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Chemistry A2 > Paper 5 > Flashcards

Paper 5 Flashcards

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0
Q

Rate =

A

k[A]m[B]n

Can on,y be determined practically by experiment

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1
Q

Rate of reaction

A

The change in conc of a reactant or product per unit time

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2
Q

Overall order

A

M+n

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3
Q

Half life

A

The time taken for the concentration of a reactant to reduce by half

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4
Q

Initial rate

A

The rate right at the start of a reaction (t=0)

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5
Q

Rate determining step

A

The slowest step in the mechanism of a multi-step reaction

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6
Q

An intermediate

A

Used up in one step of the reaction and formed in a subsequent step. Not seen as a product or reactant in the overall equation.

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7
Q

Kc=

A

[prod]/[react]

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8
Q

pH=

A

-log[H+]

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9
Q

pKa=

A

-logKa

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10
Q

[H+]=

A

10^-pH

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11
Q

Ka=

A

10^-pKa

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12
Q

Ionic product of water (Kw)

A

Kc = [H+][OH-]/[H2O]
Eq to left so v small
Kc x [H2O] = Kw = [H+][OH-]

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13
Q

Buffer

A

A solution able to oppose changes in pH when small quantities of acid or base are added
(Weak acid and conjugate base)

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14
Q

Enthalpy of neutralisation

A

The enthalpy change when an aqueous acid reacts with an aqueous base to form 1 mole of water under standard conditions (100kPa, 298K)

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15
Q

Equivalence point

A

The point in a titration at which the volume of one solution has reacted exactly with the volume of the second solution matching the stoichiometric of the reaction

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16
Q

Hess’ Law

A

States that if a reaction can take place by more that one route and the initial and final conditions and the same, the total enthalpy change is the same for each route.

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17
Q

Lattice enthalpy (LE)

A

The enthalpy change when 1 mole of a solid ionic compound is formed from its gaseous ions under standard conditions (298K, 100kPa).
e.g. K+(g) + Cl-(g) ➡️ KCl(s)

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18
Q

Standard enthalpy change of formation (

A

The enthalpy change when 1 mole of a compound is formed from its constituent elements in their standard States under standard conditions (298K, 100kPa)
e.g. K(s) + 1/2Cl2(g) ➡️ KCl(s)
-

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19
Q

Standard enthalpy change of atomisation (

A

The enthalpy change when 1 mole of gaseous atoms forms from the elements in their standard states under standard conditions (298K, 100kPa)
e.g. 1/2Cl2(g) ➡️ Cl(g)
+

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20
Q

First ionisation energy (

A

The enthalpy change when 1 electron is removed from each atoms in 1 mole of gaseous atoms to form 1 mole of gaseous 1+ ions.
e.g. Cl(g) ➡️ Cl+(g) + e-

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21
Q

Second ionisation energy (

A

The enthalpy change when 1 electron is removed from each ion in 1 mole of 1+ gaseous ions to form 1 mole of gaseous 2+ ions.
e.g. Ca+(g) ➡️ Ca2+(g) + e-

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22
Q

First electron affinity (

A

The enthalpy change when 1 electron is added to each atom in 1 mo,e of gaseous atoms forming 1 mole of gaseous 1- ions.
e.g. Cl(g) + e- ➡️ Cl-(g)
-

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23
Q

Second electron affinity (

A

The enthalpy change when 1 electron is added to each ion in 1 mole of gaseous 1- ions forming 1 mole of gaseous 2- ions.
e.g. O-(g) + e- ➡️ O2-(g)
+

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24
Q

Born-Haber cycles

A

Used to calculate enthalpy change that cannot be measured direct,y.

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25
Q

Standard enthalpy change of solution (

A

The enthalpy change when 1 mole of a compound is fully dissolved in water under standard conditions (298K, 100kPa)
e.g. KCl(s) ➡️ K+(aq) + Cl-(aq)
+/-

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26
Q

Standard enthalpy change of hydration (

A

The enthalpy change when 1 mole of aqueous ions are formed from gaseous ions under standard conditions (298K, 100kPa).
e.g. K+(g) + aq ➡️ K+(aq)
+

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27
Q

Standard entropy change of a reaction (

A

The entropy change of a reaction in the molar quantities expressed in th equation under standard conditions (298K, 100kPa) in standard States.

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28
Q

Standard entropy of a substance (S⚪️)

P

A

The entropy content of 1 mole of a substance under standard conditions (298K, 100kPa).

29
Q
A

sum of products - sum of reactants

30
Q

The overall energy or Gibb’s free energy of a system (G)

A

Results from the contributions of both enthalpy and entropy

31
Q
A
32
Q

Oxidation

A

The gain of oxygen or hydrogen, the loss of electrons or the increase in oxidation number.

33
Q

Reduction

A

The loss of oxygen or hydrogen, the gain of electrons or the decrease in oxidation number.

34
Q

Oxidation number of elements

A

0

35
Q

Oxidation number of combined group 1 atoms

A

+1

36
Q

Oxidation number of combined group 2 atoms

A

+2

37
Q

Oxidation number of aluminum

A

+3

38
Q

Oxidation number of hydrogen

A

+1

39
Q

Oxidation number of flourine

A

-1

40
Q

Oxidation number of oxygen

A

-2

41
Q

Oxidation number of chlorine, bromine and iodine

A

-1

42
Q

Order of priority of oxidation numbers

A 
Elements 0
Group 1 +1
Group 2 +2
Aluminium +3
Hydrogen +1
Flourine -1
Oxygen -2
Cl, Br, I -1
43
Q

Standard electrode potential of a half cell (E⚪️)

A

The electromotive force (e.m.f.) of a half cell compared with a standard hydrogen half cell, measured at 298K with solution concentrations of 1 moldm-3 and a gas pressure of 100kPa (1 atmosphere).

44
Q

Transition metal

A

A d-block element that forms at least one ion with an incomplete d sub-shell.

45
Q

Precipitation reaction

A

2 solutions mixed together to produce an insoluble product

46
Q

Copper (II) hydroxide precipitation reaction

A

Cu2+(aq) + 2OH-(aq) ➡️ Cu(OH)2(s)

Cu2+ pale blue ➡️ pale blue precipitate (beige in air)

47
Q

Cobalt (II) hydroxide precipitation reaction

A

Co2+(aq) + 2OH-(aq) ➡️ Co(OH)2(s)

Co2+ pink ➡️ blue precipitate

48
Q

Iron (II) hydroxide precipitation reaction

A

Fe2+(aq) + 2OH-(aq) ➡️ Fe(OH)2(s)

Fe2+ pale green ➡️ green precipitate (rusty-brown in air)

49
Q

Iron (III) hydroxide precipitation reaction

A

Fe3+(aq) + 3OH-(aq) ➡️ Fe(OH)3

Fe3+ pale yellow ➡️ rusty-brown precipitate

50
Q

Complex ion

A

A central transition metal ion bonded to one or more Luganda by coordinate bonds (dative covalent bonds).

51
Q

Ligand

A

An ion, molecule or atom with a lone pair of electrons that can be donated to a transition metal to form a coordinate bond.

52
Q

Co-ordination number

A

The total number of coordinate bonds between a central metal ion and its ligands.

53
Q

Monodentate ligand

A

A ligand that donates one pair of electrons to the central metal ion

54
Q

A bidentate ligand

A

Donates two lone pairs of electrons to the central transition metal ion, forming two co-ordinate bonds.

55
Q

Shape of 6 co-ordinate bonds?

A

Octahedral

90 degrees

56
Q

4 co-ordinate bonds shape?

A

Tetrahedral - 109.5 degrees

For nickel, palladium or platinum - 90 degrees

57
Q

Ligand substitution

A

A reaction in which one ligand in a complex ion is replaced by another ligand.

58
Q

Cis-trans isomerism

A

Cis - 90 degrees

Trans - 180 degrees

59
Q

Optical isomerism

A

Non-superimposable mirror images that rotate plane polarised by equal amounts in opposite directions.
Have no plane of symmetry.

60
Q

Cis-platin

A

[PtCl2(NH3)2]

An anti-can we drug that binds to cancer cells’ DNA and prevents division as it alters the structure.

61
Q

Stability constant

A

The equilibrium constant for the formation of the complex ion from its constituent ions

62
Q

Kstab=

A

[products]/[formation]
Ignoring water
Large = equilibrium to right = more stable

63
Q

Hydrogen fuel cell equations

A

H2 ➡️ 2H+ + 2e-
1/2O2 + 2H+ + 2e- ➡️ H2O

2H2 + O2 ➡️ 2H2O

64
Q

[Cu(H2O)6] 2+

A

Blue

65
Q

[CuCl4]2-

A

Yellow

66
Q

[Cu(NH3)4(H2O)2]2+

A

Deep blue

67
Q

[Co(H2O)6]2+

A

Pink

68
Q

[CoCl4]2-

A

Blue

69
Q

PH of buffer

A

pKa + log([A-]/[HA])

Chemistry A2 (4 decks)

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