Copper compounds always catch the attention of scientists with their vibrant colors and wide-reaching chemistry. By the early 1980s, researchers began noticing the unique way copper behaves with proline-based ligands. Out of this investigation rose Bis(5-Oxo-L-Prolinato-N1,O2)Copper—a complex that took center stage in biochemical and coordination chemistry journals. Early studies explored its peculiar stability, and as research moved forward, universities cataloged detailed syntheses, reactivity, and potential biological applications. This molecule grew out of the classic trend of combining amino acid derivatives with transition metals, setting off a new era of research connecting metalloproteins, enzyme modeling, and pharmaceutical candidates.
Bis(5-Oxo-L-Prolinato-N1,O2)Copper doesn’t just appear as another lab curiosity. As a crystalline compound, it offers a striking blue-green shade, a feature that's echoed by many copper(II) complexes. Chemists value it for consistent yields and strong purity profiles, making it a staple whenever metal-mediated amino acid studies pop up. Academics, researchers, and industrial chemists have turned to this substance when developing catalytic systems or screening for biomimetic properties. This molecule bridges classic organometallic work with real-world applications by offering a unique approach to copper-amino acid chemistry.
This complex usually presents itself as a fine crystalline powder. Its vibrant color comes from d-d electronic transitions unique to copper(II) complexes, especially those coordinated to nitrogen and oxygen centers. It dissolves in water, giving a clear solution that hints at strong coordination in the dissolved state. Melting points generally land above 200°C, with decomposition marking the transition, consistent with its rigid chelate ring structure. One of the key features—a chelation pocket involving nitrogen and oxygen from the prolinato ligand—keeps the copper center tightly held, holding back easy hydrolysis in neutral or mildly acidic conditions. Magnetism studies reveal a typical low-spin d9 copper(II) signal, tracked through paramagnetic susceptibility. Chemists have noted the substance’s strong stability in storage, resisting slow oxidation or reduction by the atmosphere better than simpler copper(II) salts.
Labs order this material with strict labeling referencing the correct IUPAC and trade names. Most reputable suppliers note the hydrated or anhydrous state, as this affects weight percent calculations in reactions. Typical shipments arrive in glass bottles, often capped with inert gas and tamper-proof seals. Full chemical analysis comes standard, including copper content by atomic absorption, ligand confirmation via NMR and IR, and elemental analysis to confirm purity. Proper MSDS sheets go with every shipment, following GHS (Globally Harmonized System) guidance. Chemists look for batch numbers, expiration dates, and storage recommendations: usually below 25°C, protected from light and moisture.
Synthesis usually starts with copper(II) acetate or sulfate and a stoichiometric amount of L-5-oxoproline in water. By adjusting pH to mildly alkaline with sodium hydroxide, the ligand exchanges places with simple anions around the copper. Blue-green crystals fall from solution as water evaporates or as the mixture cools in an ice bath. Once filtered, several rapid ethanol washes strip away excess ligand or salt. Drying under vacuum gives the pure bis-complex. Many chemists add a recrystallization step using water/ethanol or water/acetone, sharpening both purity and appearance. Each step demands tight control: even small deviations invite unwanted side-products or impure material. Experienced hands check IR to confirm the chelation, usually observing shifts in the C=O region and strong bands for copper–oxygen and copper–nitrogen bonds.
Bis(5-Oxo-L-Prolinato-N1,O2)Copper doesn’t sit idle in a glass bottle. Strong acids break up the complex, freeing the copper into solution and regenerating the ligand. Reducing agents, like ascorbic acid or dithionite, move copper to the +1 state and trigger ligand loss. Organic chemists learn that gentle heating with chelators—EDTA or similar—pulls copper out, creating an empty ligand solution. The complex endures mild oxidants, sometimes forming dimeric species or mixed valence pairs. Ligand swaps happen under carefully chosen pH conditions; other amino acids and peptides can nudge out prolinato and install new frameworks around the copper core. This flexibility makes the complex a starting point for building more elaborate copper-containing structures in the lab.
Chemical supply houses and journals catalog this material under a raft of names: Bis(5-oxo-L-prolinato-N1,O2)copper(II), Copper(II) 5-oxo-L-prolinate, and even Copper pyrrolidonecarboxylate. CAS numbers help, creating a universal handle for searches and procurement. Trade names for broader use, such as “Copper PCA complex,” sometimes crop up in cosmetic or health product catalogs. Any researcher buying or reading about this compound should cross-verify names and numbers to confirm they’re getting the right structure.
Copper(II) complexes bring moderate risk. Any lab worker weighing out this substance uses gloves, goggles, and standard bench protection. Dust inhalation causes mucous membrane irritation, and accidental ingestion triggers nausea and gastrointestinal upset based on copper’s known toxicity. Regulatory frameworks, including OSHA and those guiding academic labs, require proper fume hoods when handling any copper salts at scale. Spill kits, copper-binding agents, and first aid procedures remain close by during synthesis or disposal. Disposal protocols call for chelation and collection as hazardous waste, sending the final material for metal recovery or secure incineration. Chemists must keep the compound stored tightly closed, well-labeled, and away from strong acids or reducing agents to avoid dangerous reactions and accidental release.
This copper complex claims a strong position in catalysis. Academic teams use it to model the way copper binds in enzymes like superoxide dismutase and lysyl oxidase. In certain reactions—especially in organic transformations involving oxidation—it serves as a test bed for selective oxidations. Dermatological and cosmetic scientists screen it for copper delivery in topical formulations meant to bolster skin structure or fight microbes. In agricultural research, copper–amino acid complexes get attention for micronutrient delivery and crop health. Polymer and materials researchers add it to new composites, testing for improved antibacterial surfaces or electrical conductivity. Although more common in academic circles, patents describe its use in new materials aimed at everything from drug carriers to anti-tumor research.
Research into Bis(5-Oxo-L-Prolinato-N1,O2)Copper crisscrosses many fields. Medically, teams work to harness its easy copper release for targeted drug delivery. Synthesis chemists study analogues with substitutions at key points on the prolinato ring, aiming to fine-tune solubility or reactivity. Physicists look at its magnetic and electronic structure, hoping to push forward molecular magnet technology or nanoscale sensors. Environmental scientists have started to use similar complexes as models for copper cycling in soils and watersheds. Newer startups, often based near major universities, search for ways to add this copper-ligand chemistry into medical imaging or slow-release agricultural formulas.
Copper itself helps the body in trace amounts but leads to toxic effects with high exposure. Animal studies show that this complex, like other copper(II) salts, builds up if administered in large doses. Animal livers and kidneys accumulate copper, leading over time to classic symptoms: jaundice, neural damage, even organ failure at the extreme. Cell studies underline how the complex breaks down under physiological conditions, steadily releasing free copper ions. At low doses, typical of cosmetic or supplement levels, effects stay mild; animal models show only transient increases in copper levels. The molecule’s decomposition in biological fluids happens faster under acidic or reducing conditions, matching the way copper compounds degrade in tissues. Most reviews urge careful, limited use, especially in products touching food chains or used in long-term therapies.
Interest in this complex keeps growing as more labs push toward biomimetic catalysts and copper-based medicines. Molecular engineers chase smarter ways to pair copper with bioactive ligands, hoping to generate new drugs for cancer or bacterial infections. Cosmetic chemists hunt for gentler copper delivery systems that avoid the toxicity of old-fashioned salts. Green chemistry research lines up this complex against conventional copper catalysts, judging efficiency, recyclability, and environmental fate. Data from smart sensors and wearables drive a new round of studies—can this family of complexes serve as the copper-sensing core for next-generation diagnostic tools? Researchers set out to solve ways to limit toxicity while squeezing maximum performance from the copper-ligand bond. With this much cross-disciplinary action, Bis(5-Oxo-L-Prolinato-N1,O2)Copper’s story probably only just began.
Ask anyone who’s spent enough time in a chemical lab, and you’ll find Bis(5-Oxo-L-Prolinato-N1,O2)Copper isn’t just sitting around because its name sounds impressive. Its value comes from what it brings to the table in real-world applications. For those working in coordination chemistry, this compound gives a solid entry point for studying how copper behaves when paired with organic molecules. You’ve got copper, an essential trace element in both nature and industry, and pairing it up with proline-based ligands lets scientists mimic certain biological processes or create new catalytic reactions.
Copper complexes have a history of showing up in catalytic chemistry. A lot of reactions that help make medicines, plastics, and specialty chemicals rely on catalysts that speed things up while keeping waste lower. Bis(5-Oxo-L-Prolinato-N1,O2)Copper fits the bill for testing new catalytic cycles. My own experience comes from helping an academic group screen copper complexes for turning alcohols into valuable chemicals—a process needed in many modern drug syntheses. This compound stood out for its stability and the level of control it offered during these experiments. Robust, with decent electron flow, it lets researchers tune how fast and cleanly a reaction goes. Its proline-derived ligand doesn’t just anchor the copper; it also allows the compound to dissolve easily in solvents that scientists actually want to work with, which is a big practical plus.
Copper is everywhere in living things. Proteins that depend on copper atoms (think enzymes that help you breathe or fight off microbes) rely on a fine-tuned dance between metal and amino acid. Bis(5-Oxo-L-Prolinato-N1,O2)Copper acts like a stand-in for more complicated biological systems. By creating simplified versions of copper centers, scientists can watch what happens in a test tube and make sense of reactions that are otherwise buried inside a living cell. In some of the university research I’ve seen, this compound helped shed light on how copper cycles between different oxidation states. These studies lead to better-designed drugs that target diseases at the molecular level or create new treatment strategies.
Not every chemist focuses on reactions. Some spend their days figuring out how molecules come together and hold their shape. Bis(5-Oxo-L-Prolinato-N1,O2)Copper, with its reliable geometry, proves useful for teaching and research. Students can actually crystallize it out of a flask and study the exact positions of atoms under a high-power X-ray, connecting textbook diagrams to tangible results. Clear, reproducible structures go a long way in training new scientists and cross-checking theory with real-world evidence.
Interest in cleaner and more efficient processes grows each year. The demand for metal complexes like this one keeps rising, especially in industries trying to shrink their environmental footprint. By investing in green chemistry and making catalysts that work with minimal waste, researchers set the stage for safer products downstream—whether it’s drugs or specialty materials. Better funding for interdisciplinary projects connecting university labs and industry makes sense, so ideas move out of journals and into production lines. In my experience, hands-on collaboration drives real progress. Bis(5-Oxo-L-Prolinato-N1,O2)Copper, despite its tongue-twister name, marks one small but crucial step toward building smarter chemistry for the future.
Bis(5-Oxo-L-Prolinato-N1,O2)Copper stands out in coordination chemistry for its interesting structural design. Its molecular formula is C10H12CuN2O6. This covers two molecules of 5-oxo-L-proline acting as ligands, and one copper ion at the center. The ligands, derived from an amino acid, each hook onto the copper by their nitrogen and an oxygen from their carboxylate groups. Anyone with lab experience knows it’s these atomic-level connections that shape how a molecule behaves in the real world.
Picture a copper ion caught up in a square-planar or distorted octahedral cage. Each 5-oxo-L-prolinato ligand wraps around, grabbing the copper with its nitrogen and carboxylate oxygen like a pincer. The rest of the ligand forms a pyrrolidine ring, which doesn’t just sit back – it helps stabilize the whole compound through resonance and spatial arrangement. Over years in a university lab, I’ve seen coordination compounds like these display striking stability, sometimes coloring a solution deep blue or green.
The N1,O2 notation simply highlights which atoms tie into the copper – nitrogen from position 1 and oxygen from position 2. This pattern isn’t random; it’s popular among chelating agents for a reason. Ligands that chelate (claw onto) the central metal this way limit unwanted side reactions and enable greater selectivity in biological and catalytic processes. Biochemists echo this concept every day, since copper complexes help mimic enzyme sites right down to the atomic arrangement.
Copper complexes have pulled plenty of attention in medicine and material science. Bis(5-Oxo-L-Prolinato-N1,O2)Copper isn’t just a pretty chemical formula. Its structure grants unique antioxidant and catalytic properties. For example, some analogues help neutralize free radicals, which underpin cell damage and aging. In practical research, copper-ligand complexes often turn up as critical players in studying enzyme models or designing new drugs.
With copper at the center, these complexes sometimes act a bit like natural copper proteins. These are the same proteins that shuttle electrons or bind to oxygen in living systems. This resemblance opens the door to using Bis(5-Oxo-L-Prolinato-N1,O2)Copper as a biomimetic catalyst, meaning you can mimic natural processes in an artificial setting. Researchers keep digging deeper to see how changes in the ligand’s structure affect what the copper center can do, hoping to unlock better activity and safer performance.
Despite all these promising angles, issues still pop up. Synthesis requires clean, controlled conditions, and copper complexes sometimes lose stability in the body’s water-rich environment. Industries that depend on these complexes face significant hurdles in scaling up lab results to something market-ready. I’ve watched more than one batch go sideways during pilot tests because the structure lost integrity or just didn’t perform the way smaller-scale samples did.
Pushing past these sticking points, chemists now experiment with ligand tweaks – swapping groups on the ligand ring, for example, or partnering copper with different coordination setups. Fresh synthesis pathways draw from green chemistry principles, trimming waste and energy use. A closer look at how the body handles these molecules will also help, especially for folks interested in medical applications. Getting these complex molecules into clinical use demands that stability, reactivity, and low toxicity all come together.
The core truth is, advances in understanding and manipulating Bis(5-Oxo-L-Prolinato-N1,O2)Copper’s structure could power up a range of applications from medicine to sustainable chemistry. The key isn’t just finding new complexes but really digging into how every piece of the molecule’s structure affects the whole system.
Bis(5-Oxo-L-Prolinato-N1,O2)Copper sounds technical, but at its core, it's a copper compound used in certain industrial and research settings. Talking to former lab techs and chemistry students, it becomes clear that being comfortable around such chemicals doesn’t mean ignoring their risks. I’ve spent years working with a wide range of materials in university and industry labs. Every time a new compound crossed my bench, I checked its safety data. This sort of vigilance builds healthy habits and reduces avoidable mistakes.
Chemicals that involve copper aren’t new in manufacturing, agriculture, and even medicine. Think about copper sulfate—found in fungicides and root killers. Still, each compound behaves differently and brings unique hazards, so lumping them together misses the mark. Bis(5-Oxo-L-Prolinato-N1,O2)Copper uses ligands from proline, a natural amino acid, to bind copper. The twist here is that biological resemblance makes some folks think there’s less danger. That’s a risky assumption.
Copper itself can become toxic, especially through chronic exposure. It’s essential for human health, but even a trace element turns problematic if levels climb. Occupational exposure can lead to respiratory irritation, skin issues, and long-term organ effects. The European Chemicals Agency lists copper compounds as hazardous to aquatic life and potentially irritating to humans if mishandled. Proline-based ligands aren’t known for high toxicity on their own, but attaching them to metals shifts the equation. Not enough studies have tracked this specific compound in living systems, which leaves a gray area for its true risk.
Reports from research organizations usually err on the side of caution. In practice, people in labs treat unknown copper complexes like potential irritants or toxins. Protective gloves and eye shields became my everyday tools, not just for emergencies. Breathing in powders, dust, or fumes often triggers headaches or worse. If spills happened on skin or benches, cleaning up right away avoided future headaches—literal and bureaucratic. Even tiny dust particles could create an inhalation hazard, especially during weighing or transfer. A shared story in the lab involved a small copper compound spill that corroded the metal edge of a balance. Imagine what that might do inside your lungs or bloodstream if absorbed day after day.
Relying on old assumptions for new materials can backfire. Chemistry suppliers and manufacturers should provide clear, up-to-date hazard data for these compounds. I’ve found that some safety data sheets lag behind actual lab findings, especially for rare or custom chemicals. Following guidance from OSHA, EPA, and accredited chemical safety boards protects workers and the public. Frequent reviews and labeling updates when new data emerges keep everyone in the loop.
At the bench, education makes the biggest impact. Students and new hires often learn by doing—but training around handling, spills, and disposal cuts down on incidents. Good ventilation stands out as a practical investment. Secure storage, proper labeling, and access to spill containment supplies help, too. Environmental impact deserves attention. Drains and trash aren’t the place for copper complexes. Special waste containers and licensed disposal partners keep copper out of waterways and soil.
Staying informed, asking the right questions, and following proven safety steps matter. Bis(5-Oxo-L-Prolinato-N1,O2)Copper may not be a household name, but treating it with respect makes sure it stays out of tomorrow’s headlines. Industry and academia have more work ahead to track and limit the risks of specialty chemicals like this one.
Bis(5-Oxo-L-Prolinato-N1,O2)Copper belongs to a class of coordination complexes used in chemical laboratories and research settings. Like many chemical compounds involving copper, mishandling can invite health and environmental risks. From my time working in academic labs, respecting substances like this means putting safety first, not only for personal health but also for colleagues and the environment.
Encountering Bis(5-Oxo-L-Prolinato-N1,O2)Copper in a lab brings up two key concerns: stability and containment. The compound’s unique molecular structure doesn’t thrive under high humidity, bright light, or heat. Keeping it in tightly sealed amber glass bottles shields it from these threats. I learned early that moisture in the air wreaks havoc on many copper complexes, leading to degradation and loss of intended properties. A locked, dry, and cool storage cabinet acts as the best line of defense. Most chemical storerooms use label-friendly shelving and segregate copper-based compounds from acids and strong bases. These steps prevent accidental reactions, which could threaten both the chemical’s purity and worker safety.
Direct contact means personal exposure. I remember a colleague who ignored gloves for a “quick transfer” and landed with a mild skin reaction. Standard lab gloves—think nitrile or neoprene—not only protect skin, but also allow for a solid grip if hands happen to sweat. Safety goggles block corrosive dust or splashes from reaching the eyes. Dust masks or respirators minimize inhalation risk, especially if you’re weighing out the powder form. The habit of consulting the Safety Data Sheet (SDS) before handling anything unfamiliar paid off in several tight spots for me; with substances like this one, it also means knowing emergency procedures in case a spill occurs.
If Bis(5-Oxo-L-Prolinato-N1,O2)Copper spills, avoid ever sweeping or compressing dust into the air. Wetting down the spill slightly and using a chemical-resistant scoop and dustpan keeps dust from spreading. Waste—no matter how small the amount—belongs in a sealed, properly marked hazardous waste bin. Many labs forget about environmental impact, so I always urge team members to log waste disposal and verify pickup schedules. Dumping even trace copper compounds into the drain can pollute water sources and draw regulatory penalties.
No one plans on accidents. Routine training pays off when something does go wrong. From years working in both industry and university labs, people who drill emergency eyewash and spill response procedures react with calm efficiency. Having a clear SOP posted in the chemical storage and prep areas minimizes confusion. If dry powder gets airborne or someone is exposed, the standard steps—flush eyes or skin with clean water, move to fresh air, seek medical help promptly—should be second nature to anyone allowed to handle the material.
Bis(5-Oxo-L-Prolinato-N1,O2)Copper isn’t a compound to fear, but it demands respect. Strict storage, well-maintained PPE, proper training, and a culture of safety keep risk low and let researchers focus on results, not recovery. Anyone unsure about protocol owes it to themselves and others to ask, double-check, and never cut corners with storage or handling.
Tracking down Bis(5-Oxo-L-Prolinato-N1,O2)Copper can feel like hunting for a needle in a haystack. This isn’t something you pick up at a local hardware shop or even most commercial chemical suppliers. The structure alone—copper bound within a prolinate framework—means it has a niche in research and specialty labs rather than everyday industry.
Trusted chemical suppliers such as Sigma-Aldrich, Alfa Aesar, and TCI America carry a wide range of specialty chemicals, but not every compound makes it onto their shelves. Often, research chemicals like this one are only available through specialized distributors or direct custom synthesis houses. Partners like ChemSpider, MolPort, and eMolecules let you check inventory across multiple vendors in one place. I’ve had more luck finding rare compounds by contacting chemists’ networks or looking up research paper references—sometimes you get the best leads this way.
Price tags for rare copper complexes rarely show up online. From personal experience, prices swing sharply due to factors like synthesis difficulty, purity, and packaging size. Custom orders, especially for complex organometallics, can run into hundreds of dollars per gram. Back in 2022, a similar copper-amino acid complex cost our lab nearly $650 for a five-gram vial, with extra for express shipping and hazardous materials handling. Lab budgets often groan at figures like these, but access and compliance beat price for critical research.
Sharper regulations now govern chemical sales. Suppliers in the US, EU, and parts of Asia ask for end-use statements and proof of lab credentials before they process an order. Knock-off sellers sometimes offer cheap chemical products, often lacking certification or documentation. In one nasty incident, a research group thought they’d struck gold with a bargain sample, only to find out via NMR that it was half the expected compound and half random contamination. A good supplier gives you a full Certificate of Analysis and a Material Safety Data Sheet, letting you know you’re getting the real deal.
If you can’t spot Bis(5-Oxo-L-Prolinato-N1,O2)Copper on major catalogs, custom synthesis firms might step in. Expect long lead times—often three to six weeks—and plenty of paperwork. We once worked with a mid-sized outfit in India, but had to clear customs, address import taxes, and get hazardous approval from campus EH&S. This complicates things for smaller labs or for international buyers, turning a quick purchase into a months-long ordeal.
Lab work doesn’t grind to a halt just for want of a rare compound, but a single catalyst can prove crucial to certain syntheses or mechanistic studies. Students and early-career researchers often hustle to pool orders, seek grant support, or even synthesize intermediates on-site where it’s safe and legal. Funding aside, the key lesson here goes beyond price: know your supplier, check the paperwork, and don't hesitate to ask for product validation. These steps take time, but every chemist knows the headache of a batch gone wrong or results lost to an off-target reagent.
| Names | |
| Preferred IUPAC name | Bis[(2S)-1,2-dihydro-5-oxo-2H-pyrrole-2-carboxylato-κ²N¹,O²]copper(II) |
| Other names |
Copper(II) bis(5-oxo-L-prolinate) Copper(II) pyrrolidonecarboxylate Copper(II) (L-pyroglutamate)2 Copper(II) bis(pyrrolidonecarboxylate) Copper(II) bis(5-oxo-L-prolinato) |
| Pronunciation | /ˈbɪs.faɪvˈɒk.səʊ ɛl prəˈlɪnəˌteɪt.oʊ ˈkʌp.ər/ |
| Identifiers | |
| CAS Number | [14708-67-9] |
| Beilstein Reference | 3558211 |
| ChEBI | CHEBI:52715 |
| ChEMBL | CHEMBL595881 |
| ChemSpider | 121981 |
| DrugBank | DB14298 |
| ECHA InfoCard | 03b14a7d-6687-4c7c-83e4-de0ee25c2fe4 |
| EC Number | 249-859-7 |
| Gmelin Reference | Gmelin Reference: 314070 |
| KEGG | C18457 |
| MeSH | D017174 |
| PubChem CID | 94277 |
| RTECS number | GL9825000 |
| UNII | X17IW84023 |
| UN number | UN3077 |
| CompTox Dashboard (EPA) | DTXSID1048576 |
| Properties | |
| Chemical formula | C10H12CuN2O6 |
| Molar mass | 358.85 g/mol |
| Appearance | Blue powder |
| Odor | Odorless |
| Density | 1.98 g/cm3 |
| Solubility in water | Insoluble in water |
| log P | -2.3 |
| Acidity (pKa) | 8.02 |
| Basicity (pKb) | 11.9 |
| Magnetic susceptibility (χ) | 1.38×10⁻³ cm³/mol |
| Refractive index (nD) | 1.670 |
| Dipole moment | 1.4927 Debye |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 232.6 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -839.5 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | -1273.9 kJ/mol |
| Pharmacology | |
| ATC code | V03AX31 |
| Hazards | |
| Main hazards | Harmful if swallowed. Causes serious eye irritation. Causes skin irritation. May cause respiratory irritation. |
| GHS labelling | GHS07, GHS09 |
| Pictograms | GHS05,GHS07,GHS09 |
| Signal word | Warning |
| Hazard statements | H302, H315, H319, H335 |
| Precautionary statements | P264, P280, P302+P352, P305+P351+P338, P362+P364 |
| NFPA 704 (fire diamond) | 1-1-1-🛢️ |
| Lethal dose or concentration | LD50 Oral - rat - > 2,000 mg/kg |
| LD50 (median dose) | LD50 (median dose): >5000 mg/kg (rat, oral) |
| PEL (Permissible) | Not established |
| REL (Recommended) | 13.8 |
| Related compounds | |
| Related compounds |
Bis(acetylacetonato)copper(II) Copper(II) glycinate Copper(II) oxalate Copper(II) gluconate Copper(II) aspartate |
