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A2 Chemistry > Transition Metals > Flashcards

Transition Metals Flashcards

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1
Q

what is a transition metal?

A

metals that can form one or more stable ions w a partially filled d sub-shell

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2
Q

where are transition metals found in periodic table?

A

d-block

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3
Q

which orbital fills first 3d or 4s? And what is the exception in two transition metals?

A

4s fills first
Cr and Cu are exceptions
- Cr prefers to have 1 electron in each orbital of 3d sub-shell & just 1 in 4s sub-level, gives it more stability
- Cu prefers to have full 3d sub-level and just 1 electron in 4s sub-level, more stable

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4
Q

which orbital are electrons lost first from, 3d or 4s?

A

4s

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5
Q

why aren’t Sc and Zn transition elements?

A

Sc forms one ion Sc^3+ which has an empty 3d sub-level
Zn forms one ion Zn^2+ which has a full 3d sub-level
(transition metals form stable ions with PARTIALLY filled d sub-levels)

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6
Q

physical properties of transition metals

A

high density
high MP and BP
‘same’ ionic radii (more or less)

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7
Q

chemical properties of transition metals

A

they act as good catalysts
they exist in variable oxidation states
they can form complex ions
they can form coloured ions in solution

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8
Q

why do transition metals have variable oxidation states?

A
  • the electrons sit in 4s and 3d energy levels which are very close
  • so electrons are gained and lost using similar amount of energy when they form their ions
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9
Q

what ions do Scandium form and state oxidation states?

A

Sc^3+ (Oxidation state: +3)

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10
Q

what ions do Vanadium form and state oxidation states?

A

V2+ (+2), V^3+ (+3), VO^2+ (+4), VO2+ (+5)

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11
Q

what ions do Chromium form and state oxidation states?

A

Cr^3+ (+3) and Cr2O7^2- (+6)

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12
Q

what ions do Manganese form and state oxidation states?

A

Mn^2+ (+2) and MnO4- (+7)

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13
Q

what ions do Iron form and state oxidation states?

A

Fe^2+ (+2) and Fe^3+ (+3)

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14
Q

what ions do Cobalt form and state oxidation states?

A

Co^2+ (+2)

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15
Q

what ions do Nickel form and state oxidation states?

A

Ni^2+ (+2)

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16
Q

what ions doCopper form and state oxidation states?

A

Cu^2+ (+2)

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17
Q

what ions do Zinc form and state oxidation states?

A

Zn^2+ (+2)

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18
Q

state colours of vanadium ions formed

A

V2+ violet when surrounded by 6H2O, they’re normally substituted so usually look green
V^3+ green
VO^2+ blue
VO2+ yellow

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19
Q

state colours of chromate and dichromate ions formed

A

Cr2O7^2- orange

Cr^3+ violet, 6H20 usually substituted so appears green sometimes

20
Q

state colours of Manganate ions formed

A

MnO4^- purple

Mn^2+ pale pink

21
Q

state colours of Iron ions formed

A

Fe^2+ pale green

Fe^3+ orange/yellow

22
Q

state colours of Cobalt ion formed

A

Co^2+ pink

23
Q

state colours of Nickel ion formed

A

Ni^2+ green

24
Q

state colours of Copper ion formed

A

Cu^2+ blue

25
Q

what is a complex?

A

central atom or ion surrounded by co-ordinatedly bonded ligands

26
Q

what is a co-ordinate bond?

A

(or dative covalent bond)
covalent bond where both electrons are in shared pair come from SAME atom
- in a complex they come from the ligands

27
Q

what is a ligand?

A
  • atom/ion/molecule that donates a pair of electrons to central transition metal ion to form a co-ordinate bond
    (they must have at least 1 pair of lone electrons)
  • can be monodentate, bidentate or polydentate
28
Q

what is the co-ordinate number?

A

the number of co-ordinate bonds that are formed with the central metal ion
(not the number of ligands)

29
Q

monodentate ligands

A 
ligands which have one lone pair of electrons 
examples:
H2O:
\:NH3
\:Cl-
30
Q

bidentate ligands

A

ligands which have two lone pairs of electrons
examples:
ethanedioate C ₂O²⁻ ₄
ethane-1,2-diamine C₂H₄(NH₂)

31
Q

multidentate ligands

A

ligand capable of donating two or more pairs of electrons (to from co-ordinate bonds)
examples:
Haem
EDTA^4- (forms 6 co-ordinate bonds w central metal ion)

32
Q

which are small ligands and what does this mean for complex shapes?

A

H2O:
:NH3

  • means 6 can fit around central metal ion forming octahedral shape (bond angles 90 degrees)
33
Q

which are bigger ligands and what does this mean for complex shapes?

A

:Cl-

  • can only fit 4 ligands around central metal ion (usually forming tetrahedral shape, bond angle is 109.5 degrees, BUT can also form square planar e.g. cisplatin bond angles 90 degrees)
34
Q

what kind of size are these ligands: ethanedioate and ethane-1,2-diamine? and how many can fit around a central ion?

A
  • they are ‘larger’ (than the other ones e.g. :Cl-)

- three

35
Q

complexes with co-ordinate number two form what coplex shapes? Give an example

A
  • form linear shapes (bond angle is 180 degrees)

- some silver complexes e.g. [Ag(NH3)2}+ (this is tollens reagent/silver mirror)

36
Q

How do you work out oxidation state of metal ion?

A

total oxidation state - total oxidation state of ligands

37
Q

a complex’s overall charge is the same as its what?

A

its total oxidation state (number and charge outside square bracket)

38
Q

what is haem?

A

a multidentate ligand that is found in molecule haemoglobin

39
Q

what is haemoglobin?

A

quarternary protein used to transport oxygen around body in blood

40
Q

what do the ligands NH3 and H2O have in common?

A

similar in size and are uncharged

41
Q

exchnage of ligands NH3 and H2O occurs without what?

A

without change of co-ordination number (eg Co2+ and Cu2+)

42
Q

what occurs when you dissolve the salt of a transition metal in water?

A
  • becomes surrounded by water molceules acting as ligands

called aqua ions

43
Q

what kind of isomers can transition metals form?

A

optical isomers and geometric (E-Z) isomers

44
Q

what kind of complexes does geometric isomerism occur in?

A

octahedral and square planar

45
Q

in what complexes does optical isomerism occur?

A
  • this occurs when there are two or more bidentate ligands in a complex

A2 Chemistry (9 decks)

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