© 2026 Nanjing Finechem Holdings Co., Ltd,
All Right Reserved
Chemists stumbled onto Salicylaldehyde back in the days of lively discovery and hands-on trial. Friedrich Wöhler and Justus von Liebig, heavyweights in 19th-century chemistry, found that breaking down salicin produced an aromatic compound with a sharp, almond-like scent: salicylaldehyde. No modern lab equipment, just a knack for observation and the will to persist through smelly glassware. After the initial discovery, academic efforts dug a bit deeper into the benzene ring structure, inspired by this pungent little molecule, and opened new doors in both synthetic chemistry and medicine. As years ticked by, research on aromatic aldehydes expanded, but salicylaldehyde always made its mark as a lab staple, thanks to its ready reactivity and straightforward preparation.
Today, salicylaldehyde shows up in production plants that churn out tonnage for big-name labs and eager researchers. It’s that sharp liquid you notice in the stockroom, used in more places than most folks realize—organic synthesis, analytical chemistry, and even the world of aromas and flavorings. It’s never flashy on the market, but chemists value it for sheer reliability and the structural punch it packs, especially with its ortho-hydroxy group beside the aldehyde, giving it unique chemical personality among dozens of aromatic aldehydes.
Pour out salicylaldehyde and you’ll spot a colorless to yellowish oily liquid. That smell will hit—bitter almonds, unmistakable and strong, enough to make you check the cap twice. It doesn't dissolve in water, but most alcohols and ethers invite it in. The mix of a benzene ring with an aldehyde and a hydroxyl group opens the door to lots of transformations. Salicylaldehyde resists casual breakdown: it’s stable at room temp, but keep it sealed away from sunlight and air to curb slow oxidation. With a melting point just under room temp and a boiling point around 196-198°C, it’s practical to use for lab syntheses, but don’t let the manageable boiling point fool you—the volatility combined with the strong odor means ventilation isn’t optional.
Ask any chemist about purity, and you'll hear complaints about trace impurities causing headaches under sensitive conditions. For most lab work, salicylaldehyde rolls in at over 98% purity, enough for reactions to run smoothly. Labels don’t just warn about the fumes or the possibility of eye or skin irritation—they list the CAS number so researchers know what sits inside and so regulatory officers can track movement.
Most of the salicylaldehyde on the shelves starts in chemical reactors where phenol meets chloroform under alkaline conditions. Called the Reimer-Tiemann reaction, this process originates in the late 19th century but has stuck around because it works—simple, reproducible, but not always neat. Anyone who’s run it knows the grim clean-up and the challenge of controlling side reactions that nibble away at yield. Today’s chemical plants automate large-scale production—the principle stays the same, but with catalysts, solvent recovery, and rigorous waste handling. Teams keen on reducing environmental impact look at alternatives, like green oxidations of salicyl alcohol, but old habits die hard.
Salicylaldehyde isn’t just a quiet reagent. Its structure hands it a place in the spotlight of organic synthesis: chemists reach for it to build heterocyclic rings, Schiff bases, and chelating ligands. The hydroxyl and aldehyde work together to steer reactions—condensations, cyclizations, and complexations flow easily. Even the pharmaceutical industry taps into these functions: salicylaldehyde forms the bedrock for key metal complexes, dynamic dyes, and selective sensors, all thanks to the flexible combination of functional groups. In coordination chemistry, it helps build ligands that bind metals tightly, yielding compounds with magnetic, catalytic, or bioactive properties.
Walk through catalogs and you’ll see names like o-Hydroxybenzaldehyde or 2-Hydroxybenzaldehyde. The IUPAC guides formal naming, but across continents and suppliers, the common names persist and become shorthand for researchers everywhere. Sometimes, the name of a compound gets tangled up in language or trade—here, the core structure and the classic use hold its identity steady.
Open a fresh bottle of salicylaldehyde in a small, quiet lab, and a strong, bitter almond odor sticks around. The old rule kicked in—handle with gloves, wear eye protection, and make sure there's a fume hood running. Salicylaldehyde irritates skin and eyes, and overexposure can lead to headaches or, at high concentrations, problems with breathing. Rules from main regulatory bodies, such as OSHA and REACH, set exposure limits and require documentation for safe handling and disposal. People who work around this compound quickly learn the importance of tight protocols and fastidious housekeeping, even if it feels like overkill. A clean workspace isn’t just about pride: with volatile, stubborn-smelling compounds like this one, it’s about health and peace of mind.
Salicylaldehyde sits quietly in many fields, showing up in organic synthesis for simple aldehyde tests in undergrad labs, all the way to industry-scale ligands for separation and catalysis. Its ability to form Schiff bases finds use in analytical chemistry—color tests and sensors benefit from clear, distinct changes on reaction. Coordination chemists flock to salicylaldehyde for preparing chelates that bind metals in medical imaging or industrial processes. In the world of fragrances, its bitter-almond note brings depth to blends that need something sharp and aromatic. There’s more: researchers chase new uses in medicine, probing derivatives for antimicrobial, antiviral, and anticancer properties, always banking on the molecule’s ready reactivity.
Labs around the world don’t let up on salicylaldehyde—it’s a jumping-off point for hundreds of projects, from bimetallic ligands to chiral catalysts. What used to be a simple analytical standard now gets validation in sensor design. In my own experience, running reactions with this aromatic aldehyde often means quick feedback—yields pop, colors form, and purification doesn’t cause too many late nights. Academic groups keep publishing new modifications, pushing the envelope on what this single functional group arrangement can do. The raw curiosity that spurred Wöhler now fuels USB-connected analytical devices and complex pharmaceuticals, all with a dash of salicylaldehyde magic in the mix.
Toxicity studies show that, like many aromatic aldehydes, salicylaldehyde doesn’t play nice in uncontrolled settings. Animal tests mark it as acutely toxic at high doses—irritation to mucous membranes and central nervous system effects crop up fast. Chronic exposure leads to nervous system depression and breathing trouble. Compared to some nastier aldehydes, it sits in the middling range, but that's not a pass to get sloppy with care. Regulatory agencies track limits closely, and documented cases of occupational exposure guide new workplace rules. The goal is to keep progress moving without ignoring what overexposure can do—clear guidelines, better engineered controls, and plenty of technical education fix most risks before they cause trouble.
Salicylaldehyde isn’t running out of potential. Surveys of current research show new sensor designs that rely on its ability to coordinate metals with pinpoint selectivity, delivering faster results in medical diagnostics and environmental screenings. Development of green chemistry techniques stands out: catalyzed oxidations or renewable feedstock production could lower environmental loads, matching public pressure and stricter regulations. Technological advances mean faster screening of new derivatives, some already showing action against bacteria resistant to classical therapeutics. The past century built the foundation—now, both legacy and innovation will keep salicylaldehyde at the center of lab benches and factory floors. Anyone in chemistry knows—simple scaffolds, when explored with fresh curiosity, deliver surprises beyond the standard catalog page.
Salicylaldehyde shows up as a colorless to pale-yellow oily liquid, best known for a distinct almond-like aroma. It comes from salicylic acid and belongs to the group of aromatic aldehydes. Many who use it in the lab know it’s more than just a curious bottle on a shelf. It serves as a solid foundation for a range of chemicals. The chemical formula, C7H6O2, doesn’t tell the whole story. What matters is how people use it and the impact that use holds for science and daily life.
Anyone who’s spent time in an organic lab, whether in school or industry, has probably worked with this compound to some degree. Salicylaldehyde takes a key spot in the production of complex molecules. It acts as a versatile starting material because of its reactivity. Chemists use it to make ligands, which help create materials for research and industrial applications. For example, the field of coordination chemistry depends on compounds like salicylaldehyde for creating chelating agents. These agents are essential for metal ion binding, which helps with everything from making batteries to cleaning up environmental toxins.
Salicylaldehyde carries weight in drug development. It has seen use as a precursor in the synthesis of pharmaceuticals and fine chemicals. Salicylaldehyde itself isn’t an active pharmaceutical ingredient, but it helps generate other compounds, like coumarins and Schiff bases, which researchers then test for antibacterial, antifungal, or anticancer activity. In my research experience, modifying salicylaldehyde’s structure leads to compounds with new characteristics. This experimentation helps open doors for treatments that may otherwise remain undiscovered. Researchers regularly look for structural tweaks to improve bioactivity, and this compound gives them a reliable place to start.
Look outside the laboratory and the compound still makes its mark. Makers of dyes and pigments rely on salicylaldehyde for unique colorants. Its strong reactivity with certain chemicals means it provides deep shades in dye products and some inks. The fragrance industry taps into that almond-like aroma, using salicylaldehyde as part of perfumes and soaps. Its presence brings a natural, pleasant note that sticks around. The scope even reaches agrochemicals, with salicylaldehyde helping to synthesize products that protect crops or keep pests at bay.
Handling salicylaldehyde calls for respect. Anyone in the field remembers the importance of protective gear. Exposure to vapors can cause irritation, and it’s toxic at higher concentrations. From my own work, spills always meant stopping production until a full cleanup happened—nobody cut corners. Strict storage and waste handling protocols help prevent environmental contamination. Companies take care to meet safety regulations, recognizing that responsible handling keeps communities and ecosystems safer.
One area that stands out involves greener synthetic pathways. While traditional methods generate chemical waste, recent advances in catalysis encourage less hazardous processes. As researchers find new ways to recycle starting materials or cut emissions, chemical plants improve sustainability. Sharing open-access research and best practices helps broaden this shift. In my own projects, collaboration across academic and industrial lines produced smoother, less wasteful syntheses. These changes not only lower costs but reduce the long-term footprint of chemical manufacturing, showing how the smallest innovations can make a big difference.
Salicylaldehyde pops up in a lot of labs and factories. It shows up as a colorless to pale yellow oily liquid. Many chemists recognize its signature almond-like scent. The compound plays a part in making dyes, perfumes, and pharmaceuticals. For those who have spent time in a research setting, that sharp smell always tells you to reach for gloves and eye protection right away.
Every time someone handles salicylaldehyde, there's the question of safety. Breathing its vapors can really irritate your nose, throat, and lungs. Spilling it on unprotected skin leads to redness and discomfort faster than you might expect. Eyes don’t like it one bit, either. Cases of chemical burns or lingering irritation aren’t rare if goggles stay in the drawer. The liquid doesn't explode or catch fire instantly, but it is flammable and releases fumes that spread through poorly ventilated rooms in no time. Once those fumes reach an ignition source, their risk multiplies.
Salicylaldehyde does more than short-term harm. Swallowing even small amounts brings on headache, dizziness, and nausea. That's what makes food and drink bans in the lab more than just annoying rules. Chronic exposure paints a bleaker picture. The compound can be absorbed into the body through the skin, lungs, or mouth, gradually affecting the nervous system and even causing liver issues. Studies in animals reveal possible mutagenic effects, though long-term data for humans still needs more depth.
In the workplace, I’ve seen gloves eaten away by spills. People sometimes roll their sleeves up and pay for it later with chemical burns. In stories passed around lab benches, you hear of minor mistakes snowballing because someone didn’t respect the warning labels. This isn’t just lab folklore—hospital visits linked to exposure make the paperwork stack high for both workers and employers.
A locked cabinet and clearly labeled bottles always beat crossed fingers. Good airflow goes a long way, so fume hoods end up on the wish list for every chemist. Proper gloves matter—a thin nitrile glove might hold up for a quick job but will break down with longer exposure. Safety goggles protect your sight from splashes. Companies that provide regular safety training and easy access to safety data sheets keep people prepared and help reduce accidents. Standards from organizations like OSHA push supervisors to set clear rules and make protective gear non-negotiable, not optional.
Accidental spills can harm water supplies and surrounding wildlife. Salicylaldehyde breaks down slowly outside, threatening streams and soil. Industry players must stick to responsible disposal—using chemical waste containers, not pouring leftovers down the drain. Smaller operations sometimes cut corners, but fines and public awareness campaigns push everyone to respect environmental safety.
Lab managers do better when they provide easy-to-read instructions and keep cleanup gear handy. For smaller companies, regular audits by outside safety professionals help spot oversights. Digital checklists and in-person drills keep the focus on best practices. On a larger scale, switching to less toxic substitutes works for some procedures. Finding alternatives means asking tough questions about supplier practices and finished product quality, but it gives peace of mind to everyone along the supply chain.
Salicylaldehyde doesn’t grab headlines like some molecules, but this aromatic compound packs a punch in chemistry circles. Anyone who remembers their high school experiments catching the unmistakable almond scent of benzaldehyde might notice some similarities here. Salicylaldehyde carries the formula C7H6O2. Basically, each molecule is made of seven carbon atoms, six hydrogens, and two oxygens. It looks like a benzene ring with an aldehyde and a hydroxyl group packed onto it. Chemists call that an “ortho” relationship because both groups share adjacent spots on the benzene ring. This layout changes the molecule’s reactivity compared to simpler aromatic aldehydes.
The presence of both an aldehyde and a hydroxyl group in salicylaldehyde gives it a split personality. That unique structure opens doors across several fields. In the lab, chemists reach for this molecule when they need to create ligands (the kinds of things that help stabilize metal atoms in coordination complexes). Its formula allows for easy condensation with amines, so it serves as a cornerstone for making Schiff bases. These are the kinds of materials that show up in everything from antibacterial agents to sensors.
In biochemistry, salicylaldehyde stands out for its role in the synthesis of natural products. You won’t find it on a pharmacy shelf, but the building blocks it helps create matter for medicine. Take the antibiotic family of salicylates—they draw lineage from the same ring structure. The formula C7H6O2 lets it react in ways that power up a whole host of discoveries.
Folks working in the flavor and fragrance business know salicylaldehyde by scent before they read about it. Even minor shifts in that molecular structure (just one atom moved over or swapped out) can take the smell from sweet to pungent, so industry pays close attention to its chemical fingerprint. This molecule plays well with solvents, dissolves easily in organic mixtures, and fits neatly into synthesis plans for flavor creation.
Research groups working with this compound keep safety at the top of the list. Salicylaldehyde doesn’t present the kind of risks that some aldehydes carry, but prolonged exposure isn’t smart either. Good ventilation, gloves, and goggles are musts. Every lab’s safety data sheet highlights how even small spills or inhalation can irritate the skin, eyes, or respiratory system. Industry experience teaches that even familiar substances demand respect and handling with care.
Synthesizing, storing, and using salicylaldehyde requires clear protocols. My colleagues have found routine labeling, proper sealing, and training go a long way. Investing in fume hoods improves air quality, which helps keep exposure to a minimum. Specialists in chemical logistics learn quickly that tracking inventory and regularly reviewing storage guidelines reduce accidents. Lessons learned over time: putting safety above speed wins every time.
The formula for salicylaldehyde—C7H6O2—may look simple, but the molecule’s value comes from what people do with it. Whether the goal is creating new ligands, fine-tuning a fragrance, or laying groundwork for next-gen antibiotics, understanding the formula means understanding opportunity. For those building careers in chemistry, respect for small details and safe practices makes all the difference in results.
Salicylaldehyde isn’t just another bottle on the chemistry shelf. Its strong almond-like smell gives early warning, but it hides real dangers. Touching it can irritate your skin or eyes. Its vapor finds its way into the air, and breathing too much can harm your lungs. Leaving it out leaves people at risk, especially anyone who doesn’t realize how hazardous a spill or stray vapor might be. I’ve seen what happens when someone ignores chemical safety; a moment of distraction left a colleague with a chemical burn. Salicylaldehyde isn’t as forgiving as some people expect.
Heat kicks off all sorts of trouble with this chemical. At higher temperatures, it gives off more vapor, which doesn’t just stink up the lab—they become a fire risk. Direct sunlight speeds up breakdown, and what’s left can turn dark and gunky. Everyone should keep salicylaldehyde in a cool spot, away from sunny windows and heating vents. Experience teaches that even a few degrees too warm can cause problems after months of storage.
Glass bottles with tight-fitting seals work best. The chemical’s fumes find the smallest cracks, so screw caps or Teflon-lined stoppers stay the norm. Avoid plastic containers. Salicylaldehyde can react with some plastics, and I’ve seen labels smudge and bottles turn soft after just a few months. That one shortcut tends to backfire, risking leaks or dangerous reactions that no one wants to clean up.
Salicylaldehyde reacts with oxygen over time. Leaving the bottle open, or half-sealed, builds up pressure or lets the chemical go bad. Not only does this make it less useful, but it ramps up the risk of inhaling vapors the next time someone opens it. Many seasoned chemists flush the bottle with nitrogen before closing it, though at the very least keep the cap tight between uses. I learned early on to double-check tightness, and every serious lab keeps backup seals handy.
This substance doesn’t play well with oxidizing agents. Store it near nitric acid or bleach and you’ve set the stage for a dangerous chemical reaction. In educational labs, color-coding shelves and putting clear labels on storage zones cuts confusion. Even in a busy setting, making it obvious where salicylaldehyde should go means fewer accidents and quick checks for everyone working late or hurried by deadlines.
Accidents happen, and cleanup should always include proper ventilation and gloves that can handle organic chemicals. Spill kits meant for solvents belong close by. After one close call involving a broken bottle, I never store anything volatile right at eye level or where someone can knock it over by mistake. Sturdy back shelves or designated cabinets prove their worth over time.
Treating salicylaldehyde with respect isn’t about following unnecessary rules. Every safe lab doubles down on these habits: closed bottles, cool dark storage, chemical-resistant labels, and clear shelf assignments. Sharing stories about mistakes means new lab members learn before they put themselves at risk. It’s not about fear—it’s about trust and responsibility for everyone working around these chemicals. Salicylaldehyde can be handled without worry when everyone takes care. In the end, safe storage protects us all.
Salicylaldehyde stands out in industrial labs for all the ways it unlocks new molecules. Chemists reach for it to build agents that block corrosion, tweak flavors, and design medicines. Anyone who's worked with organic synthesis knows salicylaldehyde often acts as a starting block. Most experienced researchers remember their first successful Schiff base synthesis, which happens as its aldehyde group reacts with amines. Take a walk in any chemical plant and you’ll find this compound fueling work in both classic and innovative reactions.
Color in textiles, plastics, and inks owes a debt to small molecules like salicylaldehyde. Industrial dye makers count on its reliability. Coupling salicylaldehyde with aromatic amines leads to deep yellow or orange shades, used for both strength and stability. Years of textile work have taught fabric engineers not to cut corners with the quality here—dyes built from this foundation resist fading far better than plenty of alternatives. It’s not just about color either; salicylaldehyde-based dyes hold on through tough laundry cycles and sun exposure, which saves manufacturers from constant warranty complaints.
Drug development stories often include a stop at salicylaldehyde. It’s inexpensive, reactive, and easy to tweak—making it indispensable for research teams. Some antifungal and antibacterial compounds start here, relying on its scaffold to fast-track early-stage candidates. The flavor and fragrance industries use it too, usually as an in-between step before moving on to more complex, pleasant-smelling molecules. My own stint working with medicinal chemists taught me that any shortcut which simplifies synthesis without extra cost gets a quick nod, and salicylaldehyde has certainly filled that role for decades.
Anyone in specialty materials or catalysis circles knows complexes of metals with salicylaldehyde show up everywhere. Scientists studying the behavior of nickel, cobalt, or copper analyze structure and reactivity, and salicylaldehyde ligands shape those outcomes. I remember visiting a lab where the team cranked out sensors and magnetic materials, using these complexes as anchors. Because these metal complexes prove both robust and customizable, manufacturers cut expenses and improve yields.
Salicylaldehyde finds another use fighting rust. Blend it into protective coatings, and pipelines or marine equipment last longer. As oil and gas operators battle salt spray, every edge matters. Engineers testing corrosion inhibitors have repeatedly chosen this compound for its ability to coat metal surfaces, adding years to expensive infrastructure. Experienced corrosion technicians note how small changes in inhibitor chemistry can tip the balance between early repairs and smooth sailing. Reliable outcomes in these environments build trust—anything that holds up during field trials earns respect quickly.
Environmental chemists rely on salicylaldehyde to trap and detect trace metals in water or air samples. Its sensitivity and selectivity matter. Surveyors in municipal water plants, in particular, praise its repeatability for routine tests. Across the field, lab techs stress how familiar reagents speed up training and avoid costly mistakes. Students entering analytical labs get hands-on experience using this compound to calibrate instruments. In all, seasoned professionals appreciate how salicylaldehyde’s reliability cuts troubleshooting time so they can focus on bigger challenges.
| Names | |
| Preferred IUPAC name | 2-hydroxybenzaldehyde |
| Other names |
2-Hydroxybenzaldehyde o-Hydroxybenzaldehyde Salicylal Aldehydoortho-cresol |
| Pronunciation | /ˌsælɪˈsɪl.æl.dɪˌhaɪd/ |
| Identifiers | |
| CAS Number | 90-02-8 |
| 3D model (JSmol) | `/data/mol/props/saldhyde/cid_8027.sdf` |
| Beilstein Reference | 1209221 |
| ChEBI | CHEBI:28241 |
| ChEMBL | CHEMBL1438 |
| ChemSpider | 505 |
| DrugBank | DB03899 |
| ECHA InfoCard | ECHA InfoCard: 100.003.166 |
| EC Number | 203-836-6 |
| Gmelin Reference | 82128 |
| KEGG | C01506 |
| MeSH | D010473 |
| PubChem CID | 6950 |
| RTECS number | VO5075000 |
| UNII | A2J09C4U8O |
| UN number | UN2810 |
| CompTox Dashboard (EPA) | `DTXSID9020706` |
| Properties | |
| Chemical formula | C7H6O2 |
| Molar mass | 122.12 g/mol |
| Appearance | Colorless to yellow liquid |
| Odor | Aromatic, almond-like |
| Density | 1.174 g/mL at 25 °C(lit.) |
| Solubility in water | Slightly soluble |
| log P | 1.65 |
| Vapor pressure | 0.042 mmHg (25°C) |
| Acidity (pKa) | 7.40 |
| Basicity (pKb) | 13.35 |
| Magnetic susceptibility (χ) | -41.5·10⁻⁶ cm³/mol |
| Refractive index (nD) | 1.589 |
| Viscosity | 2.07 mPa·s (20 °C) |
| Dipole moment | 1.94 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 160.6 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -69.5 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | -3071.8 kJ/mol |
| Pharmacology | |
| ATC code | D02AE14 |
| Hazards | |
| GHS labelling | GHS02, GHS07 |
| Pictograms | GHS07 |
| Signal word | Warning |
| Hazard statements | H302, H315, H319, H402 |
| Precautionary statements | P261, P280, P305+P351+P338, P337+P313 |
| NFPA 704 (fire diamond) | 2-2-0 |
| Flash point | 87 °C |
| Autoignition temperature | 165 °C |
| Explosive limits | Explosive limits: 1.1–8.4% |
| Lethal dose or concentration | LD50 oral rat 729 mg/kg |
| LD50 (median dose) | LD50 (median dose): 920 mg/kg (oral, rat) |
| NIOSH | SN 8525000 |
| PEL (Permissible) | PEL (Permissible Exposure Limit) of Salicylaldehyde: 5 ppm (25 mg/m³) |
| REL (Recommended) | 0.1 ppm |
| IDLH (Immediate danger) | 90 ppm |
| Related compounds | |
| Related compounds |
Salicyl alcohol Salicylic acid Aspirin Methyl salicylate |
