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Chemistry A-Level James > A level Definitions > Flashcards

A level Definitions Flashcards

1
Q

Relative Isotopic Mass

A

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

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2
Q

Relative Atomic Mass (Ar)

A

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

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3
Q

Isotopes

A

Atoms of an element with the same number of protons but different number of neutrons.

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4
Q

Molar Mass

A

Mass per mole units g mol^-1

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5
Q

Mole

A

The amount of substance 1 mole is 6.02 x 10^23 particles

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6
Q

Acid

A

Releases H+ ion aqueous solution

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7
Q

Alkali

A

A soluble base that releases OH- ions in an aqueous solution.

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8
Q

Strong Acid

A

Fully dissociates in solution

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9
Q

Weak Acid

A

Partially dissociates in solution

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10
Q

Orbital

A

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

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11
Q

Disproportionation

A

Oxidation and reduction of the same element

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12
Q

First Ionisation Energy

A

The energy needed to remove 1 mole of electrons from 1 mole gaseous of atoms to form one mole of gaseous 1+ ions.

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13
Q

Ionic bonding

A

The electrostatic attraction between oppositely charged ions. (usually between a metal and non-metal)

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14
Q

Covalent Bonding

A

Strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms ( 2 non-metals)

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15
Q

Polar molecule

A

Compound has polar bonds with dipoles that do not cancel due to their direction

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16
Q

Metallic bonding

A

The electrostatic attraction between positively charged metal ions and the sea of delocalised electrons.

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17
Q

Electronegativity

A

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

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18
Q

Standard states

A

physical states under standard conditions

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19
Q

Standard conditions

A

Temperature: 298 kelvin Pressure: 100 KPa

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20
Q

Enthalpy change of formation

A

The enthalpy change when one mole of a compound is formed from its elements in their standard states

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21
Q

Enthalpy change of combustion

A

The enthalpy change for the complete combustion of one mole of a substance

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22
Q

Enthalpy change of neutralisation

A

The enthalpy change for the formation of 1 mol of water from a neutralisation reaction

23
Q

Activation energy

A

the minimum energy required for a reaction to take place

24
Q

Homologous Series

A

(a series of organic compounds having) the same functional group but with each successive member differing by CH2

25
Q

Structural isomers

A

Compounds with the same molecular formula but different structural formula

26
Q

Homolytic fission

A

Breaking a covalent bond to form two radicals

27
Q

Heterolytic fission

A

Breaking a covalent bond to form two oppositely charged ions

28
Q

E/Z isomerism

A

an example of stereoisomerism, due to restricted rotation about a double bond and two different groups attached to each carbon atom of the C=C group

29
Q

Cis-trans isomerism

A

A special case of E/Z isomerism in which two of the substituent groups attached to each carbon atom of the C=C group are the same

30
Q

Electrophile

A

An electron pair acceptor

31
Q

Nucleophile

A

An electron pair donor

32
Q

Homogeneous catalyst

A

A catalyst in the same state as the reactants (usually in solutions)

33
Q

Heterogeneous catalyst

A
  • A catalyst in a different state to the reactants (usually a solid catalyst with reactants in solution or gas)
34
Q

Dynamic equilibrium

A

When the rate of the forward reaction is equal to the rate of the reverse reaction and the concentrations of reactants and products do not change in a closed system

35
Q

Catalyst

A

Chemical that increases the rate of both forward and reverse reactions in an equilibrium by the same amount resulting in an unchanged position of equilibrium

36
Q

σ-bond

A

Overlap of orbitals directly between the bonding atoms

37
Q

π-bond

A

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

38
Q

Stereoisomerism

A

Compounds with the same structural formula but a different arrangement of atoms in space

39
Q

Curly arrow

A

Shows the movement of an electron pair during a reaction

40
Q

Rate of reaction

A

the rate at which the concentration of a reactant or product is formed/used

41
Q

Half-life

A

The time taken for the concentration of a reactant to half

42
Q

Rate-determining step

A

the slowest step in a multistep reaction

43
Q

Brønsted-Lowry acid

A

a species that donates a proton (H+)

44
Q

Brønsted-Lowry base

A

a species that accepts a proton (H+)

45
Q

Buffer solution

A

a system that minimises pH changes on addition of small amounts of an acid or a base

46
Q

Lattice Enthalpy

A

enthalpy change for the formation of 1 mole of ionic lattice from gaseous ions, ΔLEH

47
Q

Enthalpy change of solution

A

enthalpy change for dissolving of 1 mol of solute, ΔsolH

48
Q

Enthalpy change of hydration

A

enthalpy change for dissolving of 1 mol of gaseous ions in water, ΔhydH

49
Q

Oxidising agent

A

the chemical that is reduced and oxidises another species

50
Q

Reducing agent

A

the chemical that is oxidised and reduces another species

51
Q

Standard electrode (redox) potential, Eo

A

the voltage produced when a half cell is connected to a standard hydrogen half-cell, measured at 298K with solution concentrations of 1 mol dm^-3 and a gas pressure of 100KPa.

52
Q

Ligand

A

species that donates a pair of electrons forming a coordinate/dative covalent bond to a metal ion

53
Q

Optical isomer

A

non-superimposable mirror images about a chiral centre

Chemistry A-Level James (7 decks)

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