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Chemistry > Keywords 1 > Flashcards

Keywords 1 Flashcards

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1
Q

Accuracy

A

Measure of how close values are to the corrected/accepted value.

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2
Q

Activation Energy

A

Ea, the minimum energy that colliding particles must possess for a reaction to occur.

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3
Q

Actual yield

A

The actual mass obtained in a reaction.

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4
Q

Addition reaction

A

Two molecules combine to form one molecule.

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5
Q

Aldehydes

A

A homologous series of organic compounds formed by the partial oxidation of primary alcohols.

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6
Q

Atom economy

A

Molar mass of the desired product divided by the sum of the molar masses of all the products, expressed as a percentage.

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7
Q

Atomic Number (z)

A

The number of protons in the nucleus of an atom of an element.

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8
Q

Avogadro’s constant

A

The number of atoms of carbon 12 in exactly 12g of carbon 12.

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9
Q

Avogadro’s Law

A

Equal volumes of gases under the same conditions of temperature and pressure contain the same numbers of molecules.

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10
Q

Base peak

A

Peak with the greatest abundance.

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11
Q

Basic oxides

A

Oxides of metals that react with water to form metal hydroxides, and with acids to form salts and water.

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12
Q

Bioalcohols

A

Fuels made from plant matter, typically using enzymes or bacteria.

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13
Q

Biodegradable polymers

A

Can be broken down by microbes.

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14
Q

Biodiesel

A

Fuel made from vegetable oils obtained from plants.

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15
Q

Biofuels

A

Fuels obtained from living matter that has died recently.

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16
Q

Bond enthalpy

A

The enthalpy change when one mole of the bond in the gaseous state is broken.

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17
Q

Bond length

A

The distance between the nuclei of the two atoms that are covalently bonded together.

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18
Q

Carbocation

A

A positive ion in which the charge is shown on the carbon atom.

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19
Q

Carboxylic acids

A

A homologous series of organic compounds formed by the complete oxidation of primary alcohols.

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20
Q

Catalyst

A

Substance that increases the rate of a chemical reaction, but is chemically unchanged at the end of the reaction.

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21
Q

Coefficients

A

Numbers written in front of species when balancing an equation.

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22
Q

Complete Combustion

A

All of the atoms in the fuel are fully oxidised.

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23
Q

Concordant titres

A

Those that are close together, usually within 0.20 cm3 of each other.

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24
Q

Cracking

A

The breakdown of molecules into shorter ones by heating with a catalyst.

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25
Q

Curly arrows

A

Represent the movement of electron pairs.

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26
Q

Dehydration reaction

A

Results in the removal of the hydroxyl group in an alcohol molecule, together with a hydrogen atom from an adjacent carbon atom, forming a C=C double bond.

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27
Q

Delocalised electrons

A

Electrons not associated with any single atom or any single covalent bond.

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28
Q

Diol

A

A compound containing two OH groups.

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29
Q

Dipole

A

Said to exist when two charges of equal magnitude but opposite signs are separated by a small distance.

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30
Q

Discrete simple molecule

A

An electrically neutral group of two or more atoms held together by covalent bonds.

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31
Q

Displacement reaction

A

A reaction in which one element replaces another element in a compound.

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32
Q

Displayed formula

A

Shows every atom and every bond.

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33
Q

Disproportionation

A

The simultaneous oxidation and reduction of an element in a single reaction.

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34
Q

Distillation with addition

A

Involves heating a reaction mixture, but adding another liquid and distilling off the product as it forms.

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35
Q

Electronegativity

A

The ability of an atom to attract a bonding pair of electrons in a covalent bond.

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36
Q

Electronic configuration

A

Shows the number of electrons in each sublevel in each energy level of an atom.

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37
Q

Electron-releasing

A

A group that pushes electrons towards the atom to which it is joined.

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38
Q

Electrophile

A

A species that is attracted to a region of high electron density.

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39
Q

Electrophilic addition

A

A reaction in which two molecules form one molecule and the attacking molecule is an electrophile.

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40
Q

Elimination

A

Reaction in which a molecule loses atoms attached to the adjacent carbon atoms forming a C=C double bond.

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41
Q

Empirical formula

A

Shows the numbers of each atom in the simplest whole-number ratio.

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42
Q

End point

A

Point at which the indicator just changes colour. Ideally, the end point should coincide with the equivalence point.

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43
Q

Endothermic

A

Heat energy is transferred from the surroundings to the system.

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44
Q

Equivalence point

A

Point at which there are exactly the right amounts of substances to complete the reaction.

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45
Q

Error

A

The difference between an experimental value and the accepted/correct value.

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46
Q

Ethanolic solution

A

One in which ethanol is the solvent.

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47
Q

Feedstock

A

Converting polymer waste into feedstock that can be used to make new polymers.

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48
Q

First ionisation energy

A

The energy required to remove an electron from each atom in one mole of atoms in a gaseous state.

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49
Q

Fractional distillation

A

Process used to separate a liquid mixture into fractions by heating and condensing.

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50
Q

Fragmentation

A

Occurs when the molecular ion breaks into smaller pieces.

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51
Q

Functional group

A

An atom or group of atoms in a molecule that is responsible for its chemical reactions.

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52
Q

Geometric isomers

A

Compounds containing a C=C bond with atoms or groups attached at different positions.

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53
Q

Halogenation

A

Involves the addition of a halogen.

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54
Q

Heating under reflux

A

Heating a reaction mixture with a condenser fitted vertically.

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55
Q

Hess’s Law

A

The enthalpy change of a reaction is independent of the path taken in converting reactants into products, provided the initial and final conditions are the same in each case.

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56
Q

Heterogeneous catalyst

A

One in a different phase to that of the reactants.

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57
Q

Heterogeneous system

A

Where at least two different systems are present.

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58
Q

Heterolytic fission

A

The breaking of a covalent bond, so that both bonding electrons are taken by one atom.

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59
Q

Homogeneous system

A

System in which all components are in the same phase.

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60
Q

Homologous series

A

A family of compounds with the same functional group, which differ in formula by CH2 from the next member.

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61
Q

Homolytic fission

A

The breaking of a covalent bond where each of the bonding electrons leaves with one species, forming radicals.

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62
Q

Hund’s Rule

A

Electrons will occupy orbitals singly before pairing takes place.

63
Q

Hydrates

A

Compounds containing water of crystallisation, indicated in the formulae by .H2O .

64
Q

Hydration

A

Involves the addition of water or steam.

65
Q

Hydrocarbon

A

A compound that contains ONLY carbon and hydrogen atoms.

66
Q

Hydrogen bond

A

Intermolecular interaction between a hydrogen atom of a molecule (or molecular fragment) bonded to another atom which is more electronegative than hydrogen and another atom in the same or a different molecule.

67
Q

Hydrogenation

A

Involves that addition of hydrogen.

68
Q

Hydrolysis

A

Reaction in which water or hydroxide ions replace an atom in a molecule with an —OH group.

69
Q

Incinerator

A

Converts polymer waste into energy.

70
Q

Incomplete combustion

A

Some of the atoms in the fuel are not fully oxidised.

71
Q

Infrared radiation

A

Part of the EM spectrum with frequencies below that of red light.

72
Q

Initiation step

A

Involves the formation of free radicals, usually as a result of bond breaking caused by UV radiation.

73
Q

Intensity of an infrared absorption

A

The amount of infrared radiation absorbed.

74
Q

Isotopes

A

Atoms of the same element with different masses.

75
Q

Ketones

A

A homologous series of organic compounds formed by the oxidation of secondary alcohols.

76
Q

Locant

A

Number used to indicate which carbon atom in the chain an atom or group is attached to.

77
Q

Mass concentration of a solution

A

Mass in grams of the solute divided by the volume of the solution.

78
Q

Mass number

A

The sum of the number of protons and the number of neutrons in the nucleus of an atom.

79
Q

Mean bond enthalpy

A

Enthalpy change when one mole of a bond, averaged out over many different molecules, is broken.

80
Q

Measurement uncertainty

A

The potential error involved when using a piece of apparatus to take a measurement.

81
Q

Mechanism

A

The sequence of steps in an overall reaction. Each step shows what happens to the electrons involved in bond breaking or bond formation.

82
Q

Meniscus

A

The curving of the upper surface in a liquid in a container. The lowest, horizontal part of the meniscus should be read.

83
Q

Metallic bonding

A

Electrostatic force of attraction between the nuclei of metal cations and the delocalised electrons.

84
Q

Molar concentration of a solution

A

The amount in moles of a solute divided by the volume of the solution.

85
Q

Molar mass

A

The mass per mole of a substance. Symbol: M. Units: gmol -1.

86
Q

Molar volume

A

Volume occupied by 1 mole of any gas.

87
Q

Mole

A

The amount of a substance that contains the same number of particles as the number of carbon atoms in exactly 12g of the carbon-12 isotope.

88
Q

Molecular formula

A

Shows the actual number of atoms of each element in a molecule.

89
Q

Molecular ion peak

A

Peak with the highest m/z ratio in the mass spectrum, the M peak.

90
Q

Monomers

A

Small molecules that combine together to form a polymer.

91
Q

Multiple bond

A

Two or more covalent bonds between two atoms.

92
Q

Nitriles

A

Organic compounds containing the C—CN group.

93
Q

Non-renewables

A

Energy sources not being replenished, except over geological timescales.

94
Q

Nucleophile

A

Species that donates a lone pair of electrons to form a covalent bond with an electron-deficient atom.

95
Q

Nucleophilic substitution

A

Reaction wherein an attacking nucleophile replaces an existing atom or group in a molecule.

96
Q

Orbital

A

Region within an atom that can hold up to 2 electrons with opposite spins.

97
Q

Oxidation

A

Loss of electrons.

98
Q

Oxidation number

A

Charge that an ion has or that a species would have, if it were ionic.

99
Q

Oxidised

A

An element is oxidised when its oxidation number increases.

100
Q

Oxidising agent

A

Species that oxidises another species by removing one or more electrons. When an oxidising agent reacts, it gains electrons, so is reduced.

101
Q

Pauli Exclusion Principle

A

Two electrons cannot occupy the same orbital unless they have opposite spins. Spin is shown by up and down arrows.

102
Q

% uncertainty

A

The actual measurement uncertainty x 100 and divided by the value recorded.

103
Q

% yield

A

100 x the actual yield divided by the theoretical yield.

104
Q

Periodicity

A

Regularly repeating pattern of chemical, physical and atomic properties with increasing atomic number.

105
Q

Pi bonds

A

Covalent bonds formed when electron orbitals overlap sideways.

106
Q

Polar covalent bond

A

Type of covalent bond between two atoms where the bonding electrons are unequally distributed. One atom carries a partial positive charge and the other a partial negative charge.

107
Q

Precipitation reaction

A

An insoluble solid is one of the products.

108
Q

Precision

A

A measure of how close values are to each other.

109
Q

Primary amines

A

Compounds containing the C—NH2 group.

110
Q

Primary standards

A

Substances used to make a standard solution by weighing.

111
Q

Propagation

A

Two steps that, when repeated many times, convert the starting materials into the products of the reaction.

112
Q

Quantum shell

A

The energy level of an electron.

113
Q

Radical

A

Species that contains an unpaired electron.

114
Q

Random errors

A

Errors caused by unpredictable variations in conditions.

115
Q

Recycling

A

Converting polymer waste into other materials.

116
Q

Redox reaction

A

A reaction; that involves both reduction and oxidation.

117
Q

When an element is reduced…

A

Its oxidation number decreases.

118
Q

Reducing agent

A

Species that reduces another species by adding one or more electrons. When a reducing agent reacts, it loses electrons, so is oxidised.

119
Q

Reduction

A

Gain of electrons.

120
Q

Reforming

A

The conversion of straight-chain hydrocarbons into branched-chain and cyclic hydrocarbons.

121
Q

Relative atomic mass (Ar)

A

The weighted mean of a mass of an atom of an element compared to 1/12 the mass of an atom of carbon 12.

122
Q

Relative isotopic mass

A

The mass of an individual atom of a particular isotope relative to 1/12 the mass of an atom of carbon-12.

123
Q

Renewable

A

Energy sources that can be continuously replaced.

124
Q

Repeat unit

A

The set of atoms that are joined together in large numbers to produce the polymer structure.

125
Q

Restricted rotation…

A

Around a C=C double bond fixes the position of the atom or groups of atoms attached to the C=C atoms.

126
Q

Saturated

A

A compound containing only single bonds.

127
Q

Second ionisation energy

A

The energy required to remove an electron from each singly-charged, positive ion in one mole of positive ions in the gaseous state.

128
Q

Sigma bonds

A

Covalent bonds formed when electron orbital overlap axially/end on.

129
Q

Simple distillation

A

Used to separate liquids with very different boiling temperatures.

130
Q

Skeletal formula

A

Shows all the bonds between carbon atoms.

131
Q

Solute

A

A substance that is dissolved.

132
Q

Solution

A

Solute dissolved in a solvent.

133
Q

Solvent

A

Substance that dissolves a solute.

134
Q

Solvent extraction

A

Used to separate a liquid from a mixture by causing it to move from the mixture to the solvent.

135
Q

Spectator ions

A

Ions in an ionic compound that do not take part in a reaction.

136
Q

Standard enthalpy change of combustion

A

The enthalpy change measured at 100kPa and a stated temperature, usually 298K, when one mole of a substance is completely burnt in oxygen.

137
Q

Standard enthalpy of formation

A

The enthalpy change measured at 100kPa and a specified temperature, usually 298K, when one mole of a substance is formed from its elements in their standard states.

138
Q

Standard enthalpy change of neutralisation

A

The enthalpy change measured at 100kPa and a stated temperature, usually 298K, when one mole of water is produced by the neutralisation of an acid with an alkali.

139
Q

Standard enthalpy change of a reaction

A

The enthalpy change measured at 100kPa and a stated temperature, usually 298K, when the number of moles of substances in the equation as written react.

140
Q

Standard solution

A

A solution whose concentration is accurately known.

141
Q

Stereoisomers

A

Compounds with the same structural formula, but with atoms or groups arranged differently in 3D.

142
Q

Stretching

A

Occurs when a bond absorbs infrared radiation and uses it to alter the length of the bond.

143
Q

Structural formula

A

Shows how the atoms are joined together.

144
Q

Structural isomers

A

Compounds with the same molecular formula, but with different structural formulae.

145
Q

Substitution reaction

A

One in which an atom or group is replaced by another atom or group.

146
Q

Systematic errors

A

Errors that are constant or predictable, usually because of the apparatus used.

147
Q

Termination step

A

Involves the formation of a molecule from two radicals.

148
Q

Theoretical yield

A

The maximum possible mass of a product, assuming complete reaction and no losses.

149
Q

Thermal stability

A

A measure of the extent to which a compound decomposes when heated.

150
Q

Titre

A

The volume added from a burette during a titration.

151
Q

Transmittance

A

Value in an infrared spectrum that represents the amount of radiation absorbed at a particular wavelength.

152
Q

Unsaturated

A

A compound containing one or more multiple bonds.

153
Q

Wave number of an infrared absorption

A

Represents the frequency of infrared radiation absorbed by a particular bond in a molecule.

Chemistry (23 decks)

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