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Chemistry George > ALL DEFINITIONS > Flashcards

ALL DEFINITIONS Flashcards

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1
Q

Acid

A

A species that is a proton donor.

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2
Q

Activation energy

A

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

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3
Q

Addition polymer

A

A very long molecular chain formed by repeated addition reactions of many unsaturated alkene molecules

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4
Q

Addition reaction

A

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

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5
Q

Adsorption

A

The process that occurs when a gas, liquid or solute is held to the surface of a solid or a liquid(rare).

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6
Q

Alicyclic hydrocarbon

A

A hydrocarbon with carbon atoms joined together in a ring structure

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7
Q

Aliphatic hydrocarbon

A

A hydrocarbon with carbon atoms joined together in a straight or branched chain

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8
Q

Alkali

A

A type of base that dissolves in water forming hydroxide ions, (OH-, aqueous ions)

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9
Q

Alkanes

A

The homologous series with the general formula CnH2n+2

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10
Q

Alkyl group

A

An alkane with a hydrogen atom removed (often denoted R)

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11
Q

Amount of Substance

A

The quantity with unit mole, used for counting atoms

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12
Q

Anhydrous

A

A substance that contains no water molecules

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13
Q

Anion

A

A negatively charged ion (no one likes onions-negative anions)

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14
Q

Atom economy

A

(Mr of desired product)/(Mr of all products) *100%

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15
Q

Atomic orbital

A

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

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16
Q

Atomic number

A

Number of protons in the nucleus of an atom

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17
Q

Average bond enthalpy

A

Average enthalpy change that takes place when 1 mol of a type of bond in the molecules of a gas are broken by homolytic fission

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18
Q

Avogadro constant (Na)

A

The number of atoms per mole of the carbon-12 isotope (6.02 *10^23 mol^-1)

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19
Q

Base

A

A species that is a proton acceptor

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20
Q

Biodegradable material

A

A substance that is broken down naturally in the enviroment by living organisms

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21
Q

Carbanion

A

An organic ion in which a carbon atom has a negative charge

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22
Q

Carbocation

A

An organic ion in which a carbon atom has a positive charge

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23
Q

Catalyst

A

A substance that increases the rate of chemical reaction without being used up in the process

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24
Q

Cation

A

A positively charged ion (everyone likes cats)

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25
Q

Cis-trans isomerism

A

Type of E/Z isomerism, hydrogen and non hydrogen atom on each C in C=C, CIS: hydrogen on same side of bond, TRANS: hydrogen on opposite sides of bond

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26
Q

Concentration

A

The amount of solute, in mol, per 1 dm^-3 of solution

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27
Q

Coordinate bond

A

A shared pair of electrons which has been provided by only one of the bonding atoms (aka dative covalent)

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28
Q

Covalent bond

A

A bond formed by a shared pair of electrons

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29
Q

Cracking

A

The break down of a long chained saturated hydrocarbon to form a mixture of shorter chained alkanes and alkenes

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30
Q

Curly arrow

A

Symbol used in reaction mechanisms to show the movement of an electron pair in the breaking or formation of a covalent bond

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31
Q

Dative covalent

A

A shared pair of electrons which has been provided by only one of the bonding atoms

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32
Q

Dehydration

A

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

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33
Q

Delocalised electrons

A

Electrons that are shared between more than two atoms

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34
Q

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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35
Q

Disproportionation

A

The oxidation and reduction of the same element in a redox reaction

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36
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

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37
Q

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 due to restricted rotation of C=C bond

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38
Q

Electron configuration

A

The arrangement of electrons in an atom

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39
Q

Electronegativity

A

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

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40
Q

Electron sheilding

A

The repulsion between electrons in different inner shells, sheilding reduces the net attractive force from the positive nucleus on the outer shell electrons

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41
Q

Electrophile

A

An atom, or group, that is attracted to an electron dense space or atom, where it accepts a pair of electrons to form a new covalent bond

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42
Q

Electrophillic addition

A

A type of addition reaction in which an electrophile is attracted to an electron dense atom, it accepts an electron pair to form a new covalent bond

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43
Q

Elimination reaction

A

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

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44
Q

Emperical formula

A

The simplest whole number ratio of atoms of each element in a compound

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45
Q

Endothermic reaction

A

A reaction in which the enthalpy of the products is greater than the enthalpy of the reactants, results in heat being taken in from the surroundings

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46
Q

Enthalpy

A

The heat content that is stored in a chemical system

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47
Q

Standard enthalpy change of combustion

A

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

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48
Q

Standard enthalpy of formation

A

The enthalpy change that takes place when one mole of a compound is formed from its pure elements in their standard states under standard conditions

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49
Q

Standard enthalpy of reaction

A

The enthalpy change of a reaction in molar quantities expressed in a chemical equation under standard conditions

50
Q

Enthalpy cycle

A

Diagram showing alternative routes between reactants and products to allow indirect determination of enthalpy change (from other known enthalpy changes using Hess’ Law)

51
Q

Enthalpy profile diagram

A

Diagram comparing enthalpy levels of reactants and products in a reaction

52
Q

Esterification

A

The reaction of an alcohol with a carboxylic acid to produce an ester and water

53
Q

Exothermic reaction

A

A reaction in which the enthalpy of the products is smaller than the enthalpy of the reactants, results in heat loss to surroundings

54
Q

Fractional Distillation

A

The seperation of components in a liquid mixture into fractions which differ in boiling point by distillation, using a fractionating column

55
Q

Fragmentation

A

The process in mass spectrometry that cause a postive ion to split into pieces, one of which is a positive fragment ion

56
Q

Functional group

A

The part of the organic molecule responsible for its chemical properties and reactions

57
Q

General formula

A

The simplest algebraic formula of a member of a homologous series

58
Q

Giant covalent lattice

A

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

59
Q

Giant ionic lattice

A

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

60
Q

Giant metallic lattice

A

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

61
Q

Greenhouse effect

A

Process in which the absorption and subsequent emission of infrared radiation by the atmospheric gases warms the lower atmosphere and planet’s surface

62
Q

Hess’ Law

A

If a reaction can take place by more than one route and the intital and final conditions are the same, the total enthalpy along each route will be the same

63
Q

Heterogeneous catalysis

A

A reaction in which the catalyst has a different physical state to the reactants

64
Q

Homogeneous catalysis

A

A reaction in which the catalyst and reactants are in the same physical state

65
Q

Heterolytic fission

A

Breaking of a covalent bond with both of the bonded electrons going to one of the atoms, forming a cation and anion

66
Q

Homolytic fission

A

Breaking of a covalent bond with one of the bonded electrons going to each atom, forming two radicals

67
Q

Homologous series

A

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

68
Q

Hydrated

A

Crystalline and containing water molecules

69
Q

Hydrogen bond

A

A strong dipole attraction between an electron deficient hydrogen atom on one molecules and a lone pair of electrons on a highly electronegative atom of a different molecule

70
Q

Hydrolysis

A

A reaction with water or aqueous hydroxide ions that breaks a chemical compound into two compounds

71
Q

Initiation

A

The first step in radical substitution where radicals are generated by UV radiation

72
Q

Intermolecular forces

A

Attractive force between neighbouring molecules: induced dipole/permenant dipole/ hydrogen bonds

73
Q

Ionic bonding

A

Electrostatic attraction between oppositely charged ions

74
Q

First ionisation energy

A

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

75
Q

Second ionisation energy

A

The energy required to remove one electron from each ion in one mole of gaseous 1+ ions to from one mole of gaseous 2+ ions

76
Q

Isotope

A

Atoms of the same element with a different number of neutrons and different masses

77
Q

le Chatelier’s principle

A

When a system in dynamic equilibrium is subjected to a change the, the position of equilibrium will shift to minimise the change

78
Q

Limting reagent

A

The substance in a chemical reaction that runs out first

79
Q

Lone pair

A

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

80
Q

Metallic bond

A

The electrostatic attraction between positive metal ions and decolised electrons

81
Q

Molar volume

A

The volume per mole of gas, units dm^3 mol^-1, at RTP molar volume is 24 dm^3 mol^-1

82
Q

Mole

A

The amount of any substance containing as many particles as there are carbon atoms in 12g of carbon-12

83
Q

Nucleophile

A

An atom (or group of atoms) that is attracted to an electron deficient center or atom, where it donates a pair of electrons to form a new covalent bond

84
Q

Oxidation

A

Loss of electrons or an increase in oxidation number

85
Q

Oxidising agent

A

A reagent that oxidises (takes electons from) another species

86
Q

Percentage yeild

A

(Actual mol of product)/ (theoretical mol of product) *100%

87
Q

Periodicity

A

A repeating pattern or trend shown across periods

88
Q

Permenant dipole

A

A small charge difference across a bond resulting from a difference in electronegativity of bonded atoms

89
Q

Permanent dipole-dipole force

A

An attractive force between permenant dipoles in neighbouring polar molecules

90
Q

Pi - bond

A

The reactive part of a double bond, formed above and below the plane of the bonded atoms by sideways overlap of p-orbitals

91
Q

Polar covalent bond

A

A bond with a permanent dipole

92
Q

Polar molecule

A

A molecule with an overall dipole, accounting for dipoles across bonds

93
Q

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

94
Q

Principal quantum number, n

A

Number representing the relative overall energy of each orbital, increases with distance from the nucleus, sets of orbitals with the same n value are referred to as energy levels

95
Q

Propogation

A

The two repeated step in radical substitution that build up the products in a chain reaction

96
Q

Redox reaction

A

A reaction in which both reduction and oxidation take place

97
Q

Reducing agent

A

A reagent that reduces (adds electrons to) another species

98
Q

Reflux

A

Continual boiling and condensing of a reaction mixture to ensure that the reaction takes place fully between reactants and intermediates

99
Q

Relative atomic mass, Ar

A

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

100
Q

Relative formula mass

A

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

101
Q

Relative isotopic mass

A

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

102
Q

Salt

A

A chemical compound formed from an acid when a H+ ion from the acid has been replaces by a metal ion of other positive ion

103
Q

Saturated hydrocarbon

A

A hydrocarbon with single bonds only

104
Q

Shell

A

A group of atomic orbitals with the same principal quantum number

105
Q

Simple molecular lattice

A

A 3D structure of molecules, bonded together by weak intermolecular forces

106
Q

Species

A

Any type of particle that takes part in a chemical reaction

107
Q

Specific heat capacity

A

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

108
Q

Spectator ion

A

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

109
Q

Standard conditions

A

A pressure of 100kPa (1 atm), a temp of 298K (25*C), conc of 1 mol dm^-3

110
Q

Standard solution

A

A solution of known concentration, standard solutions used in titrations to determine unknown information about another substance

111
Q

Standard state

A

The physical state of a substance under standard conditons

112
Q

Stereoisomers

A

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

113
Q

Stoichiometry

A

The molar relationship between the relative quantities of substances taking part in a reaction

114
Q

Stratosphere

A

The second layer of the Earth’s atmosphere, containing the ‘ozone layer’, 10-50km above Earth

115
Q

Structural isomers

A

Molecules with the same molecular formula but with different structural arrangements of atoms

116
Q

Substitution reaction

A

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

117
Q

Termination

A

The end step of radical substitution when two radicals combine to form a molecule

118
Q

Thermal decomposition

A

The breaking up of chemical substance with heat into atleast 2 products

119
Q

Unsaturated hydrocarbon

A

A hydrocarbon containing carbon to carbon multiple bonds

120
Q

Van deer Waal’s forces

A

Very weak attractive forces between induced dipoles in neighbouring molecules (induced dipole)

121
Q

Volatility

A

The ease with which a liquid turns into a gas, volatility increases as boiling point decreases

122
Q

Water of crystallisation

A

Water molecules that form an essential part of the crystalline structure of a compound

Chemistry George (4 decks)

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