Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Chemistry A2 definitions > Module 5 > Flashcards

Module 5 Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
0
Q

complex ion

A

transition metal ion bonded to one or more ligands by coordinate bonds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
1
Q

Transition element

A

A d-block element that forms at least 1 ion with an incomplete d sub-shell

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

ligand

A

an ion or molecule with a lone pair of electrons that can be donated to a transition metal to form a coordinate bond

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

co-ordination number

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

monodentate ligand

A

a ligand that donates one pair of electrons to the cental metal ion

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

bidentate ligand

A

donates 2 lone pairs of electrons to form 2 coordinate bonds with a metal ion

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

multidentate ligand

A

ligand with more than 2 lone pairs

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

stereoisomerism

A

same molecular formula and same structural formula but different arrangement of atoms in space

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

ligand substitution

A

a reaction where one ligand in a complex ion is replaced by another ligand

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Stability constant, Kstab

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

redox

A

both reduction and oxidation reactions taking place

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

oxidation

A

loss of electrons, increase in ON

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

reduction

A

gain of electrons, decrease in ON

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

oxidation number

A

a measure of the number of electrons that an atom uses to bond with atoms of another element. They are derived from a set of rules

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

oxidising agent

A

causes something to be oxidised, it is reduced itself-its ON decreases

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

reducing agent

A

causes something to be reduced, it is oxidised itself - its ON increases

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Dynamic Equilibrium

A

exists in a closed system when the rate of the forward reaction is equal to the rate of the reverse reaction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Kc

A

the equilibrium constant

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Homogeneous equilibrium

A

an equilibrium where all the species making up the reactants and products are in the same physical state

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Heterogeneous equilibrium

A

an equilibrium in which the species making up the reactants and products are in different physical states

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

rule for changing equilibrium conditions

A

If there is a change in concentration, pressure or temp, the equilibrium will move to help counteract the change

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

what affects kc

A

temp

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

increasing the pressure shifts equilibrium to…

A

…the side with fewer gas molecules

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

A Bronsted-Lowry Acid

A

Proton, H+, donor

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

A Bronsted-Lowry Base

A

Proton, H+, acceptor

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

An Alkali

A

a base that dissolves in water forming OH- ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

Neutralisation

A

a chemical reaction where an acid and a base react together to produce a salt and water

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

what is responsibe for all acid-base reactions?

A

H+ ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

acid + carbonate

A

salt + water + CO2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

acid + base

A

salt + water

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

acid + alkali

A

salt + water

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q

acid + metal

A

salt + hydrogen

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
32
Q

Acid-Base pair

A

A pair of two species that transform into each other by gain or loss of a proton

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
33
Q

pH scale

A

a measure of the hydrogen ion concentration

34
Q

pH =

A

-log[H+]

35
Q

[H+] =

A

10^-pH

36
Q

Strong Acid

A

an acid that completely dissociates in solution

37
Q

Weak acid

A

An acid that partially dissociates in solution

38
Q

Ka

A

the acid dissociation constant - extent of dissociation in solution

Ka= [H+][A-]/[HA]

39
Q

pKa =

A

-log10Ka

40
Q

Ka = ( in terms of pka)

A

10^-pKa

41
Q

what are the Ka and pKa values for a weak acid?

A

small Ka and large pKa

42
Q

what are the Ka and pKa values for a strong acid

A

large Ka and small pKa

43
Q

How do you find the pH of a strong monobasic acid?

A

[H+] = [HA]

pH = -log[H+]

44
Q

How do you find the pH of a weak monobasic acid?

A

[H+] = sq root of Ka*[HA]

pH = -log[H+]

45
Q

How do you find Ka for a weak acid?

A

Ka= [H+]^2/[HA]

46
Q

what is Kw

A

the ionic product of water

47
Q

Kw =

A

[H+][OH-] = 1.00 x 10^-14 mol2dm-6 at 25•C

48
Q

How do you find the pH of a strong monobasic base?

A

MOH —-> M+ + OH-

[MOH-] = [OH-]

using ionic product of water:
[H+] = Kw/[OH-]

pH = -log[H+]

49
Q

Buffer solution

A

a system or mixture that minimises pH changes on addtion of small amounts of acid or base

50
Q

what is a buffer solution made from?

A

a weak acid and its conjugate base

51
Q

How do you find the pH of a buffer solution?

A

[H+] = Ka x [HA]/[A-]

pH = -log[H+]

52
Q

Equivalence point

A

the point in a titration at which the vol of one solution has reacted exactly with the vol the second solution

53
Q

End Point

A

point in a titration at which there are equal concentrations pf the weak acid and conjugate base forms of the indicator

54
Q

Standard enthalpy change of neutralisation

A

the energy change that accompanies the neutralisation of an aq acid by an aq base to form 1 mole of H2O, under standard conditions

55
Q

Hess’ Law

A

If a reaction can take place by more than 1 route and the initial and final conditions are the same, the total enthalpy change is the same for each route

56
Q

Lattice Enthalpy

A

the enthalpy change when 1 mole of a solid ionic compound is formed from its gaseous ions under standard conditions (1 atm, 298K)

57
Q

Enthalpy of formation

A

the enthalpy change when 1 mole of a compound is formed from its elements in their standard states

58
Q

Enthalpy of Atomisation

A

the enthalpy change when 1 mole of gaseous atoms form from the elements in their standard states

59
Q

First Ionisation Energy

A

The enthalpy change when 1 electron is removed from each atom in 1 mole of gaseous atoms forming 1 mole of gasous 1+ ions

60
Q

Second Ionisation Energy

A

The enthalpy change when 1 electron is removed from each ion in 1 mole of gaseous 1+ ions forming 1 mole of gaseous 2+ ions

61
Q

First Electron Affinity

A

The enthalpy change when 1 electron is added to each atom in 1 mole of gaseous atoms forming 1 mole of gaseous 1- ions

62
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

63
Q

Standard Enthalpy Change of Solution

A

The enthalpy change when 1 mole of a compound is fully dissolved in water under standard conditons (1 atm, 298K)

64
Q

Standard Enthalpy Change of Hydration

A

The enthalpy change when 1 mole of aq ions are formed from their gaseous ions under standard conditions (1 atm, 298K)

65
Q

Factors affecting lattice enthalpy and enthalpy of hydration:

A
  • ionic size

- ionic charge

66
Q

Entropy, S

A

a quantitative measure of the degree of disorder in a system

67
Q

Stnadard entropy of a substance

A

the entropy content of 1 mole of the substance under the standard conditions (298K, 1atm)

68
Q

Standard entropy change of a reaction

A

the entropy change that accompanies a reaction in the molar quantities expressed in a chemical equation under standard conditions, all reactants and products being in their standard states

69
Q

For a reaction to be feasible, deltaG…

A

… must be negative or zero

70
Q

Delta G =

A

DeltaH - TDeltaS

71
Q

Standard electrode potential of a half cell

A

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

72
Q

Rate of reaction

A

change in concentration of a reactant or product per unit time

73
Q

Initial rate of reaction

A

change in conc of a reactant, or product, per unit time at the start of the reaction, when t=0

74
Q

order

A

order with respect to a reactant is the power to which the concentration of the reactant is raised in the rate equation

75
Q

rate equation of A+B=C

A

rate = k[A]^m[B]^n

76
Q

overall order of reaction

A

the sum of the individual orders, m+n

77
Q

rate constant, k

A

the constant that links the rate of reaction with the concentrations of the reactants raised to the powers of their orders in the rate equation

78
Q

half-life

A

the time taken for the concentration of the reaction to reduce by half

79
Q

Reaction mechanism

A

series of steps that, together, make up the overall reaction

80
Q

rate-determining step

A

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

81
Q

intermediate

A

species formed in one step of a multistep reaction that is used up in a subsequent step, and is not seen as either a reactant or a product of overall equation

82
Q

overall equation

A

sum of equations from each step in reaction mechanism

Chemistry A2 definitions (2 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions