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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
Q

3 bonding and 2 non-bonding

A

T-shaped

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26
Q

2 bonding and 3 non-bonding

A

Linear

27
Q

Temperature is directly proportional to…

A

average KE of particles

28
Q

First law of thermodynamics (Hess’s law)

A

Energy is always conserved

29
Q

Second law of thermodynamics

A

Entropy (disorder) always increases irrespective of route

30
Q

Third law of thermodynamics

A

Entropy of a system approaches 0 as temp approaches 0K

31
Q

ΔHf

A

Enthalpy of formation is ΔH when one mole of compound forms from its constituent elements in their standards states, under standard conditions (theoretical)

32
Q

ΔHc

A

Enthalpy change when 1 mole of a substance burns completely in oxygen (measureable)

33
Q

ΔHc(O)

A

0

34
Q

ΔHf(pure element)

A

0

35
Q

ΔHat

A

Atomisation - ΔH of elements in standard state to 1 mole of gaseous atoms

36
Q

IE

A

Ionisation - ΔH of energy to remove 1 mole of electrons to form 1 mole of gaseous ions (+ve)

37
Q

EA

A

Electron affinity - ΔH of energy to add 1 mole of electrons to form 1 mole of gaseous ions (-ve)

38
Q

ΔHlat

A

Lattice enthalpy - ΔH of energy to break 1 mole of ionic compound into its constituent gaseous ions

39
Q

ΔH of solution

A

1 mole of ionic compound into aqueous solution of infinite dilution

40
Q

ΔHlat

A

((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
Q

NMR

A
  • Number of peaks = chemical environment
  • Area under peaks = ratio of atoms in those environments
42
Q

IR

A
  • ≈1700cm-1 CO double bond
  • ≈3000cm-1 and wide OH single bond
43
Q

Standards enthalpy change of reaction

A

Σ(ΔtHθproducts)-Σ(ΔtHθreactants)

44
Q

What is an aldehyde?

A

A molecule with the carbonyl group at the end of the chain

45
Q

What is a ketone?

A

A molecule with the carbonyl group bonded to a carbon atom either side

46
Q

How do you produce aldehydes?

A

Heat a primary alcohol with oxidising agent (K2Cr2O7 acidified with H2SO4) and distil it

47
Q

How do you produce ketones?

A

Heat a secondary alcohol with oxidising agent (K2Cr2O7 acidified with H2SO4)

48
Q

Can aldehydes be oxidised?

A

Yes, to produce carboxylic acids

49
Q

Can ketones be oxidised?

A

They are very resistant to oxidisation

50
Q

Positive Tollens’ Reagent result

A

The aldehyde is oxidised, reducing the silver ions to solid silver which creates a silver mirror

51
Q

Negative Tollens’ Reagent result

A

When gently warmed with a ketone, no silver mirror will be seen as the ketone cannot be oxidised

52
Q

Positive Fehling’s solution result

A

The aldehyde will be oxidised and the blue Cu2+ ions reduced to Cu+ turning it brick red

53
Q

Negative Fehling’s solution result

A

The ketone will not be oxidised so no change occurs

54
Q

What colour change can be seen in ketones when heating with potassium dichromate?

A

None

55
Q

What colour change can be seen in aldehydes when heating with potassium dichromate?

A

Orange to green as the aldehyde reacts to form a carboxylic acid

56
Q

nm

A

1*10-9

57
Q

mm

A

1*10-3

58
Q

cm

A

1*10-2

59
Q

dm

A

1*10-1

60
Q

km

A

1*103

61
Q

Mm

A

1*106

62
Q

Gm

A

1*109

63
Q

µm

A

1*10-6

64
Q

pm

A

1*10-12

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