Chemistry > Further physical > Flashcards

Further physical Flashcards

(88 cards)

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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
Affect of Δtemp on rate constant
As Temp↑, k↑ , rate↑
26
Homogenous eqm
eqm species all in **same** state
27
Hetrogenous eqm
eqm species have **different** states/ phase
28
How to determine Kc/Kp experiementally?
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
29
Factors that affect(/not) Kc/Kp
**Temp. ** Does not: 1. pressure 2. conc. (causes eqm to shift to restore value)
30
effect of temp on Kc | if LHS -> RHS is endo
1. eqm shifts to the right 2. to restore temp 3. ↑[products] ∴ ↑Kc
31
Define Bronsted-Lowry acid
A species that donates a proton
32
Define bronsted-Lowry bases
a species that accept proton
33
Define monobasic acid
A species that contains **1 ionisable hydrogen atoms** per molecule
34
Assumptions made when doing weak acid calculations
1. [HA]i = [HA]eqm 2. [H+]=[A-]
35
Ka equation for strong acid
36
pKa to Ka conversions
pka = -log Ka
37
How to find pH of strong bases
1. Find the conc of [OH-] 2. use Kw = [H+][OH-] 3. find [H+]
38
2 methods of preparing buffer
1. weak acid + its salt (conjugate base) 2. weak acid + strong base
39
Define buffer solution
minimises change in pH when small amount of acid/base is added
40
# Buffer senario How does buffer minimises change in pH when **acid** is added | (3)
1. [H+] ↑ 2. eqm shifts to the left 3. ↓ [H+]
41
How does buffer minimises change in pH when **base** is added | (5)
1. [OH-] increases 2. H+ + OH- -> H20 3. [H+] ↓ 4. eqm shifts to the LHS 5. restores [H+]
42
How to set up neutralisation reaction | (5)
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
What are pH indicators? How do they change color
Weak acid conjugate acid-base have different color
44
what is the difference between end point and equivilance point
End point - physical observation equivilance point - theroritical, n(titrate) =n(analyte)
45
How to choose an indicator?
indicator range aligns with vertical section pKa in the pH range of color change
46
why does pKa tell the range of the indicator
1.[A-] = [HA] 2.Ka = [H+] 3. pH = -log[H+] position of the end point
47
Define Isoelectric point
pH at which a particular molecule carries no net electrical charge
48
# redox chem MnO4 2- reduced to ...
Mn 2+ [+7] -> [+2]
49
# redox chem Fe 2+ oxidised to ...
Fe 3+ [+2] -> [+3]
50
# redox titration which acid is used to dissolve iron sulphate
sulphuric acid
51
# redox titration Why other acids are not suitable to dissolve | in manganate + iron sulphate
Maybe oxidised or act as oxidising agent for other substance
52
# Redox chem iodine and thiosulphate redox eq.
53
What is in the conical flask for following redox + purpose | iodine + thiosulphate
excess KI oxidising agent to generate Iodine
54
steps to determine end point | iodine + thiosulphate
1. turning from yellow-brown to yellow 2. add starch 3. blue-black End point at colourless
55
End point for iron + manganate
purple to 1st permanent pale pink colour
56
What is calorimetry measure
Wavelength of light - depending on color
57
Define transition metal
d-block element that forms at least 1 ion with incomplete d-subshell
58
2 d-block element that is not transition metal
Sc - only form Sc 3+ Zn - only form Zn 2+
59
two transition element that don't have 4s ^2
copper and chromium [4s^1]
60
Bond angle of square planar
90 deg
61
how many water ligand is formed in aqueos metal complex ?
6
62
Colour of Cr 3+ (aq)
violet
63
Colour of Fe 2+ (aq)
green
64
Colour of Fe 3+ ion (aq)
yellow
65
Colour of Mn 2+ (aq)
pale pink
66
colour of Cu 2+ ion (aq)
Blue
67
Two transition aqueous ion with same colour with the OH substituted ligand
Fe 2+ and Cu 2+
68
Colour of Cr (OH)3 p.p.
grey-green
69
colour of Fe (OH)2 p.p.
green
70
colour of Fe (OH)3 p.p.
brown
71
colour of Mn (OH)2 p.p.
pale brown
72
colour of Cu(OH)2 p.p.
Blue p.p.
73
transition metal that has a colour change in **ex. OH-**
Cr 3+ -> dark green
74
2 transition metals that changes colour in **ex. NH3 **
Cr 3+ - purple Cu 2+ - dark blue
75
3 types of transition metal reaction
1. ligand substitution 2. p.p. reaction 3. redox
76
3 ligand substitution reaction
1. Cr (aq) complex + NH3 ex. 2. Cu (aq) complex + NH3 ex. 3. Cu (aq) complex + 4 Cl- ligands
77
what is the **formula + coordination no** of the complex formed from Cu(H2O)6 + 4Cl-
[CuCl4]2-
78
colour of [CuCl4]2-
yellow
79
What is Haem and its function
1. iron complex 2. forms ligand bonds with O2 3. also bond with CO ligand - but stronger
80
what is the oxidising agent of Fe 3+ (to Fe 2+)
MnO4- ( goes to Mn 2+ )
81
reducing agent of Fe 3+ (to Fe 2+)
I- (iodide ion)
82
colour of Fe 3+
orange-brown
83
colour of Fe 2+
pale-green
84
colour change of iron-manganate titration
purple to colourless
85
colour of Cr^3+ in redox
green
86
colour of Cr2O7^2-
orange
87
colour of Cr 2+
Blue
88
Colour of Copper iodide p.p. (CuI)
white
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