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Chemistry > D block elements > Flashcards

D block elements Flashcards

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1
Q

Sc3+

A

Colourless

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2
Q

Ti4+

A

Colourless

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3
Q

Cr3+

A

Violet

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4
Q

Mn2+

A

Pale pink

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5
Q

Fe3+

A

Brown yellow

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6
Q

Fe2+

A

Pale green

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7
Q

Co2+

A

Pink

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8
Q

Ni2+

A

Green

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9
Q

Cu2+

A

Blue

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10
Q

Cu+

A

Colourless

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11
Q

Zn2+

A

Colourless

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12
Q

MnO4-

-

A

Purple

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13
Q

MnO42-

A

Green

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14
Q

CrO42-

A

Yellow

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15
Q

Cr2O72-

A

Orange

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16
Q

Transition and non-transition d block elements

A

d block elements contain incompletely filed d subshell at elemental state or with the ability to form at least one stable ion with incompletely filled d subshell are called transition elements. Therefore, d block elements producing ions only with d10 configurations are considered as non-transition elements.(Zn,Cd,Hg)

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17
Q

Properties of transition elements

A

Has less variations in atomic radii than main group elements. The atomic radii decreases slightly and then increase.
Nuclear charge increases across a group.
But at the end elements like Zn, Cu atomic radii increases as repulsion between electrons are high due to the pairing of electrones.

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18
Q

Which d block element has the highest melting point

A

Cr- theoretical value
V- practically
Higher the number of unpaired electrons higher the melting point (refer)

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19
Q

Mn3+

A

Violet

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20
Q

V2+

A

violet

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21
Q

V3+

A

green

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22
Q

Ti3+

A

purple

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23
Q

NO

A

nitrosyl- neutral

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24
Q

CO

A

carbonyl- neutral

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25
Q

C2H5N

A

pyridine-neutral

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26
Q

MnO2

A

Dark brown/black

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27
Q

under acidic conditions, MnO4- reduces to

A

Mn2+.

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28
Q

H3O+

A

Hydronium

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29
Q

What is coordination number

A

The no. of coordination bonds formed between the central metal ion and ligands.
Depends on size, charge, nature of the ligand and the electronic configuration of the central metal ion.

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30
Q

Factors affecting the color of complexes

A

Central metal ion, oxidation state of the central metal ion and the nature of the ligand

31
Q

Colors of complexes

Aqueous

A

Same color as the metal ion

32
Q

Cr(OH)3

A

Blue-green

33
Q

Mn(OH)2

A

white/ cream

34
Q

Fe(OH)2

A

Dirty green

35
Q

Fe(OH)3

A

Reddish-brown

36
Q

Co(OH)2

A

Pink

37
Q

[Co(OH)4]2-

A

Deep-blue

38
Q

Ni(OH)2

A

green

39
Q

Cu(OH)2

A

Blue

40
Q

Zn(OH)2

A

white

41
Q

[Zn(OH)4]2-

A

Colorless

42
Q

Cr(OH)3 -NH3

A

Blue-green

43
Q

Mn(OH)2 -NH3

A

White/ cream

44
Q

Fe(OH)2 -NH3

A

Dirty green ppt

45
Q

Fe(OH)3 -NH3

A

Reddish-brown ppt

46
Q

[Co(NH3)6]2+

A

yellowish-brown

47
Q

[Co(NH3)6]3+

A

Brownish-red

48
Q

[Ni(NH3)6]2+

A

Blue

49
Q

[Cu(NH3)4]2+

A

Deep blue

50
Q

[Zn(NH3)4]2+

A

Colourless

51
Q

[CrCl6]3-

A

Blue-violet

52
Q

[MnCl4]2-

A

Greenish yellow

53
Q

[FeCl4]-

A

Yellow

54
Q

[Co(Cl)4]2-

A

Blue

55
Q

[NiCl4]2-

A

Yellow

56
Q

[CuCl4]2-

A

Yellow

57
Q

[ZnCl4]2-

A

Colourless

58
Q

[Cr(H2O)6]3+ + 3NH3 (aq)

A

Cr(OH)3(s) + 3NH4+(aq) + 3H2O(l)

Blue-green gelatinous ppt

59
Q

[Co(H2O)6]2+(aq) + 2OH-(aq)

A

Co(OH)2(s) + 6H2O(l)

Pink ppt

60
Q

Co(OH)2(s) + 2OH-(aq)

A

[Co(OH)4]2-(aq)

Deep blue solution

61
Q

[Co(H2O)6]2+(aq) + 6NH3 (aq)

A

[Co(NH3)6]2+(aq) + 6H2O(l)
Forms a yellowish-brown solution however due to the auto oxidation it forms[Co(NH3)6]3+(aq) which is brownish-red in colour.

62
Q

Co(H2O)6]2+(aq) + 4Cl-(aq)

A

[CoCl4]2-(aq) + 6H2O(l)

Forms a blue solution

63
Q

[Ni(H2O)6]2+(aq) + 2OH-(aq)

A

Ni(OH)2(s) + 6H2O(l)

Forms a green precipitate

64
Q

[Ni(H2O)6]2+(aq) + 6NH3 (aq)

A

[Ni(NH3)6]2+(aq) + 6H2O(l)

Forms a deep-blue solution

65
Q

[Ni(H2O)6]2+(aq) + 4Cl-(aq)

A

[NiCl4]2-(aq) + 6H2O(l)

Forms a yellow solution

66
Q

[Mn(H2O)6]2+(aq) + 2OH-(aq)

A

Mn(OH)2(s) + 6H2O(l)

Forms white/cream ppt

67
Q

[Fe(H2O)6]3+(aq) + 3OH-(aq)

A

Fe(OH)3(s) + 6H2O(l)

Forms reddish-brown ppt

68
Q

[Cu(H2O)6]2+(aq) + 2OH-(aq)

A

Cu(OH)2(s) + 6H2O(l)

Pale blue solution turns into blue solution

69
Q

[Cu(H2O)6]2+(aq) + 4NH3(aq)

A

[Cu(NH3)4]2+(aq) + 6H2O(l)

Forms a deep-blue complex

70
Q

[Cu(H2O)6]2+(aq) + 4Cl-(aq)

A

[CuCl4]2-(aq) + 6H2O(l)

Solution turns yellow

71
Q

[Zn(H2O)6]2+(aq) +2OH-(aq)

A

Zn(OH)2(s) + 6H2O(l)

Colorless solution turns in to a white precipitate.

72
Q

Metal cations which forms precipitates with Cl

A

Pb
Ag
Hg

73
Q

Colors of carbonates formed by group 2 metals

A

All carbonates formed by group 2 metals are white.

Chemistry (15 decks)

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