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Chemistry A-Level > 4.1 basic organic chem > Flashcards

4.1 basic organic chem Flashcards

(68 cards)

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1
Q

define nomenclature

A

system of naming compounds

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2
Q

what is a homologous series? give 3 examples

A

series fo substances with the same functional group and the successive members only differing by a CH₂ unit.

eg. alkanes, alkenes and alcohols

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3
Q

what is an alkane?

A

a saturated hydrocarbon

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4
Q

what is the alkane general formula?

A

CnH2n+2

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5
Q

name the first 10 alkanes

A

methane, ethane, propane, butane, pentane, hexane, heptane, octane, nonane, decane

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6
Q

define an aliphatic hydrocarbon

A

a hydrocarbon in which carbon atoms are joined in a straight chain or branched chains

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7
Q

define an alicyclic hydrocarbon

A

a hydrocarbon that is an aliphatic compound arranged in non-aromatic rings with or without side chains
(no benzene rings, still ring structure)

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8
Q

define aromatic hydrocarbon

A

a compound with a benzene ring

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9
Q

define general formula

A

an algebraic formula that can generate any molecular formula in a family.

eg. CnH2n+2

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10
Q

define empirical formula

A

simplest whole number ratio of atoms of each element in a compound.

eg. C2H6 –> CH3

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11
Q

define molecular formula

A

the actual number of atoms of each element in a compound

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12
Q

define structural formula

A

the minimal detail that shows the arrangement of atoms in a molecule.

eg. CH3CH2CH2CH2OH

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13
Q

what is the displayed formula

A

the relative positioning of atoms and the bonds between them

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14
Q

define skeletal formula

A

the simplified organic formula shown by removing hydrogen atoms, leaving just carbon chains and alkyl chains, with the functional groups.

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15
Q

what is the general formula for alkyl groups?

A

CnH2n+1

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16
Q

what is the prefix of an alcohol?

A

hydroxyl-

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17
Q

what is the suffix of an alcohol?

A

-ol

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18
Q

what is the suffix of an aldehyde?

A

-al

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19
Q

what is the suffix of a carboxylic acid?

A

-oic acid

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20
Q

what are the prefixes of the first 4 haloalkanes?

A

fluoro-
chloro-
bromo-
iodo-

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21
Q

what is the suffix of ketones?

A

-one

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22
Q

define haloalkane

A

an alkane with a halogen attached to it

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23
Q

define structural isomer

A

compounds with the same molecular formulae but different structural formulae

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24
Q

what is the shape of an alkane molecule?

A

tetrahedral - 109.5 degrees

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25
what kind of bonds are there in alkanes? define this term
sigma bonds - the overlap of orbitals between two atoms
26
in alkanes, what happens to boiling point as chain length increases? why?
as chain length increases boiling point increases - because there are more carbons - so more electrons - so stronger induced dipole-dipole interactions - more energy to break bonds.
27
in alkanes, what happens to boiling point after chains become very long?
boiling point levels off because the percentage increase of electrons become insignificant so the boiling doesn't increase by that much.
28
how does a branched isomer effect the boiling point of an alkane?
branched isomers have lower boiling points - because straight chains have more surface contact - which means more induced dipole interactions. branched isomers can't get as close together so they have less interactions.
29
state the word equation for the complete combustion of an alkane
alkane + oxygen --> carbon dioxide + water
30
state the word equation for the incomplete combustion of an alkane
alkane + oxygen --> carbon monoxide + carbon dioxide + water
31
define heterolytic fission
the breaking of a covalent bond in which one of the bonded elements receives all of the bond pair electrons, resulting in a positive an negative ion
32
define homolytic fission
the breaking of a covalent bond in which each of the previously bonded atoms are given one electron each, resulting in two radicals
33
define a radical
a species with an unpaired electron (that is highly reactive)
34
what are the 3 steps of homolytic free radical substitution? describe them in terms of radicals present
initiation - in which 2 free radicals are formed propagation - no. of radical doesn't change. the reaction continues due to the continuous formation of radicals termination - free radicals are consumed and react together
35
example of homolytic free radical substitution: making chloromethane from methane and chlorine. 1. what is the balanced symbol equation?
CH₄ + Cl➝ HCl + CHCl
36
example of homolytic free radical substitution: making chloromethane from methane and chlorine. 2. what happens in the initiation step? what is needed for this step? give the equation for it
initiation: UV light is needed to break the chlorine bond to create two chlorine radicals. Cl₂ ➝ Cl• + Cl•
37
example of homolytic free radical substitution: making chloromethane from methane and chlorine. 3. what happens in the propagation step? give the equations for it
propagation: radicals are used then regenerated, creating a chain reaction. Cl• + CH₄ ➝ CH₃• + HCl Cl₂ + CH₃• ➝ CH₃Cl + Cl•
38
example of homolytic free radical substitution: making chloromethane from methane and chlorine. 4. what happens in the termination step? write 3 equations of how the reaction could come to this
termination: reaction stops because the radicals react together, removing themselves Cl• + Cl• ➝ Cl₂ Cl• + CH₃• ➝ CH₃Cl CH₃• + CH₃• ➝ C₂H₆
39
what shape do alkenes have? what bond angle? why?
trigonal planar - 120 degrees | because the sigma and pi bonds repel by equal amounts so create angles of 120 degrees (I think..?)
40
define sigma bond
overlap of orbitals between 2 atoms
41
define pi bond
overlap of p-orbitals above and below atoms -creates double bond in alkenes
42
what is an addition reaction?
when something is added to a species, creating only ONE product
43
alkene + hydrogen =? what is needed for the reaction?
alkane - nickel catalyst
44
alkene + water =? what is needed for the reaction?
alcohol - water must be steam and a phosphoric acid catalyst
45
define electrophile
something that accepts electrons
46
outline the three main steps of electrophilic addition of alkenes
1. C=C electrons are accepted by electrophile and one bond is created 2. a carbocation is formed and the lone electrons from the left over electrophile attract to it (intermediate) 3. saturated substance is formed.
47
electrophilic addition: what three typed of carbocations can be formed? which is more stable?
primary: carbocation only bonded to ONE other carbon secondary: carbocation bonded to TWO other carbons tertiary: carbocation bonded to THREE other carbons TERTIARY is more stable
48
electrophilic addition: how is the major product decided?
the most stable = the major product
49
define stereoisomerism
compounds with the same structural formula but different arrangement in space
50
what must an alkene have for there to be stereoisomerism?
each carbon in the C=C must have two distinct groups bonded EACH if one carbon has two of the same group, there is no stereoisomerism
51
why can alkenes have stereoisomerism?
because the double bond restricts rotation
52
name two methods of identifying stereoisomers
cis-trans | E-Z
53
when would you use cis-trans methods?
when each of the two groups in question that are bonded to each carbon are the same
54
what would a cis alkene look like?
two groups on the SAME side of the C=C
55
what would a trans alkene look like?
two groups on OPPOSITE sides of the C=C
56
how do you decide whether an alkene is E or Z?
split the alkene in half decide which is the high priority group see whether they are on the same side or opposite sides.
57
what is considered a high priority group?
groups with the highest Mr
58
what would an E alkene look like?
two highest priority groups are on opposite sides E for Enemies
59
what would a Z alkene look like?
two highest priority groups on the same side Z for Zee Zame Zide
60
define polymerisation
monomers reacting together to make a polymer - repeated chain
61
how are monomers and polymers drawn in a polymerisation equation?
both with brackets with an 'n' outside representing number of units polymer has extra bonds continued out the brackets
62
why can't addition polymers be broken down in the environment?
because they are: - saturated - very stable so bonds aren't broken easily
63
suggest 6 ways of disposing of polymers
``` organic feedstock biodegradable combustion landfill photodegradable recycling ```
64
name 2 positives and 1 negative of using combustion to dispose of polymers
positives: 1. produces heat which can generate electricity 2. greenhouse gases (below) can be avoided using alkali scrubbers negative: 1. CO2 is produced = greenhouse gas, and HCl gas is produced from burning Cl based compounds
65
how do you make a polymer biodegradable?
mixing plant based polymers with regular polymers to help them break down in the earth
66
what is photodegradable?
something that can be broken down by light | bonds are weakened by the absorption of light
67
how do you make a polymer photodegradable?
mixing photodegradable substances into the regular polymers
68
what is one problem with photodegradable polymers?
photodegradable polymers in landfill may not receive enough sunlight if they are buried in rubbish = not break down

Chemistry A-Level (13 decks)

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