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IB CHEMISTRY 2017 EXAM > Topic 10; Organic Chemistry > Flashcards

Topic 10; Organic Chemistry Flashcards

1
Q

saturated reactant

A

compound which contain only single bonds

e.g. alkanes

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2
Q

unsaturated reactant

A

compounds which contain double or triple bonds

e.g. alkenes, arenes

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3
Q

alipathic

A

compounds which don’t contain a benzene ring; can be saturated or unsaturated

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4
Q

arene

A

compounds with a benzene ring; unsaturated compounds

e.g. benzene, phenol

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5
Q

electrophile

A

(electron-seeking)

  • an electron-deficent specie which is therefore attracted to pars of a molecule which are electron rich
  • are positive ions or have partial positive charge
  • e.g. NO2, H+
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6
Q

nucleophile

A

(nucleus seeking)

  • an electron-rich species which is therefore attracted to parts of molecules which are elctron deficient
  • have alone pair of electrons
  • may have negative/partial negative charge

e.g. Cl-, OH-, NH3

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7
Q

addition reaction

A
  • occurs when two reactants combine to form a single product
  • characteristics of unsaturated compounds

C2H4 + Br2–> C2H4Br2

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8
Q

substituion reaction

A
  • occurs when on atom or group of atoms is replaced by a different atom or group
  • characteristics of saturated compounds and aromatic compounds

e.g.
CH3 + Cl2—> CH3Cl + HCL

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9
Q

addition-eliminiation reaction

A
  • occurs when two reactants join together (addidtion) and in the process a small molcule such as water, hydrocholric acid or ammonia is lost (elmination)
  • reaction occurs betwen functional group in each reactant
  • CONDENSATION reaction
  • e.g.
    alcohol + acid —> ester + water
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10
Q

homolytic fission

A

is when a covalent bond breaks by splitting the shared pair of electrons between the two products
- produces two free radicals, each with an unpaired electron
X2– > Xo and Xo

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11
Q

heterolytic fission

A

is when a covalent bond breaks with both the shared electrons going to one of the produces
- produces two oppositely charged ions
X2– > X+ and X-

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12
Q

homologous series

A
  • successive members differ by CH2 group
  • same general formula
  • show gradation in physical properties (e.g.boiling point, density, viscocity) increases with mass as london forces (increases due to more electrons)
  • similar chemical properties (same functional groups)
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13
Q

IUPAC names for carbon chains

A 
1- meth
2- eth
3- prop
4- but
5- pent
6- hex
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14
Q

alkene

  1. functional group?
  2. suffix?
  3. example?
  4. general formula/representation?
A

no functional group
-ane
CnH2n+2

e.g. ethane (C6H6)

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15
Q

alkane

  1. functional group?
  2. suffix?
  3. example?
  4. general formula/representation?
A

alkenyl

  • ene
  • ethene C2H4

CnH2n

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16
Q

alkyne

  1. functional group?
  2. suffix?
  3. example?
  4. general formula/representation?
A

alkynyl

  • yne
  • ethyne; C2H2

formula; CnH2n-2

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17
Q

alcohol

  1. functional group?
  2. suffix?
  3. example?
  4. general formula/representation?
A

hydroxyl

  • anol
  • ethanol; C2H5OH

CnH2n+1OH

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18
Q

ether

  1. functional group?
  2. suffix?
  3. example?
  4. general formula/representation?
A

ether

  • oxyalkane
  • methoxyethane; H3–C–O–C2H5
  • R–O–R
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19
Q

aldehyde

  1. functional group?
  2. suffix?
  3. example?
  4. general formula/representation?
A

aldehyde (carbonyl)

  • anal
  • propanal; C2H5CHO
  • R—CHO
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20
Q

ketone

  1. functional group?
  2. suffix?
  3. example?
  4. general formula/representation?
A

carbonyl
-anone
- propanone; CH3COCH3
R–CO–R

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21
Q

carboxylic acid

  1. functional group?
  2. suffix?
  3. example?
  4. general formula/representation?
A

carboxyl
-anoic acid
C2H5COOH3; propanoic acid
- CnH2n+1COOH

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22
Q

ester

  1. functional group?
  2. suffix?
  3. example?
  4. general formula/representation?
A

ester

  • anoate
  • methyl propanoate; C2H5COOCH3
  • R—COO—R
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23
Q

amide

  1. functional group?
  2. suffix?
  3. example?
  4. general formula/representation?
A

carboxyamide

  • anamide
  • propanamide; C2H5CONH2
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24
Q

amine

  1. functional group?
  2. suffix?
  3. example?
  4. general formula/representation?
A

amine
-anamine
C2H5NH2; ethanamine

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25
Q

nitrile

  1. functional group?
  2. suffix?
  3. example?
  4. general formula/representation?
A

nitrile

  • anenitrile
  • C2H5CN; propanenitrile
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26
Q

arene

  1. functional group?
  2. suffix?
  3. example?
  4. general formula/representation?
A

phenyl

  • benzene
  • C6H5CH3; Methyl Benzene
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27
Q

alkane side chains

A
  • methyl
  • ethyl
  • propyl, etc
28
Q

halogenoalkane side chains

A

fluoro
chloro
bromo
iodo

29
Q

amine side chains

30
Q

structural isomers

A

molecules that have the same molecular formula, but different arrangement of the atoms

31
Q

primary carbon compound

A
  • attached to a functional group and at least two other hydrogen atoms
32
Q

secondary carbon compounds

A
  • attached to a functional group and also to one hydrogen atom and two alkyl groups
33
Q

tertiary compounds

A
  • attached to functional group and three allkyl groups (no hydrogen atoms)
34
Q

primary alcohols

A

oxidation: two step process; form aldehyde and then carboxylic acids
- cause orange to green colour change of potassium dichromate
- aldehyde can be removed using distillation; stops full reaction

e.g.
ethanol —> ethanal—> ethanoic acid (using reflux)
- use exces oxygen and heat

35
Q

secondary alcohols

A

oxidize to ketone
cause orange to green colour change in potassium dichromate

e. g. pronan-2-ol becomes propanone and water
- uses excess oxygen and heat in a reflux reaction

36
Q

tertiary alchol

A

isnt oxidized

no colochange

37
Q

oxidization reaction; why does Cr(VI) change colour?

A
  • use of acidified potassium dichromate (VI); orange solution
  • Cr(VI) ion reduced to Cr(III) caues the orange to green colour change
38
Q

arene

A

derived from benzene (C6H6); phenyl functional group

- no isomers, atypical reactivity for an unsaturated particle

39
Q

explain benzene structure

A
  • benzene cyclic structure; 120 bond angles
  • hexagonal; stable structure
  • high degree of unsaturation
  • delocalized electrons cause resonant structure
  • stable arragangement; lowers internal energy
40
Q

explain benzene properties

A
  • all C-C bonds are equal and intermediate in length between single and double bonds (each bond has three electrons between bonded atoms)
  • hydrogenation enthalpy for reaction is stable; its in between a double and single bond due to resonant structure (delocalization minimizes repulsion; stable structure and low internal energy)
  • benzene udnergoes substitution reactions; reculant to addition reaction (doesn’t want to disrupt cloud of delocalization)
  • 1, 2-dibromobenzene is the only isomer
41
Q

physical properties of organic compounds

A
  • in response to increasing mass/ branching (lower members of series usually gas, higher members become liquid and solids)
  • branching affects volaitity due strength of intermolecular forces; harder to stack
  • different polarities + intermolecular forces; functional groups affect
42
Q

halogen affect on boiling point of organic compound

A

alkane>halogenoalkane> aldehyde>ketone>alcohol>carboxylic acid

43
Q

intermolecular force order in boiling point

A

london forces

dipole-dipole

hydrogen bonding 
(as strength of intermolecular attraction increases)
44
Q

alkanes

A
  • low reactivity
  • undergo free radical substitution reactions
  • saturated hydrocarbons
  • use as fuels (combustion)
45
Q

alkane combustion

A
  • used as fuels in international combustion engines or household heating
  • highly exothermic reaction due to energy released in forming double bond sin CO2 and H2O bonds
  • burn in presence of excess oxygen to produce carbon dioxide and water
46
Q

alkane incomplete combistion

A
  • produces carbon monoxide and water

- extreme oxygen limitation produces just carbon and water

47
Q

alkane combustion implications

A
  • carbon dioxide and water both green house gases; absorb IR radiation and contribute to global warming/climate change
  • carbon monoxide is toxic; combines irreversibly with haemoglobin; important to provide ventilation in fuel burning places
  • unburned carbon causes issues in human healthy, and act as catalysts in polluted air; cause global dimming
48
Q

alkane halogenation (free radical subsitution)

A
  • alkanes satured; can undergo substitution with chlorine or bromine
  • reaction only takes places if there is UV light to break covalent bond in chlorine bond
  • doesnt work in the dark
  • forms free radicals to start a chain reaction to form halogenalkane
49
Q

free radical substitution; intiation

A
  • UV breaks bond in chlorine (photochemical homolytic fission)
  • produces two chlorine radicals
50
Q

free radical substituion; propagation

A
  • free radicals reaction with carbon compounds
  • continous process

e.g.
CH4+ Clo—> CH3o + HCL
CH3o + Cl2—> CH4Cl + Clo
CH2CLo + Cl2–> CH2CL + Clo

51
Q

free radical substitution; termination

A
  • when two radicals react together to pair up their electrons
    e. g.

Clo + Clo–> Cl2

CH3o + Clo–> CH3CL

CH3o + CH3o—> C2H6

52
Q

free radical?

A

a free radical contains an unpaired electron and is very reactive

53
Q

how can you tell if a compound is an alkane or alkene?

A
  • use bromine water test in dark; as alkane need UV light to react whereas alkene don’t
54
Q

alkenes

A 
unsaturated hydrocarbons
high reactivity 
double bond 
undergo addition reactions
are used as starting matierals in the manufacture of many indusrially imporatnt chemicals
55
Q

halogenation of alkene

A
  • addition of halogen (bromine, chlorine, iodine) to form halogenoalkane
  • room temperature
  • loss of color in solutions
  • HBr, HCl or HI can be used ad addition halogen hallides
  • HI> HBr> HCl reactivity order
56
Q

hydrogenation of alkene

A
  • addition of hydrogen to form an alkane
  • Nickle Catalyst
  • 150 C
  • used to convert oils to saturated compounds such as transfats
57
Q

hydration of alkene

A

alkene —> alcohol

  • addition of water to produce an alcohol
  • concentrated sulfuric acid catalyst
  • head with steam
  • industrial significance; ethanol is important solvent
58
Q

polymerization of alkene

A
  • addition polymers formed
  • repeating units
  • polymers contain thousands of monomer molecules

e.g. ethene polymerizes to form poly(ethene)

59
Q

alcohols

A
  • hydroxyl functional group

- hydroxyl is polar; icnreases solubliity of compounds in water (relative to comparable molar masses)

60
Q

alcohol combustion

A
  • used as fuel; burn in oxygen to form carbon dioxide and water
  • used in alcohol burners, etc
  • enthalpy increases up the homologous series
  • limited oxygen, produces carbon monoxide
61
Q

oxidizing agents used in alcohol combustion

A
  • acidified potassium dichromate (VI)
62
Q

alcohol esterification reaction

A
  • condensation reaction
    carboxylic acid + alcohol produces ester and a water
  • ethanol + ethanoic acid produces ethyl ethanoate
  • concentrated sulfuric acid catalyst
63
Q

halogenalkane

A

F, Cl or I bonded to a hydrocarbon
saturated molecules; reactions involve substitution
- polar bond makes them more reactive

64
Q

nucleophillic substitution

A
  • halogen atom more electronegative than carbon= more polar than carbon; halogen has partially negative charge and carbon partially positive (electron deficient)
  • nucleophiles (electron rich reactants with lone pair or negative charge) attracted to electron deficient carbon in halogen; replace the halogen
    e. g. NaOH + CH3Cl—> CH3OH + NaCl
65
Q

benzene

A
  • delocalized electrons give it a special stability; adiddtion reactions are favoured to avoid loss of stable aromatic rings
  • delocalized ring of electrons is the site of reactivity
66
Q

benzene electrophyllic reactions

A
  • electrophile; electron deficient species that wants electron pairs and forms a bond (positive ion)
  • benzne reacts with nitronium ion (NO2+ from nitric acid) to form nitro-benzene and water
  • aluminium trichloride in dry ether used as catalyst

IB CHEMISTRY 2017 EXAM (12 decks)

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