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Inorganic Chemistry > Inorganic 5: Transition Metals > Flashcards

Inorganic 5: Transition Metals Flashcards

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1
Q

What is a transition element?

A

An element that forms at least one stable ion with a partially filled d-shell of electrons

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2
Q

What are the main physical properties of transition elements?

A

1) Good conductors of heat and electricity
2) Hard, strong, and shiny
3) High melting and boiling points

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3
Q

What can iron be used for?

A

Making the alloy steel, useful in reinforcing concrete and vehicle bodies

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4
Q

What can copper be used for?

A

Water pipes

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5
Q

What can titanium be used for?

A

Jet engine parts that need to withstand high temperatures

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6
Q

What are the main chemical properties of transition metals?

A

1) Variable oxidation states
2) Form complex ions
3) Form coloured ions
4) Act as catalysts

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7
Q

What is the only ion that scandium can form?

A

Sc3+

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8
Q

What is the only ion that zinc can form?

A

Zn2+

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9
Q

Which two d-block elements are not transition metals?

A

Scandium and zinc
Because they only form one stable ion each
And they have filled d-orbitals

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10
Q

What is a ligand?

A

A molecule that contains an atom with a lone pair of electrons that can be donated to a transition metal ion

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11
Q

Give four examples of common ligands.

A

Water and ammonia
- Similar size
- Uncharged

Chloride
- Larger
- Charged (-1)

Cyanide
- Charged (-1)

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12
Q

What is a co-ordination number?

A

The number of co-ordinate bonds in a complex ion

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13
Q

What shape would a complex ion with six co-ordinate bonds form?

A

Octahedral

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14
Q

What shape would a complex ion with four co-ordinate bonds form?

A

Tetrahedral
Square planar

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15
Q

What shape would a silver complex ion form?

A

Linear

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16
Q

What is an aqua ion?

A

The salt of a transition metal is dissolved in water
The positively charged metal ions become surrounded by water molecules

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17
Q

What is a multidentate ligand?

A

A ligand that has more than one atom with a lone pair of electrons that can form a bond to a transition metal ion

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18
Q

Give three examples of bidentate ligands.

A

1,2-diaminoethane
Benzene,1-2,diol
Ethanedioate (oxalate)

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19
Q

Draw the structure of 1,2-diaminoethane.

A

Neutral ligand
Often abbreviated to (en)
E.g. [Cr(en)3]3+

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20
Q

Draw the structure of ethanedioate.

A

2- charge

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21
Q

Draw the structure of benzene,1-2,diol.

A

Neutral

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22
Q

What is a common multi dentate ligand?

A

EDTA 4-

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23
Q

What is a chelate?

A

A complex ion with polydentate ligands

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24
Q

What are chelates used for?

A

Removing d-block metal ions from solutions

25
Q

What is the chelate effect?

A

If a hexadentate ligand such as EDTA is added to a solution of a transition metal salt, the EDTA will replace all six water ligands in the aqua ion
This causes a significant increase in entropy which increases stability
Chelate complexes with polydentate ligands are favoured

26
Q

Give the formula for Tollen’s reagent.

A

[Ag(NH3)2]+

27
Q

What two complex structures can show cis-trans isomerism and how?

A

Square planar
Octahedral
The same ligand can be next to each other or opposite (cis or trans)

28
Q

What complexes can show optical isomerism?

A

Any complex with two or more bidentate ligands
The two isomers are non-superimposable mirror images of each other

29
Q

Why is carbon monoxide toxic?

A

It replaces oxygen by co-ordinately bonding to Fe(II) in haemoglobin

30
Q

How is oxygen transported in blood?

A

It co-ordinately bonds to Fe(II) in the blood

31
Q

What is anaemia?

A

Anaemia is a condition which may be caused by a shortage of haemoglobin
The body suffers from a lack of oxygen and the symptoms include fatigue, breathlessness, and pale skin
Could be caused by blood loss or ion deficiency

32
Q

How can anaemia be treated?

A

Taking iron tablets containing iron(II) sulfate

33
Q

Why are transition metal ions coloured?

A

They have partially filled d-orbitals, so electrons can move from one d-orbital to one of a higher energy level
When electrons move to a higher energy level, they absorb energy in the visible region of the spectrum equal to the difference in energy level
Since this energy is absorbed, this colour is not seen, so we see a combination of the colours that haven’t been absorbed

34
Q

Why do the d-orbitals in transition-metal complexes have different energy levels when they are the same in isolated transition metal atoms?

A

Because the presence of other atoms nearby makes the d-orbitals have slightly different energies

35
Q

What is the equation linking difference in energy levels and frequency of light?

A

ΔE = hv
Where E is energy, h is Planck’s constant, and v is frequency

36
Q

Which colour has the highest frequency and which colour has the lowest?

A

Violet has the highest frequency
Red has the lowest frequency

37
Q

What does the colour of a transition metal complex depend on?

A

ΔE,
Oxidation states of metal and ligands
The shape of the complex ion
Therefore different compounds of the same metal can have different colours

38
Q

What is colorimetry?

A

A technique used to measure the amount of light that can pass through a coloured solution
The more concentrated the solution, the higher the absorbance reading (less light passes through)

39
Q

What is the most common ion formed by titanium?

A

4+

40
Q

What are the common ions formed by vanadium?

A

4+ and 5+

41
Q

What are the common ions formed by chromium?

A

2+, 3+, 6+

42
Q

What are the common ions formed by manganese?

A

2+, 4+, 7+

43
Q

What are the common ions formed by iron?

A

2+, 3+

44
Q

What are the common ions formed by cobalt?

A

2+, 3+

45
Q

What is the most common ion formed by nickel?

A

2+

46
Q

What are the common ions formed by copper?

A

1+, 2+

47
Q

What are redox titrations used for?

A

To measure the concentration of an oxidising or reducing agent
E.g. analysing iron tablets

48
Q

How are redox titrations used to analyse iron tablets?

A

1) Using a burette, potassium manganate(VII) is added to a solution of Fe2+ ions acidified with excess dilute sulfuric acid
2) The purple colour of the solution disappears as Mn2+ ions are produced (pale pink), so the solution becomes virtually colourless
3) At the end point, one drop of MnO4- will turn the solution purple

49
Q

What are the two types of catalyst?

A

Heterogenous
Homogenous

50
Q

How do heterogenous catalysts work?

A

They exist in a different phase to the reactants
(Usually solid whereas reactants are gaseous or liquid)
Their catalytic action occurs on the solid surface
Reactants pass over the surface, which is fixed so catalyst is not lost and doesn’t mix with products

51
Q

How can heterogeneous catalysts be made more efficient?

A

1) Increase surface area
2) Spread the catalyst onto an inert support medium or impregnate it into one to increase the surface-to-mass ratio

52
Q

What is catalyst poisoning?

A

When the catalyst becomes covered with impurities

53
Q

Why do catalysts not last forever?

A

1) Catalyst poisoning
2) Catalyst could be gradually lost from the support medium

54
Q

What catalyst is used in the Haber process?

A

Pea-sized lumps of iron (increases surface area)
Iron becomes poisoned by impurities in gas (e.g. sulfur compounds)

55
Q

What catalyst is used in the Contact process?

A

Vanadium (V) Oxide - V2O5
Heterogenous catalyst

1)
V2O5 + SO2 –> V2O4 + SO3
Vanadium(V)oxide oxidises sulfur dioxide into sulfur trioxide, forming vanadium(IV)oxide

2)
V2O4 + 1/2O2 –> V2O5
Oxygen then oxidises vanadium(IV)oxide back into vanadium(V) oxide, regenerating the catalyst

56
Q

How do homogenous catalysts work?

A

They exist in the same phase as the reactants, and form an intermediate species

57
Q

Describe how Fe2+ acts as a catalyst in the production of iodine from iodide ions.

A

Fe2+ is a homogenous catalyst as it exists in the same phase as the reactants

Step 1:
S2O82- + 2Fe2+ –> 2Fe3+ + 2SO42-

Step 2:
2Fe3+ + 2I- –> I2 + 2Fe2+

Fe2+ is needed to form an intermediate of Fe3+ because peroxidisulfate (S2O82-) is negatively charged, as are I- ions, so they repel

58
Q

What is autocatalysis?

A

Where one of the products of a reaction is the catalyst for the reaction
The reaction starts slowly in its uncatalysed state
As the concentration of product increases, the rate of reaction increases
E.g. oxidation of ethanedioic acid by manganate (VII) ions

Inorganic Chemistry (7 decks)

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