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Chemistry Content > Transition Metals > Flashcards

Transition Metals Flashcards

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1
Q

What shape does Ni2+ and Pt2+ complexes form

A

Square planar

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2
Q

What shape does Ag+ complexes form

A

Linear

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3
Q

Ligand definition

A

A molecule or ion that forms a coordinate bond with a transition metal by donating a pair of electrons

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4
Q

Complex definition

A

A central metal atom or ion surrounded by ligands

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5
Q

Coordination number

A

Number of coordinate bonds to the central metal atom or ion

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6
Q

Examples of multidentate ligands

A

EDTA^4- and porphyrin

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7
Q

What is a haem

A

Haem is an iron(II) complex with a multidentate ligand.

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8
Q

What is haemoglobin

A

Globular protein with four Fe2+ centres each with a porphyrin ligand taking up four of the six coordination sites. One of the other two is bonded to the rest of the haemoglobin leaving the last site for oxygen to bond

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9
Q

How does haemoglobin transport oxygen

A

Haem is an iron(II) complex with a multidentate ligand.
Oxygen forms a co-ordinate bond to Fe(II) in haemoglobin, enabling oxygen to be transported in the blood.

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10
Q

Why is carbon monoxide dangerous

A

Carbon monoxide is toxic because it replaces oxygen co-ordinately bonded to Fe(II) in haemoglobin.

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11
Q

What complexes display cis-trans isomerism

A

Octahedral complexes with monodentate ligands

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12
Q

What complexes display optical isomerism

A

Octahedral complexes with bidentate ligands

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13
Q

Label which is cis/trans isomer

A

Left - cis
Right - trans (across)

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14
Q

How do you know 🔼H is negligible

A

Look at the bonds being broken and made. If 6 bonds are broken in monodentate and is replaced with bidentate, then 6 bonds being made so 🔼H is negligible

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15
Q

What are chelating agents

A

Ligands that form more than one coordinate bond or many as they are very good at bonding to the metal ion and very difficult to remove.

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16
Q

What effects the formation of coloured ions

A
  • metal
  • the oxidation state
  • the ligands
  • the coordination number
17
Q

The equation for the gap in energy

A
18
Q

How to remember the effect of ph

A

Reduced - red ( happens in acid)
Oxidised - blue ox (happens in alkali)

It is easier to oxidise a transition metal in alkali and reduce a transition metal in acidic conditions

19
Q

Tollens reagent complex

A
20
Q

Fehling’s complex

A
21
Q

Acidified dichromate complex

A
22
Q

The changes of oxidation states with vanadium

A

Vanadium ion can be reduced in acidic conditions using zinc as the reducing agent

5+ -> 4+ -> 3+ -> 2+

YBGV

23
Q

Test for vanadium oxidation states

A
24
Q

The conditions for titration of KMnO4

A

Acidic conditions using dilute sulfuric acid as the acid

25
Q

Why can you only use dilute sulfuric acid in titration with KMnO4

A

HCL cannot as MnO4- would oxidise Cl- to Cl2 - affect the volume of KMnO4 required
conc Sulfuric/nitric acid cannot - they are oxidising agents so affect the volume of KMnO4
ethanoic acid cannot - weak acid and would not provide enough H+ ions

26
Q

Why do we not need an indicator for titration of KMnO4

A
27
Q

Fe2+ and potassium manganite (VII) redox reactions

A
28
Q

Ethanedioate ion and potassium manganite (VII) redox reactions

A
29
Q

Heterogenous catalyst steps

A
  • place where adsorbed are called active sites (AS)
30
Q

What happens if heterogenous catalyst too strong

A
  • reactants cannot move around surface
  • products cannot desorb
  • eg V and Cr are too strong so block AS
31
Q

What happens when heterogenous catalyst too weak

A
  • reactants not adsorbed
32
Q

V2O5 reaction

A

Heterogenous catalyst example

33
Q

what catalyst is used in the Haber process

A

Fe catalyst

3H2 +N2 <——> 2NH3

34
Q

Importance of variable oxidation states

A

Variable oxidation states allow transition metals to act as catalysts lowering activation energy

35
Q

Reaction of iodide and peroxodisulfate ions (S2O8^2-)

A
36
Q

Why does iodide and S2O8^2- have a high activation Energy

A

Because both are negative ions so repel each other

37
Q

Reaction of Manganate (VII) ions and ethanedioate ions

A

Homogenous catalyst

Chemistry Content (31 decks)

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