Module 5 Flashcards

1
Q

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

A

Rate = [X2]^0
So rate stays constant

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2
Q

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

A

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

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3
Q

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

A

Rate = [X2]^1 = 2
Rate doubles

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4
Q

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

A

Rate = [X3]^1 = X3
Rate triples

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5
Q

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

A

Rate = [X2]^2 = 4
Rate quadruples

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6
Q

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

A

Rate = [X3]^2 = 9
Rate X9

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7
Q

Overall order : 1
Rate equation?
Units of K?

A

Rate = k [A]
S^-1

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8
Q

Overall order : 2
Rate equation?
Units of K?

A

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

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9
Q

Overall order : 3
Rate equation?
Units of K?

A

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

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10
Q

Overall order : 4
Rate equation?
Units of K?

A

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

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11
Q

Half-life of reactant, t1/2

A

Time for the concentration of the reactant to reduce by half

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12
Q

Ea=
A=
R=

A

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

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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

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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

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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

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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.

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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)

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18
Q

Rate - determining step

A

The slowest step of reaction mechanism of a multistate reaction

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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
Q

Salt

A

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
Q

Conjugate acid - base pairs

A

A pair of two species that transform into each other by the gain or loss of a proton (H+)

27
Q

pH=

A

-log[H+]

28
Q

H+=

A

10^-pH

29
Q

pKa=

A

-log[Ka]

30
Q

Ka=

A

10^-pKa

31
Q

Kw=

A

[H+][OH-]

32
Q

Buffer solution

A

A mixture that minimizes pH change on addition of small amount of acid or base

33
Q

Lattice enthalpy Delta LE H

A

Enthalpy change, when one mole of an ionic compound is formed from its gaseous ions

34
Q

Standard enthalpy change of solution Delta sol H theta

A

Enthalpy change that takes place with one mole of compound (solute) is completely completely dissolved in water under standard conditions

35
Q

Standard enthalpy change of hydration Delta hyd H theta

A

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
Q

Gibbs Equation

A

*G = H -TS
*=delta
If G > 0, reaction is not feasible
If G < 0 reaction is feasible
If G = 0 system is in equilibrium

37
Q

Standard electrode potential, E theta

A

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
Q

Transition element

A

A D-Block element that forms an ion with an incomplete d-sub shell

39
Q

Complex ion

A

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

40
Q

Ligand

A

A molecule ion that can donate a pair of electrons to the transition metal ion to form a coordinate bond

41
Q

Dative covalent bond (coordinate bond)

A

Shared pair of electrons, in which one of the bonded atoms provides both electrons for the shared pair

42
Q

Coordination number

A

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

43
Q

Monodentate ligand

A

A molecule or ion that can donate one pair of electrons to the transition metal ion to form one coordinate bond

44
Q

Bidentate ligand

A

Donate to lone pairs of electrons to the central metal ion to form two coordinate bonds

45
Q

Multidentate ligand

A

Donate more than one lone pair of electrons to the central metal ion to form more than one coordinate bond

46
Q

Optical isomer

A

Stereoisomers that are a pair of non-superimposable mirror images of each other