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inorganic chemistry Flashcards

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1
Q

how can EM radiation be described?

A

as both a wave and a particle- dual nature

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2
Q

when does EM radiation behave as particles?

A

when it is absorbed or emitted, particles are called photons

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3
Q

what do photons carry?

A

quantised energy, proportional to the frequency of radiation

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4
Q

what happens when a photon is absorbed or emitted?

A

energy is gained or lost by the electrons of the material

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5
Q

what happens when energy is transferred to atoms?

A

electrons within it may be promoted to higher energy level

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6
Q

what happens when an electron moves from a higher to lower energy level?

A

a photon is emitted, the light energy emitted produces a spectrum that is made up of a series of lines at discrete energy levels

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7
Q

wavelength definition

A

distance between two crests

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8
Q

frequency definition

A

number of waves per second

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9
Q

relationship between frequency and wavelength

A

as one increases, the other decreases - inversely proportional

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10
Q

relationship between energy and frequency

A

frequency increases = energy increases

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11
Q

what happens as the concentration of the compound in absorption spectroscopy increases?

A

intensity of radiation absorbed increases, intensity of radiation transmitted decreases

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12
Q

what is an orbital?

A

an area of space where there is a 90% chance of finding an electron

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13
Q

what tell us where in an orbital to find an electron?

A

quantum numbers

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14
Q

what is a principal quantum number (n)?

A

represent electron shells
i.e n=1, first shell
n=2, second shell

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15
Q

what are the four subshells?

A

s, p, d, f

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16
Q

how many electrons can each orbital hold?

A

2

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17
Q

angular momentum quantum number

A

s subshell = 0
p subshell = 1
d subshell = 2
f subshell = 3

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18
Q

what does degenerate mean?

A

of equal energy

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19
Q

magnetic quantum numbers

A

no. of orbitals = no. of possible magnetic quantum numbers e.g. 2p subshell could have -1,0 or +1
- you can choose any of the possible magnetic quantum numbers

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20
Q

spin quantum numbers

A
  • can either be +1/2 or -1/2
  • the two electrons in an orbital will spin opposite ways
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21
Q

pauli exclusion principle

A

no two electrons can have the same 4 quantum numbers

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22
Q

aufbau principle

A
  • orbitals of lowest energy fill up first
  • lowest energy orbitals are not necessarily closest to the nucleus (4s fills up before 3d)
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23
Q

hunds rule of maximum multiplicity

A
  • each electron will take a separate orbital until all the orbitals in the subshell are half-filled
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24
Q

what is ionisation energy?

A

energy required to remove one mole of electrons from one mole of gaseous atoms

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25
Q

why does the first I.E of Beryllium not follow the trend?

A

removing an electron involves breaking a full subshell, which requires more energy

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26
Q

what do full and half full shells provide for atoms?

A

more stability

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27
Q

what is the best definition for a transition metal?

A

it can form at least one ion with an incomplete d subshell

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28
Q

which elements dont match the definition for a transition metal?

A

scandium and zinc

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29
Q

which two elements do not follow the aufbau principle and why?

A

copper and chromium, due to the special stability associated with subshells being full or half full

30
Q

which subshell are atoms lost from first when ions are formed?

A

4s

31
Q

oxidation number in a free or uncombined element

A

zero

32
Q

oxidation number in single atom ions

A

same as number charge on the ion

33
Q

oxidation number of hydrogen in compounds

A

usually +1
in hydrides it’s -1

34
Q

oxidation number of oxygen in compounds

A

usually -2
in peroxides it’s -1

35
Q

what must the sum of all the oxidation numbers in a molecule equal?

A

zero

36
Q

what must the sum of all the oxidation numbers in a polyatomic ion equal?

A

the overall charge on the ion

37
Q

what does an increase in oxidation number mean?

A

oxidation has occurred

38
Q

what does a decrease in oxidation number mean?

A

reduction has occured

39
Q

do compounds containing metals with a high oxidation number act as oxidising or reducing agents?

A

oxidising - they are reduced to a lower oxidation number

40
Q

do compounds containing metals with a low oxidation number act as oxidising or reducing agents?

A

reducing - they are oxidised to a higher oxidation number

41
Q

what is changing oxidation states often characterised by?

A

a change in colour

42
Q

what does a transition metal complex consist of?

A

a central metal ion surrounded by ligands

43
Q

what is a ligand?

A

a molecule or ion electron donor which bonds to the metal ion by the donation of one or more electron pairs to unfilled metal ion orbitals

44
Q

what are monodentate?

A

ligands which donate 1 electron pair

45
Q

what are bidentate?

A

ligands which donate 2 pairs of electrons - pairs must be from separate parts of the molcule, not the same atom

46
Q

what is a coordination number?

A

the number of bonds between the ligand and the central ion

47
Q

when naming complexes, when should -ate be added to the metal?

A

if overall charge on ion is negative

48
Q

dative covalent bonds

A

when one atom provides both electrons that form the covalent bond

49
Q

how are transition metal complexes able to absorb light?

A

due to the 5 degenerate d orbitals splitting in terms of energy

50
Q

why do the orbitals along the axis have a higher energy than the other in metal complexes?

A

because the ligands approach the metal along the axes and the electrons that lie on these axes will be repelled y those in the ligand molecules, resulting in more energy - called splitting of d orbitals

51
Q

relationship between ligand size and energy difference

A

larger ligand = larger energy difference

52
Q

what happens when compounds absorb light from the visible spectrum?

A

the colour corresponding to the wavelength is removed and the colour that remains is the complementary colour (opposite in the colour wheel)

53
Q

when are electron transitions more likely to occur in the UV part of the spectrum?

A

when the ligands are strong field (cause greatest splitting/highest energy difference)

54
Q

what colour will the compound be if the transitions occur in the UV part of the spectrum?

A

colourless

55
Q

why are zinc and scandium complexes colourless?

A

zinc (2+) has a full 3d subshell
scandium (3+) has an empty 3d subshell

56
Q

2 categories of transition metal catalysts

A

homogeneous and heterogeneous

57
Q

homogeneous catalyst (definition)

A

catalyst that is in the same state as the reactants

58
Q

heterogeneous catalyst (definition)

A

catalyst that is in a different state to the reactants

59
Q

homogeneous catalyst (explanation)

A

changing oxidation states with the formation of intermediate complexes

60
Q

heterogeneous catalyst (explanation)

A

formation of activated complexes and the adsorption of reactive molecules onto active sites.
the presence of unpaired electrons is thought to allow activated complexes to form, this can provide alternative reaction pathways with a lower activation energy.

61
Q

what is adsorption?

A

the “sticking” of a molecule onto the surface of a catalyst

62
Q

what happens to oxidation number when transition metals are used as catalysts?

A

oxidation number may change, but the original state will be regenerated at the end of the reaction

63
Q

why is the shape of a molecule important?

A

it will determine its properties and uses

64
Q

how do you calculate the number of electron pairs?

A

add the number of outer electrons on central atom to the number of atoms attached to the number of atoms attached to the central atom, then divide by 2

65
Q

what shape is a molecule with 2 bonded pairs?

A

linear

66
Q

what shape is a molecule with 3 bonded pairs?

A

trigonal planar

67
Q

what shape is a molecule with 4 bonded pairs?

A

tetrahedral

68
Q

what shape is a molecule with 5 bonded pairs?

A

trigonal bipyramidal

69
Q

what shape is a molecule with 6 bonded pairs?

A

octahedral

70
Q

what are the shapes of molecules or polyatomic ions determined by?

A

the shapes adopted by the atoms present, based on the arrangement of electron pairs

advanced higher chemistry (4 decks)

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