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CHEMISTRY > TRANSITION METALS > Flashcards

TRANSITION METALS Flashcards

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1
Q

TRANSITION METALS

A

Forms at least one stable ion with a partially filled D-sub shell

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2
Q

What are the 2 exseption ?

A

Sc- 1s2 2s2 2p6 3s2 3p6 4s2 3d1
Zn- 1s2 2s2 2p6 3s2 3p6 4s2 3d10

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3
Q

Key features of transition metals

A

Complex ion
Coloured ion
Catalytic properties
Variable oxidation state

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4
Q

What is a coordinate bond

A

Shared pair of e- which both come from same atom

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5
Q

Ligand definition

A

Ion or molecule eith a lone pair of e- which can form a coordinate bond with a transtiom metal ion

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6
Q

Coordinate number definition

A

Number kf coordinate bonds a transition metals ions forms

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7
Q

Complex ion definition

A

Transition metals ions form surrounded by ligands

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8
Q

Monodentate ligands example

A

H2O:
-:CN
:NH3
-:OH
CL:-

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9
Q

Bidentandate ligands example

A

1,2-diaminoethane
Ethanedioate ion

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10
Q

How many bond does EDTA4- form

A

6

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11
Q

What is the chellate effect

A

Occurs when a monidentate ligand substituetes by bidentate
If there is an increase in moles on the products side
Entropy AS decreases as more disorder
So reaction is feasible

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12
Q

How does HB work

A

O2 forms a coordinate bond to Fe2+ in haemoglobin enabling oxygen to be transported in the blood
CO toxic because CO bind more strongly to the Fe2+ in haemoglobin this orevents oxygen from bonding to Fe2+ causing soffication

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13
Q

Difference between cis/trans

A

Trans- 180 degrees between ligands
Cus - 90 degrees between ligands

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14
Q

How does plactin works

A

Binds to DNA in cancerous cells
Stops cell replication
Preventing DNA. From unwinding so cancerous cells cant replicate which prevents spreading of cancerous celks

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15
Q

Rormation of coloured ions

A

Due to patrtially filled d sub-shell absirb some of the colours from white light and reflects other
ROY- low energy
BIV- high energy

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16
Q

Why are some complexes colourless

A

No e- in d shell
/
Full d-sub shell

17
Q

What causes alterstion of a compund colour

A

Change in ligands
Changd in oxidation state
Change in shape
Change in coordination number

18
Q

How to find concentration of unkown sample form calibration curve

A

Measure absorbance for a range of known concentration
Plot a graph of concentration against absorbance/transmission
Read value of the concentration for measured absorbance from graph

19
Q

What is a catalyst ?

A

Substance increases rate of reaction of a chemical reaction without being used up

20
Q

How do catalust work?

A

Provides an alternative pathway with lower activation energy

21
Q

Heterogeneous catalyst

A

Catalyst is in a different phase to the reactants

22
Q

Homogeneous catalyst

A

Catalyst in same phase to the reactant

23
Q

How xo heterogenous catalyst work

A

Reactant adsorb onto surface if catalust on active site
Reaction occurs on surface of catalyst
Products desorb form surface of catalyst

24
Q

How to make catalyst more efficient? (2)

A

Increase surface area
Spread catalust over aninert support medium

25
Q

Why dont catalyst last forever?

A

Immpurities can blocj active sites
Prevents reactants from adsorbing
Purifying reactants in the best way to prevent poisoning

26
Q

Why is rate slow initially

A

No catalyst initially
2 negatively charged reactants collide with very high Ea
As reactant that act as catalyst formed rate increases as reaction is being increasingly catalysed
Rare then decreases and levels off as reactant get used up

27
Q

Small E ROY ABS

A

Small AE between d sub shell
Low energy light
Will be absorbed to excite the e-
Blue indingo purple will be reflected

28
Q

Big E BIV abs

A

Large AE between d subshell
High energy lost
Will bd absorbed to excite e-
Red yellow oranfe will be reflected

29
Q

Harber process
Equations + catalyst

A

Catalyst: iron
N2(g) +3H2(g) <———> 2NH3(g)

30
Q

Contact process
Equation + catalyst

A

Catalyst: V2O5
SO2(g) + V2O5(s) <——-> SO3(g) + V2O4(s)
2V2O4(s) +O2(g) <———-> 2V2O5(g)

Overall equation
2SO2(g) +O2(g) ————> 2SO3(g)

31
Q

Manufucture of methanol
Catalust + equation

A

CH4(g) + H2O(g) ———-> CO(g)+ 3H2(g)
Catalyst: Cr2O3
CO(g) + 2H2(g) ———-> CH3OH(g)

32
Q

uncatalyzed reaction
Catalyst + equation

A

2MnO4-(aq) + 16H+(aq) + 5C2O42-(aq) → 2Mn2+(aq) + 8H2O(l) + 10CO2(g)
Catalyst Mn2+
4Mn2+(aq) + MnO4-(aq) + 8H+(aq) → 5Mn3+(aq) + 4H2O(l)
2Mn3+(aq) + C2O4 2-(aq) ——> 2CO2 + 2Mn2+

33
Q

Homogeneous catalyst

A

S2O82-(aq) + 2I-(aq)→2SO42-(aq) + I2(aq)

Catalyst:Fe2+
S2O82-(aq) + 2Fe2+(aq)→2SO42-(aq) + 2Fe3+(aq)
2I-(aq) + 2Fe3+(aq)→I2(aq) + 2Fe2+(aq)

CHEMISTRY (23 decks)

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