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Chemistry > Definitions for CER > Flashcards

Definitions for CER Flashcards

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0
Q

Define: saturated hydrocarbon

A

A hydrocarbon with single bonds only

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1
Q

Define: Hydrocarbon

A

An organic compound that contains only hydrogen and carbons

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2
Q

Define: unsaturated hydrocarbon

A

A hydrocarbon containing at least one carbon-carbon double bond

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3
Q

Define: Homologous series

A

Is an organic series with the same functional group but with each member differing by CH2

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4
Q

Define: functional group

A

Is part of an organic molecule responsible for its chemical properties

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5
Q

Define: Alkane

A

The homologous series without double bonds and the general formula
CnH2n+2

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6
Q

Define: Alkene

A

They Homologous series with the double bond and the general formula
CnH2n

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7
Q

Define: displayed formula

A

Shows the relative position of all atoms in the molecule and the bonds between them

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8
Q

Define: structural formula

A

Shows minimal detail of the arrangement of atoms in the molecule

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9
Q

Define: Skeletal formula

A

Four minute with hydrogen atoms removed and only the bonds between carbon atoms show, not the atoms themselves

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10
Q

Define: structural isomers

A

Isomer with the same molecular formula but different structural formula

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11
Q

Define: positional isomerism

A

A type of structural isomerism. When a functional group is on a different numbered carbon

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12
Q

Define: chain Isomerism

A

A type of structural isomerism where branches occur in a chain

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13
Q

Define: stereoisomers

A

Isomers with the same structural formula but a different arrangement in space around a double bond

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14
Q

Define: E/Z isomers

A

A type of stereoisomerism. Double bond stops rotation and different groups on the carbons on the double bond

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15
Q

Define: Homolytic fission

A

When a covalent bond breaks giving an electron to two atoms making two radicals

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16
Q

Define: heterolytic fission

A

The breaking of a covalent bond with both of the bonded electrons going to one of the atoms forming a cation (-ve) and an anion (+ve)

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17
Q

Define: radical

A

Series with an unpaired electron

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18
Q

Define: nucleophile

A

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

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19
Q

Define: Electrophile

A

(Electron loving) an electron pair acceptor

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20
Q

Define: addition reaction

A

When a species adds to another species. Requires a double bond

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21
Q

Define: substitution reaction

A

When a species replaces another species in a reaction

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22
Q

Define: elimination reaction

A

When a molecule is removed from another molecule making a double bond

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23
Q

Define: nucleophilic substitution

A

A type of substitution reaction in which a nucleophile is attracted to an electron-deficient centre or atom, where it donates a pair of electrons to form a new covalent bond

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24
Q

Define: free radical substitution

A

When a halogen replaces an H in a reaction three steps initiation, propagation, termination

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25
Q

Define: electrophilic addition

A

When a species adds across a double bond

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26
Q

Define: fractional distillation

A

When crude oil is split into its components by their boiling points

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27
Q

Define: cracking

A

When a long chain alkane is split into a short chain alkanes and an Alkene

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28
Q

Define: combustion

A

When a compound is burned completely in oxygen to form Carbon dioxide and water

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29
Q

Define: incomplete combustion

A

When a compound burned in oxygen to form carbon, or carbon monoxide and water

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30
Q

Define: pi bond

A

Formed by the sideways overlap of adjacent P orbitals - always use diagram

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31
Q

Define: polymer

A

Long chain of monomers

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32
Q

Define: monomer

A

Small monomer, usually an alkene, used to build up a polymer

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33
Q

Define: oxidation

A

Loss of electrons or an increase in oxidation number

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34
Q

Define: oxidising agent

A

A reagent that oxidises (takes electrons from) another species e.g. Acidified potassium dichromate

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35
Q

Define: reflux

A

The continual boiling and condensing of the reaction mixture to ensure that the reaction takes place without the contents of the flask boiling dry. Used to make primary alcohols into carboxylic acids or secondary alcohols into ketones

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36
Q

Define: distillation

A

Used to make primary alcohols into aldehydes or secondary alcohols into ketones

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37
Q

Define: ester

A

Formed when an alcohol and carboxylic acid react. -(C=O)-O-(CH2)-

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38
Q

Define: percentage yield

A

Found by (actual amount in moles of product/theoretical amount in moles of product) x100

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39
Q

Define: Atom economy

A

(Mr of the desired product/Mr of all products) X 100

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40
Q

Define: IR Spectra

A

Shows the absorption of IR radiation by bonds to show what bonds are present in a sample

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41
Q

Define: mass spectrometry

A

Shows the mass/charge for fragments of a molecule

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42
Q

Define: MS fragment

A

A piece of the molecule broken in mass spectrometry allows us to piece together the starting molecule

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43
Q

Define: Enthalpy (H)

A

The heat energy stored in a chemical system

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44
Q

Define: Exothermic

A

When the enthalpy is smaller at the end of a reaction than at the beginning. Resulting in heat loss. Bond making. Delta negative

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45
Q

Define: endothermic

A

When the waiter at the end of a reaction then at the beginning. Resulting in him being taken in. Bond breaking. Delta positive

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46
Q

Define: activation energy (Ea)

A

Minimum energy required to start a reaction by the breaking of Bonds

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47
Q

Define: Enthalpy profile diagram

A

Shows the enthalpy of the reactants and products along with the activation energy and Enthalpy change

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48
Q

Define: standard conditions

A

Pressure of 100 KPa and a temperature of 298K. In solution concentration of 1M

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49
Q

Define: standard state

A

The state we find a substance in under standard conditions

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50
Q

Define: standard enthalpy change of reaction

A

Is the enthalpy change that accompanies a reaction of 1 mol of reactants on the standard conditions and in standard states

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51
Q

Define: standard enthalpy change of combustion

A

Is the enthalpy change when one mole of reactant is burned completely in oxygen under standard conditions

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52
Q

Define: standard enthalpy change of formation

A

Is the enthalpy change when one mole of product is formed from its constituent elements in standard states under standard conditions

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53
Q

Define: specific heat capacity (C)

A

Energy required to heat 1g of substance by 1K

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54
Q

Define: bond enthalpy

A

Is the enthalpy change when one mole of a given bonds is broken by home and lytic vision in a gassious state

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55
Q

Define: Hess’s Law

A

“If a reaction can take place by more than one late and the little and final conditions are the same, the total involve be changed is the same for each route.”

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56
Q

Define: rate of reaction

A

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

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57
Q

Define: catalyst

A

A species that lowers the activation energy of the reaction by providing an alternative route but is not used itself

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58
Q

Define: Boltzmann distribution

A

Is the distribution of energies of molecules within the sample at a given temperature

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59
Q

Define: dynamic equilibrium

A

An equilibrium in a closed system where the rate for the reaction equals that of the reverse reaction leaving constant concentration of Products and reactants

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60
Q

Define: Le Chatelier’s principle

A

When change is imposed on the system in dynamic equilibrium the position of the equilibrium will change to minimise the change

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61
Q

Define: the greenhouse effect

A

The process by which absorption and subsequent emission of infrared radiation by atmospheric gases warms the lower atmosphere and the planets surface

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62
Q

Define: Troposphere

A

Lowest layer of atmosphere surface between 7 km and 20 km

63
Q

Define: stratosphere

A

Second layer of atmosphere contains ozone layer. From 20 km to 50 km

64
Q

Define: adsorption

A

Process by which a gas, liquid or solute is held to a solid surface - such as in the catalytic converter

65
Q

Define: acid

A

The species that is a proton donor

66
Q

Define: addition polymer

A

Molecular chain forward by repeated addition reactions of many unsaturated alkene molecules (monomers)

67
Q

Define: addition polymerisation

A

The process in which unsaturated alkene molecules (monomers) add onto a growing polymer chain one of the time to form a very long saturated molecular chain (the addition polymer)

68
Q

Define: alicyclic hydrocarbon

A

A hydrocarbon with carbon atoms joined together in a ring structure

69
Q

Define: aliphatic hydrocarbons

A

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

70
Q

Define: alkali

A

A type of bass that dissolves in water forming hydroxide ions, OH- ions

71
Q

Define: alkyl group

A

And alkane with a hydrogen atom removed, E.g. CH3, C2H5; alkyl groups are often shown as R

72
Q

Define: amount of substance

A

The quantity whose unit of the mole. Chemists use amount of substance as a means of counting atoms

73
Q

Define: anhydrous

A

A substance that contains no water molecules

74
Q

Define: anion

A

And negatively charged ion

75
Q

Define: atomic orbital

A

A region within an atom that can hold up to 2 electrons, with opposite spins

76
Q

Define: atomic (proton) number

A

The number of protons in the nucleus of an atom

77
Q

Define: Avogadro’s constant

A

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

78
Q

Define: base

A

A species that is a proton acceptor

79
Q

Define: biodegradable material

A

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

80
Q

Define: carbanion

A

And organic Ion in which a carbon atom has a negative charge

81
Q

Define: cation

A

A positively charged ion

82
Q

Define: cis-trans isomerism

A

A special type of E/Z isomerism in which there is a non-hydrogen group and the hydrogen atoms on each C of a C=C double bond: the cis isomer (Z isomer) has the H atoms on each carbon on the same side; the trans-isomer (E) has the H atoms on each carbon on different sides of the bond

83
Q

Define: compound

A

A substance formed from two or more chemically bonded elements in a fixed ratio, usually shown by chemical formula

84
Q

Define: concentration

A

The amount of solute, in mol, per 1dm³ (1000 cm³) of solution

85
Q

Define: coordinate bond

A

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

86
Q

Define: covalent bond

A

A bond formed by a shared pair of electrons

87
Q

Define: Curly arrows

A

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

88
Q

Define: dative covalent

A

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

89
Q

Define: dehydration

A

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

90
Q

Define: delocalised electrons

A

Electrons are shared between more than two atoms

91
Q

Define: displacement reaction

A

A reaction in which a more reactive element replaces a less reactive element from an aqueous solution of the latter’s ions

92
Q

Define: disproportionation

A

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

93
Q

Define: electron configuration

A

The arrangement of electrons in an atom in

94
Q

Define: electronegativity

A

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

95
Q

Define: electron shielding

A

There are potion between electrons in different in the shells. The shielding reduces the net attractive force from the positive nucleus on the outer shell electrons

96
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’ Law

97
Q

Define: giant covalent lattice

A

A three-dimensional structure of atoms, bonded together by strong covalent bonds

98
Q

Define: giant ionic lattice

A

A three-dimensional structure of oppositely charged ions, bonded together by strong ionic bonds

99
Q

Define: giant metallic lattice

A

A three-dimensional structure of positive ions and delocalised electrons bonded together by strong metallic bonds

100
Q

Define: group

A

Vertical column in the periodic table. Elements in group have similar chemical properties and the atoms have the same number of outer shell electrons

101
Q

Define: heterogeneous catalysis

A

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

102
Q

Define: 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

103
Q

Define: hydrated

A

Crystalline and containing water molecules

104
Q

Define: hydrogen bond

A

A strong dipole-dipole attraction between electron-deficient hydrogen atom (O-H[Delta +ve] or N-H[Delta +ve]) on one molecule and lone pair of electrons on the highly electronegative atom (H-O:[Delta -ve] or H-N:[delta-ve]) on a different molecule

105
Q

Define: hydrolysis

A

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

106
Q

Define: initiation

A

The first step in a radical substitution in which the free radicals are generated by ultraviolet radiation

107
Q

Define: intermolecular force

A

An attractive force between neighbouring molecules. Intermolecular forces can be van der Waals’ forces (induced dipole-dipole forces), permanent dipole-dipole forces or hydrogen bonds

108
Q

Define: Ion

A

Are positively or negatively charged atom (covalently bonded) or group of atoms (a molecular ion)

109
Q

Define: ionic bonding

A

The electrostatic attraction between oppositely charged ions

110
Q

Define: first ionisation energy

A

The energy required to remove one electron from each eye on it one mole of gaseous 1+ ions to form one mole of gaseous 2+ ions

111
Q

Define: (second) ionisation energy

A

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

112
Q

Define: (successive) ionisation

A

A measure of the energy required to remove each electron in turn

113
Q

Define: energy

A

E.g. the second ionisation energy is the energy required to remove one electron from each ion in one mole of gaseous 1+ ions to form one mole of gaseous 2+ ions

114
Q

Define: isotope

A

Atoms of the same element with different numbers of neutrons and different masses

115
Q

Define: limiting reagent

A

The substance in a chemical reaction the runs out first

116
Q

Define: lone pair

A

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

117
Q

Define: mass (nucleon) number

A

The number of particles (proton and neutron is) in the nucleus

118
Q

Define: mechanism

A

A sequence of steps showing the path taken by electrons in a reaction

119
Q

Define: metallic bond

A

The electrostatic attraction between positive metal ion is delocalised electrons

120
Q

Define: molar mass, M

A

The mass mole of a substance. The units of molar mass are gmol^-1

121
Q

Define: molar volume

A

The volume per mole of gas. Units of molar volume are dm³mol^-1. At room temperature and pressure at the mole volume is approximately
24dm³mol^-1

122
Q

Define: Mole

A

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

123
Q

Define: molecular formula

A

The number of atoms of each element In a molecule

124
Q

Define: Molecular ion, M+

A

The positive ion formed in mass spectrometry when a molecule loses an electron

125
Q

Define: molecule

A

A small group of atoms held together by covalent bonds

126
Q

Define: Oxidation number

A

A measure of the number of electrons does an atom uses the bond with atoms of another element. Oxidation numbers are derived from a set of rules

127
Q

Define: period

A

Horizontal row of elements in the periodic table. Element show trends in properties across a period

128
Q

Define: periodicity

A

A regular periodic variation of properties of elements with atomic number and position in the periodic table

129
Q

Define: permanent dipole

A

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

130
Q

Define: permanent dipole-dipole force

A

An attractive force between permanent dipoles in neighbouring polar molecules

131
Q

Define: polar covalent bond

A

A bond with a permanent dipole

132
Q

Define: polar molecule

A

A molecule with an overall dipole, taking into account any dipoles across bonds

133
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

134
Q

Define: principal quantum number, n

A

A number representing the relative overall energy of each orbital, which increases with distance from the nucleus. The sets of orbitals with the same n value are referred to as electron shells or energy levels

135
Q

Define: propagation

A

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

136
Q

Define: redox reaction

A

A reaction in which both reduction and oxidation take place

137
Q

Define: reducing agent

A

A reagent that reduces (adds electron to) another species

138
Q

Define: reduction

A

Gain of electrons or a decrease in oxidation number

139
Q

Define: relative atomic mass, Ar

A

The weighted mean mass of an atom of an element compare to 1/12 of the mass of an atom of carbon-12

140
Q

Define: relative formula mass

A

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

141
Q

Define: relative isotopic mass

A

The mass of an atom of an isotope can paired with 1/12th of the mass of an atom of carbon 12

142
Q

Define: relative molecular mass, Mr

A

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

143
Q

Define: repeat unit

A

The specific arrangement of atoms that occurs in the structure over and over again. Repeated units are included in brackets, outside of which is the symbol n

144
Q

Define: salt

A

A chemical compound formed from an acid, when an H + ion from the acid has been replaced by metal ion or another positive ion, such as the ammonium ion, NH4+

145
Q

Define: shell

A

A group of atomic orbitals with the same principal quantum number, n. Also known as the main energy level

146
Q

Define: simple molecular lattice

A

Three-dimensional structure of molecules, bonded together by weak intermolecular forces

147
Q

Define: species

A

Any type of particle that takes part in a chemical reaction

148
Q

Define: standard solution

A

A solution of known concentration. Standard solutions are normally used in titrations to determine unknown information about another unknown substance

149
Q

Define: stoichiometry

A

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

150
Q

Define: sub-shell

A

A group of the same type of atomic orbitals (S, P, D or F) within a shell

151
Q

Define: termination

A

The step at the end of a radical substitution went to radicals combine to form a molecule

152
Q

Define: thermal decomposition

A

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

153
Q

Define: van Der Waals forces

A

Very weak attractive forces between induced dipoles in neighbouring molecules

154
Q

Define: volatility

A

The ease that a liquid turned into a gas. Volatility increases as boiling point decreases

155
Q

Define: water of crystallisation

A

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

Chemistry (4 decks)

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