Digging Into Hexadecanethiol: More Than a Chemical Name
Historical Development
Hexadecanethiol's path through science stretches back well before the internet tossed chemical catalogs onto our screens. Synthetic chemists in the mid-20th century scrambled to build molecules piece by piece—making thiols, including hexadecanethiol, for quirky surface studies and building up the puzzle of organic reactions. Chemists started learning about self-assembled monolayers from the 1980s, when researchers realized these long-chain thiols would snap themselves in perfect formation over gold surfaces, just by dipping a metal plate in a solution. This ability to graft tight, ordered layers at the atomic level pulled surface chemistry out of the shadows. Those early experiments laid the groundwork for today's ultra-sensitive sensors and flexible electronics. Both basic and applied research in surface engineering, nanoelectronics, and nanomedicine built momentum thanks to what hexadecanethiol brought to the bench.
Product Overview
Hexadecanethiol sits in the camp of organosulfur compounds. Folks often spot it by the formula C16H34S. It’s made up of a sulfur atom connected to a sixteen-carbon straight chain saturated hydrocarbon—a pretty beefy tail, all things considered. Its popularity among scientists doesn’t come from bulk properties but from the way it grabs onto gold, forming a prim and proper monolayer. Labs buy it as a clear, slightly yellowish to colorless liquid, giving it an unassuming look. From electronics to surface coatings to sensors, its impact runs deeper than its slippery appearance suggests.
Physical & Chemical Properties
At room temperature, hexadecanethiol pours out as an oily liquid, turning waxy around 20-22°C. It flaunts a faint odor recognizable from other thiols—a sulfur note that lingers despite the long carbon tail. The molecule is not as volatile as shorter-chain thiols, mostly thanks to its extended chain. It doesn’t mix with water, but happily dissolves in organic solvents like chloroform, benzene, and hexane. With a boiling point tipping above 300°C, you don’t see this chemical vaporizing in a hurry. While it won’t catch fire too easily, it brings the flammability of an organic liquid and doesn’t play well with oxidizers. The sulfur atom acts as the anchor, binding tightly to gold and silver, which makes it ideal in nanotechnology and as a primer for further chemistry.
Technical Specifications & Labeling
Suppliers slap technical grades on this compound: purity above 97% usually, sometimes checking for metals like lead and copper at the parts-per-million level. Labels note the CAS number 2915-16-8, UN numbers for transport (packing it right matters, since it counts as hazardous goods by assorted regulators), and hazard pictograms calling out skin and eye irritation. Certificates include NMR, FTIR, and GC-MS analyses. Storage advice often lands on "keep cool, dry, sealed, and in the dark." You see expiration dates of one or two years. Reagent bottles spell it as hexadecanethiol, n-hexadecyl mercaptan, or 1-hexadecanethiol for searchability across labs and languages.
Preparation Method
Labs usually churn out hexadecanethiol in one of two ways. The first uses 1-bromohexadecane as a starting block, adding thiourea under reflux before hydrolyzing the adduct to free up the thiol group. Sometimes folks switch to hexadecanol, first converting it to a tosylate or mesylate, then swapping the group for sulfur through a reaction with sodium hydrosulfide or thioacetate. After some workup, including washes and distillation under reduced pressure, the product usually checks out by NMR and mass spectrometry for both purity and structure. The scale slides from grams in research settings up to kilograms for industrial batches, though the basics rarely change.
Chemical Reactions & Modifications
The thiol group on hexadecanethiol pulls plenty of attention from synthetic chemists. Oxidation transforms it into hexadecanedisulfide, which opens new avenues for surface chemistry and redox applications. Alkylation or acylation reactions protect the thiol or swap it for new functional groups. The long alkyl tail can undergo reactions that insert halogens, replace hydrogens, or even introduce double bonds, though such changes risk losing the molecule’s distinctive properties. At interfaces, the sulfur binds with gold atoms in a classic S-Au bond, fostering self-assembled monolayers often capped with terminal methyl groups. Researchers have found that by tweaking the thiol or adding secondary functional groups, they can adjust wettability, conductivity, or introduce click chemistry reactivity for surface patterning.
Synonyms & Product Names
Across catalogs and research papers, hexadecanethiol pops up under several names. Aside from its IUPAC name (1-hexadecanethiol), it goes by palmityl mercaptan, n-C16H33SH, and cetyl mercaptan. Each label points at the same 16-carbon chain, but some names highlight its origins in palm oil chemistry or its thiol identity. Chemical vendors often add catalog identifiers for ordering, but those official names shape searches across patents and academic literature alike.
Safety & Operational Standards
Handling hexadecanethiol involves standard precautions for organosulfur compounds and flammable liquids. Liquid spills demand prompt cleanup to limit inhalation or skin contact. Splashing it in eyes or on skin results in chemical burns or irritation, so gloves and goggles stay on the table. Fume hoods are a must, as repeated inhalation of vapors or accidental ingestion can have more serious effects. Waste disposal routes substances to hazardous waste streams, since even trace sulfur-containing chemicals can upset wastewater treatment and odor management. Training manuals direct researchers to avoid open flames and make sure storage containers remain sealed tightly to limit air and moisture exposure that degrade quality. Most accidents happen through carelessness, not chemical misbehavior, which is why regular drills and routine PPE checks play such a big role in keeping labs running smoothly.
Application Area
Hexadecanethiol lands on gold surfaces and transforms research in nanoscience. Self-assembled monolayers find their way into biosensors, lab-on-a-chip devices, and molecular electronics, where each molecule lines up by itself, creating a tidy, functional surface. Electronics firms use it as a molecular wire in tunneling junctions or single-electron transistors, making the most of its predictable structure. Analytical labs count on its non-polar surface for separating out complex chemical mixtures in chromatography. Its lubricating qualities ease friction in microelectromechanical systems (MEMS), protecting sensors and moving parts. Environmental chemists deploy its monolayers to study molecular interactions without the background noise from irregular surfaces. Even outside pure science, hexadecanethiol finds work as an odorant, corrosion inhibitor, and stabilizer in specialty products, making its niche unique in both everyday products and advanced tech.
Research & Development
Researchers worldwide chase ways to leverage the reliable assembly and modification potential of hexadecanethiol. Teams experiment with patterned surfaces, using photolithography or microcontact printing to control fluid flow or cell growth on a microscopic scale. Nanomedicine engineers couple therapeutic agents to these monolayers, hoping to target drugs more precisely or signal biological changes in real time. Analytical chemists stretch its use into sensors for viruses, pesticides, or toxins. Some collaborative projects cross into sustainable chemistry, modifying hexadecanethiol into greener analogs that degrade more easily, or borrow its backbone for biodegradable coatings. The sheer number of peer-reviewed articles, patents, and research grants that center around this compound underscores its utility and adaptability.
Toxicity Research
Toxicologists map out the effects of organosulfur compounds like hexadecanethiol with a practical mindset. Direct exposure causes skin and eye irritation, but the long chain dilutes volatility, limiting inhalation hazards compared to shorter-chain mercaptans. Chronic exposure questions linger since most workplaces don’t deal with large volumes day to day. Animal testing and cell assays document minimal acute toxicity at low concentrations. Environmental risk grows at industrial scales, where disposal practices matter, since thiol compounds can stress aquatic organisms. Regulatory agencies keep a close watch, setting exposure limits and requiring clear labeling. By enforcing waste management, personal protective equipment, and ventilation protocols, labs and factories keep both workers and ecosystems safer from the harsher side of sulfur chemistry.
Future Prospects
Interest in hexadecanethiol keeps growing as surface science becomes more central to electronics and health tech. Researchers tinker with analogs—adding fluorines or branching the carbon tail—to tune properties further. Microfluidics continues to expand, pushing the need for reliable coatings that guide liquids with pinpoint accuracy. 3D nanoprinting and single-molecule electronics seek molecules like hexadecanethiol for both patterning and as structural parts. With green chemistry gaining traction, producers investigate renewable feedstocks to cut down on the environmental impact of production. Even as new surface-active molecules arrive, the reliability and affordability of hexadecanethiol secure its place in the researcher’s toolkit, helping to build safer, smarter, and more responsive devices for the future.
What Makes Hexadecanethiol Stand Out?
Hexadecanethiol isn’t something most of us come across at the grocery store, but in the world of science and tech, it’s got a reputation. It’s a chain of carbon atoms—with one end capped off by sulfur—that holds a special place in labs working on new materials. The sulfur acts like a magnet for metals, and that’s the secret to why researchers use this stuff almost like glue to bond other molecules to surfaces.
Molecular Self-Assembly: The Building Blocks
A lot of material scientists I’ve met have delighted in showing off “self-assembled monolayers.” These single, ordered sheets only a molecule or two thick can change how a surface behaves. Gold is a favorite in the lab, and hexadecanethiol snaps right onto it. Drop a gold chip in a solution of the compound and the sulfur head goes for the metal, while the long tail floats away, forming a well-packed blanket.
Surface chemistry has a real impact in places like sensor development. Think of devices that can sniff out toxins at trace levels. These sensors depend on coatings that attract or repel only the right molecules, and hexadecanethiol’s ability to create predictable, customizable surfaces makes it a natural choice. It’s chemistry with a purpose.
Electronics and Miniaturization
We ask more from electronics every year, whether it’s fitting more memory onto a chip or creating circuits invisible to the naked eye. Lately, anyone serious about nanotechnology has heard stories from cleanrooms where the tiniest details matter. Hexadecanethiol has earned a permanent spot on that bench because it blocks unwanted reactions. Lab technicians treat gold circuits with the compound, so other chemicals only bond where they’re wanted. This sort of chemical masking helps shrink devices and push boundaries on what’s possible with circuit design.
Corrosion Barriers and Next-Gen Materials
Rust is every engineer’s headache. Hexadecanethiol’s waterproof tail helps clothes metal surfaces in a way that keeps water and air out—a big help for gold and even silver. Researchers at universities and commercial labs report fewer pinholes and longer metal lifespan with these coatings. While we don’t see these barriers on massive bridges or ships, the principle is the same: better coatings, longer life.
Safety and Handling
No one should treat laboratory chemicals lightly, and hexadecanethiol is no exception. It lends a faint, rotten odor, reminding you there’s sulfur in the mix. Protective gloves, good ventilation, and careful waste disposal make it safer for those working with it. Following safety protocols keeps the promise of these advanced materials without the headaches.
What Comes Next?
Every new generation of electronics or sensors rides on small breakthroughs, not just sparkling discoveries. Hexadecanethiol reminds me that progress often comes from finding the right building blocks, not just the flashiest tech. Scientists now look to tweak its molecular cousins to suit tougher tasks, like bioengineering and renewable energy. As research into greener chemistries grows, the stable, reliable standbys get a second look.
If there’s a lesson here, it’s that small tweaks—whether it’s a tiny molecule or a slight change in how we protect metals—can change what’s possible in science and industry. The world keeps moving, and sometimes the right compound for the job looks like a bottle of clear liquid on a lab shelf.
Chemistry in Everyday Life: What’s in a Name?
Hexadecanethiol sounds pretty complex, but its real chemical formula is straightforward: C16H34S. Sixteen carbon atoms, thirty-four hydrogens, one sulfur — that’s all it takes. Most people wouldn’t give a second thought to a molecule like this. Until you run across it in a lab or on a product label, hexadecanethiol barely registers. For scientists, tinkerers, or students, though, these simple chemical combinations shape everything from research outcomes to manufacturing advances.
Hexadecanethiol in Practice
At first glance, this compound might seem forgettable. I remember seeing it for the first time in a university research project on self-assembled monolayers. One tiny change to a carbon chain, toss a sulfur atom on the end, and you’ve got a substance with the power to change surface properties. Hexadecanethiol forms a neat one-molecule-thick layer on gold surfaces. That layer organizes itself without coaxing — nature loves regularity more than we do — and just that simple habit gives project teams a way to design water-repellent surfaces, biosensors, and electronic components at the tiniest scale.
How Does C16H34S Affect Industries?
Without hexadecanethiol, a bunch of modern electronics would lose their special coatings. It protects, it repels, it sticks in just the right way. Its value goes beyond laboratories. In my own experience, research on anti-corrosion coatings and specialty packaging often circles back to the same basic building blocks — compounds like hexadecanethiol. Gold electrodes, which play a big role in tiny sensors and circuits, need that organized self-assembling property to stay clean and stable.
Proper handling means fewer defects, longer shelf life, and quicker development of new technologies. No surprise, universities and companies have both published studies showing how this little chemical, by lining up just so on a gold surface, keeps expensive materials from breaking down. Without protection, gold electrodes attract all kinds of unwanted molecules from their environment. Just a hint of C16H34S makes a world of difference in consistency.
Safety, Handling, and Environmental Factors
The flip side? Wherever chemicals show up, risk tags along. Hexadecanethiol should always be treated with care. According to safety data, it can irritate the skin and lungs. Working in a research setting means implementing real safeguards — fume hoods, gloves, solid waste collection plans, not just for compliance but to keep work safe for everyone involved.
Disposal also deserves attention. Responsible laboratories look at environmental impact, not just process yield. I’ve seen strong moves in recent years toward greener chemistry, switching up solvents or reusing gold-coated substrates to minimize waste. Regulatory guidance suggests managing small-scale disposal through licensed facilities and never pouring it down the drain, for good reason.
The Bigger Picture: Why Getting the Formula Right Matters
Small molecules often have outsized impacts. C16H34S provides a bridge between base science and real-world products. For engineers, chemists, or students, remembering the chemical formula isn’t just about tests or trivia—it ties back to the exact way a substance works in the field: from waterproof gadgets to medical sensors. It pays to know your basics. Sometimes the plainest formulas bring about the most significant results.
Understanding Why Caution Matters With Hexadecanethiol
Hexadecanethiol pops up in many research labs, especially in work involving organic surfaces or nanotechnology. It might look like a regular chemical on a shelf, but this waxy powder carries hidden risks. Anyone in a university or industrial lab can recall stories about close calls—maybe a forgotten glove, a fume hood fan that stopped working, or a chemical splash no one ever expects until it happens. Those slip-ups can turn a routine day into a medical situation. That’s the reason for respecting every bottle with a yellow warning label, especially when you know its vapor can irritate the airways or its residue can leave your skin red and raw.
Personal Protective Equipment Makes a Difference
Splashy science videos online rarely show the basic gear, but real lab work means gloves, safety goggles, and a proper lab coat. If that sounds overcautious, consider the sharp smell Hexadecanethiol carries. Catch even a tiny whiff and you know it doesn’t belong in your body. Anyone who’s wrangled with it without gloves remembers the burn, and the odd, stubborn stink lingering for hours. Nitrile gloves hold up best after several tests; latex doesn’t last long, and no one wants to gamble with skin exposure.
Goggles that seal tightly work better than glasses. All it takes is one pipette mishap for droplets to splash. Regular coats cover sleeves, but chemical-resistant aprons go the extra mile in case of a bigger spill. Home laundering of lab coats or jackets only brings the risk back into your house, so sending them to a professional laundry keeps everyone safer—especially family or roommates.
Don’t Skip Ventilation or Engineering Controls
Working with volatile organosulfur compounds in an open room leads to headaches, coughing, or worse. The chemical’s boiling point means it won’t turn to vapor at room temperature, but in warm stirred reactions or heated setups, vapor drifts where you least expect. A fume hood, cleaned and checked every few months, traps airborne residues and blows them outside where nobody is breathing. My own lab keeps a chart near the hood—filters get checked off, airflow logs updated. It’s tedious, but seeing older colleagues coughing or rubbing their eyes during incidents drives the point home fast.
Clean-Up and Storage Aren’t Optional
Every handler who’s knocked over Hexadecanethiol on a busy bench knows the silent panic that follows. Absorbent pads, neutralizing agents like sodium bicarbonate, and waste bags on hand make all the difference. Quick spills stayed contained in local areas, but lazy cleanup turned small drops into sticky, hazardous patches others would later touch.
The storage shelf matters as much as the workspace. I remember one near-miss when two incompatible bottles stored together began to sweat and corrode. Keep containers tightly sealed, away from heat sources and grouped only with friendly chemicals. A separate, ventilated box—locked if undergraduates share the lab—keeps curious hands out and odors in.
Training and Smart Habits Save Trouble
Every new arrival welcomes safety briefings with eye-rolls, but I’ve seen how experienced technicians sprint for eyewashes or spill kits faster than juniors. Regular drills and check-ups catch dangerous shortcuts before they become accidents. Calling out unsafe habits in the moment—nicely—builds a culture that keeps accidents down.
No shortcut replaces solid habits. Slow down, wear the right gear, keep your space clear, and learn from every small mistake before it turns big. Hexadecanethiol won’t give a second chance if you get complacent. Laboratory work always demands respect, not fear, but nobody wants to become tomorrow’s safety training story.
Understanding the Needs for Purity
Hexadecanethiol shows up in labs and manufacturing settings that need tight control over chemical quality. Scientists and product engineers often demand purities above 95%. Modern suppliers recognize this, so most offer Hexadecanethiol with assay values around 96% to 98%. Some lab protocols and industry processes, like building self-assembled monolayers on gold substrates, push expectations even higher. During my own postgrad research, anything less than 97% led to headaches with irreproducible results or odd side reactions. Purity isn’t just a marketing number here—it defines whether a project reaches solid results or drifts into guesswork.
Usable purity also matters for specialty coatings and electronics work. Trace metals and other impurities can throw off surface chemistry. That’s probably why most reputable suppliers back up their numbers with certificates of analysis, and usually also list levels for sulfur, iron, and moisture. Some customers ask about 99% or higher material, especially in electronics or if the end product gets close regulatory scrutiny. Knowing exactly what sits in your flask helps pull down the risk of failed product batches, wasted time, or, even worse, outright dangerous reactions.
Packaging Realities in the Chemical World
Logistics play a bigger role in chemical work than most folks think. Hexadecanethiol comes as a waxy solid, so packaging must protect not just from leaks but from air, light, and sometimes even minor bumps or static. Labs usually pull this material from glass bottles—these tend to range from tiny 1-gram vials up to 100-gram containers. In my time at a smaller university lab, we dealt with 10-gram glass bottles. Larger-scale buyers, such as electronics manufacturers, can ask for 500-gram or even kilogram jars. Still, glass remains popular: it’s inert, it protects against accidental contamination, and it helps avoid reaction with the thiol itself.
Plastic isn’t usually the first choice for packing Hexadecanethiol, despite its popularity for other chemicals, since thiols give off persistent odors and can sometimes degrade plastics over time. Some suppliers line containers or wrap glass bottles in protective secondary bags to keep shipping handlers happy and labs smelling fresh.
Temperature control comes up, but mostly for long-term shelf life instead of urgent hazard. Most suppliers suggest storing at room temperature or slightly cooler, away from direct sunlight. In my own storage experiences, a dark cabinet with sturdy shelves worked just fine, but we made sure the lids sealed tight—a single spilled bottle could coat a room with sulfurous fumes that linger for weeks.
Buying Smart and Staying Safe
A purchase of Hexadecanethiol often links to specific needs. Academic groups go through grams per year, so they focus on smaller bottles and easy online ordering. Commercial outfits push for bulk buying discounts and sometimes custom packaging, driven by long production runs. Careful record keeping matters with thiols, both because of the cost and due to the handling risks. I always kept a log of open and close dates—one bad batch, or a mistaken substitution, could delay months of work.
Relying on trusted suppliers protects more than the experiment—it shields everyone in the lab from accidental exposure and project delays. Reliable sources not only confirm purity but will also respond to questions about recent lots, packaging changes, or even special needs like tamper-evident seals. For anyone involved in buying or storing this chemical, it pays to keep the focus on practical, safety-minded choices and look for vendors with a record of solid analytical support.
Recognizing What’s on the Shelf
Hexadecanethiol doesn’t show off with wild colors or dramatic warnings, but the chemical deserves real respect. Having spent years working alongside folks in university labs and small research outfits, I’ve seen what can go wrong with careless chemical storage. Our textbooks mention long-chain thiols give off a strong sulfur smell; the reality hits your nose hard once you open a bottle that sat too long in the wrong spot. A headache isn’t the worst risk—skin exposure can leave lasting irritation, and the compound’s volatility means simple mistakes could turn small spills into real hazards.
Keeping the Risk Low
Hexadecanethiol prefers a cold, dark home, away from direct light and far from oxidizing agents. Leaving a bottle out near window sills or next to bleach promises trouble. Temperature matters—a cool storeroom, preferably below 25°C, holds the line against premature degradation and smelly surprises. I’ve watched students shove bottles next to open reagent bins and then scramble once the air grew harsh. Fume cupboards make a safer temporary stop, but never a permanent one. The best safeguard comes from designated, labeled shelving: nobody wants to grab hexadecanethiol by accident, mistaking it for something friendlier.
Averting Contamination and Accidents
Glass containers, sealed with PTFE-lined caps, stop air and moisture from spoiling hexadecanethiol. Plastic stoppers soak up the smell, staining the material for months—best avoided. Vendors usually ship new bottles with secondary containment and careful labeling, but after opening, discipline drops. I’ve seen folks pour off just a bit, lost in conversation, and forget to replace the tight seal. Even a bit of exposure encourages oxidation; yellowing means it’s no longer fresh. Sticking to a “one bottle, one workbench” mindset cuts back on cross-contamination and keeps workspaces safe. If you’ve ever sifted through a fridge packed with solvents from previous years, you’ll know why clear separation helps everyone.
Wearing the Right Gear
No storage discussion stands alone without a nod to personal protection. Even quick handling means gloves—nitrile, not latex, thanks to the permeation risk. Eye protection stops accidental splashes, especially since hexadecanethiol sometimes surprises with a bit more volatility on warm days. I’ve seen someone learn this the hard way after a pipette mishap. Changing gloves and rinsing skin fast after any exposure keeps irritation down. Good habits with PPE and handwashing keep lab teams safer for the long haul.
Relying on Training, Not Guesswork
Proper storage depends less on fancy cabinets and more on well-trained hands. Someone who knows the difference between storing acids and thiols catches errors before they escalate. Experienced staff should always brief newcomers, reviewing storage hazards, proper labeling, and emergency procedures in plain language—no jargon. Regular audits help, too. Peer feedback points out lazy habits—like leaving caps loose or labels fading into unreadable smudges. These conversations may feel tedious, but they keep everyone alert and focused.
Seeking Support and Official Guidance
Real expertise draws on solid sources. Safety data sheets backed by regulatory bodies such as OSHA or the European Chemicals Agency don’t just tick boxes for compliance. Over the years, they’ve helped me write clear SOPs and lab manuals for teams looking after hundreds of chemicals. Honest respect for that guidance, followed by daily practice, solves most storage headaches before they start. The routine—store cold, keep containers closed, label every bottle, segregate from oxidizers—pays off with safer, smoother research days.
| Names | |
| Preferred IUPAC name | hexadecanethiol |
| Other names |
1-Hexadecanethiol
Cety mercaptan Cetylmercaptan n-Cetyl mercaptan n-Hexadecyl mercaptan n-Hexadecanethiol n-Cetylthiol Cetyl sulfide |
| Pronunciation | /ˌhɛk.səˌdiː.keɪnˈθaɪ.ɒl/ |
| Identifiers | |
| CAS Number | 29150-23-8 |
| 3D model (JSmol) | `3D model (JSmol)` string for **Hexadecanethiol**: ``` CCCCCCCCCCCCCCCCS ``` This is the **SMILES** string for Hexadecanethiol, usable in JSmol/3D viewers. |
| Beilstein Reference | 1209248 |
| ChEBI | CHEBI:35771 |
| ChEMBL | CHEMBL1546 |
| ChemSpider | 33217 |
| DrugBank | DB14096 |
| ECHA InfoCard | 100.239.773 |
| EC Number | 206-203-2 |
| Gmelin Reference | Gm: 26812 |
| KEGG | C01635 |
| MeSH | D006523 |
| PubChem CID | 7719 |
| RTECS number | MI8585000 |
| UNII | J4E8U5604U |
| UN number | UN3077 |
| CompTox Dashboard (EPA) | DTXSID9020702 |
| Properties | |
| Chemical formula | C16H34S |
| Molar mass | 270.54 g/mol |
| Appearance | Colorless to pale yellow liquid |
| Odor | mild mercaptan |
| Density | 0.845 g/mL |
| Solubility in water | Insoluble |
| log P | 6.93 |
| Vapor pressure | < 0.01 hPa (20 °C) |
| Acidity (pKa) | 10.6 |
| Basicity (pKb) | pKb ≈ 13.8 |
| Magnetic susceptibility (χ) | -73.0e-6 cm³/mol |
| Refractive index (nD) | 1.435 |
| Viscosity | 3.24 mPa·s (25 °C) |
| Dipole moment | 2.07 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 536.3 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -285.75 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | -10750.7 kJ/mol |
| Hazards | |
| GHS labelling | GHS02, GHS07, GHS08 |
| Pictograms | GHS06, GHS08 |
| Signal word | Warning |
| Hazard statements | H315, H319, H335 |
| Precautionary statements | P261, P273, P280, P305+P351+P338, P310 |
| Flash point | 113 °C |
| Autoignition temperature | 375 °C |
| Lethal dose or concentration | LD50 (oral, rat): 22,000 mg/kg |
| LD50 (median dose) | LD50 (median dose): Oral, rat: 16 g/kg |
| NIOSH | SN 7000000 |
| PEL (Permissible) | PEL (Permissible Exposure Limit) for Hexadecanethiol: Not established |
| REL (Recommended) | 24 months |
| Related compounds | |
| Related compounds |
Dodecanethiol
Octadecanethiol Hexadecanol Hexadecanoic acid |
