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Transition Metal And Qeous Salts > Uhm > Flashcards

Uhm Flashcards

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1
Q

Why do transition metal characteristics of elements arise in Ti-Cu

A

They have incomplete d subshell

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2
Q

Why is scqandium not a transition metal

A

Sc3+ ion has no d electrons

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3
Q

Why is titanium a transition metal

A

Titanium forms Ti3+ ions which has electronic configuration of [Ar] 3d1

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4
Q

Why might coordinate number and shape change when substitution used with Cl- ions

A

Only 4 will fit around the central metal ion because the chloride ligands are larger than the water ligands

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5
Q

What is heam

A

Iron (II) complex with multidentate ligand
4 N atoms in the porphyria ring form 4 coordinate bonds

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6
Q

How does oxygen bond to hemoglobin

A

Forms coordinate bond to Fe(II) in haemoglobin

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7
Q

Why si CO toxic

A

Replaces Oxygen coordinately bonded to Fe(II) in haemoglobin

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8
Q

Chelate effect

A

Bindentate and multidentate ligands replace monodentate ligands

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9
Q

What shape is often made with small ligands

A

E.g. H2O and NH3
Octahedral

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10
Q

What isomerism do octahedral complexes show

A

cis/trans with monodentate and optical isomerism with bidentate

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11
Q

What shape do TM often form with larger ligands

A

E,g, Cl-
Tetrahedral

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12
Q

What other shapes are formed

A

Square planar, cis trans isomerim

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13
Q

What is cisplatin

A

[Pt(NH3)2Cl2]
Is the cis isomer

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14
Q

Tollens reagent

A

[Ag(NH3)2]2+

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15
Q

How does colour arise

A

Metal ion absorbs light
D electrons are excited
Some of the wavelengths of visible light are absorbed and the complementary wavelengths are transmitted or reflected

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16
Q

Equation for difference between the ground state and excited state of d electrons

A

∆ E = h ν = hc /λ

E =2.718 energy, J
h = Planck constant = 6.63 x10 -34 Js
v = frequency, Hz/s-1
λ = wavelength, metres
c = speed of light m/s

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17
Q

Why are there changes in colo

A

Changes in oxidationns tate, cootdinate number and tupe of ligand change E of d electrons being excited, which leads to change in colour

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18
Q

Colour of [Cu(H2O)6]2+

A

Blue

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19
Q

Colour of [CuCl4]2-

A

Yellow/green

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20
Q

What are the 4 vanadium oxidation states

A

5+
4+
3+
2+

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21
Q

Colour of vanadium oxidation states

A

5+ = yellow
4+ = blue
3+ = green
2+ = violet
You better get vanadium

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22
Q

How are different vanadium species formed

A

By reduction with zinc

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23
Q

Order of reduction of vanadium

A

VO2 +
VO 2+
V3+
V2+

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24
Q

Why is conc HCl used to reduce vanadium

A

Acidic conditions favour reduction of TM

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25
What is first used when reducing vanadium
Ammonium vanadate (V) White solid, can be dissolved in HCl to give ate low solution When zinc is added to this acidic solution, the V is reduced
26
What is the redox potential for a TM changing from higher to lower oxidation state influenced by
PH and ligand
27
Heterogenous catalyst
Catalyst is in different phase or state to reactants. Reaction occurs at active sites on the surface
28
Homogenous catalyst
Same phase as the reactants and an intermediate species is formed.
29
Can TM act as both homogenous and heterogenous catalysts
Yes
30
How to minimise cost and maximise efficiency of catalyst
Increasing surface area of catalyst Coating an inert surface medium with the catalyst to avoid using large amounts of catalyst. E.g honeycomb structure
31
Contact process
Manufacture of H2SO4 Heterogenous catalyst = V2O5 SO2 -> SO3
32
Equations of contact process
S + O2 -> SO2 V2O5 + SO2 -> V2O4 + SO3 V2O4 + 1/2 O2 -> V2O5 Overall equation: SO2 + 1/2 O2 -> SO3 Heterogenous
33
Haber process
Making NH3 from N2 Fe is used as a heterogenous catalyst N2 + 3H2 -> 2NH3
34
Why may heterogenous catalysts become less efficient
Can become poisoned by impurities that block the active sites and so reduced efficiency, this has a cost implication
35
What is the importance of variable oxidation states in catalysis
TM can adopt more than one stable oxidation state, so they can accept and lose electrons easily to go from one oxidation state to another, so they can catalyse redox reactions by acting as both oxidising and reducing agents
36
Explain with the aid of equations how Fe2_ ions catalyse the reaction between I- and S2O8 2- What's the catalyst? Why? What type of catalyst is it?
S2O8 2- is made into SO4 2- with I- S2O8 2- + 2I- -> 2SO4 2- + I2 1. S2O8 2- + 2Fe2+ -> 2SO4 2- + 2Fe3+ 2. 2Fe3+ + 2I- -> Fe2+ + I2 Fe2+ catalyst, Without catalyst, rate of reaction is very low due to both negative ions, ESF repulsion Homogenous catalyst
37
Autocatalyst
A product of the reaction is a catalyst for the reaction
38
Equation for MnO4- to....
Mn2+ 5e- + Mno$- + 8H+ -> Mn2+ + 4H2O
39
Equation for C2O4 2- to ...
CO2 C2O4 2- -> 2CO2 + 2e-
40
What's the autocatalyst in this
Mn2+
41
Equation between Mn2+ and MNo4 -
4MN2+ + MnO4 - + 8H+ -> 5Mn3+ + 4H2O 2MN3+ + C2O4 2- -> 2Mn2+ + 2CO2
42
What complexes are made in aqueous solution
[M(H2O)6]2+ Where M is only Fe or Cu [M(H2O)6]3+ Where M = Al and Fe
43
Acidity of [M(H2O)6]3+ compared to [M(H2O)6]2+
More acidic Because M3+ ion is more charge dense ( smaller, higher charge) then M2+ ion. So M3+ draws electrons from O atoms in the water ligands towards itself more strongly, weakening in the OH bonds, so the water ligands are polarised and release H+ into solution
44
Amphoteric character
Able to act as both a base and acid
45
Why do some metal hydroxides show amphoteric character
Dissolving in both acids and bases E.g. hydroxides of Al3+
46
Colour og [Fe(H2O)6]2+
Green
47
Addiiton of NaOH to [Fe(H2O)6]2+
[Fe(H2O)6]2+ + 2OH- -> Fe(H2O)4(OH)2 + 2H2O Green precipitate, slowly turns born as is oxidised to iron 3 hydroxide Doesn't redissolve on addition of excess
48
Addition of NH3 to [Fe(H2O)6]2+
Fe(H2O)6]2+ + 2NH3 -> Fe(H2O)4(OH)2 + 2NH4+ Green precipitate that turns brown in air as it is oxidised to iron 3 hydroxide Doesn't redissolve with excess NH3
49
Addiiton of Na2CO3 to Fe(H2O)6]2+
Fe(H2O)6]2+ + CO3 2- -> FeCO3 + 6H2O Green precipitate
50
What colour is [Cu(H2O)6]2+
Pale blue
51
Adding NaOH to [Cu(H2O)6]2+
[Cu(H2O)6]2+ + 2OH- -< Cu(H2O)4(OH)2 + 2H2O Pale blue precipitate Does not redissolve on the addiiton of excess NaOH
52
Addition of NH3 to [Cu(H2O)6]2+
[Cu(H2O)6]2+ + 2NH3 -> Cu(H2O)4(OH)2 + 2NH4+ Does redissolve in addiiton of excess NH3 to form deep blue solution of [Cu(NH3)4(H2O)2]2+ Cu(H2O)4(OH)2 + 4NH3 -> [Cu(NH3)4(H2O)2]2+ + 2OH- + 2H2O
53
Addiiton of Na2CO3 to [Cu(H2O)6]2+
Blue Green precipitate [Cu(H2O)6]2+ + CO3 2- -> CuCO3 + 6H2O
54
What colour is [Fe(H2O)6]3+
Purple/yellow/brown
55
Addiiton of NaOH to [Fe(H2O)6]3+
[Fe(H2O)6]3+ + 3OH- -> Fe(H2O)3(OH)3 + 3H2O Brown precipitate Doesn't redissolve on addiiton of excess NaOH
56
Addiiton of NH3 to [Fe(H2O)6]3+
[Fe(H2O)6]3+ + 3NH3 -> Fe(H2O)3(OH)3 + 3NH4 + Brown ppt that doesn't redissolve on addition of excess NH3
57
Addiiton ofNa2CO3 o [Fe(H2O)6]3+
2[Fe(H2O)6]3+ + 3Co3 2- -> 2Fe(OH)3(H2O)3 + 3CO2 + 3H2O Brown ppt and bubbles of gas (CO2)
58
Colour of [Al(H2O)6]3+
Colourless solution
59
Addiiton of NaOH to [Al(H2O)6]3+
[Al(H2O)6]3+ + 3OH- -> Al(H2O)3(OH)3 + 3H2O Whit Epps which redissolve on addiiton of excess NaOH because its amphoteric
60
Reaction of Al(H2O)3(OH)3 with base
Al(OH)3(OH)3 + OH- -> Al(OH)4 - + 3H2O Or Al(OH)3(OH)3 + OH- -> [Al(OH)4(H2O)2] - + H2O
61
Al(OH)3(OH)3 in acid
Al(OH)3(OH)3 + 3HCl -> [Al(H2O)6]3+ + 3Cl-
62
Addiiton of NH3 to [Al(H2O)6]3+
White ppt which doesnt redissolve n excess NH3 [Al(H2O)6]3+ + NH3 -> Al(OH)3(H2O)3 + 3NH4 +
63
Addiiton of Na2CO3 to [Al(H2O)6]3+
White ppt, bubbles of gas (CO2) 2[Al(H2O]6]3+ + 3CO3 2- -> 2Al(OH)3(H2O)3 + 3CO2 + 3H2O
64
What type of catalysis if th

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