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Chemsitry > Transition Metals > Flashcards

Transition Metals Flashcards

1
Q

What is a complex

A

A species in which a number of molecules or anions are bonded to a central metal ion by dative covalent bond

Has no overall charge

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2
Q

What is a complex ion

A

Ion in which a number of molecules or anions are bound to a central metal atom by dative covalent bonds

Has an overall charge

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3
Q

What is a ligand

A

Molecule or anion that donates a lone pair of electrons to form a dative covalent bond with a central metal cation

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4
Q

What is Co- ordination number

A

The number of dative covalent bonds formed in a complex

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5
Q

What shape and bond angle is formed with a 6 co-ordination number

A

Octahedral

90degrees

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6
Q

What shape and bond angle is formed with a 4 co-ordination number

A

Tetrahedral
109.5 degrees

OR

Square planar
90 degrees

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7
Q

Which 4 co-ordinate number shape is most common and when is the other formed

A

Tetrahedral is more common

Square planar formed with two seperate monomers

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8
Q

What shape and bond angle is formed with a 2 co-ordination number

A

Linear
180 degrees

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9
Q

What is a monodenate ligand

A

Form one co-ordinate bond per ligand

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10
Q

What is a bidenate ligand

A

Forms two co-ordinate bonds per ligand

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11
Q

What is a multidenate ligand

A

Forms more than two co-ordinate bonds per ligand

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12
Q

When is E/Z isomerism used

A

When there are more than two different groups attached around a C=C double bond

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13
Q

What is cis/trans isomerism

A

When there are only two different groups around a C=C double bond

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14
Q

Formula shape and bond angle of cis-platin

A

[Pt(Cl)2(NH3)]
Square planar
90 degrees

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15
Q

Use of cis-platin

A

Can be used to stop replication of cancerous cells by binding to them

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16
Q

Why is trans platin not used

A

Toxic and ineffective drug

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17
Q

Why does the d-orbital split in transition metal complexes

A

When ligand approach the metal ion, electrons in the ligand repel the electrons in the d-orbital of the metal ion

Causes d sub-shell to split

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18
Q

Why is there colour in transition metal complexes

A

The electrons absorb UV and are excited into space in orbitals above
The change in energy due to this corresponds to UV/ visible light

Colour we see is a mixture of what is not absorbed

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19
Q

How is colour seen predicted

A

Using the colour wheel

Colour seen is opposite to colour absorbed

20
Q

Why is no colour seen in Sc and why is it not a transition metal

A

No electrons to be promoted
Therefore no colour seen
Thus not a transition metal

21
Q

Why is no colour seen in Zn and why is it not a transition metal

A

No space in d-orbitals for electron promotion
Therefore no colour
Thus not transition metal

22
Q

Which subshell loses electrons first transition metal

A

4s electrons lost before 3d electrons

23
Q

Definition of a transition metal

A

A transition metal is an element that has one or more stable ions with partially filled d orbitals

24
Q

Colour of Cr 3+ ion

A

Violet

25
Q

Colour of Fe 2+ ion

A

Green

26
Q

Colour of Fe 3+ ion

A

Yellow

27
Q

Colour of Cu2+ ion

A

Blue

28
Q

Colour of Co2+ ion

A

Pink

29
Q

Colour of Cr3+ and drops of NaOH/HCl

A

Green

30
Q

Colour of Fe2+ and drops of NaOH/HCl

A

Green precipitate

Oxidises to brown in air

31
Q

Colour of Fe3+ and drops of NaOH/HCl

A

Brown precipitate

32
Q

Colour of Cu2+ and drops of NaOH/HCl

A

Blue precipitate

33
Q

Colour of CO2+ and drops of NaOH/HCl

A

Blue precipitate

34
Q

Colour of Cr3+ and excess NaOH

A

Green solution

35
Q

Colour of Cr3+ and excess NH3

A

Purple solution

36
Q

Colour of Cu2+ and excess NH3

A

Deep blue solution

37
Q

Colour of Co2+ and excess NH3

A

Brown solution

Oxidises in air to form yellow solution

38
Q

Colour of Cu2+ and conc HCl

A

Yellow

39
Q

Colour of Co2+ and conc HCl

A

Blue solution

40
Q

What factors affect the colour in a complex ion

A

The identity of the metal
Oxidation state of the metal
Identity of the ligands
Co- ordination number

41
Q

What is Ligand exchange

A

When one or more ligands are replaced by other ligands

42
Q

What can ligand exchange cause

A

A change in co-ordination number

A change in colour

43
Q

When is ligand exchange actually acid base

A

When adding a few drops of OH- or NH3, the OH- or NH3 removes H+ ions from some of the water molecules

44
Q

Reaction of hexaaquacopper and a few drops of dilute ammonia

A

[Cu(H2O)6]2+ + 2NH3 becomes [Cu(H2O)4(OH)2] + 2NH4+

45
Q

Reaction of tetraaquabihydroxycopper and excess ammonia

A

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

46
Q

Reaction of hexaaquacopper (II) and concentrated HCl

A

[Co(H2O)6]2+ + 4HCl becomes [Co(Cl)4] + 6H2O + 4H2

47
Q

Why does hexaaquacopper (II) change into tetrachlorocuprate (II)

A

Because of the size of the Cl- ion, only four can fit around a central metal ion

Chemsitry (15 decks)

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