Dat Organic Chem

Front 1

two atomic orbitals combine to form

Back 1

bonding molecular orbital+ antibonding molecular orbital

Front 2

molecular/atomic orbitals can contain a maximum of --- electrons

Back 2

2

Front 3

pi bonds are formed by ---

Back 3

overlapping p orbitals

*2 p orbitals

Front 4

sigma bond can be formed by

Back 4

2 s orbitals
2 p orbitals
1 s and 1 p orbital

Front 5

formation of carbocation is

Back 5

rate limiting step

Front 6

rate limiting step involves 2 molecules

Back 6

SN2

Front 7

CN is a good/strong ---

Back 7

nucleophile

Front 8

tosylate is a good/strong ---

Back 8

leaving group

Front 9

produce several different radical compounds

Back 9

Cl2

Front 10

produce major product under radical reactions

Back 10

Br2

Front 11

Br2 + Alkyne

Back 11

trans addition

Front 12

hydroboration of alkynes

Back 12

syn addition (cis alkene)

Front 13

hydroboration:

terminal alkynes require --- borane

Back 13

disubstituted

(page 314)

Front 14

halogens are EWG that are

Back 14

ortho-paradirecting

Front 15

R-O-R (ether) + HX (strong acid) =

Back 15

2 X-R

Front 16

carbonyl + excess alcohol

Back 16

ACETAL

Front 17

expected to decarboxylate in the presence of heat

Back 17

beta-keto acids

Front 18

example of conformational isomer

Back 18

cis and trans

Front 19

hydrolysis of acid chloride results in

Back 19

HCl and carboxylic acid

Front 20

steric hinderence is important in formation of ---

Back 20

esters

page 402

Front 21

carboxylic acids in the presence of base

Back 21

deprotonated in the form of a salt

Front 22

carboxylic acids in the presence of acid

Back 22

protonated

Front 23

R-C-N

Back 23

nitrile

Front 24

N-N

Back 24

diazocompound

Front 25

RNHCOOR

Back 25

urethane

Front 26

N-N-N

Back 26

azide

Front 27

amine + R- I
AgO
H2O

Back 27

Hoffman rearrangement

yields:
1) trisubstituted amine
2) least substituted alkene

Front 28

separates dissolved substances based on differential solubility in aq. vs organic solvents

Back 28

extraction

Front 29

separates solids from liquids

Back 29

filtration

Front 30

separates solids based on different solubilities

Back 30

recrystallization

Front 31

separates large macromolecules and cells based on mass and density

Back 31

centrifugation

Front 32

separates liquid based on boiling point

Back 32

distillation

Front 33

separates compounds based on how polar they are and sometimes size

Back 33

chromatography

Front 34

used to separate biological macromolecules (proteins or nucleic acids) based on size and sometimes charge

Back 34

electrophoresis

Front 35

used to separate molecules who have very similar boiling point

Back 35

fractional distillation

Front 36

Rf value

Back 36

distance traveled/solvent distance traveled

Front 37

less polar solvent in TLC means
--- distance traveled for solvent

Back 37

less

Front 38

--- molecules elute first in column chromatography

Back 38

nonpolar

Front 39

ether extractions are more successive when---

Back 39

when you perform multiple reactions

Front 40

no IR spectrum for molecules that do not change their ---

Back 40

dipole moment

example: O2

Front 41

Carbon 12 is not used for NMR because

Back 41

it has no magnetic moment

Front 42

9-10 ppm

Back 42

aldehyde proton

Front 43

2-3 ppm

Back 43

alkyne proton

Front 44

5-6 ppm

Back 44

alkene proton

Front 45

10-12

Back 45

carboxylic acid proton

Front 46

splitting of spectrum lines in CNMR

Back 46

coupling between a carbon atom and protons attached to that carbon

Front 47

most useful for detecting conjugated alkenes

Back 47

UV spectroscopy

Front 48

mass spectrometry results in separation of fragments according to---

Back 48

mass to charge ratio

Front 49

alkene nomenclature

Back 49

start numbering with alkene

Front 50

halide nomenclature

Back 50

give halide lowest possible number

Front 51

alcohol nomenclature

Back 51

give OH group lowest possible number

Front 52

ketone has --- double bond in nomenclature

Back 52

priority

Front 53

rotation about one or more single bond

Back 53

conformational isomers

*person sitting up or sitting down

Front 54

most stable/energy minima conformation in newman projection

Back 54

staggered or anti conformation

(2 methyls are 180 apart)

Front 55

two methyls are 60 degrees apart

Back 55

gauche

Front 56

highest energy state in newman projection

Back 56

totally eclipsed

Front 57

when 2 methyls overlap each other (0 degrees apart)

Back 57

totally eclipsed

Front 58

two methyls are 120 degrees apart

Back 58

eclipsed

Front 59

bond angles deviate

Back 59

angle strain

Front 60

cyclic molecules are eclipsed

Back 60

torsional strain

Front 61

atoms compete for the same space

Back 61

nonbonded strain

Front 62

high energy state of cyclohexane

Back 62

boat

A --> E
eclipsed!

Front 63

all 3 types of strain are limited in which cyclohexane conformation

Back 63

chair

Front 64

large atoms tend to be better nucleophiles in --- solvents

Back 64

protic

CN > I > RO > HO > Br> Cl > F

Front 65

smaller atoms tend to be better nucleophiles in --- solvents

Back 65

aprotic

F> Cl > Br > I

Front 66

--- bases make good leaving groups

Back 66

weak bases

Front 67

formation of peptide bond involves

Back 67

condensation reaction

Front 68

other covalent bonds found in amino acids

Back 68

disulfide bonds

Front 69

carbanion stability

Back 69

opposite of carbocation

1>2>3

Front 70

carbocation stability

Back 70

3>2>1

Front 71

whether a molecular orbital is bonding or antibonding depends solely on ---

Back 71

the signs of the atomic orbitals

Front 72

--- DO NOT show up in net ionic equations

Back 72

spectator ions

Front 73

how do you determine mass of a single atom

Back 73

atomic weight/ avogadros number

Front 74

calculating bond length of pure compounds

Back 74

take average

Front 75

pure gases have low melting points because

Back 75

they are covalently bonded, non-polar, and have very minimal IMF

Front 76

8.314 is used for

Back 76

kPa

Front 77

---does not change with temperature and remains constant as a solution is heated

Back 77

molality

Front 78

pka + pkB=

Back 78

14

Front 79

(Acids or Bases) dissolve things

Back 79

acids

Front 80

spontaneous reactions produce an --- in entropy

Back 80

increase

Front 81

units for 2nd order reaction

units for third order reaction

Back 81

(M-1)(s-1)

(M-2)(s-1)

Front 82

two unequal concentrations will tend to equalize due to

Back 82

entropy

*drives current

Front 83

as period number increases ---- increases

Back 83

molecular weight

Front 84

occurs after the reaction takes place to balance the charges and does not drive the current

Back 84

deposition of ions from the salt bridge

Front 85

reducing sugars are ----

Back 85

hemiacetals

look for OH on anomeric carbon

Front 86

test used for alkenes

Back 86

KMnO4

Front 87

Test for aldehydes and ketones

Back 87

Schiff Base
Tollens
Bisulfite
Iodoform

Front 88

to determine which resonance structure is most stable...

Back 88

count and see if all atoms have FULL octet!

Front 89

example of ketohexafuranoside

Back 89

fructose

Front 90

grignard + epoxide =

Back 90

basic condition

least sub side gets attacked
most sub gets OH
retention of stereochemistry

Front 91

trans alkene from alkyne

Back 91

Na, NH3

Front 92

Diels Alder Reaction:

groups with pi bonds placed in --- position

Back 92

endo position