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adv chemistry > 1.3 transition metals > Flashcards

1.3 transition metals Flashcards

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1
Q

how do homogeneous catalysts work?

A

by changing oxidation state, which allows the formation of intermediate complexes.

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2
Q

how do heterogeneous catalysts work?

A

they adsorb reactant molecules to their active sites, where the presence of unpaired d electrons allows an activated complex to form

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3
Q

what is a homogeneous catalyst?

A

a catalyst in the same state as the reactants

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4
Q

what is a heterogeneous catalyst?

A

a catalyst in a different state to the reactants

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5
Q

why may a complex be colourless?

A

the absorbed energy from the d-d transition is in the UV part of the spectrum rather than the visible
the TM has a full d subshell so there is no capacity for electrons to transfer

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6
Q

what makes the colours in TM metals?

A

if light from the visible spectrum is absorbed

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7
Q

when is light absorbed?

A

during d-d transition

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8
Q

what is the spectrochemical series, from largest to smallest split?

A

CN-, H20, OH-, F-, Cl-, Br-, I-

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9
Q

how is the ability of ligands to cause splitting given by?

A

the spectrochemical series

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10
Q

how is the loss of degeneracy referred to?

A

splitting of d orbitals

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11
Q

why is there a loss of degeneracy in a transition metal ion in a compound?

A

the ligands create an electrostatic field and repel electrons in some of the TM’s orbitals

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12
Q

in which type of transition metal ion are the 3d orbitals degenerate?

A

a free ion

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13
Q

why are simple and complex ions of transition metals often coloured?

A

because they absorb light in the visible spectrum

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14
Q

when writing the formula of a coordination compound, which order should ligands be written in?

A

alphabetical order by formulae

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15
Q

when writing the formula of a coordination compound, how should the formula of a ligand be written?

A

with the element connecting to the transition metal ion appearing first

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16
Q

in coordination compounds, what should the charges balance to?

A

0

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17
Q

when naming coordination compounds, where should the negative ion be written?

A

after the complex

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18
Q

when naming coordination compounds, where should the positive ion be written?

A

before the complex

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19
Q

when is a coordination compound formed?

A

when a complex ion combines with an oppositely charged ion

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20
Q

what are two examples where metals use their Latin name when converted to ‘ate’?

A

ferrate, cuprate

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21
Q

what is the name of water in a complex ion?

A

aqua

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22
Q

what is the name of carbon monoxide in a complex ion?

A

carbonyl

23
Q

what is the name of ammonia in a complex ion?

A

ammine

24
Q

what changes about negative ligand names when the complex ion is negative?

A

the e changes to an o

25
Q

what changes about the transition metal name if the complex ion is negative?

A

it ends in ‘ate’

26
Q

what must the metal part of the complex name be followed by?

A

its oxidation number written as roman numerals

27
Q

which part of the complex is named first?

A

the ligand(s) in alphabetical order

28
Q

what is the coordination number?

A

the number of bonds formed between the central metal ion and the surrounding ligands

29
Q

what are the three common types of ligands?

A

monodentate, bidentate, hexadentate

30
Q

how are ligands classified?

A

based on the number of electron pairs they donate/the number of bonds they form with the central ion

31
Q

which type of bond do ligands form with the central metal ion?

A

dative

32
Q

how do ligands bond to the metal?

A

they donate non-bonding electron pairs into unfilled metal orbitals

33
Q

what are ligands?

A

a molecule or negative ion with one or more non-bonding pairs of electrons. they are electron donors

34
Q

what does a complex consist of?

A

a central metal ion surrounded by ligands

35
Q

ions in different oxidation states often show different…

A

colours

36
Q

which compounds tend to be reducing agents?

A

compounds with metals in low oxidation states

37
Q

which compounds tend to be good oxidising agents and why?

A
  • compounds with metals in high oxidation states
  • the ions are easily reduced to lower oxidation states
38
Q

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

A

equal to the charge

39
Q

what is the sum of all of the oxidation numbers in a molecule?

A

0

40
Q

what is always the oxidation number of fluorine?

A

-1

41
Q

what is always the oxidation number of group 2 metals?

A

+2

42
Q

what is always the oxidation number of group 1 metals?

A

+1

43
Q

what is the oxidation number of a hydride ion?

A

-1

44
Q

what is the oxidation number of hydrogen in most compounds?

A

+1

45
Q

what is the oxidation number of oxygen in most compounds?

A

-2

46
Q

what is the oxidation number of monatomic ions?

A

equal to the charge

47
Q

what is oxidation number related to?

A

the number of electrons a species has lost or gained

48
Q

what is the oxidation number of a free element?

A

0

49
Q

what the typical transition meta properties?

A

forming coloured ions
forming complexes
having variable oxidation states
showing catalytic activity

50
Q

which two metals do not have an incomplete d subshell in any of their ions, meaning that they don’t have typical transition metal properties?

A

scandium and zinc

51
Q

transition metals have a __ valency, meaning…

A

variable, they can form ions of different charges by losing different numbers of electrons

52
Q

what are some important uses of TMs?

A

piping and wiring, coins, construction, jewellery and catalysts

53
Q

what is the definition of a TM?

A

metals with an incomplete d subshell in at least one of their ions

adv chemistry (22 decks)

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