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chem yr 13 NI > Transition Metals > Flashcards

Transition Metals Flashcards

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1
Q

Transition metal definition

A

Forms at least one stable ion with a partially filled d sublevel

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2
Q

Transition metal features

A

Form complex ions
Coloured ions
Catalytic properties
Variable oxidation states

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3
Q

Mono dentate ligands

A

Each ligand forms 1 coordinate bond

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4
Q

Bidentate ligands

A

Each ligand forms 2 coordinate bonds

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5
Q

Multidentate ligands

A

Each ligand forms 2 or more coordinate bonds

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6
Q

Need to know monodentate ligands

A

Water h2o:
Chloride cl-:
Ammonia :nh3
Cyanide :c-n

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7
Q

Need to know bidentate ligands

A

NH2ch2ch2nh2
Coordinate bonds from the lone pairs on the 2 n

C2o42-
Bonds form between 2 o- atoms

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8
Q

EDTA4-

A

Can form six coordinate bonds
Two from n atoms
Fourth from o- atoms

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9
Q

Chelate effect

A

Large increase in entropy

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10
Q

When does chelate effect occur

A

When a monodentate ligand is substituted by a bidentate or multidentate ligand
Number of moles increase so entropy change is positive

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11
Q

Why reaction is thermodynamically favourable

A

Use gibs equation
>h is zero as six n bonds broken and six n bonds made
<s is positive as entropy change is positive
G<0 so reaction is feasible

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12
Q

Heamoglobin

A

Can make six coordinate bonds
Four between fe2+ and n
One between fe 2+ and globin protein
Space for one more with oxygen
When oxygen has been transported bond is broken and co2 forms a bond to brung back to the lungs
Co makes a stronger bond so could permanently bind which is co poisoning

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13
Q

If ligands are next to each other

A

Cis isomers
Can show optimal isomerism if at least 2 bidentate ligands present

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14
Q

If ligands are not next to each other

A

Trans isomers

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15
Q

Visible light

A

Some colours from white light are absorbed and some transmitted through
Transmitted colours combine to make the visible colour

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16
Q

Process of absorbing and transmitting light

A

The d orbitals split in energy levels
D electrons are promoted to a higher d orbital by absorbing energy in the form of light
The colour transmitted through and observed is the light not absorbed by the compound

17
Q

Equation for change in energy

A

Change in energy = h(Planck constant 6.26x10-34) x f(frequency of light)
Change in energy = h x c/l
C=speed of light
L= wavelength of light

18
Q

Large change in energy between d subshells

A

High energy light absorbed to excite electrons (blue and purple)
Red/orange transmitted through

19
Q

Small change in energy between d subshells

A

Low energy light will be absorbed to excite electrons (red and orange)
Blue and purple will be transmitted

20
Q

Change in colour

A

Transition metal compounds can change colour
Can be caused by
Change in ligands
Change in oxidation state
Change in coordination number
Change in shape of a complex

21
Q

Calorimetry

A

Measure the amount of light absorbed when it passes through a sample

22
Q

Heterogenous catalysts

A

Catalysts is in a different phase to the reactants
Reactants adsorb onto surface of the catalyst
Reaction occurs on the surface of catalyst
Products desorb from surface of the catalyst

23
Q

Catalysts are expensive so

A

Make it more efficient by increasing surface area or spread catalyst over an inert support medium
Catalyst poisoning can happen though as impurities can block the active sites

24
Q

Need to know heterogenous catalyst examples

A

Ammonia in haber process
N2 + 3h2 <-> 2nh3
Catalysed by solid iron

Making sulfur trioxide in the contact process
Catalysed by vanadium oxide v2o5
2so2 + o2 <-> 2so3
Steps
1-so2 + v2o5 <-> so3 + v2o4
2-2v2o4 + o2 <-> 2v2o5

25
Q

Homogenous catalysts

A

Catalysts and reactants are in the same phase
S2o82- + 2I- -> 2so42- + I2
Catalysed by fe2+ ions

1-2fe2+ + s2o82- -> 2so42- + 2fe3+
2- 2fe3+ +2I- -> I2 + 2Fe2+
These could happen in either order

26
Q

Autocatalyst

A

Where a product of the reaction catalysts the reaction further
16H+ + 2mno4- + 5c2o42- -> 2mn2+ + 8h2o + 10co2
Mn2+ catalyse the reaction further
4mn2+ mno4- + 8h+ -> 5mn3+ + 4h2o
2mn3+ + c2o42- -> 2co2 + 2mn2+

27
Q

Potassium manganate reactions

A

8h+ + mno4- + 5fe2+ -> mn2+ +4h2o + 5fe3+
When using in titration ratio is always 1:5

28
Q

Reducing vanadium(v) to vanadium(IV)

A

Zn + 4h+ + 2vo2+ -> zn2+ 2vo^2+ + 2h2o
Yellow to blue
Can look green if there’s some left

29
Q

Reducing vanadium(V) to vanadium(III)

A

Zn + 4h+ + vo2+ ->zn2+ + v3+ + 2h2o
Yellow to green

30
Q

Reducing vanadium (V) to vanadium(II)

A

3Zn + 8h+ + 2vo2+ -> 3Zn2+ + 2v2+ + 4h2o
Yellow to purple

chem yr 13 NI (17 decks)

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