Module 5 Flashcards

1
Q

Order w.r.t [A] = 0
Change in [A] = X2

A

Rate = [X2]^0
So rate stays constant

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

Order w.r.t [A] = 0
Change in [A] = X3

A

Rate = [X3]^0 = X1
Rate stays constant

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

Order w.r.t [A] = 1
Change in [A] = X2

A

Rate = [X2]^1 = 2
Rate doubles

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

Order w.r.t [A] = 1
Change in [A] = X3

A

Rate = [X3]^1 = X3
Rate triples

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

Order w.r.t [A] = 2
Change in [A] = X2

A

Rate = [X2]^2 = 4
Rate quadruples

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

Order w.r.t [A] = 2
Change in [A] = X2

A

Rate = [X3]^2 = 9
Rate X9

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

Overall order : 1
Rate equation?
Units of K?

A

Rate = k [A]
S^-1

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

Overall order : 2
Rate equation?
Units of K?

A

rate = k [A]^2
dm^3mol^-1s^-1

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

Overall order : 3
Rate equation?
Units of K?

A

rate = k [A]^2 [B]
dm^6mol^-2s^-1

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

Overall order : 4
Rate equation?
Units of K?

A

rate = k[A]^2 [B]^2
dm^9mol^-3s^-1

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

Half-life of reactant, t1/2

A

Time for the concentration of the reactant to reduce by half

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

Ea=
A=
R=

A

activation energy
pre-exponential factor
gas constant (on data sheet)

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

Enthalpy change of atomization Delta at H theta

A

The enthalpy change, when one mole of gaseous atoms is formed from its elements under standard conditions

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

First electron affinity Delta EA1 H theta

A

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

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

Second electron affinity Delta EA2 H theta

A

The enthalpy change, when one electron is added to each ion in one mole of gaseous 1- ions, to form one mole of gaseous 2- ions

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

Entropy, S

A

The measure of the dispersal of energy in a system. The entropy is greater when the system is more disordered. System becomes energetically more stable when it becomes more disordered.

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

Standard entropy change of reaction, Delta S theta

A

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

Delta S theta (entropy) = sum of entropy of products - sum of entropy of reactants
(See A2 paper 1 definition list for module 5)

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

Rate - determining step

A

The slowest step of reaction mechanism of a multistate reaction

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

Mole fraction x(A)

A

Number of moles of A / total number of moles in a gas mixture

20
Q

Partial pressure p(A)

A

Mole fraction of A x total pressure P

21
Q

Bronsted-Lowry acid

A

A proton (H+) donor

22
Q

Bronsted-Lowry base

A

A proton (H+) acceptor

23
Q

Strong acid

A

Completely dissociates into its ions in solution to donate a proton

24
Q

Weak acid

A

Partially dissociates in its ions in solution to donate a proton

25
Salt
A compound produced when a H+ ion from an acid is replaced by a metal ion or another positive ion, such as the ammonium ion NH4+
26
Conjugate acid - base pairs
A pair of two species that transform into each other by the gain or loss of a proton (H+)
27
pH=
-log[H+]
28
H+=
10^-pH
29
pKa=
-log[Ka]
30
Ka=
10^-pKa
31
Kw=
[H+][OH-]
32
Buffer solution
A mixture that minimizes pH change on addition of small amount of acid or base
33
Lattice enthalpy Delta LE H
Enthalpy change, when one mole of an ionic compound is formed from its gaseous ions
34
Standard enthalpy change of solution Delta sol H theta
Enthalpy change that takes place with one mole of compound (solute) is completely completely dissolved in water under standard conditions
35
Standard enthalpy change of hydration Delta hyd H theta
The enthalpy change that takes place when one mole of isolated gaseous ions is dissolved in water filming one mole of aqueous ions under standard conditions
36
Gibbs Equation
*G = *H -T*S *=delta If G > 0, reaction is not feasible If G < 0 reaction is feasible If G = 0 system is in equilibrium
37
Standard electrode potential, E theta
Of a half cell; is the e.m.f of a half cell compared with a standard hydrogen half cell measured at 298K or -25° C with solution concentrations of 1moldm^-3 and a gas pressure of 100 kPa (1atm) Species undergoing reduction must have the more positive E theta value
38
Transition element
A D-Block element that forms an ion with an incomplete d-sub shell
39
Complex ion
A transition metal ion bonded to one or more ligands by coordinate bonds
40
Ligand
A molecule ion that can donate a pair of electrons to the transition metal ion to form a coordinate bond
41
Dative covalent bond (coordinate bond)
Shared pair of electrons, in which one of the bonded atoms provides both electrons for the shared pair
42
Coordination number
The total number of coordinate bonds formed between central metal ion and its ligands
43
Monodentate ligand
A molecule or ion that can donate one pair of electrons to the transition metal ion to form one coordinate bond
44
Bidentate ligand
Donate to lone pairs of electrons to the central metal ion to form two coordinate bonds
45
Multidentate ligand
Donate more than one lone pair of electrons to the central metal ion to form more than one coordinate bond
46
Optical isomer
Stereoisomers that are a pair of non-superimposable mirror images of each other