Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

Chemistry A2 definitions > Module 5 > Flashcards

Module 5 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
A Bronsted-Lowry Base
Proton, H+, acceptor
25
An Alkali
a base that dissolves in water forming OH- ions
26
Neutralisation
a chemical reaction where an acid and a base react together to produce a salt and water
27
what is responsibe for all acid-base reactions?
H+ ions
28
acid + carbonate
salt + water + CO2
29
acid + base
salt + water
30
acid + alkali
salt + water
31
acid + metal
salt + hydrogen
32
Acid-Base pair
A pair of two species that transform into each other by gain or loss of a proton
33
pH scale
a measure of the hydrogen ion concentration
34
pH =
-log[H+]
35
[H+] =
10^-pH
36
Strong Acid
an acid that completely dissociates in solution
37
Weak acid
An acid that partially dissociates in solution
38
Ka
the acid dissociation constant - extent of dissociation in solution Ka= [H+][A-]/[HA]
39
pKa =
-log10Ka
40
Ka = ( in terms of pka)
10^-pKa
41
what are the Ka and pKa values for a weak acid?
small Ka and large pKa
42
what are the Ka and pKa values for a strong acid
large Ka and small pKa
43
How do you find the pH of a strong monobasic acid?
[H+] = [HA] pH = -log[H+]
44
How do you find the pH of a weak monobasic acid?
[H+] = sq root of Ka*[HA] pH = -log[H+]
45
How do you find Ka for a weak acid?
Ka= [H+]^2/[HA]
46
what is Kw
the ionic product of water
47
Kw =
[H+][OH-] = 1.00 x 10^-14 mol2dm-6 at 25•C
48
How do you find the pH of a strong monobasic base?
MOH ----> M+ + OH- [MOH-] = [OH-] using ionic product of water: [H+] = Kw/[OH-] pH = -log[H+]
49
Buffer solution
a system or mixture that minimises pH changes on addtion of small amounts of acid or base
50
what is a buffer solution made from?
a weak acid and its conjugate base
51
How do you find the pH of a buffer solution?
[H+] = Ka x [HA]/[A-] pH = -log[H+]
52
Equivalence point
the point in a titration at which the vol of one solution has reacted exactly with the vol the second solution
53
End Point
point in a titration at which there are equal concentrations pf the weak acid and conjugate base forms of the indicator
54
Standard enthalpy change of neutralisation
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
Hess' Law
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
Lattice Enthalpy
the enthalpy change when 1 mole of a solid ionic compound is formed from its gaseous ions under standard conditions (1 atm, 298K)
57
Enthalpy of formation
the enthalpy change when 1 mole of a compound is formed from its elements in their standard states
58
Enthalpy of Atomisation
the enthalpy change when 1 mole of gaseous atoms form from the elements in their standard states
59
First Ionisation Energy
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
Second Ionisation Energy
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
First Electron Affinity
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
Second Electron Affinity
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
Standard Enthalpy Change of Solution
The enthalpy change when 1 mole of a compound is fully dissolved in water under standard conditons (1 atm, 298K)
64
Standard Enthalpy Change of Hydration
The enthalpy change when 1 mole of aq ions are formed from their gaseous ions under standard conditions (1 atm, 298K)
65
Factors affecting lattice enthalpy and enthalpy of hydration:
- ionic size | - ionic charge
66
Entropy, S
a quantitative measure of the degree of disorder in a system
67
Stnadard entropy of a substance
the entropy content of 1 mole of the substance under the standard conditions (298K, 1atm)
68
Standard entropy change of a reaction
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
For a reaction to be feasible, deltaG...
... must be negative or zero
70
Delta G =
DeltaH - TDeltaS
71
Standard electrode potential of a half cell
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
Rate of reaction
change in concentration of a reactant or product per unit time
73
Initial rate of reaction
change in conc of a reactant, or product, per unit time at the start of the reaction, when t=0
74
order
order with respect to a reactant is the power to which the concentration of the reactant is raised in the rate equation
75
rate equation of A+B=C
rate = k[A]^m[B]^n
76
overall order of reaction
the sum of the individual orders, m+n
77
rate constant, k
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
half-life
the time taken for the concentration of the reaction to reduce by half
79
Reaction mechanism
series of steps that, together, make up the overall reaction
80
rate-determining step
slowest step in the reaction mechanism of a multi-step reaction
81
intermediate
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
overall equation
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.
© 2025 Bold Learning Solutions. Terms and Conditions