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transition metals Flashcards

1
Q

appearance of [Cu(NH3)4(H2O)2]2+

A

dark blue solution

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2
Q

appearance of [Cu(H2O)6]2+

A

light blue solution

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3
Q

appearance of Cu(OH)2

A

light blue precipitate

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4
Q

appearance of Cu2O

A

brick red

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5
Q

CuI appearance

A

white

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6
Q

appearance of [CuCl4]2-

A

yellow/green solution

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7
Q

how to get from [Cu(H2O)6]2+ to [Cu(NH3)4(H2O)2]2+

A

excess NH3

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8
Q

how to get from [Cu(H2O)6]2+ to Cu(OH)2

A

NH3/NaOH

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9
Q

how to get from Cu(OH)2 to [Cu(H2O)6]2+

A

H2O/H+

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10
Q

definition of a transition metal

A

elements with an incomplete d-sub shell that can form at least one stable ion with an incomplete d subshell

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11
Q

which d block elements are not transition metals

A

scandium and zinc

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12
Q

electron configuration of the ion sc forms

A

sc3+ (Ar)3d0

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13
Q

electron configuration of the ion zn forms

A

Zn 2+ (Ar)3d10

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14
Q

which transition metals have different electronic configuration to what youd expect

A

Cr and Cu

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15
Q

4s orbitals are filled before 3d ones but which are lost first

A

4s

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16
Q

Cr electron configuration

A

[Ar] 3d5 4s1

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17
Q

Cu electron configuration

A

[Ar] 3d10 4s1

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18
Q

Cr3+ aqua ion solution with NaOH

A

[Cr(H20)6]3+ violet solution

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19
Q

Fe2+ aqua solution

A

[Fe(H20)6]2+ green solution

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20
Q

Fe3+ aqua solution

A

[Fe(H20)6]3+ yellow solution

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21
Q

Mn2+ aqua ion solution

A

[Mn(H20)6]2+ pale pink solution

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22
Q

Cu2+ aqua ion solution

A

[Cu(H20)6]2+ blue solution

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22
Q

cr3+ reacting with NaOH/NH3

A

Cr(OH)3(H2O)3 green precipitate

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23
Q

Cr3+ with excess NaOH/NH3

A

NaOH [Cr(OH)6]3- green solution
NH3 [Cr(NH3)6]3+ purple solution

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24
Q

Fe2+ with NaOH/NH3

A

Fe(OH)2(H2O)4 green precpitate

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25
Q

Fe3+ with NaOH/NH3

A

Fe(OH)3(H2O)3 brown precipitate

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26
Q

Cu2+ with NaOH/NH3

A

Cu(OH)2(H2O)4 blue precipitate

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26
Q

MN2+ with NaOH/NH3

A

Mn(OH)2(H2O)4 pale brown precipitate

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27
Q

[Fe(H2O)6]2+ +2OH-

A

2H2O + [Fe(OH)2(H2O)4]

27
Q

which ion changes colour/state when adding EXCESS OH- ions

28
Q

which ion changes colour/state when adding EXCESS NH3 ions

A

Cr3+ and Cu2+

29
Q

Cr3+ with excess NH3

A

[Cr(NH3)6]3+ purple solution

30
Q

Cu2+ with excess NH3

A

[Cu(NH3)4(H2O)2]2+

31
Q

[Fe(H2O)6]2+ + 2NH3 =

A

[Fe(H2O)2(OH)4] +2NH4+

32
Q

[Cu(OH)2(H2O)4]2+ + 4NH3 =

A

[Cu(NH3)4(H2O)2]2+ + 2H2O + 2OH-

33
Q

monodentate ligands

A

can only form one dative covalent/ coordinate bond to the central metal ion

34
Q

4 examples of monodentate ligands

A

H2O
NH3
CN-
Cl-

35
Q

why can bidentate ligands form 2 dative covalent bonds with the central metal ion

A

because each ligand contains two atoms with lone pairs of electrons

36
Q

what shape are 4 coordinate complexes with chlorine

A

tetrahedral

36
Q

what shape are 6 coordinate complexes and what shape are they

A

octahedral 90

37
Q

which metals form 4 coordinate complexes as square planar shapes

42
Q

what bonding is there within the complex ion [Cu(H2O06]2+

A

covalent (in water molecule) and dative covalent bond (between water and ligand)

43
Q

why may a reaction not be reversible

A

large increase in entropy and is irreversible due to effect on Gibbs free energy equation

44
Q

optical isomerism definiton

A

type of stereoisomerism found in molecules that contain a chiral centre. they are non superimposable mirror images of each other

45
Q

4 properties of transition metal

A

form complexes
good catalysts
form coloured ions in solutions
variable oxidation states

46
Q

when can Cu2+ be used as a catalyst

A

reactions between zinc and an acid

47
Q

When can MnO2 be used as a catalyst

A

decomposition of H2O2

48
Q

pro and con of transition metal catalyst

A

reduce energy uses
increased risk from toxicity of traction metals

49
Q

enantiomer

A

optical isomer

50
Q

ligand

A

molecule/ion with a lone electron pair that can form dative covalent / coordinate bonds with a central metal ion by donating of this electron pair

51
Q

when is an ion colourless

A

when there are no available electrons to excite, no united/partially filled orbital

52
Q

octahedral bond angle

53
Q

what is the cis isomer of ptcl2NH3 used as

A

cancer therapy drug

54
Q

are dashes at the front or back

A

dashes at the back
wedges at the front

55
Q

do wedges get bigger or smaller

A

bigger as they move away from central metal ion

56
Q

cis platin is bad even though it is a cancer therapy drug because…….

A

it can cause side effects like hairless. It needs to be administered in small amounts

57
Q

central metal ion in Haem

58
Q

what type of ring does Haem have

A

tetradentate porphyrin ring

59
Q

what structure/ bond angle does Haem have

A

octahedral 90

60
Q

what kind of reaction occurs when CO replaces O2 bound to Haem

A

ligand substation reaction

61
Q

chelate effect

A

positive entropy change is more favourable as a more stable complex is formed. Great entropy=more negative free energy change and more favourable the reaction

62
Q

enthalpy change for ligand substitution reactions

A

very small, near to zero

63
Q

what colour is (Cr2O7)2-

A

orange solution

64
Q

how do you change (Cr2O7)2- to [Cr(H2O)5SO4]+

A

you need to add Zn

65
Q

what colour is [Cr(H2O)6]2+

A

blue solution ( at zinc to [Cr(H2O)5SO4]+) do not confuse with the 3+ charge one which is a violet solution

66
Q

what colour is CrO4 2-

A

yellow solution

67
Q

how to get CrO4 2- from [Cr(H2O)5SO4]+

A

add H2O2/OH-

68
Q

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

A

very pale green solution

69
Q

what colour is MnO4

A

purple solution

70
Q

How to get from [Fe(H2O)6]3+ to [Fe(H2O)6]2+ and colour change

A

yellow to pale green solution
Add I-

71
Q

why do some elements like Al only form compounds in which its oxidation number is 3+ but there’s form compounds with a v variety of oxidation numbers

A

there are several removable d electrons of similar energies

chemistry (16 decks)

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