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Chemistry > Further physical > Flashcards

Further physical Flashcards

1
Q

Enthalpy

A

A value that represents heat content of system

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2
Q

Enthalpy change of atomization

A

enthalpy change when 1 mol of gaseous atom is formed from an element in standard state

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3
Q

Enthalpy change of hydration

A

enthalpy change when 1 mol of gaseous ions are dissolved in water

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4
Q

Enthalpy change of solution

A

enthalpy change when 1 mol of solute is dissolved in water

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5
Q

1st electron affinity

A

energy released when 1 mol of electron is added to 1 mol of gaseous atom, forming 1 mol of gasous 1- ions

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6
Q

Lattice enthalpy

A

Formation of 1 mol of ionic lattice from 1 mol of gasous ions

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7
Q

What is lattice enthalpy a measure of?

A

strength of ionic bonds in lattice

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8
Q

Describle born-haber cycle diagram

A

atomization + Ionisation + electron affinity + ΔH(LE)
= enthalpy change of formation

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9
Q

How to increase lattice enthalpy ?

A

1.↑ ionic charge ( ↑ p : e ratio )
2.↓ ionic radius ( ↓ dist. = ↑ attraction )

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10
Q

0th order conc-time graph

A
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11
Q

1st order conc-time graph

A
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12
Q

2nd order conc-time graph

A
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13
Q

0th order rate-conc graph

A
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14
Q

1st order rate-conc graph

A
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15
Q

2nd order rate-conc graph

A
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16
Q

properties of 1st order conc-time graph

A

exponential decay
[constant half-life]

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17
Q

how to find rate constant for 1st order reaction

A

k = ln(2) / t1/2

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18
Q

2 methods of investigating rate

A
  1. initial rate
  2. continuous monitoring of conc.
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19
Q

Describle measuring intial rate with
E.g. iodine clock

A

record time for color change
(e.g. colorless to blue-black)

initial rate = 1/time for color change

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20
Q

Assumption made to record initial rate

A

no significant change in rate in the period recorded

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21
Q

Describle how calorimetry is used to determine rate

A
  1. certain wavelength of light is emitted to solution
  2. absorbance is recorded
  3. conc is monitored as proportional to absorbance
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22
Q

Desrible lattice enthalpy cycle

A
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23
Q

Describle enthalpy change of hydration cycle

A

ΔH(LE) + ΔH(solution) = ΔH(hydration)

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24
Q

Factors that affects ΔH(hydration)

A
  1. ↑ionic charge
  2. ↓ionic radius

↑ionic density = ↑ attraction on H2O= ↓ΔH

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25
Q

Affect of Δtemp on rate constant

A

As Temp↑, k↑ , rate↑

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26
Q

Homogenous eqm

A

eqm species all in same state

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27
Q

Hetrogenous eqm

A

eqm species have different
states/ phase

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28
Q

How to determine Kc/Kp experiementally?

A
  1. Mix known moles of reactant and acid
  2. wait
  3. then titrate one of the products to find the conc at eqm
  4. then find all conc at eqm by stoichiometry
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29
Q

Factors that affect(/not) Kc/Kp

A

**Temp. **

Does not:
1. pressure
2. conc.
(causes eqm to shift to restore value)

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30
Q

effect of temp on Kc

if LHS -> RHS is endo

A
  1. eqm shifts to the right
  2. to restore temp
  3. ↑[products]
    ∴ ↑Kc
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31
Q

Define Bronsted-Lowry acid

A

A species that donates a proton

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32
Q

Define bronsted-Lowry bases

A

a species that accept proton

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33
Q

Define monobasic acid

A

A species that contains
1 ionisable hydrogen atoms
per molecule

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34
Q

Assumptions made when doing weak acid calculations

A
  1. [HA]i = [HA]eqm
  2. [H+]=[A-]
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35
Q

Ka equation for strong acid

A
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36
Q

pKa to Ka conversions

A

pka = -log Ka

37
Q

How to find pH of strong bases

A
  1. Find the conc of [OH-]
  2. use Kw = [H+][OH-]
  3. find [H+]
38
Q

2 methods of preparing buffer

A
  1. weak acid + its salt (conjugate base)
  2. weak acid + strong base
39
Q

Define buffer solution

A

minimises change in pH when small amount of acid/base is added

40
Q

Buffer senario

How does buffer minimises change in pH when acid is added

(3)

A
  1. [H+] ↑
  2. eqm shifts to the left
  3. ↓ [H+]
41
Q

How does buffer minimises change in pH when base is added

(5)

A
  1. [OH-] increases
  2. H+ + OH- -> H20
  3. [H+] ↓
  4. eqm shifts to the LHS
  5. restores [H+]
42
Q

How to set up neutralisation reaction

(5)

A
  1. Add measured volume of acid/base into conical flask
  2. place electrode (of pH meter) into solution
  3. Add base/acid to burrette
  4. add 1 cm3 at a time
  5. go to dropwise when pH changes rapidly
43
Q

What are pH indicators?
How do they change color

A

Weak acid
conjugate acid-base have different color

44
Q

what is the difference between
end point and equivilance point

A

End point - physical observation
equivilance point - theroritical, n(titrate) =n(analyte)

45
Q

How to choose an indicator?

A

indicator range aligns with vertical section

pKa in the pH range of color change

46
Q

why does pKa tell the range of the indicator

A

1.[A-] = [HA]
2.Ka = [H+]
3. pH = -log[H+]

position of the end point

47
Q

Define Isoelectric point

A

pH at which a particular molecule carries no net electrical charge

48
Q

redox chem

MnO4 2-
reduced to …

A

Mn 2+

[+7] -> [+2]

49
Q

redox chem

Fe 2+
oxidised to …

A

Fe 3+

[+2] -> [+3]

50
Q

redox titration

which acid is used to dissolve
iron sulphate

A

sulphuric acid

51
Q

redox titration

Why other acids are not suitable to dissolve

in manganate + iron sulphate

A

Maybe oxidised or act as oxidising agent for other substance

52
Q

Redox chem

iodine and thiosulphate
redox eq.

A
53
Q

What is in the conical flask for following redox
+
purpose

iodine + thiosulphate

A

excess KI
oxidising agent

to generate Iodine

54
Q

steps to determine end point

iodine + thiosulphate

A
  1. turning from yellow-brown to yellow
  2. add starch
  3. blue-black
    End point at colourless
55
Q

End point for iron + manganate

A

purple to
1st permanent pale pink colour

56
Q

What is calorimetry measure

A

Wavelength of light - depending on color

57
Q

Define transition metal

A

d-block element that forms at least 1 ion with incomplete d-subshell

58
Q

2 d-block element that is not transition metal

A

Sc - only form Sc 3+
Zn - only form Zn 2+

59
Q

two transition element that don’t have 4s ^2

A

copper and chromium [4s^1]

60
Q

Bond angle of square planar

A

90 deg

61
Q

how many water ligand is formed in aqueos metal complex ?

A

6

62
Q

Colour of Cr 3+ (aq)

A

violet

63
Q

Colour of Fe 2+ (aq)

A

green

64
Q

Colour of Fe 3+ ion (aq)

A

yellow

65
Q

Colour of Mn 2+ (aq)

A

pale pink

66
Q

colour of Cu 2+ ion (aq)

A

Blue

67
Q

Two transition aqueous ion with same colour with the OH substituted ligand

A

Fe 2+ and Cu 2+

68
Q

Colour of Cr (OH)3 p.p.

A

grey-green

69
Q

colour of Fe (OH)2 p.p.

A

green

70
Q

colour of Fe (OH)3 p.p.

A

brown

71
Q

colour of Mn (OH)2 p.p.

A

pale brown

72
Q

colour of Cu(OH)2 p.p.

A

Blue p.p.

73
Q

transition metal that has a colour change in
ex. OH-

A

Cr 3+ -> dark green

74
Q

2 transition metals that changes colour in
**ex. NH3 **

A

Cr 3+ - purple
Cu 2+ - dark blue

75
Q

3 types of transition metal reaction

A
  1. ligand substitution
  2. p.p. reaction
  3. redox
76
Q

3 ligand substitution reaction

A
  1. Cr (aq) complex + NH3 ex.
  2. Cu (aq) complex + NH3 ex.
  3. Cu (aq) complex + 4 Cl- ligands
77
Q

what is the formula + coordination no
of the complex formed from

Cu(H2O)6 + 4Cl-

A

[CuCl4]2-

78
Q

colour of [CuCl4]2-

A

yellow

79
Q

What is Haem and its function

A
  1. iron complex
  2. forms ligand bonds with O2
  3. also bond with CO ligand - but stronger
80
Q

what is the oxidising agent of Fe 3+ (to Fe 2+)

A

MnO4- ( goes to Mn 2+ )

81
Q

reducing agent of Fe 3+ (to Fe 2+)

A

I- (iodide ion)

82
Q

colour of Fe 3+

A

orange-brown

83
Q

colour of Fe 2+

A

pale-green

84
Q

colour change of iron-manganate titration

A

purple to colourless

85
Q

colour of Cr^3+ in redox

A

green

86
Q

colour of Cr2O7^2-

A

orange

87
Q

colour of Cr 2+

A

Blue

88
Q

Colour of Copper iodide p.p. (CuI)

A

white

Chemistry (6 decks)

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