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Chemistry > PDG Definitions > Flashcards

PDG Definitions Flashcards

(69 cards)

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1
Q

Isotopes

A

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

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2
Q

Relative isotopic mass

A

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

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3
Q

Relative atomic mass

A

The weighted mean mass of atoms of an element compared with 1/12th mass of carbon-12

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4
Q

Relative molecular mass

A

The weighted mean mass of molecules of a compound compared with 1/12th mass of carbon-12

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5
Q

Relative formula mass

A

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

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6
Q

Amount of substance

A

The quantity of substance whose unit is the mole

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7
Q

Mole

A

One mole contains exactly 6.02 × 10²³ elementary entities

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8
Q

Avogadro constant

A

The number of particles per mole, 6.02 × 10²³ mol⁻¹

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9
Q

Molar mass

A

Mass per mole, units g mol⁻¹

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10
Q

Molar gas volume

A

Gas volume per mole, units dm³ mol⁻¹

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11
Q

Empirical formula

A

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

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12
Q

Molecular formula

A

The number and type of atoms of each element in a molecule

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13
Q

Anhydrous

A

Contains no water

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14
Q

Hydrated

A

Containing water molecules

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15
Q

Water of crystallisation

A

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

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16
Q

Acids

A

Substances that release H⁺ ions in aqueous solution

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17
Q

Alkalis

A

Substances that release OH⁻ ions in aqueous solution

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18
Q

Strong acid

A

An acid that dissociates completely

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19
Q

Weak acid

A

An acid that only dissociates partially in solution

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20
Q

Oxidation

A

Loss of electrons or increase in oxidation number

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21
Q

Reduction

A

Gain of electrons or decrease in oxidation number

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22
Q

Atomic orbital

A

A region around the nucleus that can hold up to 2 electrons with opposite spins

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23
Q

Ionic bonding

A

The electrostatic attraction between positive and negative ions

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24
Q

Covalent bond

A

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

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25
Electronegativity
The ability of an atom to attract the bonding electrons in a covalent bond
26
First ionisation energy
The energy required to remove 1 mole of electrons from 1 mole of gaseous atoms
27
Metallic bonding
The strong electrostatic attraction between cations and delocalised electrons
28
Disproportionation
A reaction in which the same species is both oxidised and reduced
29
Activation energy
The minimum energy required for a reaction to take place
30
Standard conditions
100kPa and a stated temperature, 298K
31
Standard states
The physical state under standard conditions
32
Enthalpy change of reaction
The enthalpy change associated with a stated equation
33
Enthalpy change of formation
The enthalpy change when 1 mole of a compound is formed from its elements in their standard states under standard conditions
34
Enthalpy change of combustion
The enthalpy change when 1 mole of a substance is completely burned in excess oxygen under standard conditions
35
Enthalpy change of neutralisation
The enthalpy change when an acid and alkali react to form 1 mole of water, under standard conditions
36
Average bond enthalpy
The average enthalpy change on breaking 1 mole of bonds in gaseous molecules
37
Catalyst
A substance that increases the rate of reaction without being used up, by allowing the reaction to proceed by an alternative route with a lower activation energy
38
Homogeneous catalyst
Catalyst in the same state as the reactants
39
Heterogeneous catalyst
Catalyst in a different state from the reactants
40
Dynamic equilibrium
An equilibrium that exists in a closed system when the rate of the forward reaction is equal to the rate of the backward reaction so the concentrations of the reactants and products do not change
41
General formula
The simplest algebraic formula of a homologous series
42
Structural formula
A formula showing the arrangement of atoms in a molecule
43
Displayed formula
A formula that shows all the atoms and bonds within a molecule
44
Skeletal formula
A simplified organic formula showing just the carbon skeleton and associated functional groups
45
Homologous series
A series of organic compounds having the same functional group but with each successive member differing by CH₂
46
Functional group
A group of atoms responsible for the characteristic reactions of a compound
47
Alkyl groups
A side chain
48
Aliphatic
Any non-aromatic organic compounds
49
Alicyclic
Any non-aromatic organic compounds containing a ring structure
50
Aromatic
Contains one or more benzene rings
51
Saturated
Contains single bonds only
52
Unsaturated
Containing multiple bonds
53
Structural isomers
Molecules with the same molecular formula but with a different structural formula
54
Radical
A species with an unpaired electron
55
Stereoisomers
Compounds with the same structural formula, but with a different arrangement in space
56
E/Z isomers
Stereoisomerism in which different groups attached to each carbon of a C=C double bond may be arranged differently in space due to the restricted rotation around the double bond
57
Cis-trans isomerism
A specific type of E/Z isomerism when there are two H atoms and two non-hydrogen groups on each carbon of the C=C double bond
58
Electrophile
An electron pair acceptor
59
Nucleophile
An electron pair donor
60
Rate of reaction
The change in concentration of a reactant or product over time
61
Buffer solution
A system that minimises pH changes on addition of small amounts of an acid or a base
62
Lattice enthalpy
The enthalpy change when 1 mol of ionic lattice is formed from gaseous ions
63
Enthalpy change of atomisation
The enthalpy change that takes place for the formation of one mole of gaseous atoms from the element in its standard state under standard conditions
64
1st electron affinity
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
65
Enthalpy change of solution
The enthalpy change when 1 mol of solute is dissolved
66
Enthalpy change of hydration
The enthalpy change when 1 mol of gaseous ions are dissolved in water
67
Entropy
The dispersal of energy and disorder within the chemicals making up a chemical system
68
Oxidising agent
A reagent that accepts electrons from another species
69
Reducing agent
A reagent that donates electrons to another species

Chemistry (1 decks)

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