Topic 15 Transition Metals Flashcards

1
Q

What is the definition of transition metals?

A

d-block elements that form one or more stable ions with incompletely filled d-orbitals

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2
Q

Why aren’t Scandium and Zinc non transition metals?

A

Zn can only have 2+ charge (lost from 4s orbital, no e-s can be lost from d block, most stable full)
Sc only does 3+ charge (can only form an empty d-block, symmetrical again)

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3
Q

When are d block elements most stable?

A

Half full (5 electrons)
Or full (10 electrons)

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4
Q

Why can transition metals change oxidation numbers so much?

A

3d energy level is very close to 4s, transition metals usually lose 4s and capable of losing any unpair 3d e-s as well

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5
Q

What are properties of transition metals?

A
  • form complex ions
  • colourful compounds
  • catalytic properties (both ions and compounds)
  • variable oxidation states
  • hard / dense / high mp bp
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6
Q

What does hydrated mean for ions?

A

Ions surrounded by H2O molecules

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7
Q

How do transition metals interact with water?

A

covalent bonds
(dative sometimes)

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8
Q

What are properties of transition metal complex ions?

A
  • small
  • highly charged = high charge density
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9
Q

What is a ligand?

A

Ion or molecules w lone pair
forms dative covalent bond with a (transitional) metal ion (except aluminium)
Forming complex ions

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10
Q

How to write a complex ion?

A

[M(H2O)6] ^3+ (aq)

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11
Q

What do molecules with lone pairs have to be?

A

nucleophile

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12
Q

What is a monodentate ligand?

A

Has 1 lone pair

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13
Q

What is a bidentate ligand?

A

Has 2 lone pairs that are the same distance from each other so they can form 2 co-ordinate bonds
eg H2N-CH2CH2-NH2

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14
Q

What is a coordination number?

A

number of dative covalent bonds
(NOT number of ligands)

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15
Q

Chromium has oxidation numbers +2, +3, +6.
Why can chromium show variable oxidation numbers? (1 mark)

A
  • 3d and 4s orbitals have similar energy levels to remove an e-
  • ionisation energies are similar in value
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16
Q

How to work out transition metal compounds that are unlikely to exist?

A

Eg electronic configuration 3d5 4s1
There are only 6 electrons to lose
So ox num 7+ and above are unlikely to exist

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17
Q

Are electrons from transition metals lost from 3d or 4s orbital first?

A

4s ALWAYS

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18
Q

Explain why brass is malleable but sodium chloride is not. (3 marks)

A
  • brass is alloyed with similar sized atoms
  • so layers can slide
    In NaCl
  • any shift in ionic lattice will repel
  • won’t occur in brass as delocalised e-s prevents repulsion
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19
Q

Why is vanadium classified as a transition metal?

A

It forms stable ions with incompletely filled d orbitals

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20
Q

Why does Cu have extra high 2nd ionisation energy / big jump from 1st?

A

2nd e- is from 3d not 4s

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21
Q

What complexes form square planar complex ions?

A

Pt 2+ and Ni 2+

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22
Q

What angle is octahedral complexes?

A

90 degrees

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23
Q

Why is Cl- as ligands, forming only 4 single co-ordinate bond with Cu 2+ not 6?
What shape does it make?

A

Cl- ions are large
So can only fit 4, not 6
Makes tetrahedral, 109.5

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24
Q

What is the most common bidentate ligand and give molecular formula.

A

1,2-diaminoethane
NH2CH2CH2NH2

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25
Q

What is the most common multidentate ligand we need to know?

A

EDTA 4-

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26
Q

In Pt(NH3)2Cl2 - it is square planar.
When is it a cis and trans isomer?

A

cis when Cl are next to each other, NH3 next to each other.
trans when opposite each other

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27
Q

With reference to electrons, explain why aqueous copper(II) ions are blue. (3 marks)

A
  • e-s in 3d shell split into 2 energy levels
  • e-s from lower energy level absorbs energy (red) , can be promoted to higher energy level
  • remaining light (blue) is reflected/transmitted
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28
Q

State the origin colour of transition-metal complexes. (2 marks)

A
  • e-s absorb energy from visible spectrum in 3d shell
  • wavelengths not absorbed produce the colour (transmitted)
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29
Q

Give 3 changes to a transition-metal complex which result in a change of colour. (3 marks)

A
  • oxidation state of metal
  • charge density / type of metal
  • charge density / type of ligands
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30
Q

How to use colorimeter to determine the conc of iron(III) ions in a solution of unknown conc?

A
  • calibration curve
  • use 1 moldm-3 solution of Fe3+, measure, dilute and repeat (known concs)
  • measure absorbance of sample after reference cuvette
  • measure absorbance of unknown conc and see which matches on graph
  • can add ligand to intensify colour
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31
Q

In terms of electrons, explain why an aqueous solution of cobalt(II) sulfate has a red colour. (3 marks)

A
  • Co2+ has 2 energy levels in d orbital
  • energy difference corresponds to energy of blue photons - electron promoted to higher orbital when absorbed
  • red light reflected
32
Q

Why is colorimetry preferred over titration?

A

get results quicker

33
Q

Explain why the aqueous solution of complex ion has an acidic pH by considering the interaction between metal ions and ligands. / why is the higher the charge in metal aqua ion, the more acidic the solution?

A
  • to lose H+, OH bond must break
  • will break when e-s in bond pulled towards O
  • higher charge = stronger pull = release H+ more readily = more acidic
34
Q

Which metal aqua ions + ligand combo would result in redissolving?

A

If TM begins with ‘C’ (like chromium, copper, cobalt)
Will re dissolve in excess

35
Q

How many ammonia swap in for metal aqua ions for which metals?

A

Chromium & cobalt - (NH3)6 swaps in
Copper - only (NH3)4, makes [Cu(NH3)4(H2O)2]2+

36
Q

Why do sometimes predictions with oxidation/reducing agents don’t work?

A

Reactions are too slow
(As activation energy is too high)

37
Q

What are the colour changes from V5+ to V4+ to V3+ to V2+ ?

A

Yellow
Blue (green first, as it’s a mixture of yellow and blue)
Green
Violet

38
Q

How to work out which reducing/oxidising agents to use for transition metals?

A

Use E cell values
For reducing agents, use E cell values higher up (more negative) than itself
Vice versa

39
Q

How to reduce Cr6+ to Cr2+?

A

Zinc or H+

40
Q

What colours are Cr6+, Cr3+ and Cr2+ ?

A

Orange
Green
Blue

41
Q

How to convert Cr^3+ to CrO4^2-?

A

+ H2O2 or OH-

42
Q

How to convert Cr^2+ to Cr^3+ ?

A

Oxygen / air

43
Q

Why is Cr2O7 bad?

A

Very carcinogenic

44
Q

How to convert Cr2O7^2- -> CrO4^2- ?
And
How to convert CrO4^2- ->Cr2O7^2- ?

A

Cr2O7^2- + NaOH → CrO4^2-
CrO4^2- + H2SO4 → Cr2O7^2-
(Think 2 to 1 Chromates, NaOH all singular 1 ; 1 to 2, has H2SO4

45
Q

What 4 factors affect the transition metal’s colours?

A

Type of metal
Oxidation state of metal
Type of ligands
Coordination number

46
Q

Why do changes in factors eg types of metals and ligands affect the colour of the Complex ion?

A

Size of energy gap between d orbitals would be changed
So frequency of light absorbed would be changed
Hence colour reflected changes

47
Q

What is a ligand substitution?

A

Reaction when a ligand replaces another ligand
(No change in ox num at all)

48
Q

What colours are [Cu(H2O)6]2+ (aq) and [CuCl4]2- (aq) ?

A

Blue
And
Yellow

49
Q

What colours are [Co(H2O)6]2+ (aq) and [CoCl4]2- (aq) ?

A

Pale pink
To
Blue

50
Q

How do catalysts work?

A
  • reactants adsorb to active site of catalyst
  • bonds weaken
  • reaction takes place
  • desorption
  • by providing alternative route with a lower activation energy
51
Q

What is a heterogeneous catalyst? (1 mark)

A

catalyst that is in a different phase to reactants.

52
Q

Why must catalysts not be too strong or too weak?

A

too strong: risk of poisoning as may bind irreversibly
too weak: not many molecules adsorbed to catalyst, little effect to reaction AND won’t weaken bonds enough

53
Q

What is the equation and catalyst for the Haber process?

A

3 H2 + N2 ⇌ 2NH3
Fe catalyst

54
Q

What are the 2 steps of the contact process and what catalyst is used?
+ give half equation

A

2 SO2 + O2 ⇌ 2 SO3
V2O5 catalyst
half eq
SO2 + V2O5 → SO3 + V2O4(intermediate)
V2O4 + 1/2 O2 → V2O5

55
Q

How to maximise efficiency of a catalyst?

A

Increase the surface area for adsorption
by using a mesh or honeycomb structure

56
Q

What is catalyst poisoning and how does it happen?

A

Adsorption is too strong, binding is irreversible
active site is blocked
- catalyst is ruined, v costly

57
Q

What is a homogeneous catalyst?

A

catalyst in the same phase as reactants

58
Q

Why are transition metals great catalysts?

A
  1. have variable oxidation states
  2. are position ions so will bind with anions and have low activation energy
59
Q

Can catalysts alter the value of equilibrium constant?

60
Q

What reactions use heterogeneous catalysts?

A

Haber
Contact
Car exhaust

61
Q

What is the reaction of the car exhaust system and what catalyst is used?

A

CO + NO → CO2 + 1/2 N2
Pt catalyst

62
Q

What is the reducing agent in
CO + NO → CO2 + 1/2 N2 ?

63
Q

State the general property of transition metals that allows the vanadium in vanadium(V) oxide to act as a catalyst in the Contact process.

A

variable oxidation states

64
Q

Suggest why the vanadium(V) oxide is used in small pellets form rather than as large lumps. (1 mark)

A

increases surface area
so more efficient

65
Q

State why the reactant should be purified before they some into contact with V2O5 in the contact process. (1 mark)

A

To remove potential poisons

66
Q

What is autocatalysis?

A

When one of the products in a reaction acts as a catalyst.

67
Q

What is the reaction between iodide ions and peroxodisulfate ions? What catalyst is used?
give half eq

A

2I- + S2O8 2- → I2 + 2 SO4 2-
Fe2+/Fe3+ as catalyst
2 Fe^2+ + S2O8^2- → 2 Fe^3+ + 2 SO4^2-
2 Fe^3+ + 2I- → 2 Fe^2+ + I2

68
Q

What is the equation of reaction between manganate(VII) ions and ethanedioate ions? What catalyst?

A

2 MnO4^- + 14H+ + 5C2O4^2- → 2 Mn^2+ + 8 H2O + 10 CO2
Mn2+ the product

69
Q

How to prove Mn2+ is the catalyst in the manganate(VII) ions and ethanedioate ions reaction?

A

Add Mn2+ from the start

70
Q

Suggest why ions from s block elements do not usually act as catalysts. (1 mark)

A

No variable oxidation states

71
Q

Give one reason why, in the absence of a catalyst, the activation energy for the reaction between S2O8^2- ions and I- ions is high. (1 mark)

A

they are both negative ions
so will repel

72
Q

How do catalysts catalyse reactions between two negative ions?

A

Transition metal catalysts are positively charged - so oppositely charged to anions
lowers activation energy, so less energy needed to overcome

73
Q

[Co(H2O)6]^2+ + ethane-1,2-diamine →

A

[Co(NH2CH2CH2NH2)3]2+ + 6H2O
(as it is bidentate!!)

74
Q

Name the ligands
H2O
NH3
Cl-
OH-
CN-

A

aqua
ammine
chloro
hydroxo
cyano

75
Q

How to name transition metals in complex ions?

A

if complex is +ve charged - regular name
if -ve charged - latin name + ‘ate’

76
Q

What is the formula of the manganese species formed from MnO4- and excess dilute sulfuric acid
From purple to colourless

77
Q

Suggest why zinc does not produce hydrogen with nitric acid.

A

Using E cell values
It is not feasible (and expand using data equations)