© 2026 Nanjing Finechem Holdings Co., Ltd,
All Right Reserved
Researchers first laid eyes on 1,3-Diphenylisobenzofuran thanks to the drive to solve problems in organic synthesis, especially where reactive intermediates show up. In the heyday of aromatic chemistry, chemists noticed furo[2,3-f]isoindole derivatives like this one showing up as sensitive color reagents or intermediates, sparking interest in exploring their unique reactivity. Chemists across Europe and the United States dug deeper, mapping out pathways for making this compound and exploring its potential as a trapping agent in Diels-Alder reactions. Organic chemists favor 1,3-Diphenylisobenzofuran not just for its effect in the flask but for a knack at teaching students about the nuances of aromatic ring systems—showing how structure shapes function. Watching the literature swell over the decades, those historical roots continue to inspire new generations to look at classic heterocycles with fresh eyes.
Anyone who has worked with polycyclic aromatic compounds knows that 1,3-Diphenylisobenzofuran stands out thanks to its deep yellow color and crystalline texture. A simple glance gives chemists a clue: this molecule absorbs visible light like few others, hinting at uses in dye chemistry and photochemistry. Its structure—two phenyl rings flanking an isobenzofuran core—builds in stability and a predictable reactivity pattern. Over the years, this compound has become a staple where singlet oxygen reactions need a diagnostic tool. In the classroom, a vial of 1,3-Diphenylisobenzofuran feels almost like a rite of passage, representing the intersection of synthetic practicality and real-world application.
1,3-Diphenylisobenzofuran catches light with a strong yellow hue, thanks to its extended conjugation, and melts just over 120°C—a detail that has saved countless reactions from accidental decomposition. The compound dissolves well in nonpolar organic solvents, making it easy to introduce into many reaction systems. Chemically, it stands out for its high reactivity with singlet oxygen, which leads to endoperoxide formation, a reaction visible by a simple loss of color in the lab. This reactivity makes it a go-to probe for detecting reactive oxygen species.
On a technical level, chemists demand rigor in purity when they reach for 1,3-Diphenylisobenzofuran. Any trace impurities show up right away by TLC or NMR, so specifications tend to center around a purity of at least 98 percent. Labels on bottles always warn of light sensitivity—any stray sunlight eventually breaks down this delicate furoisobenzofuran backbone. Handling guidelines include low-temperature and dark storage, or else that bright yellow quickly fades. Other key identifiers like CAS number and molecular weight rarely confuse, since professionals depend on such data for cross-referencing procedures across journals and catalogs.
Old and new methods both have a place in producing 1,3-Diphenylisobenzofuran, though most chemists now stick with straightforward condensations. Reacting phthalic anhydride with diphenylacetylene in the presence of a Lewis acid still works as a reliable path, producing solid yields and clean product with careful purification. Some modern tweaks employ different catalysts or gentle heating, but that classic method keeps showing up, a testament to the efficiency of time-tested organic transformations. Experienced hands know the importance of careful temperature control and purification, since overlooking details often leads to colored byproducts or partial ring closure—problems seen and solved through decades of benchwork.
Ask an organic chemist what makes 1,3-Diphenylisobenzofuran unique, and the answer circles back to its Diels-Alder reactivity. Eager to participate with reactive dienophiles, especially singlet oxygen, it forms bicyclic endoperoxides with a clear visual signal—a loss of its yellow color. This signature transformation not only helps in mechanistic investigations but also lets scientists track reactions in real time. Derivative chemistry also opens up possibilities; adding substituents to the phenyl rings or tweaking the core can tailor properties for specific applications, though the delicate balance between stability and reactivity keeps chemists on their toes. The range of reactions stretches beyond textbooks, with users exploiting that furan ring’s susceptibility to both nucleophilic and electrophilic attack.
For anyone searching literature or chemical databases, 1,3-Diphenylisobenzofuran shows up under several names—DPBF is a common abbreviation. Sometimes references call it o-Quinodimethane trap or simply identify it by its function as a reactive probe, but most synthesis and application papers stick to the main IUPAC naming conventions. These synonyms matter for tracing safety data, technical reports, or alternate preparation routes across journals.
Handling polyaromatic compounds in the lab means paying attention to safety at every step. Researchers always store DPBF in a cool, dark place to preserve its integrity; heat or prolonged light will degrade both the compound and the experiment. Anyone who has spilled a bottle or inhaled the dust learns fast that wearing gloves and working in the fume hood feels less like a formality and more like a standard operating procedure. While direct toxicity data remains limited, prudence dictates minimizing skin contact and avoiding inhalation, since extended aromatic systems often contain risks not apparent at first glance. Waste handling—especially in academic or industrial settings—demands proper disposal by organic chemical waste protocols. Years of lab experience reinforce the lesson: treat every new bottle with respect to both compound and safety.
When evaluating real-world value, 1,3-Diphenylisobenzofuran finds its strongest use as a chemical probe. Nearly every research group exploring singlet oxygen turns to DPBF for its clear visual reaction; by tracking the disappearance of the yellow color, analysts quantify oxygen generation in photodynamic therapy and environmental chemistry. The compound’s role isn’t limited to oxygen chemistry. It helps monitor oxidative performance in organic and pharmaceutical synthesis and turns up in studies of antioxidants and reactive oxygen species scavengers. In undergraduate teaching labs, DPBF often anchors practical demonstrations of organic reactivity, while in industrial research, scientists use it for fine-tuning reaction conditions where oxygen or other electrophiles play a role.
Current research takes DPBF beyond its classic oxygen-trapping role. Scientists now develop structure-activity relationships, modifying the core and side groups to shift optical properties or tune solubility. Such efforts benefit from open collaboration across photochemistry, pharmaceutical industry, and polymer chemistry. Papers over the past decade suggest new luminescent derivatives and improved stability, raising hopes for expanded use in sensors or organic electronics. New analytical techniques, such as time-resolved spectroscopy, coax out subtle details in DPBF’s reaction kinetics and electronic structure, with high-level computation supporting experimental roles. These cross-disciplinary efforts inspire upgrades in both classroom and industry settings, keeping DPBF relevant amid shifting research priorities.
A recurring challenge with aromatic compounds involves fully characterizing toxicity. Detailed studies on DPBF itself remain relatively sparse, though its structural relatives sometimes trigger caution. Data from analogous compounds suggest digestive and respiratory irritation as primary acute risks, with longer-term exposure risks remaining only partly understood. In a modern regulatory climate, this underscores the need for ongoing research into chronic and environmental toxicity, including breakdown products formed as DPBF reacts with environmental oxygen. Using DPBF as a tracer in biomedical research also requires careful calibration, since even low-toxicity compounds can pose risks at higher concentrations or over repeated exposures. Every experienced chemist learns to review the emerging literature, update their risk assessments, and educate new lab members on best practices to keep personal and collective hazards to a minimum.
Chemists and materials scientists look at 1,3-Diphenylisobenzofuran and see more than a time-honored probe—they see an open door for innovation. As interest grows in photoactive therapies, organic electronic devices, and real-time sensor platforms, DPBF stands out as a flexible building block for new materials. Modifying its core opens up the possibility of next-generation chemical sensors for healthcare, more stable light-absorbing compounds in solar technologies, and bespoke intermediates in pharmaceutical design. In the broader drive for greener chemistry, new process development for DPBF could deliver less waste, higher selectivity, and greater safety. These advances rely not only on technical breakthroughs, but also on international cooperation and transparent sharing of toxicity data, synthesis advances, and real-world application results. Any research group with the ambition to push boundaries in organic chemistry can find in DPBF an enduring partner for discovery.
Take a look at 1,3-Diphenylisobenzofuran, and the part that jumps out right away is its unmistakable structure. The main skeleton centers on an isobenzofuran core, and this is a fused ring made by combining a benzene ring with a furan ring. Bolt on two phenyl groups at the 1 and 3 positions—each of these brings a whole new dimension to the molecule's stability and reactivity. The entire structure comes down to three benzene rings and a furan ring, all tied together into a compact and resilient molecule.
Chemistry teaches us that the secrets of a molecule hide in its shape. The two phenyl groups hanging off the isobenzofuran backbone aren't just there for decoration; they give the compound its punch. These extra rings soak up electrons, making the molecule less reactive than a bare isobenzofuran. As someone who has spent hours losing sleep to reaction specificity, additions like these don't just influence how a molecule reacts—they write the whole play.
For 1,3-Diphenylisobenzofuran, chemists get a compound packed with potential. The extended pi-system allows this molecule to absorb visible light—a trick that makes it popular as a chemical probe in research labs. The rigid structure, the planarity provided by that backbone, the spread of electrons across the molecule—all these play into why this molecule pops up in studies of singlet oxygen, which is a big topic these days in fields like photodynamic therapy and environmental monitoring.
Researchers worldwide use 1,3-Diphenylisobenzofuran to track and trap singlet oxygen, which plays a big role in biological degradation and pollution control. Publications in Journal of the American Chemical Society and Journal of Organic Chemistry often use this molecule for its fluorescent properties and robust stability. The chemical structure lets it act as a real-time sensor, changing color or fluorescence in response to certain reactive oxygen species. In my own experience, seeing a solution turn from yellow to colorless within minutes of irradiation makes it impossible to overlook how structure and application work hand in hand.
Lots of folks in research run into roadblocks with chemical stability. Not everything on the market stays fresh after you open it. Here, that sturdy aromatic system helps 1,3-Diphenylisobenzofuran shrug off light and air a bit better than most furan-based compounds. Still, storage under inert gas and protection from light keep it in top shape. Spotting this particular structure on a label helps a lab team plan synthesis and experimental workflows, knowing they have a tool that won’t fail overnight.
Chemical structure carries weight—from driving discoveries in renewable energy to pinpointing how cells defend themselves against stress. In research or industry, 1,3-Diphenylisobenzofuran's bones serve as a foundation for new probes and sensors. Smarter approaches in chemical design draw on molecules like this, thanks to a backbone that refuses to quit and an electron system ready for action.
I have seen plenty of complicated molecules come and go, but 1,3-diphenylisobenzofuran (DPBF) holds a special spot for chemists tracking singlet oxygen. In the lab, DPBF is a lightweight probe. It reacts with singlet oxygen and gives a color change you can actually see. No advanced equipment necessary, just a pair of eyes and a UV-vis spectrophotometer. This trait simplifies life for folks doing photochemistry, where singlet oxygen pops up in photodynamic therapy, wastewater treatment, and the creation of new drug molecules. DPBF helps chemists measure how much reactive oxygen forms during light-activated reactions — basically, if you're tweaking something with light, DPBF gives you feedback right away.
Cancer treatment research has explored light-activated therapies for years. The effectiveness of these therapies depends on how well a compound can generate singlet oxygen to destroy cancer cells. DPBF doesn’t just appear in basic chemistry classes — research labs keep it on the shelf because it offers proof that singlet oxygen appears during these light-driven reactions. I’ve seen researchers keep logs, jotting down absorbance readings and tracking singlet oxygen generation using DPBF. This hands-on tracking speeds up therapy development, offering a checkpoint for safety and potency, and also helps researchers tweak their approach without needing costly trials early on.
Industries that produce dyes, inks, and pigments test their products for lightfastness. Singlet oxygen can degrade organic compounds in these products, causing fading or breakdown. DPBF serves here as a trouble detector. Manufacturers test samples under bright light, mix in some DPBF, and track any decrease in color or absorbance. If DPBF’s signal drops fast, it’s a warning: either the product or the process may be prone to oxidative damage outside the lab. Companies can then adjust processes, mix in antioxidants, or pick new raw materials quickly, long before a defect shows up in the hands of a customer.
Environmental scientists need tools to check how pollutants break down and whether their treatments work. In advanced oxidation processes, researchers aim to eliminate toxins in wastewater using light and reactive oxygen species. DPBF steps in as a tracker for real-time monitoring. As wastewater treatments churn and process, a dip in DPBF signal means the process generates enough reactive oxygen. Teams can then adjust dosing or UV exposure on the fly, making operations more efficient and eco-safe. I’ve seen university research teams lean on DPBF to fine-tune pilot-scale water purification right in the field.
DPBF’s popularity shows that chemical tools don’t have to be complex to show real results. Still, chemists and manufacturers need to handle it with care, since DPBF also degrades with light and air exposure. Improving its stability or creating similar trackers that last longer could help the industry. More collaborations between chemists, manufacturers, and environmental scientists may speed up these improvements, giving everyone more reliable and robust ways to measure singlet oxygen and manage oxidation in products and processes.
Chemistry loves its complexity. Compounds with intimidating names, like 1,3-Diphenylisobenzofuran, get tossed around in research labs and pharmaceutical discussions, a reminder that molecules don’t always play fair. Questions often pop up about the basic blocks: structure, formula, use, and molecular weight. So, let’s look at why the molecular weight of 1,3-Diphenylisobenzofuran matters beyond lab notes and classroom tests.
For those digging into organic chemistry, molecular weight means everything. With 1,3-Diphenylisobenzofuran, it clocks in at 334.38 grams per mole. That’s not a trivia pursuit point. That number is the foundation for any precise work in the lab—be it synthesis, analysis, or application in industry.
Accurately dialling in on that figure changes the stakes. I remember mixing solutions as a student and noticing how a miscalculation—something as “small” as one gram off across a batch—derailed the experiment. If we’re talking research, pharmaceuticals, or dyes, misjudging the amount you have (or need) can waste time, burn through budgets, or even spoil months of long work.
Let’s break it down. 1,3-Diphenylisobenzofuran’s molecular formula is C20H14O. Plugging in atomic weights, carbon gives you 12.01, hydrogen provides 1.01, and oxygen sits at 16. Add twenty carbons, fourteen hydrogens, and one oxygen together, and you hit that 334.38 mark exactly. That simple math tells us how much of the substance sits in a mole, but also steers chemists when they decide how much reagent they need, how to scale projects, and what to expect from a reaction.
Discussions about numbers might seem dry, but they stretch far beyond dusty textbooks. Tiny discrepancies create a ripple effect—the kind that messes up the purity of a compound, twists experimental outcomes, or in big industry, leads to product recalls. No one wants to be the person who sank thousands into a failed lot because the numbers went unchecked. In a field constantly on the hunt for precision, molecular weight isn’t just a detail; it’s a non-negotiable starting point.
The practical edge of getting molecular weight right shows up everywhere quality matters. In semiconductors, dyes, solar panels, or pharmaceuticals using isobenzofurans, doses hinge on precise milligram amounts. A small excess can totally change physical properties or introduce unwanted contaminants. Even with modern spectrometry and advanced scales, that first math check—the molecular weight—sets everything in motion.
Mistakes slip in easily if someone copies a wrong entry from a database or a paper. It pays to double check, using trustworthy sources like reputable chemical suppliers or peer-reviewed journals. For extra peace of mind, spot the numbers in several databases. I’ve learned to trust but always verify—seeing seasoned scientists trip over minor numbers drives that lesson home.
Smart labs set up cross-checks for all raw data early in a project. A team that respects the basics—like confirming molecular weights—saves headaches down the line. Institutions and companies investing in strong reference materials and continuous staff training wind up catching mix-ups before they turn into lost time or failed shipments.
Getting the molecular weight right for compounds like 1,3-Diphenylisobenzofuran feels small, but for scientists, it has an impact that ripples out through every project, product, and publication that follows.
1,3-Diphenylisobenzofuran often lands on the laboratory shelf because of its sensitivity to light and air. Having worked with similar organic compounds, it’s clear that overlooking their fragile personality usually leads to spoiled batches or safety headaches. You crack open a bottle too many times or expose it to sunlight through a lab window, the bright yellow color starts to fade, and purity slips away before you notice. This chemical doesn’t like surprises, and it doesn’t forgive neglect.
I once watched a teaching assistant hurry along a demonstration, ignoring the UV shielding on a furan solution. Not five minutes later, the sample had both lost color and lost its value. 1,3-Diphenylisobenzofuran is highly photoreactive; exposure to visible or UV light can destroy its structure. Laboratories that store this compound in clear glass or leave it under open lights often see whole supplies turn useless. Brown glass vials or amber bottles work much better, blocking light and keeping out accidental degradation.
Oxygen also gets into the act. Oxidation eats away at organic reagents, and for a compound like this one, an inert atmosphere really helps. Filling vials with nitrogen or argon before sealing keeps the environment protective. For longer-term stashing, it pays to wrap bottles tightly and double-bag them in foil. This keeps not just photons, but also air, at bay. I’ve seen labs lose months of planning because a seal was loose.
Don’t ignore water. Humidity in the air reacts slowly with organics and the consequences creep in silently. Storing 1,3-Diphenylisobenzofuran in a desiccator solves this problem. When rare or expensive chemicals turn into sticky messes, it comes back to one culprit: moisture. Keeping dessicant packs handy lets everyone play it safe. This kind of routine feels minor, but it’s the difference between successful experiments and wasted afternoons.
Some colleagues put all their chemicals in the fridge and forget them. Cold storage can help, but not every compound needs freezing. For 1,3-Diphenylisobenzofuran, room temperature is usually fine as long as light, air, and water stay out. Refrigerators can help for longer storage, just avoid freeze-thaw cycles. Labeling dates and conditions saves a lot of effort, especially when projects run long.
Transparent practices protect everyone who uses the chemical down the line. Safety data sheets deserve more than a passing glance—these documents recommend gloves, eye protection, and proper ventilation not just during experiments, but even for transfers and storage. Last year, a colleague discovered a decades-old sample with degraded labels and leaking seal. That bottle forced an evacuation and special disposal—luckily, nothing worse happened.
Storing 1,3-Diphenylisobenzofuran isn’t about overengineering; it’s about respect for chemistry and for the people at the bench beside you. Keeping the bottle dark, sealed, dry, and at a steady temperature helps everyone focus less on damage control and more on discovery.
Anytime you’re working with chemical compounds, especially ones like 1,3-Diphenylisobenzofuran, readiness protects everyone. Stories from the lab tend to stick with scientists longer than the reactions themselves—one wrong move, and things can get messy fast. I once saw a small incident with a furan derivative—nothing catastrophic, just a costly fume hood clean-up and one bruised ego. Taking shortcuts only teaches regret. Safe habits save time in the long run, and they remind you that every bottle holds more than a label.
This molecule brings more than a tongue-twister name. Many sources warn that compounds in the isobenzofuran family cause skin and eye irritation. Some risk harm to your respiratory tract. Even if you’ve handled dozens of organics, skin contact can still lead to allergies or more severe reactions over time. Breathing in powder, splashing a solution—it only takes a moment for an accident to sideline a project.
Every chemistry lab should boast a fume hood with fans strong enough to pull away harmful vapors and limit exposure to the person doing the work. Relying on open benches spells trouble, especially with fine powders or when dissolving in volatile solvents. Support from good ventilation means less risk for everyone in the room, no matter who opens the bottle.
Gloves should never be considered optional. Nitrile gloves stop most chemical splashes far better than bare skin. Pair them with tight-fitting safety goggles. Ordinary glasses won’t block a rogue drop from sneaking through gaps. I keep face shields on hand for larger transfers or weighing operations. If your skin or eyes sting after working, you missed something. Simple steps outweigh regret every day.
Benches collect more than dust. Traces of spills, forgotten pipette tips, or solvent residue open doors for accidental contact. I wipe down workspaces before every setup and again at the end. Confusion in the middle of a procedure raises the chance of mistakes. You can’t disinfect time, but you can control clutter right now.
Most labs keep absorbent materials like pads or vermiculite on hand for chemical spills. Kits suited for organic solvents make cleanup quicker and safer. If 1,3-Diphenylisobenzofuran lands on skin or eyes, clean water matters more than heroics—flush for at least fifteen minutes and seek help. Have emergency showers and eyewash stations within reach. Clear labeling and easy access to these resources skips panic when seconds count.
Used compounds shouldn’t just disappear into the sink. I collect all waste, even contaminated gloves or paper towels, in marked organic solvent bins. This keeps hazardous stuff away from landfills and local water sources. Regulations exist for a reason—environmental safety stretches beyond the lab walls. Check local rules to keep disposal above board.
Training matters. Watching a veteran chemist handle delicate materials taught me to pause and double-check every step. Risk shrinks when you prepare, ask questions, and respect materials. Every researcher, experienced or new, deserves a safe space to discover. Labs run smoother and more confidently when everyone chooses safety first—no exceptions and no excuses.
| Names | |
| Preferred IUPAC name | 2,2-Diphenyl-2H-isoindole-1,3(2H)-dione |
| Other names |
DPIBF o-Quinodimethane dimer 1,3-Diphenyl-2-benzofuran 1,3-Diphenylisobenzo[b]furan |
| Pronunciation | /ˈwaɪlənˌtriːˈfenəlˌaɪ.soʊˌbɛn.zəˈfjʊər.ən/ |
| Identifiers | |
| CAS Number | [2761-62-0] |
| Beilstein Reference | 87361 |
| ChEBI | CHEBI:52033 |
| ChEMBL | CHEMBL131434 |
| ChemSpider | 235812 |
| DrugBank | DB08415 |
| ECHA InfoCard | 100.049.226 |
| EC Number | 205-076-6 |
| Gmelin Reference | 273961 |
| KEGG | C10633 |
| MeSH | D000071658 |
| PubChem CID | 70924 |
| RTECS number | OV8400000 |
| UNII | 3433D2MGU3 |
| UN number | Not regulated |
| Properties | |
| Chemical formula | C20H14O |
| Molar mass | 334.40 g/mol |
| Appearance | Yellow solid |
| Odor | Odorless |
| Density | 1.194 g/cm³ |
| Solubility in water | Insoluble |
| log P | 3.5 |
| Vapor pressure | 2.61E-10 mmHg at 25°C |
| Acidity (pKa) | No data |
| Magnetic susceptibility (χ) | -79.7·10⁻⁶ cm³/mol |
| Refractive index (nD) | 1.707 |
| Dipole moment | 2.13 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 531.6 J·mol⁻¹·K⁻¹ |
| Std enthalpy of combustion (ΔcH⦵298) | -5292.7 kJ/mol |
| Hazards | |
| GHS labelling | GHS02, GHS07 |
| Pictograms | GHS07 |
| Signal word | Warning |
| Hazard statements | H302 + H312 + H332: Harmful if swallowed, in contact with skin or if inhaled. |
| Precautionary statements | P261, P280, P305+P351+P338, P337+P313 |
| NFPA 704 (fire diamond) | 1-2-0-Health_1-Flammability_2-Instability_0 |
| Flash point | 120 °C |
| Lethal dose or concentration | LD₅₀ (oral, rat): >9600 mg/kg |
| LD50 (median dose) | LD50 (median dose): 3000 mg/kg (oral, rat) |
| NIOSH | UY5250000 |
| PEL (Permissible) | Not established |
| REL (Recommended) | 0.5 mg/m³ |
