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AH Chemistry > Inorganic and physical chemistry - part 1 > Flashcards

Inorganic and physical chemistry - part 1 Flashcards

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1
Q

What is dual nature?

A

term used to describe light/matter as being able to be both waves and particles

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2
Q

what is a photon?

A
  • particles of electromagnetic radiation

- bundles of fixed energy

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3
Q

what happens when matter emits a photon of radiation?

A

electrons are moving to a lower energy

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4
Q

what is atomic emission spectroscopy used for?

A

used in identification of unknown substances

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5
Q

how is a photon of light emitted?

A
  • electrons absorb energy and become excited
  • move to higher energy level
  • on moving down to lower energy level, a photon of light is emitted
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6
Q

what is the energy difference of an electron transition related to?

A

the wavelength of light

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7
Q

how would you find the quantity of a substance when using AES?

A

measure the intensity of emitted radiation

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8
Q

what does AES give evidence for?

A

gives evidence that electrons occupy energy levels as it shows a number of lines of fixed frequency, corresponding to precise emissions of energy

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9
Q

what is ionisation energy?

A

energy required for electron to break away from the atom

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10
Q

what does ionisation energy correspond to?

A

the difference in energy between the ground state and the convergence limit

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11
Q

what does each line on the emission spectrum represent?

A

a photon of light

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12
Q

what produces a photon of light on the emission spectrum

A

an electron falling from a higher energy state to a lower energy state

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13
Q

what does atomic absorption spectroscopy measure?

A

measures the absorbed radiation needed to promote electrons to higher energy levels

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14
Q

in the Bohr model what is fixed?

A

enthalpy change

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15
Q

what is represented by the Bohr model?

A
  • electrons and energy levels

- photons emitted during transitions

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16
Q

what is Heisenburg’s uncertainty principle?

A

impossible to simultaneously know both the location and momentum of an electron

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17
Q

what are the 4 quantum numbers?

A
  • principal
  • angular momentum
  • magnetic
  • spin
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18
Q

what does the principal (n) quantum number represent?

A

energy, size

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19
Q

what does the angular momentum quantum number represent?

A

shape

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20
Q

what does the magnetic quantum number represent?

A

multiplicity, orientation

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21
Q

as the principal quantum number (n) increases what happens to the energy and size of orbital?

A
  • energy increases

- orbital is larger

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22
Q

when l=0 (angular momentum) what type of orbital is it?

A

s-orbital

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23
Q

what shape is an s-orbital?

A

spherical

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24
Q

what shape is a p-orbital?

A

dumbell

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25
Q

when l=1 what type of orbital is it?

A

p-orbital

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26
Q

when l=2 what type of orbital is it?

A

d-orbital

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27
Q

when l=3 what type of orbital is it?

A

f-orbital

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28
Q

state Pauli exclusion principal

A
  • no two electrons can share a set of quantum numbers

- electrons have the property of spin

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29
Q

what does degenerate mean?

A

having equal energy

30
Q

state Hund’s rule

A

when degenerate orbitals are available, electrons fill each degenerate orbital singly and with parallel spins before pairing up to fill orbitals

31
Q

what is Aufbau principle?

A

filling orbitals in order of increasing energy

32
Q

what is the order of orbitals?

A

1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p

33
Q

what is special about transition metals and their orbitals?

A

they have an incomplete d-orbital in at least on of their ions

34
Q

when a transition metal forms an ion, electrons are removed from which orbital first - 3d or 4s

A

4s

35
Q

why is there some irregularities in the trends for first ionisation energy?

A

some elements have a special stability as they have a full or half-full shell which requires more energy to remove an electron

36
Q

orientation of electron pairs around a central atom, is arranged to minimise what?

A

repulsion

37
Q

what is a dative covalent bond?

A

both electrons in the bond originate on the same atom

38
Q

shape - 2 bonding pairs

A

linear

39
Q

shape - 3 bonding pairs

A

trigonal planar

40
Q

shape - 4 bonding pairs

A

tetrahedral

41
Q

shape - 5 bonding pairs

A

trigonal bipyramidal

42
Q

shape - 6 bonding pairs

A

octahedral

43
Q

what is the colour of compound related to?

A

the oxidation state of the transition metal

44
Q

does oxidation cause an increase or decrease in the oxidation number?

A

increase

45
Q

does reduction cause an increase or decrease in the oxidation number?

A

decrease

46
Q

what is the oxidation number of an element or molecule?

A

zero

47
Q

what is the oxidation number of an ion?

A

the charge

48
Q

what makes a good oxidising agent?

A

a high oxidation state

49
Q

what makes a good reducing agent?

A

a low oxidation state

50
Q

what is the co-ordination number?

A

total number of bonds from the ligand to the central metal ion

51
Q

what is a complex?

A

a central metal ion surrounded by ligands

52
Q

what is a ligand?

A

negative ions or uncharged molecules with one or more non-bonding pairs of electrons

53
Q

what type of bonds do ligands form?

A

dative bonds

54
Q

when would a ligand be described as monodentate?

A

when it donates one pair of electrons to the central metal ion

55
Q

when a ligand donates 2 pairs of electrons to the central metal ion it is described as being what?

A

bidentate

56
Q

if a complex is overall negative what does the name end in?

A

-ate

57
Q

why are transition metal compounds coloured?

A

a d-d transition occurs

58
Q

what is a d-d transition?

A

electron from one of the lower energy d orbitals is promoted to a higher energy d orbital

59
Q

what colour is observed in metals?

A

the complimentary colour to that absorbed

60
Q

what does the spectrochemical series show?

A

the ability of ligands to cause the splitting of d orbitals

61
Q

if there is a large difference in energy in the d-orbitals what is produced?

A

strong field ligands

62
Q

if there is a small difference in energy in the d-orbitals what is produced?

A

weak field ligands

63
Q

why is a solution colourless?

A

no d electrons, so no d-d transitions can occur

64
Q

what is used to study the effects of d-d transitions?

A

spectroscopy

65
Q

what is a homogeneous catalyst?

A

catalyst in the same physical state as the reactants

66
Q

what is a heterogeneous catalyst?

A

catalyst in a different physical state as the reactants

67
Q

what are the three main steps to a heterogeneous catalyst?

A
  • adsorption
  • reaction
  • desorption
68
Q

describe adsorption (in terms of a heterogeneous catalyst)

A
  • molecules of one or both reactants form bonds with the catalyst
  • weakens bonds within molecules
69
Q

describe reaction (in terms of a heterogeneous catalyst)

A
  • the molecules react on the catalyst surface
70
Q

describe desorption (in terms of a heterogeneous catalyst)

A
  • the product molecules leave the catalyst

- vacant site can be occupied by another reactant molecule

71
Q

how does a catalyst speed up a reaction?

A
  • by presence of unpaired electrons or unfilled d-orbitals
  • allows intermediate complexes to form
  • provides reaction pathways or lower energy
72
Q

what makes transition metals good catalysts?

A

they have variable oxidation states

AH Chemistry (8 decks)

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