Ch. 12 - Alkanes (sat’d HCs). Alkanes Acyclic Saturated Hydrocarbons (chains) General Formula: C n...
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Transcript of Ch. 12 - Alkanes (sat’d HCs). Alkanes Acyclic Saturated Hydrocarbons (chains) General Formula: C n...
Alkanes
Acyclic Saturated Hydrocarbons (chains)
General Formula: CnH2n+2
Structural: (ex.: C4H10)
Complete
Condensed
Skeletal
Line AngleDecomposition of plant and animal matter in marshes is a good source of methane gas.
Alkane Isomerism
Isomers: compounds that share the same molecular formula but have different structural formulas
With an increased number of C atoms, there is an exponentially increased number of isomersConstitutional - same molecular formula, different structural formula;
differ in connectivity of atoms
Ex. C4H10 butane ; isobutane
Ex. C8H18 octane; 3-methyl heptane
Alkyl Groups & IUPAC namesUse the following rules to properly name hydrocarbon molecules:
1. Identify the longest, continuous chain of C atoms and name it (parent C chain and suffix.2. # the C atoms in the chain from the end nearest an alkyl group.3. # and name the attached alkyl group(s).4. If more than one alkyl group:
1st substituent must have lower number.Alkyl groups are listed in alphabetical order.If two or more identical substituents are bonded, use prefixes to indicate how many
5. Separate #s from each other with commas; separate names from numbers with hyphens; do not use a hyphen/space after the last substituent, before the parent alkane name.
Carbons are classified 4 ways in a chain:Primary, secondary, tertiary, quaternaryBased on the # of C atoms to which the carbon atom is bonded.
Branched-chain Alkyl Groups
“Simple”: 4 important ones to know!
Complex: “select the longest chain as the “base” alkyl, add “substituents.”
Ex.
Isomerism of Cycloalkanes
Constitutional (ex.: C5H10) 5 isomers
Stereoisomers: possible with substituted cycloalkanes (ex.: 1,2-Dimethylcyclohexane)
Cis- (SAME side)
Trans- (ACROSS from)
Sources of Saturated Hydrocarbons
Natural Gas:Methane (50-90%)
Ethane (1-10%)
Propane & Butane (up to 8%)
Petroleum (crude oil): this is a complex mixture of both cyclic and acyclic hydrocarbons which can be separated by a process known as fractional distillation.
Physical Properties of Hydrocarbons
All are insoluble in waterConsider the polarity of the compoundsTherefore they can make good protective coatings
All are less dense than water (0.6-0.8 g/mL)
Oil & water
Boiling Points & States of MatterGenerally, BP increases with increasing # C atoms
Reason: increasing LDF
1-4 C atoms = gas; 5-17 C atoms = liquid; >17 C atoms = solidIsomers: Branched BP < Unbranched BPCyclic Compounds have higher BP than Acyclic.
Chemical Properties of Hydrocarbons
Alkanes are the least reactive organic compounds (they have no fcn’l groups). However, two major reactions are common:
CombustionR (some hydrocarbon) + O2 → CO2 + H2O + energyenergyvery exothermic reaction.
If the quantity of O2 is insufficient, it will form a poison called carbon monoxide (CO). Here is an example with methane:
CH4 + 2 O2 → CO2 + 2 H2O
with less O2:
2 CH4 + 3 O2 → 2 CO + 4 H2O (poison!)
with even less O2:
CH4 + O2 → C + 2 H2O (black soot forms)
HalogenationR-H + X2 --> R-X + H-X
Hydrocarbon fuelsFossil fuels (solid, liquid, or gas) form from organic material being covered by successive layers of sediment over millions of years
Oil & natural gas: slow decomposition & burying of marine phytoplankton & zooplankton that sank to the sea floor. Coal: ancient swamps and bogs - slow decomposition of land plants in anaerobic conditions:
e.g. peat bogs of Ireland
Petroleum, Naphtha, or crude oilFrom Greek petra = rock and oleum = oil
Thick, dark brown or greenish liquid
Complex mixture of various hydrocarbons,
largely of the alkane series
May vary much in appearance, composition, and
purity
Petroleum is also the raw material for many chemical products: fuels & solvents
Can be altered into: fertilizers, pesticides, and plastics
Think of the impact of a substantial oil crisis on our economy & society!
Crude Oil History•1st oil wells drilled in China in 4th century depth up to 800 ft. •Drilled using bits attached to bamboo poles •Burned oil to evaporate brine & produce salt.•10th century, bamboo pipelines connected oil wells with salt springs.
Ancient Persian tablets indicate the medicinal and lightinglighting uses of petroleum in the upper society.8th century: streets of Baghdad paved with tar.In the 9th century, oil fields were exploited in Baku, Azerbaijan, to produce naphtha.
Discovery of oil in 1859, near Titusville, Pennsylvania. Great demand for kerosene and oil lamps. Medicinal purposes, lighting, and lubricants for new steam engines.Introduction of internal combustion engine lead tomajor "oil booms" in Texas, Oklahoma, and California.
The complex hydrocarbon mixture present in petroleum is separated into simpler mixtures by means of a fractionating column.
Differences in BPs of hydrocarbon chains
can separate out sections of
the crude oil:Fractional Distillation
Fuel type Mega Joules / Liter
BTU / US gal Research octane #
Gasoline 29.0 125,000 91 to 98
Diesel fuel oil
32.19 138,690 N/A
Residential heating oil
34.74 149,690 N/A
Gasahol10% ethanol
90% gasoline
28.06 120,900 93 to 94
Octane: major component of gasoline
•Octane is an alkane hydrocarbon:CH3(CH2)6CH3. •octane isomer: 2,2,4-Trimethylpentane = 100 pts on the octane rating scale
•n-heptane is the zero point (greatest engine knocking or “pinging”)•Octane ratings are used to represent antiknock performance (less premature combustion)
Natural gasNatural gas mainly methane (does contain other “small” HC cpds).Highly flammableNo ash and very little air pollution. From light portion of petroleumRises thru fissures in earth’s crustMan-made wells can tap it Discovered thousands of years ago could be burned for heat and light. Colorless, odorless, & lighter than air.Mercaptan, chemical odorant, is added for gas leaks. natural gas combustion CO2 + H2ONatural gas found in different underground formations: shale, sandstone beds, coal seams, & deep, salt water aquifers
New sources of methane gas:Decomposition of organic
matter in landfills
CH4 gas can be tapped instead of vented
Kivu Lake
3 lakes contain large concentrationsof dissolved CO2 gas.
Lake Nyos & Lake Monoun sites of gas explosions: 40 dead at Monoun & 1800 at Nyos
3rd lake is Kivu, which contains a 1,000x more gas than Lake Nyos.
Coal formation
•Vegetable matter accrues •Prevented from decay•Forms peat beds. •Over time: buried & compressed, forms lignite.
Increased P & T makes bituminous
coal (higher C content). •At great depths, high temps reduce CH4 & forms anthracite (very high in C)
Fossil Fuel “Facts”
Source: Shell Oil
Current Consumption?What about as China and India
modernize?These countries
have 33% of world population!
The U.S. has 4% of the World's population. The U.S. uses 34% of Earth's natural resources.
U.S. Sources of Energy Production
Fossil Fuels 86% Geothermal 0.5% Nuclear 8% Wind Farms 0.1% Hydroelectric 2% Solar 0.1% Biofuels 3.3%source: US Dept of Energy
Remember that, while hydrocarbons serve as a transportation fuel, they are also used to produce plastics, etc.
Enormous dependence on a limited resource.Other alternatives?
-Wave energy-Tidal energy-New technology for solar panels, turbines, etc.
-Conservation!!-Efficiency!!!
Problems associated with alkane hydrocarbons
Hydrocarbon pollution: (oil spills) of aquatic environments (e.g. BP in the Gulf of Mexico)
Global warming: CO2 and H2O
Acid rain due to sulfur impurities in oil and coal: damage crops, lakes, buildings, etc.
Smog and soot: increase respiratory problems
Land fill: non-decomposing plastics
Ozone depletion / increased UV radiation
Global warming: Global warming: The The Greenhouse effect:
Short wavelength solar radiation releases energy
as it hits molecules.Turns into long
wavelength energy.Gases in atmosphere trap it and warm the
atmosphere.
Arctic ice sheet 1979 and 2000
CO2 increase correlates to average global temperature increase
Can cause: changes in sea level, reduction of reflective ice caps, increased storm ferocity, plant & animal re-distribution,shift ocean currents, createdroughts & forest fires, increased short-term temperature fluctuations.
Alkane substitution reaction:Incoming atom or group of atoms (orange sphere) replaces a hydrogen atom in the alkane model.
Naming:Treat halogen atoms like alkyl groups.
F = fluoro; Cl = chloro; Br = bromo; I = iodo
Ex.: CH3-CHBr-CHBr-CHI-CH2-CH3
Halogenation Reactions
General equation: RH + X2 → RX + HX
Hydrocarbon + Halogen Halogenated + acid (diatomic) hydrocarbon
Ex. CH4 + Cl2 --> CH3Cl + HCl
Highly exothermic reaction: can lead to an explosion
The process can continue to alter the resulting products as long as the halogen remains in sufficient quantities to drive further reactions. (The halogen would be the __________ reactant.)
Chlorofluorocarbons (CFCs)
Developed in the 1930's
Very stable compounds composed of C, F, Cl, & H
Freon is the tradename:
Trichlorofluoromethane
Dichlorodifluoromethane
Trichloro-trifluoroethane Dichloro-tetrfluoroethane Chloropentafluoroethane
Safe, non-toxic,
non-flammable
alternative to
dangerous
substances
(e.g. ammonia)
for aerosol-spray
propellants,
refrigerants,
solvents, and
foam-blowing agents
The Ozone Layer Chemistry
CFCl3 + UV LightUV Light ==> CFCl2 + Cl Cl + O3 ==> ClO + O2
ClO + O ==> Cl + O2
The chlorine free radical atomis then able to attack anotherozone molecule
Cl + O3 ==> ClO + O2
ClO + O ==> Cl + O2
and again ... Cl + O3 ==> ClO + O2
ClO + O ==> Cl + O2
and again... thousands of times!A catalyst!
The ozone destruction process requires conditions cold enough (-80oC) for stratospheric clouds to form. Once these stratospheric clouds form the process can take place, even in warmer conditions
Ozone consumption has been greatly reduced,
1997 ozone
hole
2003 ozone
hole
however CFCs may linger for another 150 years in the atmosphere
Ozone layer thickness
What do you need to know (about saturated hydrocarbons)?
Structural characteristics (know the functional group)Substituents
Nomenclature (the rules for naming the molecules)
Physical and Chemical properties (basic/simple)
Occurrence and uses (common)
Preparation (what basic reactions produce the molecules)
Characteristic reactions of the molecules