Key Definitions Flashcards
1
Q
Acid
A
A proton donor
2
Q
Activation energy
A
The minimum energy required to start a reaction by the breaking of bonds
3
Q
Addition polymer
A
A very long molecular chain, formed by repeated additional reactions of many unsaturated alkene molecules (monomers).
4
Q
Addition polymerisation
A
The process in which unsaturated alkene molecules (monomers) add on to a growing polymer chain one at a time to form a very long saturated molecular chain (the addition polymer).
5
Q
Addition reaction
A
A reaction in which a reactant is added to an unsaturated molecule to make a saturated molecule
6
Q
Absorbtion
A
The process that occurs when a gas, liquid or solute is held to the surface of a solid or, more rarely, a liquid.
7
Q
Alicyclic hydrocarbon
A
A hydrocarbon with carbon atoms joined together in a ring like structure
8
Q
Aliphatic hydrocarbon
A
A hydrocarbon with carbon atoms joined together in straight or branched chains
9
Q
Alkali
A
A type of base that dissolves in water forming hydroxide ions, OH-(aq) ions.
10
Q
Alkanes
A
The homologous series with the general formula: CnH2n+2
11
Q
Alkyl group
A
An alkane with a hydrogen atom removed, e.g. CH3, C2H5
12
Q
Amount of substance
A
The quantity whose unit is the mole. Chemists use ‘amount of substance’ as a means of counting atoms.
13
Q
Anhydrous
A
A substance containing no water molecules
14
Q
Anion
A
A negatively charged ion
15
Q
Atom economy
A
molecular mass of the desired product
= ————————————————————- X100
sum of molecular masses of all products
16
Q
Atomic orbital
A
A region within an atom that can hold up to two electrons, with opposite spins
17
Q
Atomic (proton) number
A
The number of protons in the nucleus of an atom
18
Q
Average bond enthalpy
A
The average enthalpy change that takes place when breaking by homolytic fission 1 mol of a given type of bond in the molecules of a gaseous species
19
Q
Avogadro constant, Na
A
The number of atoms per mole of the carbon-12 isotope (6.02 x 10(23) mol -1
20
Q
Base
A
A proton acceptor
21
Q
Biodegradable material
A
A substance that is broken down naturally in the environment by living organisms
22
Q
Boltzmann distribution
A
The distribution of energies of molecules at a particular temperature, usually shown as a graph
23
Q
Bond enthalpy
A
The enthalpy change that takes place when breaking by homolytic fission 1 mol of a given bond in the molecules of a gaseous species
24
Q
Carbanion
A
An organic ion in which a carbon atom has a negative charge
25
Carbocation
An organic ion in which a carbon atom has a positive charge
26
Catalyst
A substance that increases the rate of a chemical reaction without being used up in the process
27
Cation
A positively charged ion
28
cis-trans isomerism
A special type of E/Z isomerism in which there is a non-hydrogen group and hydrogen on each C of a C=C double bond: the cis isomer (Z isomer) has the H atoms on each carbon on the same side; the trans isomer (E isomer) has the H atoms on each carbon on different sides.
29
Compound
A substance formed from two or more chemically bonded elements in a fixed ratio, usually shown by a chemical formula
30
Concentration
The amount of solute, in mol, per 1dm3 (1000cm3) of solution
31
Coordinate bond
A shared pair of electrons which has been provided by one of the bonding atoms only; also called a dative covalent bond
32
Covalent bond
A bond formed by a shared pair of electrons
33
Cracking
The breaking down of a long-chained saturated hydrocarbons to form a mixture of shorter-chained alkanes and alkenes
34
Curly arrow
A symbol used in reaction mechanisms to show the movement of an electron pair in the breaking or formation of a covalent bond
35
Dative covalent bond
A shared pair of electrons which has been provided by one of the bonding atoms only; also called a coordinate bond
36
Dehydration
An elimination reaction in which water is removed from a saturated molecule to make an unsaturated molecule
37
Delocalised electrons
Electrons that are shared between more than two atoms
38
Displacement reaction
A reaction in which a more reactive element displaces a less reactive element from an aqueous solution of the latter's ions
39
Displayed formula
A formula showing the relative positioning of all the atoms in a molecule and the bonds between them
40
Disproportionation
The oxidation and reduction of the same element in a redox reaction
41
Dynamic equilibrium
The equilibrium that exists in a closed system when the rate of the forward reaction is equal to the rate of the reverse reaction
42
E/Z isomerism
A type of stereo-isomerism in which different groups attached to each carbon of a C=C double bond may be arranged different in space because of the restricted rotation of the C=C bond
43
Electron configuration
The arrangement of electrons in an atom
44
Electronegativity
A measure of the attraction of a bonded atom for the pair of electrons in a covalent bond
45
Electron sheilding
The repulsion between electrons in different inner shells. Shielding reduces the net attractive force from the positive nucleus of the outer-shell electrons
46
Electrophile
An atom (or group of atoms) that is attracted to an electron-rich centre or atoms, where it accepts a pair of electrons to form a new covalent bond
47
Electrophilic addition
A type of addition reaction in which an electrophile is attracted to an electron-rich centre or atom, where it accepts a pair of electrons to form a new covalent bond
48
Elimination reaction
The removal of a molecule from a saturated molecule to make an unsaturated molecule
49
Empirical formula
The simplest whole-number ratio of atoms of each element present in a compound
50
Endothermic reaction
A reaction in which the enthalpy of the products is grater than the enthalpy of the reactants, resulting in heat being taken from the surroundings. (deltaH +ve)
51
Enthalpy, H
The hear content that is stored in a chemical system
52
Standard enthalpy change of combustion
The enthalpy change that takes place when one mole of a substance reacts completely with oxygen under standard conditions, all reactants and products being in their standard states
53
Standard enthalpy change of formation
The enthalpy change that takes place when one mole of a compound in its standard state is formed from its constituent elements in their standard states under standard conditions
54
Standard enthalpy change of reaction
The enthalpy change that accompanies a reaction in the molar quantities expressed in a chemical equation under standard conditions, all reactants and products in their standard states
55
Enthalpy cycle
A diagram showing alternative routes between reactants and products that allows the indirect determination of an enthalpy change from other known enthalpy changes using Hess' law.
56
Enthalpy profile diagram
A diagram for a reaction to compare the enthalpy of the reactants with the enthalpy of the products
57
Esterification
The reaction of an alcohol with a carboxylic acid to produce an ester and water
58
Exothermic reaction
A reaction in which the enthalpy of the products is smaller than the enthalpy of the reactants, resulting in heat loss to the surroundings (deltaH -ve)
59
Fractional distillation
The separation of the components in a liquid mixture into fraction which differ in boiling point (and hence chemical composition) by means of distillation, typically using a fractionating column.
60
Fragmentation
The process in mass spectrometry that causes a positive ion to split into pieces, one of which is a positive fragment ion
61
Functional group
The part of the organic molecule responsible for its chemical reactions.
62
General formula
The simplest algebraic formula of a member of a homologous series. For example, the general formula of the alkanes is CnH2n+2
63
Giant covalent lattice
A three-dimensional structure of atoms, bonded together by strong covalent bonds.
64
Giant ionic lattice
A three-dimensional structure of oppositely charged ions, bonded together by strong ionic bonds.
65
Giant metallic lattice
A three-dimensional structure of positive ions and delocalised electrons, bonded together by strong metallic bonds.
66
Greenhouse effect
The process in which the absorption and subsequent emission of infra-red radiation by atmospheric gases warms the lower atmosphere and the planet's surface
67
Group
A vertical column in the Periodic Table. Elements in a group have similar chemical properties and their atoms have the same number of outer-shell electrons
68
Hess' law
If a reaction can take place by more than one route and the initial and final conditions are the same, the total enthalpy change is the same for each route
69
Heterogeneous catalysis
A reaction in which the catalyst has a different physical state from the reactants; frequently, reactants are gases whilst the catalyst is a solid
70
Heterolytic fission
The breaking of a covalent bond with both of the bonded electrons going to one fo the atoms, forming a cation (+ ion) and an anion (- ion).
71
Homogeneous catalysis
A reaction in which the catalyst and the reactants are in the same physical state, which is most frequently the aqueous or gaseous state
72
Homologous series
A series of organic compounds with the same functional group, but with each successive member differing by CH2
73
Homolytic fission
The breaking of a covalent bond with one of the bonded electrons going to each atom, forming two radicals
74
Hydrated
Crystalline and containing water molecules
75
Hydrocarbon
An organic compound of hydrogen and carbon only
76
Hydrogen bond
A strong dipole-dipole attraction between an electron-deficiant hydrogen atom (O-H[sightly]+ or N-H[slightly]+) on one molecule and a lone pair of electrons on a highly electronegative atom (H-O:[slightly]- or H-N:[slightly]- ) on a different molecule.
77
Hydrolysis
A reaction with water or aqueous hydroxide ions that breaks a chemical compound into two compounds
78
Initiation
The first step in a radical substitution in which the free radicals are generated by ultraviolet radiation
79
Intermolecular force
An attractive force between neighbouring molecules. Intermolecular forces can be van der Waals' forces (induced dipole-dipole forces), permanent dipole-dipole forces or hydrogen bonds.
80
Ion
A positively or negatively charged atom or (covalently bonded) group of atoms (a molecular ion).
81
Ionic bond
The electrostatic attraction between oppositely charged ions.
82
(first) ionisation energy
The energy required to remove one electron from each atom in one molecule of gaseous atoms to form one mole of gaseous 1+ ions.
83
(second) ionisation energy
The energy required to remove one electron from each ion in one mole of gaseous 1+ ions to form one mole of gaseous 2+ ions
84
(successive) ionisation energy
A measure of the energy required to remove each electron in turn, e.g. the second ionisation energy is the energy required to remove one electron from each ion in one mole of gaseous 1+ ions to form one mole of gaseous 2+ ions
85
Isotopes
Atoms of the same element with different number of neutrons and different masses
86
le Chatelier's principle
When a system in dynamic equilibrium is subjected to a change, the position of equilibrium will shift to minimise the change
87
Limiting reagent
The substance in a chemical reaction the runs out first
88
Lone pair
An outer shell pair of electrons that is not involved in chemical bonding
89
Mass (nucleon) number
The number of particles (protons and neutrons) in the nucleus
90
Mechanism
A sequence of steps showing the path taken by electrons in a reaction
91
Metallic bond
The electrostatic attraction between positive metal ions and delocalised electrons
92
Molar mass, M
The mass per mole of a substance. The units of molar mass are g mol-1
93
Molar volume
The volume per mole of a gas. The units of molar volume are dm3 mol-1. At room temperature and pressure the molar volume is approximately 24.0 dm3mol-1
94
Mole
The amount of any substance containing as many particles as there are carbon atoms in exactly 12g of the carbon-12 isotope
95
Molecular formula
The number of atoms of each element in a molecule
96
Molecular ion, M+
The positive ion formed in mass spectrometry when a molecule loses an electron
97
Molecule
A small group of atoms help together by covalent bonds
98
Monomer
A small molecule that combines with many other monomers to form a polymer
99
Nomenclature
A system of naming compounds
100
Nucleophile
An atom (or group of atoms) that is attracted to an electron-deficient centre or atom, where it donates a pair of electrons to form a new covalent bond
101
Nucleophilic substitution
A type of substitution reaction in which a nucleophile is attracted to an electron-deficient centre or atom, where it donates a pair of electrons to form a new covalent bond
102
Oxidation
Loss of electrons or an increase in oxidation number
103
Oxidation number
A measure of the number of electrons that an atom uses to bond with atoms of another element. Oxidation numbers are derived from a set of rules
104
Oxidising agent
A reagent that oxidises (takes electrons from) another species
105
Percentage yield
actual amount, in mol, of product
= ------------------------------------------------------------ x100
Theoretical amount, in mol, of product
106
Period
A horizontal row of elements in the periodic table. Elements show trends in properties across a period
107
Periodicity
A regular periodic variation of properties of elements with atomic number and position in the periodic table
108
Permanent dipole
A small charge difference across a bond resulting from a difference in electronegativities of the bonded atoms
109
Permanent dipole-dipole force
An attractive force between permanent dipoles in neighbouring polar molecules
110
pi-bond
The reactive part of a double bond formed above and below the plane of the bonded atoms by sideways overlap of p-orbitals
111
Polar covalent bond
A bond with a permanent dipole
112
Polar molecule
A molecule with an overall dipole, taking into account any dipoles across bonds
113
Polymer
A long molecular chain built up from monomer units
114
Precipitation reaction
The formation of a solid from a solution during a chemical reaction. Precipitates are often formed when two aqueous solutions are mixed together
115
Principal quantum number, n
A number representing the relative overall energy of each orbital, which increases with distance from the nucelus. The sets of orbitals with the same n value are referred to as electron shells or energy levels
116
Propagation
The two repeated steps in radical substitution what build up the products in a chain reaction
117
Radical
A species with an unpaired electron
118
Radical substitution
A type of substitution reaction in which a radical replaces a different atom or group of atoms
119
Rate of reaction
The change in concentration of a reactant or a product in a given time
120
Redox reaction
A reaction in which both reduction and oxidation take place
121
Reducing agent
A reagent that reduces (add electrons to) another species
122
Reduction
Gain of electrons of a decrease in oxidation number
123
Reflux
The continual boiling and condensing of a reaction mixture to ensure that the reaction takes place without the contents of the flask boiling dry
124
Relative atomic mass, Ar
The weighted mean mass of an atom in an element compared with one-twelfth of the mass of an atom of carbon-12
125
Relative formula mass
The weighted mean mass of a formula unit compared with one-twelfth of the mass of an atom of carbon-12
126
Relative isotopic mass
The mass of an atom of an isotope compared with one-twelfth of the mass of an atom of carbon-12
127
Relative molecular mass, Mr
The weighted mean mass of a molecule compared with one-twelfth of the mass of an atom of carbon-12
128
Repeat unit
A specific arrangement of atoms that occurs in the structure over and over again. Repeat units are included in brackets, outside of which is the symbol, n.
129
Salt
A chemical compound formed from an acid, when a H+ ion from the acid has been replaced by a metal ion or another positive ion, such as the ammonium ion, NH4+
130
Saturated hydrocarbon
A hydrocarbon with single bonds only and have the maximum number of hydrogen atoms bonded to it. CnH2n+2
131
Shell
A group of atomic orbitals with the same principal quantum number, n. Also known as a main energy level
132
Simple molecular lattice
A three-dimensional structure of molecules, bonded together by weak intermolecular forces
133
Skeletal formula
A simplified organic formula, with hydrogen atoms removed from alkyl chains, leaving just a carbon skeleton and associated functional groups.
134
Species
Any type of particle that takes part in a chemical reaction
135
Specific heat capacity
The energy required to raise the temperature of 1g of a substance by 1 degree C
136
Spectator ions
Ions that are present but take no part in a chemical reaction
137
Standard conditions
A pressure of 100kPa (1 atomsphere), a stated temperature, usually 298 K (25 degrees C), and a concentration of 1 mol dm-3 (for reaction with aqueous solutions).
138
Standard solution
A solution of known concentration. Standard solutions are normally used in titrations to determine unknown information about another substance.
139
Standard state
The physical state of a substance under the standard conditions of 100kPa (1 atmosphere) and 298 K (25 degrees C).
140
Stereoisomers
Compounds with the same structural formula but with a different arrangement of the atoms in space
141
Stoichiometry
The molar relationship between the relative quantities of substances taking part in a reaction
142
Stratosphere
The second layer of the Earth's atmosphere, containing the 'ozone layer', about 10 km to 50 km above the Earth's surface
143
Structural formula
A formula showing the minimal detail for the arrangement of atoms in a molecule
144
Structural isomers
Molecules with the same molecular formula but with different structural arrangements of atoms
145
Sub-shell
A group of the same type of atomic orbitals (s, p, d or f) within a shell
146
Substitution reaction
A reaction in which an atom or group of atoms is replaced with a different atom or group of atoms
147
Termination
The step at the end of a radical substitution which when two radicals combine to form a molecule
148
Thermal decomposition
The breaking up of a chemical substance with heat into at least two chemical substances
149
Troposphere
The lowest layer of the Earth's atmosphere, extending from the Earth's surface up to about 7 km (above the poles) and to about 20 km (above the tropics).
150
Unsaturated hydrocarbon
A hydrocarbon containing carbon-to-carbon multiple bonds
151
van der Waals' forces
Very weak attractive forces between induced dipoles in neighbouring molecules.
152
Volatility
The ease with which a liquid turns into a gas. Volatility increases as boiling point decreases
153
Water of crystallisation
Water molecules that form an essential part of the crystalline structure of a compound.
