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Chemistry > DEFINITIONS > Flashcards

DEFINITIONS Flashcards

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1
Q

Atomic number (Z)

A

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

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2
Q

Mass number

A

The sum of the number of protons and the number of neutrons in the nucleus of that atom

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3
Q

Isotope

A

Atoms of the same element with different masses ( different number of neutrons )

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4
Q

Relative atomic mass (Ar)

A

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

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5
Q

Relative isotopic mass

A

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

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6
Q

Molecular ion peak

A

The peak with the highest m/z ratio in the mass spectrum; the M peak

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7
Q

Quantum shell

A

Defines the energy level of an electron

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8
Q

Orbital

A

A region within an atom that can hold up to two electrons with opposite spins

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9
Q

Electronic configuration

A

The number of electrons in each sublevel in each energy level of the atom

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10
Q

Hund’s rule

A

States that electrons will occupy the orbitals singly before pairing takes place

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11
Q

Pauli Exclusion Principle

A

States that two electrons cannot occupy the same orbital unless they have opposite spins

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12
Q

First ionisation energy

A

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

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13
Q

Second ionisation energy

A

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

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14
Q

Groups

A

The vertical columns in the Periodic Table

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15
Q

Periods

A

The horizontal rows in the Periodic Table

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16
Q

Blocks

A

The Periodic Table is divided into three ; s-block , p-block and d-block

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17
Q

Periodicity

A

A regular repeating pattern of atomic, physical and chemical properties with increasing atomic number

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18
Q

Delocalised electrons

A

Electrons that’s are not associated with any single atom or any single covalent bond

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19
Q

Metallic bonding

A

The electrostatic force of attraction between the nuclei of metal cations and delocalised electrons

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20
Q

Fragmentation

A

The process is mass spectrometry that causes a positive ion to split into pieces, one of which is a positive fragment ion, which will be registered at the detector.

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21
Q

Hydrocarbon

A

A compound that contains only carbon and hydrogen atoms

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22
Q

Saturated

A

A compound containing only single bonds

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23
Q

Unsaturated

A

A compound containing one or more multiple bonds

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24
Q

Multiple bonds

A

Two or more covalent bonds between two atoms

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25
Q

Displayed formula

A

Shows every atom and every bond

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26
Q

Structural formula

A

Shows ( unambiguously ) how the atoms are joined together

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27
Q

Skeletal formula

A

Shows all the bonds between carbon atoms

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28
Q

Molecular formula

A

Shows the actual numbers of each atom in the molecule

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29
Q

Empirical formula

A

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

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30
Q

Functional group

A

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

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31
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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32
Q

Structural isomers

A

Compounds with the same molecular formula but with different structural formulae

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33
Q

Stereoisomers

A

compounds with the same structural formula (and molecular formula) but the atoms or groups arranged differently in three dimensions

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34
Q

Geometric isomers

A

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

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35
Q

Restricted rotation

A

When a C=C bond fixes the position of the atoms or groups attached to the C=C atoms

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36
Q

Fractional distillation

A

The process used to separate a liquid mixture into fractions by boiling and condensing

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37
Q

Cracking

A

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

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38
Q

Reforming

A

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

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39
Q

Complete combustion

A

Means that all the atoms in the fuel are fully oxidised

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40
Q

Incomplete combustion

A

Means that some of the atoms in the fuel are not fully oxidised

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41
Q

Biofuels

A

Fuels obtained from living matter that has died recently

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42
Q

Renewable

A

Sources that can be continuously replaced

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43
Q

Non-renewable

A

Sources that are not being replenished, except over geological timescales

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44
Q

Biodiesel

A

A fuel made from vegetable oils obtained from plants

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45
Q

Bioalcohols

A

Fuels made from plant matter, often using enzymes or bacteria

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46
Q

Substitution reaction

A

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

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47
Q

Mechanism

A

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

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48
Q

Homolytic fission

A

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

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49
Q

Radical

A

A species that contains an unpaired electron

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50
Q

Initiation

A

Step that involves the formation of radicals, usually as a result of bond breaking caused by ultraviolet radiation

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51
Q

Propagation

A

The two steps that , when repeated many times over , concert the starting materials into the products of a reaction

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52
Q

Termination

A

Step that involves the formation of a molecule from 2 radicals

53
Q

Addition reaction

A

Reaction in which two molecules combine to form one molecule

54
Q

Hydrogenation

A

Involves the addition of hydrogen

55
Q

Halogenation

A

Involves the addition of a halogen

56
Q

Hydration

A

Involves the addition of water ( or steam )

57
Q

Diol

A

Compound containing two OH ( alcohol ) groups

58
Q

Curly arrows

A

Represent the movement of electron pairs

59
Q

Electrophile

A

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

60
Q

Electrophilic addition

A

A reaction in which 2 molecules form one molecule and the attacking molecule is an electrophile

61
Q

Heterolytic fission

A

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

62
Q

Electron-releasing

A

A group that pushed electrons toward the atom it is joined to

63
Q

Monomers

A

The small molecules that combine together to form a polymer

64
Q

Repeat unit ( of a polymer )

A

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

65
Q

Recycling (polymers)

A

Converting polymer waste into other materials

66
Q

Incinerator

A

Converts polymer waste into energy

67
Q

Feedstock

A

Involves converting polymer waste into chemicals that can be used to make new polymers

68
Q

Biodegradable (polymer)

A

One that can be broken down by microbes in the environment

69
Q

Nucleophile

A

A species that donates a lone pair of electrons to form a covalent bond with and electron-deficient atom

70
Q

Hydrolysis

A

A reaction in which water or hydroxide ions replace an atom in a molecule with an —OH group

71
Q

Nitriles

A

Organic compounds containing the C-CN group

72
Q

Primary amines

A

Compounds containing the C-NH2 group

73
Q

Nucleophillic substitution

A

A reaction in which an attacking nucleophile replaces an existing atom or group in a molecule

74
Q

Ethanolic (solution)

A

One in which ethanol is the solvent

75
Q

Elimination (reaction)

A

One in which a molecule loses atoms attached to adjacent carbon atoms , forming a C=C double bond

76
Q

Halogenation

A

A reaction that results in the replacement of the hydroxyl group in an alcohol molecule by a halogen atom

77
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

78
Q

Ketones

A

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

79
Q

Aldehydes

A

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

80
Q

Carboxylic acids

A

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

81
Q

Heating under reflux

A

Involves heating a reaction mixture with a condenser fitter vertically

82
Q

Distillation with addition

A

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

83
Q

Simple distillation

A

Used to separate liquids with very different boiling temperatures

84
Q

Fractional distillation

A

Used to separate liquids with very similar boiling temperatures

85
Q

Solvent extraction

A

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

86
Q

Molar mass

A

The mass per mole of a substance. It has the symbol M and the units g mol-1

87
Q

Mole

A

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

88
Q

Avogadro constant

A

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

89
Q

Hydrates

A

Compounds containing water of crystallisation

90
Q

Avogadro’s law

A

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

91
Q

Solute

A

Substance that is dissolved

92
Q

Solvent

A

Substance that dissolves absolute

93
Q

Solution

A

Absolute dissolved in a solvent

94
Q

Mass concentration

A

The mass (g) of the solute divided by the volume (dm3) of the solution

95
Q

Molar concentration

A

The amount (mol) of the solute divided by the volume (dm3) of the solution

96
Q

Standard solution

A

A solution whose concentration is accurately known

97
Q

Primary standards

A

Substances used to make a standard solution by weighing

98
Q

Equivalence point

A

The point at which there are exactly the right amount of substances to complete the reaction

99
Q

End point

A

The point at which the indicator just changes colour

100
Q

Meniscus

A

The curving of the upper surface in a liquid in a container

101
Q

Titre

A

The volume added from the burette during a titration

102
Q

Concordant titres

A

Those that are close together (usually within 0.20 cm3 of each other)

103
Q

Error

A

The difference between an experimental value and the accepted or correct value

104
Q

Accuracy

A

A measure of how close values are to the accepted or correct value

105
Q

Precision

A

A measure of how close values are to each other

106
Q

Random errors

A

Errors caused by unpredictable variations in conditions

107
Q

Systematic errors

A

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

108
Q

Measurement uncertainty

A

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

109
Q

Percentage uncertainty

A

The actual measurement uncertainty multiplied by 100 and divided by the value recorded

110
Q

Theoretical yield

A

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

111
Q

Actual yield

A

The actual mass obtained

112
Q

Percentage yield

A

100 x the actual yield divided by the theoretical yield

113
Q

Atom economy

A

The molar mass of the desired product divided by the sun of the molar masses of all the products , expressed as a percentage

114
Q

Displacement reaction

A

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

115
Q

Precipitation reaction

A

Reactions in which an insoluble solid is one of this products

116
Q

Homogeneous system

A

A system in which all the components are in the same phase

117
Q

Heterogenous system

A

A system in which at least two different phases are present

118
Q

Exothermic

A

Heat energy is transferred from the system to the surroundings

119
Q

Endothermic

A

Heat energy is transferred from the surroundings to the system

120
Q

Standard enthalpy change of 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

121
Q

Standard enthalpy change of combustion

A

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

122
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

123
Q

Standard enthalpy change of formation

A

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

124
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

125
Q

Bond enthalpy

A

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

126
Q

Mean bond enthalpy

A

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

127
Q

Electronegativity

A

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

128
Q

Polar covalent bond

A

A type of covalent bond between two atoms where the bonding electrons are unequally distributed. Because of this, one atom carries a slight negative charge and the other a slightly positive charge

Chemistry (6 decks)

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