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A level- Chemistry > Inorganic and foundations definitions > Flashcards

Inorganic and foundations definitions Flashcards

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1
Q

Define acid

A

A speices that releases H+ ions in aqueous solution

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2
Q

Define acid dissociation constant Ka

A

The equilibrium constant that shows the extent of dissociation of a weak acid.
For weak acid HA Ka=[H+ (aq)] [A-(aq)] / [HA(aq)]

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3
Q

Define acid-base pair

A

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

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4
Q

Define 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 reaction

A

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

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7
Q

Define 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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8
Q

Define alkali

A

A type of base that dissolves in water forming hydroxide ions

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9
Q

Define amount of substance

A

The quantity whose unit of the mole, used as a means of counting any species such as atoms, ions and molecules

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10
Q

Define anhydrous

A

Containing no water molecules

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11
Q

Define anion

A

A negatively charged ion with more electrons than protons

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12
Q

Define atom economy

A

Atom economy= (Sum of molar masses of desired products)/ (Sum of molar masses of all products) *100

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13
Q

Define atomic number

A

The number of protons in the nucleus of an atom

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14
Q

Define atomic orbital

A

A region around the nucleus that can hold up to two electrons with opposite spins

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15
Q

Define 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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16
Q

Define Avogadro constant

A

The number of atoms per mole of the carbon-12 isotope (6.023*10^23 mol-1)

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17
Q

Define base

A

A proton acceptor. A compound that neutralises an acid to form a salt

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18
Q

Define binary compound

A

A compound containing two elements only

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19
Q

Define bonded pair

A

A pair of electrons shared between two atoms to make a covalent bond

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20
Q

Define buffer solution

A

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

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21
Q

Define 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 lower activation energy

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22
Q

Define cation

A

A positively charged ion with fewer electrons than protons

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23
Q

Define closed system

A

A system isolated from its surroundings

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24
Q

Define 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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25
Q

Define complex ion

A

A transition metal ion bonded to ligands by coordinate bonds

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26
Q

Define concentration

A

The amount of solute, in mols dissolved in 1 dm3 of solution

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27
Q

Define conjugate acid

A

A species that releases a proton to form a conjugate base

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28
Q

Define a conjugate base

A

A species that accepts a proton to form a conjugate acid

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29
Q

Define coordinate bond

A

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

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30
Q

Define coordination number

A

THe total number of coordinate bonds formed between a central metal ion and ligands

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31
Q

Define covalent bond

A

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

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32
Q

Define dative covalent

A

A shared pair of electrons in which the bonded pair has been provided by one of the bonding atoms only; also called a coordinate bond

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33
Q

Define dehydration

A

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

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34
Q

Define delocalised electrons

A

Electrons that are shared between more than two atoms

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35
Q

Define desorption

A

Release of an adsorbed substance from a surface

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36
Q

Define dipole

A

A separation in 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

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37
Q

Define displacement reaction

A

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

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38
Q

Define disproportionation

A

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

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39
Q

Define 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 concentrations do not change

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40
Q

Define E/Z isomerism

A

A type of stereoisomerism in which different groups 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 bond

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41
Q

Define electronegativity

A

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

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42
Q

Define elimination reaction

A

The removal of a molecule from a saturated molecule to make an unsaturated molecule

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43
Q

Define enantiomers

A

Stereoisomers that are non-superimposable mirror images of each other; also called optical isomers

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44
Q

Define end point

A

The point in a titration where the indicator changes colour; the endpoint indicated when the reaction is just complete

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45
Q

Define 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 in from the surroundings

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46
Q

Define enthalpy

A

The heat content that is stored in a chemical system

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47
Q

Define enthalpy change

A

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

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48
Q

Define enthalpy cycle

A

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

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49
Q

Define entropy

A

Used to describe the dispersal of energy and disorder within the chemicals making up the chemical system

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50
Q

Define equilibrium constant

A

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

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51
Q

Define 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

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52
Q

Define 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

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53
Q

Define 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

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54
Q

Define first ionisation energy

A

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

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55
Q

Define free energy change deltaG

A

The balance between enthalpy, entropy and temperature for a process.
Given by ΔG= ΔH-T ΔS
A process is feasible when ΔG<0

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56
Q

Define giant covalent lattice

A

A 3d structure of atoms, bonded together by strong covalent bonds

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57
Q

Define giant ionic lattice

A

A 3d structure of oppositely charged ions bonded together by strong ionic bonds

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58
Q

Define giant metallic lattice

A

A 3d structure of of positive ions bonded together by strong metallic bonds

59
Q

Define 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

60
Q

Define half-life

A

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

61
Q

Define 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 energy change is the same for each route

62
Q

Define heterogeneous catalysis

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

63
Q

Define heterogeneous equilibrium

A

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

64
Q

Define homogeneous catalysis

A

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

65
Q

Define homogeneous equilibrium

A

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

66
Q

Define hydrated

A

A crystalline compound containing water molecules

67
Q

Define hydrogen bond

A

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

68
Q

Define induced dipole-dipole interactions

A

Attractive forces between induced dipoles in different molecules- London forces

69
Q

Define initial rate of reaction

A

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

70
Q

Define intermolecular force

A

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

71
Q

Define ionic bonding

A

The electrostatic attraction between positive and negative ions

72
Q

Define ionic product of water Kw

A

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

73
Q

Define isotopes

A

Atoms of the same element with different numbers of neutrons and different masses but the same number of protons

74
Q

Define lattice enthalpy

A

The enthalpy change that accompanies the formation of one mole of an ionic compound from its gaseous ions under standard conditions

75
Q

Define Le Chatelier’s principle

A

When a system in dynamic equilibrium is subjected to a external change, the system readjusts itself to minimise the effect of the chage and to restore equilibrium

76
Q

Define ligand

A

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

77
Q

Define ligand substitution

A

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

78
Q

Define limiting reagent

A

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

79
Q

Define lone pair

A

An outer shell pair of electrons that is not involved in chemical bonding

80
Q

Define metallic bond

A

The electrostatic attraction between positive metal ion sand delocalised electrons

81
Q

Define molar gas volume

A

The volume per mole of gas molecules at a stated temperature and pressure

82
Q

Define molar mass

A

The mass per mole of a substance in units g mol-1

83
Q

Define mole

A

The amount of any substance containing as many elementary particles as there are carbon atoms in exactly 12g of the carbon-12 isotope that is, 6.02*10^23 particles

84
Q

Define molecule

A

The smallest part of a covalent compound that can exist while retaining its chemical identity, consisting of two or more atoms covalently bonded together,

85
Q

Define neutralisation

A

A chemical reaction in which an acid and a base react together to produce a salt

86
Q

Define optical isomers

A

Stereoisomers that are non-superimposable mirror images of each other; also known as enantiomers

87
Q

Define order

A

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

88
Q

Define overall order

A

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

89
Q

Define oxidation

A

Loss of electrons of an increase in oxidation number

90
Q

Define oxidation number

A

A measure of the number of electrons that an atom uses to bond with atoms of another element.

91
Q

Define oxidising agent

A

A reagent that oxidises another species

92
Q

Define pi-bond

A

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

93
Q

Define percentage yield

A

percentage yield= (amount in mol, of a product)/ (theoretical amount, in mol, of product) *100

94
Q

Define period

A

A horizontal row of elements in the periodic table. Elements show trends in properties across a period

95
Q

Define periodicity

A

A repeating trend in properties of the elements across each period of the periodic table

96
Q

Define permanent dipole

A

A small charge difference that does not change across a bond, with delta positive and delta negative partial charges on the bonded atoms: the result of the bonded atoms having different electronegativities

97
Q

Define permanent dipole-dipole interactions

A

An attractive force between permanent dipoles in neighbouring polar molecules

98
Q

Define pH

A

pH= -log[H+(aq)]

99
Q

Define polar molecule

A

A molecule that has an overall dipole taking into account all dipoles across bonds and the shape of molecules.

100
Q

Define polyatomic ion

A

An ion containing more than one atom

101
Q

Define position of equilibrium

A

The relative quantities of reactants and products, indicating the extent of a reversible reaction at equilibrium

102
Q

Define precipitation reaction

A

The formation of a solid from a solution during a chemical reaction. Precipitates are often formed when two aqueous solutions are mixed together

103
Q

Define rate constant k

A

The constant that links the rate of reaction with the concentration of the reactants raised to the powers of their orders in the rate equation

104
Q

Define rate equation

A

For a reaction A+B→C with orders m for A and n for B, the rate equation is give by; rate=k[A]^m[B]^n

105
Q

Define rate of reaction

A

The change in concentration of a reactant or product in a given time

106
Q

Define rate-determining step

A

The slowest step in the reaction mechanism of a multi-step reaction

107
Q

Define redox reaction

A

A reaction involving both reduction and oxidation

108
Q

Define reducing agent

A

A reagent that reduces another species

109
Q

Define reduction

A

Gain of electrons or a decrease in oxidation number

110
Q

Define reflux

A

The continual boiling and condensing of a reaction mixture back to the original container to ensure that the reaction takes place without the contents of the flask burning dry

111
Q

Define relative atomic mass

A

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

112
Q

Define relative formula mass

A

The weighted mean mass of the formula unit of a compound compared with 1/12 of the mass of an atom of carbon-12

113
Q

Define relative isotopic mass

A

The mass of an atom of an isotope compared with 1/12 of the mass of an atom of carbon-12

114
Q

Define relative molecular mass

A

The weighted mean mass of a molecule of a compound compared with 1/12 of the mass of an atom of carbon-12

115
Q

Define reversible reaction

A

A reaction that takes place in both forward and reverse directions

116
Q

Define sigma bond

A

A bond formed by the end on overlap of one orbital from each bonding atom, consisting of two electrons and with the electron density centred around a line directly between the nuclei of the two atoms.

117
Q

Define salt

A

The product of a reaction in which the H+ ions from the acid are replaced by metal or ammonium ions

118
Q

Define shell

A

A group of atomic orbitals with the same main energy level

119
Q

Define shielding effect

A

The repulsion between electrons in different inner shells. Shielding reduces the net attractive force between the positive nucleus and the outer shell electrons

120
Q

Define specific heat capacity

A

The energy required to raise the temperature of 1g of a substance by 1 degrees

121
Q

Define spectator ions

A

Ions that are present but take no part in a chemical reaction

122
Q

Define standard conditions

A

A pressure 100kPa
Temperature 298 K
Concentration 1 mol dm-3

123
Q

Define standard electrode potential

A

The e.m.f of a half cells compared with a standard hydrogen half-cell, measured under standard conditions

124
Q

Define standard enthalpy change of atomisation

A

The enthalpy change that takes place when one mole of gaseous atoms are formed from its elements in their standard state

125
Q

Define standard enthalpy change of combustion

A

The enthalpy change that takes place when one mole of a substance reacts completely with oxygen under standard conditions, all reactants and products being in their standard states

126
Q

Define standard enthalpy change of formation

A

Enthalpy change when one mole of a compound is formed from its elements in their standard states under standard conditions

127
Q

Define standard enthalpy change of hydration

A

The enthalpy change that takes place when one mole of gaseous ions is dissolved in water forming one mole of aqueous ions under standard conditions

128
Q

Define standard enthalpy change of neutralisation

A

The enthalpy change that accompanies the reaction of an acid by a base to form one mole of H2O (l), under standard conditions, with all reactants and products in their standard states

129
Q

Define standard enthalpy change of reaction

A

The enthalpy change that accompanies a reaction in the molar quantities expressed in a chemical equation under standard conditions, all reactants and products being in their standard states

130
Q

Define standard enthalpy change of solution

A

The enthalpy change that takes place when one mole of a compound is completely dissolved in water under standard conditions.

131
Q

Define stereoisomers

A

Compounds with the same structural formula but with a different arrangement of the atoms in space

132
Q

Define stoichiometry

A

The ratio of the amount, in mols, of each substance in a chemical equation

133
Q

Define strong acid

A

An acid that dissociates completely in solution

134
Q

Define structural isomers

A

Molecules with the same molecular formula but a different structural formula

135
Q

Define sub-shell

A

A group of orbitals of the same type within a shell

136
Q

Define substitution reaction

A

A reaction in which an atom or group of atoms is replaced with a different atom or group of atoms

137
Q

Define surroundings

A

Everything that is not the chemical system

138
Q

Define system

A

The chemicals involved in the reaciton

139
Q

Define theoretical yield

A

The yield resulting from complete conversion of reactants to products

140
Q

Define thermal decomposition

A

The breaking up of a chemical substance with heat into at least two chemical substances

141
Q

Define transition element

A

A d-block element which forms at least 1 stable ion with an incomplete d sub-shell

142
Q

Define volatility

A

The ease at which a liquid turns into a gas. Volatility increases as boiling point decreases

143
Q

Define water of crystallisation

A

Water molecules that are bonded into a crystalline structure of a compound

144
Q

Define weak acid

A

An acid that dissociated only partially in solution

A level- Chemistry (31 decks)

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