Transition Metals Flashcards

1
Q

Define Transition Metal

A

Metal atom with partially filled d subshell

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2
Q

What transition metals do we cover?
What is an exception that isn’t a transition metal?

A

Top row Sc-Zn
Zn exception 3d10 subshell for atoms & ions

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3
Q

How do transition metals form complexes?

A

Forms coordinate bond with ligand from e-s from ligand for dative bond

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4
Q

Define a Ligand

A

Particle with lone pair that forms a co-ordinate bond with metals

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5
Q

Define a Complex

A

Metal ion + ligand with a co-ordinate bond

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6
Q

Define co-ordination number

A

Number of co-ordinate bonds in a complex

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7
Q

Define a Lewis Base

A

Lone pair donor

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8
Q

Define a Lewis Acid

A

Lone pair acceptor

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9
Q

What shapes do 4 co-ordinate bonds make?

A

Tetrahedral mostly but sometimes square planar

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10
Q

What shape do 6 co-ordinate bonds make?

A

Octahedral

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11
Q

What shape do 2 co-ordinate bonds make

A

Linear

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12
Q

What type of ligand forms 2 co-ordinate bonds?

A

Bidentate ligands

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13
Q

How do transition metals form coloured ions?

A

They absorb different wavelengths of light

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14
Q

What does the colour of the transition metal ion depend on?

A
  1. The metal ion
  2. The Type of ligand attached
  3. The co-ordination number
  4. The oxidation state of the transition metal
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15
Q

What happens to transition metal d orbitals when ligands bond?

A

When ligands bond 5 d orbitals don’t have same energy
e- excited from lower d orbitals to higher d orbitals

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16
Q

How do coloured ions form?

A

Different energy of d orbitals is in the UV/Visible region -> d-d

17
Q

Outline the Planck equation with units

A

E diff between 2 d-d orbitals (J) = Planck’s constant (6.63x10-34 Jhz-1) X frequency (hz)
E diff = hf

18
Q

Outline the variable oxidation state use in Tollen’s reagent

A

Has [Ag(NH3)2]+
Ag (+1) reduced to Ag (0)

19
Q

Outline the variable oxidation state use in Fehling’s solution

A

Contains Cu (+2) reduced to Cu (+1)

20
Q

Outline the variable oxidation state use in acidified potassium dichromate

A

Has Cr2O7^2-
Cr(+6) reduced to Cr(+3)

21
Q

Outline the variable oxidation state use in redox titrations

A

e.g: acidified KMnO4 used to analyse Fe2+

22
Q

How do pH & ligands affect redox reactions?

A

Reduction of V (+5) to V(+2) due to an acid with Zn

23
Q

Outline all the colour stages of Vanadium

A

V(+5) VO2 = Yellow
V(+4) VO^2+ = Blue
V(+3) V3+ = Green
V(+2) V2+ = Violet

24
Q

Outline the anagram for the colour change of V

A

You
Better
Get
Vanadate

25
Q

Outline how redox potentials impact oxidation states of transition metals

A

Lower O2 state = Reducing agent in acidic conditions

Higher O2 state = Oxidising agent in alkaline conditions

26
Q

Define complete ligand substitution

A

Substitution of similar sized ligands -> entropy is the =

27
Q

Define Partial ligand substitution

A

Substitution of different sized ligands -> entropy changes

28
Q

Chelate

29
Q

Define Heterogeneous catalyst

A

Catalysts in different phase to reactants (usually solid e.g: C2H4 + H2 -> C2H6

30
Q

Define homogeneous catalysts

A

Catalysts that are the = phase as reactants (normally aq)

31
Q

Define Adsorbed

A

Forms bond to the atoms in solid surface

32
Q

Outline how Heterogeneous catalysts work in 3 steps

A
  1. Reactants adsorbed onto surface
    - Weakens bonds
    - brings molecules closer
    - more favourable orientation
  2. Reaction takes place
  3. Products desorbed (leave surface)
33
Q

Outline how too strong of an adsorption impacts heterogeneous catalysis

A

Too strong (e.g Tungsten/W)
- Reactants can’t move round surface
-Products can’t desorb

34
Q

Outline how too weak of an adsorption impacts heterogeneous catalysis

A

Reactants not adsorbed (e.g: silve/Ag)

35
Q

Outline ideal adsorption for heterogeneous catalyst

A

Nickel and Platinum

36
Q

Outline the characteristics of heterogeneous catalysts

A

Large SA
Spread thinly over ceramic honeycomb