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AQA Chemistry A Level > Transition metals > Flashcards

Transition metals Flashcards

(53 cards)

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1
Q

What are transition metals?

A

Metals that contain an incomplete 3D subshell

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2
Q

What 4 properties do transition metals have?

A

Form complexes
Form coloured ions
Have variable oxidation states
Act as catalysts

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3
Q

What is a ligand

A

Molecule or ion that forms coordinate bond with transition metal

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4
Q

What is a complex

A

Metal central atom or ion and its ligands

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5
Q

What is the coordinate number?

A

Number of coordinate bonds to the central metal atom or ion

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6
Q

What are monodentate ligands?

A

Ligands that form 1 coordinate bond
E.G H2O, NH3, Cl-

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7
Q

What are bidentate ligands + the 2 bidentate ligands we must know?

A

Ligands that form 2 dative covalent bonds
H2NCH2CH2NH2
1,2-diaminoethane
C2O4^2- –> Ethandioate

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8
Q

What are multidentate ligands + the 1 we need to know?

A

Forms multiple coordinate bonds per ligand
EDTA^4- Forms 6 coordinate bonds

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9
Q

What are the 4 ligand substitution reactions

A

Complete with no change in coordination number -

Complete with change in coordination number -

Incomplete with no change in coordination number -

The Chelate effect -

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10
Q

Write a complete ligand substitution with no change in coordination number using [Co(H2O)6]^3+

A

[Co(H2O)6]^3+ + 6NH3 –> [Co(NH3)6]^3+ + 6H2O

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11
Q

Write a complete ligand substitution with a change in coordination number using [Cu(H2O)6]^2+

A

[Cu(H2O)6]^2+ + 4Cl- –> [CuCl4]^2- + 6H2O

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12
Q

Write a incomplete ligand substitution with no change in coordination number using [Cu(H2O)6]^2+

A

[Cu(H2O)6]^2+ + 4NH3 –> [Cu(H2O)2(NH3)4]^2+ + 4H2O

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13
Q

Write the equation for the chelate effect using [Cu(H2O)6]^2+

A

[Cu(H2O)6]^2+ + 3C2O4^2- –> [Cu(C2O4)3]^4- + 6H2O

OR

[Cu(H2O)6]^2+ + EDTA^4- —> [Cu(EDTA)]^2- + 6H2O

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14
Q

What is the chelate effect and what is the enthalpy and entropy like and why?
Use the equation [Cu(H2O)6]^2+ + 3C2O4^2- –> [Cu(C2O4)3]^4- + 6H2O to help

A

Where multidentate ligands form thermodynamically stable complexes

Enthalpy is almost 0 as 6 Cu-O bonds formed and broken
Entropy is large as 7 species is produced from 4 species
Therefore, reaction is feasible with very low activation energy

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15
Q

What is the enthalpy of a complete ligand substitution with no coordinate number change like?

A

Small as bond energies of ligands are similar
Ligands must be a similar size for this substitution

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16
Q

When drawing a complex, how are the cis and trans complexes orientated?

A

Cis - X is found next to each other
Trans - X is found opposite each other

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17
Q

What transition metal complex do we need to know?

A

Cisplatin

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18
Q

What is the structure of cisplatin and its charge?

A

[Pt(NH3)2Cl2)
No overall charge

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19
Q

Why are some transition metal ions coloured? (edit these)

A

Some wavelengths of light are absorbed and the remaining are transmitted or reflected

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20
Q

Why are complexes formed from transition metals coloured?

A

It absorbs some wavelengths of light
Exciting electrons in the d orbital
Remaining wavelengths are reflected or transmitted.

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21
Q

What is the use of cisplatin?

A

Cancer therapy drug

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22
Q

What is the structure of cisplatin?

Study These Flashcards
A

Square planar

23
Q

Why is carbon monoxide toxic?

Study These Flashcards
A

It forms a coordinate bond with Fe2+ in haem B, replacing oxygen

24
Q

What equation is used to find the difference between resting state and excited state electrons?

Study These Flashcards
A

E = hf = hc/λ,
E = energy (J)
h = plank constant = 6.63x10^-34
f = frequency (Hz)
λ = wavelength (m)
c = speed of light = 3x10^8 m/s

25
What factors affect the colour of an ion?
Change in oxidation state Coordination number Ligands
26
How can colourimetry be used to measure an unknown concentration of coloured ions?
Make a series of dilutions of a standard solution of know conc Find absorbance using colorimeter Plot graph of absorbance vs conc and add line of best fit Find absorbance of unknown sample Use graph to find conc
27
What oxidations states does vanadium exists in and what are the colours of these ions?
VO2+ = yellow VO^2+ = blue V^3+ = green V2+ = purple
28
What can vanadium be reduced by?
Zinc metal
29
What can vanadium be oxidised by?
Common oxidising agents such as mangate (VII) solution (MnO4^-)
30
WHat factors affect redox potential for a transition metal ion
pH Type of ligand Conditions (temp, press, conc)
31
Redox titration of iron (II) and manganate (VII) equation + The colour change
5Fe^2+ + MnO4^- + 8H^+ --> Mn^2+ + 5Fe^3+ + 4H2O Pink due to MnO4 being self indicating
32
Redox titration between ethanedioate and manganate (VII) + colour change and observations
5C2O4^2- + 2MnO4^- + 16H^+ --> 10CO2 + 8H2O + 2Mn^2+ Pink due to MnO4- being self indicating Effervescence from CO2
33
Why can transition metals act as catalysts
They can form variable oxidation states and temporarily donate and accept electrons
34
How do catalysts speed up reactions?
Provide an alternative reaction pathway with a lower activation energy, therefore more particles have energy greater than Ea so more collisions cause a reaction.
35
What are heterogenous catalysts?
Catalysts that are in a different phase than the reactants.
36
How do heterogenous catalysts work?
Reaction occurs in active sites on the surface where vacant d orbitals can form weak bonds.
37
How must a heterogenous catalyst be suitable for a reaction?
Must be strong enough bonds to adsorb reactants but weak enough to de-adsborb
38
Write the contact process for the reaction of SO2 and 1/2O2 with a vanadium (V) catalyst
SO2 + 1/2O2 --> SO3 V2O5(s) + SO2(g) -- > V2O4(s) + SO3(g) V2O4(s) + 1/2O2(g) --> V2O5(s)
39
What is the contact process mechanism?
Via variable oxidation states of vanadium
40
Write the mechanism of the haber process
Reactants adsorb to active sites on the surface Bonds in reactants weaken New bonds form in products Products de-adsorb from the surface
41
What reaction do we know uses the haber process + its catalyst
N2(g) + 3H2(g) --> 2NH3(g) With Fe(s) catalyst
42
What is a homogenous catalyst?
Catalyst in the same phase as the reactants. Forms an intermediate species.
43
Reaction between Iodide ions and peroxodisulfate
S2O8^-2 + 2I^- —> 2SO4^2- + I2
44
Write equations showing how iron (II) acts as a catalyst in the reaction between peroxodisulfate and Iodide ions
S2O8^2- + 2Fe^2+ —> 2SO4^2- + 2Fe^3+ 2Fe^3+ + 2I^- —> 2Fe^2+ + I2
45
What is catalyst poisoning?
Where impurities permanently adsorbs and blocks the active site
46
How can catalysts be used in a cost effective way?
Used as a fine powder sprayed across a wire mesh to increase SA and use less amount of expensive material
47
What is autocatalysis
A reaction where one of the products catalyses the reaction
48
Write how Mn2+ ions catalyse the reaction between manganite (VII) ions and ethandioate
5Mn^2+ + MnO4^- + 8H^+ —> 5Mn^3+ + Mn^2+ + 4H2O 2Mn^3+ + C2O4^2- —> 2Mn^2+ + 2CO2
49
How does a normal rate graph compare with a rate graph involving autocatalysis
Rate initially slower Once product is catalyst and conc of product increases, catalyst increases so rate increases
50
What is the relationship between frequency of light and energy
Energy is directly proportional to frequency of light
51
Explain why, for example, a solution of copper II sulfate appears blue?
Absorbs all parts of the visible spectrum and reflect blue light
52
Explain why transition metals absorb light in the visible part of the spectrum with reference to electron transitions
d-subshell orbitals have a ground and excited state Electrons absorb light with energy equivalent to visible light Electrons promoted to excited state Relax back and release thermal energy
53
Explain why different ligands, oxidation state and coordination number change the colour of a complex of the same metal
Variation of these factors changes the energy gap between ground and excited state d subshell orbitals This causes a different frequency of light to be absorbed E = hf

AQA Chemistry A Level (43 decks)

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