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HL Chem > 10.1 organic chemsitry > Flashcards

10.1 organic chemsitry Flashcards

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1
Q

define homologous series

A
  • series of compounds
  • same family
  • same general formula
  • differ from each other from a common structural unit
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2
Q

alkane general formula

A

CnH2n+2

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3
Q

nucleophile vs electrophile

A

electron pair donor vs acceptor

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4
Q

drawing arrows convntion

A

full arrow — electron pair
half arrow – single electron
these are curved

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5
Q

chiral carbon (a sterocenter)

A

diff groups on all sides

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6
Q

how to determine if a double bond is a stereo center

A

if it can form cis/trans, 4 distinct grpsh

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7
Q

how to calculate no of enantiomers

A

2^no of seterocenters

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8
Q

nitration of benzene conditions

A

conc H2SO4, 50C
benzene + conc HNO3

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9
Q

definition nitration (of benzene)

A

electrophillic substitution of a H atom by a nitro grp. -MO2

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10
Q

equation (drawn) for nitration of benzene

A

(o) + HNO3 (conc) –H2SO4 (conc), 50C–> (o)–NO2 + H2SO4 (regenerated)

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11
Q

mechanism of nitration of benzene *

A
  1. generation of electrophile, NO2+
    HNO3 + 2H2SO4 <—> NO2+ + H3O+ + 2HSO4-
  2. no2+ attacked by delocalised pi electrons,
    - 1 pair (curved arrow) removed to NO2+ –SLOW–> complicated intermediate. –> (O)–NO2 + H2SO4 (regen)

intermediate
H and NO2 on same corner, HSO4-: (curved arrow to H). (O) interior missing that end of the circle. plus sign in center

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12
Q

boiling point trends for organic molecules

A

BP incr with incr size

each -CH2- = incr London Dispersion Forces = incr

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13
Q

how is a molecule represented with condensed structural formula (propene?)

A

propene –> CH2 = CHCH3

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14
Q

what are strucural isomers

A

same molecular formula but different structural formulae

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15
Q

what is branch-chain isomerism

A

same molecular formula BUT longest hydrocarbon chain is not the same

  • caused by branching
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16
Q

name the 3 types of structural isomerism

A

branch-chain

positional

functional

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17
Q

what are positional isomers

A

differences in position of functional group

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18
Q

what is functional group isomerism

A

diff functional grps result in the same molecular formula

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19
Q

when given a formula eg CH3CH(CH3)CH2CH3 what do the brackets mean

A

side chain!

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20
Q

how is a side chain named

A

it is an alkyl group!

CH3 = methyl

tri/di etc eg trimethyl – this is the total in the molecule

carbon number is listed in from eg
3, 3, 4

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21
Q

what if theres more than one type of side chain? how do you name them then

A

alphabetical order

eg 4-ethyl-2-methyl hexane

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22
Q

alkene general formula

A

CnH2n

23
Q

how is the double bond in an alkene presented

A

but-1-ene

24
Q

alkynes general formula

A

CnH2n-2

they have a triple bond!

pent - 1 -yne

25
Q

what are arenes

A

compounds with 1 or 2 more rings with pi electrons that are delocalised

26
Q

what compounds are aromatic

A

arenes

27
Q

what is the one aromatic hydrocarbon covered in IB!

A

BENZENE !!! C6H6

28
Q

what is the functional group of benzene

A

phenyl group

29
Q

general formula of halogenoalkanes

A

Cn H2n+1 X

30
Q

how are haloalkanes named

A

prefix is the halogen
chloro-

ending -ane

1,1-dibromopropane
1-bromo-2-chloropropane

31
Q

what are ethers

A

the ones with the O in the middle
R-O-R

functional group isomers of alcohols

32
Q

general formula of ethers

A

CnH2n+2O

33
Q

naming ethers 2

A

meth oxy ethane

(older)
ethyl methyl ether (the two sides then ether)

34
Q

what is the functional group of carbonyls

A

C = O

35
Q

general formula for carbonyl

A

CnH2nO

36
Q

aldehydes vs ketones

A

aldehydes: carbonyl grp on the end of the chain

ketones: min. 3 carbons, carbonyl not on ends

37
Q

nomenclature of aldehydes vs ketones

A

a: – al
k: – one

ethanal
propanone

38
Q

differences in reactions between aldehydes and ketones is bc of ?

A

the H on the aldehyde / nature of the R group

39
Q

consequences of having a C=O bond (polarity)

A

diff in electrongeativity = polar = dipole-dipole

  • higher BP (for small molc)
  • solubility in water for lower members
40
Q

carboxylic acids general formula

A

RCOOH

41
Q

what are esters

A

functional grp isomers of carboxylic acids

carboxylate
-COOR

42
Q

nomencalture of esters

A

so its like the C=O sticks out and the -C-O- is bonded to groups SO the name “methyl ethanoate” the first part is for the group bonded to the O, the second is for the part bonded to the C (including the C)

so that would be
C - C - O - C
O

43
Q

why are chemical and physical properties of carboxylic acids and esters different despite benig functional group isomers

A

carboxylic acids have H-BONDS

CA: smaller chain soluble in water, higher BP
esters: insoluble, lower BP

44
Q

amines vs amides vs nitriles

A

amines: NH2
amides: CONH2
nitriles: CN (cyanide grp)(triple bond)

45
Q

what is sterochemistry

A

the study of relative spatial arrangements of atoms in molecules

46
Q

how to determine if its a primary, secondary, or tertiary alcohol/halogenoalkane

A

ok so look at the carbon that the OH is attached to. then how many C atoms is that C attached to. tahts it

47
Q

primary sec ter for AMINES yes its different

A

number of alkyl grps attached to the N

48
Q

kekules structure for benzene PROBLEMS 3

A
  • similar reactivity to ethene: NAH ethene has addition reactions while benzene has substitution reactions
  • shorter double, longer single bonds: ERM ACTUALLY they were the same lenght
  • banzene is actually more stable than expected
49
Q

lenght of bonds in benzene

A

intermediate between single and double bonds

50
Q

kekule strucure for benzene

A

hexagon with 3 double bonds
equivalent to 3 ethene molecules

51
Q

why is benzene more stable than expected

A

delocalisation energy from the delocalised electrons

52
Q

benzene is a (shape) with bond angles of ()

A

planar regular hexagon

120 degrees

53
Q

all carbons in benzene are sp?

A

sp2

forms sigma bonds with

54
Q

explain the delocalisation of electrons in benzene

A

sp2 hybridised carbons form sigma bonds with 2 other C + 1 H

remaining p orbital overlaps = forms system of pi bonds spread across whole ring

electrons are not bound to specific atoms, freely move around

HL Chem (28 decks)

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