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Chemistry A-Level > Definitions ALL > Flashcards

Definitions ALL Flashcards

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1
Q

First ionisation energy

A

Enthalpy change when one mole of electrons are removed from one mole of gaseous atoms

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2
Q

Relative atomic mass

A

Average mass of an atom, relative to 1/12th the mass of the carbon-12 isotope

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3
Q

Empirical formula

A

Simplest ratio of elements in a compound

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4
Q

Relative molecular mass

A

Average mass of a molecule, relative to 1/12th the mass of the carbon-12 isotope

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5
Q

Atom economy

A

Molecular mass of desired product/sum of molecular masses of all reactants

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6
Q

Dative bonding

A

Bonding where one atom provides both of an electron pair to another atom

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7
Q

Electronegativity

A

The power of an atom to attract the bonded pair of electrons toward itself

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8
Q

Enthalpy change

A

Energy change under constant pressure

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9
Q

Standard conditions

A

298K and 100kPa

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10
Q

Standard enthalpy of formation

A

Enthalpy change when one mole of a compound is formed from its constituent elements under standard conditions

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11
Q

Standard enthalpy of combustion

A

Enthalpy change when one mole of a compound is burned completely in excess oxygen under standard conditions

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12
Q

Hess’ Law

A

Enthalpy change is constant, regardless of the path taken

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13
Q

Bond dissociation enthalpy

A

Enthalpy change when one mole of a bond is broken to give gaseous atoms

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14
Q

Mean bond enthalpy

A

Enthalpy change when one mole of a bond is broken, averaged over different compounds

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15
Q

Activation energy

A

Energy required for a reaction to occur

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16
Q

Catalyst

A

A chemical that speeds up a reaction by providing a different pathway with a lower activation energy

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17
Q

Dynamic equilibrium

A

Forward rate = Backward rate. Moles of reactants and products are constant

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18
Q

Disproportionation

A

A reaction in which a substance is simultaneously oxidised and reduced

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19
Q

Homologous series

A

A family of hydrocarbons with similar chemical properties who share the same general formula

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20
Q

Structural isomerism

A

Same molecular formula but different structural formula

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21
Q

Stereoisomerism

A

Same structural formula but different spacial arrangement

22
Q

Nucleophile

A

Lone pair donor

23
Q

Electrophile

A

Lone pair acceptor

24
Q

Standard enthalpy of atomisation

A

Enthalpy change when one mole of gaseous atoms are formed under standard conditions

25
Q

First electron affinity

A

Enthalpy change when one mole of electrons are added to one mole of gaseous atoms

26
Q

Lattice enthalpy of formation

A

Enthalpy change when one mole of a solid ionic compound is formed from its gaseous ions

27
Q

Lattice enthalpy of dissociation

A

Enthalpy change when one mole of a solid ionic compound is dissociated into its gaseous ions

28
Q

Enthalpy of hydration

A

Enthalpy change when water molecules surround one mole of gaseous ions

29
Q

Enthalpy of solution

A

Enthalpy change when one mole of solute dissolves completely to form a solution where the ions are far enough apart that they don’t interact

30
Q

Hydration

A

When ions are surrounded by water molecules

31
Q

Entropy

A

Measure of randomness of a reaction

32
Q

Order of reaction

A

The power of the concentration of the molecule in the rate equation

33
Q

Rate-determining step

A

Slowest step in a reaction

34
Q

Salt bridge

A

Filter paper soaked in a solution to allow ions to pass and complete the circuit

35
Q

Bronsted-Lowry acid

A

Proton donor

36
Q

Bronsted-Lowry base

A

Proton acceptor

37
Q

Weak acid

A

Acid that has a very low degree of dissociation.

38
Q

Equivalence point

A

The point in titration where enough acid or alkali has been added to neutralise the solution

39
Q

Buffer

A

A solution that can resist changes in pH

40
Q

Transition metal

A

Metals found in the d-block and with partially filled d-orbitals

41
Q

Ligand

A

Molecules that have a lone pair of electrons, available to form a dative bond with a metal ion

42
Q

Complex ion

A

An ion made with a metal ion datively bonded with one or more ligands

43
Q

Chiral centre

A

A carbon atom bonded to 4 different groups

44
Q

Pair of enantiomers

A

Two isomers showing optical isomerism

45
Q

Optical isomerism

A

Pairs of molecules which differ in the way they rotate polarised light; contains chiral carbons

46
Q

Racemic mixture

A

A mixture of a pair of enantiomers, causing no rotation on a plane of polarised light

47
Q

Fatty acids

A

Carboxylic acids found in oils and fats

48
Q

Acid derivatives

A

Compounds containing the acyl group in the structure

49
Q

Hydrolysis

A

Breakdown of a molecule using water

50
Q

Inductive effect

A

Unequal sharing of the bonding electron pair between atoms

Chemistry A-Level (34 decks)

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