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Chemistry UNIT 3 > 3.4 - D Block Transition metals > Flashcards

3.4 - D Block Transition metals Flashcards

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1
Q

Transition metal?

A

metal with a partially filled D orbital

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1
Q

Orbitals of transition metals?

A

Ti to Zn all with an Ar core

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2
Q

what are the only exceptions?

A

copper + chromium as there is only a small difference between the energy of 3d and 4s
more energy is required to pair up the electrons to create a half filled D orbital and a fully filled D orbital

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3
Q

electron configuration for Fe

A

4S2 3D6

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4
Q

Electron configuration for Fe2+

A

4S03D6

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5
Q

Electron configuration for Fe3+

A

4S03D5

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6
Q

Where are electrons lost from first?

A

4S orbital first

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7
Q

Oxidation states for transition metals?

A
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8
Q

Sc?

A

+3 - common and only 1

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9
Q

Ti

A

+3 and + 4
+1 and +2

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10
Q

V?

A

+ 2+3+4,+5
+1

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11
Q

Cr?

A

+3 and +6
+1, +2,+4, and +5

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12
Q

Mn?

A

+2,+3+4,+6,+7
+1,+5

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13
Q

Fe?

A

+2, +3
+1,+4+5,+6

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14
Q

C?

A

+2,+3
+1,+4,+5,+6

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15
Q

Ni?

A

+2
+1,+3,+4

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16
Q

Cu?

A

+1,+2
+3

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17
Q

Zn?

A

+2

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18
Q

What is a Ligand?

A

a small molecule with a lone pair that can form a bond to a transition metal

H2O
NH3
Cl

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19
Q

What are 2 forms of transition metals?

A

Octahedral + Tetrahedral

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20
Q

what colour is
(Fe(H2O)6)2+

A

Pale green complex

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21
Q

what colour is
(Fe(H2O)6)3+

A

Yellow complex

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22
Q

What colour is (Cu(H2O)6)3+

A

Blue complex

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23
Q

What colour is
(Cr(H2O)6)3+?

A

dark green complex

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24
Q

What colour is (Co(H2O)6)2+?

A

Pink complwx

25
Q

What does adding Ammonia solution to (Cu(H20)62+ cause?

A

4 ammonium molecules to replace the water molecules which form (Cu(NH3)4(H20)2+ which is a royal blue complex

26
Q

What is cobalt chloride used for?

A

Test for H20
colour change is blue to pink

27
Q

formula for it?

A

(CoCl4)2- —– (Co(H2o)6)2+

28
Q

How is the complex formed?

A

when Cu2+ or Co2+ reacts with concentrated HCL which displaces the water molecules
this causes a colour change which is due to the absorption of light
Cu2+ goes from blue to yellow to green and cobalt goes from pink to blue

29
Q

What is a ligand exchange?

A

when a transition metal ion is exposed to a mixture of ligands such as an aqeous solution of Chloride, ligands can be exchanged to form new complexes
This is Le chatelier’s principle

30
Q

What is the equation for this?

A

(Cu(H20)6)2+ + 4NH3——(Cu(NH3)4(H2O)6)2+ + 4H2O

31
Q

According to Le Chatelier’s principle what does adding ammonia do?

A

fores the equilibrium to the right, which produces more of (Cu(NH3)4(H2O2)2+
Adding water forces the equilibrIum to the left which produces more of Cu(H2O)2+

32
Q

What is the equation?

A

(CoCH20)6)2+ + 4Cl- ——- (CoCl4)2- + 6H20

33
Q

What is the colour of transition metal complexes?

A

always coloured but in the absence of ligands around the metal ion, the compound would be colourless

34
Q

What effect does the ligands have when introduced to the metal ion?

A

a significant effect as without ligands, the transition metals have 5 degenerate orbitals where all the orbitals have the same energy

35
Q

In an octahedral complex what happens?

A

6 negatively charged ligands approach the transition metals along the 3 axis DX, DY DZ
the negative charges repel the electrons in the orbitals which make the orbitals unstable and now no longer degenerate as each have a different energy
causing the 5 degenerate orbitals to split into 2 higher energy levels and 3 lower energy levels

36
Q

What must an electron in the D Orbital now move from the lower to the higher?

A

gain energy through the absorption of light

37
Q

When is only 1 frequency of light absorbed?

A

corresponds to the energy gap between the orbitals
energy is found from E=Hf

38
Q

what does the D-D transition metals depend on?

A

the splitting and the D- orbitals and this varies between ions of different transition metals

39
Q

What happens if the splitting varies?

A

the frequency of the colour of light absorbed also varies
Cu(H2O)6) 2+ is typically blue so absorbs all colours apart from blue

40
Q

What does Cu+ complexes have?

A

a full D orbital so there are no empty orbitals to allow the electrons to move so Copper (I) does not absorb light in the visible range so appears colourless

41
Q

What is Iron used in?

A

Haber Process to produce Ammonia from Nitrogen to Hydrogen

42
Q

What is the formula?

A

N2(g) + 3H2(g)—-2NH3(g)

43
Q

When is Nickel used?

A

Hydrogenation of vegetable oil to form margerine

44
Q

When is Vanadium Oxide used?

A

in the contact process fot the production of H2SO4

45
Q

MnO2?

A

used in the catalytic decomposition of H202

46
Q

Why are Catalysts needed?

A

to save money, energy + time

47
Q

What is a catalyst?

A

a substance which increases the rate of a chemical reaction by providing an alternate pathway with a lower activation energy

48
Q

What is a homogenous catalyst?

A

A catalyst that is in the same physical phase as tHe reactants e.g V2O5

49
Q

Heterogenous Catalyst?

A

a catalyst that is in a different state as the reactants

50
Q

Why do transition meals act as Catalysts?

A

1) have empty orbitals
2) have variable oxidation states

51
Q

What increases the reactivity of the bonded species?

A

when molecules with lone pairs can form coordinate bonds with the metal atom
or brings the 2 reactive molecules closer together
( heterogenous provide a solid surface where molecules = adsorbed)

52
Q

Def of adsorbed?

A

attatched to the surface

53
Q

What does having variable oxidation states do?

A

allow a metal ion to act as a catalyst in a redox reaction
(the metal is either the oxidising or reducing agent)

54
Q

What do homogenous catalysts form?

A

coordinate bonds with the reactants and use their variable oxidation states to oxidise or reduce

55
Q

Reaction of Cr3+ with NaOH?

A

ion = Cr3+
Colour of solution = pale green
Green/grey ppt is formed when NaOH is formed
when excess NaOH is added, ppt redissolves to form green solution

56
Q

Reaction of Fe2+ with NaOH

A

Pale green solution
Dark green ppt is formed when NaOH is added
nvc in excess NaOH

57
Q

Reaction of Cu2+ with NaOH?

A

colour of solution is blue
Pale blue PPT is formed when NaOH is added
NVC when IN excess NaOH

58
Q

Equation for Cr3+?

A

Cr3+(aq) + 3OH-(aqO —— Cr(OHo3
GREEN GREY PPT
Cr(OH)3 + 3OH-)(aqO —– Cr(OH)6)3-
GREEN SOLUTION

59
Q

Equation for Fe2+?

A

Fe2+(aq)+ 2OH-(aq) —–Fe(OH)2)S
DARK GREEN

60
Q

Equation for Fe3+?

A

Fe3+(aq)+3OH-(aq)—- Fe(OH)3(s)
Rust brown

61
Q

Equation for Cu2+?

A

Cu2+(aq) + 2OH-(aq) ——- Cu(OH)2(s)
pale blue

Chemistry UNIT 3 (7 decks)

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