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Inorganic chem > Transition metal chemistry > Flashcards

Transition metal chemistry Flashcards

topic 3

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1
Q

Transition metals

A
  • hard, high melting solids
  • conduct heat and electricity
  • readily lose electrons to form stable cations
  • variety of oxidation states available to most
  • form a wide range of coordination compounds with different ligands and molecular geometrics centre on metal ions
  • many are highly coloured and/or paramagnetic
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2
Q

Aufbau principle

A

electrons are added to the lowest energy orbital first

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3
Q

Hund’s rule

A

electrons fill empty orbitals before pairing and the unpaired electrons adopt the same spin values

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4
Q

Pauli exclusion principle

A

no two electrons may have the same set of quantum numbers (n, l, mI, ms)

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5
Q

groups 3 to 7 redox

A

highest oxidation state corresponds to group number

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6
Q

platinum metals - important in catalysis

A
  • Ruthenium
  • Osmium
  • Iridium
  • Palladium
  • Platinum
  • Rhodium
    Form stable cations in water
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7
Q

d block ions

A

lost s electrons before d electrons
Mn2+ and Fe3+ are d5 ions

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8
Q

lower oxidation states what compound type

A

ionic

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9
Q

higher oxidation states what compound type

A

covalent

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10
Q

f-block/group 3/elements of the first transition series (not Cu) react with aqueous solution of acids to give what?

A

hydrogen gas and solutions of corresponding salts

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11
Q

Transition metals and halogens form?

A

anhydrous halides

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12
Q

anhydrous halides reaction from halogen and metal

A

2Fe + 3Cl2 –> 2FeCl3 iron (III) chloride

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13
Q

anhydrous halide reaction from metal halide and additional metal

A

Fe + 2FeCl3 –> 3FeCl2 iron (II) chloride
gives metal halide of lower oxidation state

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14
Q

Ox state of product of F + transition metal

A

highest possible

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15
Q

synthesis of aqueous sol of halides

A

react with salts of hydrohalic acids
NiCo3 + 2HF –> NiF2(aq) + H2O + CO2
nickel (II) fluoride
Co(OH)2 + 2HBr –> CoBr2(aq) + 2H2O
cobalt (II) bromide

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16
Q

Transition metal + acid

A

dissolves to halide salt and hydrogen gas
Mn + 2HCl –> MnCl2 +H2

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17
Q

Electronegativity and ox states

A

transition metals halides with low ox. states are more ionic

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18
Q

heavy d-block elements have significant covalent character

A

.

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19
Q

oxides and ox. state

A

low ox = ionic
high ox = covalent

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20
Q

Oxides and ph

A

low ox = basic
high ox = acids

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21
Q

Soluble hydroxide + aq sol of transition metal

A

gelatinous precipitate
sometimes the precipitate is a hydrated oxide (composed of metal ion, oxide ions and water of hydration)

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22
Q

transition metal salt + soluble carbonate salt

A

insoluble carbonate

23
Q

carbonates + acids

A

metal salts, CO2 and H2O

24
Q

Carbonates decompose on heating to form

A

transition metal oxides

25
Q

coordinate covalent bond

A

donation of electrons from lewis base/ligand to lewis acid/central metal atom

26
Q

Coordination bonding

A

secondary valence
secondary valence electrons don’t have to be bound to a charged species

27
Q

Coordination compounds/werner complexes

A

ligands bond to a metal central atom

28
Q

lewis acid

A

metal

29
Q

lewis base

A

ligand

30
Q

Common neutral ligands

A

water, ammonia, pyridine

31
Q

common anionic ligands

A

cyanide, nitrate, carbonate, sulphate

32
Q

monodentate ligands

A

connect with the central atom through one ligand

33
Q

polydentate ligand

A

same ligand attaches multiple times at different points

34
Q

chelation

A

polydentate ligands attaching to central atom

35
Q

some bidentate ligands

A

ethylenediamine

36
Q

macrocylic ligands

A

polydentate ligands in a ring

37
Q

macrocycles in biological processes

A

used to immobilise metal ions and to increase their reactivity

38
Q

naming coordination complexes

A

if ionic, name cation then anion
ligand first then central
ligands alphabetically
multiples of a ligand -> di/tri/tetra
if cation/neutral metal name is same with ox state at the end
if anion then add ate

39
Q

lanthanides

A

silvery metals abundant
+3 oxidation states mainly

40
Q

actinides

A

radioactive
+3 oxidation states mainly

41
Q

only actinides in nature

A

thorium and uranium

42
Q

condensed electron config of lanthanides

A

[noble gas] ns2 (n - 2)4fx (n - 1)d0

exceptions:
Ce, Gd and Lu have 5d1

43
Q

crystal field theory

A
  • Occurs for the d-orbitals of transition metals
  • The metal ion and the ligand electron pairs are treated as point charges
  • The interaction between them is purely electrostatic (ionic)
  • If the ligand is charged: ion-ion interaction; if ligand is neutral: ion-dipole interaction
44
Q

Porphyrins in biology

A

tetradentate macrocycle
metalloporphyrin e.g. haeme b
vital to life

45
Q

colours of d0 and d10 transition metals

A

white solids
i.e. titanium (IV) oxide and copper (I) iodide

46
Q

how does colour arise in partially filled transition metals

A

transition of element from t2g to 3g by UV light

47
Q

relationship between value of delta-o and wavelength max

A

direct relationship for d1 metals
in Ti (III), delta-o = wavelength max

48
Q

determining colour transmitted

A

opposite on colour wheel to whats absorbed

49
Q

Ti (III) colour transmitted

A

violet

50
Q

colour wheel nm

A

400, 430, 480, 560, 590, 630, 700

51
Q

spectrochemical series

A

list of ligands based on the strength of their interactions with metal ions

52
Q

strong field

A

high delta-o
low spin
shorter wavelength absorbed
CN

53
Q

weak field

A

low delta-o
high spin
longer wavelength absorbed
H2O
F

Inorganic chem (4 decks)

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