Chemistry extension Flashcards

1
Q

Why do chemical reactions violate thermodynamics?

A

ΔG = ΔH - TΔS

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2
Q

Why can redox reactions be impossible?

A

AGo = -RT(Keq) = -nFEocell

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3
Q

The octet rule

A

The number of electrons in a shell is 2n2

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4
Q

What does polar mean?

A

Soluble in water

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5
Q

The higher the lattice enthalpy…

A

The stronger the bond

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6
Q

F (lattice enthalpy)

A

(KQ1(charge on ion)Q2)/r2(size of ion)

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7
Q

Reduction (oxygen,electrons,hydrogen,o.s.)

A

-,+,+,-

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8
Q

Oxidation (oxygen,electrons,hydrogen,o.s.)

A

+,-,-,+

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9
Q

Balancing acid half equations

A
  • Any atoms not O or H
  • O using water
  • H using H+
  • Charge using electrons
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10
Q

Balancing alkali half equations

A
  • Any atoms not O or H
  • OH using O
  • H using water
  • Charge using electrons
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11
Q

Oxidation state of F

A

-1

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12
Q

Oxidation state of O

A

-2 (except when bonded to F or O)

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13
Q

Oxidation state of H

A

+1 (except when bonded to a metal)

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14
Q

Oxidation state of a metal

A

Its charge

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15
Q

The sum of o.s.

A

0 or the charge on the ion

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16
Q

2 pair bonding angle

A

180o - linear

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17
Q

3 pair bonding angle

A

120o - trigimal planar

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18
Q

4 pair bonding angle

A

109.5o - tetrahedral

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19
Q

5 pair bonding angle

A

90o and 120o - trigimal biplanar

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20
Q

6 pair bonding angle

A

90o - octahedral

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21
Q

2 bonding and 1 non-bonding

A

<120o - bent or V-shaped

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22
Q

3 bonding and 1 non-bonding

A

107o - trigonal pyramidal

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23
Q

2 bonding and 2 non-boning

A

104.5o - bent or V-shaped

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24
Q

4 bonding and 1 non-bonding

A

See-saw

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25
3 bonding and 2 non-bonding
T-shaped
26
2 bonding and 3 non-bonding
Linear
27
Temperature is directly proportional to...
average KE of particles
28
First law of thermodynamics (Hess's law)
Energy is always conserved
29
Second law of thermodynamics
Entropy (disorder) always increases irrespective of route
30
Third law of thermodynamics
Entropy of a system approaches 0 as temp approaches 0K
31
ΔHf
Enthalpy of formation is ΔH when one mole of compound forms from its constituent elements in their standards states, under standard conditions (theoretical)
32
ΔHc
Enthalpy change when 1 mole of a substance burns completely in oxygen (measureable)
33
ΔHc(O)
0
34
ΔHf(pure element)
0
35
ΔHat
Atomisation - ΔH of elements in standard state to 1 mole of gaseous atoms
36
IE
Ionisation - ΔH of energy to remove 1 mole of electrons to form 1 mole of gaseous ions (+ve)
37
EA
Electron affinity - ΔH of energy to add 1 mole of electrons to form 1 mole of gaseous ions (-ve)
38
ΔHlat
Lattice enthalpy - ΔH of energy to break 1 mole of ionic compound into its constituent gaseous ions
39
ΔH of solution
1 mole of ionic compound into aqueous solution of infinite dilution
40
ΔHlat
((Na(Avagadro's number)M(Madelung constant)Z1Z2(charges)e2)/4πEo(Permeability of free space)ro(Distance between ions))(1-1/n(Born exponent))
41
NMR
- Number of peaks = chemical environment - Area under peaks = ratio of atoms in those environments
42
IR
- ≈1700cm-1 CO double bond - ≈3000cm-1 and wide OH single bond
43
Standards enthalpy change of reaction
Σ(ΔtHθproducts)-Σ(ΔtHθreactants)
44
What is an aldehyde?
A molecule with the carbonyl group at the end of the chain
45
What is a ketone?
A molecule with the carbonyl group bonded to a carbon atom either side
46
How do you produce aldehydes?
Heat a primary alcohol with oxidising agent (K2Cr2O7 acidified with H2SO4) and distil it
47
How do you produce ketones?
Heat a secondary alcohol with oxidising agent (K2Cr2O7 acidified with H2SO4)
48
Can aldehydes be oxidised?
Yes, to produce carboxylic acids
49
Can ketones be oxidised?
They are very resistant to oxidisation
50
Positive Tollens' Reagent result
The aldehyde is oxidised, reducing the silver ions to solid silver which creates a silver mirror
51
Negative Tollens' Reagent result
When gently warmed with a ketone, no silver mirror will be seen as the ketone cannot be oxidised
52
Positive Fehling's solution result
The aldehyde will be oxidised and the blue Cu2+ ions reduced to Cu+ turning it brick red
53
Negative Fehling's solution result
The ketone will not be oxidised so no change occurs
54
What colour change can be seen in ketones when heating with potassium dichromate?
None
55
What colour change can be seen in aldehydes when heating with potassium dichromate?
Orange to green as the aldehyde reacts to form a carboxylic acid
56
nm
1*10-9
57
mm
1*10-3
58
cm
1*10-2
59
dm
1*10-1
60
km
1*103
61
Mm
1*106
62
Gm
1*109
63
µm
1*10-6
64
pm
1*10-12