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Chemistry OCR A > Some Important Terms. > Flashcards

Some Important Terms. Flashcards

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1
Q

Atom

A

The smallest possible particle of an element.

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2
Q

Compound

A

A substance composed of two or more elements chemically bonded together.

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3
Q

Molecule

A

An arrangement of atoms covalently bonded together.

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4
Q

Covalent bond

A

A shared pair of electrons holding atoms together in a molecule.

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5
Q

Ions

A

Particle formed from an atom or group of atoms by loss or gain of electrons with, respectively, a positive or negative charge.

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6
Q

Ionic bonding

A

Electrostatic attraction between oppositely charged ions.

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7
Q

Atomic number

A

How many protons there are in an atom.

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8
Q

Mass

A

The number of protons and neutrons in an atom.

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9
Q

Isotopes

A

Atoms that are the same element with a different mass because of a different number of neutrons.

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10
Q

Element

A

A substance Taft cannot be broken down chemically into anything simpler.

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11
Q

Accurate result

A

A result that is close to the true answer

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12
Q

Acid

A

A substance that release hydrogen ions in an aqueous solution– a proton donor

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13
Q

Activation energy

A

The minimum amount of KE that particles need in order to react when they collide

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14
Q

Additional polymer

A

A long-chain molecule made by lots of small Alkene molecules adding together

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15
Q

Alcohol

A

A substance either the general formula CnH2nOH

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16
Q

Aldehyde

A

A substance with the general formula CnH2nO which has a hydrogen and one alkyl group attached to the carbonyl carbon atom

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17
Q

Alicyclic compound

A

An organic compound that contains carbon and hydrogen joined together in a non-aromatic ring.

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18
Q

Aliphatic compound

A

An organic compound that contains carbon and hydrogen joined together in straight chains, branches chains or a non-aromatic ring.

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19
Q

Alkali

A

A base that is soluble in water and release hydroxide ions in aqueous solution

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20
Q

Alkaline earth metal

A

An element in group 2 of the periodic table

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21
Q

Alkene

A

Hydrocarbon with the general formula CnH2n+2. Contains single bonds only.

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22
Q

Alkene

A

A hydrocarbon with the general formula CnH2n and containing at least one carbon-carbon double bond

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23
Q

Alkyl group

A

Hydrocarbon fragment with the general formula CnH2n+1

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24
Q

Anhydrous salt

A

A salts that doesn’t contain any water of crystallisation

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25
Q

Antacid

A

A substance that neutralises stomach acid

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26
Q

Aromatic compounds

A

And organic compound that contains the benzene ring

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27
Q

Atom economy

A

The proportion of reactant atoms that become part of the desired product expressed as a percentage

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28
Q

Proton number

A

The number of protons in the nucleus of an atom

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29
Q

Atomic radius

A

The distance between the nucleus of an atom and the outermost electrons

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30
Q

Average bond enthalpy

A

The energy needed to break one mole of a bond in the gas phase averaged over the different compounds that the bond is found in

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31
Q

Avogadro constant

A

6.02 x 10^23 The number of particles in one mole of a substance

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32
Q

Base

A

A substance that removes hydrogen ions from an aqueous solution- a proton acceptor

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33
Q

Biodegradable

A

A substance that naturally decomposes because organisms can digest it

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34
Q

Bohr model

A

A model for the structure of an atom proposed by Neils Bohr. He suggested that electrons only exist in fixed orbitals (shells) and not anywhere else

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35
Q

Bond enthalpy

A

The energy required to break the bonds between two atoms. Usually given as an average bond enthalpy.

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36
Q

Bond fission

A

The process of breaking a covalent bond

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37
Q

Carbocation

A

An organic ion containing a positively charged carbon atom

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38
Q

Carbonyl compound

A

And organic compound that contains a carbon oxygen double bond

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39
Q

Carboxylic acid

A

A substance that has a COOH Group attach the end of the carbon chain

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40
Q

Catalyst

A

A substance that increases the rate of reaction by providing an alternative reaction pathway with a lower activation energy. The catalyst is chemically unchanged at the end of the reaction.

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41
Q

Catalytic converter

A

A device fitted to a car exhaust system to remove pollutant gases such as carbon Monoxide, nitrogen monoxide and unburned hydrocarbons

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42
Q

Chain Isomer

A

A molecule that contains the same atoms is another molecule that has a different arrangement of the carbon skeleton

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43
Q

Charge density

A

The amount of charge in relation to the size of an ion

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44
Q

CFC

A

A Halo alkane containing fluorine and chlorine and no hydrogen. CFCs contributed ozone-depletion

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45
Q

Cis- teams isomerism

A

A special type of E/Z I summarise them were two of the groups attached to the carbon atoms around the carbon to carbon double bond are the same

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46
Q

Collision theory

A

The theory that a reaction will not take place between two particles unless they collide in the right direction and with at least a certain minimum amount of kinetic energy

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47
Q

Complete combustion

A

Burning a substance is completely in an access of oxygen. Complete combustion of a hydrocarbon will produce carbon dioxide and water only

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48
Q

Concentration

A

A measure of how many moles of a substance or dissolved in a volume of solution

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49
Q

Coordinates or dative covalent bond

A

A covalent bond formed when one atom provides both of the shared electrons

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50
Q

Covalent bond

A

Strong electrostatic attraction between a shared pair of electrons and the nucleus of bonded atoms

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51
Q

Curly arrow

A

And Aaron are used in a reaction mechanism to show the movement of the pair of electrons

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52
Q

Cyclo alkanes

A

A type of alkane which is one or more nonaromatic carbon rings

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53
Q

Dehydration reaction

A

A reaction in which water is eliminated from an organic molecule

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54
Q

Delocalised electrons

A

An electron that is not attached to a specific atom

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55
Q

Dipole

A

The difference in charge between two atoms caused by a shift in the electron density in the bond

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56
Q

Displacement reaction

A

I reaction where a more reactive element pushes out a less reactive element from an ionic solution

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57
Q

Disproportionation

A

When an element is both oxidised and reduced in a single chemical reaction

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58
Q

Displayed formula

A

I way of representing a molecule that shows how all the atoms are arranged and all the bonds between them

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59
Q

Distillation

A

A technique used to separate liquids with different boiling points. A mixture is gently heated so that substances are VAT rate and can be collected in order of increasing boiling point.

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60
Q

E/Z isomerism

A

A type of stereoisomerism that is caused by the restricted rotation about a carbon to carbon double bon. Each of the carbon atoms must be attached to 2 different groups.

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61
Q

Electron configuration

A

The number of electrons that an atom or ion has and how they are arranged

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62
Q

Electron shell

A

A region of an atom with a fixed energy that contains electrons orbiting the nucleus

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63
Q

Electron shell repulsion theory

A

The theory that in a molecule lone pair/ lone pair Bond angles are the biggest, lone pair/ bonding pair Bond angles are the second biggest, and bonding pair/ bonding pair bond angles are the smallest.

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64
Q

Electron shielding

A

Went into electrons affectively screen the other electrons from the pull of the nucleus

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65
Q

Electronegativity

A

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

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66
Q

Electrophile

A

And electron pair exceptor

67
Q

Electrophilic addition

A

A reaction mechanism where the double bond in an alkene opens and atoms are added to the carbon atoms

68
Q

Elimination reaction

A

A reaction in which a pair of atoms or groups of atoms are removed from an organic molecule

69
Q

Empirical formula

A

I thought you like giving the simplest whole number ratio of atoms of each element in a compound

70
Q

Endothermic reaction

A

I reaction that absorbs energy in the form of heat (deltaH is positive)

71
Q

Enthalpy change

A

Heat energy transferred in a reaction at a constant pressure(deltaH)

72
Q

Enthalpy profile diagram

A

A graph showing how the enthalpy changes during a chemical reaction

73
Q

Exothermic reaction

A

If reaction that gives out energy in the form of heat (deltaH is negative)

74
Q

First ionisation energy

A

The energy needed to remove one mole of electrons from one mole of gaseous atoms

75
Q

False positive

A

A result that suggests the presence of something eh ions that isn’t actually there

76
Q

Functional group

A

Group of atoms that is responsible for the characteristic reactions of a molecule

77
Q

Functional group isomers

A

A molecule that has the same molecular formula as another molecule that with atoms are arranged into different functional groups

78
Q

General formula

A

An algebraic formula that can describe any member of a homologous series of compounds

79
Q

Giant covalent lattice

A

A structure consisting of a huge network of covalently bonded atoms

80
Q

Giant ionic lattice structure

A

A regular repeated structure made of oppositely charged ions strongly attracted to each other in all directions

81
Q

Giant metallic lattice structure

A

A regular structure consisting of closely packed positive metal irons in a sea of delocalised electrons

82
Q

Global warming

A

The warming of the planet due to an increased concentration of greenhouse gas in the troposphere which enhanced greenhouse effect

83
Q

Greenhouse effect

A

The absorption and real mission of infrared rays creation by greenhouse gases in this troposphere

84
Q

Greenhouse gas

A

Aigas absorbs and emits infrared radiation and so contributes to the greenhouse effect

85
Q

Halide

A

A negative ion of a halogen

86
Q

Haloalkane

A

An alkane with at least one halogen atom in the place of a hydrogen atom

87
Q

Hesses law

A

The total entropy change of reaction is always the same no matter which route is taken

88
Q

Heterolytic fission

A

When a covalent bond breaks unevenly with one of the bonding atoms receiving both of the electrons from the bonded pair resulting in the formation of a positively charged cation with a negatively charged anion

89
Q

Homologous series

A

A family of organic compounds that have the same general formula and similar chemical properties

90
Q

Homolytic fission

A

When a covalent bond breaks evenly with each bonding atoms receiving one electron from the bonding pair resulting in the formation of two electrically uncharged radicals

91
Q

Hydrated salt

A

A salt that contains water of crystallisation

92
Q

Hydrocarbon

A

A molecule that only contains hydrogen and carbon atoms

93
Q

Hydrogen bond

A

The strongest intermolecular force it occurs when polarised covalent bonds cause hydrogen atoms to form weak bonds with lone pairs of electrons on the fluorine, nitrogen oxygen atoms of other molecules

94
Q

Hydrolysis reaction

A

I reaction when molecules are split apart by water molecules the water molecules are also split into hydrogen ions and hydroxide ions

95
Q

Incomplete combustion

A

Burning a substance in a poor supply of oxygen incomplete combustion of hydrocarbons and produces carbon monoxide water and sometimes carbon and carbon dioxide

96
Q

Induced dipole dipole interactions

A

A type of intermolecular force close by temporary dipole is which causes all atoms and molecules to be attracted to each other

97
Q

Infrared spectroscopy

A

And analytical technique used to identify the functional groups present in a molecule by measuring the infrared absorption frequencies of its bonds

98
Q

Intermolecular forces

A

Forces between molecules

99
Q

Ionic bond

A

Electrostatic attraction between positive and negative ions

100
Q

Ionic equation

A

And equation which only shows the reacting particles of a reaction involving ions

101
Q

Ionisation

A

The removal of one or more electrons from an atom or molecule, resulting in an ion forming

102
Q

Isotopic abundance

A

The relative amount of a particular isotope occurring in a sample of an element

103
Q

Ketone

A

A substance with the general formula CnH2nO which has two alkyl groups attached to the carbonyl-carbon atom

104
Q

Lattice

A

A regular structure made of atoms or ions

105
Q

Mass number

A

The total number of protons and neutrons in the nucleus of an atom

106
Q

Mass spectrometry

A

And analytical technique used to find the structure of a molecule by measuring the masses of the ions it produces when it is bombarded with electrons

107
Q

Mass spectrum

A

A chart produced by a mass spectrometer

108
Q

Molar mass

A

Mass of one mole of something

109
Q

Molar ratio

A

Ratio of the number of moles in each reactant and product in a balanced chemical equation

110
Q

Mole

A

The unit of amount of substance

111
Q

Molecular formula

A

A way of representing molecules that shows the actual number of atoms of each element in a molecule

112
Q

Molecular ion

A

And I on made up of a group of atoms with an overall charge

113
Q

Monomer

A

A small molecule which is used to make a polymer

114
Q

Neutralisation reaction

A

A reaction between an acid and a base to produce a salt and water

115
Q

Noble gas

A

An element in group 0 of the periodic table. These elements are extremely stable because they have a full outer shell of electrons

116
Q

Nomenclature

A

Naming organic compounds

117
Q

Nucleophile

A

An electron-pair donor

118
Q

Nucleus

A

Central part of an atom ion only made up of protons and neutrons

119
Q

Orbital

A

Region of a sub shell that contains a maximum of two electrons with opposite spins

120
Q

Oxidation

A

Loss of electrons

121
Q

Oxidation number

A

The total number of electrons an element has donated or excepted

122
Q

Oxidising agent

A

Something that accepts electrons and gets reduced

123
Q

Percentage yield

A

Amount of product that is actually obtained during a reaction expressed as a percentage of the amount of product that should form

124
Q

Permanent dipole dipole interactions

A

Intermolecular forces that exist because the difference in electronegativity is in a polar bond causes week electrostatic forces of attraction between molecules

125
Q

Pi bond

A

A type of bond formed when 2P orbitals overlap sideways

126
Q

Polar bond

A

A true they don’t bond were difference in electronegativity has cause a shift in electron density in the bond

127
Q

Polar molecule

A

Emily still containing polar bonds that are arranged so that the dipoles don’t cancel each other out causing an overall dipole to be created across the molecule

128
Q

Polymer

A

A long molecule formed from lots of small molecules joined together

129
Q

Radical

A

A particle with an unpaired electron

130
Q

Redox reaction

A

A reaction where reduction and oxidation happen simultaneously

131
Q

Reducing agent

A

Something that donates electrons and gets oxidised

132
Q

Reduction

A

Gain of electrons

133
Q

Refluxing

A

Heating a reaction mixture in such a way that you boil it without losing volatile solvents reactants or products. Any vaporised compounds call condense and get back into the reaction mixture

134
Q

Relative atomic mass

A

The average mass of an atom Auger and elements compare to 1/12 of the mass of an atom of carbon 12

135
Q

Relative formula mass

A

The average mass of a molecule or formula unit compared to 1/12 of the mass of an atom of carbon 12

136
Q

Relative isotopic mass

A

The mass of an atom of an isotope of an element compared to 1/12 of the mass of an atom of carbon 12

137
Q

Relative molecular mass

A

The average mass of a molecule compared to 1/12 of the mass of an atom of carbon 12

138
Q

Salt

A

A compound formed when hydrogen in an acid molecule is replaced by a metal ion or ammonium ion

139
Q

Saturated hydrocarbon

A

A hydrocarbon where all the carbon carbon bonds are single bonds

140
Q

Sigma bond

A

Type of bond formed when two orbitals overlap directly between the bonded atoms

141
Q

Silver nitrate test

A

A test that uses silver nitrate to identified halide ions in the solution

142
Q

Simple molecular structure

A

A compound with strong covalent bonds with in its molecules but weak forces between is molecules

143
Q

Skeletal formula

A

A simplified organic formula which only shows the carbon skeleton and associated functional groups

144
Q

Specific heat capacity

A

The amount of heat energy it takes to raise the temperature of 1 g of given substance by 1K

145
Q

Spin

A

The type of momentum possessed by an electron spin can either be down or up

146
Q

Standard conditions

A

100kPa 298K

147
Q

Standard enthalpy change of combustion

A

The ends of the change one month one mole of substance is completely burned in oxygen under standard conditions we all reactants and products in their standard states

148
Q

Standard enthalpy change of formation

A

The Exelby change when one mole of a compound is formed from its elements in the standard states under standard conditions

149
Q

Standard entropy change of neutralisation

A

The answer will be change when an acid and alkali react together to form one mole of water under standard conditions

150
Q

Standard enthalpy change of reaction

A

The answer be change when a reaction occurs in the molar quantities shown in the chemical equation under standard conditions

151
Q

Stereoisomer

A

A molecule that has the same structural formula as another molecule but it’s atoms are arranged differently in space

152
Q

Strong acid or base

A

And acid or base that almost completely ionises in aqueous solution

153
Q

Structural formula

A

Away representing molecules that shows the items carbon by carbon with the attached hydrogens and functional

154
Q

Structural isomer

A

A molecule with the same molecular formula is another molecule but with the atoms connected in a different way

155
Q

Sub shell

A

The subdivision of an energy level subshells may be SPDF

156
Q

Substitution reaction

A

A reaction were some items from one react in a swap with atoms from another reactant

157
Q

Successive ionisation energy

A

The energy needed to remove one mole of each subsequent electron from each ion in one mole of positively charged gaseous ions

158
Q

Titration

A

A type of experiment used find the concentration of a solution that involves gradually adding one solution to a known volume of another until the reaction between the two is complete

159
Q

Unsaturated hydrocarbon

A

A hydrocarbon with one or more carbon to carbon double bond is carbon to carbon triple bonds or an aromatic group

160
Q

Van der Waals forces

A

Term referring to both and do you induced dipole dipole interactions and permanent dipole dipole interactions

161
Q

Volatility

A

Substances tendency to evaporate

162
Q

Water of crystallisation

A

The water contained in an ionic lattice

163
Q

Weak acid or base

A

Said or base that only slightly ionises in aqueous solution

164
Q

Yield

A

Amount products you get from a reaction

Chemistry OCR A (8 decks)

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