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A level- Chemistry > Organic definitions > Flashcards

Organic definitions Flashcards

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1
Q

Define addition polymerisation

A

Formation of a very long molecular chain, by repeated addition reactions of many unsaturated alkene molecules

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2
Q

Define addition reaction

A

A reaction in which a reactant is added to an unsaturated molecule to make one saturated molecule

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3
Q

Define alicyclic

A

Containing carbon atoms joined together in a non aromatic ring

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4
Q

Define actual yield

A

The amount of product obtained in a reaction

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5
Q

Define aliphatic

A

Containing carbon atoms joined together in straight or branched chains

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6
Q

Define alkanes

A

The hydrocarbon homologous series with single carbon-carbon bonds only and the general formula CnH2n+2

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7
Q

Define acid

A

A species that releases H+ ions in aqueous solution

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8
Q

Define alkali

A

A type of base that dissolves in water forming hydroxide ions OH- (aq)

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9
Q

Define alkenes

A

The hydrocarbon homologous series with at least one double carbon-carbon bond and the general formula CnH2n

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10
Q

Define alkynes

A

The hydrocarbon homologous series with one triple carbon-carbon bond and the general formula CnH2n-2

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11
Q

Define amount of substance

A

The quantity whose unit of the mole, used as a means of counting any species such as atoms, ions and molecules

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12
Q

Define anhydrous

A

Containing no water molecules

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13
Q

Define anion

A

A negatively charged ion with more electrons than protons

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14
Q

Define aromatic

A

Containing one or more benzene rings

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15
Q

Define atom economy

A

Atom economy= (Sum of molar masses of desired products)/ (Sum of molar masses of all products) *100

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16
Q

Define atomic number

A

The number of protons in the nucleus of an atom

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17
Q

Define atomic orbital

A

A region around the nucleus that can hold up to two electrons with opposite spins

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18
Q

Define Avogadro constant

A

The number of atoms per mole of the carbon-12 isotope

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19
Q

Define base

A

Bases are protons acceptors, they neutralise an acid to form a salt

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20
Q

Define a binary compound

A

A compound containing two elements only

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21
Q

Define bonded pair

A

A pair of electrons shared between two atoms to make a covalent bond

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22
Q

Define carbocation

A

An ion that contains a positively charged carbon atom.

An intermediate in electrophilic addition

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23
Q

Define cation

A

A postively charged ion with fewer electrons than protons

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24
Q

Define chain reaction

A

A reaction in which the propagation steps release new radicals that continue the reaction

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25
Q

Define chemical shift

A

A scale, in ppm, that compares the frequency of an NMR absorption with the frequency of the reference TMS

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26
Q

Define chiral carbon

A

A carbon atom attached to four different atoms or groups of atoms

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27
Q

Define chromatogram

A

A visible record showing the result of separation of the components of a mixture by chromatography

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28
Q

Define Cis-trans isomerism

A

A special case of E/Z isomerism in which 1 of the two groups attained to each carbon of the double bond is the same.
If the same group on the same side of double bond-cis
otherwise-trans

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29
Q

Define concentration

A

The amount of solute, in moles, dissolved in 1dm3 of solution

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30
Q

Define condensation reaction

A

A reaction in which two small molecules react together to form a larger molecule with elimination of a small molecule such as water

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31
Q

Define coordinate bond

A

A shared pair of electrons in which the bonded pair has been provided by one of the bonding atoms only, also called a dative covalent bond

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32
Q

Define covalent bond

A

The strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms

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33
Q

Define dative covalent

A

A shared pair of electrons in which the bonded pair has been provided by one of the bonding atoms only, also called a coordinate bond

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34
Q

Define dehydration

A

An elimination reaction in which water is removed from a saturated molecule to make an unsaturated one

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35
Q

Define delocalised electrons

A

Electrons that are shared between more than two atoms

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36
Q

Define dipole

A

A separation in electrical charge so that one atom of a polar covalent bond, or one end of a polar molecule has a small positive charge and the other has a small negative charge

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37
Q

Define displayed formula

A

A formula showing the relative positioning of all the atoms in a molecule and the bonds between them

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38
Q

Define disproportionation

A

A redox reaction in which the same element is both oxidised and reduced

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39
Q

Define E/Z isomerism

A

A type of stereoisomerism in which different groups attached to each carbon of a C=C double bond may be arranged differently in space because of the restricted rotation of the C=C bond

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40
Q

Define electronegativity

A

A measure of the attraction of a bonded atom for the pair of shared electrons in a covalent bond

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41
Q

Define electrophile

A

An atom or group of atoms which is attracted to an electron-rich centre or atom, where it accepts a pair of electrons to form a new covalent bond

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42
Q

Define electrophilic addition

A

An addition reaction in which the first step is attack by an electrophile on a region of high electron density

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43
Q

Define elimination reaction

A

The removal of a molecule from a saturated molecule to make an unsaturated molecule

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44
Q

Define enantiomers

A

Stereoisomers that are non-superimposable mirror images of each other; also called optical isomers

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45
Q

Define esterification

A

A reaction in which a carboxylic acid reacts with an alcohol to form an ester and water

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46
Q

Define fingerprint region

A

An area of infrared spectrum below 1500cm-1 that gives a characteristic pattern for different compounds.
Very difficult to interpret

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47
Q

Define fragment ions

A

Ions formed from the breakdown of the molecular ion in a mass spectrometer

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48
Q

Define fragmentation

A

The process in mass spectrometry that causes a positive ion to split into smaller pieces, one of which is a positive fragment ion

49
Q

Define functional group

A

The part of an organic molecule responsible for its chemical reaction

50
Q

Define general formula

A

The simplest algebraic formula of a member of a homologous series

51
Q

Define giant covalent lattice

A

A 3d structure of atoms, bonded together by strong covalent bonds

52
Q

Define giant ionic lattice

A

A 3d structure of oppositely charged ions bonded together by strong ionic bonds

53
Q

Define giant metallic lattice

A

A 3d structure of of positive ions bonded together by strong metallic bonds

54
Q

Define heterolytic fission

A

The breaking of a covalent bond forming a cation and an anion. All the shared electrons go to the same atom

55
Q

Define homologous series

A

A series of organic compounds with the same functional group but with each successive member differing by CH2

56
Q

Define homolytic fission

A

The breaking of a covalent bond with one of the bonded electrons going to each atom, forming two radicals

57
Q

Define hydrated

A

A crystalline compound containing water molecules

58
Q

Define hydrocarbon

A

A compound of hydrogen and carbon only

59
Q

Define hydrogen bond

A

A strong dipole-dipole attraction between an electron-deficient hydrogen atom of -NH, -OH, -HF on one molecule and a lone pair of electrons on a highly electronegative atom containing N,O or F on a different molecule.

60
Q

Define hydrolysis

A

A reaction with water that breaks a chemical compound into two compounds, the H and OH in a water molecule becomes incorporated into the two compounds

61
Q

Define induced dipole-dipole interaction

A

Attractive forces between induced dipoles in different molecules- London forces

62
Q

Define infrared spectroscopy

A

An instrumentation method of analysis that identifies bonds from absorption of the infrared radiation of different wavelengths

63
Q

Define intermediate

A

A species formed during a reaction that reacts further and is not present in the final products

64
Q

Define intermolecular force

A

An attractive force between molecules. Intermolecular forces can be London forces, permanent dipole-dipole interactions or hydrogen bonding

65
Q

Define ionic bonding

A

The electrostatic attraction between positive and negative ions

66
Q

Define isotopes

A

Atoms of the same element with different numbers of neutrons and different masses but the same number of protons.

67
Q

Define limiting reagent

A

The reactant that is not in excess, which will be used up first and stop the reaction

68
Q

Define lone pair

A

An outer shell pair of electrons that is not involved in chemical bonding

69
Q

Define metallic bond

A

The electrostatic attraction between positive metal ions and delocalised electrons

70
Q

Define mobile phase

A

The phase that moves in chromatography

71
Q

Define molar gas volume

A

The volume per mole of gas molecules at a stated temperature and pressure

72
Q

Define molar mass

A

The mass per mole of a substance in units g mol-1

73
Q

Define mole

A

The amount of any substance containing as many elementary particles as there are carbon atoms in exactly 12g of the carbon-12 isotope that is, 6.02*10^23 particles

74
Q

Define molecular ion

A

The positive ion formed in mass spectrometry when a molecule loses an electron

75
Q

Define monomer

A

A small molecule that combines with many other monomers to form a polymer

76
Q

Define neutralisation

A

A chemical reaction in which an acid and a base react together to produce a salt

77
Q

Define nucleophile

A

An atom (or group of atoms) which is attracted to an electron deficient centre or atom, where it donates a pair of electrons in form a new covalent bond

78
Q

Define nucleophilic substitution

A

A reaction in which a nucleophile is attracted to an electron deficient carbon atom and replaces an atom or group of atoms on the carbon atom

79
Q

Define optical isomers

A

Stereoisomers that are non-superimposable mirror images of each other; also called enantiomers

80
Q

Define oxidation

A

Loss of electrons or an increase in oxidation number

81
Q

Define oxidation number

A

A measure of the number of electrons that an atom uses to bond with atoms of another element.

82
Q

Define oxidising agent

A

A reagent that oxidises another species

83
Q

Define pi-bond

A

A bond formed by the sideways overlap of two p-orbitals, with the electron density above and below the plane of the bonding atoms

84
Q

Define percentage yield

A

percentage yield= (amount in mol, of a product)/ (theoretical amount, in mol, of product) *100

85
Q

Define permanent dipole

A

A small charge difference that does not change across a bond, with delta postive and delta negative partial charges on the bonded atoms: the result of the bonded atoms having different electronegativities

86
Q

Define permanant dipole-dipole interactions

A

An attractive force between permanent dipoles in neighbouring polar molecules

87
Q

Define polar molecule

A

A molecule that has an overall dipole taking into account all dipoles across bonds and the shape of molecules.

88
Q

Define polymer

A

A large molecule formed from many thousands of repeat units of smaller molecules known as monomers

89
Q

Define radical

A

A species with an unpaired electron

90
Q

Define reaction mechanism

A

The sequence of bond breaking and bond-forming steps that shows the path taken by electrons during a reaction

91
Q

Define reducing agent

A

A reagent that reduces another species

92
Q

Define reduction

A

Gain of electrons of a decrease in oxidation number

93
Q

Define reflux

A

The continual boiling and condensing of a reaction mixture back to the original container to ensure that the reaction takes place without the contents of the flask boiling dry

94
Q

Define relative atomic mass

A

The weighted mean mass of an atom of an element compared with 1/12 of the mass of an atom of carbon-12

95
Q

Define relative formula mass

A

The weighted mean mass of the formula unit of a compound compared with 1/12 of the mass of an atom of carbon-12

96
Q

Define relative isotopic mass

A

The mass of an atom of an isotope compared with 1/12 of the mass of an atom of carbon-12

97
Q

Define relative molecular mass

A

The weighted mean mass of a molecule of a compound compared with 1/12 of the mass of an atom of carbon-12

98
Q

Define retention time

A

In gas chromatography, the time taken for a component to pass from the column inlet to the detector

99
Q

Define repeat unit

A

The specific arrangement of atoms that occurs in the structure over and over again

100
Q

Define Rf value

A

Rf= distance moved by component/ distance moved by solvent

101
Q

Define sigma-bond

A

A bond formed by the end on overlap of one orbital from each bonding atom, consisting of two electrons and with the electron density centred around a line directly between the nuclei of the two atoms.

102
Q

Define salt

A

The product of a reaction in which the H+ ions from the acid are replaced by metal or ammonium ions

103
Q

Define saturated

A

Containing single bonds only

104
Q

Define shell

A

A group of atomic orbitals with the same main energy level

105
Q

Define skeletal formula

A

A simplified organic formula, with hydrogen atoms removed from alkyl chains leaving just a carbon skeleton and associated functional groups

106
Q

Define spin-spin coupling

A

In an NMR spectrum, the interaction between spin states in non-equivalent nuclei result in the splitting of a signal

107
Q

Define standard conditions

A

A pressure of 100 kPa
Temperature 298 K or 25 degrees
Concentration of 1 mol dm-3

108
Q

Define standard solution

A

A solution of known concentration

109
Q

Define stationary phase

A

The phase that does not move in chromatography

110
Q

Define stereoisomers

A

Compounds with the same structural formula but with a different arrangement of the atoms in space

111
Q

Define strong acid

A

An acid that completely dissociated in solution

112
Q

Define structural formula

A

A formula showing the minimal detail for the arrangement of atoms in molecule

113
Q

Define structural isomers

A

Molecules with the same molecular formula but with different structural formula

114
Q

Define sub-shell

A

A group of orbitals of the same type within a shell

115
Q

Define theoretical yield

A

The yield resulting from complete conversion of reactants into products

116
Q

Define unsaturated

A

Containing a multiple carbon-carbon bond

117
Q

Define volatility

A

The ease at which a liquid turns into a gas. Volatility increases as boiling point decreases

118
Q

Define water of crystallisation

A

Water molecules that are bonded into a crystalline structure of a compound

119
Q

Define weak acid

A

An acid that dissociated only partially in solution

A level- Chemistry (31 decks)

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