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Key Terms Flashcards

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1
Q

acid

A

a species that releases H+ ions in an aq solution

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2
Q

acid dissociation constant Ka

A

the equilibrium constant that shows the extent of dissociation of a weak acid

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3
Q

acid-base pairs

A

A pair of two species that transform into each other by gain or loss of a proton

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4
Q

activation energy

A

the minimum energy required to start a reaction by the breaking of bonds

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5
Q

actual yield

A

the amount of product obtained from a reaction

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6
Q

addition polymerisation

A

formation of a very long molecular chain, by repeated addition reactions of many unsaturated alkene monomers

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7
Q

addition reaction

A

a reaction in which a reactant is added to an unsaturated molecule to make a one saturated molecule

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8
Q

adsorption

A

the process that occurs when a gas or liquid or solute is held to the surface of a solid

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9
Q

alicyclic

A

containing carbon atoms joined together in a ring that is not aromatic

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10
Q

aliphatic

A

containing carbon atoms joined together in a straight or branched chains.

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11
Q

alkili

A

a type of base that dissolves in water forming hydroxide ions

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12
Q

alkanes

A

the hydrocarbon homologous series with single carbon to carbon bonds and the general formula CnH2n+2

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13
Q

alkenes

A

the hydrocarbon homologous series with at least 1 double carbon to carbon bond and the general formula CnH2n

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14
Q

alkyl group

A

a side chain formed by removing a hydrogen atom from an alkane parent chain, CH3

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15
Q

alkynes

A

the hydrocarbon homologous series with at least one triple carbon to carbon bond and the general formula CnH2n-2

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16
Q

aromatic

A

containing one or more benzene ring

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17
Q

atom economy

A

(sum of molar masses of desired products)/(sum of molar masses of all products)

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18
Q

atomic number

A

number of protons in the nucleus of an atom.

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19
Q

atomic orbital

A

A region around the nucleus that can hold up 2 electrons with opposite spins.

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20
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.

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21
Q

Base

A

A compound that neutralises an acid to form a salt.

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22
Q

Binary compound

A

A compound containing 2 elements only.

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23
Q

Bond dissociation 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.

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24
Q

Bronsted-lowry acid

A

A species that is a proton donor.

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25
Q

Bronsted-lowry base

A

A species that is a proton acceptor.

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26
Q

Buffer solution

A

A system that minimises the pH changes on addition of small amounts of an acid or a base.

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27
Q

Carbocation

A

An ion that contains a positively charged carbon atom.

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28
Q

Catalyst

A

A substance that increases the rate of a chemical reaction without being used up in the process; a catalyst provides an alternative route for the reaction with a lower activation energy.

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29
Q

Cation

A

A positively charged ion with fewer electrons than protons.

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30
Q

Chain reaction

A

A reaction in which the propagation steps release new radicals that continue the reaction.

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31
Q

Chemical shift

A

A scale in ppm, that compares the frequency of an NMR absorption with the frequency of the reference TMS at delta=0 ppm.

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32
Q

Chiral carbon

A

A carbon atom attached to four different atoms or groups of atoms.

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33
Q

Chromatogram

A

A visible record showing the result of separation of the components of a mixture by chromatography.

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34
Q

cis-trans isomerism

A

A special type of E/Z isomerism in which there are 2 non-hydrogen groups and two hydrogen atoms around the c=c double bond; the cis isomer- Z- has H atoms on each carbon on the same side; the trans isomer- E- has H atoms on each carbon on different sides.

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35
Q

Closed system

A

A system isolated from it’s surroundings

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36
Q

Collision theory

A

Two reacting particles must collide for a reaction to occur, and must be in the correct orientation and have sufficient energy to overcome the activation energy of the reaction.

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37
Q

Complex ion

A

A transition metal ion bonded to ligands by coordinate bond- dative covalent bonds.

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38
Q

Concentration

A

The amount of solute, in moles, dissolved in 1dm3 of solution.

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39
Q

Condensation reaction

A

A reaction in which two small molecules react together to form a larger molecule with elimination of a small molecule such as water.

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40
Q

Conjugate acid

A

A species that releases a proton to form a conjugate base

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41
Q

Cojugate base

A

A species that accepts a proton to form a conjugate acid.

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42
Q

Coordinate bond

A

A shared pair of electrons in which the bonded pair has been provided by one of the bonding atoms only; dative covalent bond.

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43
Q

Coordination number

A

The total number of coordinate bonds formed between a central ion and ligands.

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44
Q

Covalent bond

A

The electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms.

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45
Q

Dehydration

A

An elimination reaction in which water is removed from a saturated molecule to make an unsaturated molecule.

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46
Q

Delocalised electrons

A

Electrons that are shared between more than 2 atoms.

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47
Q

Desorption

A

Release of an adsorbed substance from a surface.

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48
Q

Dipole

A

A separation of electrical charge so that one atom of a polar covalent bond =, or one end of a polar molecule, has a small positive charge and the other has a small negative charge.

49
Q

Displacement reaction

A

A reaction in which a more reactive element replaces a less reactive element from an aqueous solution of its ions.

50
Q

Displayed formula

A

A formula showing the relative positioning of all the atoms in a molecule and the bonds between them.

51
Q

Disproportionation

A

A redox reaction in with the same element is both oxidised and reduced.

52
Q

Dynamic equilibrium

A

The equilibrium that exists in a closed system when the rate of the forward reaction is equal to the rate of the reverse reaction and concs don’t change.

53
Q

E/Z isomerism

A

A type of stereoisomerism in which different groups are attached to each carbon of a C=C double bond may be arranged differently in space because of the restricted rotation of the C=C.

54
Q

Electronegativity

A

A measure of the attraction of a bonded atom of the pair of electrons in a covalent bond.

55
Q

Electrophile

A

An atom or group of atoms which is attracted to an electron-rich centre or atom where it accepts a pair of electrons to form a new covalent bond.

56
Q

Electrophilic addition

A

An addition reaction in which the first step is attack by an electrophile on a region of high electron density.

57
Q

Electrophilic substitution

A

A type of substitution 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.

58
Q

Elimination reaction

A

Removal of a molecule from a saturated molecule to make an unsaturated molecule.

59
Q

Empirical formula

A

The formula that shows the simplest whole-number ratio of atoms of each element present in a compound.

60
Q

Enantiomers

A

Stereoisomers that are non-superimposable mirror images of each other- optical isomers.

61
Q

End point

A

The point in a titration where the indicator changes colour; the end point indicates when the reaction is just complete.

62
Q

Endothermic reaction

A

A reaction in which the enthalpy of the products is greater than the enthalpy of the reactants, resulting in heat being taken from the surroundings - delta H is +

63
Q

Enthalpy H

A

The heat content that is stored in a chemical system.

64
Q

Enthalpy change

A

The difference between the enthalpy of the products and the enthalpy of the reactants.

65
Q

Enthalpy cycle

A

A diagram showing the alternative routes between reactants and products which allows the indirect determination of an enthalpy change from other known enthalpy changes using Hess’s Law.

66
Q

Enthalpy profile diagram

A

A diagram for a reaction to compare the enthalpy of the reactants with the enthalpy of the products.

67
Q

Entropy

A

The dispersal of energy within a chemical system.

68
Q

Equilibrium constant

A

A measure of the position of equilibrium; the magnitude of an equilibrium constant indicates whether there are more reactants or more products in an equilibrium system.

69
Q

Equivalence point

A

The point in a titration at which the volume of one solution has reacted exactly with the volume of the second solution.

70
Q

Esterification

A

A reaction in which a carboxylic acid reacts with an alcohol to form water and an ester.

71
Q

Exothermic reaction

A

A reaction in which the enthalpy of the products is smaller than the enthalpy of the reactants, resulting in heat loss to the surroundings. Delta H is -

72
Q

First ionisation energy

A

The energy requires to remove one electron from each atom in one mole of gaseous atoms of an element to form one mole of gaseous 1+ ions.

73
Q

Fractional distilation

A

The separation of components in a liquid mixture by their different boiling points into fractions with different compositions.

74
Q

Fragment ions

A

Ions formed from the breakdown of the molecular ion in a mass spectrometer.

75
Q

Fragmentation

A

The process in mass spectrometry that causes a positive ion to split into smaller pieces, one of which is a positive fragment ion.

76
Q

Free energy change- ΔG

A

The balance between enthalpy, entropy and temperature for a process given by;
ΔG= ΔH-TΔS. A process feasible when ΔG>0.

77
Q

Giant covalent lattice

A

A 3D structure of atoms bonded together by strong covalent bonds.

78
Q

Giant metallic lattice

A

A 3D structure of positive ions and delocalised electrons, bonded together by strong metallic bonds.

79
Q

Giant ionic lattice

A

A 3D structure of oppositely charged ions, bonded together by strong ionic bonds.

80
Q

Group

A

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.

81
Q

half-life

A

The time taken for the concentration of a reactant to decrease by half

82
Q

Hess’s Law

A

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..

83
Q

Heterogeneous catalyst

A

A reaction in which the catalyst has a different physical state from the reactants; frequently reactants are gases whilst the catalyst is a solid.

84
Q

Fingerprint region

A

An area of an infrared spectrum below 1500cm-1 that gives a characteristic pattern for different compounds

85
Q

First electron affinity

A

The enthalpy change that takes place when one electron is added to each atom in one mole of gaseous atoms to form one mole of gaseous 1- ions.

86
Q

heterogeneous equilibrium

A

An equilibrium in which the species making up the reactants and products have different physical states.

87
Q

heterolytic fission

A

The breaking of a covalent bond forming a cation and an anion.

88
Q

Homogeneous catalyst

A

A reaction in which the catalyst and reactants are in the same physical state, which is most frequently the aqueous or gaseous state.

89
Q

Homogeneous equilibrium

A

An equilibrium in which all the species making up the reactants and products have the same physical state.

90
Q

Homologous series

A

A series of organic compounds with the same functional group but with each successive member differing by CH2.

91
Q

Homolytic fission

A

The breaking of a covalent bond with one of the bonded electrons going to each atom, forming 2 radicals.

92
Q

Hydrated

A

A crystalline compound containing water molecules.

93
Q

Hydrogen bond

A

A strong dipole-dipole attraction between an electron- deficient hydrogen atom of -NH, -OH of HF on one molecule and a lone pair of electrons on a highly electronegative atom containing an N, O or F on a different molecule.

94
Q

Hydrolysis

A

A reaction with water that breaks a chemical compound into 2 compounds, the H and OH in a water molecule becomes incorporated into the two other compounds.

95
Q

Induces dipole-dipole interaction

A

Attractive forces between induced dipoles in different molecules- london forces.

96
Q

Initial rate of reaction

A

The change in concs. of a reactant or product per unit of time at the start of the reaction t=0

97
Q

initiation

A

The first stage in a radical reaction in which radicals start when a covalent bond is broken by homolytic fission of a covalent bond.

98
Q

intermediate

A

A species formed during a reaction that reacts further and is not present in the final products.

99
Q

Intermolecular forces

A

An attractive force between molecules. IM forces can be london forces, permanent dipole-dipole interactions or hydrogen bonding.

100
Q

ion

A

A positively or negatively charged atom or a covalently bonded group of atoms where the number of electrons is different from the number of protons.

101
Q

ionic bonding

A

The electrostatic attraction between positive and negative ions.

102
Q

ionic product of water Kw

A

The product of the ions formed in the partial dissociation of water, given by Kw= [H+(aq)][OH-(aq)]

103
Q

lattice enthalpy

A

The enthalpy change that accompanies the formation of one mole of an ionic compound from it’s gaseous ions under standard conditions.

104
Q

Le Chatelier’s principle

A

When a system under dynamic equilibrium is subjected to an external change, the system readjusts itself to minimise the effect of the change and restore equilibrium.

105
Q

Ligand

A

A molecule or ion that can donate a pair of electrons to the transmission metal ion.

106
Q

Ligand substitution

A

A reaction in which one or more ligands in a complex ion are replaced by different ligands.l

107
Q

limiting reagent

A

The reactant that is not in excess, which will be used up first and stop the reaction.

108
Q

metallic bond

A

The electrostatic attraction between positive metal ions and delocalised electrons.

109
Q

Neutralisation

A

A chemical reaction in which an acid and a base react together to form a salt and one mole of water.

110
Q

nucleophile

A

An atom which is attracted to an electron- deficient centre or atom, where it donates a pair of electrons to form a new covalent bond.

111
Q

Nucleophilic substitution

A

A reaction in which a nucleophile is attracted to an electron-deficient carbon atom, and replaces an atom or group of atoms on the carbon atom.

112
Q

Optical isomers

A

Stereoisomers that are non-superimposable mirror images of each other; also called enantiomers.

113
Q

Order

A

The power to which the conc. of a reactant is raised in the rate equation.

114
Q

Overall order

A

The sum of the individual orders of reactants in the rate equation.

115
Q

Oxidation number

A

A measure of the number of electrons that an atom uses to bond with atoms of other elements.

116
Q

Pi- bond

A

A bond formed by the sideways overlap of 2 p-orbitals, with the electron density above and below the plane of the bonding atoms.

117
Q

Partial dissociation

A

The splitting of some of a species in solution into an aq ion.

118
Q

Pauling electronegativity value

A

A value assigned as a measure of the relative attraction of a bonded atom for the pair of electrons in a covalent bond.

119
Q
A

Chemistry (6 decks)

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