CHEMISTRY/ORGANIC CHEMISTRY FINAL REVIEW Flashcards

Question

Ionic bonds in solid state

Answer 1

In solid state, the ionic constituents of the compound form a crystalline lattice of repeating positive and negative ions

Answer 2

Valence shell - dots - dashes

Answer 3

Draw out backbone with the least electronegative atom in the center Count all the valence electrons Complete the octets of all atoms bonded to the central atom, using the remaining valence electrons left to be assigned Place any extra electrons on the central atom VSEPR Theory Arrange the electron pairs around the central atom so that they are as far apart as possible

Answer 4

Spatial arrangement of all pairs of electrons

Answer 5

spatial arrangement of only the bonding pairs of electrons determined by coordinate number -number of atoms that surround and are bonded to a central atom

Answer 6

Even hydrogen bonds have only about 10 percent the strength of a covalent bond Nitrogen, Oxygen, or fluorine bonded to hydrogen

Answer 7

Moles = mass of sample/ molar mass

Answer 8

the amount of a compound, measured in grams, that produces one equivalent of the particle of interest Gram equivalent weight = molar mass/n where n is the number of particles of interest produced or consumed Ex: gram equivalent weight of H2Co3 is half of its molar mass with interest towards h+ ions Useful for acid-base chemistry

Answer 9

equivalents/L (where molarity is moles per liter) most commonly used for hydrogen ions concentration Ex: A 1N solution of acid would be like HCL, and 2N would be like H2So4

Answer 10

Normality/n or moles per liter

Answer 11

gives the simplest whole-number ratio

Answer 12

involves a fuel (usually hydrocarbon) and a oxidant (normally oxygen), forming carbon dioxide and water

Answer 13

a specific type of double-displacement reaction: acid + base = water + salt

Answer 14

For metals the charge is indicated by a Roman numeral in parentheses - ous: less charge, -ic: greater charge - ide: monatomic anions Hypo- indicates less oxygen, per- indicates more oxygen

Answer 15

A solute is considered a strong electrolyte if it dissociates completely into its constituent ions

Answer 16

k = Ae^(-Ea/RT) k is the rate constant, A is the frequency factor, Ea is the activation energy of the reaction, R is the ideal gas constant, and T is the temperature in kelvins

Answer 17

Transition state/activation complex has greater energy than both the reactants and the products and is denoted by the symbol ‡

Answer 18

the catalyst is in the same phase as the reactants

Answer 19

the catalyst is in a distinct phase

Answer 20

For the general reaction aA + bB -\> cC + dD, rate = k[A]^x[B]^y The values of x and y are almost never the same as the stoichiometric coefficients, the orders of a reaction must be determined experimentally

Answer 21

refer to either non-integer orders (fractions) or to reactions with varying rate orders fractions are specifically described as broken-order

Answer 22

For a generic reversible reaction aA + bB ⇔ cC + dD, if the system is at equilibrium constant temperature Keq = [C]^c[D]^d / [A]^a[B]^b products over reactants Keq = (x)^2/1-x - if x amount of A has reacted and x amount of B and C have been produced, and 1 is the starting concentration - can be rounded so the denominator is simply the starting concentration (in this case 1)

Answer 23

Isolated System cannot exchange energy or matter with surroundings Closed System can exchange energy but not matter with surroundings Open System can exchange energy or matter with surrounds

Answer 24

Change in internal energy can only occur through heat or work ΔU = Q - W

Answer 25

Constant temperature, Internal energy is constant ΔU = 0

Answer 26

no heat exchanged between the system and environment ΔU = - W

Answer 27

constant pressure does not alter the first law, but appears as a flat line on a P-V graph

Answer 28

constant volume ΔU = Q

Answer 29

describe the system in an equilibrium state without respect to process Pressure, density, temperature, volume, enthalpy, internal energy, Gibbs free energy, entropy

Answer 30

Standard conditions: 298K 1atm and 1 M concentrations Standard temperature and pressure (STP): 273K and 1 atm

Answer 31

the temperature and pressure above which there is no distinction between the phases -supercritical fluid

Answer 32

equivalent to heat under constant pressure (an assumption the MCAT usually makes) ΔHrxn = Hproducts - Hreactants

Answer 33

q = mcΔT specific heat of water = 1cal/g\*K

Answer 34

the product mc, mass times specific heat

Answer 35

constant-volume calorimetry Because W = PΔV, no work is done in an isovolumetric process, and (ΔU = Q) Also an adiabatic process, no heat is exchanged between the calorimeter and the rest of the universe, but it is exchanged between the steel decomposition vessel and the surrounding water

Answer 36

q=mL m is mass and L is latent heat

Answer 37

time’s arrow, entropy always increases if not hindered from doing so

Answer 38

ΔS = Qrev/T change in entropy = heat gained or lost in a reversible process/ Temperature in Kelvin

Answer 39

ΔG = ΔH - TΔS get higher test scores

Answer 40

ΔGrxn = -RTlnK deriving the standard free energy change for a reaction ΔGrxn = -RTlnQ/K deriving the free energy change for a reaction not at equilibrium K is equilibrium constant

Answer 41

1 atm = 760mmHG = 760 torr = 100kPA

Answer 42

STP is generally used for gas law calculations; standard state conditions are used when measuring standard enthalpy, entropy, free energy changes, and electrochemical cell voltage

Answer 43

p (density) = mass/Volume = PM/RT **density = pressure\*molar mass / R\*Temperature** R = 0.0821 liter·atm/mol·K R = 8.3145 J/mol·K

Answer 44

PV/T is constant, PV is constant, V/T is constant, n/V is constant and equals k (moles/volume is constant) -these can all be derived from the PV=nRT equation

Answer 45

M = (Density@STP) \* 22.4L/mol Molar Mass can be calculated as the product of the gases density at STP and the STP volume of one mole of gas

Answer 46

Pt = Pa + Pb + Pc Partial pressure of gas is related to its mole fraction Partial pressure = moles of gas A / total moles of gas The relationship between concentration and pressure is constant

Answer 47

explains the behavior of gases Assumptions 1 Particles have negligible volume 2 There is no intermolecular attractions or repulsions 3 Particles are in continuous, random motion, undergoing collisions with other particles and the container walls 4 Collisions between any two gas particles are elastic, with conservation of both momentum and kinetic energy 5 The average kinetic energy of gas particles is proportional to the absolute temperature of the gas, and is the same for all gases at a given temperature, irrespective of chemical identity or atomic mass

Answer 48

KE = 1/2mv^2 = 3/2kBT proportional to 3/2 the absolute temperature of the gas and Boltzmann constant uRMS = sqr(3RT/M) M is molar mass

Answer 49

Graham’s law: under isothermal and isobaric conditions, the rate at which two gases diffuse are inversely proportional to the square roots of their molar masses r1/r2 = sqr(M2/M1) r is the diffusion rate, M is the molar mass

Answer 50

the rates of effusion are proportional to the average speeds

Answer 51

corrects the ideal gas law of intermolecular attractions and molecular volume

Answer 52

Solvation is the electrostatic interaction between solute and solvent molecules. This is also known as dissolution, and when water is the solvent it can be called hydration Sparingly soluble salts dissolve minimally in the solvent

Answer 53

H+ is never found alone in solution, it is found bonded to an electron pair donor in a coordinate covalent bond

Answer 54

All salts containing Ammonium and alkali metal cations are water-soluble All salts containing nitrate (NO3-) and acetate (CH3COO-) anions are water-soluble Halides excluding fluorides are water-soluble, with the exception of those formed with Ag+, Pb2+, and Hg2+ All salts of the sulfate ion (SO4) are water soluble, with the exceptions of those formed with Ca, Sr, Ba, and Pb All metal oxides are insoluble, with the exception of those formed with the alkali metals, ammonium, and CaO, SrO, and BaO All hydroxides are insoluble, with the exception of those formed with the alkali metals, ammonium, and Ca2+, Sr2+, and Ba2+ All carbonates, phosphates, sulfides, and sulfites are insoluble, with the exception of those formed with the alkali metals and ammonium WE WON'T BE EXPECTED TO MEMORIZE THESE RULES, BUT ALL GROUP 1 METALS SALTS AND ALL NITRATE SALTS ARE SOLUBLE

Answer 55

Complexes are held together with coordinate covalent bonds In some complexes, the central cation can be bonded to the same ligand in multiple places (chelation) -generally requires large organic ligands that can double back to form a second (or even third) bond with the central cation

Answer 56

Moles/kilogram

Answer 57

reaction dependent, equal to the number of equivalents of interest per liter of solution

Answer 58

Ksp = [A^n+]^m[B^m-]^n -does not take into account solid compounds ion product (IP) - analogous to the reaction quotient Q for other chemical reactions - same form as the equation for the solubility product constant but the values aren't at equilibrium

Answer 59

reduction in molar solubility with the addition of common ions

Answer 60

Properties dependent on concentration but not chemical identity Vapor pressure, boiling point elevation and freezing point depression, osmotic pressure

Answer 61

Mole fraction of solvents \* Vapor pressure of solvent in pure state

Answer 62

iKm m is molality, moles/kg value is negative for freezing point

Answer 63

iMRT M is molarity, i = van't Hoff factor

Answer 64

dissociate H+ in solution or dissociate OH- in solution c ontain either H at the beginning of their formula or OH at the end

Answer 65

donates H+ or accepts H+ not limited to aqueous solutions conjugate base pairs

Answer 66

electron pair acceptor (acid) or electron pair donor (base) same chemistry as coordinate covalent bond formation, complex ion formation, or nucleophile-electrophile interactions (nucleophile is a base, electrophile is an acid)

Answer 67

if the anion ends in -ite (less oxygen), then the acid will end with -ous acid If the anion ends in -ate (more oxygen), then the acid will end with -ic acid

Answer 68

Kw = [H3O+][OH-] = 10^-14 @ 298K

Answer 69

if H+ is .001 or 10^-3 , pH = 3 -log(**n\*10^-m**) = m-1.10-n or **m-.n** dissociation of strong acids and bases is said to go to completion

Answer 70

HCl (Hydrochloric acid) HBr (Hydrobromic acid H2SO4 (Sulfuric acid) HNO3 (Nitric acid) HCLO4 (Perchloric Acid)

Answer 71

NaOH (sodium hydroxide) KOH (potassium hydroxide)

Answer 72

Ka = [H3O][A-] / [HA] Kb = [B+][OH-] / [BOH] Ka and Kb are mostly used to determine the concentration of one of the species at equilibrium

Answer 73

Strong acid + strong base: HCl + NaOH -\> NaCl + H2O Strong acid + weak base: HCl + NH3 -\> NH4Cl Weak acid + strong base: HCLO + NaOH -\> NaClO + H2O Weak acid + weak base: HCLO + NH3 -\> NH4ClO

Answer 74

At the equivalence point, the number of equivalents of acid and base are equal NormalityA \* VolumeA = NormalityB \* VolumeB Indicators are weak organic acids or bases that have different colors in their protonated and deprotonated states Polyvalent acids and bases yield multiple equivalence points -at each half-equivalence points, half of a given species has been protonated or deprotonated

Answer 75

Co2 \<=\> H2CO3 ⇔ H+ + HCO3-

Answer 76

For a weak acid buffer solution pH = pKa + log [A-]/[HA] For a weak base buffer solution pOH = pKb + log [B+]/[BOH] remember concentration ratio as products over reactants If the concentration of both the acid and conjugate base were double the buffering capacity would double, not the pH

Answer 77

the oxidation number of a free element is zero the oxidation number for a monatomic ion is equal to the charge of the ion the sum of the oxidation numbers in a compound must add to that compounds charge

Answer 78

contained systems in which oxidation-reduction reactions occur oxidation always occurs at the anode, and reduction occurs at the cathode electron always travels from anode to cathode

Answer 79

all the batteries you own spontaneous, + emf, -ΔG in a galvanic cell the anode is negative and the cathode is positive has an aqueous electrolyte solution composed of cations and anions, the charge gradient is dissipated by the presence of a salt bridge, which contains ions that will not react with the electrodes or with the ions in solution

Answer 80

opposite of galvanic cells, except for An Ox Red Cat and anode-\> cathode driven by an external battery source, known as electrolysis nonspontaneous, - emf, +ΔG in an electrolytic cell the anode is positive and the cathode is negative

Answer 81

shorthand notation representing the reactions in an electrochemical cell Ex: Zn (s) | Zn2+ (1M) || Cu2+ (1M) | Cu (s) 1. The reactants and products are always listed from left to right in anode | anode solution (concentration) || cathode solution (concentration) | cathode 2. A single vertical line indicates a phase boundary whereas a double vertical line indicates the presence of a salt bridge or other barrier

Answer 82

10^5 C/mol e-

Answer 83

mol M = It/nF mol metal ion being deposited = current \* time / 10^5 \* number of electron equivalents for a specific metal ion OR **mol e- = It/10^5**

Answer 84

a type of galvanic cell, contains two half-cells connected by a conductive material allowing a spontaneous oxidation-reduction to proceed, which generates a current and delivers energy

Answer 85

Describes the electrochemical cell, if the emf is positive, the cell is spontaneous Ecell = Ered,cathode - Ered,anode

Answer 86

ΔG\* = -nFE\*cell where ΔG\* is the standard change in free energy, n is the number of moles of electrons exchanged, F is the Faraday constant, and E\*cell is the standard emf of the cell

Answer 87

Ecell = E\*cell - (RT/nF)lnQ Q = [C]c[D]d / [A]a[B]b

Answer 88

ΔG\* = -RTlnKeq

Answer 89

O=C-H indicated with the suffix -al or the prefix oxo- when not the highest priority group

Answer 90

R-(C=O)-R indicated with the suffix -one

Answer 91

O=C-OR indicated with the suffix -oate

Answer 92

O=C-N indicated with the suffix -amide

Answer 93

O=C-O-C=O indicated with the suffix -anhydride

Answer 94

O=C-C-C-OH aldehyde plus alcohol

Answer 95

Conformational isomers differ in rotation, Configurational isomers require bond breaking to interconvert (enantiomers and diastereomers)

Answer 96

eclipsed staggered - anti - two largest groups are on opposite sides - gauche - two largest groups are 60\* apart

Answer 97

Enantiomers differ at all chiral centers when present in equal concentrations they form racemic mixtures, which can be separated with a single enantiomer of another compound, leading to two diastereomers

Answer 98

Cis-Trans molecules differ in arrangment around an immoveable bon

Answer 99

Cyclic conformations can be either stable or unstable depending on ring strain Angle strain bond angles deviate from their ideal values Torsional strain cyclic molecules are eclipsed or gauche Nonbonded strain (van der waals repulsion) nonadjacent atoms or groups compete for the same space

Answer 100

a molecule with at least 2 chiral centers that has an internal plane of symmetry

Answer 101

polysubstituted double bonds Z if the highest priority (atomic number) are on the same side, E if opposite

Answer 102

highest atomic number is highest priority clockwise is R where counterclockwise is L switch if the lowest priority is in front of molecule (wedge in Fischer, side in skeleton)

Answer 103

acidity increases towards the bottom right of the periodic table

Answer 104

either lone pairs or pi bonds that can form new bonds to electrophiles determined by four major factors

Answer 105

Charge - nucleophilicity increases with electron density / negative charge Electronegativity - nucleophilicity decreases as electronegativity increase because these atoms are less likely to share electron density Steric hindrance - bulkier molecules are less nucleophilic Solvent - protic solvents can hinder nucleophilicity by protonation of the nucleophile or through hydrogen bonding For protic solvents, nucleophilicity goes I- \> Br- \> Cl- \> F- For aprotic solvents, nucleophilicity goes I- \< Br- \< Cl- \< F-

Answer 106

Unimolecular, contain two steps rate of the reaction depends only on the concentration of the substrate rate = k[R-L], where R-L is an alkyl group containing a leaving group

Answer 107

Bimolecular, contain only one step rate of the reaction depends on both the concentration of the substrate and the nucleophile rate = k[R-L][Nu:] nucleophile must be strong and the substrate cannot be sterically hindered accompanied by an inversion of relative configuration, the position of the substituents around the substrate carbon will be inverted (R -\> S or vice versa)

Answer 108

A redox reagent will tend to act on the highest priority functional group

Answer 109

adjacent carbons are called ortho, separated by a carbon is called meta, opposite sides is called para

Answer 110

Primary alcohols can be oxidized to aldehydes -only be PCC, a mild oxidant Primary alcohols can be oxidized past aldehydes to geminal (same carbon) diols to carboxylic acid -with stronger oxidizing agents than PCC Secondary alcohols can be oxidized to ketones with any oxidizing agent Tertiary alcohols cannot be oxidized

Answer 111

Mesylate have the functional group -SO3CH3 Tosylates contain the functional group -SO3-C6H4(benzene)-CH3 these groups can serve as protecting groups or can be formed from alcohols to make better leaving groups

Answer 112

Treatment of phenols with oxidizing agents produces quinones (O=ring) example of secondary alcohol oxidation not necessarily aromatic because they lack the conjugated ring structure Hydroxyquinones share the same ring and carbonyl backbone as well as a hydroxyl group Ubiquinone (CoQ) is a biologically active quinone

Answer 113

In the presence of water, aldehydes and ketones react to form geminal diols (same carbon diols) -the reaction rate can be increased by adding a small amount of catalytic acid or base

Answer 114

Acetals C-(OR-)C(-OR)-H or ketals C-(OR-)C(-OR)-C can be created with the reaction of aldehydes or ketones with two equivalents of alcohol or a diol catalyzed by anhydrous acid

Answer 115

Hemiacetals C-(OR-)C(-OH)-H or hemiketals C-(OR-)C(-OH)-C can be created with the reaction of aldehydes or ketones with one equivalent of alcohol endpoint in basic conditions

Answer 116

Simplest case of imine formation from aldehyde/ketone: -ammonia adds to the carbon and water is lost --examples of a condensation reaction and nucleophilic substitution Imines can tautomerize to enamines

Answer 117

HCN + aldehydes or ketones can create cyanohydrins, as the CN group adds to the carbonyl carbon and forces reduction

Answer 118

Aldehydes can be oxidized to carboxylic acids with any oxidizing agent stronger than PCC

Answer 119

Aldehydes and ketones can be reduced to form alcohols -most often performed with the hydride reagents LiALH4 and NaBH4

Answer 120

the enol is named for its C=C and -OH the two isomers are called tautomers, and interconvert through tautomerization/enolization the thermodynamic intermediate is most stably substituted but forms less quickly Enamines are tautomers of imines in the same way

Answer 121

An aldehyde or ketone acts as both an electrophile (in keto form) and a nucleophile (in enolate form), and the end result is a formation of a carbon-carbon bond from a beta carbon to an alpha carbon -requires a catalytic amount of base Aldol has a carbonyl and a hydroxyl group sharing a beta carbon -aldehyde and alcohol = aldol An example of a condensation reaction and a dehydration reaction because two molecules are joined with the loss of a small molecule

Answer 122

reverse of aldol condensation, aqueous base (OH-) is added and heat is applied

Answer 123

Groups like -NO2 or halides are electron withdrawing and increase acidity -Dicarboxylic acids are therefore more acidic than analogous monocarboxylic acids due --beta-dicarboxylic acids have high acidity of the alpha-carbon that they share, although not as high as the hydroxyl hydrogens Groups like -NH2 or -OCH3 are electron donating and decrease the acidity

Answer 124

As described above, oxidation of aldehydes and primary alcohols with strong oxidizing agents ((N)Cr2O7, CrO3, KMnO4)

Answer 125

Nucleophile- can add to carboxylic acid and substitute for -OH while donating a proton Different than aldehydes or ketones because those participate in addition Weak bases (Conjugate bases of strong acids) make good leaving groups

Answer 126

Amides - Carboxylic acids can be converted into amides with the addition of an amine in an acidic or basic solution - Amides that are cyclic are called lactams and replace -oic with -lactam

Answer 127

A reaction of carboxylic acids with alcohol under acidic conditions results in formation of an ester, with the R- of the ester replacing the -H of the carboxylic acid’s hydroxyl group - occurs most rapidly with primary alcohols - in acidic conditions Condensation reaction with water side product Esters that are cyclic are called lactones and replace -oic with -lactone

Answer 128

Anhydrides can be formed by the condensation of two carboxylic acids

Answer 129

Carboxylic acids can be reduced to primary alcohols by the use of LiALH4

Answer 130

beta-keto acids like 1,3-dicarboxylic acids may spontaneously decarboxylate when heated

Answer 131

Long chain carboxylic acids reacted with sodium or potassium hydroxide to create a salt (H of the hydroxyl is replaced with Na or K) Know the product as soap

Answer 132

Amides, Esters and Anhydrides are all formed by a condensation reaction with a carboxylic acid

Answer 133

synthesized by reaction of other carboxylic acid derivatives with either ammonia or an amine

Answer 134

dehydration synthesis products of other carboxylic acid derivatives and alcohols

Answer 135

Under acidic conditions, mixtures of carboxylic acids and alcohols will condense into esters with the R replacing the H of the hydroxyl group

Answer 136

condensation dimers of carboxylic acids, wherein the oxygen of one carboxylic acids hydroxyl group bonds to the alpha carbon of another

Answer 137

Anhydrides are most reactive, followed by esters (tied with carboxylic acids although they usually have lower boiling points) and then amides

Answer 138

certain times lactams and lactones are more reactive to hydrolysis because they contain more strain four membered rings have torsional strain from eclipsing interactions and angle strain from not having a 109.5\* angle

Answer 139

Addition of a nucleophile to an anhydride results in carboxylic acid derivative and carboxylic acid -derivative depends on nucleophile; if amine the derivative is an amide

Answer 140

Alcohols can act as nucleophiles and displace the esterifying group on an ester, transforming one alcohol for another

Answer 141

Amides can be hydrolyzed under highly acid conditions via nucleophilic substitution, replacing an -NH2 with a -OH from water

Answer 142

generates an amino acid from an aldehyde An aldehyde is mixed with **ammonium chloride (NH4Cl) and potassium cyanide**. The ammonia attacks the carbonyl carbon, generating an **imine**. The imine is attacked by the cyanide, generating an **aminonitrile** The aminonitrile is hydrolyzed by two equivalents of water, generating an amino acid

Answer 143

generates an amino acid from **potassium phthalimide, diethyl bromomalonate, and an alkyl halide** phthalimide attacks the diethyl bromomalonate, generating a phthalimid-omalonic ester The phtalimidiomalongic ester attacks an alkyl halide, adding an alkyl group to the ester The product is hydrolyzed, creating phthalic acid and converting the esters into carboxylic acids One carboxylic acid of the resulting 1,3-dicarbonyl is removed by decarboxylation

Answer 144

fingerprint region of 1500 to 400 cm-1 Hydroxyl group at 3300 for alcohols, 3000 for carboxylic acids with broad peak carbonyl at 1700 with sharp deep peak (aldehydes and ketones) NH bonds at 3300 with sharp peak

Answer 145

never have to interpret but is obtained by passing light through a sample and recording the absorbance

Answer 146

left is downfield and increasing chemical shift TMS is marked at 0, ignore it The height of each peak is proportional to the number of protons it contains electronegative atoms pull electron density downfield the number of peaks indicates the number of adjacent protons

Answer 147

Aldehyde Hydrogens \> 9 to 10 ppm Carboxylic acids Hydrogens \> 10.5 to 12 ppm Aromatics Hydrogens \> 6.0 to 8.5 ppm

Answer 148

sp3 hydrogens -\> 0 to 3 ppm sp2 (alkene) hydrogens -\> 5 to 7 ppm sp hydrogens -\> 2 to 3 ppm

Answer 149

have an aqueous phase and a organic phase once the desired product has been isolated in the solvent, we can obtain the product alone by evaporating the solve, usually with a rotovap

Answer 150

isolates a solid (residue) from a liquid (filtrate) Gravity filtration is used when the product of interest is in the filtrate, hot solvent is used to maintain solubility Vacuum filtration is used when the product of interest is solid. A vacuum is connected to the flask to pull the solvent through more quickly

Answer 151

separates liquids according to their boiling point Simple distillation if the boiling points are under 150C and are at least 25C apart Vacuum distillation if the boiling points are over 150C to prevent degradation of the product Fractional distillation if the boiling points are less than 25C apart because it allows more refined separation of liquids by boiling point

Answer 152

Use two phases to separate compounds based on physical or chemical properties the stationary phase or adsorbent is a polar solid the mobile phase runs through the stationary phase and is usually a liquid or gas

Answer 153

TLC and paper chromatography the stationary phase is a polar material, such as silica, alumina, or paper the mobile phase is a nonpolar solvent, which climbs the card through capillary action

Answer 154

need to insert

Answer 155

Rf- Retardation factor distance spot moved / distance solvent front moved

Answer 156

uses an entire column filled with silica or aluminum beads as an adsorbent ion exchange chromatography, size exclusion chromatography, affinity chromatography

Answer 157

Ion exchange chromatography the beads are coated with charged substance to bind compounds with opposite charge Size exclusion chromatography the beads have small pores which trap smaller compounds and allow larger compounds to travel through faster Affinity chromatography the column is made to have high affinity for a compound by coating the beads with a receptor or antibody

Answer 158

separates vaporizable compounds according to how well they adhere to the adsorbent in the column the stationary phase is a coil of crushed metal or a polymer, the mobile phase is an inert gas can be combined with mass spectroscopy to ionize the fragments and determine molecular weight or structure

Answer 159

similar to column chromatography but uses sophisticated computer-mediated solvent and temperature gradients

CHEMISTRY/ORGANIC CHEMISTRY FINAL REVIEW Flashcards

(188 cards)