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3-Methylpentane
3-Methylpentane
3-Methylpentane
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3-Methylpentane
Skeletal formula of 3-methylpentane
Skeletal formula of 3-methylpentane
Ball and stick model of 3-methylpentane
Ball and stick model of 3-methylpentane
Spacefill model of 3-methylpentane
Spacefill model of 3-methylpentane
Names
Preferred IUPAC name
3-Methylpentane[1]
Identifiers
3D model (JSmol)
1730734
ChEBI
ChEMBL
ChemSpider
ECHA InfoCard 100.002.257 Edit this at Wikidata
EC Number
  • 202-481-4
MeSH 3-methylpentane
RTECS number
  • SA2995500
UNII
UN number 1208
  • InChI=1S/C6H14/c1-4-6(3)5-2/h6H,4-5H2,1-3H3 checkY
    Key: PFEOZHBOMNWTJB-UHFFFAOYSA-N checkY
  • CCC(C)CC
Properties
C6H14
Molar mass 86.178 g·mol−1
Appearance Colorless liquid
Odor Odorless
Density 664 mg mL−1
Melting point −162.8 °C; −261.1 °F; 110.3 K
Boiling point 62.9 to 63.7 °C; 145.1 to 146.6 °F; 336.0 to 336.8 K
Insoluble
log P 3.608
Vapor pressure 18.0 kPa (at 17 °C)
8.8 mol Pa−1 kg−1
−75.52·10−6 cm3/mol
1.376
Thermochemistry
191.16 J K−1 mol−1
292.5 J K−1 mol−1
−203.0 – −201.0 kJ mol−1
−4.1608 – −4.1590 MJ mol−1
Hazards
GHS labelling:
GHS02: Flammable GHS07: Exclamation mark GHS08: Health hazard GHS09: Environmental hazard
Danger
H225, H304, H315, H336, H411
P210, P261, P273, P301+P310, P331
Flash point −7 °C (19 °F; 266 K)
278 °C (532 °F; 551 K)
Explosive limits 1.2–7.7%
NIOSH (US health exposure limits):
PEL (Permissible)
 none[2]
Related compounds
Related alkanes
Related compounds
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☒N verify (what is checkY☒N ?)

3-Methylpentane is a branched alkane with the molecular formula C6H14. It is a structural isomer of hexane composed of a methyl group bonded to the third carbon atom in a pentane chain. It is of similar structure to the isomeric 2-methylpentane, which has the methyl group located on the second carbon of the pentane chain.

As of early 1990s, it was present in American[3] and European[4] gasoline in small amounts, and by 2011 its share in US gas varied between 1.5 and 6%[5] It has close research and motor octane numbers of 74.5 and 74.3.[6]

References

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3-Methylpentane

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from Grokipedia
3-Methylpentane is a branched-chain with the molecular formula C₆H₁₄. It is a of , featuring a backbone with a attached to the third carbon atom, and its systematic IUPAC name is 3-methylpentane. This compound appears as a colorless, volatile with a mild, gasoline-like at . Key physical properties include a of 63°C, a of -118°C, a of 0.66 g/cm³ at 20°C, and negligible in (approximately 18 mg/L at 25°C). Its is around 190 mmHg at 25°C, contributing to its flammability, with a of -7 °C and an auto-ignition temperature of 278°C. 3-Methylpentane occurs naturally as a component of and is produced commercially through and processes in the of crude oil. It serves as a human and has been detected in trace amounts in foods such as and nectarines, as well as in environmental samples like (average 2.4% composition). Industrially, it is employed as a in , the preparation of vegetable oils, glues, coatings, and paints, and as a raw material for production; it also functions as a additive and a minor constituent in fuels like and rubber solvents. Safety concerns for 3-methylpentane stem primarily from its high flammability, forming explosive vapor-air mixtures, and its reactivity with strong oxidants, which can generate fire hazards; it also attacks certain plastics. Inhalation may cause drowsiness, dizziness, or narcotic effects, with occupational exposure limits set at 500 ppm (TWA) and 1000 ppm (STEL) by bodies like ACGIH. It is classified as toxic to aquatic life with long-lasting effects, necessitating precautions to prevent environmental release.

Structure and nomenclature

Molecular formula and structure

3-Methylpentane has the molecular formula C6H14C_6H_{14}, characteristic of hexane isomers as saturated alkanes with six carbon atoms and the general formula CnH2n+2C_nH_{2n+2}. Its structural formula is CH3CH2CH(CH3)CH2CH3CH_3CH_2CH(CH_3)CH_2CH_3, representing a branched hydrocarbon chain consisting of a five-carbon main chain (pentane backbone) with a methyl group (−CH3-CH_3) attached to the third carbon atom. This branching occurs at the central carbon, which is bonded to one hydrogen, two ethyl groups (−CH2CH3-CH_2CH_3), and the methyl substituent, resulting in a total of 14 hydrogen atoms distributed across the carbons to satisfy valence requirements. The molecule is achiral, as the branched carbon at position 3 is attached to two identical ethyl groups, a methyl group, and a hydrogen atom. In representation, 3-methylpentane is depicted as a line of five carbons with a single carbon branch extending from the third position, omitting the hydrogens for clarity while emphasizing the carbon skeleton. The three-dimensional conformation features tetrahedral around each carbon atom, with bond angles approximately 109.5° and sp³ hybridization, allowing for conformational flexibility such as staggered or eclipsed arrangements along the C-C bonds. As a of straight-chain (CH3(CH2)4CH3CH_3(CH_2)_4CH_3), 3-methylpentane shares the same molecular formula but differs in atomic connectivity due to the branch, which alters the overall shape from linear to more compact. All bonds in the are single covalent bonds, including five C-C bonds and 14 C-H bonds, with no multiple bonds or functional groups present.

Naming conventions and isomers

The IUPAC name of 3-methylpentane is derived from the longest continuous carbon chain of five atoms, designated as the parent structure "pentane," with a single methyl substituent attached to the third carbon atom in the chain. The chain is numbered starting from the end that provides the lowest locant to the substituent, adhering to the IUPAC rule for alkanes that prioritizes the minimum numerical value for branch points. This systematic approach ensures unambiguous identification among branched hydrocarbons. 3-Methylpentane lacks a widely adopted but appears in chemical literature under synonyms such as "pentane, 3-methyl-" and "diethylmethylmethane." In contexts, it is sometimes grouped with other branched under the term "isohexane," though this designation more precisely applies to , highlighting the need for IUPAC names to distinguish specific isomers. Hexane (C₆H₁₄) has five constitutional isomers, each differing in the branching pattern of their carbon skeletons while sharing the same molecular formula:
  • n-Hexane: A linear chain of six carbon atoms with no branches.
  • 2-Methylpentane: A pentane chain with a single attached to the second carbon.
  • 3-Methylpentane: A pentane chain with a single attached to the third carbon.
  • 2,2-Dimethylbutane: A butane chain with two attached to the second carbon.
  • 2,3-Dimethylbutane: A butane chain with attached to both the second and third carbons.
These structural variations arise from different ways to arrange six carbon atoms connected by single bonds, without rings or multiple bonds. n-Hexane, the straight-chain , was isolated from distillates in the , while branched isomers including 3-methylpentane were first separated in the early using advanced and chemical methods. Systematic IUPAC naming conventions were formalized in the early to standardize identification in industrial and scientific applications.

Physical properties

Thermodynamic properties

3-Methylpentane exhibits a of -118 °C and a of 63 °C at standard atmospheric pressure. These values reflect the compound's branched , which lowers the melting point compared to linear isomers due to reduced molecular packing efficiency. The density of 3-methylpentane is 0.664 g/mL at 20 °C, decreasing slightly to 0.660 g/mL at 25 °C, consistent with typical behavior under increasing temperature. Its is approximately 135 mm Hg at 17 °C, rising to 190 mm Hg at 25 °C, indicating moderate volatility suitable for applications. The is -7 °C (open cup), highlighting its high flammability and the need for careful handling to prevent ignition. The for 3-methylpentane is -4160 kJ/mol (equivalent to -994 kcal/mol) at 25 °C, similar to other isomers and underscoring its energetic content as a . in is very low at 13-18 mg/L at 25 °C, rendering it practically insoluble, while it is fully miscible with common organic solvents such as , , and acetone. Critical properties include a critical of 231 °C and a critical of 3.11 MPa, defining the conditions beyond which the and gas phases become indistinguishable. The is 30.3 kJ/mol near the , contributing to its energetics.

Optical and spectroscopic properties

3-Methylpentane is a colorless with a mild, gasoline-like . Its is 1.3765 at 20 °C. The (IR) of 3-methylpentane exhibits characteristic absorption bands for , including C-H in the 2900-3000 cm⁻¹ region and C-C bending modes around 1460 cm⁻¹. These peaks confirm the presence of saturated functionalities, with the serving as a reference for branched identification. In (¹H NMR) spectroscopy, 3-methylpentane displays signals typical of alkyl protons: the s appear around 0.9 ppm as doublets and triplets, methylene protons at 1.2-1.5 ppm as multiplets, and the methine proton at approximately 1.5 ppm. The integration ratios reflect the proton environments, with nine methyl protons (a 6H triplet for the two equivalent terminal methyl groups and a 3H doublet for the branched methyl group), four methylene protons, and one methine proton. NMR (¹³C NMR) shows four distinct signals corresponding to the unique carbon atoms, with chemical shifts ranging from 11.5 to 36.4 ppm in CDCl₃ solvent. Mass spectrometry of 3-methylpentane reveals a molecular peak at m/z 86, consistent with its C₆H₁₄ . Prominent fragmentation patterns include s at m/z 71 (loss of methyl), 57 (C₄H₉⁺, base peak from cleavage at the branched carbon), 56, and 41, typical of beta-cleavage and stability. As a model branched , 3-methylpentane is employed in studies to investigate solution properties and phase behavior in binary mixtures.

Chemical properties

Reactivity and stability

As a branched , 3-methylpentane exhibits the typical chemical inertness of hydrocarbons under standard conditions, showing no reactivity toward acids or bases due to the high pKa values (>50) of its C-H bonds, which prevent proton abstraction or nucleophilic attack. It is also stable to oxidation in the absence of catalysts or initiators, as the strong σ-bonds in its carbon skeleton resist electrophilic or radical attack without activation. This stability under ambient conditions makes it suitable for use as a or component, though it underscores the need for specific conditions to induce reactions. The primary reaction pathway for 3-methylpentane is combustion, where it undergoes complete oxidation to carbon dioxide and water, releasing significant energy as a flammable liquid. The balanced equation for this process is: 2\ceC6H14+19\ceO2→12\ceCO2+14\ceH2O2 \ce{C6H14} + 19 \ce{O2} \rightarrow 12 \ce{CO2} + 14 \ce{H2O} This reaction occurs readily in the presence of oxygen, with an auto-ignition temperature of 278°C and explosive vapor-air mixtures between 1.2% and 7.0% by volume, highlighting its utility in fuel applications but also its fire hazard potential. Under free radical conditions, such as UV light or heat, 3-methylpentane undergoes with or , preferentially substituting at the (position 3) due to the relative weakness of the tertiary C-H bond (bond dissociation energy ≈ 96.5 kcal/mol compared to 98-101 kcal/mol for primary and secondary). shows higher selectivity (>90% at the tertiary site) than (low selectivity, ≈15-20% at the tertiary site), yielding products like 3-halo-3-methylpentane as major isomers for . In catalytic processes, 3-methylpentane participates in cracking and , breaking C-C bonds or rearranging to more stable isomers like under acidic conditions (e.g., over H-zeolites or superacids at 200-400°C). Cracking produces lighter alkenes and alkanes via β-scission mechanisms, with rates influenced by the branched structure, while isomerization favors equilibrium mixtures favoring dimethylbutanes. These transformations are key in to improve ratings. Reactivity with strong oxidants, such as permanganates or peroxides, is highly exothermic, leading to violent reactions that generate and risks rather than controlled oxidation products. stability is maintained up to approximately 400°C, beyond which decomposition initiates via free radical pathways, yielding olefins, , and smaller alkanes without catalysts.

Biological metabolism

3-Methylpentane is a compound metabolized in humans following or from environmental or occupational exposure to petroleum-derived hydrocarbons. In biological systems, 3-methylpentane undergoes phase I metabolism through P450-mediated , primarily at the terminal or branched positions, yielding monoalcoholic derivatives such as 3-methyl-2-pentanol as the predominant . These hydroxylated intermediates are then subject to phase II conjugation or further oxidation to carboxylic acids, facilitating excretion via urine. This enzymatic process, involving isoforms like common to oxidation, enables but can vary based on exposure levels and individual enzyme activity. Due to its volatility and detectability in biofluids, 3-methylpentane and its metabolites hold potential as biomarkers for monitoring human exposure to volatile organic compounds (VOCs) from fuels or industrial solvents. It is quantifiable in , , and exhaled breath, with elevated levels correlating to recent events, as observed in occupational studies of workers. Breath analysis, in particular, offers a non-invasive method for real-time assessment, though specificity requires differentiation from similar branched alkanes. Unmetabolized 3-methylpentane can exert effects on the , contributing to symptoms like and drowsiness at high exposure concentrations before significant occurs. In animal models, leads to narcosis at levels around 30,000 ppm within 30-60 minutes, highlighting the role of incomplete in . Chronic low-level exposure may prolong these effects if hepatic is saturated, underscoring the importance of metabolic capacity in mitigating risks. In natural ecosystems, 3-methylpentane occurs as a trace component in hydrocarbons, influencing biota through in soils, sediments, and bodies derived from oil spills or natural seeps. It contributes to the toxicity of fractions affecting benthic organisms, where drives sublethal effects like reduced microbial degradation rates and altered community structures in vadose zones. by hydrocarbonoclastic partially attenuates its persistence, yet residual levels can bioaccumulate in aquatic food webs.

Synthesis and production

Industrial production methods

3-Methylpentane is primarily obtained as a component of commercial fractions during , where it typically constitutes 3-10% by volume of the light distillates processed in crude oil units. These fractions arise from the of crude oil, with 3-methylpentane emerging alongside other C6 isomers in the 60-70°C range, serving as a key intermediate in blending and production. In refinery isomerization processes, 3-methylpentane is produced through the catalytic conversion of n-hexane, a straight-chain abundant in feeds. This reaction employs bifunctional catalysts such as platinum supported on chlorinated alumina (Pt/Al₂O₃), operating at temperatures of 260-315°C under hydrogen pressure to promote skeletal rearrangement while minimizing cracking. The process achieves near-equilibrium distributions of branched isomers, including 3-methylpentane, enhancing the of the resulting stream for high-quality production. Following production, 3-methylpentane is separated from mixtures via , leveraging differences in boiling points—n- at 69°C, 3-methylpentane at 63°C—to achieve high-purity fractions for downstream applications. Globally, 3-methylpentane forms part of the annual commercial output, estimated at approximately 1.1 million metric tons, primarily from processing in integrated refineries.

Laboratory synthesis routes

One common laboratory route for preparing 3-methylpentane involves the catalytic of the corresponding , 3-methyl-2-pentene. This reduction is typically carried out using gas in the presence of a (Pd/C) catalyst, often in an solvent at and . Another synthetic approach utilizes Grignard reagents to construct the branched carbon skeleton, followed by and . For instance, the addition of to 2-butanone generates 3-methyl-3-pentanol as the intermediate alcohol; subsequent acid-catalyzed affords 3-methyl-2-pentene, which is then hydrogenated under Pd/C conditions to produce 3-methylpentane. 3-Methylpentane can also be obtained via ring-opening isomerization of methylcyclopentane under catalytic conditions. This transformation employs metal catalysts such as platinum or iridium supported on alumina or zeolites, at temperatures of 200-400°C and hydrogen pressures of 1-10 atm, favoring central bond cleavage to yield 3-methylpentane as one of the primary acyclic products alongside 2-methylpentane and n-hexane. Regardless of the synthetic route, purification of 3-methylpentane to greater than 99% purity is achieved via fractional distillation, exploiting its boiling point of 63.3°C to separate it from isomers like 2-methylpentane (boiling point 60.3°C) and n-hexane (68.7°C) in a packed column apparatus under reduced pressure if needed.

Applications and uses

Industrial applications

3-Methylpentane serves as a non-polar solvent in organic synthesis, particularly for extractions and reactions involving non-polar compounds, owing to its low polarity as a branched alkane. Its solvency properties stem from its thermodynamic characteristics, such as a boiling point of 63°C and density of 0.66 g/mL, which facilitate efficient separation in industrial processes. In the lubricant industry, 3-methylpentane is incorporated as a component in specialty oils and formulations, providing low and aiding in the delivery of lubricating agents for applications like and metal surface . Products such as extreme pressure moly lubricants and dry film lubricants list it among key hydrocarbons that enhance fluidity without compromising performance. As a , 3-methylpentane undergoes to produce , a critical filler and in and rubber reinforcement. This process leverages its structure to yield high-quality carbon particles through in controlled furnaces. In fuel applications, 3-methylpentane is blended into as an additive to adjust ratings, with its research octane number of approximately 74 contributing to improved stability in standard fuels. It naturally occurs in fractions and helps meet specifications for regular-grade . Additionally, 3-methylpentane functions as a calibration standard in analysis of hydrocarbons, enabling accurate quantification of components in fuels and environmental samples. Standards mixtures containing it, such as those compliant with ASTM methods, ensure precise instrument for assessments.

Research and analytical uses

3-Methylpentane serves as a model in numerous studies investigating the physical of branched alkanes, including , , , and excess enthalpies of mixing. For instance, it has been employed in binary mixtures with chloroalkanes to measure kinematic viscosities at temperatures ranging from 283.15 to 313.15 K, allowing researchers to correlate experimental data with predictive models like the McAllister equation and assess deviations in isomeric systems. Similarly, its role in ternary systems with ethers and alcohols has facilitated determinations of these thermophysical under standard conditions, providing insights into intermolecular interactions in alkane-based mixtures. In toxicology, 3-methylpentane has been detected in exhaled breath samples from workers in occupational studies, such as those exposed to crystalline silica dust, analyzed via gas chromatography-mass spectrometry (GC-MS), where peak areas were compared across groups to evaluate potential indicators, though no significant elevations were observed relative to controls. However, it is not a validated for aliphatic exposure in breath; instead, the primary for monitoring occupational exposure to 3-methylpentane is its 3-methyl-2-pentanol, measured in by GC, providing a sensitive and specific indicator of exposure levels. As a spectroscopic reference, 3-methylpentane is included in infrared (IR) and nuclear magnetic resonance (NMR) databases to aid in the identification of hexane isomers. Its IR spectrum, featuring characteristic C-H stretching and bending vibrations, serves as a fingerprint for structural confirmation in gas-phase analyses. In NMR, both ^1H and ^13C spectra display distinct signals for its branched structure—such as multiplets around 0.9–1.4 ppm for protons and shifts from 11–36 ppm for carbons—enabling differentiation from linear or differently branched C6H14 congeners. Thermodynamic modeling of 3-methylpentane often incorporates its low-temperature properties, measured alongside analogs like 3-methylheptane, to refine equations of state for branched hydrocarbons. Adiabatic calorimetry from 10 to 330 has yielded heat capacities, enthalpies of fusion, and values, including a at 110.25 and ideal gas of 85.3 cal_th ^{-1} mol^{-1} at 298.15 , supporting group-contribution methods for predicting methylene increments in larger isoalkanes. These data enhance models for phase behavior in cryogenic applications. In radical halogenation research, 3-methylpentane is utilized to probe site selectivity, particularly favoring tertiary C-H bonds over primary or secondary ones. Site-selective chlorination methods, such as those employing azidoiodinane with catalysis, achieve up to 91% yield at the tertiary position without detectable over-chlorination, contrasting with traditional photochemical approaches that yield only 18% selectivity. This makes it a valuable substrate for developing controlled C-H functionalization techniques in .

Safety and environmental impact

Health and safety hazards

3-Methylpentane is a highly classified as NFPA Class IB, with a of -7 °C and an of 278 °C. It forms mixtures with air, having lower and upper limits of 1.2% and 7.7% by volume, respectively, necessitating strict control of ignition sources during storage and use. Its relatively high at increases the risk of vapor accumulation, potentially leading to fire or hazards in poorly ventilated areas. In terms of toxicity, 3-methylpentane produces narcotic and anesthetic effects primarily through inhalation, acting as a . The American Conference of Governmental Industrial Hygienists (ACGIH) has established a (TLV) of 500 ppm as an 8-hour time-weighted average (TWA), with a (STEL) of 1000 ppm. Acute exposure to vapors can cause , , drowsiness, and to the eyes, , and ; it is also an aspiration , potentially fatal if swallowed and entering the airways. Oral administration shows low , with an LD50 greater than 5 g/kg in rats. Chronic exposure to 3-methylpentane may result in , similar to other branched hexane isomers, though specific long-term studies are limited. Exposure monitoring can involve biomarkers such as urinary 3-methyl-2-pentanol. Safe handling requires use in well-ventilated areas or under fume hoods, with including chemical-resistant gloves, safety goggles, and respiratory protection if vapor levels exceed limits; all operations should avoid open flames, sparks, and hot surfaces to prevent ignition.

Ecological and regulatory considerations

3-Methylpentane exhibits moderate in the environment, primarily due to its biodegradability under aerobic conditions. In tests simulating , it achieves 100% after 30 days, though with an initial acclimation period of approximately 27.4 days for microbial adaptation. Estimated half-lives in and range from 10 to 20 days under aerobic conditions, based on studies of similar branched alkanes in mixtures, where degradation proceeds via oxidative pathways involving terminal methyl groups. Volatilization can accelerate removal in surface waters, with modeled half-lives of 57 minutes in rivers and 3.7 days in lakes, outpacing in dynamic systems. The compound has a moderate bioaccumulation potential in aquatic organisms, with an (log Kow) of 3.60 and a factor (BCF) estimated at 320. Despite this, it poses notable to aquatic life, evidenced by a 96-hour LC50 of approximately 4.7 mg/L in fish species such as fathead minnows (Pimephales promelas). This toxicity contributes to long-lasting effects in ecosystems, classifying it as harmful to aquatic environments with chronic hazard category 3 under global harmonized system guidelines. Emissions of 3-methylpentane primarily arise from and spills, where it constitutes a significant fraction of volatile organic compounds (VOCs), often 7-8% in exhaust profiles. As a VOC, it contributes to the formation of and photochemical , particularly in industrial areas, through reactions with hydroxyl radicals in the atmosphere. Its low (approximately 14 mg/L at 25°C) limits immediate aquatic dispersion but enhances aerial transport from spills. Regulatory oversight of 3-methylpentane reflects its role as a . In the United States, it is listed as an active substance on the Toxic Substances Control Act (TSCA) inventory, subjecting it to reporting and risk management requirements for industrial uses. Under the European Union's REACH regulation, it is registered (EC 202-481-4) with restrictions on use as a in products to minimize environmental releases, including XVII limits on volatile hydrocarbons in certain formulations. Spill response guidelines, such as those from the U.S. Agency, mandate containment and cleanup to prevent VOC emissions and aquatic contamination. Mitigation strategies leverage with alkane-degrading bacteria, such as species, which oxidize branched alkanes like 3-methylpentane under aerobic conditions in contaminated soils and waters. These microbes, often enriched from petroleum-impacted sites, can achieve degradation rates enhanced by nutrient addition, reducing persistence in bioreactors or field applications. Global environmental monitoring includes 3-methylpentane in air quality assessments near refineries, where it serves as a marker for fugitive VOC emissions. Programs like fenceline monitoring in the U.S. and track its concentrations to evaluate compliance with emission standards and assess smog precursors in industrial zones.

References

  1. https://pubchem.ncbi.nlm.nih.gov/compound/3-Methylpentane
  2. https://www.inchem.org/documents/icsc/icsc/eics1263.htm
  3. https://www.tcichemicals.com/US/en/p/M0383
  4. https://www.chemicalbook.com/ProductChemicalPropertiesCB8694838_EN.htm
  5. https://webbook.nist.gov/cgi/cbook.cgi?ID=C96140
  6. https://www.indigoinstruments.com/molecular_models/orbit/sets/alkane-chemical-structure-molecule-models-68845nv.html
  7. https://chem.libretexts.org/Bookshelves/Organic_Chemistry/Organic_Chemistry_(Morsch_et_al.)/03:_Organic_Compounds-_Alkanes_and_Their_Stereochemistry/3.04:_Naming_Alkanes
  8. https://webbook.nist.gov/cgi/cbook.cgi?ID=C96140&Mask=200
  9. https://pubchem.ncbi.nlm.nih.gov/compound/Hexane
  10. https://nvlpubs.nist.gov/nistpubs/jres/5/jresv5n4p933_a2b.pdf
  11. https://webbook.nist.gov/cgi/cbook.cgi?ID=C96140&Mask=4
  12. https://webbook.nist.gov/cgi/cbook.cgi?ID=C96140&Type=IR-SPEC&Index=1
  13. https://webbook.nist.gov/cgi/cbook.cgi?ID=C96140&Mask=300
  14. https://www.sigmaaldrich.com/US/en/product/aldrich/m66005
  15. https://chem.libretexts.org/Bookshelves/Organic_Chemistry/Supplemental_Modules_%28Organic_Chemistry%29/Alkanes/Properties_of_Alkanes/Chemical_Properties_of_Alkanes
  16. https://chem.libretexts.org/Courses/Alma_College/Organic_Chemistry_I_%28Alma_College%29/08%253A_Organohalides-_Radical_Halogenation_of_Alkanes_and_Alkenes/8.03%253A_Preparing_Alkyl_Halides_from__Alkanes_-_Radical_Halogenation
  17. https://www.sciencedirect.com/science/article/abs/pii/S0021951784711006
  18. https://www.sciencedirect.com/science/article/abs/pii/0021951779900757
  19. https://pubs.acs.org/doi/10.1021/ja01356a053
  20. https://tsapps.nist.gov/publication/get_pdf.cfm?pub_id=50620
  21. https://www.hmdb.ca/metabolites/HMDB0061885
  22. https://pubmed.ncbi.nlm.nih.gov/8535496/
  23. https://www.jstor.org/stable/27730437
  24. https://pmc.ncbi.nlm.nih.gov/articles/PMC2820140/
  25. https://www.rupahealth.com/biomarkers/3-methylpentane
  26. https://pmc.ncbi.nlm.nih.gov/articles/PMC10339195/
  27. https://weekly.chinacdc.cn/en/article/doi/10.46234/ccdcw2024.278
  28. https://haz-map.com/Agents/3242
  29. https://pmc.ncbi.nlm.nih.gov/articles/PMC4946417/
  30. https://www.sciencedirect.com/science/article/abs/pii/S0045653523015424
  31. https://academic.oup.com/femsec/article/48/3/387/583915
  32. https://www.sciencedirect.com/science/article/abs/pii/S0926860X0000569X
  33. https://www.sciencedirect.com/science/article/abs/pii/S0263876212002584
  34. https://pubs.acs.org/doi/10.1021/ie202995g
  35. https://pmc.ncbi.nlm.nih.gov/articles/PMC9655691/
  36. https://www.chemicalbook.com/synthesis/3-methylpentane.htm
  37. https://www.chemicalbook.com/ChemicalProductProperty_EN_CB31097279.htm
  38. https://www.dillonsupply.com/Product/sprayon-s00202000
  39. https://www.researchgate.net/publication/281059433_Octane_Rating_of_Gasoline_and_Octane_Booster_Additives
  40. https://www.accustandard.com/media/assets/catalogsbrochures/Petroleum_Catalog_2023_4_LK.pdf
  41. https://chemetrix.co.za/wp-content/uploads/2021/07/catalog-ust-astm-standards-ultra-5994-0620en-agilent.pdf
  42. https://pubs.acs.org/doi/10.1021/je200213h
  43. https://pubs.acs.org/doi/10.1021/acs.jced.2c00298
  44. https://pmc.ncbi.nlm.nih.gov/articles/PMC7191029/
  45. https://stacks.cdc.gov/view/cdc/193974
  46. https://www.sciencedirect.com/science/article/abs/pii/S0021961473800850
  47. https://escholarship.org/content/qt2j87m531/qt2j87m531_noSplash_1115f6eddb45e92988d1f17a944fd751.pdf
  48. https://pubs.rsc.org/en/content/articlehtml/2018/sc/c8sc01756e
  49. https://www.sigmaaldrich.com/US/en/sds/sial/68320
  50. http://www.inchem.org/documents/icsc/icsc/eics1263.htm
  51. https://www.echemi.com/sds/3-methylpentane-pid_Rock34942.html
  52. https://19january2021snapshot.epa.gov/sites/static/files/2015-07/documents/c16752rt.pdf
  53. https://www.yncc.co.kr/common/download.do?fidx=40&fkey=1&fnum=2&ftype=d
  54. https://www.sigmaaldrich.com/IN/en/sds/sial/68320
  55. https://www.sciencedirect.com/science/article/abs/pii/S0269749117339404
  56. https://www.fishersci.com/store/msds?partNumber=AAL03133AE&productDescription=3-METHYLPENTANE%2B99%252B%2525%2B100ML&vendorId=VN00024248&countryCode=US&language=en
  57. https://echa.europa.eu/registration-dossier/-/registered-dossier/24591
  58. https://www.epa.gov/tsca-inventory
  59. https://pubs.acs.org/doi/10.1021/acs.est.7b05624
  60. https://www.jeeng.net/pdf-194841-115801?filename=115801.pdf
  61. https://acp.copernicus.org/articles/18/4567/2018/acp-18-4567-2018.pdf
  62. https://www.mdpi.com/2073-4433/16/5/543
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