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41 Cards in this Set
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Explain Distillation: (5)
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1. liquid molecules are in constant motion
2. molecules at surface escape into vapor phase and will do so until equilibrium is established 3. If temp increases, molecular motion, # molecules escaping and vapor pressure all increase 4. Tpressure=Vpressure+Lpressure+Apressure 5. When temp is reached where equilibrium vapor pressure of the sample=total pressure, evaporation increases and bubbles form and boils |
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When to use simple distillation:
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-separation of components if thier boiling points differ by 40-50
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When to use fractional distillation:
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-liquid is composed of two volatile components, # molecules of x,y in a volume of vapor is proportional to their respective partial vapor pressures
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Using fractional distillation, explain how boiling points work:
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-liquid will have specific boiling point based on mole fraction of each component
-raoult's law, composition of vapor can be determined, relative to volatility -the composition of vapor will be richer in more volatile species than the original mixture -then vapor recondenses and the liquid now has a lower bp than the vapor -vapor of second distillation is now even more rich in volatile species |
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If the lower part of the distillation column is at a higher temperature than that of the top, some condensed vapor will revaporize....even as
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it flows down the column to return to the still-pot
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What should the ideal temperatures be?
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1. bottom of column: bp of less volatile component
2. at the top: bp of more volatile component (there is a cycle where uncondensed and revaporized samples rise higher and cycle, each time making it richer in volatile) |
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If entire column is same temp then: If bottom is too hot and top is too cool then:
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-no separation
-column will FLOOD with returning condensate |
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Reflux Ratio:
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compares amount of condensate returning to pot vs. amount of vapor being collected
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Difference in BP to affect good separation should be no less than....
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20-30 degrees C
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In an ideal fractional separation:
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there should be two plateaus, first at the bp of more volatile and second at bp of less volatile, with very little volume separating the two
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What does Gas-Liquid Chromatography do?
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-partitions components of a mixture between a mobile gaseous phase and a stationary liquid phase
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What's the process in GL Chromatography?
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1. sample injected, immediately vaporized
2. vapor carried through column by flowing inert CARRIER GAS (he or n2) -the mobile phase 3. column is packed with solid support which is coated with viscous, high bp liquid-the stationary phase 4. as mobile phase moves, components continually partition between two |
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What is Retention Time?
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1. elapsed time required for a component to move from injection point to detector
2. independent of presence of other components 3. dependent upon: nature of stationary phase (polarity), length of column, flow rate of gas 4. the more volatile component of a mixture will have the smaller retention time |
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Partition Coefficients:
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1. dependent on solubility of component in liquid phase
2. solubility of a gas in liquid phase decreases a its vapor pressure increases, more volatile components pass through column more rapidly with liquid phase (polar w/carbowax, nonpolar with silicon gum rubber) |
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How to detect components on GC:
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1. separate into bands
2. voltage proportional to mole fraction 3. flame ionization detector detects ions 4. but not all compound ionize to form same types or number of ions 5. so peak areas in chromatogram will not be exact unless corrected by RF |
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Response Factors:
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-determine volume of each component that contributes using molar mass and density, scale down x100
-find ratio of peak areas - |
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Column Efficiency or Resolution:
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-increases with increasing column length, decrease diameter
-increase temp leads to shorter retention times because gas solubility in the liquid phase decreases at temp rises, up flow rate downs retention times |
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Our substitution reaction was reversible, so it was performed in the excess of the _______________ and in the presence of _______ to add an H+
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Lewis Acid, H2SO4
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Verify that the SN2 occurred takes two tests:
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1. Addition of AgNO3 precips to get silver halide,,,halide colors: AgCl is white, AgBr is cream, AgI is bright yellow.
Fast reaction= tertiary, Slow reaction=primary... alkyl bromides and iodides are faster than chlorides |
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Alkyl halide + NaI= insoluble NaCl or NaBr
speeds: |
primary bromides <3 at RT
primary chloride, NaCl if heated 2/3 bromides if heated 2/3 chlorides don't react |
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Definition of Alkenes:
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organic compound where there is a polarizable C-C pi bond
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polarizable:
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ease with which e- cloud of a Lewis base is distorted by atom bearing a full or partial + charge
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bimolecular processes: elimination, substitution
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nuc attacks carbon bonded to leaving group form backside in e, or in s, it can pull acidic proton form beta carbon, moving its bonding electron to form a pi bond (ANTI PERI-PLANAR)
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unimolecular processes:
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nuc attacks carbocation in sub, in elim it pulls the acidic proton from c and forms a pi bond to alleviate positive charge on alpha carbon
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Substitution favored by which nuc's: Elim favored by which nuc's:
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1. weakly basic, highly polarizable nucleophiles (i-,br-,cl-h2o)
2. strongly basic, slightly polarizable nucs (ro-, oh-,nh2- h-) these bulky nuc's favor elim because its easier to remove a proton than approach a carbocation (also the more substituents the more likely elimination) |
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Major product of an E2 is the _________ substituted on the double bond, its of lower energy
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most
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When can the major product be really the minor product in and E2?
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when the steric hinderance causes a nuc: to need to attack a less substituted carbon
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Alkanes are chemically non-reactive toward most reagents T or F
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True, except in free radical where an alkyl chloride or bromide forms x2--> 2Xdot, radical attacks R-H bond of alkane to give R-X + H
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GO OVER FREE RADICAL CHLORINATION OKAY?
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okay.
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In one of three termination steps, two alkane radicals can form a new sigma-bond, effectively forming a _______
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dimer
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Free radical halogenation of saturated alkanes produces both mono- and poly- substituted products: ex. 1-chlorobutane is chlorinated to get
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di-chloro and tri-chloro, poly-sub can be minimized by using excess alkane compared to reagent eg 2 alkane: 1 SO2Cl2
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If you perform the radical chlorination with care not avoid poly-sub then your end reaction "product mass" will really be...
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mass of actual dichlorobutanes + mass of unreacted 1-chlorobutane
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so before you do GC on a radical problem....
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you don't really actually know the masses
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zero % yield shows:
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mass of 1-chlorobutane used
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100 % yield shows:
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mass of number of moles of SO2Cl2 used (since its limiting and its 1:1:1) PLUS the difference between the mass of the #moles 1-cholorbutane used
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for 100% yield: mass in reaction flask at the end is the mass of:
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the number of moles of SO2Cl2 + (# moles started with - # moles used to create product) (all turned to grams)
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Theoretical yield:
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difference between the mass from zero product and 100 % product, it will be less than actual yield
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Experimental yield:
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difference between mass of mixture in the flask at the end (before drying) and the mass of o% yield
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once a GC is run, you can calculate the relative fraction of 1. the original reactant used which remains unreacted
vs 2. sum of all dichloro-products to get... |
actual % yield
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The step that determines what products will form is the one which ------ which has a more likely to go?
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the 'H' is extracted from the alkane, H on an internal C because statistical factor
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Energetically, a secondary C-H is weaker than a primary C-H bond. True of False so what?
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True, so 1,2 dichloro and 1,3-dichloro are favored over 1,1 or 1,4. To determine statistical factor, take area under GC peak for each product and divide by #H capable of producing that product
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