1-Chloropentane: From Discovery to Emerging Applications
Historical Development
Long before 1-chloropentane found its way into laboratories and industry, chemists experimented with alkyl halides in search of versatile building blocks. Early interest in simple haloalkanes came in the late 1800s, as Wilhelm Ostwald and his contemporaries started manipulating chain lengths to explore their reactivity. By the early 20th century, 1-chloropentane took on a practical role beyond scientific curiosity. Researchers discovered that tailoring the carbon chain and halogen types provided a way to create molecules that could react in predictable ways. As organic synthesis matured, 1-chloropentane joined the roster of standard reagents, making its way into teaching labs and industrial processes that called for a primary chloroalkane.
Product Overview
Today, 1-chloropentane stands as a primary alkyl chloride with the formula C5H11Cl. Anyone working with the compound notices its distinct, sharp odor and oily texture. Commercially, its appeal comes from its relative chemical simplicity and straightforward reactivity. Because it is structurally simple but capable of a wide array of transformations, 1-chloropentane sits in an important spot between the lower-chain chlorides like 1-chloropropane and longer, heavier molecules. Many suppliers offer it at different grades, but nearly all feature an emphasis on purity, since trace contaminants can seriously impact its behavior in fine chemical or pharmaceutical settings.
Physical & Chemical Properties
1-chloropentane appears as a clear, colorless liquid at room temperature, with a boiling point sitting around 107°C to 109°C, and a melting point well below freezing at -93°C. Its density reaches about 0.87 g/cm3, making it less dense than water and fairly easy to separate in two-phase extractions. It doesn’t mix well with water, which reflects the relationship between its nonpolar five-carbon chain and the polar, but small, chlorine atom. In the lab, other solvents like ether or hexane blend with it effortlessly, enhancing its appeal. This compound isn’t particularly flammable, but it still vaporizes readily, letting its characteristic odor travel throughout the workspace if not handled in a fume hood. Reactivity-wise, it performs as a classic alkyl halide — it readily participates in SN2 and E2 mechanisms, which forms the backbone of its use in synthesis.
Technical Specifications & Labeling
Suppliers typically provide 1-chloropentane with a purity north of 98%, along with data on refractive index (usually close to 1.410 at 20°C), and often GC analysis breakdowns. Packaging always highlights its flammable and harmful nature, using clear hazard pictograms in line with GHS standards. Labels stress the need to avoid inhalation and skin contact because of the risk of central nervous system effects and irritation. Shipping and storage adhere to UN number 1993 or 1123, with chemical-resistant seals and tight caps designed to restrict vapor loss. Some suppliers include trace impurity data such as water content or residual salts for highly sensitive synthetic routes, where small contaminants might make or break a process.
Preparation Method
The industrial route for 1-chloropentane stems mostly from the direct chlorination of pentane or the reaction of 1-pentanol with thionyl chloride (SOCl2), phosphorus trichloride, or hydrochloric acid. In many labs, converting 1-pentanol using SOCl2 remains a trusted method, simply because it minimizes side reactions. The overall reaction swaps a hydroxyl group for a chloride, often in the presence of a base like pyridine to mop up acidic byproducts. For those aiming at high-throughput or green chemistry protocols, other halogenating agents or even electrochemical approaches started grabbing some attention in the last decade or so. Despite that, the thionyl chloride route still dominates the field, mainly for cost and reliability.
Chemical Reactions & Modifications
Chemists prize 1-chloropentane for the way it launches SN2 reactions with nucleophiles, creating a diverse set of five-carbon derivatives. Swap out the chlorine with an azide, amine, or thiol, and each reaction turns into a useful transformation for building drug molecules, agricultural chemicals, or new materials. Under basic conditions, it sometimes veers towards E2 elimination, yielding pentenes if a lab needs an alkene intermediate. Coupling reactions show up too, particularly in recent work where palladium catalysis links 1-chloropentane to aromatic partners. In my own projects, I've used it for alkylating carbanions – it’s solid at delivering its pentyl group with decent yields, though the chlorine must be coaxed a bit since it isn't as reactive as a bromide or iodide. Storage in light-protected bottles keeps it from slowly decomposing or forming traces of HCl, which could compromise those sensitive reactions down the process line.
Synonyms & Product Names
Some catalogs list 1-chloropentane as n-pentyl chloride or amyl chloride, with “1-chloropentane” often holding the position as the IUPAC-preferred name. The “pentyl chloride” moniker survives from days when common names rather than formal nomenclature held sway. Occasionally, trade suppliers might list it under abbreviations or catalog numbers, but these rarely make their way into scientific literature or regulatory filings.
Safety & Operational Standards
Handling 1-chloropentane calls for gloves, goggles, and a good fume hood. Even a whiff too close to the bottle can provoke dizziness and headaches, so strict attention to ventilation matters in both teaching and professional labs. Spills demand immediate cleanup with absorbent materials, followed by washing down with plenty of water — not just a cursory wipe. Regular training and chemical hygiene protocols make a big difference, and I always recommend double-checking container tightness before putting anything on a storage shelf. Enforcing those habits means exposure incidents stay vanishingly rare, even as volumes handled increase in scale-up work.
Application Area
The uses for 1-chloropentane sweep across research and industry. Synthetic organic chemistry often employs it to introduce pentyl chains into target molecules. In pharmaceuticals, that pentyl group can improve the solubility or effectiveness of new compounds, and alkylating agents like 1-chloropentane may serve both during route scouting and final manufacturing. Agricultural research taps it for making new pesticides or plant growth regulators. The compound shows up in surfactant and lubricant research, too, altering the way molecules assemble at interfaces. My encounters have come mostly in synthetic routes leading toward flavors or intermediates, since it brings five carbons and a manageable leaving group in a single molecule. A few studies even look at its role in preparing new stationary phases for chromatography, highlighting its adaptability across research goals.
Research & Development
Interest in refining safer and greener methods for making and using 1-chloropentane continues to grow. The search for less hazardous halogenating agents inspires graduate students and chemists alike, since ditching thionyl chloride or phosphorus-based reagents lowers the toxic footprint of many procedures. Some work investigates bio-based routes to pentyl chlorides, feeding into the broader movement for sustainable chemistry. Attention also goes towards how changing the leaving group or chain length adjusts product selectivity and process economics — hot topics at conferences and in industry partnerships. Publications from the last five years show a healthy level of innovation, from new use cases in medicinal chemistry to unique coupling approaches for making specialty materials. This progress keeps the molecule relevant amid the rush toward less-polluting and higher-yielding reactions.
Toxicity Research
Toxicologists haven’t shied away from examining 1-chloropentane. It's clear that inhaling even moderate concentrations causes dizziness and sometimes CNS depression, especially if a spill isn't contained or a bottle is left open. Animal studies point to potential liver and kidney strain after prolonged exposure, and the compound poses a risk to aquatic life if dumped down the drain. Real-world incidents where poor ventilation or broken seals led to acute toxic effects drive home how easily issues can emerge, even with experience on hand. Standard practice involves storing the chemical in ventilated flammable cabinets and double-bagging any waste bound for disposal. Ignoring these habits leads to increased risk, far more quickly than most expect.
Future Prospects
New research trends hint at changing the way chemists approach 1-chloropentane and related alkyl chlorides. Shifting focus towards green chemistry pushes for alternative synthesis strategies that produce less waste and rely on less hazardous starting materials. Intersection with biotechnology may bring pentyl chain introductions via engineered enzymatic processes, though this remains on the horizon. Advances in organometallic chemistry and catalysis keep broadening its application base, letting the molecule serve roles in making materials for electronics, pharmaceuticals, or sustainable polymers. Looking ahead, the compound’s core versatility as a robust, straightforward alkylating agent all but guarantees continued relevance — provided that handlers and innovators address the long-standing safety, environmental, and toxicity concerns along the way.
Exploring Where 1-Chloropentane Fits In
1-Chloropentane looks easy to miss in a catalog of chemicals, overshadowed by more famous compounds. Digging into how it touches real work and daily products, its role stretches from classic chemistry experiments to quiet contributions in industry. I’ve spent enough hours in cramped college labs to recognize its unmistakable, sweetly sharp smell, a marker that something interesting sits in the flask.
Why Batch After Batch Chooses This Compound
At its core, 1-Chloropentane is an alkyl halide. That means it opens doors in organic synthesis that simple pentane can’t. I watched instructors pick this compound again and again for teaching the SN2 reaction. In labs, many budding chemists use it to synthesize higher alcohols or amines, reacting through its accessible chlorine atom. Years later, talking with plant chemists, I found its value doesn’t stop with education.
Manufacturers of specialty chemicals often choose 1-Chloropentane as a starting block in creating lubricants, flavor additives, and certain pharmaceuticals. It does straightforward work—transferring that chlorine to build more complex molecules. The flexibility it gives makes it a backbone ingredient for intermediate production.
Inside Industrial Processes and Research Labs
Chemical companies rely on 1-Chloropentane for designing new compounds, especially for research and development. Formulations for some pesticides and herbicides owe their structure to reactions kicked off using this alkyl halide. It helps build larger, more sophisticated molecules that go on to make a real difference in agriculture.
Some industries apply it as a solvent for organic reactions. You won’t see bottles of it lined up at hardware stores, but inside chemical warehouses, drums labeled with its precise name mark it out for specialized roles. In research, its straightforward reactivity helps chemists test reaction mechanisms and invent new routes to promising drugs.
Not Without Its Risks
Handling 1-Chloropentane never felt casual to me, even in supervised lab settings. Contact can irritate the skin or eyes, and fumes tickle the nose in a way you remember. Worries about accidental spills or inhalation aren’t just red tape—they reflect real hazards. The Global Harmonized System flags it for its flammability and toxicity, so any chemist working with it needs to respect these warnings.
Care for safe storage stands out here. Well-ventilated shelves, chemical fume hoods, and proper gloves become daily routine. For industries that produce in bulk, environmental safety joins the mix. Proper waste treatment means separating this compound from water and soil, preventing it from affecting local communities.
Finding Balance in Practical Use
Balancing the need for progress with the need for safety isn’t a new story, but it plays out lining the walls of every lab and plant that works with chemicals like 1-Chloropentane. Regulations can help by setting sensible exposure limits and requiring staff training. This foundation lets researchers and workers unlock the compound’s benefits—as a springboard to medicines, crop innovations, and specialty additives—while minimizing risk. In my view, pairing solid science with genuine caution builds trust, not just in products, but in the hands that make them.
Digging Into the Structure
Not everyone spends their days thinking about organic chemistry, but there’s a quiet satisfaction in breaking down a compound like 1-chloropentane. This molecule holds its own in labs and industry, showing off how reshaping a hydrocarbon chain can change a substance's nature. 1-chloropentane comes from a family of compounds named haloalkanes, where a halogen atom, in this case chlorine, finds its way into a straight carbon chain. In school, I would sometimes wonder why we fussed over formulas and diagrams for these seemingly simple substances. The answer showed up when I started working in real-life settings—knowing what's in a compound, mole for mole and atom for atom, keeps science grounded.
The Numbers Behind the Name
Pull apart the name “1-chloropentane”—the “pentane” part points to five carbons linked up in a row. The “1-chloro” tag means a chlorine atom sits at the very first carbon in that line. Think about pentane: five carbons and twelve hydrogens, formula C5H12. Swap one hydrogen on the end for a chlorine atom and you line up with C5H11Cl. This is more than number play. Every hydrogen or chlorine might sound replaceable, but their swap shapes everything from boiling point to the way a molecule reacts with others.
Where It Shows Up and Why the Formula Matters
Back in undergrad labs, we ran reactions where 1-chloropentane became a key ingredient or a product, depending on the experiment. This wasn’t just for busy work; making compounds like this one paves the way for medicines, plastics, and solvents. Even outside chemistry, the shape and formula of a molecule speak volumes. The safety data sheet that comes with a drum of 1-chloropentane traces right back to C5H11Cl. Workers rely on that to gauge how it interacts with other substances, or if it needs special storage. It’s not only the folks in lab coats paying attention—anyone handling chemicals should know what they’re dealing with and how each molecule might behave.
Room for Mistakes and the Need for Care
Mixing up formulas can create unpleasant surprises. Misreading 1-chloropentane’s makeup as C5H12Cl by accident throws off entire reaction plans or safety calculations. In chemical manufacturing, missing by just one atom may mean a different product comes out, or an unforeseen risk appears. In my experience, labs with the cleanest records kept sharp eyes on the fine print, never treating chemical formulas as afterthoughts. Some rushed workplaces ran into trouble from skimming over details like this small difference.
Bridging the Lab and Real Life
Molecular formulas like C5H11Cl don’t stay locked in textbooks. Each symbol and subscript stands for a physical component you can weigh, measure, and put to work. A good chemistry education drills home that these letters and numbers stay tied to results—both in what gets made and how it gets managed. The best bet for safety, reliable results, and smart science is to treat every detail as purpose-built, right down to each hydrogen or chlorine. Taking shortcuts just ends in clean-ups and corrections, not progress.
Wrapping Safety and Learning Together
Handling 1-chloropentane or any similar compound, a strong grasp of its formula is protection. It means the right precautions, the right storage, the right reaction setups. Nobody benefits from vague ideas about what’s in a container or test tube. For those stepping into the world of chemistry, taking this detail seriously builds up habits that last across careers. The formula of 1-chloropentane, C5H11Cl, shows how one small substitution echoes through the whole science—real, readable, and indispensable.
What Is 1-Chloropentane?
1-Chloropentane pops up in the world of solvents and industrial chemicals. It's a colorless liquid, known for its mild, sweet smell. I’ve spent time in more than one lab with bottles of this stuff keeping company with a long line of other organic compounds. Its main appeal comes from its ability to dissolve certain waxes, oils, and greases — so industries keep it handy for cleaning, degreasing, and chemical synthesis.
Looking at Toxicity and Exposure
Whenever I talk with folks about chemicals at work, safety always comes up fast. For 1-chloropentane, most worry centers on its vapor. Breathe too much, and irritation kicks in pretty quick — headache, dizziness, and maybe nausea after a longer whiff. My own experience with solvents tells me to stay cautious with skin as well. This isn’t something to splash around with bare hands; redness or dryness can follow.
Studies on rats and mice laid the groundwork for what scientists know. Exposure over time caused signs of nerve stress and affected organ health at higher doses. Researchers also keep tabs on whether chemicals like this could have long-term effects, such as impacting liver enzymes or causing reproductive effects. At this point, cancer links aren’t strong for 1-chloropentane, but the limited research isn’t a free pass.
International workplace hazard agencies, including OSHA in the United States, focus on common solvents, but 1-chloropentane hasn’t landed a concrete legal limit in the air. Still, it belongs in the larger group of simple chlorinated hydrocarbons, plenty of which do carry firm rules because of chronic toxicity risks.
Environmental and Community Impact
With solvents like this, spills don’t stay put. 1-Chloropentane evaporates easily, so a careless pour slips into the air. Concerns about groundwater turn real if leaks happen, since chlorinated organics rarely break down quickly. Fish and aquatic life handle these sorts of chemicals poorly, and local ecology can take a hit if bigger spills reach streams or rivers.
Communities living near chemical plants often worry most. Living near a place that stores bulk solvents changes how you see safety news. I’ve talked with people whose wells had to be tested after solvent leaks. Peace of mind fades pretty quick if water turns suspicious and regulators are slow to act.
Precautions in Daily Handling
Most labs or industrial shops keep risk low with strong ventilation, gloves, and eye protection. Using it outdoors, or near a flame, brings trouble because it catches fire at modest temperatures. Simple common sense — paired with safety data sheets — keeps mishaps rare. Still, not everyone has up-to-date training or reads labels carefully, raising the chances for accidents.
Keeping smaller amounts for short jobs and storing the bulk in tighter, locked containers cuts down on spills. General awareness — reading the label, following storage guidelines, and using fresh gloves — goes a long way. I've seen plenty of incidents avoided just by people slowing down and checking the surroundings before opening a bottle.
Better Solutions Moving Forward
Plenty of places now look for safer solvent replacements, especially for routine cleaning or degreasing. Engineering controls, safer product swaps, and regular safety education give workers confidence to handle 1-chloropentane, or anything else that comes through the dock doors. Companies able to track and trace their chemical storage — even with something as common as a solvent — build trust with employees and nearby households. Less risk, less anxiety, more peace of mind.
Looking Closer at 1-Chloropentane
I’ve spent quite a bit of time in chemistry labs and warehouses. Some chemicals just have an attitude—1-chloropentane is one of them. At first glance, a simple clear liquid might not look like much. Real life says otherwise. Even a single mishap with this solvent can create a headache, if not worse. So, getting the storage and handling right matters.
Why Proper Storage Isn’t Optional
1-chloropentane doesn’t joke around with flammability. Its flash point—that’s the lowest temperature where fumes can catch fire—hovers around 30–34°C. Most lab rooms and storage spaces in summer can swing into that range without much effort, so a forgotten jug too close to any heat source spells trouble. Experience teaches that storing 1-chloropentane in a dedicated flammables cabinet, away from sunlight, radiators, or any spark-producing machinery, is not just recommended—it’s common sense.
Glass or high-grade polyethylene containers work best. Metal containers can corrode or react. Vapor-tight sealing prevents the sometimes-pungent fumes from filling up the room. Not only do the vapors ignite easily, they cause irritation—eyes, nose, even the lungs if you’re unlucky enough to breathe deep around an open bottle.
Handling in the Real World
Personal protective equipment isn’t just for the rulebook here. Splash goggles, chemical-resistant gloves, and a lab coat meaningfully limit skin exposure. People sometimes underestimate how easily this compound soaks through thin gloves. If you work with solvents as much as I have, you know that one accident can put someone out of commission with a nasty rash.
Work with 1-chloropentane always involves solid ventilation. Fume hoods serve as the gold standard. Lab directors obsess over airflow for a reason. It’s not just about comfort. Chronic exposure to chlorinated solvents—like 1-chloropentane—has tied into central nervous system effects, headaches, dizziness, and longer-term risks that nobody wants to roll the dice on.
Safeguards in Storage
Labeling tells the story. If you glance around a tight chemical cupboard, you want to spot every risk without squinting. Sticking bold hazard tape or chemical warning labels on containers keeps everyone honest and safe. Spills happen all the time: proper signage helps bystanders know what not to touch.
Secondary containment—like spill trays—catches leaks. I’ve seen more than one careless moment turn into a carpet nightmare because a cracked bottle dripped just enough to threaten an entire work area. Don’t leave 1-chloropentane in glass pipettes or flasks long-term, either. Even thick-walled flasks have limits if someone knocks them off a counter.
Thinking About Alternatives
Sometimes, finding a safer solvent can be worth the hassle. Green chemistry pushes for less hazardous substitutes, but 1-chloropentane keeps showing up in research for a reason. If it’s unavoidable, lock down processes. Run regular safety audits and make chemical inventory checks a habit. You learn which shelves run hot, which corners stay cool, and which lab mates cut corners when no one’s looking.
Training can’t just be a sign-off on paperwork. Every new student, technician, or operator benefits from a walkthrough with real, used containers. Nothing replaces learning what a dense 1-chloropentane vapor cloud smells like before a real emergency hits. Fire extinguishers marked “Class B” for flammable liquids stay near workstations, because you never want to discover too late that the wrong one sits by your bench.
Building a Safer Lab Culture
Making safety stick isn’t about one set of rules or a quarterly reminder. For 1-chloropentane and others like it, build habits through hands-on lessons and reminders. Shortcuts make bad headlines. A sturdy cabinet, a sharp eye for vapor leaks, and proper gear keep labs running and workers healthy.
Chemistry in Daily Life
A lot of people rarely think about the physical properties of chemicals, but they drive practical choices in labs, industries, and classrooms. Take 1-chloropentane, for example. This compound sits in a family of chlorinated hydrocarbons, used in all sorts of basic organic synthesis. Here, the boiling point stands as more than one number on a data sheet—it shapes how professionals handle and store the substance, and even what safety gear they pick out before heading into the lab.
Getting to the Point: 1-Chloropentane Boiling Point
1-Chloropentane boils at about 107°C (225°F). It might sound like a small detail, but as someone who’s worked in both teaching labs and applied research, I can say that boiling points help you pick the right heating equipment and control ventilation. In the chemistry world, lower boiling points spell out a higher risk of vapors in the workspace. You end up with stricter measures for storage and spill clean-up.
Why the Boiling Point Really Changes Handling
A boiling point near 107°C puts 1-chloropentane out of reach of typical room temperatures, but pretty close to what you see in many lab processes. Unlike pentane, which boils around 36°C and disappears if you even look at it sideways, 1-chloropentane keeps its cool longer. Still, heated baths or open flames can push it quickly from liquid to vapor. Inhaling too much vapor, even from “harmless-appearing” organochlorines, can really mess up your health, leading to headaches, dizziness, or worse with long-term exposure.
It shows up outside the lab too. Cleaners and degreasing agents sometimes use related compounds. Even if you’re handling small amounts, like dropping some in a reaction to see a new compound form, the temperature at which a substance vaporizes tells you when you need goggles, gloves, and a fume hood.
Data with Purpose: Comparing Other Chlorinated Compounds
For reference, 1-chlorobutane boils at about 77°C, and 1-chlorohexane hits about 133°C. Adding a single carbon atom usually bumps the boiling point a notch, but the chlorine keeps the number reasonable. Among all these, 1-chloropentane ends up as a middle-of-the-road solvent: it doesn’t float away under your nose at room temp, but it doesn’t resist heat for long either.
Making Safer Choices in Chemistry
Some researchers chase ever-faster reactions without pausing to ask what happens if the solvent catches fire or releases toxic fumes. In my own work, I’ve seen the best chemists insist on triple-checking boiling points before even weighing out a gram, especially once you factor in contamination or old glassware. Storing these chemicals in temperature-controlled environments cuts down risks. Thicker gloves and well-maintained fume hoods cut them even further.
Fact-based guidelines, published by governments and leading chemical companies, stay rooted in years of testing and heavy-duty review. If a label says 107°C, you can trust thousands of hours went into nailing it down. These numbers become a compass, guiding safer handling, better results, and a healthier environment for everyone involved in the experiment.
| Names | |
| Preferred IUPAC name | 1-chloropentane |
| Other names |
n-Pentyl chloride
Amyl chloride Pentyl chloride |
| Pronunciation | /ˌwʌn.klɔː.rəʊ.pɛnˈteɪn/ |
| Identifiers | |
| CAS Number | 543-59-9 |
| Beilstein Reference | 1209247 |
| ChEBI | CHEBI:82252 |
| ChEMBL | CHEMBL15461 |
| ChemSpider | 8338 |
| DrugBank | DB13810 |
| ECHA InfoCard | ECHA InfoCard 100.006.182 |
| EC Number | 203-937-5 |
| Gmelin Reference | 7801 |
| KEGG | C01831 |
| MeSH | D017357 |
| PubChem CID | 11255 |
| RTECS number | RZ6900000 |
| UNII | 2E0LQ4Q69N |
| UN number | UN1123 |
| Properties | |
| Chemical formula | C5H11Cl |
| Molar mass | 120.62 g/mol |
| Appearance | Colorless liquid |
| Odor | Penetrating odor |
| Density | 0.87 g/mL |
| Solubility in water | Insoluble |
| log P | 2.67 |
| Vapor pressure | 3.6 kPa (at 20 °C) |
| Acidity (pKa) | 16.0 |
| Basicity (pKb) | pKb > 14 (very weak base) |
| Magnetic susceptibility (χ) | -7.41 × 10⁻⁵ |
| Refractive index (nD) | 1.406 |
| Viscosity | 0.725 mPa·s (at 25 °C) |
| Dipole moment | 2.03 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 217.9 J⋅mol⁻¹⋅K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | –142.6 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | -3507.7 kJ/mol |
| Pharmacology | |
| ATC code | Not assigned |
| Hazards | |
| GHS labelling | GHS02, GHS07 |
| Pictograms | GHS02, GHS07 |
| Signal word | Danger |
| Hazard statements | H225, H315, H319, H335 |
| Precautionary statements | P210, P261, P280, P301+P312, P303+P361+P353, P305+P351+P338, P370+P378, P403+P235 |
| NFPA 704 (fire diamond) | Health: 2, Flammability: 3, Instability: 0, Special: - |
| Flash point | 62 °F (17 °C) |
| Autoignition temperature | 160 °C |
| Explosive limits | 1.1–7.2% (in air) |
| Lethal dose or concentration | Lethal dose or concentration: LD50 oral (rat): 4150 mg/kg |
| LD50 (median dose) | LD50 (median dose): Oral, rat: 4,080 mg/kg |
| NIOSH | CN8400000 |
| PEL (Permissible) | Not established |
| IDLH (Immediate danger) | 500 ppm |
| Related compounds | |
| Related compounds |
Pentane
1-Bromopentane 1-Iodopentane 1-Fluoropentane 2-Chloropentane 3-Chloropentane |
