Chemistry textbooks in the 1970s began shining a light on N-Hexadecyltrichlorosilane, known to many as HDS or C16H33SiCl3, though its story started earlier in labs focusing on unusual surface treatments. By the late twentieth century, researchers in materials science grew curious about ways to control the wetting properties of surfaces, and this molecule—with its brainy design featuring a long hydrocarbon tail and reactive trichlorosilane head—offered a one-step ticket to new interface possibilities. Laboratories from Tokyo to Berlin contributed recipes and tweaks, sparking a trail of journal articles charting its growing reach across semiconductors, biosensors, and anti-fouling coatings. The early fascination with its ability to form organized monolayers at the molecular level turned into serious business across electronics, biotechnology, and even naval engineering.
N-Hexadecyltrichlorosilane stands out as a clear, colorless to faintly yellow, pungent liquid. Pour it into a beaker and the smell alone makes an impression, thanks to its silane backbone. Its C16 hydrocarbon chain gives the substance plenty of physical heft, keeping it oily even as the trichlorosilane group races to react with anything bearing a hydroxyl group—like glass or metal oxide. Drop a few microliters on a cleaned silicon wafer, and you can watch it do its magic, lining up molecules into tight rows one layer deep, banishing water with its waxy tail. Years in the lab have shown this isn't just chemistry showing off. It delivers self-assembled monolayers (SAMs) that cut down on corrosion, resist fingerprints, and provide new test beds for nanotechnology schemes.
Eyeing the technical sheet, N-Hexadecyltrichlorosilane weighs in at 367.0 g/mol, boiling around 110°C at 2 mmHg, while it settles on a melting point near -4°C. Its density hovers close to 0.92 g/cm³ at 25°C, making it heavy enough to distinguish from simple hydrocarbons. The trichlorosilane group reacts rapidly with moisture, atmospheric or otherwise, instantly generating heat and hydrochloric acid. This high reactivity to water requires clever dry handling, but it's exactly what makes the molecule stick so well to surfaces, creating Si-O bonds that last. Under an FTIR microscope, fingerprints from the Si–C and C–H stretches read loud and clear, confirming formation of those sturdy monolayers, whether under test conditions or on real-world devices.
Commercial N-Hexadecyltrichlorosilane generally ships in glass bottles, with purity scores above 95%. Most vendors insist on low-temperature storage, out of sunlight, with argon or nitrogen to fend off hydrolysis. Labels display hazard codes, pictograms covering corrosive and flammable risks, and guidance on appropriate disposal. Each lot carries batch data, expiration, and sometimes spectroscopic scans for those who like to check authenticity. Storage near water is strongly discouraged—one errant splash can turn expensive stock to a hazardous gunk in seconds. For researchers, only a glimpse at a tiny barcode gets them from shipment to the bench, where the molecule’s behavior shapes the next step in an experiment.
Lab synthesis takes a classic organosilicon route: powered by chlorinating agents like thionyl chloride, hexadecanol transforms into N-Hexadecyltrichlorosilane in a dry, inert atmosphere. Nosing around this reaction calls for careful control, since wafting clouds of HCl evolve at the slightest trace of moisture. Commercial producers rely on large-scale glassware, vacuum lines, and specialized distillation columns to pull pure product from a tangle of byproducts. Strict exclusion of water extends to shipping and storage, so the bottle that lands in a lab comes ready for use in ultra-dry conditions where scientists hope to form their best monolayers.
A scientist will find N-Hexadecyltrichlorosilane leaps eagerly into reactions with just a hint of exposed surface hydroxyls. Place a clean silicon wafer or a bit of oxidized aluminum in a vapor-phase chamber, add a hint of HDS under vacuum, and immediately, the molecule forms a Si-O-Si bond, swinging its long tail outward—building order where chaos ruled before. Chemists use the reaction’s speed to their advantage, covering everything from medical sensors to microelectronic chips with tightly controlled molecular layers. Over the years, tweaks in humidity, deposition time, and even surface primer choice allowed for ever-finer tailoring of the SAM structure. Further modifications—adding reactive groups at the far end, swapping carbon chain lengths—open up applications in electronics, diagnostics, biosensors, and microfluidic devices.
N-Hexadecyltrichlorosilane also pops up on shipping lists and chemical catalogs under names like HDS, 1-Hexadecyltrichlorosilane, Trichloro(hexadecyl)silane, and C16 SiCl3. Cas numbers, such as 5894-60-0, help avoid confusion as a batch moves from supplier to customer. Over time, these naming conventions became essential for compliance departments, who rely on product data sheets and safety references to ensure the right bottle lands on each bench—spare no room for confusion with similar silanes lurking nearby, given overlapping hazards but wildly different effects at the molecular level.
A moment spent scanning material safety data sheets shows that N-Hexadecyltrichlorosilane commands real respect in the lab. It corrodes skin, eyes, and mucous membranes on contact, while its vapors singe the nose and lungs. It breaks down into hydrochloric acid on exposure to humidity, making glove boxes, fume hoods, and tight protocols a non-negotiable part of any experiment. Safety goggles, gloves resistant to organosilanes, and disposable lab coats make the difference between a smooth day at the bench and a call to the medical unit. For waste, the rule is simple: containerize and neutralize with care, as dumping into a regular drain can spell environmental headache. With strict labeling, waste handling, and technician training, facilities around the world turn a dangerous reagent into a manageable research partner.
N-Hexadecyltrichlorosilane fixes problems wherever surface interactions need changing. Engineers on semiconductor lines turn to it for building hydrophobic barriers, controlling residue, and supporting lithographic patterns. Biomedical teams use its monolayers to repel proteins from sensor chips, slash background noise in DNA microarrays, and ensure only the right molecules stick to diagnostic devices. It’s a favorite for research on anti-fog lenses, optical switches, and nanoelectromechanical systems, where one thin molecular coat makes a world of difference to device behavior. Researchers interested in the future of corrosion resistance, anti-fouling ship hulls, and low-friction surfaces pull from the same silane, relying on its proven record for consistency and ease of application—once the setup accounts for its handling needs.
Demand for better biosensors, smarter electronics, and more durable coatings drives fresh investment in N-Hexadecyltrichlorosilane research. Labs test new gradients of hydrophobicity by blending it with silanes of different chain lengths, building sophisticated micro-patterns for emerging microfluidic tools. Some teams engineer hybrid surfaces that can sprint between water-loving and water-hating states with the flip of a switch, exploring ways to reduce maintenance or boost sensitivity. As imaging technology improves, scientists map the arrangement and packing density of HDS-derived monolayers at the nanoscale, tuning recipes that once felt like black magic into repeatable workflows. Through this relentless cycle—from chemical plant to publication—innovation pushes boundaries, offering industries new options for performance problems that seemed beyond solution only a decade ago.
Handling and disposal of N-Hexadecyltrichlorosilane raise questions not just about worker safety, but also longer-term exposure and environmental release. Animal studies show that, thanks to its rapid hydrolysis, direct environmental persistence is low, yet acute exposure brings risk for severe eye and skin damage, respiratory irritation, and—in the worst case—chemical burns. Regulatory agencies watch for improper waste disposal, noting that breakdown products can acidify waterways or disrupt waste treatment systems. Efforts from the chemical industry and academic labs focus on refining handling procedures, providing training, and designing containment for accidental spills. Ongoing research explores safer derivatives and greener application methods to lower risk across the product’s life cycle.
Imagination drives new ideas for N-Hexadecyltrichlorosilane in both science and industry. As electronics shrink to nanoscales, this molecule’s knack for laying down predictable layers grows only more useful. Researchers consider responsive coatings, medical implants, and reusable microfluidics as next frontiers, blending molecular chemistry with electronics and biology for results that seemed outlandish only a decade ago. With concerns over sustainability, green chemistry teams remix the synthesis and recovery of HDS, aiming to cut hazardous byproducts and set safer benchmarks for widespread use. A future where self-healing surfaces, ever-smarter biosensors, and energy-efficient coatings become routine owes a nod to the careful work already done with this once obscure, now essential molecule.
Walk into a research lab working on surfaces and coatings, and you might spot a bottle labeled “N-Hexadecyltrichlorosilane,” or HDS for short. To someone in chemistry or material science, HDS spells reliability. Its long carbon tail and reactive trichlorosilane head give it special powers on glass, metals, and silicon. My own time in a university nanofabrication facility taught me this chemical’s role in one core task—making surfaces that shed water, dirt, and sometimes even proteins, like a raincoat shields you from the elements.
N-Hexadecyltrichlorosilane bonds to surfaces like glass and silicon wafers in a way that looks invisible, but it transforms their behavior. Drop water on a treated surface and rather than soaking in, the water forms a bead and then slides away at the slightest tilt. The transformation, called “hydrophobic modification,” matters for microelectronics, sensors, lab-on-a-chip devices, and scientific experiments focused on making tiny things. I remember researchers carefully cleaning silicon chips, laying them flat in a closed container, then placing a drop of HDS nearby; the chips emerge an hour later with a layer just one molecule thick.
Engineers often use HDS as a “mold release agent.” Picture tiny features etched into metal molds for advanced plastics or flexible electronics. Uncoated, these molds can stick and destroy both the product and the mold itself. With a coating of HDS, parts pop free cleanly. I’ve seen this approach speed up production lines in university spin-off companies working on microfluidic devices, cutting both costs and frustration.
The magic of HDS comes from “self-assembled monolayers.” Each molecule floats down and sticks headfirst to the surface, covering it with a tightly packed forest of hydrocarbon chains. This self-organization leads to a surface with new chemical properties. Labs use these monolayers to protect delicate electronics or to prevent unwanted reactions in experiments. I’ve worked with scientists who spent hours optimizing this layer for DNA chips, because a good monolayer stops stray molecules from sticking, cutting down noise in crucial medical tests.
Coating surfaces with HDS also helps in the world of micro- and nanotechnology, where friction between tiny moving parts can cause catastrophic failures. Think of miniaturized machines, or the storage tips in atomic force microscopes. A surface covered in HDS feels slicker, so these parts move smoothly. Less friction leads to devices that work longer, more reliably, and without as much heat buildup.
N-Hexadecyltrichlorosilane comes with some caveats. It reacts violently with water, belching out hydrochloric acid fumes and heat. Anyone using it needs strong fume hoods, protective gloves, and respect for the rules that keep labs safe. I became a stickler for safety from day one, after seeing what even a small spill can do.
Scientists keep pushing the envelope, finding ways to combine HDS with other chemicals to tune how surfaces interact with the world. Most progress in nanotech, sensors, and even next-generation diagnostics will build on humble molecules like HDS that let us control surfaces at the atomic scale. The search for chemical solutions can’t ignore safety, of course. Teams now focus on greener handling procedures, and companies look for substitutes whenever possible, but for now, HDS remains a staple in the toolkit for anyone shaping the future at the smallest scales.
N-Hexadecyltrichlorosilane carries the formula C16H33SiCl3. Each part of that formula tells a story. The hexadecyl group brings a long hydrocarbon chain. On the other end, three chlorine atoms attach to silicon. This simple arrangement packs a powerful punch in the lab and in industry.
Ask anyone who's spent hours in a surface science lab—N-Hexadecyltrichlorosilane shows up again and again. It doesn’t act flashy. The molecule’s real calling card comes from the way it reacts with surfaces. If you’ve ever tried to create a self-assembled monolayer on glass or silicon, chances are this is your go-to reagent. The combination of the long carbon tail and the trichlorosilane group lets it anchor to surfaces and present a smooth, dense layer. That kind of coating can keep surfaces from soaking up water, shift the way proteins interact with glass, and even change the friction between two materials.
I worked with this molecule during grad school, using it to build water-repellent slides that would stay clean for weeks. The process came down to a simple dip and rinse. Afterward, the surface transformed—the once-grabby glass sheet felt slick and smooth. That’s direct, hands-on chemistry making a real difference. Such hydrophobic surfaces don’t just help scientists; they matter in real-world tech. Cell phone screens, lab chips, and even solar panels stay cleaner and last longer when they’re covered in coatings based on molecules like this.
N-Hexadecyltrichlorosilane’s popularity doesn’t excuse carelessness. Open a bottle and a biting, sharp smell hits you right away. The trichlorosilane group reacts with water—including the moisture in your skin, eyes, and lungs. That reaction releases hydrochloric acid. From my own experience, accidents in the fume hood cause disasters quickly. Long sleeves, gloves, and good ventilation make a huge difference. Companies that manufacture and ship this molecule have detailed safety instructions. It’s smart to study those before pouring a single drop.
It’s clear this molecule unlocks all sorts of advances. But new research keeps pushing for safer, less toxic alternatives. Scientists keep testing other silanes that don’t throw off corrosive byproducts. They also work to design processes that use less solvent and create less hazardous waste. There’s real momentum behind the push for better handling and greener surface technologies.
It’s easy to get lost in a chemical structure, but the real world impact goes much deeper. The way N-Hexadecyltrichlorosilane changes a surface shapes everything from science labs to consumer goods. By paying close attention to safety and exploring alternatives, research can keep improving both performance and health outcomes. This straightforward molecule offers a strong case for the value of chemical know-how mixed with practical focus.
N-Hexadecyltrichlorosilane’s reputation mostly comes from its role as a silanization agent in labs and industry. While those shiny laboratory results draw a lot of attention, the tough side of this substance appears in storage rooms and chemical cabinets. This colorless, oily liquid reacts quickly with water and release hydrochloric acid—a very unpleasant surprise for anyone unprepared.
This isn’t theory. In my early days in chemical research, I walked into a storeroom on a humid day and saw the consequences of a single forgotten bottle of silane: corrosive vapors, a rusting shelf, and some fairly nervous colleagues. A chemical like this deserves more than just clear labeling; it requires respect for its reactivity and the right equipment for proper storage.
Keeping things dry isn’t just about comfort. Even a trace of moisture inside or around the container can trigger a slow reaction—one drop at a time. The use of tightly sealed, reliable glass containers lined with Teflon or similar inert material reduces exposure to atmospheric humidity. Plastic containers often can’t stand up to the chemical action here; only glass or special alloys offer long-term peace of mind.
Temperature creates its own hazards. Store this silane at room temperature, ideally between 15 to 25°C (59 to 77°F). Storage near heat sources opens the door for vapor formation, pushing up pressure within the container or even causing a leak. Many labs believe a refrigerator or climate-controlled cabinet is overkill—until somebody forgets to close a window in midsummer, and the bottle starts to weep.
N-Hexadecyltrichlorosilane belongs nowhere near acids, bases, or moisture. Mixing incompatible substances feeds disaster. Separate shelves and dedicated cabinets make sense, and good facilities get specific: a sturdy metal cabinet designed for flammables or reactives, lined with chemical-resistant trays, stands firm against accidental spills or drips.
You never spot leaks with your eyes closed. Regular inspections—yes, an old-school checklist—makes all the difference. Replace any stained or battered bottles. Familiarity here never breeds contempt; it keeps everyone safer.
Ventilation forms a hidden but crucial layer of defense. Even tightly capped containers can leak small amounts of vapor over time. Chemical cabinets with vented systems pull those fumes away. Room air shouldn’t carry the tang of hydrochloric acid or harsh solvents. If it does, the storage system needs immediate attention.
It’s easy to drop into routine: glance at the MSDS, check the label, and move on. But real understanding comes with hands-on, human-centered safety training. Staff need regular refreshers on chemical reactions, emergency procedures, and the signs of trouble. In my experience, one quick group demonstration with a water-sensitive chemical fixes memories far longer than a thick safety manual ever could.
Every chemical tells a story about risk and reward. N-Hexadecyltrichlorosilane’s story only ends well for organizations that put people, equipment, and habits ahead of shortcuts. In a world hungry for innovation, neglecting safe storage isn’t simply careless—it risks research, reputations, and lives.
N-Hexadecyltrichlorosilane gets plenty of attention in labs because of its ability to modify surfaces and build self-assembled monolayers. Despite these handy properties, anyone using it needs to take safety seriously. N-Hexadecyltrichlorosilane won’t back down easily; it reacts quickly with moisture and produces hydrochloric acid fumes, which sting eyes and burn lungs. Pink eyes, red skin, or sore throats don’t belong in the lab.
Anyone who’s worked with potent chemicals knows one accidental splash lingers in the memory. Routine use of nitrile gloves reduces the risk of skin contact. Latex can degrade, so nitrile stands up better. Chemical splash goggles and a face shield do the heavy lifting for your eyes and lungs. Even a whiff or a tiny splash can spark an emergency. Always remove contaminated clothing and wash skin thoroughly at the safety shower if contact occurs.
Strong fumes sneak out quickly. Fume hoods aren’t just expensive furniture—they’re your real insurance policy. Work with the sash down low; keep as little of your body inside as possible. Never rely on regular room ventilation to clear out acid vapor. Fume hoods keep air fresh and push hazardous vapors away fast.
N-Hexadecyltrichlorosilane reacts strongly with water, even tiny amounts in the air. Mixing the chemical with wet containers or pipettes won’t just ruin your experiment. It could trigger a release of corrosive acid gas. Keep tools dry and only open bottles in the lowest possible humidity.
Keep bottles tightly sealed and clearly labeled. Use a secondary containment tray so a spill stays in one spot, not all over shelves or the floor. Store away from anything containing water—including acids or alcohols that throw off water during reactions. Separate storage areas for incompatible chemicals reduce accidents. Place containers somewhere cool and ventilated, away from direct sunlight and busy walkways.
Spills deserve careful attention, no matter their size. Use dry sand or a chemical spill kit to absorb any liquid—never grab a wet rag or paper towel. Afterward, bag up waste materials and label them for hazardous waste disposal. Regular lab trash won’t cut it. Washing hands before leaving the work area, even after glove use, becomes a habit quickly.
Nobody expects accidents until they happen. Knowing the shortest route to the eyewash station and safety shower is as important as remembering which bottle to use. Tell others what you’re working with, especially if you break out the silanes. Team awareness gives everyone time to react if things go wrong.
Review safety data sheets before every new chemical, and take warnings seriously. The World Health Organization and OSHA offer guidelines that bring practices up to standard. Reading recent studies helps spot updates and lessons from others. Collective experience keeps chemicals from becoming new hazards.
N-Hexadecyltrichlorosilane grabs attention in nanofabrication, surface treatment, and electronics due to its silane group and hydrophobic tail. Labs across the globe use this compound to create self-assembled monolayers or to modify surfaces for experiments where water resistance and controlled interactions matter. Smooth performance hinges on how this silane interacts with the rest of the recipe, especially solvents. The question of compatibility isn’t just technical—it shapes the quality of final results and can make or break a protocol.
Most scientists I know try to dissolve or suspend N-Hexadecyltrichlorosilane in easy-to-handle organic solvents. Good results often come from dry, anhydrous solvents like toluene, hexane, or chloroform. These choices steer clear of the reactivity headaches you can run into with water. The silane part, with its three reactive chlorines, loves to go after water—if there's any, you get hydrolysis. That’s bad news. Instead of smooth deposition, those surface layers turn rough, and you end up with clumps or gels instead of clean, flat coatings. The surface loses the qualities you worked so hard to build.
I’ve seen mistakes where someone used ethanol, hoping for better safety or handling. Ethanol works for some surface applications, but the water content in standard ethanol causes the same headaches as water itself. You end up with a cloudy solution and a “snowstorm” on your substrate. Often, new students think any solvent marked 'organic' will work. The reality is, unless you check the dryness and purity, you risk confusing results and wasted money.
Labs need to keep N-Hexadecyltrichlorosilane away from humid air. This isn’t about being perfectionist—it might look clear in a bottle, but atmospheric moisture sneaks in and triggers slow changes. You open the bottle a month later, and it just doesn’t behave the way it did last time. That means storing unopened bottles in cool, dry places and prepping solvents only right before use. If you work in a place where budget is tight and waste adds up, small missteps grow into big costs over time.
The field races to find safer and more reliable ways to handle silanes like this. Some groups try solvent-free deposition, but those methods don’t match the fine control you find with traditional solvents. The push toward “greener” chemistry pushes people to experiment with less hazardous solvents, but drying agents and careful workflows keep popping up as necessary steps. Even with improvements in surface chemistry, most people I talk to won’t risk skipping the effort it takes to keep things airtight and anhydrous.
If you want repeatable surface coatings, don’t cut corners on solvent choice and handling. Each experiment teaches how these small details make a difference, not just in data but in safety and cost. People who work hands-on with N-Hexadecyltrichlorosilane get to know its quirks the hard way—those lessons shape every future protocol.
| Names | |
| Preferred IUPAC name | N-hexadecyltrichlorosilane |
| Other names |
Hexadecyltrichlorosilane Trichloro(hexadecyl)silane Trichlor(hexadecyl)silane n-Hexadecyltrichlorosilane C16H33SiCl3 |
| Pronunciation | /ɛn hɛk.səˈdiː.sɪl traɪˌklɔːr.əˈsɪ.leɪn/ |
| Identifiers | |
| CAS Number | 5894-60-0 |
| Beilstein Reference | 1368949 |
| ChEBI | CHEBI:87757 |
| ChEMBL | CHEMBL1616559 |
| ChemSpider | 109786 |
| DrugBank | DB14506 |
| ECHA InfoCard | 100.164.993 |
| EC Number | 208-807-6 |
| Gmelin Reference | 78491 |
| KEGG | C19275 |
| MeSH | D017568 |
| PubChem CID | 3034265 |
| RTECS number | TP2110000 |
| UNII | QDD242B5BK |
| UN number | UN2810 |
| CompTox Dashboard (EPA) | DTXSID3058936 |
| Properties | |
| Chemical formula | C16H35Cl3Si |
| Molar mass | 389.00 g/mol |
| Appearance | Colorless to pale yellow liquid |
| Odor | Odorless |
| Density | 0.905 g/mL at 25 °C |
| Solubility in water | Insoluble |
| log P | 6.1 |
| Vapor pressure | 0.01 mmHg (25 °C) |
| Acidity (pKa) | ~10.5 |
| Basicity (pKb) | -3.3 |
| Magnetic susceptibility (χ) | -82.0e-6 cm³/mol |
| Refractive index (nD) | 1.450 |
| Viscosity | 3.84 mPa·s (25 °C) |
| Dipole moment | 2.33 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 817.9 J·mol⁻¹·K⁻¹ |
| Hazards | |
| Main hazards | Causes severe skin burns and eye damage. Reacts violently with water. |
| GHS labelling | GHS02, GHS05, GHS07, GHS08 |
| Pictograms | GHS05,GHS07,GHS08 |
| Signal word | Danger |
| Hazard statements | H314, H410, H301, H331 |
| Precautionary statements | P261, P264, P271, P273, P280, P301+P330+P331, P303+P361+P353, P304+P340, P305+P351+P338, P312, P321, P330, P363, P391, P403+P233, P501 |
| NFPA 704 (fire diamond) | 2-1-0-W |
| Flash point | > 110 °C |
| LD50 (median dose) | LD50 (median dose): Oral, rat = 2450 mg/kg |
| NIOSH | TT4025000 |
| PEL (Permissible) | Not established |
| REL (Recommended) | 0.5 mg/m³ |
| IDLH (Immediate danger) | Not established |
| Related compounds | |
| Related compounds |
Trichlorooctadecylsilane Trimethylchlorosilane Octadecyltrichlorosilane n-Octyltrichlorosilane Octyltrichlorosilane Dimethyldichlorosilane |
