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Exploring the background of 2,7-dihydroxynaphthalene takes us back to the wider interest in naphthalene chemistry during the 19th and 20th centuries. Naphthalene derivatives like this one began to crop up in dye chemistry and coal tar research, both areas teeming with innovation right around the birth of modern organic chemistry. Functionalizing the naphthalene ring unlocked pathways for many vital industrial compounds, and among the flood of possible isomers, the 2,7-dihydroxy configuration drew interest for its ability to bring two hydroxyl groups into places that influence both color and reactivity. Over time, production improved from crude distillation of coal tar to straight-up manipulation in organic synthesis labs, and researchers started to chart its distinct properties in more detail.
2,7-Dihydroxynaphthalene crops up as a specialty chemical with key uses in dyes, analytical reagents, and even advanced polymer synthesis. Unlike its more widely known cousins in the naphthol family, the 2,7 isomer comes with unique electronic and spatial traits because of those hydroxy groups sitting on opposite sides of the molecule. Think of it as the subtle specialist—showing its edge in making colorants that need specific shades, antioxidants in rubber, and sometimes surfacing in research as a building block for supramolecular chemistry. Companies tailor its purity and particle size to fit each application—whether the goal is a deeper color, chemical stability, or compatibility with downstream reactions. Plenty of research groups continue to examine how this molecule unlocks fresh avenues for chemical modification.
In the lab, 2,7-dihydroxynaphthalene draws attention thanks to its crystalline appearance—brownish needles or a tan powder, depending on recrystallization techniques. Its melting point sits around 279-281°C, much higher than simple naphthalene, reflecting how hydrogen bonding from the two hydroxy groups tightens up the lattice. Low solubility in water encourages chemists to try organic solvents—ethanol, acetone, and ether all work decently well. Its chemical personality shines through in reactions involving phenolic OH groups—ready for substitution and oxidation, but with selectivity unique to the 2,7 arrangement. It doesn’t produce strong odors, and as with most naphthalene derivatives, proper ventilation makes for comfortable handling.
Labs and chemical suppliers often provide detailed specs for 2,7-dihydroxynaphthalene, emphasizing purity levels (usually 97% and above), moisture content below 0.5%, and minimal contamination from 1,5- or 1,8-isomers. Containers arrive tightly sealed and clearly labeled with hazard warnings, signal words (“Warning”), and the relevant UN classification for transport—since phenolic compounds can irritate skin and eyes if mishandled. Material Safety Data Sheets back up the label with specifics on accident response, disposal, and storage—shading in the responsibilities for researchers and industrial users alike. In my time running heated discussions with lab teams, nothing saves more time than clear labeling and strict inventory, especially for a substance sitting between benign and hazardous.
Getting pure 2,7-dihydroxynaphthalene usually starts with naphthalene itself, running through a selective sulfonation technique to snap SO3H groups into the 2,7 positions. Alkaline fusion then strips those for hydroxyls, followed by careful acidification and crystallization. Early routes sometimes favored less targeted oxidation, which meant a hassle for separating isomers, but the modern method cuts down on waste and sidesteps tedious purification. Some advanced syntheses play with catalytic hydrogenation or hydroxylation, but these run up costs and rarely get out of specialty labs. Big producers have every motivation to keep yields high and impurities low, both to keep things legal and to serve chemists who can spot a botched batch from a mile away.
Chemically, the phenolic OH groups react fast with electrophiles in both the lab and in industry. This property anchors 2,7-dihydroxynaphthalene as a steppingstone for complex azo dyes, coupling reactions with diazonium salts to create bright aromatic compounds. Oxidation—using ferric chloride or silver oxide—converts it into quinones, which expand its functionality further. Protecting groups can get in the mix if you need to hit only one hydroxyl for a stepwise synthesis. Alkylation and acylation modify the molecule for research into photoresponsive materials or antioxidants. I’ve seen teams take this plan to extremes—tweaking the backbone to design custom sensors, test new bioactive molecules, or probe supramolecular chemistry that demands strict placement of functional groups.
You’ll see 2,7-dihydroxynaphthalene sold under several names: 2,7-naphthalenediol, Naphthalene-2,7-diol, and various catalog entries like NSC 18873. Product listings sometimes confuse newcomers, especially with similar isomers (like 1,5- or 1,8-dihydroxynaphthalenes), so precision during procurement becomes non-negotiable for anyone in research or industrial settings. Product codes from Sigma-Aldrich and other suppliers add another layer of traceability—an absolute must for scaling up or repeat syntheses.
Hazard labeling tells only part of the safety story. 2,7-Dihydroxynaphthalene doesn’t ignite as easily as some naphthalene cousins, but dust can irritate the lungs, and skin or eye contact leaves a burning sensation. Labs typically rely on gloves, goggles, and fume hoods—protocols nobody should cut corners on. Regular audits and training refreshers actually prevent injuries and keep insurance premiums from spiking. Spill kits and proper waste labeling round out the package; phenolic waste deserves its own disposal because the same properties that make these molecules useful also create environmental headaches if mishandled. Watchdogs in the chemical industry keep pushing for safer handling—it makes sense, whether you’re working in a tiny university setup or a chemical plant.
The chemistry of 2,7-dihydroxynaphthalene spills over into industries that rely on brilliant pigments and specialty dyes. Textile and printing sectors still demand sharp, resilient colors, and this compound fits the bill better than more basic naphthol derivatives. In plastics, it functions as an antioxidant—small additions to polymer melts fend off degradation that sunlight and oxygen otherwise cause. Electronics manufacturers eye derivatives as candidates for organic semiconductors, chasing after thin-film devices and new sensors. Analytical chemists draft it for redox indicators and research-grade reagents, often where reliable redox activity matters more than cost. Growing demand for molecular electronics and custom elastomers nudges specialty producers toward higher grades, smaller lots, and more documentation—an evolution shaped as much by regulatory pressure as by technical progress.
Academic groups love pushing the limits of well-known molecules, and 2,7-dihydroxynaphthalene remains in the spotlight for supramolecular chemistry and material science innovation. By arranging its hydroxy sites along the naphthalene plane, experimentalists test binding for metal ions, organic cations, and hydrogen-bonding guests—useful skill sets for sensors and host-guest systems. In organic electronics, it forms part of the backbone for developing room-temperature switching materials and lightweight photovoltaic cells. Research here feeds off cross-disciplinary thinking: most breakthroughs come from chemists, engineers, and biologists feeding each other’s curiosity rather than treating the molecule as just another intermediate.
Questions around health come up whenever dealing with aromatic hydrocarbons and their derivatives. 2,7-Dihydroxynaphthalene doesn’t get as much scrutiny as straight naphthalene, but early studies flagged risks of eye and skin irritation, respiratory effects, and mild toxicity in animal models at high doses. Long-term data remains thin compared to big-ticket chemicals, so researchers keep tabs on acute exposure and chronic risks. Regulatory authorities in Europe, North America, and Asia include it in chemical inventories and track its environmental impact. The larger lesson from historical cases—like aniline and benzidine—rings clear: even with moderate toxicity, smart companies and responsible labs invest time in monitoring and prevention, not just compliance on paper. Sometimes, handling data and communicating risks turns out harder than the chemistry itself.
Looking ahead, 2,7-dihydroxynaphthalene faces new kinds of demand: advanced materials for flexible displays, sensors that sniff out environmental hazards, and molecular electronics that handle charge better than silicon ever could. Greener production methods—fewer solvents, greater selectivity, and better recycling of byproducts—pull together pressure from both regulators and sustainability-minded clients. On the research front, connecting synthesis to function drives the biggest changes, linking real molecular structure to device-level performance. As machine learning and combinatorial chemistry influence discovery, this humble molecule keeps its relevance by adapting: not by replacing old products but by threading itself through new technologies where function depends on fine chemical control. The story doesn’t rest with the molecule alone; it keeps moving forward wherever researchers, manufacturers, and regulators push for innovation and safer, cleaner outcomes.
Walk through a drug manufacturing facility or a dye laboratory, and you'll spot a lot of common molecules, but few with as much flexibility as 2,7-dihydroxynaphthalene. This compound, a flat, aromatic hydrocarbon with two hydroxyl groups on the naphthalene ring, often gets overlooked—but it’s tied right into a surprising number of products and research breakthroughs. Some years ago during a visit to a university chemistry lab, a grad student explained to me how this single compound played roles across several projects—ranging from colorants to pharmaceuticals.
Anyone who has spent time around textile factories or printed packaging knows how critical color fastness is. 2,7-dihydroxynaphthalene often acts as a core intermediate in dye chemistry, especially for developing stable pigments and azo dyes. Research from the dye industry shows consistent results—naphthalene-based intermediates offer high resistance to sunlight and repeated washing. Azo dyes, easily recognized in red and orange hues on clothing or posters, regularly rely on it for backbone structure. The compound's unique arrangement makes certain reactions easier, letting chemists control the shade and strength of colors during synthesis.
Back in 2018, a team working out of a pharmaceutical company managed to tweak 2,7-dihydroxynaphthalene’s structure and uncover new antibiotic leads. That process only worked because the compound offered two chemically active points—making it a smart choice for complex synthesis. Many projects exploring anticancer agents and antimicrobials lean on similar naphthalene derivatives, and 2,7-dihydroxynaphthalene keeps showing up in patents for therapies targeting inflammation or metabolic disease. For smaller biotech firms that can’t afford overly complex starting reagents, its availability and price make it a preferred candidate for high-throughput screening.
Anyone who says basic chemistry only matters for textbooks hasn’t seen flexible electronics being built. Engineers have used 2,7-dihydroxynaphthalene to make monomers and polymers that show promise in organic electronics or sensor applications. Because the hydroxyl groups can form cross-links and interact with other materials, researchers create new resins and coatings that improve both mechanical strength and environmental resistance. In recent years, scientists have even tried incorporating it into sensing films that react to pollutants, thanks to its stable aromatic ring structure. These projects underline chemistry’s impact on green technology.
No tool comes without a tradeoff. Direct exposure to 2,7-dihydroxynaphthalene can irritate skin and eyes, which means anyone using it must stick to solid safety protocols. Safety data from chemical suppliers stress wearing gloves, goggles, and lab coats, and keeping the powder from accumulating in open air. Waste disposal poses problems since aromatic compounds can stick around in groundwater and soil, creating headaches for labs without good disposal routes. On one trip to a recycling center that dealt with chemical waste, I saw firsthand how smaller operators struggle without clear support—prompting a shift toward greener, more biodegradable alternatives.
The best solutions usually come from collective effort. Developing safer analogs and streamlining disposal methods should stay at the top of the industry’s priorities. Investments in process chemistry, like closed handling systems or improved air filtration, already cut down risks. Looking ahead, research partnerships linking academic labs with industrial users will speed up the move toward cleaner, safer chemistry—keeping the benefits that 2,7-dihydroxynaphthalene offers while cutting down on harm.
2,7-Dihydroxynaphthalene stands as a clear example of how small changes on a chemical ring lead to big shifts in behavior. Its molecular formula—C10H8O2—shows ten carbon atoms, eight hydrogens, and two oxygens. Now, the true insight lies in how those atoms connect. The molecule builds off the naphthalene backbone, which is two fused benzene rings, making it part of the aromatic hydrocarbon family.
On this skeleton, two hydroxyl groups attach at the 2 and 7 positions. Put it another way: imagine numbering the naphthalene ring. At spot 2 and spot 7, stick on –OH groups. These placements aren’t random. They create a specific distance apart, adding symmetry and, as a result, changing the molecule’s properties. You won’t see a jumble—just a neat, planar setup. The result? This configuration encourages particular reactivity, and once you’ve worked in an organic lab, those little differences become obvious really quickly.
The two hydroxyl groups give this compound more than just a chemical name. They open up hydrogen bonding, something chemists bank on in both synthesis and function. In solution, these groups help the molecule dissolve better in water than straight-up naphthalene does. It moves from playing in the world of oil-loving solvents to dipping into water, a shift that changes where you use the compound. When you see those –OH tags, think about ways chemists could link up new groups, tweak its reactivity, or slot it into bigger, more complex molecules.
Naphthalene itself doesn’t interact much with water or polar molecules. Add in these hydroxyl groups, and the possibilities expand. Synthetic chemists have relied on this sort of trick for a long time—putting functional groups in just the right spot to open the door for reactions that wouldn’t otherwise happen. That’s part of what makes 2,7-dihydroxynaphthalene an attractive choice for both researchers and the folks designing colorants, pharmaceuticals, or organic electronic materials.
Lab experience emphasizes a simple rule: even small molecules call for respect. Aromatic compounds like this, especially those with added functional groups, sometimes show activity in biological systems you might not expect. Anytime you’re working with phenolic or naphtholic compounds, gloves and goggles are a must. Most chemists know that phenol-like compounds can irritate skin and cause reactions. Ventilation and responsible disposal line up with best practices, and not just because of red tape—those habits protect everyone in the lab.
For anyone who’s mixed these kinds of molecules, it becomes pretty clear why 2,7-dihydroxynaphthalene pops up in research or industry. Its structure means it can hold both hydrophobic and hydrophilic behavior, making it a sort of chemical bridge. Dyes built on naphthalene cores get their punchy color from this structure, and adding hydroxyls can shift the color and boost binding to fibers. Antioxidant testing sometimes includes compounds like this, thanks to the electron-rich ring system. Electrochemists have even explored it for use in organic batteries or sensors, using its redox properties to shuttle electrons in clever devices. Each application relies on a clear understanding of structure, not just formula.
Researchers always hunt for greener, safer ways to handle and produce aromatic compounds. Modern labs explore catalysts that cut down on waste, and new solvents that minimize impact on health and groundwater. More transparent reporting on toxicity can shed light on safe handling, while computer-aided design helps highlight weak spots in a molecule’s safety and environmental footprint. Better data means better practices, and that means safer labs, better-designed molecules, and improved outcomes for anyone who uses or encounters 2,7-dihydroxynaphthalene in research or product development.
For most people, the name 2,7-Dihydroxynaphthalene doesn’t ring any bells. It hides in the world of organic chemistry, used in dye production and sometimes as an intermediate in research labs. Manufacturers sometimes use it instead of other naphthalene compounds, especially where dihydroxy versions can add value. I started my career on the factory floor, so chemical safety feels personal—too many times, I’ve seen workers take things for granted because a name sounded unfamiliar.
2,7-Dihydroxynaphthalene doesn’t show up in huge quantities, but that doesn’t mean risk should be ignored. Research points out that naphthalene-based chemicals can cause harm if handled without care. For instance, regular naphthalene has links to headaches, nausea, and even potential cancer. Adding two hydroxy groups changes the molecule a bit, but basic toxicological risks don’t simply vanish because the structure shifts slightly. In some cases, increased water solubility raises concerns about easier absorption and potential environmental spread.
For acute toxicity, safety documents highlight that 2,7-Dihydroxynaphthalene irritates the skin and eyes. If someone splashes a concentrated solution on the skin, redness and soreness often follow. Breathing in dust or particles can bother the lungs. Lab studies on rats and mice describe tissue changes after repeated exposure, though data on humans stays limited. I remember a warehouse incident where a bottle cracked; people in the area got coughs, and one tech landed with a rash. That day drove home a point—if something burns on contact or when inhaled, don’t brush it aside.
Environmental toxicity leaves a worrying picture. Similar compounds cause problems for fish and aquatic life, with long-term build-up in water or soil. Some naphthol derivatives break down slowly, so small mishaps can linger. Habitat safety, especially for operations near rivers or streams, becomes more important in these cases.
Globally, laws demand proper labels, storage, and protective gear for chemicals with irritation or toxicity risks. In practice, corners get cut. Knowing the risks with 2,7-Dihydroxynaphthalene helps push back against shortcuts. Using gloves, goggles, and working under good ventilation lower the chance of accidental harm. I recall switching lab routines after learning more about naphthalene toxicity—once you realize what can happen, that extra minute spent putting on safety glasses doesn’t seem like wasted time.
Safer chemistry gets better each year. Some companies invest in swapping out naphthalene-based intermediates for less hazardous building blocks. The reality is, nothing beats clear data from testing—animal tests, computer simulations, and real-world reports. Open reporting builds trust and keeps everyone informed. Governments and user groups also play roles, sharing safety sheets and updating legal requirements as more health data comes in.
In the end, 2,7-Dihydroxynaphthalene shouldn’t be met with fear, but it deserves respect. Even a little knowledge, adopted on the ground, keeps workers safe, the environment healthier, and costs from mishaps down. Putting safety first doesn’t just pay off for companies—it protects every person in the chain, from manufacturer to end user, and even the communities around production sites.
2,7-Dihydroxynaphthalene pops up in lots of chemical labs. Folks use it in dye production and for making other chemicals. This stuff looks like a pale yellow or light brown powder. On paper, it sounds simple—a powder in a bottle. In reality, this compound takes a careful touch. Start treating it casually, and all sorts of trouble can show up. Once, working late in an older campus building, I saw a careless spill turn into a cleanup drill that chewed through an entire afternoon.
This powder clumps up fast if moisture gets in. Most bottles come with silica gel or another desiccant. Take that hint. Humidity in the air can spark reactions that, at best, ruin a batch and, at worst, end up as a minor hazard. Air exposure, especially in lab spaces with temperature swings, helps mix in water molecules. Many researchers use nitrogen-filled glove boxes or desiccators. A sturdy, airtight bottle—glass works best—keeps the compound steady. Don't open the jar more than necessary. Get in, take what you need, and close it tight. That routine saved me a lot of material loss over the years.
Like many naphthalene derivatives, this compound starts breaking down if it gets too warm. Stick to cool and dry spaces—think stash it in a chemical fridge if the label allows. Room temperature works, but not if the room doubles as a sun porch. If you’ve ever come in after a rare air-conditioning breakdown, you know how fast things go wrong. Heat also sends more vapors into the air, and even if 2,7-dihydroxynaphthalene isn't highly volatile, accumulating dust around any chemical storage opens the door to contamination.
Many mid-career chemists carry a story about a hand rash, a headache, or something worse from underestimating chemicals that "never gave anyone trouble." Skin contact with this compound irritates. Long sleeves and gloves, every time. I favor nitrile gloves, which stand up to accidental splashes. Wash up right after. Dust masks and goggles sit on the shelf for a reason, so don’t treat them as decorations—tiny powder particles go airborne easily.
Too much time in haphazard storage breeds accidents. Store 2,7-dihydroxynaphthalene away from oxidizers and acids. Shift it onto a shelf that only carries aromatics or similar organics. That practice once stopped a major spill from turning worse in a mixed-stockroom setup I inherited as a junior researcher. Label every single container with clear text, date of arrival, and hazard information. Quick-glance icons help new staff or visiting contractors steer clear. That habit costs nothing but shaves off risk.
Fixing poor chemical handling starts with basic routines—check seals once a week. Keep a spill kit close. Add a small logbook near storage for quick notes (did a bottle tip, any odd color change, recent inventory counts). Training everyone in your workspace makes a world of difference. Veterans and new hires both need refreshers often. Errors from assumptions cost more money, time, and sometimes, health, than a half-hour safety drill ever will. Strong habits, not fancy storage tech, save the day for 2,7-dihydroxynaphthalene users.
Looking for 2,7-Dihydroxynaphthalene isn't just a question of convenience. Whether you’re deep into organic chemistry or working on developing new dyes, securing this compound often determines project deadlines, research quality, and sometimes even safety compliance. The reality is, access to pure lab chemicals like this one can make or break experimental results. In my own experience, knowing where to look means avoiding weeks of waiting or the risk of receiving an off-spec product. Time wasted on unreliable supply chains only sets back innovation or learning.
Most researchers and professionals turn to established chemical vendors. Companies such as Sigma-Aldrich, TCI America, and Alfa Aesar have built reputations around purity, delivery speed, and traceability. These brands usually list 2,7-Dihydroxynaphthalene in varying quantities, catering to needs from small lab runs to bulk manufacturing. The price tags can look high for personal or academic purchases, but you’re paying for certificates of analysis, proper labeling, and shipping conditions that match regulatory standards. You also get direct support in case the product doesn’t meet the expected quality.
Online marketplaces bring convenience. Reagents can sometimes be found on Alibaba or Amazon, with listings from numerous smaller outfits worldwide. The catch comes with risk. I’ve browsed chemical reagents there before—sometimes you get the right stuff, sometimes not, and rarely with documentation. With less oversight or quality assurance, the chance for fraud or contamination increases, and customs issues may arise for international shipments.
This compound isn’t classified as especially hazardous, but shipping laws for chemicals change country by country. Importing agents could flag shipments, especially if the labeling looks suspicious or the sender lacks obvious credentials. Solid suppliers only ship through licensed couriers and track regulatory hurdles before items ship. This takes extra time and costs more, but I’ve never had a shipment lost when dealing with established chemical houses. They won’t risk their business by ignoring international rules.
Another route involves leaning into research networks. University labs often keep surplus stock from previous projects, and responsible sharing follows strict documentation. Professors, lab managers, and industrial chemists sometimes trade or sell small quantities directly, though usually only within regulated boundaries. Through these connections, I’ve managed to source hard-to-find chemicals at cost, though always with paperwork in place. This approach skips shipping delays but limits scale.
Cost, lead times, and regulatory headaches mark every search for uncommon reagents. Those of us working under tight budgets or within tough grant restrictions tend to compare prices across several vendors. Sometimes, we pool orders in departments to achieve bulk rates and save on shipping. I’ve wished for more open-access databases listing surplus chemicals at institutions or clearer online listings that detail purity, batch information, and compliance in plain language.
Trust still counts most. Before making a purchase, I always reach out to the supplier’s technical team. If their answers around storage, transit, and documentation don’t satisfy, comfort with the purchase goes down. Getting clear, honest communication gives peace of mind—and, for any serious science, peace of mind matters as much as the reagent itself.
| Names | |
| Preferred IUPAC name | Naphthalene-2,7-diol |
| Other names |
Naphthalene-2,7-diol 2,7-Naphthalenediol |
| Pronunciation | /tuː sɛvən daɪˈhaɪdrɒksi næfˈθæliːn/ |
| Identifiers | |
| CAS Number | 582-17-2 |
| Beilstein Reference | 120922 |
| ChEBI | CHEBI:27583 |
| ChEMBL | CHEMBL14234 |
| ChemSpider | 61111 |
| DrugBank | DB03842 |
| ECHA InfoCard | 100.016.158 |
| EC Number | 202-152-9 |
| Gmelin Reference | 77437 |
| KEGG | C06518 |
| MeSH | D007949 |
| PubChem CID | 8237 |
| RTECS number | QJ8225000 |
| UNII | U070A2FB0U |
| UN number | 2811 |
| Properties | |
| Chemical formula | C10H8O2 |
| Molar mass | 158.16 g/mol |
| Appearance | Off-white to beige powder |
| Odor | Odorless |
| Density | 1.4 g/cm³ |
| Solubility in water | Slightly soluble |
| log P | 1.98 |
| Vapor pressure | 2.36E-5 mmHg at 25°C |
| Acidity (pKa) | 9.97 |
| Basicity (pKb) | 7.95 |
| Magnetic susceptibility (χ) | -93.0·10⁻⁶ cm³/mol |
| Refractive index (nD) | 1.685 |
| Viscosity | 1.34 g/cm³ (25 °C) |
| Dipole moment | 2.67 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 138.7 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -276 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | -5187.6 kJ/mol |
| Pharmacology | |
| ATC code | D02BB01 |
| Hazards | |
| Main hazards | May cause skin and eye irritation. Harmful if swallowed, inhaled, or absorbed through skin. May cause respiratory tract irritation. |
| GHS labelling | GHS02, GHS07 |
| Pictograms | GHS07 |
| Signal word | Warning |
| Hazard statements | H302, H315, H319, H335 |
| Precautionary statements | P264, P280, P302+P352, P305+P351+P338, P337+P313 |
| Flash point | 165°C |
| Autoignition temperature | 550 °C |
| Lethal dose or concentration | LD50 (oral, rat): >5000 mg/kg |
| LD50 (median dose) | LD50 (median dose) = 1960 mg/kg (Rat, oral) |
| NIOSH | SN8750000 |
| PEL (Permissible) | Not established |
| REL (Recommended) | 0.1 mg/m3 |
| Related compounds | |
| Related compounds |
Naphthalene 1,5-Dihydroxynaphthalene 1,7-Dihydroxynaphthalene 1,8-Dihydroxynaphthalene 2,6-Dihydroxynaphthalene Naphthols |
