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A levels > Chemistry AQA AS > Flashcards

Chemistry AQA AS Flashcards

Key facts revision

0
Q

Absolute zero

A

The lowest possible temperature theoretically achieveable -273.15 degrees celius or zero Kelvin

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1
Q

Absolute temperature

A

Temperature measured in Kelvin

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2
Q

Acceleration

A

The stage in mass spectrometry where positive ions are speeded up by an electric field

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3
Q

Acid rain

A

Rain that has been acidified by pollutants such as sulfur dioxide

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4
Q

Actual yield

A

Mass of product obtained in a reaction

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5
Q

Addition polymer

A

Polymer formed when many small unsaturated molecules join together

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6
Q

Addition reaction

A

The adding together of two or more more to form one larger molecule

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7
Q

Aldehyde

A

An organic compound containing the -CHO functional group

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8
Q

Alkaline earth metal

A

An element from group 2 of the periodic table

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9
Q

Alkane

A

A saturated hydrocarbon with the general molecular formula CnH2n

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10
Q

Allotrope

A

Allotropes are different forms of the same element that exist in the same physical state. Diamond and graphite are allotropes of carbon

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11
Q

Alloy

A

A mixture of two or more metals or a mixture of metal and a non metal

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12
Q

Alpha particle

A

A particle consisting of two protons and two neutrons ejected from a nucleus

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13
Q

Amine

A

An organic compound that contains nitrogen atom joined to one or more carbon atoms and two or less hydrogen atoms

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14
Q

Amount of substance

A

The number of particles present, symbol n. It is measured in mole, mol

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15
Q

Anion

A

A negatively charged ion attracted to the anode during electrolysis

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16
Q

Antacid

A

A base taken as a medicine to neutralise excess stomach acid

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17
Q

Aromatic

A

Containing one or more benzene rings

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18
Q

Atom

A

The smallest particle of an element that has the properties of that element

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19
Q

Atom economy

A

The proportion of reactants that are converted into useful products rather than waste products

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20
Q

Atomic number

A

The number of protons in the nucleus of an atom, symbol Z

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21
Q

Atomic radius

A

The distance from the centre of the nucleus to the outer electrons of an atom

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22
Q

Aufbau principle

A

The building up process that describes the filling of atomic orbitals in order of increasing energy

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23
Q

Avogadro constant

A

The number of particles in one mole of a substance- 6.022*10^23

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24
Q

Avogadro’s principle

A

The idea that equal volumes of gases contain the same number of molecules under the same conditions of temperature and pressure

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25
Q

Axial atom

A

Atom positioned at the top or bottom of a trigonal bipyramidal molecule

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26
Q

Barometer

A

An instrument for measuring atmospheric pressure

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27
Q

Base peak

A

The tallest peak in a mass spectrum

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28
Q

Batch process

A

An industrial process that is started and stopped at intervals. Production of ethanol by fermentation is a batch process

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29
Q

Bent line

A

The shape of a molecule that contains two bonding pairs and two lone pairs of electrons

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30
Q

Biofuel

A

A fuel made from the products of living things

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31
Q

Bond angle

A

The angle between two adjacent bonds on the same atom

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32
Q

Bond

A

Attractive force between two atoms, ions or molecules

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33
Q

Boyle’s law

A

The volume of a fixed mass of gas (at a constant temperature) is inversely proportional to its pressure

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34
Q

Burette

A

Labatory apparatus used to add precise volumes of liquid during a titration

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35
Q

Carbocation

A

Ion with a positively charged carbon atom

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36
Q

Carbonyl

A

An organic compound containing the -C+O functional group, found in baldheads and ketones

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37
Q

Carboxyl

A

An organic compound containing the _COOH functional group

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38
Q

Carboxylic acid

A

Organic acids with the general formula RCOOH. Their names end in -oic acid

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39
Q

Cation

A

A positively charged ion, attracted to the cathodde during electrolysis

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40
Q

CFC

A

Abbreviation for chloroflurocarbon, a hydrocarbon in which some or all the hydrogen atoms are replaced by chlorine and fluorine atoms

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41
Q

Chain isomerism

A

A type of structural isomerism in which compounds have identical molecular formulae but their carbon atoms are joined together in different arrangments. Chain isomers involve branched and unbranched carbon chains

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42
Q

Charge density

A

The charge: size ratio of an ion. Small ions with high charges have large charge densities

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43
Q

Charle’s law

A

The volume of a fixed mass of gas (at constant pressure) is proportional to its aboslute temperature

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44
Q

Coke

A

Solid produced by heating coal in the absence of air, almost pure carbon

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45
Q

Complete combustion

A

Burning a fuel in excess oxygen. Carbon dioxide and water vapour are produced from the complete combustion of hydrocarbons

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46
Q

Concordant results

A

Titres that are in agreement usually within 0.10cm3 of each other

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47
Q

Continous process

A

An industrial process in which products are made all the time without any break. Production of iron in the blast furnace is a continuous process

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48
Q

Co-ordinate bond

A

A covalent bond in which the shared pair of electrons is provided by only one of the bonded atoms. In the bond X_>Y, X provides both electrons

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49
Q

Covalent bond

A

A shared pair of electrons

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50
Q

Cracking

A

A process used by the petroleum industry to produce shorter alkanes and alkenes from longer alkanes

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51
Q

Cyclic

A

Hydrocarbons in which there are closed rings of carbon atoms are described as cyclic

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52
Q

D block

A

The central section of the periodic table between groups 2 and 3 containing the transition metals

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53
Q

Dative covalent bond

A

Another name for a coordinate bond

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54
Q

Decomposition reaction

A

A reaction where one substance is broken down into two or more different substances

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55
Q

Deflection

A

The stage in mass spectrometry where positive ions are moved from their original path by a magnetic field

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56
Q

Dehydration reaction

A

A reaction where elements hydrogen and oxygen are removed from a reactant in the ratio of 2:1 effectively the removal of water

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57
Q

Delocalized

A

Electrons that are free to move between all atoms in a structure are delocalized. Delocalized electrons are found in metals and graphite

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58
Q

Detection

A

The stage in mass spectrometry where positive ions reach a detector and produce an electrical signal

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59
Q

Diastereoisomers

A

Stereoisomers that are mirror images of each other, sometimes called geometrical isomers

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60
Q

Diatomic

A

A molcule containing just two atoms

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61
Q

Dimer

A

A molecule consisting of two monomer molecules joined together

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62
Q

Dipole

A

Opposite charges separated by a short distance in a molecule or ion

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63
Q

Displace

A

To replace an atom or ion in a compound in a chemical reaction eg chlorine displaces iodine in sodium iodide

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64
Q

Displayed formula

A

A chemical formula showing all the atoms in a compound and their bonds

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65
Q

Disproportionate

A

The simultaneous oxidation and reduction of a species

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66
Q

Dot and cross diagram

A

A diagram showing all of the bonding electrons in a molecule. The electrons in one atom are shown as dots and the electrons in the other atom are shown as crosses

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67
Q

Double covalent bond

A

A bond in which two atoms are joined by two shared pairs of electrons

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68
Q

Ductile

A

Easily pulled into a thin wire

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69
Q

Electrolysis

A

The decomposition of a compound into simpler substances using an electric current

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70
Q

Electron gun

A

The source of high- energy electrons used to ionize the sample in mass spectrometry

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71
Q

Electron-deficient

A

An atom with a vacant orbital

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72
Q

electro negativity

A

The power of an atom to withdraw electron density from a covalent bond

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73
Q

Electrophile

A

A species that can accept a pair of electrons

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74
Q

Electrophilic addition

A

A reaction in which an electrophile is attracted to a region of high electron density such as a carbon-carbon double bond and adds on to an atom or group

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75
Q

Electrostatic

A

Involving opposite charges

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76
Q

Elimination reaction

A

A reaction in which a small simple molecule is removed from a compound forming a double covalent bond.

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77
Q

Empirical formula

A

A formula that gives the simplest whole number ratio of atoms of each element in a compound

78
Q

Endothermic

A

A reaction in which heat energy is absorbed from the surroundings

79
Q

Endpoint

A

Where the indicator just changes colour in a titration

80
Q

Energy level

A

A certain fixed amount of energy that electrons in an atom can have also called a shell

81
Q

Equatorial atom

A

Atom positioned around the middle of a trigonal bipyramidal molecule

82
Q

Equivalence point

A

In an acid-base titration the point where equal numbers of moles of hydrogen ions and hydroxide ions have reacted

83
Q

Excess

A

More than the amount of reactant needed in a reaction

84
Q

Feedstock

A

Raw material used in a manufacturing process

85
Q

Fermentation

A

the process for making ethanol from sugar using yeast

86
Q

Fingerprint region

A

The part of an infrared spectrum that is unique to a particular compound

87
Q

First ionization energy

A

The energy needed to remove one mole of electrons from one mole of gaseous atoms forming one mole of ions with a single positive charge

88
Q

Flue gas desulfurization

A

Removing sulfur compounds from waste gases produced by combustion

89
Q

Flue gas

A

Waste gases from the combustion of a fuel for example in a power station

90
Q

Fraction

A

A part of a mixture collected at a particular temperature range by fractional distillation. A crude oil fraction contains hydrocarbons with a similar chain length

91
Q

Fractional distillation

A

A method of separating mixtures of liquids or gases according to their boiling temperatures

92
Q

Free radical

A

A species that contains an unpaired electron produced by homolytic fission of a covalent bond

93
Q

Frequency

A

The number of waves per second measured in hertz, Hz

94
Q

Functional group

A

An atom, or group of atoms in a molecule which determines its chemical properties

95
Q

Gas constant

A

The constant used in the ideal gas equation. Symbol R and is approximately 8.31JK^-1mol^-1

96
Q

Giant covalent

A

A structure in which very many atoms are joined by covalent bonds to form a regular structure. Diamond and graphite have giant covalent structures

97
Q

Greenhouse effect

A

Absorption of thermal energy by certain gases in the atmosphere keeping the planet warmer than it would be otherwise

98
Q

Greenhouse gas

A

An atmospheric gas that traps infrared raiation that would otherwise be radiated from the earth’s surface into space

99
Q

Halide ion

A

A negatively charged ion formed when a halogen atom gains an electron

100
Q

High resolution mass spectroemter

A

Device capable of measuring relative atomic masses and relative molecular masses to a high degree of precision

101
Q

Homologous series

A

A series od compounds with the same general formula and functional group. Each member differs from the next by the presence of one more -CH2 group

102
Q

Homolytic fission

A

Breaking of a covalent bond so that each atom takes one electron from the shared pair becoming a radical

103
Q

Hund’s rule

A

Only when all the orbitals in a particular sub level contain an electron do electrons begin to ccupy the orbitals in pairs

104
Q

Hydration

A

The addition of water across a double bond

105
Q

Hydrocarbon

A

A compound containing hydrogen and carbon atoms only

106
Q

Hydrogen bond

A

An intermolecular force between a lone pair of electrons on an N, O or F atom in one molecule and an H atom joined to an N, O or F atom in another molecule

107
Q

Hydrolysis

A

The splitting of a compound by reaction with water

108
Q

Hydroxyl group

A

An -OH group, the functional group found in alcohols

109
Q

Ideal gas equation

A

The equation that describes the relationship between pressure, volume, amount of substance and absolute temperature of a gas pV=nRT

110
Q

Incomplete combustion

A

Burning of a fuel in a restricted amount of oxygen

111
Q

Indicator

A

A substance that changes colour according to the pH of a solution

112
Q

Induced dipole

A

An uneven distribution of charge in a molecule or atom caused by a charge in an adjacent particle

113
Q

Infrared radiation

A

Electromagnetic radiation with a lower frequency than visible light, felt as heat

114
Q

Infrared absorption spectrum

A

Spectrum produced when infrared radiation of various frequencies is absorbed by covalent bonds in a molecule

115
Q

Infrared spectroscopy

A

Method used to analyze compounds by their absorption of infrared radiation

116
Q

Initiation

A

The first stage in a free radical reaction

117
Q

Intermediate

A

Unstable species produced during a reaction before the final product is made

118
Q

Intermolecular force

A

Weak attractive force between molecules

119
Q

Ionic bond

A

Electrostatic force of attraction between oppositely charged ions

120
Q

Ionic radius

A

The distance from the centre of the nucleus to the outer electrons of an ion

121
Q

Ionization

A

Producing an electrically charged particle by adding or removing electrons from an atom or molecule

122
Q

Ionized

A

An atom or molecule that has gained or lost electrons is said to be ionized

123
Q

Isoelectronic

A

Having the same electrong formula but different structural formulae

124
Q

Kelvin

A

The unit of absolute temperature symbol K

125
Q

Ketone

A

An organic compound containing the carbonyl functional group -C=O and with the general formula R1COR2

126
Q

Lattice

A

A regular arrangement of atoms, ions or molecules in a structure

127
Q

Limiting reactant

A

A reactant that is completely used up before the other reactants are converted into products

128
Q

Linear molecule

A

A molecule with all of its atoms in a straight line

129
Q

Lone pair

A

A pair of electrons in the highest occupied energy level that are not used in bonding

130
Q

Malleable

A

Can be bent or hammered into shape without breaking

131
Q

Mass spectrometer

A

An instrument used to determine the relative atomic mass of an element or relative molecular mass of a compound. The structure of a complex molecule can be worked out by analysis of a mass spectrum

132
Q

Mass spectrum

A

The output from a mass spectrometer plotting relative abundance against mass to charge ratio m/z

133
Q

Mass to charge ratio

A

The mass of an ion divided by its charge symbol m/z

134
Q

Metallic bond

A

The electrostatic force of attraction between metal ions and the delocalized electrons in a metallic lattice

135
Q

Metalloid

A

Element with properties that are intermediate between the properties of a metal and the properties of a non metal

136
Q

Molar volume

A

The volume occupied by one mole of gas at a specified temperature and pressure

137
Q

Molarity

A

The concentration of a solution measured in moles of solvent per cubic decimetre of solution mol dm^-3

138
Q

Molecular crystal

A

Covalent molecules held together in a regular arrangement by intermolecular forces

139
Q

Molecular ion

A

In mass spectrometry the ion that produces a peak in a mass spectrum at the highest m/z value

140
Q

Molecular sieve

A

Porous materials such as zeolites that let some molecules pass through but not others

141
Q

Monoprotic

A

An acid containing one replaceable hydrogen ion such as Hcl and HNO3

142
Q

Nitrile

A

An organic compound containing the -C=-tripleN functional group

143
Q

Non polar

A

Having no dipole. A molecule with polar bonds may be non polar if its shape is such that the dipoles cancel each other out

144
Q

Nucleophile

A

A species with a lone pair of electron that is available to form a coordinate bond

145
Q

Nucleophilic substitution

A

A chemical reaction in which one nucleophile replaces another in a molecule

146
Q

Orbital

A

The volume of space in an atom where one or two electrons are most likely to be found

147
Q

Ore

A

A mineral from which metals can be extracted and purified

148
Q

Ozone

A

An allotrope of oxygen with the formula 03

149
Q

Ozone layer

A

The part of the atmosphere with the greatest concentration of ozone. Found in the stratosphere it absorbs harmful ultraviolet radiation from the sun

150
Q

Pauli exclusion principle

A

The idea that an orbital cannot hold more than two electrons

151
Q

Pauling electro negativity scale

A

A scale showing the ability of elements to withdraw electron density from a covalent bond. The larger the number the more electronegative the element

152
Q

Permanent dipole-dipole forces

A

Attractive forces that exist between polar molecules

153
Q

Polar bond

A

A covalent bond between atoms with different electro negativities

154
Q

Polarized

A

Having opposite charges separated by a small distance

155
Q

Polyatomic ion

A

An ion containing more than one atom

156
Q

positional isomerism

A

A type of isomerism where the functional group can be joined at different places on the carbon skeleton

157
Q

Precipitate

A

An insoluable solid formed when two solutions are mixed

158
Q

Primary haloalkane

A

An haloalkane with one carbon atom or where the carbon atom carrying the halogen atom is directly attached to just one other carbon atom

159
Q

Propagation

A

The stage in a free radical mechanism where a particular radical is used in one reaction then produced again in a subsequent reaction

160
Q

Reaction mechanism

A

A step by step description of how a reaction happens

161
Q

Roast

A

Heating strongly in a steam of air usually apllied to metal ores

162
Q

Saturated

A

A compound containing only single covalent bonds between carbon atoms

163
Q

Semiconductor

A

A substance that is an electrical insulator at room temperature but a conductor when warmed or when other elements are added to it

164
Q

Solute

A

The substance that will dissolve in a solvent

165
Q

Solvent

A

The substance in which a solute will dissolve

166
Q

Spectator ion

A

An ion that appears on both sides of an equation but does not take part in the reaction

167
Q

Standard solution

A

A solution whose exact molarity is known

168
Q

Standard temperature and pressure

A

273K and 100kPa

169
Q

Stereoisomer

A

Moelcules with the same structural formula but a different arrangement of their bonds in space

170
Q

Stratosphere

A

Upper part of the atmosphere

171
Q

Structural isomerism

A

When two or more compounds have the same molecular formulae but different structures

172
Q

Sub level

A

Part of an energy level in an atom containing pairs of electrons
S sub levels contain up to one electron pair
P sub levels contain up to three electron pairs
D sub levels contain up to five electron pairs

173
Q

Sublime

A

To pass directly from the solid state to the gas state

174
Q

Substitution

A

The replacement of one atom or group of atoms in a molecule by another atom or group of atoms

175
Q

Temporary dipole

A

The asymmetrical distribution of the electron pair in a covalent bond

176
Q

Termination

A

The final stage in a free radical substitution reaction

177
Q

Theoretical yield

A

The maximum mass of product possible calculated using th emas sof reactants and the balanced equation

178
Q

Thermal cracking

A

The thermal decomposition of hydrocarbons to produce shorter alkanes and alkenes

179
Q

Titrant

A

The solution added from the burette in a titration

180
Q

Titration

A

Method used to find the concentration of a sample using a reactant og known concentration

181
Q

Titre

A

The volume of titrant added to reach the end point in a titration

182
Q

Trigonal bipyramial

A

The shape of a molecule with 5 bonding pairs of electrons

183
Q

Trigonal planar

A

The shape of a molecule with 3 bonding pairs of electrons

184
Q

Trigonal pyramidal

A

The shape of a molecule with 3 bonding pairs and 1 lone pair of electrons

185
Q

Unburned hydrocarbons

A

Pollutants in the exhaust from car engines due to incomplete combustion of the fuel

186
Q

Unsaturated

A

Containing at least one carbon- carbon double bond

187
Q

Valence shell

A

The energy level in an atom that is involved in forming bonds

188
Q

Van der waals forces

A

Temporary induced dipole-dipole attractions between covalent moelcules

189
Q

Volatile

A

A liquid that easily vaporizes is said to be very volatile

190
Q

Volumetric flask

A

An item of glassware used to make up a standard solution. Also called a graduated/standard flask

191
Q

VSEPR

A

Valence shell electron pair repulsion theory. The theory used to predict the shape of a covalent molecule using the idea of repulsion by pairs of electrons

192
Q

Zeolite

A

Compound of aluminium, silicon and oxygen with microscopic pores. Zeolites are used as catalysts and molecular sieves in the petrochemical industry

A levels (5 decks)

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