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chemistry module 4 definitions Flashcards

(75 cards)

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1
Q

aliphatic

A

a hydrocarbon where all carbon and hydrogens are contained in either branched chains, unbranched chains or non-aromatic rings

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2
Q

alicyclic

A

an aliphatic compound arraged in non-aromatic rings

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3
Q

alkyl

A

a group with the general formula CnH2n+1

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4
Q

dipole

A

a partial charge created by differences in electronegativity between two covalently bonded atoms

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5
Q

curly arrow

A

shows the movement of electrons & has to start from

-lone pair
-bond
-negative charge

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6
Q

empirical formula

A

the simplest whole number ratio of each element present in a compound

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7
Q

displayed formula

A

the relative positions of atoms and the bonds between them

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8
Q

general formula

A

the simplest algebraic formula for a member of a homologus series

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9
Q

homologus series

A

a series of organic compounds containing the same functional group with each member successive by ch2

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10
Q

heterolytic fission

A

when a covalent bond breaks, one bonding pair of electrons receives both electrons from the bonded pair

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11
Q

homolytic fission

A

when a covalent bond breaks, each bonding pair of electrons receives one electron from the bonded pair

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12
Q

nomenclature

A

the naming system for compounds

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13
Q

radical

A

species with an unpaired electron

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14
Q

reaction mechanism

A

a series of steps that represent the reaction by showing the breaking and forming of bonds using curly arrows

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15
Q

structural isomers

A

same molecular formula but different structural formula

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16
Q

structural formula

A

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

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17
Q

bond enthalpy

A

the energy required to break down 1 mol of gaseous atoms

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18
Q

london forces

A

induced dipole-dipole forces that caused by the random movement of electrons

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19
Q

polar bond

A

when a large disparity in electronegativity makes it so that the bonded pair of electrons are held closer to the more electronegative element. there is a permanent dipole

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20
Q

initiation

A

first step in free radical substitution mechanism where free radicals are created from UV

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21
Q

termination

A

last step in free radical substitution wherein 2 radicals react to create a species with only paired electrons

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22
Q

propagation

A

intermediate step in free radical sub in which the free radical reacts with another species

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23
Q

sigma bond

A

single bond, formed by the overlapping of the s-orbitals head-on and these can rotate freely

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24
Q

pi bond

A

a type of covalent bond formed where adjacent p orbitals overlap sideways above and below the bond
ing atoms

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25
addition reaction
a reaction where molecules combine to form a single product
26
addition polymerisation
the formation of long chain molecules when many monomers join together
27
bond enthalpy
the energy required to break one mole of gaseous bonds. Actual bond enthalpies may differ from the average as the average bond enthalpy considers a particular bond in a range of molecules.
28
e isomer
when highest priority groups are on the opposite sides of the double bond (entengen)
29
z isomer
when the highest priority group is on the same end of the double bond
30
catalyst
speed up rate of reaction without being used up
31
cis isomer
highest priority groups on the same side of the double bond
32
trans isomer
highest priority group on opposite sides of the double bond
33
covalent bond
strong bond formed by the strong electrostatic attraction between the shared pair of electrons and the positive nuclei
34
markovnikov's rule
the halogen attaches to the carbon that is attached to more carbons
35
photodegradeable
can be broken down by light
36
primary carbocation
a molecule where the positive carbon is only attached to one alkyl group
37
secondary carbocation
a molecule where the positive carbon is attached to two alkyl groups
38
tertiary carbocation
a molecule where the positive carbon is attached to three alkyl groups. most stable
39
stereiosomer
same strctural and molecular formula but have a different arrangement of atoms in space
40
primary alcohol
an alcohol in which the OH is attached to a primary carbon atom (i.e. RCH2OH). Primary alcohols can be oxidised to form either an aldehyde or a carboxylic acid, depending on the conditions.
41
secondary alcohol
an alcohol in which the OH is attached to a secondary carbon atom. secondary alcohols can be oxidised to form a ketone under reflux
42
tertiary alcohol
an alcohol in which the OH is attached to a tertiary carbon atom (i.e. R3COH). Tertiary alcohols cannot be oxidised.
43
bond enthalpy
the energy required to break one mole of gaseous bonds. The bond enthalpy of the carbon halogen bond in haloalkanes decreases from C-F to C-I.
44
CFCs
a class of compound made up of carbon, fluorine and chlorine, used as refrigerants and aerosol propellants. CFCs can be broken down by UV light in the upper atmosphere to form chlorine radicals which catalyse the breakdown of ozone. in air cons and bad for environment
45
hydrolysis
the breakdown of a compound as a result of a reaction with water. The rate of haloalkane hydrolysis for different carbon-halogen bonds can be determined via a reaction with water in the presence of AgNO3 and ethanol
46
nucelophilic substitution
a reaction in which an electron pair donor attacks an electrophilic atom (an atom with a partial or full positive charge) to replace an atom / group of atoms.
47
electrophile
electron pair acceptor
47
nucleophile
electron pair donor
48
ozone
a molecule with the formula O3 , which absorbs UV light in the atmosphere. The breakdown of ozone can be catalysed by chlorine radicals as well as other radicals such as *NO.
49
breakdown and reform of ozone in the stratosphere naturally equ
BREAKDOWN O=O ----> 2 O (FREE RADICALS) and UV above the arrow --------------------------------------- REFORM O(FR)+O2 ---> O£
50
breakdown and reform of ozone in the stratosphere naturally def
ozone breaks down into oxygen free radicals but then that reacts with the oxygen in the stratosphere in order to reform back into O3 or ozone and in doing this it absorbs UV radiation. therefore conc of ozone and oxygen in the stratosphere should remain roughly constant
51
what do cfcs do to make it worse
cfcs= chlorofluorocarbons and these are haloalkanes -relatively stable due to high bond enthalpy of halogen to carbon bonds -relatively non toxic -however the travel up into the stratosphere and causes a carbon to chlorine bond to break as it reacts with the UV THIS IS CALLED PHOTODISSOSCIATION
52
steps in cfcs working: initiation
CFCL3 --->CFCL2' +CL' ('= free radical)
53
steps in cfcs working: propagation step 1
CL'+ O3 ----> CLO' +O2 CLO' which is chlorine monoxide is a highly reactive free radical
54
steps in cfcs working: propagation step 2
CLO'+O -----> CL' + O2 this means that the chlorine radical seen in p1 can go on back and destroy many ozone molecules as it's essentially a catalyst
55
what else can ozone be destroyed by
nitrogen oxide radicals that come from lightning and from aircraft
56
propagation step 1 NO fr
NO' + O3 ----> NO2' + O2
57
propagation step 2 NO fr
NO2' + O ----> NO' +O2 NO free radical reproduced so reaction can continue on
58
anhydrous salt
a salt such as MgSO4 or CaCl2 which is used to remove traces of water from an organic solution.
59
distillation
a technique in which a liquid is heated then the vapour is cooled and collected in a separate flask to the reaction mixture. During distillation, the condenser must be positioned horizontally.
60
QuickFit apparatus
glassware that easily fits together in a variety of arrangements
61
redistillation
a technique used to purify an organic liquid using multiple distillations
62
reflux
the continual boiling and condensing of a reaction mixture. This is to ensure that the reaction goes to completion. During reflux, the condenser must be positioned vertically
63
separating funnel
a piece of apparatus that is used to purify an organic liquid by removing the organic layer from an aqueous layer
64
synthetic route
a series of steps that are followed to make a specific compound
65
elemental analysis
a sample is analysed to determine the proportion of elements that make up the compound present. This is done by converting a known amount of an unknown sample into simple known compounds
66
fragmentation
during mass spectrometry, unstable molecular ions break down into smaller fragments
67
fragment ions
smaller ions formed when an unstable molecular ion breaks down during mass spectrometry
68
infrared radiation
a type of electromagnetic radiation that is absorbed by covalent bonds, causing them to vibrate at a specific frequency
69
infrared spectroscopy
a technique used to identify particular bonds and functional groups within a molecule. This technique has been used to link global warming with increased energy usage as atmospheric gases containing C=O, O-H and C-H bonds (such as CO2 , H2O and CH4 ) show distinct peaks on IR spectra. IR spectroscopy is used to monitor gases causing air pollution (CO and NO from car emissions) and to measure alcohol in the breath in modern breathalysers
70
M+1 Peak
a small peak on a mass spectrum caused by the presence of a small proportion of carbon-13.
71
m/z ratio
the mass to charge ratio on a mass spectrum. This is equivalent to the mass of an ion
72
mass spectroscopy
a technique used to identify compounds and determine relative molecular mass
73
molecular ion peak
the peak on a mass spectrum with the highest m/z value, used to determine molecular mass of a compound
74
molecular mass
the total number of atoms of each element in the compound

chem (7 decks)

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