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Chemistry > Transition Metals - Topic 15 > Flashcards

Transition Metals - Topic 15 Flashcards

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1
Q

transition elements characteristics

A
  • variable oxidation states
  • form complexes
  • used as catalysts
  • coloured compounds
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1
Q

how to transition metals arise

A

incomplete d sub shell in ions

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2
Q

cu and cr electronic config

A

4s1 3dx

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3
Q

zn forms which ion

A

2+

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4
Q

sc forms which ion

A

3+

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5
Q

what is monodentate ligand

A

a ligand that forms one coordinate bond when bonding to the central positive ion

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6
Q

monodentates examples

A

H2O, NH3, Cl-

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7
Q

bidentates examples

A

ethanedioate ion

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8
Q

charge of ethanedioate ion

A

2-

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9
Q

example of multi dentate ligand + how many coordination bonds

A

EDTA4-
6 coordination bonds

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10
Q

define ligand

A

atom, molecule, ion which can donate a lone pair

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11
Q

define complex

A

a central metal ion surrounded by ligands

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12
Q

why do colour changes arise

A

change in ox state
change in ligand
change in coordination number

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13
Q

when solution is blue, what light is absorbed

A

orange (opposite on colour wheel)

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14
Q

ligands do what to the orbitals in d subshell

A

five d orbitals split into two and three

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15
Q

common compounds with NO colour + why for each one

A

Zn2+ - full d shell, no electrons can move
Cu+ - full d shell, no electrons can move
Sc3+ - empty d shell, no electrons to move around

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16
Q

spectrophotometry method

A
  1. add ligand to intensify colour
  2. make solutions of known concentrations
  3. measure absorption/transmission
  4. plot calibration curve
  5. measure absorbance of unknown compound
  6. use relationship that concentration is proportional to absorbance and work out concentration.
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17
Q

cisplatin in body how does it bond

A

two chloride ions are displaced and it bonds onto dna

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18
Q

show cisplatin in body

A

Pt(NH3)2Cl2 + H2O –>(Pt(NH3)2Cl(H2O))+ + Cl-

Ligand substitution

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19
Q

how does cisplatin bond to dna

A

mix of dative and h-bonding

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20
Q

haem

A

ironII complex with multidentate ligand

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21
Q

shape with small ligands and say what the ligands are

A

octahedral
h2o and nh3

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22
Q

shape with large ligands and say the ligand

A

tetrahedral
cl-

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23
Q

shape that Ag+ forms + examples and their colours

A

linear
(Ag(NH3)2)+
(Ag(2sO3)2)3-
(Ag(CN)2)-

COLOURLESS ALL

24
Q

transition metals lose 4s or 3d first

A

4s

25
Q

why can transition metals receive and donate electrons

A

partially filled sub shell d

26
Q

compounds with low oxidation states are…

A

reducing agents

27
Q

compounds with high oxidation states are…

A

oxidising agents

28
Q

(VO2)+ ox state and colour

A

yellow
+5

29
Q

(VO)2+ ox state and colour

A

blue
+4

30
Q

V3+ ox state and colour

A

+3
green

31
Q

V2+ ox state and colour

A

+2
violet

32
Q

tell me about V with ox state +5

A

exists as solid compound in form of (VO3)- , usually as NH4VO3 (ammonium vanadate)
very strong ox agent
adding acid to the solution –> yellow (VO2)+ solution

33
Q

addition of zinc to vanadium (V) in acidic solution

A

down through each ox state
colour will change from yellow, blue, green, violet

34
Q

transition metals and ion formation across period trend is…

A

stability of 2+ ox state compared to 3+ increases across the period

35
Q

why does zinc reduce vanadium through all the ox states?

A

its electrode potential is more negative than all of vanadium’s electrode potential - will be oxidised and will reduce the vanadium

36
Q

Cr3+ colour

A

green

37
Q

Cr2+

A

blur

38
Q

zinc in HCl + (Cr2O7)2- produces…
conditions for one of the reactions and why

A

Cr3+ and Cr2+ (two separate equations)
hydrogen atmosphere for reduction to Cr2+, as oxygen in air will oxidise the Cr2+ to Cr3+

39
Q

(Cr2O7)2- colour

A

orange

40
Q

Fe2+ and (Cr2O7)2-

A

less strong reducing agent than zinc
reduces chromate to Cr3+

41
Q

how can the cr2+ state be stabilised

A

forming stable complex ion with ligand like the ethanoate ion

42
Q

cr2+ ion bubbled through sodium ethanoate…

A

red precipitate STABLE

43
Q

more positive electrode potential means…

A

reduced

44
Q

transition metals with low oxidation states are easier to be oxidised in…and why

A

alkaline solutions than in acidic
form negative ions, and electrons are easier to remove from negative ions

45
Q

what alkali to add to transition metals

A

H2O2
NaOH

46
Q

half equations in alkaline conditions…

A

KOHES but ADD OH- TO CANCEL OUT THE H+

47
Q

chromate dichromate equilibrium

A

(CrO4)2- + 2H+ double headed arrow Cr2O7 2- + H2O

48
Q

What is the colour of (CrO4)2-

A

yellow

49
Q

addition of zinc and HCl OR Fe2+ and acidified HCl to dichromate

A

(Cr(H2O)6)3+ green solution

50
Q

Lewis acid and base in complexes

A

Lewis acid: metal ion
Lewis base: ligand

51
Q

colour of (Fe(H2O)6)2+ solution

A

green

52
Q

colour of (Co(H2O)6)2+ solution

A

pink

53
Q

colour of (Cu(H2O)6)2+ solution

A

blue

54
Q

colour of (Cr(H2O)6)3+ SOLID

A

ruby

55
Q

colour of (Fe(H2O)6)3+ SOLID

A

violet

56
Q

colour of (Fe(H2O)6)3+ solution

A

yellow/brown

57
Q

colour of (Cr(H2O)6)3+ solution

A

green

Chemistry (3 decks)

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