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organics Flashcards

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1
Q

saturated vs unsaturated

A

saturated = max number of hydrogen bonds (alkanes)
unsaturated = contains double or triple carbon bonds which can be broken to add more hydrogen atoms

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2
Q

functional groups

A

specific groups of atoms within molecules that have their own properties and characteristics in a chemical reaction

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3
Q

homologous series

A

a series of compounds containing the same functional group, differing by only the number of carbon atoms in the chain

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4
Q

isomers

A

compounds with the same molecular formula but different arrangement of atoms

there is chain, position, and functional

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5
Q

requirements for geometrical isomers

A
  • molecule is asymmetrical
  • each carbon atom is bonded to two different atoms/groups of atoms
  • there is a double bond to prevent rotation and fix the atoms in place

cis and kiss

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6
Q

properties of alkanes

A

saturated, single bonds only, relatively low mp and bp due to weak intermolecular forces.

alkanes with 1-4 carbons are gases at room temperature

alkanes are not polar, they are not soluble. they will form layers in water. they are also non-conductors due to electrons being fixed in covalent bonds

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7
Q

substitution reaction of alkanes

A

requires a halogen, Cl2 or Br2.

UV light catalyst required, the reaction is slow

hydrogen gas product

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8
Q

distinguishing test of alkanes and alkenes

A

add (MnO4)- or (Cr2O7)2- the alkane will form a layer on top and there is no colour change. the alkene will oxidise and go colourless

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9
Q

properties of alkenes

A

unsaturated, higher mp and bp due to its double bond which also makes it more reactive

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10
Q

hydrogenation of alkenes

A

hydrogen gas is added, the double bond is broken and an alkane is produced

conditions: Pt, at 150c

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11
Q

halogenation of alkenes

A

hydrogen halide or halogen gas is added to make a haloalkane

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12
Q

hydration of alkenes

A

water is added to produce an alcohol

conditions: H+ and heat

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13
Q

markovnikovs rule

A

the rich get richer

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14
Q

oxidation of alkenes

A

a strong oxidation will produce a diol

naming: butan-1,2-diol

colour change of (MnO4)- = purple to brown in the absence of acid

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15
Q

properties of alcohols

A

there is strong hydrogen bonding between the OH group and neighbouring alcohol molecules. it has a higher mp and bp than alkanes.

alcohols with 1-8 carbons are liquid at room temperature

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16
Q

solubility of alcohols

A

decreases as carbon chain increases

1-3C = very soluble
4C = soluble
5-6C = partially soluble
7+ C = insoluble due to large non-polar reigons

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17
Q

substitution of alcohols to produce a halogen

A

reagents = SOCl2, PCl3, PCl5

SOCl2 is a good reagent as HCl and SO2 product are gases. Liquid product is purely the haloalkane

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18
Q

nucleophiles

A

they are attracted to nuclei, positive charge. they have lone electron pairs / negative charge.

examples = Cl-, Br-, OH-, NH3, H2O

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19
Q

nucleophilic substitution of primary alcohols

A

reagent = NH3

produces an amine (NH2)
excess NH3 is required, the H from the amine (of the original NH3) produces NH4, producing NH4OH (ammonium hydroxide) as the OH is removed from the alcohol

conditions = heat
- this is to increase the rate of reaction and help particles overcome activation energy

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20
Q

nucleophilic substitution of tertiary alcohols

A

has 2 steps

  1. slow reaction which just removes the OH group producing a carbocation
  2. fast reaction where a nucleophile is attached. it is attracted to the carbon which the OH group was attached to due to its positive charge. must draw an arrow between the carbocation and nucleophile

conditions = heat is required for both steps

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21
Q

elimination of alcohols

A

alkene and water is produced

conditions = conc.H2SO4 or Al2SO3 and heat

conc.H2SO4 is a dehydrating agent

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22
Q

zaitseff’s rule

A

the poor get poorer

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23
Q

oxidation of primary alcohols

A

two steps

  1. distillation, an aldehyde is produced (C double bonded to H)
  2. reflux, a carboxylic acid is produced

conditions: H+ and heat

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24
Q

oxidation of secondary alcohols

A

a ketone is produced (C double bonded to O) hydronium ions and electrons are produced

unlike aldehydes, ketones cannot be further oxidised

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25
oxidation of tertiary alcohols
cannot happen - activation energy is too high - carbon has max bonds already
26
properties of haloalkanes
almost insoluble, colourless, odourless, partially cloudy, less flammable than alkanes but more reactive, mostly liquid or solid at room temp
27
nucleophilic substitution of haloalkanes
1. NaOH or KOH (aq) an alcohol is produced conditions = reflux 2. conc. ammonia (alc) produces an amine conditions = heat (warm) and excess ammonia to produce ammonium
28
elimination of haloalkanes
conc. NaOH or KOH (alc) alkene, water and halogen product conditions = reflux
29
properties of amines
has hydrogen bonding and temporary dipole-dipole attractions between amine molecules, high mp + bp, slightly polar due to NH2 group, low molar mass amines are volatile liquids, high molar mass amines are solids at room temp
30
amine in water reaction
NH2 becomes NH3+ and an OH- is produced
31
how does an amine produce a salt
amines are bases so they react with acid to produce a salt Ethylamine + HCl produces ethylammonium chloride. H in HCl adds to amine and Cl is added after
32
Amine and CuSO4
produces a pale blue precipitate then a deep blue solution.
33
how to produce a secondary amine
add chloroalkane H attached to amine is slightly positive and Cl in haloalkane is slightly negative. they produce HCl. Two new bonds are in each molecule so they combine together
34
what does HCl do after the production of secondary amines
they may react with the amine reactant to produce a salt
35
physical properties of carboxylic acids
weak acids, high mp and bp than alkanes of a similar molar mass, they have 2 functional groups blue litmus goes pink insoluble in water unless they have a low molar mass water insoluble carboxylic acids are soluble in NaOH due to conversion of the acid to a carboxylate ion hydrogen bonding between acid molecules which can produce a dimer
36
carboxylic acid behaviour in water
they partially dissociate the H in COOH donates an H to H2O to produce H3O+ there is an equilibrium that is positioned to the left
37
carboxylic acids and metal
a salt is produced and hydrogen gas ex. magnesium ethanoate
38
carboxylic acids and base
salt and water
39
acid and carbonate
salt, water, carbon dioxide
40
nucleophilic substitution of carboxylic acids
the OH group can be substituted to produce an acyl chloride with SOCl2, PCl3, PCl5 they can also produce an amide with NH3 (alc) but not haloalkanes
41
physical properties of esters
lower mp and bp than alcohols and carboxylic acids due to no hydrogen bonding insoluble in water forming layers distinctive odour, fruity volatile high mass esters are waxy solids with a less distinctive smell
42
what functional groups are isomers
carboxylic acids and esters aldehydes and ketones
43
the slow way to produce an ester
esterification / condensation requires: heat, reflux, conc. H2SO4 (dehydrating agent) propanoic acid and alcohol
44
faster way to produce an ester
acyl chloride and alcohol no conditions and higher yield. no catalyst or heat is needed
45
hydrolysis of esters in acid conditions
equilibrium reaction splits ester back into alcohol and carboxylic acid reagent: H2O/H+
46
hydrolysis of esters in basic conditions
creates alcohol and a salt (conjugate salt of the acid) reagent: NaOH conditions: conc. H2SO4
47
esterification of glycerol
stearic acid + glycerol (1,2,3 - propantriol) heat, reflux, conc. H2SO4 esterification that produces soap triglyceride is produced (a fat)
48
hydrolysis of triglyceride to produce soap
NaOH breaks the ester links in basic conditions. 3 fatty acid chains are produced which are ionic salts, soaps this is saponification glycerol is also produced fat + acid -) soap and triol
49
physical properties of acid chlorides
OH group of carboxylic acids are replaced by a Cl conc. HCl cannot be used to produce it as it would react with the acid chloride to produce a carboxylic acid low mp and bp due to no hydrogen bonding pungent fuming liquids
50
reactivity of acid chlorides
they are highly reactive due to the terminal carbon being bonded to two electronegative atoms. it is readily attacked by nucleophiles
51
hydrolysis of acid chlorides
rapid and violent a carboxylic acid and HCl is produced. the Cl is replaced by OH example of nucleophilic substitution 2 acids are produced, blue litmus goes pink
52
nucleophilic substitution of acid chlorides to produce primary amines
NH3 (alc) is required and replaces the OH group. excess is needed to produce NH4 combines with Cl to produce NH4Cl salt (ammonium chloride)
53
nucleophilic substitution of acid chlorides to produce secondary amines
primary amines react with acyl chlorides the OH group is replaced by the NH2 group and joins the two molecules together the H from the NH2 that joins to acid chloride is added to excess amine to produce a salt, the amine becomes NH4 at the end and Cl is added
54
why is NH3 (alc) used in substitution
because H2O is also a nucleophile and there would be competition
55
physical properties of amides
low carbon chain amines are soluble in water neutral to litmus, they are not bases like amines mp and bp is is high due to hydrogen bonding only found on terminal carbon
56
how are amides produced
acyl chlorides with ammonia (much faster) or esters with ammonia
57
thermal decomposition of ammonium salt to produce amide
ammonium salt = CH3CH2COONH4 will react with heat to produce an amide and water CH3CH2CONH2 + H2O the O comes from hydroxy O and the 2H comes from NH4
58
hydrolysis of amides in basic/alkaline conditions
with NaOH produces a salt and NH3 the Na and O produce salt and the H produces NH3
59
hydrolysis of amides in acid conditions
H2O and/or HCl (aq) produces a carboxylic acid and NH3 With HCl, NH4Cl is produced alongside carboxylic acid requires heat
60
describe enantiomers
enantiomers have the same physical properties such as solubility and melting point - they have the same atoms/groups of atoms. however, they rotate plane polarised light in equal but opposite directions - which non-optically active compounds cannot
61
requirements for an enantiomer
a chiral carbon. a carbon atom that is bonded to 4 different atoms/groups of atoms
62
racemic solution
a solution composed where both optical isomers are present equally. they cancel each other out when light is shone

chemistry (2 decks)

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