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transition metals Flashcards

(68 cards)

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1
Q

what is the colour of [Cu(h2o)]^2+

A

blue

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2
Q

what is the colour of [CuCl4]^2-

A

yellow

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3
Q

what is the colour of [Cu(NH3)4(H20)2]^2+

A

dark blue

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4
Q

what is the colour of [Cu(edta)]^2-

A

light blue

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5
Q

why stability increases from [Cu(h2o)]^2+ to [CuCl4]^2- to [Cu(NH3)4(H20)2]^2+ to [Cu(edta)]^2-

A

as one edta molecule can replace the six smaller ligands, ligands are released into the solution, greater disorder, entropy increases

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6
Q

why colour change is observed (ligand exchange of Cu2+ )

A

when ligands change, size of the energy gap between the split of d orbitals change, frequency of white light absorbed during promotion of electrons from lower to higher energy levels change and the remainder is the colour that we see

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7
Q

what is the colour of VO3^- / VO2^+

A

yellow

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8
Q

what is the colour of VO^2+

A

blue

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9
Q

what is the colour of V^3+

A

green

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10
Q

what is the colour of V^2+

A

purple

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11
Q

what is a black solid compound

A

CuO

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12
Q

what is the colour of Cu2O and how it is made

A

red solid ,
made by reduction of fheling’s/ Benedict’s solution (while oxidising aldehyde)

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13
Q

what are the observations that can be made when Cu^+ is dissolved in water

A

blue solution and pink-brown solid forms

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14
Q

how Cu^2+ reacts with I^-

A

Cu^2+ oxidises iodide to iodine and Cu^2+ itself gets reduced to Cu^+, CuI is a white precipitate.
when there is xs I^- blue colour disappears to give brown solution and white precipitate
( you can make a titration with sodiumthiosulphate and add starch to have blue-black colour disappear towards end-point)

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15
Q

what is the colour of Cr^2+ ( Cr(H2O)6^2+ )

A

blue

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16
Q

what is the colour of Cr^3+ (Cr(H2O)6^3+ )

A

green

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17
Q

what is the colour of CrO4^2-

A

yellow

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18
Q

what is the colour of Cr2O7^2-

A

orange

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19
Q

why the solution of Cr^3+ is more acidic than the solution of C^2+

A

Cr^3+ has greater polarising power,
it causes O-H bond in water ligands to be broken why resilts in hydronium ions to form and hence lower the pH

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20
Q

colour of Cr^3+ and its form in complex ion in aq solution

A

[Cr(H2O)6]^3+
green

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21
Q

colour of Mn^2+ and its form in complex ion in aq solution

A

[Mn(H20)6]^2+
colourless

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22
Q

colour of Fe^2+ and its form in complex ion in aq solution

A

[Fe(H2O)6]^2+
green

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23
Q

colour of Fe^3+ and its form in complex ion in aq solution

A

[Fe(H2O)6]^3+
yellow- orange

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24
Q

colour of Co^2+ and its form in complex ion in aq solution

A

[Co(H2O)6]^2+
blue

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25
colour of Ni^2+ and its form in complex ion in aq solution
[Ni(H2O)]^2+ green
26
colour of Cu^2+ and its form in complex ion in aq solution
[Cu(H2O)6]^2+ blue
27
colour of Zn^2+ and its form in complex ion in aq solution
[Zn(H2O)6]^2+ colourless
28
observation for Cr^3+ with a few drops of NaOH(aq) or NH3(aq) and the complex ions that are formed
Cr(OH)3(H2O)3 pale green ppt
29
observation for Mn^2+ with a few drops of NaOH(aq) or NH3(aq) and the complex ions that are formed
Mn(OH)2(H2O)4 beige ppt darkens upon standing MnO2
30
observation for Fe^2+ with a few drops of NaOH(aq) or NH3(aq) and the complex ions that are formed
Fe(OH)2(H2O)4 green ppt turns red-brown on standing Fe(OH)3(H2O)3
31
observation for Fe^3+ with a few drops of NaOH(aq) or NH3(aq) and the complex ions that are formed
Fe(OH)3(H2O)3 red-brown ppt
32
observation for Co^2+ with a few drops of NaOH(aq) or NH3(aq) and the complex ions that are formed
Co(OH)2(H2O)4 blue ppt turns pink upon standing Co(OH)2(H2O)4.xH2O
33
observation for Ni^2+ with a few drops of NaOH(aq) or NH3(aq) and the complex ions that are formed
Ni(OH)2(H2O)4 green ppt
34
observation for Cu^2+ with a few drops of NaOH(aq) or NH3(aq) and the complex ions that are formed
Cu(OH)2(H2O)4 blue ppt
35
observation for Zn^2+ with a few drops of NaOH(aq) or NH3(aq) and the complex ions that are formed
Zn(OH)2(H2O)4 white ppt
36
observation of Cr^3+ with xs NaOH(aq)
ppt disappaers to form a green solution [Cr(OH)6]^2-
37
observation of Mn^2+ with xs NaOH(aq)
no further reaction
38
observation of Fe^2+ with xs NaOH(aq)
no further reaction
39
observation of Fe^3+ with xs NaOH(aq)
no further reaction
40
observation of Co^2+ with xs NaOH(aq)
no further reaction
41
observation of Ni^2+ with xs NaOH(aq)
no further reaction
42
observation of Cu^2+ with xs NaOH(aq)
no further reaction
43
observation of Zn^2+ with xs NaOH(aq)
ppt disapperas to form colourless solution [Zn(OH)4]^2-
44
observation of Cr^3+ with xs NH3(aq)
ppt disappers to form a green solution [Cr(NH3)6]^3+
45
observation of Mn^2+ with xs NH3(aq)
no further reaction
46
observation of Fe^2+ with xs NH3(aq)
no further reaction
47
observation of Fe^3+ with xs NH3(aq)
no further reaction
48
observation of Co^2+ with xs NH3(aq)
ppt disappears to form brown solution [Co(NH3)6]^2+
49
observation of Ni^2+ with xs NH3(aq)
ppt disappears to give a lavendar blue solution (Ni(NH3)6]^2+
50
observation of Cu^2+ with xs NH3(aq)
ppt disappearsto give a deep blue solution [Cu(OH)2(NH3)4]^2+
51
observation of Zn^2+ with xs NH3(aq)
ppt disappears to form a colourless solution [Zn(NH3)4]^2+
52
observations of Ag^+ in aq solution
colourless
53
observation of Ag^+ with a few drops of NH3(aq)
brown ppt Ag2O forms which is hard to see as it dissolves in ammonia
54
observations of Ag^+ with xs NH3(aq)
any ppt disappears to give a colourless solution
55
what does amphoteric hydroxides mean
they both react with acids and bases example; hydroxides of zinc and chromium
56
what are d block elements
elements which has its last electron placed in d-subshell
57
what are transition elements
d block elements which form one or more stable ions that have incomplete d orbitals
58
electronic configuration of cr (24)
Cr: [Ar] 3d5 4s1
59
electronic configuration of Cu ( 29)
Cu: [Ar] 3d10 4s1
60
why Fe3+ is more stable than Fe2+
has an electronic configuration which has no electron repulsion in the partially filled d subshell
61
why successive ionization energies of d block elements increase
1st and 2nd ionization energy values of transition elements are similar as 1st and 2nd electron are removed from the same 4s orbital The 3rd electron is then removed from an inner subshell which has LESS SHIELDING and is closer to the nucleus so there is an increase in value of the 3rd ionization energy
62
complex ion
one with central positive ion surrounded by ligands which are datiively bonded
63
ligand
molecule or negative ion which has lone pair electrons and can use its lp electrons to form dative bonds to metal ions
64
why only transition metals form complex ions
transition metal ions are small and polarising since their nuclei are poorly shielded adn so they attract ligands strongly
65
explain d-d transitions
In an isolated transition metal all the d orbitals are at the same level. When a ligand binds with the transition metal ion the orbitals split into two different energy levels forming an energy gap. When electrons are promoted from a lower energy level to a higher one some frequencies of white light are absorbed and the remainder is reflected as the coliur that we see.
66
explain heterogenous catalyst with example
In a different state fromm the reactant platinium is an example aDsorption on the surface of the catalyst reactants bond length weakens and the activation energy deacreases reactants become product versions and they deabsorb from the active sites
67
expalin transition metal catalyst with example
ability comes from the availability of changing oxidation numbers SO2 + V2O5 --> SO3 + V2O4 ox no from +5 to +4 1/2 O2+ V2O4 --> V2O5 ox no from +4 to +5 again
68
explain homogenous catalyst with example
same state as teh reactants Fe2+ and persulphate overall rxn S2O8^2- + 2I^- --> 2SO4^2- +I2 ( this reaction is slow as to neagtive ions are trying to come together to react and repulsion increases the activation energy) first 2Fe^2+ +S2O8^2- --> 2SO4^2- + 2Fe^3+ second 2Fe^3+ + 2I^- --> 2Fe^2+ +I2

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