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A Level Chemistry Inorganic > Transiton Metals > Flashcards

Transiton Metals Flashcards

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1
Q

What are transition metals

A

They are metals that form at least one stable ion with partially filled d orbitals

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2
Q

Why aren’t zinc and scandium considered transition metals

A

Scandium only forms 3+ions with no electrons in the d orbital

Zinc only forms 2+ ions with a full d block

So they don’t form partially field d blocks

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3
Q

What are 4 properties of transition metals

A

Complex ion formation
Formation of coloured ions
Variable oxidation state
Catalytic activity

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4
Q

What is a ligand

A

It’s a molecule that forms a co ordinate bond with a transition metal by donating pair of electrons

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5
Q

What is a complex ion

A

It’s a central metal atom surrounded by ligands and forms dative covalent bonds

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6
Q

What is the co ordination number

A

The number of co ordinate bonds to the central metal ion

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7
Q

State the ligands that form 6 bonds around a metal ion

A

NH3

H2O

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8
Q

State the ligands that form 4 bonds

A

CL

CN

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9
Q

What is a monodente ligand

A

One that has only one atom with a lone pair of electrons which forms bonds with a transition metal ion

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10
Q

What is a multidentate ligand

A

When it has more than one atom with a lone pair of electrons and it forms bonds with transition metal ions

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11
Q

What is the chelate effect and why does it occur

A

That bi dentate and multidente ligands replace monodentate ligands from complexd as they increase entropy for the reaction

There are moles of products than reactants from2-7 this creates more disorder

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12
Q

Give an example of bidente ligands

A

En

C2O4(2-)

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13
Q

What are the 4 shapes that complex ions form and give examples

A

Octahedral
Square planer-cisplatin (Pt)(NH3)2 (CL)2

Tetrahedral-[CO(CL)4

Linear- NH3–Ag–NH3

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14
Q

State how many coordinate bonds CN,H20,OH,NH3

A

6

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15
Q

How many co ordinate bonds does CL

A

4

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16
Q

State the types of isomerism that complex ions form

A

Optical isomerism

Cis-trans isomerism

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17
Q

State what optical isomerism and how it’s shown in complex ions and how can they be distinguished

A

Two non imposable mirror images are formed they can be distinguished by passing plane polarised light through the mixture and the enantiomers rotate them in equal but opposite directions

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18
Q

State the use of AG(NH3)

A

It’s used as tollens reagent

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19
Q

Give the use of cisplatin and how it works

A

It’s an anti cancer drug it prevents the cancer cell from replicating

20
Q

What 3 factors affect colour changes in transition metals

A

Ligand
Co-ordination number
Oxidation state

21
Q

Why does s change in ligand or coordination number result in a change in colour

A

It alters the energy split between the d-orbitals which changes the energy difference so the frequency of light absorbed changes

22
Q

Why do transition metals have different colours

A

When light hits a transition metal it’s absorbed which causes electrons to rise to from ground state to an excited state

The light that isn’t absorbed is transmitted which give the substance colour

23
Q

Why do Sn and Zn not have colour

A

SN ion doesn’t have any d electrons left

While Zn and cu have full n d blocks do there’s no energy transfer

24
Q

In redox titration state what acid is used and why HCL and nitric acid can’t be used

A

Conc HCL can’t be used as the CL- ions will be oxidised to chlorine

Nitric acid can’t be used as it’s an oxidising agent which leads to a small volume of managanate being produced

So dilute H2SO4 is produced

25
Q

What is the difference between heterogenous catalyst and homogenous catalyst

A

Heterogenous is in a different phase than the reactants

Homogenous is in the same phase as reactants

26
Q

Give a way to improve the effectiveness of a catalyst

A

Increase the surface area

27
Q

Give an example of a homogenous catalyst and state where it’s used

A

Fe 2+

Reaction between I- and S2O8 2-

28
Q

Give the equation for the catalyses reaction between I- and S2O82-

A

S2O8(2-) +2Fe(2+) -> 2SO4(2-) +2Fe3+

Stage 2- 2I- +2Fe(3+) ->2Fe2+ +I2

29
Q

Why is the Uncatalysed reaction between iodide and persulphate ions slow

A

Because the reaction needs the collision between two negative ions and they repel meaning high activation energy

30
Q

Why do the individual stages in the catalysed mechanism result in lower activation energies

A

As it involves collision between positive and negative lonw

31
Q

What is autocataylsis and give an example

A

It’s w where one of the products can catalyse the reaction

Mn2+

32
Q

What is colorimetery and what is it used for

A

It’s when a light source is passed through in order to measure the amount of light of a certain wavelength passes through a coloured solution

It helps in finding the formula of a solution

Calibrate using a colorimeter

33
Q

Describe how colorimetery works

A

The two solutions are mixed together one which contains the metal ions and one with the ligands in different proportions

This happens until they are mixed at the same ratio as they are in the complex this is the max conc so it has the highest absorbance

34
Q

What is absorbance

A

Measure of how much light is absorbed by a solution.

The higher the concentration the higher the absorbance

35
Q

Why is water added in colorimetery

A

To maintain the volume

36
Q

What is poisoning

A

When the catalyst is poisoned by impurities and reduces the efficiency

37
Q

Give an example of a heterogenous catalyst and it’s is

A

V2O5

It’s used in the contact process

38
Q

Give the equation of V2O5 in the contact process

A

So2+V2O5->So3+V2O4

2V2O4+O2->2V2O5

39
Q

In autocatalysis why is the uncatalysed reaction slow

Between 2Mn and C2O4 (2-)

A

Because the reaction collision is between two negative ions which repel to give high activation energy

40
Q

What is the colour change of manganate in a titration and why does this occur

A

It’s goes from colourless-purple and this is because the manganate is in excess

41
Q

Give the ionic equation of the reaction between manganate and fe

A

MnO4-+8H+ 5Fe2+->Mn2+. +4H2O+5Fe3+

42
Q

What properties of transition metals enable them to be catalysts

A

The fact that they have variable oxidation states

43
Q

State what happens in adsorption and why do bonds in the reactant break

A

The reactants will form bonds with atoms at the active site on the catalyst surface

This causes the bonds in reactants to break as they are weakened

44
Q

What happens in desorption

A

New bonds form between reactants on the catalyst

This in turn weakens bonds between product and catalyst and this causes the product it leave so it desorbes

45
Q

When transition metals form ions where do they lose electrons from

A

They lose from 4s before 3D

A Level Chemistry Inorganic (5 decks)

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