swapping other substituents onto the benzene ring. Researchers run studies using computational tools to predict and avoid explosive decomposition, leveraging lessons learned from past failures. Careful R&D translates into incremental safety improvements, fewer accidents, and clearer protocols, a much-needed trend in the context of highly energetic intermediates.
Advances in synthetic chemistry often force tough conversations about worker safety, chronic exposures, and waste disposal. Toxicologists have documented the risk profile: diazonium complexes are tied to mutagenicity and possible carcinogenicity, especially after degradation. Acute effects show up as skin sensitization, respiratory difficulty, and organ damage in the unlucky and unprotected. Generating and analyzing breakdown products means more time spent with chromatographic and spectroscopic tools—no shortcuts here. Disposal must follow guidelines to neutralize active diazonium species, with verified protocols for rendering waste harmless. Datasets grow year by year, feeding into regulatory measures set by workplace safety organizations, yet plenty of smaller labs worldwide miss these steps, especially where chemical education falls short.
Looking forward, the story of 4-dimethylaminobenzenediazonium trichlorozincate continues with advances in green chemistry and safer synthetic strategies. Lab-scale automation, new containment systems, and predictive hazard modeling draw on both new technology and old lessons, aiming to harness the compound’s reactivity without sacrificing safety. Forward-thinking researchers explore alternative chemistries that achieve the same synthetic flexibility while shedding persistent toxicity and explosive risk. Smart surface coatings, low-energy photo-switches, and biocompatible dye systems barely scratch the surface of the compound’s research promise. Those willing to invest the time and care stand to push it into unexpected fields—from next-gen optoelectronics to bio-tagging—instead of consigning it to specialty synthesis alone.
Most people won’t run into 4-Dimethylaminobenzenediazonium Trichlorozincate at the drugstore or hardware shop. Its name doesn’t exactly roll off the tongue, either. But take a close look at what’s behind specialized printing or the chemistry labs at universities, and it pops up. Its use shapes discoveries and product development, even if it rarely gets mentioned outside textbooks and scientific journals.
My years tucked away in campus laboratories introduced me to the notorious world of diazonium salts. This one—4-Dimethylaminobenzenediazonium Trichlorozincate—jumped out in advanced organic chemistry. Its unique role traces back to its structure, ideal for sparking reactions known as azo coupling. This reaction creates dyes that paint vivid colors onto fabrics, inks, and plastics. It’s hardly a household step, but in the synthesis of specialty dyes, its specificity brings reliability and intensity of color that generic routes struggle to match.
Dye-making isn’t the only place this compound plays a hand. Look at photolithography—a cornerstone in printed circuit board design. Engineers reach for diazonium salts like this one to generate photoresists. These allow precise etching on metal surfaces, carving out microcircuits in electronics by hardening under UV light. This work seems distant from our daily routines, but turn on a smartphone or power up a laptop, and you depend on the fine resolution this chemistry provides.
With something this reactive, there’s no room for shortcuts. Some may have heard about diazonium compounds for the wrong reasons—accidental explosions, skin irritations, and environmental headaches if disposal plans go awry. My own lab mentors always stressed gloves, fume hoods, and airtight storage. Unstable compounds in the wrong hands mean trouble. Regulatory agencies like OSHA and EPA publish detailed rules for handling and disposing of such chemicals, but real safety comes from everyday vigilance and respect for the pitfalls.
One point that still nags at chemists is sustainability. Waste from traditional dye production, including leftover salts and metal ions, can seep into water streams if not managed well. Calls for greener alternatives keep getting louder, driven by what we now know about environmental toxicity. Research is pointing towards recyclable reagents and biodegradable components, but shifting away from proven compounds like 4-Dimethylaminobenzenediazonium Trichlorozincate will take both patience and investment.
Building safer labs starts with robust training and early adoption of less hazardous materials where possible. Universities and tech companies can run pilot projects that swap out troublesome reagents and closely track pollution footprints. Regulators might strengthen reporting requirements, so traceability comes standard. Sustainable chemistry doesn’t mean abandoning the tools that taught generations of scientists, but adapting them, so workplaces and the environment shoulder less risk.
Although obscure to outsiders, 4-Dimethylaminobenzenediazonium Trichlorozincate stands as proof that small-scale chemistry drives big changes in technology and manufacturing. Addressing its health and ecological risks isn’t about pointing fingers—it’s about making sure the next breakthrough comes without a hidden cost.
The name 4-Dimethylaminobenzenediazonium trichlorozincate rarely pops up outside specialty labs, but anyone familiar with azobenzenes or related diazonium salts knows these compounds tend to be unpredictable. Explosions, fires, and nasty decompositions aren’t just distant possibilities – they’ve left lasting impressions in both academic and industrial settings. Old hands in the lab have seen what happens when a salt like this sits out on a warm day or near sunlight. Shelf stability depends on respecting both its chemistry and its quirks.
In my experience, dry air and cool temperatures are non-negotiable with these salts. Colleagues who cut corners with unsealed lids or by storing them in busy, warm environments found their stocks degraded—or even went off with a bang. Strong desiccants and dedicated drying cabinets prevent clumping, hydrolysis, and the quick shift from safe to hazardous. I avoid placing anything this unstable near fume hood edges or on open shelves where changes in humidity sneak in. Low temperatures slow the breakdown, but there’s no substitute for a well-sealed, moisture-free space.
Even brief exposure to overhead lights has started unwanted reactions in samples I’ve witnessed. Opaque containers, aluminium foil wraps, and shaded cabinets cut down on light-induced decomposition. Refrigeration doesn’t hurt, but it’s the light-protection that really makes a difference for stability. Lab mishaps—one with a cracked clear bottle—have driven home the point that visibility for inventory checks never outweighs the risks of photodegradation.
Many labs opt for glass, though some rely on specialised plastics that resist corrosion and won’t build up static charges. Glass jars with tight PTFE-lined caps give peace of mind, but good practice always includes clear hazard labels and no overcrowding. Overstacked shelves invite bumps and spills, which in my own lab almost led to a broken bottle incident. Space and access matter as much as container choice. Never gamble by doubling up containers or skimping on compatible linings.
Even well-stored chemicals call for readiness. Once, a faulty seal led to minor exposure; a quick-thinking labmate had the spill kit, goggles, and gloves ready. Emergency shower and eyewash locations need regular checks. Staff and grad students review SOPs before ever opening a fresh shipment. Safety data sheets belong both in the storage area and online, not just filed away. Relabeling every time a new batch arrives may sound fussy, but it prevents confusion during high-stress situations.
Disposal of leftover or outdated diazonium salts lingers as a chore nobody enjoys, but lazy cleanups court disaster. Professional hazardous waste pickup beats makeshift solutions. Neutralising agents only touch these compounds under expert supervision and never go down the drain. Following federal and local environmental rules stops small errors from snowballing into major incidents. Even one forgotten vial risks more than just property.
Years spent around energetic compounds have taught me this: no fancy ventilation system or smart monitor replaces consistent, commonsense habits. Vigilance over logbooks, storage temperatures, and humidity saves more trouble than any quick fix. Every reminder to check seals and update training can keep people and property out of the headlines. Respect for chemicals never grows old, and those who lose it often get reminders they never wanted.
Some chemicals truly demand respect, and 4-Dimethylaminobenzenediazonium Trichlorozincate stands out among them. Anyone who works with diazonium salts quickly picks up on just how unstable these compounds can be. Mix moisture or warmth into the picture, and trouble follows. Frustration with rigid protocols turns into appreciation after a minor spill or close call. I learned more from hearing a bottle fizz than from any lecture. This compound often brings hidden dangers—think nasty explosions, sneaky releases of nitrogen gas, and a knack for irritating skin and eyes.
No shortcuts exist in the world of hazardous chemistry. I don’t step near material like this without heavy-duty gloves, fully sealed goggles, and a decent lab coat. Nitrile gloves beat latex, offering better resistance. Wearing splash-proof face shields brings confidence when reactions threaten to get lively. Handling such chemicals day after day, you stop treating standard safety gear as a suggestion and treat it as trusty armor.
My old lab mate never forgot to mark the calendar with synthesis dates and storage times. Label everything—names, hazards, and dates. Keep the compound in small, clearly sealed vials. Dry and cool conditions help keep instability in check. Steer clear of light and moisture—reactions move fast in the wrong environment. An explosion in a crowded storeroom a few years back still sits fresh in my mind. Lesson learned: Only make what you plan to use soon.
Closed rooms invite headaches and worse. Fume hoods don’t just control vapor—they limit exposure from accidental releases. Too many ignore the simple step of double-checking airflow before starting work, then regret it mid-procedure. Vapors from diazonium salts burn lungs and eyes. Ventilation remains a quiet ally.
Eyewash stations and showers stay ready—for real accidents, not regulations. Practice makes all the difference. My first chemical splash happened because complacency snuck in. A fast sprint to the eyewash brought home how crucial those drills stay. Not every accident ends calmly. Real plans, posted and repeated, cut panic when something spills or boils over. Don’t just count on luck; walk through every “what if” often.
Diazonium compounds do not disappear with a sink rinse. Specialized waste containers mark every corner of a prepared lab. I never toss unused material until it’s spent or properly neutralized—usually in small, controlled portions under supervision. It takes time to build habits for waste paperwork and final neutralization, but these small frustrations outweigh the real dangers of careless disposal. Contaminants from these chemicals lurk too long in ordinary drains.
Chemistry shifts fast. I check updated safety sheets regularly. Colleagues swap stories at conferences about what went wrong and how protocols adapt. Refresher courses feel like insurance against forgetfulness. Shared lessons, new gear, and evolving procedures reflect a culture that values lifelong vigilance.
Accidents don’t care about experience or confidence. Good habits—never working alone, labeling, minimizing quantities, and keeping clear communication—make the difference between an ordinary day and a crisis. Every cleanup and every checklist comes from a place of respect for chemistry’s potential for harm. With every safeguard, the odds tip just a little further toward safety.
This chemical wears a long name for a reason. Its structure packs two interesting components—a diazonium ion that’s attached to a benzene ring, and a counterion group built on zinc and chloride. The backbone starts as an aniline (that’s a benzene ring hugging an amino group), then swaps in the beefier dimethylamino function at the para position. Getting to the diazonium step involves dosing it with nitrous acid under cold conditions, which sets the stage for forming the diazonium ion—the real workhorse here. Scientists don’t just stop after this tweak; the trick is pairing that positively charged diazonium piece with a complex trichlorozincate anion, ZnCl3-, which helps stabilize the whole compound.
Visualize the molecular layout: a flat benzene ring with a -N+2 group locked in at one end and a -N(CH3)2 at the opposite end. This “para” orientation means each group points away, keeping electronic tugging in balance. Instead of floating out as free ions, the diazonium cation and the ZnCl3- anion link up in a salt, locking the molecule into a crystal lattice. The unique triple-chloride arrangement around zinc comes from the pairing of this bulky, sensitive diazonium with something that won’t break apart at the first sign of moisture or a stray light beam.
Diazonium salts behave like drama magnets in a lab—unstable and reactive, especially if the paired counterion can’t offer much support. The trichlorozincate step matters because it tempers the instability, allowing chemists to store and handle the compound for slightly longer stretches. Not safe to keep around forever, but a huge improvement over the bare-bones chloride or nitrate versions, which can explode or decompose unpredictably.
Anyone who’s spent time in a research or dye chemistry lab knows the tightrope walk that comes with diazonium salts. They’re must-haves for forming azo dyes—the vivid reds, yellows, and oranges found in inks, paints, and sometimes foods. Without a way to stabilize the diazonium group, that vivid chemistry fizzles out. Trichlorozincates, thanks to their multi-point grip, give researchers a longer window before decomposition turns a promising batch into a lost cause.
On a practical note, handling and storing solid diazonium salts in the form of trichlorozincates means less risk. Labs worry less about accidental releases of nitrogen gas or room-temperature explosions, both of which can happen if the chemistry isn’t locked down. By holding the molecules together in a snug salt, the compound actually gets used as intended—helping with coupling reactions, dye formation, and analytical research.
Nobody who’s ever seen an unexpected diazonium salt reaction in a flask forgets it. Safety rules grew up around these compounds not because they sound dangerous, but because stories of glassware shattering or splashes from runaway reactions pile up every decade. Classes in organic chemistry now weave lab tales and case studies to drive home why this stabilization matters.
Improvement in counterion chemistry—switching to trichlorozincates, for example—can shrink risk substantially. Easy-to-understand material safety data sheets highlight the lower volatility and lower explosion risk of these “safer” options. Creating better protocols, investing in solid safety training, and choosing trichlorozincate versions keep scientists, technicians, and even students out of hospital beds.
Looking for solutions that marry usefulness and safety drives innovation in the field. Smart choices in structure, driven by hard-earned experience, help chemistry labs everywhere push boundaries without pushing luck too far.
4-Dimethylaminobenzenediazonium trichlorozincate sounds like something straight out of a dusty college chemistry textbook. Most people outside advanced synthetic chemistry have never heard of it, and even fewer will have any reason to buy it. This compound belongs to a group called diazonium salts, which often show up during dye production and complex organic syntheses. They pack a punch, reactivity-wise, and that’s exactly where the complications begin.
Folks in research chemistry might work with these compounds to create special pigments, specialty polymers, or intermediates for other chemicals. In my experience, university labs occasionally look for odd or rare chemicals to tweak certain reactions. Custom synthesis companies still need to jump through hoops: paperwork, approvals, and long procurement cycles for these kinds of reagents.
Quick searches of mainstream chemical suppliers show a blank spot where 4-dimethylaminobenzenediazonium trichlorozincate should be. Sigma-Aldrich, Fisher Scientific, TCI—they all stay clear. If such big players steer clear, hobbyists and smaller operations hit a wall. Bulk resellers and brokers list some diazonium compounds, but this specific trichlorozincate just isn’t out there for easy order placement. It isn’t like asking for acetone or sodium chloride.
Several reasons pile up. Diazonium salts can be dangerously unstable. Storage becomes a nightmare, especially without rigorous controls on moisture and temperature. Transport rules get strict—governments have strong opinions about what moves through airports and highways, especially if there’s possible risk of explosion or misuse. Companies avoid stocking items that don’t move quickly and could spark insurance headaches. Safety concerns affect how chemicals are handled as much as demand does.
I’ve met chemistry grads who think about prepping difficult diazonium salts themselves using textbooks and a little nerve. That is risky. One slip in temperature or an unclean flask can cause severe accidents. Experienced chemists know stories about bench-top mishaps—those lessons get around fast, and labs don’t want to feature in those tales.
The lack of easy availability signals a few things. Regulations around precursor chemicals grow tighter every year, limiting who can buy and handle such substances. Stronger oversight over chemical sales helps prevent accidental misuse and blocks access for those with ill intent. If a researcher or business really needs 4-dimethylaminobenzenediazonium trichlorozincate, they face an uphill climb: custom synthesis through a reputable, licensed provider. That’s expensive, slow, and comes with plenty of paperwork, but it’s how the system keeps people safe.
Specialty chemicals like this shouldn’t be widely available online or at the local supplier. Supporting transparency in supply chains makes a difference. Professional groups and educators teach and learn safe handling, reporting, and documentation. Policy and enforcement won’t loosen up soon, and for good reason. Better funding for legitimate research outfits helps too, so that academic teams can access what they need without unnecessary risk. It’s possible to support real research without offering every risky reagent to just anyone with a credit card.
| Names | |
| Preferred IUPAC name | 4-(Dimethylamino)benzenediazonium trichlorozincate |
| Other names |
Benzenediazonium, 4-(dimethylamino)-, trichlorozincate (1:1) 4-(Dimethylamino)benzenediazonium trichlorozincate |
| Pronunciation | /ˌdaɪˌmɛθɪlˌæmiːnoʊˌbɛnˈziːnˌdiˌæzəˌniəm traɪˌklɔːroʊˈzɪŋkeɪt/ |
| Identifiers | |
| CAS Number | 38189-30-7 |
| 3D model (JSmol) | `3D model (JSmol)` **string** for **4-Dimethylaminobenzenediazonium Trichlorozincate**: ``` CN(C)c1ccc(N#N)cc1[Zn]Cl3 ``` |
| Beilstein Reference | 2084506 |
| ChEBI | CHEBI:53213 |
| ChEMBL | CHEMBL1406612 |
| ChemSpider | 13316153 |
| DrugBank | DB13803 |
| ECHA InfoCard | 100_216_266 |
| EC Number | 209-536-2 |
| Gmelin Reference | 85409 |
| KEGG | C05938 |
| MeSH | D016692 |
| PubChem CID | 71310861 |
| RTECS number | KH8575000 |
| UNII | HD0U87T83E |
| UN number | 3394 |
| CompTox Dashboard (EPA) | DTXSID80821495 |
| Properties | |
| Chemical formula | C8H12Cl3N3Zn |
| Molar mass | 356.87 g/mol |
| Appearance | yellow powder |
| Odor | Odorless |
| Density | 1.28 g/cm3 |
| Solubility in water | Soluble |
| log P | -2.7 |
| Vapor pressure | <0.1 mmHg (20 °C) |
| Acidity (pKa) | -2.8 |
| Basicity (pKb) | 6.0 |
| Magnetic susceptibility (χ) | -67.0 × 10^-6 cm³/mol |
| Refractive index (nD) | 1.668 |
| Viscosity | 3 cP (20 °C, 15% in H2O) |
| Dipole moment | 6.07 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 252.6 J·mol⁻¹·K⁻¹ |
| Pharmacology | |
| ATC code | V04CX |
| Hazards | |
| GHS labelling | GHS02, GHS03, GHS06, GHS09 |
| Pictograms | Exploding bomb, Skull and crossbones, Health hazard |
| Signal word | Danger |
| Hazard statements | H301 + H311 + H331: Toxic if swallowed, in contact with skin or if inhaled. |
| Precautionary statements | P264, P280, P302+P352, P305+P351+P338, P332+P313, P362+P364, P337+P313, P501 |
| NFPA 704 (fire diamond) | 3-2-3 |
| Autoignition temperature | Autoignition temperature: 550 °C |
| LD50 (median dose) | LD50 (median dose): 50 mg/kg (intravenous, mouse) |
| NIOSH | B9678 |
| PEL (Permissible) | PEL: Not established |
| REL (Recommended) | 0.2 mg/m³ |
| IDLH (Immediate danger) | NIOSH has not established an IDLH for 4-Dimethylaminobenzenediazonium Trichlorozincate. |
| Related compounds | |
| Related compounds |
Aniline 4-Dimethylaniline Benzenediazonium chloride 4-Dimethylaminobenzenediazonium chloride Diazonium salts Zinc chloride |
