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A-Level Chemistry > Keywords > Flashcards

Keywords Flashcards

1
Q

Addition reaction

A

Reaction where a molecule joins to an unsaturated molecule to produce a saturated molecule

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2
Q

Aliphatic

A

Organic compounds containing C chains and branches

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3
Q

Aromatic

A

Organic compounds containing one or more benzene ring(s)

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4
Q

Carbocation

A

A positive ion with the positive charge on a C atom

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5
Q

Cyclic

A

Organic compounds containig C rings(not aromatic rings) also called alicyclic

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6
Q

Dehydration

A

Elimination of water

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7
Q

Dehydrogenation

A

Elimination of hydrogen

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8
Q

Electrophile

A

An electron deficient atom, ion or molecule that take part in an organic reaction by attacking areas g high electron density in another reactant

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9
Q

Elimination reaction

A

Reaction where a molecule is lost from a saturated molecule to form an unsaturated molecule

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10
Q

Free radical

A

Species with an unpaired electron

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11
Q

Functional group

A

The atom or group of atoms that is responsible for most of the chemical reactions of a molecule

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12
Q

Homologous series

A

A family of compounds with the same general formula and similar chemical properties. In a series, each member differs by the addition of a CH2 group and there is a gradual change in physical properties

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13
Q

Hydration

A

Addition of water

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14
Q

Hydrocarbon

A

Molecule containing hydrogen and carbon only

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15
Q

Hydrogenation

A

Addition of hydrogen

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16
Q

Hydrolysis

A

A reaction involving the breaking of bonds due to reaction with water

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17
Q

Nucleophile

A

An ion or group of atoms with a negatively charged or partially negatively charged area that takes parts in an organic reaction by attacking an electron deficient area in another reactant

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18
Q

Organic chemistry

A

Study of compounds containing carbon

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19
Q

Saturated

A

Molecule containing no double bonds

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20
Q

Stereoisomers

A

Molecules with the same molecular and structural formulae but different spatial arrangement of atoms

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21
Q

Geometric isomers

A

Type of stereoisomerism: molecules which have different arrangement of groups around C=C

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22
Q

Optical isomers

A

Type of stereoisomerism: molecules which are non-superimposable mirror images

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23
Q

Structural isomers

A

Molecules with the same molecular formula but different structures

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24
Q

Chain isomers

A

Type of structural isomerism: structural isomers that differ by having a different carbon chain

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25
Q

Position isomers

A

Type of structural isomerism: structural isomers that differ by having the fuctional group in a different position

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26
Q

Functional group isomers

A

Type of structural isomerism: structural isomers that differ by having a different functional group

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27
Q

Substitution reaction

A

Reaction where an atom/group replaces another atom/group

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28
Q

Unsaturated

A

Molecule containing double bond(s)

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29
Q

Primary haloalkane

A

A carbon joined to a halogen and only one other alkyl group

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30
Q

Secondary haloalkane

A

A carbon joined to a halogen and two other alkyl groups

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31
Q

Tertiary haloalkane

A

A carbon joined to a halogen and three other alkyl groups

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32
Q

Alkyl

A

Groups, often attached to organic compounds, derived from alkanes with a missing H.

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33
Q

Polar

A

The description of a molecule in which the charge is not equally distributed. One area is slightly positively charged and the other is slightly negatively charged

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34
Q

Electronegativity

A

The ability of atoms to pull electrons towards themselves in a covalent bond

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35
Q

Covalent bond

A

Describes a chemical bond in which electrons are shared between two atoms

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36
Q

Ionic bond

A

Describes a chemical bond in which an electron is lost or gained resulting in oppositely charged ions with electrostatic forces of attraction between them

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37
Q

Intermolecular forces

A

Forces between molecules

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38
Q

Molecular formula

A

The actual number of atoms of each element in one molecule of the compound

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39
Q

Empirical formula

A

The formula that represents the simplest ratio of the atoms of each element present in a compound

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40
Q

Complete combustion

A

Oxidation of alkanes with plenty of oxygen and the only products are carbon dioxide and water

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41
Q

Fuel

A

A substance that burns exothermically

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42
Q

Cracking

A

The breaking of long alkane chains into shorter more useful chains some of which are alkenes

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43
Q

Global warming

A

An increase in the temperature of the Earth’s surface

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44
Q

Greenhouse gas

A

A gas that absorbs long wavelength infrared radiation given off by the Earth but does not absorb the Sun’s radiation

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45
Q

Halide

A

Group 7 ion

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46
Q

Petroleum Fraction

A

Mixture of hydrocarbons collected over a particular range of boiling points during the fractional distillation of crude oil

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47
Q

Petroleum

A

A mixture consisting mainly of alkane hydrocarbons

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48
Q

Enthalpy

A

A measure of the heat content of a substance

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49
Q

Enthalpy change

A

The energy change at a constant pressure

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50
Q

Exothermic

A

A reaction where at the end of the reaction, energy has been given out

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51
Q

Endothermic

A

A reaction where at the end of the reaction, energy has been taken in

52
Q

Activation Energy

A

The minimum amount of kinetic energy that particles need to react; the energy difference between the reactants and the transition state

53
Q

Standard enthalpy of formation

A

The enthalpy change when 1 mole of a compound is formed from its elements with all substances in their standard states under standard conditions

54
Q

Standard enthalpy of combustion

A

The enthalpy change when 1 mole of a compound is completely burnt in oxygen under standard conditions and all the reactants and products in their standard states

55
Q

Standard enthalpy of neutralisation

A

The enthalpy change when 1 mole of water is formed in a reaction between an acid and alkali under standard conditions

56
Q

Standard enthalpy of reaction

A

The enthalpy change for a reaction with the quantities shown in the chemical reaction. This means that the value should always be quoted along with the reaction

57
Q

Specific heat capacity

A

The amount of energy it takes to raise the temperature of 1g of a substance by 1K

58
Q

Alkaline earth metals

A

The metals in group 2 of the periodic table

59
Q

Aldehyde

A

An organic compound with the general formula RCHO in which there is a C=O double bond

60
Q

Alkane

A

A hydrocarbon with C-C and C-H single bonds only, with the general formula CnH2n+2

61
Q

Allotropes

A

Pure elements which can exist in different physical forms in which their atoms are arranged differently. For example, diamond, graphite and buckminsterfullerene are allotropes of carbon

62
Q

Anaerobic respiration

A

The process by which the energy is released and new compounds formed in living things in the absence of oxygen

63
Q

Atomic economy

A

This describes the efficiency of a chemical reaction by comparing the total number of atoms in the product with the total number of atoms in the starting materials

64
Q

Atomic orbital

A

A region of space around an atomic nucleus where there is a high probability of finding an electron

65
Q

Avogadro constant

A

The total number of particles in a mole of a substance. Also called the Avogadro number. it is equal to 6.022*10^23

66
Q

Bond dissociation enthalpy

A

The enthalpy change required to break a covalent bond with all species in the gaseous state

67
Q

Calorimeter

A

An instrument for measuring the heat changes that accompany chemical reactions

68
Q

Catalyst

A

A substance that alters the rate of a chemical reaction but is not used in the reaction

69
Q

Catalytic cracking

A

The breaking, with an aid of a catalyst, of long-chained alkanes into shorter chain hydrocarbons some of which are alkenes

70
Q

Carbon-neutral

A

A process, or series of processes, in which as much carbon dioxide is absorbed from the air as is given out

71
Q

Chemical feedstock

A

The starting materials in an industrial chemical process

72
Q

Co-ordinate bonding

A

Covalent bonding in which both the electrons in the bond come from one of the atoms in the bond - also called dative covalent bonding

73
Q

Delocalised electrons

A

Describes electrons that are spread over several atoms and help to bond them together

74
Q

Dipole-dipole force

A

An intermolecular force that results from the attraction between molecules with permanent dipoles

75
Q

Displayed formula

A

The formula of a compound drawn out so that each atom and each bond is shown

76
Q

Disproportionation

A

Describes a redox reaction in which the oxidation number of some atoms of a particular element increases and that of other atoms of the same element decreases

77
Q

Dynamic equilibrium

A

A situation in which the composition of a reaction mixture does not change because both forward and backward reactions are proceeding at the same rate

78
Q

Electron density

A

The probability of an electron being found in a particular volume of space

79
Q

Electron pair repulsion theory

A

A theory which explains the shapes of simple molecules by assuming that pairs of electrons around a central atom repel each other and thus take up positions as far away as possible from each other in space

80
Q

Electrophilic addition

A

A reaction in which a carbon-carbon double bond is saturated and in which the initial reaction is an attack by an electrophile

81
Q

Electrostatic forces

A

The forces of attraction and repulsion between electrically charged particles

82
Q

Elimination

A

A reaction in which an atom or group of atoms is removed from a reactant

83
Q

Enthalpy diagrams

A

Diagrams in which the enthalpies of the reactants and products of a chemical reaction are plotted on a vertical scale to show their relative levels

84
Q

Equilibrium mixture

A

The mixture of reactants and products formed when a reversible reaction is allowed to proceed in a closed container until no further change occurs. The forward and backward reactions are still proceeding but at the same rate

85
Q

Fingerprint region

A

The area of an infra-red spectrum below about 1500cm. It is caused by complex vibrations of the whole molecule and is characteristic of a particular molecule

86
Q

Group

A

A vertical column of elements in the periodic table, The elements have similar properties because they have the same outer electron arrangement

87
Q

Half equation

A

An equation for a redox reaction which considers just one of the species involved and shows explicitly the electrons transferred to and from it

88
Q

Heterogeneous catalyst

A

A catalyst which is in a different phase from the reactants. For example, iron in the haber process conversion of nitrogen and hydrogen to ammonia

89
Q

Homogeneou catalyst

A

A catalyst which is in the same phase as the reactants

90
Q

Hydrogen bonding

A

A type of intermolecular force in which a hydrogen atom covalently bonded to an electronegative atom interact with another electronegative atom

91
Q

Incomplete combustion

A

A combustion reaction in which there is insufficient oxygen for all the carbon in the fuel to burn to carbon dioxide. Carbon monoxide and/or soot are formed

92
Q

Ionic bonding

A

Describes a chemical bond in which an electron or electrons are transferred from one atom to another, resulting in the formation of oppositely charged ions with electrostatic forces of attraction between them

93
Q

Ketone

A

An organic compound with the general formula R2CO in which there is a C=O double bond

94
Q

Lattice

A

A regular three dimensional arrangement of atoms, ions or molecules

95
Q

Leaving group

A

An atom or group of atoms that is rejected from the stating material, normally taking with it an electron pair and forming a negative ion

96
Q

Lone pair

A

A pair of electrons in the outer shell of an atom that is not involved in bonding. Also called an unshared pair

97
Q

Maxwell-Boltzmann distribution

A

The distribution of energies(and therefore speeds) of the molecules in a gas or liquid

98
Q

Mean bond enthalpy

A

The average value of the bond dissociation enthalpy for a given type of bond taken from a range of different compounds

99
Q

Metallic bonding

A

Describes a chemical bond in which the outer electrons are spread over a lattice of metal ions in a delocalised system

100
Q

Mole

A

A quantity of a substance that contains the Avogadro number of particles

101
Q

Molecular ion

A

A molecule of the sample which has been ionised but which has not broken up during its flight through the mass spectrometer

102
Q

Monomer

A

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

103
Q

Nucleon

A

Protons and neutrons found in the nuclei of atoms

104
Q

Nucleophilic substitution

A

An organic reaction in which a molecule with a partially positively charged carbon atom is attacked by a reagent with a negative charge or partially negative charge. It results in the replacement of one of the groups or atoms on the original molecule by the nucleophile

105
Q

Nucleus

A

Thee tiny, positively charged centre of an atom composed of protons and neutrons

106
Q

Oxidation

A

A reaction in which an atom or group of atom loses electrons

107
Q

Oxidation state

A

The number of electrons lost or gained by an atom in a compound compared to the uncombined atom. It forms the basis of a way of keeping track of redox reactions

108
Q

Oxidising agent

A

A reagent that oxidises another species

109
Q

Percentage yield

A

The actual amount of product produced divided by the theoretical amount expressed as a percentage

110
Q

Period

A

A horizontal row of elements in the periodic table. there are trends in the properties of the elements as we cross a period

111
Q

Periodicity

A

The regular recurrence of the properties of elements when they are arranged in atomic number order in the periodic table

112
Q

Positive inductive effect

A

Describes the tendency of some atom or group of atoms to release electrons via a covalent bond

113
Q

Proton number

A

The number of protons in the nucleus of an atom

114
Q

Redox reaction

A

It describes reactions in which electrons are transferred from one species to anothe

115
Q

Reducing agent

A

A reagent that reduce (adds electron to) another species

116
Q

Reduction

A

A reaction in which an atom or group of atoms gain electrons

117
Q

Spectator ions

A

Ions that are unchanged during a chemical reaction, i.e. they take no part in the reaction

118
Q

Stoichiometry

A

Describes the simple whole number ratios in which chemical species react

119
Q

Strong nuclear force

A

The force that holds protons and neutrons together in the nucleus of the atom

120
Q

Structural fomula

A

A way of writing the formula of an organic compound in which bonds are not shown but each carbon atom is written separately with the atom or group of atoms attached to it

121
Q

Thermochemical cycle

A

A sequence of chemical reactions that convert a reactant into a product. The total enthalpy change of the sequence of reactions will be the same as that for the conversion of the reactant to the product directly

122
Q

van der Waals forces

A

A type of intermolecular force of attraction that is caused by instantaneous dipoles and acts between all atoms and molecules

123
Q

Relative atomic mass

A

The average mass of an atom of an element on a scale where an atom of carbon 12 is 12

124
Q

Relative molecular mass

A

The average mass of a molecule on a scale where an atom of carbon 12 is 12

125
Q

Relative isotopic mass

A

The mass of an atom of an isotope of an element on a scale where an atom of carbon 12 is 12

126
Q

Isotope

A

Atoms of an element which have the same number of protons but different number of neutrons

A-Level Chemistry (30 decks)

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