2-Chloropropane: More Than a Simple Halogenated Hydrocarbon
Historical Development
For chemists who grew up watching the expansion of organic chemistry in the twentieth century, 2-chloropropane feels like a familiar neighbor. Early synthetic work with small chloroalkanes hinged on lab techniques that seemed wild by modern safety standards. Even in the 1940s, students poured over glassware with open flasks and barely-there gloves, distilling compounds like 2-chloropropane as a path to broader knowledge of reactivity and substitution. Industries tinkered with halogenated compounds, chasing better refrigerants, solvents, and starting materials. Along the way, researchers learned that chlorinated hydrocarbons could impact atmospheric chemistry and human health in complicated ways. This led to tighter industrial controls and a sharper focus on what happens to these compounds after their useful life ends.
Product Overview
2-Chloropropane goes by many names—iso-propyl chloride, isopropylchloride, 2-propyl chloride—and slides in as a colorless, volatile liquid that delivers a sharp, ether-like odor. In the most basic sense, it’s built from a propane core, swapping out one hydrogen atom for a highly reactive chlorine atom. This small change opens the door to a whole range of substitution and elimination reactions, making the compound a valuable stepping stone for making more specialized molecules. The demand for 2-chloropropane doesn’t measure up to giants like chloroform, but you’ll find it used across research labs and in some manufacturing lines—notably as a building block for pharmaceuticals, agrochemicals, and functional materials.
Physical & Chemical Properties
The physical traits of 2-chloropropane make it a bit tricky to handle without the right gear. It boils at roughly 35°C, so even a modest temperature rise can fill a room with fumes. The density lands at about 0.87 g/cm³, and it does not mix well with water, hanging low in organic phases during extractions. The vapor exerts pressure quickly as temperatures climb, driving the need for ventilated spaces and solid containment. Chemically, it stands ready to shuffle its groups in substitution and elimination reactions, favoring unimolecular (SN1) or bimolecular (SN2) mechanisms depending on the reaction partner and solvent. Under uncontrolled heat, it can break down into hydrochloric acid and other nasties, which is why thermal stability gets extra attention in storage settings.
Technical Specifications & Labeling
Industrial and laboratory suppliers deliver 2-chloropropane at varying purity levels, with analytical grade samples commonly exceeding 99% purity. Standards force suppliers to monitor levels of water, alcohols, and residual chlorides. Every barrel or bottle comes with hazard symbols—“Flammable,” “Harmful if inhaled,” and “Keep away from ignition sources"—bluntly warning users about both fire and toxicity hazards. Material safety data sheets go deeper, tabulating boiling and melting points, flash points (typically around −4°C), fire-fighting methods, and the countless details regulators demand for responsible workplace safety.
Preparation Method
Synthesis leans on classic routes—starting with isopropanol and treating it with hydrogen chloride gas in the presence of a dehydrating agent, often concentrated sulfuric acid. The process stirs up a lively stream of gas and a two-phase liquid mix, demanding cool heads and a solid fume hood. Once formed, the crude product gets washed, dried, and distilled, usually under reduced pressure to hold onto as much of the volatile liquid as possible. Some production lines work up from propane, using chlorination at higher temperatures to encourage selective replacement at the middle carbon atom. Inevitably, controls are critical to avoid a mess of other chlorinated byproducts and to lower corrosion and environmental contamination risks.
Chemical Reactions & Modifications
The utility of 2-chloropropane boils down to how eager it is to hand over its chlorine atom. Push it into reaction with nucleophiles—like sodium iodide in acetone—and it swaps chlorine for iodine, serving as a textbook example in undergraduate synthesis labs. Hit it with strong bases, and it throws off hydrochloric acid as it shifts into propene, a useful olefin. Tinker with the recipe, and you can link it to amines for pharmaceuticals, build on it with metals for organometallic chemistry, or stretch its backbone for specialty elastomers. It acts, in short, as a reliable platform for quick chemical change, which matters for innovation at many scales.
Synonyms & Product Names
In catalogs and regulatory lists, 2-chloropropane appears under aliases such as isopropyl chloride, sec-propyl chloride, 2-chloropropane, and UN 2358. These alternate names show up in shipping documents, chemical supply lists, and research papers. Knowing the family tree of product names helps chemists navigate databases and international literature, where regional differences sometimes slow down a search for suppliers or regulatory advice.
Safety & Operational Standards
Handling 2-chloropropane without respect for its volatility and toxicity courts disaster. The compound lights up at the drop of a match, so proper storage far from sparks or open flames is non-negotiable. Inhalation of vapors can leave workers dizzy, short of breath, or sick, so high-grade respirators and dedicated ventilation systems make a real difference in occupational health. Industrial codes—like those from OSHA in the US or ECHA in Europe—set exposure limits and demand regular auditing. Spills bring firefighting foam and full-face protection, not a quick mop and bucket. Training matters most; reading about these risks in a data sheet is no substitute for hands-on drills and clear emergency plans.
Application Area
Bulk chemistry production uses 2-chloropropane as a link in longer synthesis chains, aiming for pharmaceuticals, herbicide intermediates, and advanced materials. Research teams draw on its reliable reactivity in mechanistic studies, sometimes as a reference compound for probing how halides leave during substitutions. A few niche uses show up in specialty solvent blends or as calibration standards. Everywhere it appears, the goal leans toward safer, cleaner, and more cost-effective routes to higher-value targets, not the consumer arena. For those of us who have worn out our fair share of nitrile gloves in chemical development, it’s a mainstay that you probably hope lurks behind a secure cabinet door rather than on a retail shelf.
Research & Development
New research often circles back to understanding and controlling side reactions, improving selectivity, and working out greener synthesis. Innovations in catalysis look to minimize waste production and avoid toxic reagents. Academic labs ask, “How can we drive reactivity higher while keeping risk lower?” The answers lie in catalyst design, process automation, real-time monitoring, and tighter regulatory compliance. Environmental chemists push for alternatives, studying the degradation of 2-chloropropane in soil and water, and assessing the formation of potentially hazardous secondary pollutants—particularly in connection with improper disposal from industrial sites.
Toxicity Research
Toxicology studies paint a picture of moderate acute toxicity. Short-term exposure causes irritation of the respiratory tract, eyes, and skin, while high doses in animal studies point toward impacts on the central nervous system and organs like the liver. Chronic effects get less attention given the relatively contained industrial use, but older data and new models alike recommend keeping workplace levels as low as possible. The chlorine atom makes metabolism in living systems worrisome at elevated exposures, and poor ventilation increases the risk of headaches, dizziness, or worse. Waste streams demand closed systems and pre-treatment before release. Environmental persistence ranks lower than heavier chlorinated compounds, but breakdown products can still present risks—pushing researchers and companies to monitor effluents and improve disposal technology year by year.
Future Prospects
The future for 2-chloropropane ties into the broader fate of chlorinated organic chemicals. Industry tends to favor compounds with clear benefits and manageable risks, so continued research aims to trim hazard profiles and cut waste. Timer-proven uses hold firm as long as regulations permit and as the economics stack up for large-scale processes. Expansion into green chemistry—using renewable feedstocks, non-chlorinated alternatives, or closed-loop systems—sits front and center for new research. Companies that have weathered decades of changing standards know that agility, transparency, and a steady eye on health and environment shape who stays in business. Today’s students hammer out reactions in controlled labs, just as chemists did generations back, but everyone feels the growing weight of accountability. With persistent innovation, the next wave of processes may cut emissions and transform both lab safety and environmental health.
A Closer Look at a Less-Famous Chemical
Not everyone has heard of 2-chloropropane, but for people working in industrial chemistry or pharmaceutical labs, it pops up more than you’d expect. I came across it myself during a stint in a small specialty chemicals firm. Someone handed me a drum labeled with its name and told me, “Handle this carefully, and make sure you use the right gloves.” From that point on, its sharp, distinct odor stuck in my memory, even though what happens after those drums leave the shipping dock is where things really get interesting.
What Makes 2-Chloropropane Useful?
This clear, flammable liquid often helps as a chemical building block. Chemists call it a "halogenated hydrocarbon," but in plain terms, that means it’s a molecule with chlorine attached to a three-carbon propane skeleton. This unique structure lets it play a role in several important chemical reactions.
Traditionally, 2-chloropropane acts as an intermediate—think of it as a halfway stop on the journey to something more complex or more useful. Factories use it to help create other chemicals, such as isopropyl alcohol and solvents. Research labs use it to study reaction pathways or, at times, as a reference material when testing instruments. In my old lab, it took part in a series of reactions leading to ingredients for everyday products. Each time someone purchased isopropyl alcohol at the pharmacy, they indirectly relied on several steps involving chemicals like this.
2-Chloropropane and the Pharmaceutical World
Some of the most fascinating applications appear in pharma. During the synthesis of active pharmaceutical ingredients, precise chemical reactions are critical. That’s where 2-chloropropane shows some value. It can help introduce a specific carbon structure, making it possible to get the desired biological effect in a drug. Not every medicine involves it, but for those that do, it can offer efficiency and purity at a key stage of the process.
In my own experience, the teams overseeing quality control watch these steps closely, knowing one misstep could lead to impurities that shouldn’t end up in a finished tablet or capsule. Regulatory guidelines set out by agencies like the FDA require thorough documentation at every move involving substances like 2-chloropropane. Companies with sloppy oversight risk both costly recalls and blown trust with their customers.
Concerns Around Use and Handling
2-chloropropane isn’t just tricky in reaction flasks; safety matters. It smells sharp and can irritate skin or eyes. I remember one colleague who got a little careless and ended up with red, itchy hands for a day. That taught everyone to double-check gloves and make sure the fume hood was working. Larger quantities bring fire risk, too, so no one should be casual about storage. In some countries, safety data on chemicals is strict, and businesses need good training and clear documentation to avoid accidents.
Looking Ahead: Safer Alternatives and Responsible Choices
Newer chemistry often aims to swap out halogenated solvents and intermediates for greener options. Universities and companies study replacements that have less impact on health and the environment. These innovations matter, because less toxic chemicals mean safer workplaces and less pollution. Sometimes, research takes inspiration from results with substances like 2-chloropropane, but pushes toward milder, safer options.
Everything I learned in my own hands-on roles—mixing solvents, cleaning up spills, tracking every transfer—underscores that chemicals with weird names often shape what ends up on store shelves. A little knowledge about these basic building blocks helps everyone make sense of why careful handling, safety, and innovation in chemical industries keep mattering year after year.
What Is 2-Chloropropane?
2-Chloropropane gets used in labs and in some chemical production processes. You’ll find it as a colorless liquid with a noticeable odor. Breathing in its vapor or letting it touch your skin comes with serious risks. Even if you work around many other chemicals, this one deserves specific attention because of its health hazards and potential for mishandling.
Why Take Extra Precautions?
Breathing in 2-Chloropropane makes your nose and throat burn and can cause coughing, headaches, or dizziness. Skin and eyes react just as quickly, leading to stinging, rashes, or persistent irritation. From what I’ve seen in industrial settings and small labs, people underestimate liquids like this. Shortcuts—like ditching gloves or skipping eye protection—felt easy at the time for some, but the aftermath of chemical burns or an asthma attack changed their minds fast.
Using the Right Gear
Gloves made from nitrile or neoprene matter here. Regular latex ones just won’t stop 2-Chloropropane from soaking through. Splash goggles go hand in hand with gloves, stopping fumes and droplets from reaching your eyes. Out in the field or the lab, one quick spill can turn into an emergency if you’re not prepared.
Lab coats and closed-toed shoes form a basic layer of defense. Open shoes or short-sleeved shirts leave skin exposed and turn simple accidents into medical issues in a hurry. Having a chemical fume hood in the workspace keeps vapors from filling the air. Even with brief use, working out in the open lets invisible fumes spread, and they’re easy to inhale without realizing it.
Proper Handling and Storage
2-Chloropropane should stay in tightly sealed containers—away from heat sources or open flames. It catches fire easily. Storing it in a cool, ventilated room reduces both fire risk and buildup of harmful vapors. I once watched someone store a bottle on top of a sunny windowsill. The bottle ended up cracked, leaking dangerous fumes, and forced an evacuation. Lesson learned.
If you do spill some, ventilate the area first, then use absorbent material meant for solvents—not just paper towels. Waste goes into specific chemical disposal containers. Never pour it down the drain or toss it in the regular trash. It harms water supplies and creates hazards for sanitation workers.
Know What to Do in an Emergency
In chemical work, accidents happen even to cautious folks. The faster you act, the better the outcome. If you splash 2-Chloropropane on your skin or in your eyes, rinse with plenty of water for at least 15 minutes. Have an eyewash station and safety shower within easy reach. Inhaling fumes sends you outside for fresh air, and lingering symptoms mean calling medical help without delay.
Training and Awareness Go a Long Way
Proper training runs circles around good intentions. Everyone on site needs clear instructions on handling, cleanup, and emergency steps. Label containers well and check safety data sheets before starting any project. Staying updated matters; chemical risks change with new information and improved gear.
Building a Culture of Safety
A workplace that talks openly about chemical risks keeps people safer over the long run. Encouraging questions and reporting near-misses helps everyone spot dangers before they turn serious. Managers who lead by wearing protective gear set the example others follow. From day one in my experience, people who respected the hazards stayed healthy and productive, while those who rolled the dice paid for it later—physically, legally, or both.
Breaking Down the Basics
I still remember my college chemistry lab sessions. The chemical names sounded like a different language. But after a few exercises, I learned they all tell a clear story. Take 2-Chloropropane. The chemical formula C3H7Cl says it all: three carbons, seven hydrogens, and a single chlorine atom. Pretty compact, but the arrangement turns out to be everything.
Plenty of fresh learners look up this compound and get hit with textbook language, but here’s what sets it apart: the chlorine bonds to the middle carbon of a three-carbon chain. Draw it out and the structure looks like this: CH3-CHCl-CH3. That’s propane with one hydrogen swapped out for a chlorine, right at carbon number two.
Understanding Why Structure Matters
Back in my lab, a change in where you stick that chlorine would totally shift how this molecule acts. Sure, it only differs from 1-chloropropane by the spot on the chain, but that’s not as trivial as it sounds. This detail transforms the chemical's physical and chemical behavior. I once spilled a little 2-chloropropane from a leaky container and got a sharp, gasoline-like smell. That’s a direct result of this structure—it’s pretty volatile and evaporates fast, thanks to the low molecular weight and limited hydrogen bonding.
Structure shapes reactivity too. In organic reactions, 2-chloropropane acts as a “secondary” alkyl halide. In my second-year organic class, we’d run SN1 and SN2 substitution reactions and spot that the middle carbon lets 2-chloropropane react faster in some cases than its straight-chain cousin. Electrons behave a little differently, bonds break more easily. Even experienced chemists might get tripped up if they miss the precise structure on a reaction scheme.
Why Does 2-Chloropropane Matter?
It pops up in more places than most folks realize. For industrial chemists, 2-chloropropane works as a solvent and as an intermediate to make other chemicals, especially pharmaceuticals and pesticides. In that world, a mistake on the placement of the chlorine can mean a failed batch, or far worse. Safety teams know that this compound, like many chlorinated hydrocarbons, brings health risks: its vapors are toxic, so solid ventilation is a must. Anyone at a chemical plant who skips this step is gambling with their lungs.
There’s also the chance 2-chloropropane can cause environmental headaches. It sticks around in air and water, and won’t break down so quickly. Contamination once hit a nearby industrial zone here, and the cleanup bill wasn’t small. You don’t need to be a scientist to grasp how vital strict handling and containment rules are. These trouble spots push companies to switch to greener, safer chemicals whenever possible.
Working Toward Better Solutions
Let’s face it—chemistry has built a lot of our comforts, but the price means taking responsibility. Industries are shifting to limit their use of compounds like 2-chloropropane, subbing in less persistent solvents or designing reactions that cut out the need for toxic chlorinated intermediates. Regulators demand better reporting of emissions, and researchers constantly chase cleaner paths. I once joined a team scrubbing vapor from an old plant using carbon filters; the difference in air quality was measurable in hours.
Understanding the fine details—right down to the carbon where a chlorine atom lands—puts more power in our hands to create safer chemicals and protect our surroundings. That starts with getting the formula and structure right every single time.
Understanding 2-Chloropropane’s Hazards
2-Chloropropane, a clear and flammable liquid, lands under substances you don’t want to store without a plan. One whiff tells you it doesn’t belong in the same room as snacks or open flames. Breathing in its vapors can cause irritation, and contact with skin might set off a rash. That pungent, sharp odor gives away its presence quickly. Not giving it the respect it deserves could spell trouble, so safe handling turns into a matter of protecting both people and property.
Storing 2-Chloropropane the Right Way
Experience in chemical storage labs and warehouses highlights the importance of sturdy, purpose-built containers. Using anything but sealed, corrosion-resistant drums or bottles only invites leaks and accidents. Metal cans make a good choice, especially if lined with a material that can stand up to chlorinated solvents. Glass works too, as long as it’s kept far from the action and away from sunlight. Plastic containers may crack or corrode over time, especially if the formulation isn’t up to task, so they rarely get picked for long-term storage.
Set those containers in a spot with lots of ventilation. Vapors from 2-Chloropropane drift and hang in the air if left unchecked, which turns a closed room into a hazard zone. A fume hood or a storage area with dedicated exhaust fans drops the risk of unwanted buildup. Every person who’s worked with volatile chemicals in tight spaces knows the sting of strong vapors—it’s never worth the shortcut.
Temperature and Fire Safety
Fires remain the biggest concern. This solvent lights up easily, and that means static sparks, pilot lights, and phone chargers should all stay out of the storage area. The room shouldn’t get warmer than room temperature, and installing temperature monitors gives you a heads up if things start to heat up. Some sites go a step further and include sprinklers and fire-resistant storage cabinets, the kind marked with glossy warning labels. Those labels aren’t for looks. Emergency crews rely on accurate information to respond fast and safely.
Segregation and Labeling
Mixing chemicals has a history full of horror stories. 2-Chloropropane blends badly with strong oxidizers, acids, and several common cleaning agents. Storing it beside bleach or nitric acid sets the stage for disaster. Keep it on shelves away from those types of substances, and post clear signage. Containers should wear bold, readable labels, listing contents, hazards, and the date received or filled. Spot-checking every so often prevents mix-ups, and seasoned staff never skip this step.
Spill Response and Equipment
Leaky containers or toppled bottles show up from time to time, despite best efforts. Absorbent pads and spill kits should stay within arm’s reach of every storage spot. These need to handle chlorinated solvents, not just water-based spills. Anyone working near the storage area deserves protective gloves, eye shields, and well-fitted masks. Training makes all the difference—every person who handles chemicals ought to know the drill for minor spills and knows who to call for anything bigger.
Legal and Environmental Considerations
Local rules govern how much can sit on site and how it’s disposed. Following these isn’t just about avoiding fines. Mishandling 2-Chloropropane risks contamination of air and groundwater, dragging out problems that last for years. Tracking inventory, checking expiry dates, and logging any shipment or disposal activity shows you’re taking the responsibility seriously. That attention to detail protects more than the company’s reputation—it keeps whole communities safe.
Building a Culture of Caution
Safe storage of 2-Chloropropane means more than sticking it on a shelf and walking away. It calls for attention to detail, respect for the hazard, and buy-in from everyone who works near it. From experience, shortcuts breed problems, and vigilance meets every standard worth following. Safety grows from clear labels, proper ventilation, and the right gear—not luck or wishful thinking.
What Is 2-Chloropropane?
2-Chloropropane belongs to the world of organic chemicals and comes across as a colorless, flammable liquid. It often pops up in chemical processing and sometimes industrial solvents. Sensible folks rarely handle it unless they're wearing gloves and lab coats. Its faint, almost sweet odor doesn’t give away much about the risks beneath the surface.
What Science Says About Health Risks
Nothing stands out like a chemical that can evaporate into indoor air or stick around on surfaces. Inhaling a strong whiff of 2-chloropropane won’t feel pleasant. Breathing it in can bring on headaches, dizziness, or irritation to the eyes and nose. Skin contact leaves behind redness and occasional blistering. Sometimes, a splash in the eye means days of stinging. Doctors often point to the liver and kidneys when talking about chemical exposures, and with 2-chloropropane, these organs take most of the stress. Long-term or high-level exposure, even unintentional, can build up risks to organs over time. Studies in animals show damage after repeated dosing, though it’s less common to see people handling enough of this stuff to match those levels.
Environmental Impact: More Than Meets the Eye
Runoff and accidental spills highlight the ways chemicals reach the wider environment. 2-Chloropropane can travel easily through soil, winding up in groundwater. Once there, it doesn’t break down quickly and may linger, giving plants and animals more time to absorb it. In streams, it tends to float away, but the harm comes in how it can affect fish and smaller aquatic life. My time spent walking creek beds behind urban factories left me with little doubt: toxic runoff changes everything. In high enough concentrations, this chemical can stunt fish growth and shake up the food chain. Once poisons find their way into water, they return to people — think wells, drinking water, and the food we catch or grow nearby.
Industry and Regulation Steps In
Few things motivate industry like clear rules. Agencies such as OSHA and the EPA keep a close watch on volatile organic compounds like 2-chloropropane. There are set limits on how much can float around in factory air. Companies working with these chemicals carry out air quality checks, train workers, and install exhaust systems. Spills get reported and cleaned up fast under strict guidelines. Industrial hygiene teams often carry personal air monitors, which beep loud enough to catch anyone’s attention. Still, not every shop meets these standards, and smaller facilities can cut corners — sometimes with real consequences.
Reducing the Danger
Labs use fume hoods for a reason — controlling what people breathe in turns out to be the single best method of prevention. Alternatives to volatile solvents deserve more love in the workplace, and simple switches in chemistry or process can shrink usage. Wearing gloves and goggles sounds simple but always makes a difference. My own experience in a research lab taught me to keep a close inventory, check labels twice, and make sure lids stay tight. Regulations matter, but a strong safety culture in every facility delivers long-term results.
Better Choices, Healthier Habitats
Chemicals like 2-chloropropane raise big questions about what we value: short-term gains or the promise of a cleaner, safer future. It pays to ask whether a substitute would work just as well. Personal safety and a clean environment connect more closely than most people believe. Reducing exposure at work, tighter waste controls, research into greener alternatives — these steps bring down risks for both people and the planet.
| Names | |
| Preferred IUPAC name | 2-Chloropropane |
| Other names |
Isopropyl chloride
2-Propyl chloride sec-Propyl chloride Isopropylchloride |
| Pronunciation | /tuːˌklɔːrəˈproʊpeɪn/ |
| Identifiers | |
| CAS Number | 75-29-6 |
| Beilstein Reference | 1200405 |
| ChEBI | CHEBI:15610 |
| ChEMBL | CHEMBL15914 |
| ChemSpider | 7787 |
| DrugBank | DB02260 |
| ECHA InfoCard | 100.006.820 |
| EC Number | 200-934-7 |
| Gmelin Reference | 5837 |
| KEGG | C02626 |
| MeSH | D017374 |
| PubChem CID | 6566 |
| RTECS number | TX9275000 |
| UNII | R8I96PZ62P |
| UN number | UN2357 |
| Properties | |
| Chemical formula | C3H7Cl |
| Molar mass | 78.54 g/mol |
| Appearance | Colorless liquid |
| Odor | Sweetish odor |
| Density | 0.872 g/mL at 25 °C |
| Solubility in water | Insoluble |
| log P | 1.98 |
| Vapor pressure | 5.0 atm (20 °C) |
| Acidity (pKa) | pKa ≈ -3.7 |
| Magnetic susceptibility (χ) | -8.41 × 10⁻⁶ cm³/mol |
| Refractive index (nD) | 1.375 |
| Viscosity | 0.41 mPa·s (20 °C) |
| Dipole moment | 2.05 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | (276.3 J·mol⁻¹·K⁻¹) |
| Std enthalpy of formation (ΔfH⦵298) | -134.3 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | –2056.7 kJ/mol |
| Hazards | |
| GHS labelling | **GHS02, GHS07** |
| Pictograms | GHS02,GHS07 |
| Signal word | Danger |
| Hazard statements | H225, H319, H336, H315 |
| Precautionary statements | P210, P304+P340, P403+P233, P501 |
| NFPA 704 (fire diamond) | 1-2-0 |
| Flash point | -32 °C |
| Autoignition temperature | 460 °C |
| Explosive limits | 2-10% |
| Lethal dose or concentration | LD₅₀ (oral, rat): 1800 mg/kg |
| LD50 (median dose) | LD50 (median dose) of 2-Chloropropane: "9600 mg/kg (rat, oral) |
| NIOSH | SN2980000 |
| PEL (Permissible) | Not Established |
| REL (Recommended) | **10 ppm (40 mg/m3)** |
| IDLH (Immediate danger) | 500 ppm |
| Related compounds | |
| Related compounds |
1-Chloropropane
2-Bromopropane 2-Iodopropane Isopropanol Propane Isopropyl chloride |
