© 2026 Nanjing Finechem Holdings Co., Ltd,
All Right Reserved
Stories from chemistry often connect to small breakthroughs—Dichloromethane-d2 stands as one of those modest yet necessary products. Regular dichloromethane first surfaced in the mid-1800s. Chemists separated it out while producing chloroform, not realizing its future role. Later on, researchers improved purification and large-scale production methods, bringing dichloromethane from the bench to the refinery. The heavy-lifting came later for its deuterated cousin, Dichloromethane-d2. As nuclear magnetic resonance (NMR) grew in scientific labs, the demand for solvents containing deuterium increased. The need didn’t come from a quest for novelty—it rose out of experimentation and the search for clearer, more interpretable NMR signals. Progress here never looked flashy, but it delivered some of the groundwork for modern analytical chemistry.
Dichloromethane-d2 is, as the name implies, a version of dichloromethane where two hydrogen atoms swap with deuterium. On the surface, the difference looks slight, yet this detail drives its value in the lab. For anyone who has ever run NMR spectroscopy, solvents like these make the heavy math and machine work possible. With its relatively low cost compared to other deuterated solvents, it’s a favored choice for researchers working with non-polar compounds.
Take a bottle of dichloromethane-d2 and you’ll see a clear liquid—without a color or sediment, much like its non-deuterated form. It boils at a lower temperature than water, so it evaporates easily in open air. The introduction of deuterium bumps up its molecular weight slightly, which matters in specific measurements but not in the hands-on work of most chemists. It dissolves a wide range of organic molecules, which only broadens its reach in the laboratory setting. I’ve seen how well it handles non-polar and slightly polar compounds, much more forgiving than some other solvents.
Chemists measure the deuterium content carefully, often aiming for around 98% or higher purity. Any contamination by regular dichloromethane shows up as stray peaks on an NMR spectrum, so those handling this chemical check for purity regularly. Labeling covers details like molecular weight, purity, boiling and melting points, and isotopic enrichment. It’s not just about compliance—it keeps experimental results meaningful. Mistakes in purity may look small on paper but can scramble an entire set of research data.
Industrial chemists generally produce dichloromethane-d2 by taking ordinary dichloromethane and replacing hydrogen through chemical exchange with heavy water or deuterium gas, using catalysts and heat. The process isn’t particularly glamorous, but it requires strict controls—a little bit of regular hydrogen can spoil a batch. Those who’ve worked this process know it’s easy to lose product through evaporation or to introduce contaminants during purification.
Dichloromethane-d2 doesn’t just serve as a passive medium. It sometimes participates in minor reaction pathways where deuterium labeling becomes a useful tracer for mechanistic studies. Laboratories have used it to map out steps in organic reactions, letting researchers see just where certain atoms travel. Other times, it becomes the backbone for custom molecules in drug design or material science.
Dichloromethane-d2 goes by several names in catalogs and publications: Deutero-dichloromethane, Methylene chloride-d2, and DCM-d2 are all common. Some chemists prefer shorthand and call it “DCM-d2,” especially in lab logs. The various terms trip up newcomers, so clear documentation makes a real difference, especially when ordering for specific experiments.
Dichloromethane-d2 requires the same caution as regular dichloromethane. The solvent produces vapors that, in high concentrations or with extended exposure, damage the nervous system, liver, and other organs. Its volatility means spills quickly become an inhalation risk. Fume hoods, gloves, and protective goggles become non-negotiable parts of the setup. Safety data sheets warn about risks of narcotic effects, so labs keep exposure durations short and storage containers tightly sealed. Over the years, my experience confirms that investing in proper ventilation pays off more than almost any other precaution when handling solvents like these. Regulatory agencies continue to review exposure limits, trying to align laboratory practices with ongoing toxicity findings.
NMR spectroscopy remains the classic arena for dichloromethane-d2. The nearly invisible background deuterium provides a stable, non-interfering field for analyzing organic compounds. Medicinal chemists, material scientists, and anyone working on small molecule research benefit from its transparency at key frequencies. Its ability to dissolve tough or unusual molecules makes it a go-to choice not only for research but for quality control in the pharmaceutical and polymer industries. I’ve seen entire research teams struggle for weeks with less accommodating solvents, returning gratefully to dichloromethane-d2 for tough analytical runs.
Ongoing research into dichloromethane-d2 focuses on improving isotopic enrichment techniques and reducing production costs. Even small increases in isotope purity can yield much better spectral data, streamlining research and reducing the time spent on troubleshooting ambiguous signals. Innovations in green chemistry press for less hazardous methods of production and handling—efforts targeting both environmental and worker safety. Product development also pushes into broader NMR applications, especially with complex biological samples and emerging material classes.
Research into dichloromethane’s toxicity continues to keep occupational health specialists busy. Despite some focus on deuterated versions, the overwhelming body of evidence on health effects comes from regular dichloromethane—where chronic exposure shows clear links to cancer and neurological harm. Animal studies and human exposure stories both reinforce the push for lower workplace limits. Those who remember the more relaxed standards from decades past can see the benefits modern safety rules bring in protecting people working hands-on with solvents daily. Every incremental finding helps labs reexamine their practices, shape new policies, and inform safer choices for young students and technicians.
The path ahead for dichloromethane-d2 ties closely to the future of analytical chemistry and industry regulation. Demand tracks with the growth in chemical and pharmaceutical research, especially in fields focused on complex molecule synthesis. At the same time, environmental and workplace safety concerns drive calls for alternatives, greener synthesis, and stricter handling protocols. Some chemists consider a solvent-free future, yet for the present, substances like dichloromethane-d2 continue to anchor daily research. Expect steady improvements—higher purities, greener processes, and possibly new generations of isotopic solvents—driven by the same pragmatic curiosity that built the field from the start.
Step into any research lab specializing in chemical analysis, and sooner or later, you run into dichloromethane-d2. Chemists know this compound for what sets it apart: it’s a “deuterated” version of regular dichloromethane. Instead of regular hydrogen atoms, it carries deuterium, a heavier cousin. This small tweak catches the eye of researchers working with nuclear magnetic resonance (NMR) spectroscopy.
NMR spectroscopy lives and dies by signal clarity. Regular solvents confuse the readout with their own hydrogen atoms. Deuterated solvents like dichloromethane-d2 keep background noise low, giving researchers clean, precise peaks for the molecules they want to study. As a chemist, nothing’s as frustrating as losing hours to messy spectra. Clean signals mean fewer mistakes and more honest data.
Work with complex organic molecules, and you’ll see how troublesome proton-rich solvents can get. Even trace impurities creep into spectra, making confirmation or identification next to impossible. A bottle of deuterated dichloromethane solves many of those problems. Researchers trust it for carbon NMR and other studies because of its solvency power and low water content — both critical for accurate analysis.
Though NMR gets most of the press, dichloromethane-d2 earns its keep elsewhere. Synthetic chemists sometimes use it in kinetic studies to understand how reactions run in real time. The deuterium label helps them track atoms, figuring out which bonds break and what forms during obscure chemical transformations.
There’s a more practical angle as well. Ever tried to separate delicate compounds that fall apart in harsh solvents? Dichloromethane-d2’s mild properties handle unstable substances, offering a safety net where regular solvents can’t. Some pharmaceutical teams rely on it for method validation when they develop new drugs, especially those based on fragile scaffolds.
Every solvent brings baggage, and dichloromethane-d2 is no saint. While it doesn’t have the acute toxicity of some chemicals, long-term exposure still raises red flags. Breathing in too much vapor causes headaches and nausea. Labs need proper ventilation and safe handling practices. After years around lab benches, you come to appreciate a strong fume hood and cautious habits more than anything.
Waste disposal isn’t a minor detail, either. Analysts carefully segregate deuterated waste from regular solvents, since disposal firms treat deuterium-labeled material differently, often at extra expense. Neglecting proper storage and paperwork risks regulatory trouble, steep fines, or worse — environmental harm.
No one expects research to slow down, but green chemistry circles argue for more sustainable alternatives and better recycling programs. Companies offering dichloromethane-d2 have responded in small ways: selling in smaller lots, offering return programs for unused solvent, and supporting stricter quality barriers to minimize waste. Labs can push further by auditing use, swapping for less harmful solvents when possible, and encouraging researchers to justify every expensive milliliter.
Behind every vial sits a larger story about how science manages risk, innovation, and cost. Every small improvement counts when the stakes involve worker safety and environmental responsibility. For anyone on the front lines of chemical research, thoughtful choices about solvents like dichloromethane-d2 shape not just data quality, but workplace health and the planet’s future.
Dichloromethane-d2 carries the formula CD2Cl2. The swap from regular hydrogen atoms for deuterium makes a subtle change in its structure, sending its molecular weight to about 86.95 g/mol. For folks in research or industry, these numbers aren’t just trivia. Small details can decide if a chemical works for a job or if it sends the results off track.
Anyone who’s handled NMR spectroscopy in an organic lab knows why the d2 part matters. Deuterium doesn’t show up in proton NMR the way regular hydrogen does. Using solvents like Dichloromethane-d2 keeps solvent peaks out of the way, letting the signals from the compounds of interest stand out. Getting clean spectra can mean accurate conclusions—or a wild goose chase. A week spent puzzling over mystery peaks quickly drives home the importance of solvent labeling and careful tracking of molecular weights.
Chemists have worked out that each atom in the formula plays a role. Chlorine atoms (Cl) bring in more mass, but trade places with nothing between the regular and deuterated version. The difference rides on those two deuteriums, each a heavy sibling to hydrogen, bumping up the mass. That leap may feel small, but isotopic purity proves essential in experiments with tight tolerances. Even a small error in solvent identification can wreck a synthesis or send a project into delay.
Even outside academic labs, producers and suppliers keep molecular weight in sight for handling and safety data. Mislabeling or incorrect documentation has sparked costly recalls and sharpened the focus on traceability for every reagent. Focusing on specification isn’t just bureaucracy; it keeps customers, workers, and the public safe. In weighing, storing, and using Dichloromethane-d2, those numbers help avoid costly mistakes.
Factual slip-ups in chemical labeling aren’t rare. Someone in a hurry might confuse regular dichloromethane (CH2Cl2) with its deuterated cousin. This mix-up wrecks experimental results and sometimes safety protocols, as isotopic versions don’t always behave identically under every scenario. I once watched a team lose weeks of solid synthetic work after a mislabeled solvent crept into a key run, leaving them with muddy data and frustrated calls to the vendor.
Verified sources like quality-controlled safety sheets, reputable chemical catalogs, and peer-reviewed journal references keep these mistakes rare. Labs that double-check chemical data have far fewer setbacks than those that rely on memory, especially as projects get more complex and stakes rise.
Training plays a big role. New lab techs learn quickly that common names can trap the careless, especially when isomers or isotopes come into play. Investing a few minutes to cross-check a chemical’s formula, mass, and labeling can save days or weeks in the long run. Workflows built on double-checks help reduce risk, whether you’re making a drug, a plastic, or just acquiring reference-grade solvents for a busy university lab.
Chemistry rewards the careful and the curious. Knowing the chemical formula—CD2Cl2—and the weight—86.95 g/mol—for Dichloromethane-d2 isn’t just for exams. It protects people, projects, and reputations in an industry where a single missing deuterium can make all the difference.
Dichloromethane-d2, or deuterated dichloromethane, pops up everywhere in the world of analytical chemistry—especially in NMR labs. It’s volatile, has a low boiling point, and the fumes catch you off guard without proper ventilation. I’ve learned the hard way that a cracked cap means the entire room smells like sweet chloroform, making you wonder if your headache’s from the experiment or the chemicals themselves.
Keeping this solvent around means treating it with respect. Researchers have seen spills dissolve bench surfaces right in front of them. The liquid evaporates fast, but the fumes hang. The container demands a tight, chemical-resistant cap. Store that bottle in a flammable chemicals cabinet, not squeezed in next to inert powders. Fires aren’t common with dichloromethane-d2, but you don’t need extra fuel for a blaze if a spark ever starts.
Fume hoods exist for a reason, and solvents like dichloromethane-d2 prove it daily. Breathing in the vapors leads to nausea, dizziness, and enough long-term exposure can increase cancer risk. I’ve talked with colleagues who worked for years in poorly ventilated spaces; the health implications become clear only after the symptoms linger. The eyes and skin burn if you splash it around, so forget about skipping the gloves just to pipette “quickly.” Nitrile gloves hold up well for brief work, but splash goggles and a lab coat protect more than you think, especially during transfer.
Unlabeled bottles confuse even experienced techs. I always check, then double-check, that DCM-d2 sits nowhere near oxidizers like nitric acid or organic bases. Mixing accidents create more than just panic—they can mean toxic fumes or violent reactions. Color-coded storage makes cross-contamination less likely, and year after year, I see how standard operating procedures save more than just the experiment.
Dichloromethane-d2 soaks up moisture and air, working best when kept dry. Sealing the bottle every time preserves purity and keeps out water that spoils the deuterium signal during spectroscopy. Labs with dedicated desiccators extend solvent life and purity. Many big labs run regular checks on solvent stocks, pulling samples to ensure deuterium content stays within spec—nobody wants to re-run hundreds of spectra for one small mistake.
Elevating safety in chemical handling always comes down to waste disposal. I’ve seen waste streams get ruined by thoughtless pouring. Pouring dichloromethane-d2 down the drain contaminates water supplies. Collected solvent waste goes in halogenated waste cans, away from acids and even non-halogenated solvents. Local laws often treat it as hazardous, and for a good reason—one spill outside the hood drifts a long way and lingers.
Regular reviews of chemical hygiene plans keep people and the environment safer. My experience with audits teaches one lesson: prepare now, not after the accident. Training new staff goes beyond a checklist. Practical drills—such as spill response or fire extinguisher demos—stick with people and strengthen habits in the long run.
Labs can cut unnecessary risk by storing only what’s needed. Smaller bottles mean less exposure. Using clear labels, keeping inventory tight, and ensuring everyone knows the rules keeps labs running smoothly. Upgrading storage units, maintaining fume hoods, and rewarding good safety practices makes everyone’s day safer. Investing in personal protective equipment pays off, especially with solvents like dichloromethane-d2 that aren’t forgiving after a single mistake.
Choosing the right solvent for NMR spectroscopy shapes the reliability of the data, the clarity of spectra, and sometimes even the safety of the experimenter. As someone who has spent crowded afternoons over a humming NMR console, I’ve learned that the quirks of each solvent decide more than just peak positions—they influence cleanup, interpretation, and repeatability.
Dichloromethane-d2, also known as CD2Cl2, has built a following among NMR spectroscopists. Its modest boiling point and fair polarity free up chemists to dissolve a tougher class of organics—think esters, some non-polar aromatics, even pesky organometallics. Not every molecule wants to play nice with CDCl3 or DMSO-d6. Once or twice, trying to crack the NMR of a greasy intermediate, only CD2Cl2 delivered clean peaks and saved a precious sample from disappearing into a sticky mess.
Because it is deuterated, CD2Cl2 cuts down background peaks in both proton and carbon spectra. Spectra usually look uncluttered except for those solvent residual peaks at 5.32 ppm (1H) and 54.0 ppm (13C). If you know your spectra, these never throw a curveball.
Lab veterans, especially those who value their lungs and skin, treat dichloromethane with respect. Its volatility brings both benefits and headaches. In an open-topped NMR tube, even moderate warmth can drive off CD2Cl2, leaving samples dry or, worse, varying concentrations during data collection. I have lost irreplaceable product because a drafty lab sucked every drop out in minutes.
Toxicity isn’t just a buzzword here. Dichloromethane vapors numb the senses and, over long exposures, affect the nervous system. Labs investing in fume hoods and careful waste handling avoid health risks and legal trouble. There’s a safety learning curve: new researchers should know that quick work in a well-ventilated hood isn’t just smart, it is non-negotiable.
Another annoyance crops up with protic or water-loving analytes. CD2Cl2 mixes poorly with water. Even a hint of moisture throws off lock, shifts peaks, and muddles integration. Old stock bottles, slow-pouring colleagues, or humid air all play a part. Drying agents help, but every extra handling step exposes the solvent to air and potential contamination.
Chloroform-d (CDCl3) usually grabs center stage in proton NMR because of its compatibility and ease of use. People go back to CD2Cl2 for samples that fall apart, react, or fail to dissolve in CDCl3. DMSO-d6 offers an alternative for polar solutes but lingers forever in glassware and complicates cleanup.
Picking CD2Cl2 depends on a real need. For tricky solubility issues, consider blending it with another solvent, or start with micro-scale to limit losses if the sample evaporates. Always run blanks and check the dryness—throwing in a few milligrams of anhydrous sodium sulfate before filtering into the NMR tube has saved many experiments.
Researchers willing to pay attention to volatility, store chemicals right, and document their steps can avoid bad surprises. Training new lab members to treat CD2Cl2 as both a valuable tool and a chemical hazard builds confidence and keeps experiments on track. As with most things, no single answer fits every project. CD2Cl2 stays useful for those moments when nothing else works.
Folks who work in NMR labs or organic synthesis meet dichloromethane-d2 regularly. In my past, nobody asked for the deuterated stuff unless accuracy in measurements really counted. Every bottle reflects careful work—chasing both high purity and reliable deuterium enrichment. These technical details might sound dense, but they shape how confident researchers feel about their results. If you miss the mark, your solvent can introduce background noise, mess with integrations, and even throw off product characterizations. It isn’t just about buying a specialty chemical. Lab budgets ride on this, as do downstream results and publication-quality data.
Think of dichloromethane-d2 with purity at 99.8% or higher. At this level, you’re talking about a solvent where nearly everything except the core molecule gets stripped away. No surprise, most labs want to see GC data or trace impurity numbers in the certificate of analysis. Chlorinated solvents love to pick up water and acidic contaminants. Left unchecked, these tiny imperfections show up as irregular peaks in NMR spectra. One time, I tried to run a sample using off-brand dichloromethane-d2 and found strange signals at 5 ppm. Turns out, enough non-deuterated solvent slipped in to drown out the meaningful parts of the spectrum.
For chemists running syntheses with moisture- or acid-sensitive reagents, even a few trace impurities ruin an entire batch. That’s not just a minor inconvenience—it costs time, money, and sometimes a whole day of experiments. Reliable purity in dichloromethane-d2 isn’t just about high-tech performance—it’s basic risk management for reproducible research.
Deuterium enrichment is where the magic happens. Dichloromethane-d2, with deuterium substituted for the usual hydrogen, turns up heavily in proton NMR applications. Suppliers aim for isotopic enrichment around 99.5 atom percent or above. If this slips, signals from ordinary hydrogen swamp the baseline, and you lose the clean silence a deuterated solvent provides. From my own experience, cutting corners here leads to muddled spectra and repeated experiments. The best suppliers publish detailed deuterium content, often verified by mass spectrometry. They’re proud of those numbers for a reason—they keep research on solid ground.
In pharmaceutical quality control or precise organic synthesis, high deuterium content wins every time. Even 1% ordinary hydrogen in the bottle leaves behind enough unwanted background. Modern chemistry relies on accurate, unambiguous data. Knowing your solvent’s isotopic footprint means you see the full picture, not a distorted one.
Labs can dodge these problems by checking supplier specs and audit trails before ordering. I’ve learned the hard way: always request batch-specific COAs, and don’t shy away from running a quick NMR check on new bottles. Some groups pool resources to buy from sources with robust quality assurance. This pays off in unmistakable baseline clarity and rarely wasted effort. Researchers should talk to their vendors—ask for impurity chromatograms and hard data on isotopic purity. If they hedge, keep walking. Good science depends on solid materials, and dichloromethane-d2 with full specs stands as a foundation for reliable research. No shortcuts work here; just careful, data-driven choices.
| Names | |
| Preferred IUPAC name | Dideuteriomethylene dichloride |
| Other names |
Methylene chloride-d2 Deuterated dichloromethane DCM-d2 Methylenchlorid-d2 |
| Pronunciation | /daɪˌklɔːr.oʊˈmɛθ.eɪn diː tuː/ |
| Identifiers | |
| CAS Number | 1665-00-5 |
| 3D model (JSmol) | `C[Cl][Cl]` |
| Beilstein Reference | 1361047 |
| ChEBI | CHEBI:85355 |
| ChEMBL | CHEMBL3305737 |
| ChemSpider | 121412 |
| DrugBank | DB14055 |
| ECHA InfoCard | 13b009af-d48f-4982-b6f1-a2b038ad37fe |
| EC Number | 200-838-9 |
| Gmelin Reference | 2035 |
| KEGG | C14422 |
| MeSH | Dichloromethane-d2 MeSH: D017225 |
| PubChem CID | 156522 |
| RTECS number | PA8050000 |
| UNII | Q9W3KD65TG |
| UN number | 1593 |
| Properties | |
| Chemical formula | DCl2D2 |
| Molar mass | 86.950 |
| Appearance | Colorless liquid |
| Odor | Sweet, chloroform-like |
| Density | 1.324 g/mL at 25 °C (lit.) |
| Solubility in water | 13.2 g/100 mL (20 °C) |
| log P | 1.25 |
| Vapor pressure | 47 kPa (20 °C) |
| Acidity (pKa) | NA |
| Magnetic susceptibility (χ) | −9.59 × 10⁻⁷ |
| Refractive index (nD) | 1.424 |
| Viscosity | 0.437 cP (25 °C) |
| Dipole moment | 1.60 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 172.1 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | –99.7 kJ·mol⁻¹ |
| Std enthalpy of combustion (ΔcH⦵298) | -503.6 kJ/mol |
| Pharmacology | |
| ATC code | D08AX |
| Hazards | |
| Main hazards | Harmful if inhaled. Causes skin and eye irritation. Suspected of causing cancer. |
| GHS labelling | GHS02, GHS07 |
| Pictograms | GHS07 |
| Signal word | Warning |
| Hazard statements | H315, H319, H332, H351 |
| Precautionary statements | P210, P280, P305+P351+P338, P304+P340, P312, P403+P233 |
| NFPA 704 (fire diamond) | 1-1-0 |
| Flash point | Closed cup: 62°C (144°F) |
| Autoignition temperature | 556 °C |
| Explosive limits | Explosive limits: 12-19% |
| Lethal dose or concentration | LD50 Oral - rat - 1,600 mg/kg |
| LD50 (median dose) | 1600 mg/kg (Rat) |
| NIOSH | KL3850000 |
| PEL (Permissible) | 50 ppm |
| REL (Recommended) | 25 ppm |
| IDLH (Immediate danger) | IDLH: 2,000 ppm |
| Related compounds | |
| Related compounds |
Chloroform-d Bromodichloromethane Carbon tetrachloride Chlorodifluoromethane Dichloromethane |
