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Computing + definitions for chem > A Level Chemistry Definitions > Flashcards

A Level Chemistry Definitions Flashcards

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1
Q

Isotopes

A

Atoms of the same element with different numbers of neutrons and different mass numbers.

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2
Q

Relative Isotopic Mass

A

The mass of an isotope compared with 1/12 of the mass of an atom of carbon-12.

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3
Q

Relative Atomic Mass

A

The weighted mean mass of an atom compared with 1/12 of the mass of an atom of carbon-12.

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4
Q

Mole

A

The amount of substance that contains 6.02 x 10^23 (Avogadro’s number) particles.

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5
Q

Empirical Formula

A

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

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6
Q

Molecular Formula

A

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

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7
Q

Anhydrous

A

A compound that doesn’t contain any water of crystallisation.

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8
Q

Hydrated

A

A compound that contains water(s) of crystallisation.

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9
Q

Water Of Crystallisation

A

Water molecules that form an essential part of a compound’s crystalline structure.

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10
Q

Acid

A

A substance that releases H+ ions in aqueous solution.

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11
Q

Alkali

A

A substance that releases OH- ions in aqueous solution.

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12
Q

Weak Acid

A

An acid that partially dissociates in solution.

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13
Q

Strong Acid

A

An acid that fully dissociates in solution.

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14
Q

Orbital

A

A region around the nucleus that can hold up to 2 electrons in opposite spin.

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15
Q

Ionic Bonding

A

Electrostatic attraction between oppositely charged ions.

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16
Q

Covalent Bonding

A

Electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms.

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17
Q

Dative Bond

A

A covalent bond where both of the shared electrons are donated by one of the bonding atoms.

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18
Q

Electronegativity

A

The ability of an atom to attract a shared pair of electrons in a covalent bond.

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19
Q

Periodicity

A

Repeating trends in physical/chemical properties across periods of the periodic table.

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20
Q

First Ionisation Energy

A

The amount of energy required to remove one mole of electrons from one mole of gaseous atoms in order to form one mole of gaseous 1+ ions.

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21
Q

Metallic Bonding

A

Electrostatic attraction between metal cations and delocalised electrons.

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22
Q

Disproportionation

A

Oxidation and reduction of the same element in a reaction.

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23
Q

Exothermic

A

More energy is released forming bonds than energy taken in breaking bonds.

24
Q

Endothermic

A

More energy is taken in breaking bonds than energy released forming bonds.

25
Q

Enthalpy

A

A measurement of the amount of thermal energy within a system.

26
Q

Activation Energy

A

The minimum amount of energy a particle needs in order to react.

27
Q

Enthalpy Change Of Formation

A

The enthalpy change when forming one mole of a compound from its elements in their standard states under standard conditions.

28
Q

Enthalpy Change Of Combustion

A

The enthalpy change when one mole of substance undergoes complete combustion/reacts with excess oxygen under standard conditions.

29
Q

Enthalpy Change Of Neutralisation

A

The enthalpy change when one mole of water is formed by an acid and an alkali under standard conditions.

30
Q

Average Bond Enthalpy

A

The amount of energy required to break 1 mole of bonds in gaseous molecules.

31
Q

Catalyst

A

A substance that increases the rate of reaction without being used up in the overall reaction by providing an alternative reaction pathway with a lower activation energy.

32
Q

Homogeneous Catalyst

A

Catalyst in the same state as the reactants.

33
Q

Heterogeneous Catalyst

A

Catalyst in a different state to the reactants.

34
Q

Dynamic Equilibrium

A

A closed system where the rate of the forward reaction is equal to the rate of the reverse reaction.

35
Q

Homologous Series

A

A series of organic compounds with the same functional group where each successive member differs by CH2.

36
Q

Functional Group

A

The group of atoms responsible for the characteristic reactions of a compound.

37
Q

Aliphatic Compound

A

A compound containing C/H atoms joined together in straight/branched chains or non-aromatic rings.

38
Q

Alicyclic Compound

A

An aliphatic compound arranged in a non-aromatic ring.

39
Q

Aromatic Compound

A

A compound that contains a benzene ring.

40
Q

Unsaturated

A

Contains a C=C or C≡C or benzene ring.

41
Q

Saturated

A

Doesn’t contain any C=C or C≡C bonds.

42
Q

Structural Isomers

A

Compounds with the same molecular formula but different structural formulae.

43
Q

Stereoisomers

A

Compounds with the same structural formula but different spatial arrangements.

44
Q

Homolytic Fission

A

The breaking of a covalent bond where each bonded atom receives 1 electron from the shared pair forming 2 radicals.

45
Q

Heterolytic Fission

A

The breaking of a covalent bond where one of the bonded atoms receives both electrons from the shared pair.

46
Q

Radical

A

A species that contains an unpaired electron.

47
Q

Electrophile

A

A species that accepts a pair of electrons in order to form a covalent bond.

48
Q

Nucleophile

A

A species that donates a pair of electrons in order to form a covalent bond.

49
Q

Pi Bond Formation

A

Sideways overlap of adjacent p-orbitals above and below the bonding carbon atoms.

50
Q

E/Z Isomerism

A

Stereoisomerism caused by the restricted rotation around a C=C double bond when there are 2 different groups attached to each of the carbon atoms.

51
Q

Cis-Trans Isomerism

A

A special case of E/Z isomerism in which there is an identical group attached to both carbon atoms of the C=C bond.

52
Q

Standard Conditions

A

298K & 101KPa

53
Q

SI Volume
SI Pressure
SI Temperature
SI Mass

A

m^3
Pa
K
Kg

54
Q

Lattice enthalpy

A

The energy released when 1 mole of an ionic compound is formed from its constituent ions in their gaseous state under standard conditions.

55
Q

enthalpy change of solution

A

The enthalpy change that takes place when 1 mole of a solute is completely dissolved in water under standard conditions.

56
Q

enthalpy change of hydration

A

The energy released when 1 mole of gaseous ions are dissolved in water under standard conditions.

57
Q

entropy

A

A measure of the dispersal of energy within a system.

Computing + definitions for chem (20 decks)

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