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Chem > Key Stuff - Module 3 + 5 > Flashcards

Key Stuff - Module 3 + 5 Flashcards

1
Q

1st ionisation energy

A

removal of 1 mole of electrons from 1 mol of gaseous atoms

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2
Q

Periodicity

A

Repeating trends in physical + chemical properties

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3
Q

Metallic bonding

A

Strong electrostatic attraction bt/w positive ions + delocalised electrons

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4
Q

Disproportionation

A

Oxidation + reduction of the same element

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5
Q

Activation Energy

A

Minumum energy required for a reaction to take place

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6
Q

Enthalpy change of formation

A

Formation of 1 mol of compound froms its elements

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7
Q

Enthalpy change of combustion

A

Compete combustion of 1 mol of a substance

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8
Q

Enthalpy change of neutralisation

A

Formation of 1 mol of water from neutralisation

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9
Q

Average bond enthalpy

A

Breaking of 1 mol of bonds in gaseous molecules

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10
Q

Homogenous catalyst

A

Same phase a reactants

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11
Q

Heterogeneous catalyst

A

Different phase as reactants

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12
Q

Bronsted-Lowry acid

A

Donates a proton

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13
Q

Bronsted-Lowry Base

A

Accepts a proton

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14
Q

What indicator should you use for strong acid + strong base reaction

A

Phenolphalein or methyl orange

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15
Q

Strong acid + weak base

A

Methyl orange

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16
Q

Weak acid + strong base

A

Phenolphthalein

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17
Q

Weak acid + weak base

A

pH at equivalence - depends on the relative strength of acid + base

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18
Q

Lattice enthalpy

A

Formation of 1 mol of ionic lattice from gaseous ions

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19
Q

Enthalpy change of solution

A

Dissolving of 1 mol of solute

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20
Q

Enthalpy change of hydration

A

Dissolving of 1 mol of gaseous ions in water

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21
Q

Entropy

A

Measure of dispersal of energy in a system which is greater, the more disorder a system

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22
Q

Standard electrode potential

A

Is a measure of the reducing power of any element or compound

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23
Q

Units for rate constant (k)

A
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24
Q

Rate graphs for 0 order reaction

A
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25
Q

Rate graphs for 1st order

A
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26
Q

Rate graphs for 2nd order

A
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27
Q

Rate determining step info

A
  • Slowest step is rate determining step
  • Species involved in this step are found in overall rate equation
28
Q

Weak acids

A

Partially dissociate into ions in aqueous solutions

29
Q

Strong acids

A

Completely dissociate into ions in aqueous solutions releasing H+ ions

30
Q

Name 3 basic strong acids

A
  • HCl
  • HNO3
  • H2SO4
31
Q

Name a basic weak acids

A

Carboxylic acids eg ethanoic acid

32
Q

Name 3 basic strong bases

A
  • NaOH
  • KOH
  • Ba(OH)2
33
Q

Name a weak base

A

Ammonia (NH3)

34
Q

State the redox reaction bt/w manganate (VII) + iron (II)

35
Q

Describe the method you would use to do a redox titration calculation

A
  1. Form redox equation
  2. FInd the moles of compound
  3. Use redox equation to find the moles of unknown
  4. Scale up if needed
36
Q

What must you remember when calculating elctrode potential

A

Reduced electrode potential is always more positive electrode potential

37
Q

Explain the process of a proton exchange fuel cell

A
  1. Hydrogen gas enters system
  2. Hydrogen oxidised to H+ at anode
  3. Electrons travel via external circuit
  4. H+ ions travel through electrolyte + membrane
  5. oxygen gas enters cell
  6. Oxygen is reduced at cathode
  7. Catalyst speeds up reaction bt/w oxygen + H+
  8. Water produced
38
Q

Advantages of fuel cells

A
  • Eliminate pollution caused by burning fossil fuels
  • Eliminates green house gases if hydrogen used comes from electrolysis of water
  • Higher efficiency than diesel or gas engines
39
Q

Alkaline Fuel Cells (AFC)

A
  • Uses alkaline electrolyte eg KOH
  • Used by NASA in space shuttles
40
Q

Direct Methanol Fuel Cells (DMFC)

A
  • Uses polymer membrane as electrolyte
  • Catalyst on anode draes hydrogen from liquid methanol
  • Eliminates need for fuel reformer, pure methanol can be used as fuel
41
Q

Rearranged Arrhenius equation for Ea

A

Ea = RT (lnA-lnk)

42
Q

Rearranged Arrhenius equation for A

43
Q

Rearranged Arrhenius equation for T

A

T = Ea / R (lnA-lnk)

44
Q

Ligand

A

Particle with lone pair thay forms a coordinate (dative covalent) bond to metal

45
Q

Complex

A

Central metal ion with ligands coordinately bonded to it

46
Q

Coordination number

A

Number of coordinate bonds from ligand to metal ions

47
Q

Cis-platin

A
  • Anti-cancer drug
  • Complex of platinum (II) with X2 chloride ions + X2 ammonia molecules in square planar shape
  • Binds to DNA preventing cell division
48
Q

Unidentate ligands

A
  • Donates one electron pair
  • Form one coordinate bond
  • Eg. [Cu(H2O)6]2+
49
Q

Bidentate ligands

A
  • Donates X2 electron pairs
  • Form two coordinate bonds
  • Eg. [Cr(NH2CH2CH2NH2)3]3+
50
Q

Multidentate ligands

A
  • Donates several electron pairs
  • Form several coordinate bonds
  • Eg. [Cu(EDTA)]2-
51
Q

Ti 3+

52
Q

Ti +2

53
Q

VO2 + (OS +5)

54
Q

VO2+ (OS +4)

55
Q

V3+

56
Q

V2+

57
Q

Cr2O7 2- (OS +6)

58
Q

Cr3+

A

Pale purple

Looks green in aqueous solutions

59
Q

MnO4 - (OS +7)

60
Q

MnO4 2- (+6)

61
Q

Mn2+

62
Q

Fe3+

63
Q

Fe2+

A

Pale green

64
Q

Co2+

65
Q

Ni2+

66
Q

Cu2+

Chem (47 decks)

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