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inorganic chemistry year 2 > transition metals > Flashcards

transition metals Flashcards

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1
Q

define transition element

A

an element which forms at least one stable ion with a partially full d- shell of electrons

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2
Q

characteristic physical properties

A 
metallic
good conductors
hard
strong
shiny
high mp/bp
low reactivity
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3
Q

uses of iron

A

vehicle bodies

reinforce concrete

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4
Q

uses of titanium

A

jet engine parts

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5
Q

uses of copper

A

water pipes

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6
Q

characteristic chemical properties

A

variable oxidation states
coloured compounds in solution
good catalyst
form complex ions

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7
Q

complex ion

A

central transition metal ion surrounded by ligands that are coordinated bonded to it

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8
Q

catalysts in processes

A

iron - haber
vanadium oxide - contact
MnO2 - decomposition of H2O2

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9
Q

which electrons do transition metals lose first when forming ions

A

4s

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10
Q

define ligand

A

an ion or molecule with at least one lone pair of electrons, that donates them to a transition metal ion to form a coordinate bond and thus a complex ion

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11
Q

monodentate ligands

A

cl-
H2O
NH3
Cn-

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12
Q

ethanedioate

A 
..            ..
O -        O -
  \        /
   C -C
  / /      \\
O           O
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13
Q

ethane-1,2-diamine

A

:NH2 - CH2 - CH2 - :NH2

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14
Q

how many coordinate bonds does EDTA4- form

A

six

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15
Q

define coordination number

A

the number of coordinate bonds the metal ion has formed to surround the ligand

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16
Q

chelate effect

A

chelate complexes with multidentate ligands are favoured over monodentate ligands or ligands that form fewer coordinate bonds per molecule

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17
Q

chelate effect in terms of entropy

A

number of molecules increases when multidentate ligands , displace ligands that form fewer coordinate bonds per molecule
more stable complex ion formed

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18
Q

transition metal in water

A

Aqua ion, 6H2O ligands

octahedral

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19
Q

transition metal with two ligands

A

linear

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20
Q

transition metal with four ligands

A

tetrahedral

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21
Q

platin

A

square planar

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22
Q

conditions needed for a complex ion to display optical isomerism

A

octahedral with two or more bidentate ligands

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23
Q

haem

A

a molecule which makes up protein chains, with an Fe2+ central metal ion
coordination number = 6
4 of which bonds to porphyrin, 1 to nitrogen of a globin protein, 1 to oxygen

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24
Q

haemoglobin transport oxygen

A

O2 forms weak coordinate bond to the metal ion which is transported around the body. the bond breaks when haemoglobin reaches cells

25
Q

why is CO toxic

A

coordinately bonds to FE2+ and is a better ligand so bonds more strongly than O2
stops O2 from bonding so it can not be transported around the body

26
Q

why are transition metal compounds coloured

A

partially filled d orbitals
in compounds with ligands the d orbital splits into different energy levels
energy gap
see reflected light

27
Q

delta E

A

\

hf= hc/ /\

28
Q

how is delta E changed

A

oxidation state of metal
number/type of ligands
shape
coordination number

29
Q

VO2^+
VO^2 +
V^3+
V^2+

A

5+ yellow
4+ blue
3+ green
2+ violet

30
Q

what reduces vanadium

A

zinc

31
Q

what colour is Fe2+ aqua ion

A

green

32
Q

what colour is Fe3+ aqua ion

A

pale brown

33
Q

what colour is Cr2+ aqua ion

A

blue

34
Q

what colour is Cr3+ aqua ion

A

red/violet

35
Q

what colour is Co2+ aqua ion

A

brown

36
Q

what colour is Co3+ aqua ion

A

yellow

37
Q

what does a colorimeter do

A

measure the absorbance of a particular wavelength of light by a solution

38
Q

which oxidation states do all transition metals have except Sc

A

2+

39
Q

colour of MnO4^-

A

deep purple

40
Q

colour of MN2+

A

pink

41
Q

reduction of MnO4^-

A

MnO4^- + 8H+ +5e- = Mn2+ + 4H2O

42
Q

colour of Cr2O7^2-

A

orange

43
Q

colour of Cr3+

A

green

44
Q

reduction of Cr2O72-

A

Cr2O72- + 14H+ + 6e- = 2Cr3+ + 7H2O

45
Q

what happens to aqua metal ions in acidic conditions

A

they get reduced

46
Q

what happens to aqua metal ions in alkaline conditions

A

they get oxidised

47
Q

define a catalyst

A

a substance that increases the rate of a reaction without being chemically changed at the end of the reaction

48
Q

how do catalysts usually work

A

provide an alternative reaction pathway with a lower activation energy

49
Q

why are transition metals good catalysts

A

they can exist in variable oxidation states so can provide alternative pathways easily

50
Q

advantages of using a catalyst

A

allows reactions to proceed at lower temperatures and pressures

51
Q

metals used in catalytic converters

A

Pt
Rd
Pd

52
Q

heterogeneous catalyst

A

catalyst is in a different phase to the reactants

activity occurs on the solid surface as the reactants pass over it

53
Q

heterogenous catalysts work

A

reactants absorb the catalyst’s surface at active sites. this weakens bonds within the reactants, holds reactants close together on the surface and/or in the correct orientation to react. once the reaction has occurred, products desorb from active sites

54
Q

what is catalyst poisoning

A

unwanted impurities adsorb to the catalyst’s active sites and do not desorb
this blocks the active sites

55
Q

how can a catalyst be degraded

A

finely divided catalyst can be gradually lost from their support medium

56
Q

Haber process

A

N2 + 3H2 = 2NH3

iron catalyst

57
Q

contact process

A

SO2 + V2O5 = SO3 + V2O4

V2O4 + 1/2O2 = V2O5

58
Q

homogenous catalyst

A

catalyst that is in the same phase as the reactants

form intermediates to give a different reaction pathway with a lower activation energy

inorganic chemistry year 2 (3 decks)

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