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Key Definitions Flashcards

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1
Q

Mass number

A

The number of protons added to the number of neutrons in the nucleus
The top number on the periodic table

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2
Q

Atomic number

A

Is the number of protons in the nucleus

The bottom number on periodic table

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3
Q

Relative isotopic mass

A

Mass of an atom of an isotope compared to 1/12th the mass of a 12C atom

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4
Q

Isotopes

A

1:
Atoms with the same atomic number but different mass numbers
2:
Atoms that have the same number of protons but different number of neutrons

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5
Q

Orbital

A

Is a region around the nucleus where there is a high probability of finding an electron, can hold 2 electrons with opposite spins

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6
Q

Hunds rule

A

Electrons occupy orbitals singly before pairing happens

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7
Q

Pauli exclusion principle

A

Electrons in the same orbital must have opposite spins

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8
Q

A group

A

Vertical column in periodic table. Electron configuration is the highest occupied shell is the same for all atoms in main group

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9
Q

First ionisation energy

A

Energy per mile needed to remove an electron from gaseous atoms
X(g) -> X 2+ (g) + e-

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10
Q

Second ionisation energy

A

Energy per mile needed to remove an electron from gaseous ions with a single positive charge

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11
Q

Shielding

A

Electron-electron repulsion. It exists between two electrons in the same orbital between electrons in different orbitals

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12
Q

Atomic radius

A

Distance from the centre of the nucleus to the boundary of the Electron cloud, shows periodicity

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13
Q

Ion

A

Charged particle formed when an atom or group of atoms have lost or gained one or more electrons

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14
Q

Ionic bonding

A

Strong electrostatic forces of attraction between oppositely charged ions

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15
Q

Giant ionic lattice

A

Solid ionic compounds comprises oppositely charged ions arranged in a highly ordered way

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16
Q

Isoelectronic ions

A

Have same electronic configuration and number of electrons

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17
Q

Covalent bond

A

Strong electrostatic attraction between two nucleus and the shared pair of electrons between them

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18
Q

Dative covalent bonding

A

Forms when an orbital white a line pair of electrons in one atom overlaps with vacant orbital in another atom

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19
Q

Bond length

A

Distance between the nucleus of two atoms that are covalently bonded together
Measured in nanometres nm

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20
Q

Bond strength

A

Given by the bond enthalpy for a particular covalent bond

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21
Q

Bond enthalpy

A

Enthalpy change when one mole of w bond in the gaseous state is broken

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22
Q

VSEPR theory

A

Valence shell electron pair repulsion, lets you predict shapes of molecules and ions

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23
Q

Electronegativity

A

Ability of an atom to attract the bonding electrons in a covalent bond

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24
Q

Polar covalent bond

A

Covalent bond is polar is two bonded atoms have different electronegativities

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25
Q

London forces

A

Type of intermolecular forces, acts between molecules

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26
Q

Instantaneous dipole

A

Don’t need differences in electronegativity, can exist in non polar molecules

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27
Q

Induced dipoles

A

Caused when a molecule comes close to a molecule with a permanent dipole or an instantaneous dipole

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28
Q

Hydrogen bonding

A

Intermolecular force between hydrogen and F O N

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29
Q

Solvent

A

Substance in which another substance can dissolve, forming a solution

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30
Q

Solute

A

Substance that dissolved in the solvent.

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31
Q

Soluble

A

Absolute is soluble if it can dissolve in given solvent

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32
Q

Solution

A

Is the mixture formed between solute and its solvent

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33
Q

Hydration

A

Water molecules surround individual ions and form strong electrostatic attractions with them

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34
Q

Metallic bonding

A

Strong electrostatic force of attraction between metal ions and the delocalised electrons

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35
Q

Oxidation number

A

Represents the number of electrons lost of gained by an atom of that element in a compound or iron

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36
Q

Systematic names

A

When an element can have more than one oxidation state, eg copper 11 oxide, copper 1 oxide

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37
Q

Redox reaction

A

Involves both reduction and oxidation, deceived in terms of transfer of electrons or changes in oxidation number

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38
Q

Oxidation

A

Gain of oxygen
Loss of electrons
Increase in oxidation number

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39
Q

Reduction

A

Loss of oxygen
Gain of electrons
Decrease in oxidation number

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40
Q

Oxidising agents

A

Gain electrons, electron acceptors

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41
Q

Reducing agents

A

Lose electrons, they are electron donors

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42
Q

Ionic half equations

A

Shows oxidation from one side of equation and reduction from the other side

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43
Q

Spectator ions

A

Present in a reaction but do not take part in the reaction

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44
Q

Ionisation

A

An atom is ionised if an electron absorbs enough energy to leave it altogether

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45
Q

Disproportionation reaction

A

Element in a single species is simultaneously oxidised and reduces

46
Q

Confirmatory tests

A

Done to be sure of the identity of the haloed ions

47
Q

Mole

A

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

48
Q

Avogadro constant

A

6.02 x 10^23 mol -1

49
Q

Relative atomic mass

Ar

A

The weighted mean mass of an atom of an element compared to 1/12th the mass of a 12C atom

50
Q

Relative formula mass

Mr

A

Calculated by adding together all Ar values for all the atoms present in a unit of a substance

51
Q

Molar mass

A

Is the mass per mole of a substance

Unit g mol -1

52
Q

Molecular formulae

A

Substance shows the actual numbers of atoms of each element in its molecules

53
Q

Empirical formulae

A

Is the simplest whole number ratio of the atoms of each element it contains

54
Q

Structural formula

A

Shows each atom and its position

CH3CH2CH2CH3

55
Q

Equation

A

Balanced when it have same number of atoms of each element in left and right side of equation

56
Q

Avogadro law

A

Equal volumes of gases under the same conditions of temperature and pressure contain the same number of molecules

57
Q

Molar volume

A

Vm

24.0 dm3 mol-1 at RTP

58
Q

Concentration

A

Of solute in a solution can be measured in Mol dm-3 or in g dm-3

59
Q

Titration

A

Method in which the volumes of two reacting solutions are measured so that the concentration of one of the solutions can be determined

60
Q

Atom economy

A

A way to assess chemical reactions, particularly in industrial processes

Is measured of how many atoms of the reactants end up in the desired product

61
Q

Percentage yield

A

Actual yield / theoretical yield x 100

A way to assess chemical reactions

62
Q

Hydrocarbons

A

Compounds of hydrogen and carbon only.

63
Q

Alkanes

A

Hydrocarbon, saturdated, general formula of CnH2n+2

64
Q

Displayed formula

A

H-c-c-h etc

Shows each atom and the bonds it has with other atoms

65
Q

Structural formula

A

CH4

Shows each carbon atom and the atoms bonded to it

66
Q

Isomers

A

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

67
Q

Structural isomers

A

Have same molecular formula but their atoms are arranged in a different order

68
Q

Alkenes

A

Unsaturated hydrocarbons, with general formula of CnH2n

69
Q

Skeleton formula

A

Lines to represent each carbon link

70
Q

Position isomers

A

Structural isomers with same carbon chain but with different functional group

71
Q

Chain isomers

A

Structural isomers in which carbon chains are different

72
Q

Stereoisomers

A

Same molecular formula. Same structural formula, different arrangement of atoms

73
Q

E-Z isomers

A

E isomer is the higher priority groups opposite sides to each other
Z isomer the higher priority groups are together

74
Q

Cis-trans isomers

A

Trans is E, when on opposite sides

Sis is Z when on same side

75
Q

Substituent groups

A

Atoms or groups attached to the carbon atoms in c double bond

76
Q

Crude oil

A

Petroleum
Mixture of hydrocarbons that can be separated by fractional distillation. Each fraction produced contains hydrocarbons with similar boiling points and chain lengths

77
Q

Fractional distillation

A

Relies on differences in boiling temperatures of the different hydrocarbons in crude oil

78
Q

Fractions

A

Crude oil heated and vapours are led into fractionating column hot at bottom and cool at top

79
Q

Cracking

A

Involves chemical reactions that happen at high temperatures using catalyst zeolites and they decompose larger alkanes to produce smaller alkenes and alkanes u

80
Q

Combustion

A

Of alkanes is an example of an oxidation reaction, in which oxygen reacts with the hydrogen and carbon atoms in the alkane molecules

81
Q

Complete combustion

A

Happens when there is sufficient oxygen to oxidise the alkanes fully

82
Q

Incomplete combustion

A

Happens when there is insufficient oxygen to oxidise the alkanes fully

83
Q

Alternative fuels

A

Include biodiesel and bioalcohols from renewable sources such as plants

84
Q

Fuel

A

Is a substance that can release energy usefully through chemical reactions

85
Q

Non renewable

A

Once they’ve been used up they cannot be replaced

86
Q

Carbon neutral

A

Refers to activity that has no overall annual carbon emissions to the atmosphere

87
Q

Renewable energy

A

Eg wind, wave, solar and tidal power

88
Q

Biodiesel

A

Made of vegetable oils such as rapeseed, sunflower and soya

89
Q

Bioalcohol

A

Most common -bioethanol. Alcohol derived from materials produced by living organisms

90
Q

Alcohols

A

Function group -OH

91
Q

Homologous series

A

Same functional group, same general formula, similar chemical properties

92
Q

Halogenalkanes

A

Functional group is halogen atom.

93
Q

Radical substitution reactions

A

Alkanes under go this with halogens to produce halogenalkanes

94
Q

Heterolytic fission

A

One atom gains both bonding electrons and ions form

95
Q

Homolytic fission

A

Each atom keeps a bonding electron and radicals form

96
Q

Radical

A

Species with an unpaired electron

97
Q

Unpaired electron

A

Represented as a dot, places next to the atom whose bond was broken to form the radical

98
Q

Substitution reaction

A

One atom or group is replaced by another atom or group

99
Q

Reaction mechanisms

A

Shows bonds broken or formed and the species (atom or ion or molecule or radical)

100
Q

Sigma bonds

A

Form end on overlap between two s orbitals, two p orbitals or an s and a p orbital

101
Q

Pi bonds

A

Sideways overlap between p orbitals once a sigma bond has formed

102
Q

Electrophilic addition reactions

A

Alkanes undergo reactions with hydrogen halides to produce halogenslkanes

103
Q

Electrophile

A

Species able to accept a pair of electrons, and are attracted to a region of negative charge

104
Q

Unsymmetrical alkenes

A

Undergo electrophilic addition reactions in which two products form, a major product and a Minor product

105
Q

Halogenation

A

Reaction in which a halogen is added to another substance

106
Q

Hydrogenation

A

Reaction in which hydrogen is added to another substance

Nickel catalyst used in hydrogenation

107
Q

Oxidising agent

A

Alkanes react with oxidising agent to produce alcohols containing two hydroxyl groups

108
Q

Exothermic

A

Overall transfer of energy from the system to the surroundings
Negative
Reactants have more energy than products

109
Q

Endothermic

A

Overall transfer of energy to system from surroundings
Positive
Goes up

110
Q

Standard conditions

A

100Kpa , 298K 1 mol dm-1

Chemistry (10 decks)

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