2.5(P2) Transition Metals Flashcards Preview

AQA A-Level Inorganic Chemistry > 2.5(P2) Transition Metals > Flashcards

Flashcards in 2.5(P2) Transition Metals Deck (53)
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1

What is significant about Aluminium?

It is not a transition metal but still forms complexes
Therefore doesn’t have a colour within the complex

2

Why are transition metals coloured as they are?

The ion absorbs certain frequencies of white light
They have partially filled 3d sub levels
So d-d transitions can take place
So when the electrons move they often absorb energy in the visible region
This colour observed is the light that is reflected

3

What affects the energy difference between d orbitals other than different transition metals?

Different ligands
Different oxidation states

4

What is the equation relating to the colours of transition metals? Units?

ΔE = hv

ΔE - energy difference between the d orbitals - J
h - plancks constant (given) - Js
v - frequency of absorbed radiation - Hz

5

What is significant about light and it’s perceived colour?

They are opposites on the colour wheel

Red light = blue solution

6

What are optical isomers? When does this occur in transition metals?

2 isomers are non-superimposable mirror images of each other
Same molecular and structural formula but has a different spacial arrangement


When there are 2 or more bidentate ligands in a complex

7

Properties of optical isomers?

Chiral
Have identical chemical properties


Distinguished by their effect on polarised light
One isomer rotates the plane of polarisation of polarised light clockwise and the other anticlockwise

8

How can we use colour to determine concentration?

By passing white light through a complementary coloured filter into two solutions
One as a test sample at a different concentration and one as the pure solvent
The light then passes through to a detector and different absorbancies will take place depending on the concentration in the samples
This will then be displayed by a meter or recorder

9

Why do transition metals have variable oxidation states?

They have partially filled 3d sublevels

10

What are Manganese’s oxidation states and colours?

Mn(7) - purple
Mn(6) -
Mn(4) - brown/black
Mn(2) - very pale pink

11

What are chromium’s oxidation states and colours?

Cr(7) - yellow
Dichromate(7) - orange
Cr(3) - green
Cr(2) - blue

Y OG B

12

What are vanadium’s oxidation states and colours?

V(5) - yellow
V(4) - blue
V(3) - green
V(2) - violet

YBGV

13

What do Vanadium’s colours go in real life? (reaction with zinc)

Yellow
Green (due to yellow and blue mixing)
Blue
Green
Violet

14

How do you do a titration calculation?

Work out the moles (of other substance that they gave you)
Work out the ratio between the reactants by forming an overall half equation if the two
Multiply the moles by the correct ratio (this will be the smaller volume)
Multiply by something to get back to the original volume size (usually 10)

Then workout what the question wants

15

What is the MnO4- half equation?

MnO4- + 8H+ + 5e-
->
Mn2+ + 4H2O




MnO4- -> Mn2+

16

What is the Fe2+ equation?

Fe2+ -> Fe3+ + e-

17

What does C2O4 2- go to?

C2O4 2-
->
CO2

18

What is the Cr2O7 2- half equation?

Cr2O7 2- + 14H+ + 6e-
->
2Cr3+ + 7H2O

19

Why are transition metals good catalysts?

They have variable oxidation states

20

What kind of catalysts can transition metals act as?

Heterogeneous - the catalyst has a different state or phase to the reactants

Homogenous - the catalyst has the same state or phase to the reactants

(State: solid/liquid/gas)
(Phase includes aqueous)

21

What is the surface adsorption theory? Using the Haber process

Heterogenous only:
Nitrogen adsorbs onto the catalyst surface (due to lone pairs it can act as a ligand and form covalent bonds)
It speeds it up as the surface holds the molecules in place - easier to react
Nitrogen forms co-ordinate bonds to the surface which weakens N≡N so more reactive with the H2
NH4 is still held by a co-ordinate bond to the surface due to another lone pair
Desorption is the product leaving

22

What is adsorption?

Attaching to the surface but not absorbing in

23

What are some heterogeneous catalysts in processes?

Haber process: uses Iron-Fe
Contact process: uses V2O5 (makes SO3)
Manufacture of Methanol: uses Cr2O3 or Cu

All these are solids btw
And occur at the surface of a catalyst

24

In the contact process - what are the equations for V2O5 being regenerated (example of oxidation state)? and overall equations?

V2O5 + SO2 -> V2O4 + SO3

V2O4 + 1/2O2 -> V2O5


Overall: SO2 + 1/2O2 ⇌ SO3
Then - SO3 + H2O -> H2SO4

25

What reactions use homogeneous catalysts?

S2O8 2- + I-

And

MnO4- + C2O4 2-

26

What is the S2O8 and I- equation?

S2O8 2- + 2I- -> 2SO4 2- + I2
(All aqueous)

27

What metal catalyses S2O8 and I-? Equations?

Fe2+ and Fe3+

S2O8 2- + 2Fe2+ -> 2SO4 2- + 2Fe3+

2Fe3+ + 2I- -> 2Fe2+ + I2

28

In homogenous catalysts why can you add only one of the catalysts ie only Fe2+?

As when you add one the other is produced via redox to then catalyse the second half of the reaction

Eventually the original is regenerated as they continually undergo redox

29

Why is S2O8 2- and I- a slow reaction?

They are both negative ions so they will repel

They require a high activation energy so collisions are unlikely to react

30

Why is an inert medium sometimes used as a support for a heterogeneous catalyst?

Maximise the surface area

Minimise the cost