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Chemistry > TRANSITION METAL CHEM > Flashcards

TRANSITION METAL CHEM Flashcards

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1
Q

to oxidise a tm to a higher oxidation state what must you add

A

an alkali followed by an oxidising agent

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2
Q

how woukd you stabilise a tm with a low oxidation state such as fe2+

A

place in acidic conditions

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3
Q

define a tm

A

a partially filled d orbital

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4
Q

what are some chemical properties of a tm

A

variable oxidation states
partially filled d orbitals
form colourful compounds
can form complex ions
they are good catalysts

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5
Q

what is a ligand

A

will donate a pair of electrons around the central metal ion to form coordinate bonds

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6
Q

what is a monodentate ligand

A

has only one coordinate bond around the central metal ion

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7
Q

what is the coordination number of a complex ion

A

how many coordinate bonds the ion has

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8
Q

can a bidentate ligand form optical isomers

A

yes

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9
Q

define a bidentate ligand

A

donates two electron pairs to a tm from different atoms on the same molecule

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10
Q

define entropy

A

amount of disorder in a system

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11
Q

what happens when you add EDTA to a solution of TM salts

A

the EDTA will replace all six water ligands in the hexa-aqua ion

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12
Q

how can a more stable complex form

A

increase entropy

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13
Q

describe what a cis molecule looks like

A

same side

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14
Q

describe what a trans molecule looks like

A

across from one another

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15
Q

which is larger ammonium ion or chloride ion

A

chloride - this will affect shape - and effect hoe many ions can fit around the central metal ion

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16
Q

are scandium and zinc tms

A

no - because they do not have partially filled d orbitals - they are full when they form stable ions
sc3+ has the configuration as Ar
Zn2+ - Ar 3d10 4s2

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17
Q

what are some physical properties of a tm

A

high density
high melting and boiling points

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18
Q

what type of isomerism is optical isomerism

A

stereoisomerism

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19
Q

define stereoisomerism

A

same molecular formula but different orientation of their bonds in space

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20
Q

how does colour arise in a tm

A

electronic transition from the ground state to the excited state. visible light is absorbed to promote these d-electrons to go to higher states. the light that is not absorbed is transmitted through a solution or reflected in a solid to give colour

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21
Q

what is the equation for the speed of light

A

speed of light = wavelength x frequency
c=lamda x f

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22
Q

what does the frequency of light absorbed depend upon

A

the energy difference between levels

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23
Q

what effects energy in an ion complex

A

the oxidation state of the central metal ion
ligands - shape -
- coordination number

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24
Q

do ligands intensify colour

A

yes

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25
Q

how do you dimerise a complex

A

add acid

26
Q

how do you monomerise a complex

A

add an alkali

27
Q

when oxidising low oxidation states why is an alkali added

A

there is a greater tendency to form negative ions
OH-

28
Q

explain the steps of colourimetry

A

make a metal ion solution of known concentrations
of decreasing concentrations - dilution series
- measure the percentage absorption in the colourimeter
- measure the unknown concentration’s percentage absorption

  • plot a calibration curve
  • interpolate the graph to find the unknown conc
29
Q

what si the colour of aq Fe2+

A

green solution

30
Q

what is the colour of NaOH with (Fe(h2O)6)2+

A

green ppt
Fe(H2O)4(OH)2

31
Q

what is the colour of excess NaOH and the Fe2+ hexaaqua ion

A

green ppt
Fe(H2O)4(OH)2

32
Q

what is the colour of FE2+ with NH3

A

Fe(H2O)4(OH)2
GREEN PPT

33
Q

what is the colout of Fe2+ with excess NH3

A

green ppt
Fe(H2O)4(OH)2

34
Q

what is the colour of the Cu2+ as an aqueous ion

A

blue solution
(Cu(H2O)6)2+

35
Q

what is the colour of Cu2+ hexa aqua ion with NaOH

A

blue ppt
Cu(h2O)4(OH)2

36
Q

what is the colour of CU2+ with excess NaOH

A

blue ppt
Cu(H2O)4(OH)2

37
Q

what is the colour of Cu2+ NH3

A

Cu(H2O)4(OH)2
blue ppt

38
Q

what is colour Cu2+ excess NH3

A

deep blue solution
Cu(H2O)2(NH3)4)2+

39
Q

what is the colour of Fe2+ with Na2CO3

A

FeCO3 SOLID
green precipitate

40
Q

what is the colour of Cu2+ with NaCO3

A

Blue ppt
CuCO3

41
Q

what is the colour of aq Fe3+ as a hexaaquaion

A

purple solution

42
Q

Fe3+ with NaOH

A

Fe(h2O)3(OH)3 BROWN PPT

43
Q

Fe3+ with excess NaOH

A

Fe(H2O)3(OH)3
brown ppt

44
Q

fe3+ with NH3

A

Fe(H2O)3(OH)3 BROWN PPT

45
Q

Fe3+ with excess NH3

A

fe(h2o)3(oh)3 brown ppt

46
Q

Fe3+ with Na2CO3

A

CO2 is evolved
Fe(h2o)3(oh)3 brown ppt

23233

47
Q

what is the colour of Al 3+ in aqueous solution

A

Al(h2o)6)3+
colourless solution

48
Q

Al3+ with NaOH

A

Al(H2O)3(OH)3
white ppt

49
Q

Al3+ with excess NaOH

A

Al(OH)4)-
colourless solution

50
Q

Al3+ with NH3

A

Al(H2O)3(OH)3
white ppt

51
Q

Al3+ with excess NH3

A

Al(H2O)3(OH)3 white ppt

52
Q

Al3+ Na2CO3

A

Al(H2O)3(OH)3
white ppt
and CO2 gas evolved

23233

53
Q

what is the colour of VO4 3-

A

yellow

54
Q

what is the colour of VO2+

A

blue

55
Q

what is the colour of V3+

A

green

56
Q

what is the colour of V2+

A

violet

57
Q

what si the oxidation state of VO4 3-

A

5

58
Q

what is special about Al(h2o)3(oh)3

A

amphoteric
it can act as an acid or a base
and can be dissolved in either

59
Q

what is the ligand substitution between Cu(h2o)6)2+ and 4Cl-

A

Cu(Cl4)2- + 6H2O

THE COMPLEXES GO FROM BLUE YELLOW

60
Q

what is the equation for the ligand substitution Co(H2O)6)2+ and 2NH3

A

Co(h2o)4(oh)2) + 2NH4+

IT IS A REVERSIBLE REACTION.

61
Q

is there a stronger bond between N AND Cu or Cu and O

A

Cu and N

61
Q
A

Chemistry (25 decks)

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