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Copper(II) oxide has a long story that weaves through alchemy, metallurgy, and modern chemistry labs. Generations back, artisans and tinkerers discovered that heating copper in air left behind a black powder with some mysterious properties. This new compound, later called copper oxide, fell into everyday use by glassmakers for coloring glass and by early proto-chemists searching for reliable reactants. Ancient manuscripts from the Middle Ages already talk about black copper oxide in smelting techniques and pigment recipes. Jump ahead a few hundred years, the stuff shows up in 18th-century chemistry books as a tool for learning about acids and bases, and for proving basic chemical reactions. When modern analytical chemistry picked up speed, copper(II) oxide made the list of dependable standards, helping refine chemical techniques like gravimetric analysis. It’s hard to find another simple compound that has crossed so many paths—from art to industry, from folk tradition to high science.
A closer look at copper(II) oxide reveals a substance lying at the intersection of utility and curiosity. Chemists know it as CuO, a black, powdery or crystalline solid. It handles a surprising variety of tasks, from acting as a break-down catalyst in chemical factories to helping stabilize batteries. Schools use it in student labs for teaching decomposition reactions, and researchers find new applications almost every decade. If you’ve worked with ceramics, you’re probably familiar with its role in adding rich blues and greens to glazes. Big industry leans on copper oxide for its electrical and antimicrobial traits, so you’ll also find it tucked inside gas sensors, semiconductors, or even medical dressings. It isn’t limited to the science textbooks—it pops up wherever someone needs a controlled reaction or a steady, predictable compound. Whether you’re in a classroom or a factory, copper(II) oxide offers a straightforward, persistent value.
Look at this black powder under a microscope, and you notice small, angular crystals. Copper(II) oxide stands out for its thermal stability, holding its structure until temperatures reach around 1,332°C, where it basically melts. It doesn’t dissolve well in water, so it usually sticks around during most wet processes, but acids eat away at it with ease. It’s denser than many everyday substances—over six grams per cubic centimeter—so even a small pile feels heavier than expected. The matte black color doesn’t just look dramatic; it signals the specific electron configuration of copper ions, which chemists can detect using X-ray or spectroscopic methods. The oxide stays tough at room temperature, but if you hit it with a strong reducing agent, it will give up its oxygen and leave behind pure copper metal. Its basic chemical nature comes out when it reacts with acids to generate copper salts, a trick known for centuries. Every physical and chemical characteristic translates into choices that influence how copper(II) oxide works in real-world systems.
Industrial batches of copper(II) oxide often come labeled with minimum copper content, grain size, and trace impurity levels. Fine-grained varieties serve chemical synthesis and electronics, so manufacturers monitor the particle size tightly. X-ray diffraction and elemental analysis are the main tools for ensuring product quality, while the presence of free metallic copper, sulfate, or chloride impurities could spell trouble in some high-tech uses. Companies stamp packages with hazard statements to meet international transportation and workplace regulations. Because heavy metals raise environmental red flags, lots of attention goes into proper storage and labeling. From shipping containers to classroom vials, finding an accurate label goes beyond formality—it helps folks stay safe and keeps the work honest.
The classic way to make copper(II) oxide uses thermal decomposition of copper(II) compounds. Heat copper(II) nitrate or copper(II) carbonate, and the green or blue materials first foam, then settle into black, powdery oxide. Some labs prefer to react copper(II) salts with concentrated sodium hydroxide, filter off the light blue precipitate, then heat it until it darkens. Large-scale producers use direct oxidation, roasting pure copper metal at high temperatures in controlled airflow, yielding product in large, economic batches. Like so much of chemistry, the real work happens in quality control and purification. Careful washing and drying keep the final product free of damaging acids or trace contaminants. Every step reflects years of refinement by thousands of researchers, all seeking a repeatable, efficient process.
Copper(II) oxide stands as a sturdy participant in a long list of reactions—from the typical redox exchanges with hydrogen gas to more complex catalytic cycles in organic synthesis. Throw it into a beaker with hydrochloric acid, and you get a bright blue solution of copper(II) chloride, releasing water. Mix it with ammonia, and the deep blue color suggests the formation of soluble copper-ammonia complexes. Reduce it using hydrogen or even simple carbon, and pure, metallic copper forms—a transformation that shaped metallurgy for generations. The oxide can also serve as a seed for making nanomaterials. Modern labs sometimes grind it into nanoparticles, altering its properties further and opening the door to electronics, catalysis, and medicine. The chemistry of copper oxide remains one of the basic tools for exploring solid-state transformations, and with every decade, tinkerers and scientists discover new ways to tailor its properties.
People working in different fields have their preferred names for copper(II) oxide. Besides CuO, the black oxide gets called cupric oxide by chemists, bluestone by old-school metallurgists, and “black copper oxide” by ceramists or pigments buyers. In pharmaceutical and agricultural contexts, names can shift to match specific regulations or supply chains. The array of synonyms occasionally causes headaches in procurement or regulatory paperwork, but every industry seems to find its own shorthand while working with the same stubborn black powder.
Handling copper(II) oxide starts with an understanding of basic chemical safety. Inhalation of the fine powder causes irritation, so gloves and dust masks offer real protection. The compound’s toxicity ranges from low in occasional lab use to more concerning in cases of chronic exposure. Heating copper(II) oxide generates fumes that you don’t want to breathe. Ventilation and careful attention to dust buildup matter most in production environments. Regulatory bodies like OSHA or the EU’s chemicals agency routinely review occupational exposure limits and require safety data sheets to accompany all shipments. Smart storage habits—springing for sealed containers, cool, dry spaces, and clear labeling—pay dividends over time, keeping both people and nearby materials safe. Waste management draws oversight from local authorities, thanks to the potential for copper compounds to harm aquatic environments.
Copper(II) oxide proves itself in many unexpected places. In ceramics, it remains a trusted glaze ingredient. Electronics and battery companies count on it for use in semiconductors, electrodes, and sensors, where its stable oxidation state makes it a solid choice for consistent conductivity. Catalysis experts take advantage of its ability to drive controlled oxidation reactions. Some agriculture products lean on copper(II) oxide to provide micronutrients essential for plant health, though regulatory scrutiny often sets strict use limits due to concerns about environmental loading. Pigment and dye manufacturers value its intensity and permanence when producing glass, tile, and enamel goods. More recently, medical researchers checked out its antimicrobial attributes for integration in hospital surfaces and wound dressings—a trend that looks set to intensify as antimicrobial resistance grows.
The future of copper(II) oxide leans on cutting-edge research across several fields. Nanoscale chemistry keeps turning out new variants, with nanoparticles showing supercharged catalytic and antiviral properties. Solid-state physicists experiment with modified copper(II) oxide in attempts to design new kinds of superconductors and quantum materials. Renewable energy projects continue testing CuO as a photocatalyst for splitting water or driving solar-powered reactions. Some researchers try to tweak its surface chemistry, changing the crystal habit or introducing rare elements to enhance electronic or magnetic behavior. Funding for more environmentally friendly preparation methods keeps flowing, with many universities searching for less polluting synthesis steps and greener recovery processes. The constant interplay of basic research and commercialization ensures that copper(II) oxide evolves with every generation of technology.
Toxicologists have dedicated plenty of effort to mapping out copper(II) oxide’s effects on both workers and the wider environment. Swallowing or inhaling significant quantities causes toxic symptoms, mostly due to copper’s biological reactivity. Chronic exposure may have more subtle, cumulative impacts, especially in poorly ventilated or unregulated settings. Research tracks its impact on aquatic life, where copper ions cause trouble even at low concentrations, affecting everything from algae to fish. Bioaccumulation remains a real concern, pushing regulators and scientists to do a better job at managing waste streams and monitoring soil and water around production sites. Newer toxicity studies look at nanoparticle forms, where the smaller size seems to boost reactivity—raising fresh questions about respiratory health and long-term accumulation in living tissue. Discussion about exactly how safe is safe enough never quite closes, ensuring vigilance keeps pace with progress.
The road ahead for copper(II) oxide ties closely to bigger shifts in technology and society. As industries hunt for cleaner, recyclable materials, the demand for metals that can be recovered, reused, and tracked sustainably comes into focus. Copper(II) oxide’s low cost, accessibility, and straightforward chemistry lend it an obvious place in renewable energy, electronic waste recycling, and environmental remediation. As the world’s electronics infrastructure grows and medical needs shift toward surfaces that resist infections, expect more effort directed at tuning its properties even further, whether in composite materials, flexible electronics, or next-generation medical coatings. The durability and versatility that put copper(II) oxide on the map centuries ago stay relevant in a world searching for smarter answers to resource challenges. Its story, still unfinished, offers lessons in adaptability and the power of simple materials to keep spawning new ideas.
Walk through a chemistry lab, glance at the shelves, and you’ll likely spot a bottle of copper(II) oxide. With its deep black powder, the substance stands out, though its uses often fly under the radar. Many folks outside of labs don’t realize how often this chemistry staple shows up in the world around us. Bringing out the fact, copper(II) oxide acts as a heavy lifter across industries, not just for scientists.
Some of my earliest memories of chemistry stretch back to a community pottery class. There, colored ceramics left a strong impression. Artists often use copper(II) oxide to get rich greens and sometimes reds in their glazes. It reacts in the kiln, helping to shape everything from coffee mugs to outdoor tiles. It’s easy to overlook, but those earthy greens and the subtle shift in color at the lip of a handmade bowl? Much of that comes from an oxide like this. You find its fingerprint on fine china, as well as on the everyday items lining kitchen cabinets across the world.
People studying chemistry know copper(II) oxide works as a building block for other copper-based compounds. Take copper sulfate, a staple in science education and agriculture. By adding copper(II) oxide to sulfuric acid, producers create the powder that fertilizes fields and cleans swimming pools. There’s another side to this story. In big chemical plants, copper(II) oxide shows up as a catalyst—helping speed up reactions, but never getting used up itself. This cuts costs and cuts down on chemical waste. For example, in hydrogen production, copper(II) oxide grabs hydrogen from water and releases clean gas. This process plays a role in building cleaner sources of fuel.
The steady push for green energy keeps copper(II) oxide part of the discussion. Manufacturers use it in batteries. This substance keeps popping up, from early dry cell batteries to research into new lithium-ion designs. Its ability to swap electrons—without putting up a fuss—makes it a favorite for research teams looking for safer, higher-capacity power sources. Not just batteries. Electronics makers rely on copper(II) oxide in making printed circuit boards and gas sensors, beyond the average smartphone, these boards hold together wind turbines and solar panels as well.
Growing up near a large body of water, you learn about the battle to keep invasive organisms off boats. Many anti-fouling paints carry copper(II) oxide, which keeps barnacles and algae from clinging to hulls. This stretches boat lifespan and fuels the marine industry, protecting jobs in shipyards. Today, scientists weigh the impact of copper pollution, but its protective effect still keeps it in play. In agriculture, copper(II) oxide goes into some fungicides that stop fungal diseases on crops—though smarter, safer use calls for tighter regulations and improved application techniques.
Copper(II) oxide comes with both benefits and risks. Direct handling, if done carelessly, can lead to respiratory or skin irritation; long-term buildup in soil or water threatens health and ecosystems. Making copper(II) oxide safer isn’t just a job for chemical engineers. Policymakers, farmers, and environmentalists keep pushing for more oversight and greener alternatives. Smarter recycling in electronics, careful paint formulations, and tweaks to manufacturing lines cut down waste and pollution—improving how copper(II) oxide gets used without losing its unique advantages.
Understanding the journey of this plain-looking powder sheds light on everything from the glazes on a handmade mug to the electronics that power our daily lives. Watching for shifts in how copper(II) oxide gets used will matter more, especially as demand for safer and cleaner technologies keeps growing.
Copper(II) oxide shows up in many places: laboratories, electronics manufacturing, even in pigments and ceramics. It’s impossible to overlook how it helps drive modern technology. Folks working with it might ask if there’s any reason to worry. From my time helping with chemistry demonstrations at community colleges, the safety question always comes up—usually for good reason.
No sense beating around the bush—touching or breathing in copper(II) oxide can cause harm. This chemical is a black, powdery substance. If it gets on your skin or in your eyes, it stings and can cause irritation. Inhaling dust often leads to coughing and a sore throat. Some people develop headaches, nausea, or even more severe lung symptoms from repeated exposure. According to the Centers for Disease Control and Prevention (CDC), occupational exposure has been linked to "metal fume fever," a flu-like illness.
Children might face bigger risks if they accidentally swallow something containing this compound. The National Institute for Occupational Safety and Health (NIOSH) reports animals developed kidney and liver problems when exposed long enough. Most people in the general public won’t run into these levels of exposure. Still, for workers and hobbyists, it’s a big consideration. I remember a teacher stressing how fine copper compounds don’t belong in a classroom vacuum because they blow right back into the air.
Copper(II) oxide mainly enters the body through inhalation of dust or by swallowing contaminated materials. Direct skin contact poses less risk, but without gloves and goggles, someone using it in a lab or workshop could face burns or rashes. Using poor ventilation in chemical work almost guarantees some exposure. More than once I've seen colleagues come away from a hasty cleanup with red eyes or itchy skin.
It’s not just human health. Dumping waste that contains copper(II) oxide can harm fish and other aquatic life. Even backyard hobbyists making their own patinas or ceramics sometimes wash runoff down the drain, not thinking about where it goes. Researchers in environmental science have linked copper ions in water to stunted plant growth and lower survival rates for small aquatic animals. Once copper builds up in the ecosystem, it doesn’t break down quickly. That linger makes it a problem for both city regulators and neighbors living near an industrial site.
There’s always a better way than winging it. Wearing gloves, goggles, and masks takes care of most workplace dangers. Labs use fume hoods as a standard because they pull dust away from the breathing zone. In shops and factories, regular air monitoring helps catch issues before symptoms start. OSHA sets legal exposure limits, but going beyond this baseline helps people stay healthier in the long run. Teachers and hobbyists need proper storage and labeled containers—no one wants a kid mistaking black powder for charcoal. At home, disposing of unused chemicals at hazardous waste sites helps keep it out of groundwater and streams.
Understanding copper(II) oxide’s hazards lets workers and enthusiasts stay safe and keeps the environment clean. Facing the facts and using available gear stops problems before they start. It’s easy to skip safety for convenience, but the extra five minutes spent on prevention usually saves much more time and money down the road.
Copper(II) oxide turns heads with its deep black color and dense, earthy look. If you've ever powdered copper(II) oxide in a lab, the stuff stains your gloves and hangs in the air, proof of its fine, almost sooty texture. It doesn’t dissolve in water, which limits spreading into the environment, but it still reacts strongly with acids. Heating up a dish of copper(II) oxide tells you right away it has a high melting point, somewhere above 1,200°C. That’s a temperature that pushes many lab setups to their limit, making it a tough customer where heat is involved.
This compound carries weight—about 6.3 grams per cubic centimeter. You won’t find it floating or volatilizing, and if you’ve ever cleaned it off glassware, you know it sticks well, showing its gritty, almost abrasive side. It’s stable in the open air, too. You can store it on a shelf for years, and it won’t blink at sunlight or normal humidity.
Copper(II) oxide packs one atom of copper and one atom of oxygen. Its structure, CuO, brings with it a distinctive way of dealing with other chemicals. Drop some into hydrochloric acid, and it fizzes up, releasing copper ions and forming that unmistakable blue-green copper chloride solution. Anyone who has run this reaction remembers the shift from black powder to clear solution—a transformation that’s almost magical in how direct it feels.
The substance acts as an oxidizer under the right conditions, giving up oxygen to speed along redox reactions. The copper(II) oxide sitting on a porcelain crucible during a science experiment often transforms into copper metal if you throw in some hydrogen gas and a little heat. That simple reduction reaction finds use in everything from metallurgy to school chemistry labs.
Copper(II) oxide doesn’t play nice with all chemicals. Mixed with reducing agents like charcoal or even sugar, especially at high temperatures, the compound breaks down quickly, which can prove dangerous if not monitored. Making pyrotechnics or chemistry demonstrations with it calls for a steady hand and solid experience, especially because it’s not just the heat but the chemical potential that ramps up risk.
People often overlook how central copper(II) oxide has become outside lab benches and chemistry sets. Ceramic glazes get their rich blue-green tints from it. Battery designers rely on copper oxides for cutting-edge electrodes, pushing the edge on energy storage tech. Even gas sensors and antifouling paints need its unique properties.
Worries about toxicity with copper compounds deserve real attention. Workers in factories or labs need tight controls—good ventilation, gloves, and awareness of the dangers, because regular exposure deals damage to kidneys and liver over time. Regulatory agencies, such as OSHA and the EPA, draw clear lines on exposure, and for a good reason.
The practical side of copper(II) oxide—its solubility in acids, quality as an oxidizer, and stubborn black color—have shaped careers in chemistry, manufacturing, and art. I learned early on to keep goggles tight and respect the dust, not just for the mess but for the health risks. Improved ventilation, thoughtful lab design, and honest training on toxicity lessen health threats in workshops and classrooms.
Switching to less toxic compounds for some uses, stepping up recovery systems in industry, and relying on personal protective equipment remain the best ways to cut risk. Copper(II) oxide won’t lose its place in science and technology any time soon, but it asks for respect, safety, and a willingness to look beyond its simple black powder image.
Copper(II) oxide, a deep black powder, looks unassuming on a shelf. I remember my first real lab job—my supervisor dropped a tub of the stuff on my bench, and all she said was “just remember, gloves.” That stuck with me.
Copper(II) oxide gets used in plenty of places: chemistry labs, ceramics, even in making batteries. It doesn’t explode or burn, and you won’t find much excitement in its day-to-day storage. People sometimes let their guard down around it because of this, but a little carelessness brings health issues or damages supplies.
Putting the material in a high, dry place sounds simple, but humidity loves to creep into corners and packaging failures happen at the worst times. Oxides draw moisture out of the air, which clumps the powder and can trigger chemical changes over time. Where I last worked, our storeroom ran a dehumidifier year-round, checked moisture by hand, not just with a wall sensor, and never left any bottle open longer than needed.
A sealable, chemically resistant container keeps the powder from leaking out or from picking up something unwanted, especially fumes from acids stored nearby—acids and copper(II) oxide don’t mix well. Plain plastic can crack and glass occasionally chips, so tough, tight poly bottles deliver peace of mind. Honest labeling avoids mix-ups, especially in teams where everyone handles similar-looking substances.
People underestimate the dust risk. One colleague over the years brushed away dust with a bare hand, convinced it “barely mattered.” Several months later, persistent cough and skin irritation landed him at employee health—turns out, repeated low-level exposure brings problems. Copper(II) oxide does irritate the lungs and eyes on direct contact, so don’t treat it like chalk dust or flour.
Regular gloves and basic safety glasses stop contact; a simple dust mask brings extra peace for those decanting larger batches. I learned to keep handwashing a habit—not only before lunch but before touching phones, doorknobs, or keyboards, since leaving fine powder anywhere just spreads the risk.
Sweeping up any spills with wet wipes instead of dry cloths prevents that dark cloud of powder from rising. Labeled disposal bins, checked weekly, avoided surprise build-ups. It took us a false alarm with a poorly closed bin to cement that practice, but after that, no one missed a beat.
Every new hire in our group practiced with a spill kit before they touched chemicals alone. Emergency showers and eyewash stations always stayed unobstructed, no matter how packed the space. Shared spaces multiply the chances of cross-contamination, so one team member checked labels and seals every Friday afternoon.
I’ve seen how routine checklists and quick reminders before a busy day do more good than a thousand safety posters. Training with actual examples rooted the lessons in memory. Our practices circled back to the goal—nobody gets hurt and nothing gets accidentally mixed up.
Copper(II) oxide invites easy handling mistakes, but keeping supplies dry, safely sealed, and away from both acids and open skin shows the same respect you’d offer any chemical. Investing in a few good habits up front keeps everyone safe and the powder just another quiet tool on the shelf.
Product purity isn’t just a number stamped on a label—it shapes results in labs, on factory floors, and in classrooms. Copper(II) oxide serves as an essential material in chemistry experiments, electronics manufacturing, and even renewable energy devices. In these settings, small impurities make a difference. For example, a trace of iron hiding in your copper(II) oxide can sneak into a reaction and change the expected color of a solution or even poison a catalyst, leaving you with unreliable results.
I once spent hours chasing a strange result during a redox experiment, only to realize later the copper(II) oxide we used was cut with zinc and iron impurities. This sort of experience sticks with you—it’s a reminder that “close enough” isn’t enough for some jobs. High purity material gives clear results and makes troubleshooting a lot less painful.
Most chemists and manufacturers trust the numbers on the bottle: 98%, 99%, sometimes even 99.9%. These numbers come from thorough testing, often using techniques like X-ray fluorescence, atomic absorption spectroscopy, or inductively coupled plasma mass spectrometry. Findings highlight common troublemakers—iron, nickel, zinc, and lead, to name a few. Even with those tiny amounts, experts agree that the difference between 98% and 99.9% purity isn’t just decimal dust. In electronics, one percent of impurity means more chances for unwanted electrical behavior and less reliability in the final gadget.
Pushing for higher purity pays off, but the threshold depends on where copper(II) oxide lands. In an industrial kiln producing colored glass, a bit more impurity may not ruin the day. On the other hand, if you’re refining copper(II) oxide for use in making solar cells, cleaner is key. Scientists push for near-perfect purity since impurities block electron flow and slow down the reaction rates that fuel power generation.
Health considerations demand another look at copper(II) oxide purity. Lower-grade material often finds its way into paint pigments or ceramics, where exposure can raise health questions due to contaminants like lead or cadmium. Using verified, high-purity material helps keep toxic elements out and protects workers along the supply chain. Safe handling information deserves a spot near every bottle in the lab, because mishandling copper(II) oxide—even the pure stuff—can lead to accidental exposure or environmental hazards.
More labs rely on suppliers who share a commitment to transparency and routine third-party testing. Documentation showing not only the purity number, but the breakdown of any traces present, makes it much easier to pick what’s right for your project. This goes for professional research settings as much as for teaching labs, where knowing what students work with means fewer mishaps and better lessons.
Process improvements and investments in filtration help remove persistent contaminants. When supply chains grow longer, collaborations between suppliers and their end-users keep standards meaningful. Strong quality control ensures purity isn’t just a claim—it’s a standard backed by shared effort, careful data, and regular review. As demand for clean, reliable materials grows, the focus on “how pure is pure?” only sharpens, guiding better choices all the way from the packing plant to the lab bench.
| Names | |
| Preferred IUPAC name | Copper(II) oxide |
| Other names |
Copper Monoxide Cupric Oxide Brown Copper Oxide Copper Oxide |
| Pronunciation | /ˌkɒp.ər.tuː ˈɒk.saɪd/ |
| Identifiers | |
| CAS Number | 1317-38-0 |
| Beilstein Reference | 136873 |
| ChEBI | CHEBI:29814 |
| ChEMBL | CHEMBL2090541 |
| ChemSpider | 2054391 |
| DrugBank | DB11174 |
| ECHA InfoCard | 03d2fe0a-8c8a-42be-8ae6-c1e57ca89847 |
| EC Number | 215-269-1 |
| Gmelin Reference | 778 |
| KEGG | C18706 |
| MeSH | D003793 |
| PubChem CID | 14829 |
| RTECS number | GL7900000 |
| UNII | 2AB009IJ54 |
| UN number | UN3077 |
| Properties | |
| Chemical formula | CuO |
| Molar mass | 79.545 g/mol |
| Appearance | Black powder |
| Odor | Odorless |
| Density | 6.31 g/cm³ |
| Solubility in water | insoluble |
| log P | -2.0 |
| Vapor pressure | 0 mmHg (25 °C) |
| Acidity (pKa) | 13.6 |
| Basicity (pKb) | 6.7 |
| Magnetic susceptibility (χ) | +80.0·10⁻⁶ cm³/mol |
| Dipole moment | 0 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 42.6 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -155.2 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | -155.2 kJ·mol⁻¹ |
| Pharmacology | |
| ATC code | V07BB |
| Hazards | |
| Main hazards | Harmful if swallowed, causes skin and eye irritation, may cause respiratory irritation, toxic to aquatic life. |
| GHS labelling | GHS02, GHS07 |
| Pictograms | GHS07,GHS09 |
| Signal word | Warning |
| Hazard statements | H410: Very toxic to aquatic life with long lasting effects. |
| Precautionary statements | P260, P264, P270, P272, P273, P301+P312, P304+P340, P305+P351+P338, P308+P313, P314, P330, P391, P403+P233, P405, P501 |
| NFPA 704 (fire diamond) | 2-2-0 |
| Explosive limits | Not explosive |
| Lethal dose or concentration | LD50 oral rat 470 mg/kg |
| LD50 (median dose) | LD50 oral rat 470 mg/kg |
| NIOSH | NT8050000 |
| PEL (Permissible) | PEL (Permissible Exposure Limit) for Copper(II) Oxide: "0.1 mg/m³ (as Cu, fume) |
| REL (Recommended) | 0.1 mg/m³ |
| IDLH (Immediate danger) | 100 mg/m³ |
| Related compounds | |
| Related compounds |
Copper(I) oxide Cuprous oxide Tenorite Copper(II) hydroxide Cupric sulfate Copper(II) chloride |
