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Chemistry Unit 1 How To Pass Book > Transition Metals > Flashcards

Transition Metals Flashcards

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1
Q

What are the d-block transition metals

A

Are metals with an incomplete d subshell in at least one of their lone pairs

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2
Q

Why are copper and chromium different

A

Due to a special stability associated with all the d orbitals being half filled or completely filled

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3
Q

When transition metals from ions what happens to the sub shells

A

4s subshell electrons are lost first rather than the 3d sub shells

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4
Q

What do compounds have that are of the same transition metal but different oxidation states

A

May have different colours

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5
Q

What can oxidation and reeducation be considered as

A

Oxidation can be considered as an increases in oxidation number and reduction can be considered as a decrease in oxidation number

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6
Q

What tends to be oxidatising agents and reducing agents

A

Compounds containing metals in high oxidation states tend to be oxidising agents
Compounds containing metals in low oxidation states are often reducing agents

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7
Q

What are the general properties of transition metals

A

Have atoms and ions with an incomplete d subshell
Can form complexes
Have variable oxidation states
Show catalytic ability
Form coloured ions

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8
Q

Whats a transition metal defined as

A

A metal that in at least one of its stable ions has a partly filled d subshell

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9
Q

What is the oxidation number equal to

A

The charge on the ion

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10
Q

LEARN HOW TO FIND OXIDATION NUMBERS!!!!!!

A
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11
Q

Whats oxidation

A

Oxidation is the loss of electrons. So oxidation can be described as an increases in oxidation number

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12
Q

Whats reduction

A

Reduction is gain of electrons and can be said to decrease oxidation number

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13
Q

What tends to be oxidising agents and reducing agents

A

Compounds containing metals in high oxidation state
Compounds containing metals in low oxidation state

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14
Q

What are examples of oxidising agents

A

Acidified permanganate and acidified dichromate

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15
Q

Whats a complex

A

A complex consists of a central metal ion or atom surrounded by ligands

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16
Q

What are ligands

A

Ligands are electron donors and may be negative ions or molecules with non bonding pairs of electrons

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17
Q

What can ligands be classified as

A

Monodentate, bidentate up to hexdenate

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18
Q

Whats the coordination number of the central atom

A

The number of bonds from the ligand to the central metal ion or atom is known as the coordination number of the central atom

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19
Q

What are coordination compounds

A

When transition metals form complexes

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20
Q

Where can you find ligands

A

The molecules or ions surrounding the central metal ion or atom

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21
Q

What do ligands have

A

At least one lone pair of electrons which can form coordination bond to the metal

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22
Q

What happens to lone pair of electrons on a ligand

A

They are donated into an empty orbital in the transition metal atom or ion

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23
Q

What are monodentate ligands

A

Ligands that form one co ordinate bond to a metal atom or ion e.g NH3, H20

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24
Q

What do lone pairs on ligands allow

A

The lone pairs of electrons are on different atoms allowing the ligand to form more than one coordinate bond

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25
Q

What is the coordination number

A

The total number of coordinate bonds from the ligand to the enthral metal ion

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26
Q

What are ligands referred to

A

A Lewis bases

27
Q

LEARN HOW TO NAME COMPEXES !!!!!

A
28
Q

What are d orbitals in transition metals

A

D orbitals are no longer degenerate

29
Q

Why do the same metal ion with different ligands have different colours

A

Different ligands produce different field splitting and so complexes of the same metal ion with different ligands will have different colours

30
Q

What are strong field ligands

A

Ligands that cause a large difference in energy between subshells of d orbitals

31
Q

What are weak field ligands

A

Cause a small energy difference between subshells of d orbitals

32
Q

What does the energy difference between subshells of d orbitals depend on

A

The position of the ligands in the spectrochemical series

33
Q

How can colours of transition metal complexes be explained

A

In terms of d-d interactions. The effects of d-d transitions can be studied using ultraviolet and visible absorption spectroscopy

34
Q

When is light absorbed

A

When electrons in a lower energy d orbital are promoted to a d orbital of higher energy

35
Q

What does ultraviolet and visible absorption spectroscopy involve

A

Transitions between electronic energy levels in atoms and molecules where the energy difference corresponds to the ultraviolet and visible region of the electromagnetic spectrum

36
Q

What does an ultraviolet/visible spectrometer

A

Measures the intensity of radiation transmitted through the sample and compares this with the intensity of incident radiation

37
Q

What can transition metals or their compounds act as

A

Act as catalysts in many chemical reactions

38
Q

What can catalysts be

A

Homogeneous- in the same state as the reactants
Heterogeneous-in different state to the reactants

39
Q

What causes intermediate complexes to form

A

It’s believed that the presence of unpaired d electrons or unfilled d orbitals allows intermediate complexes to form, providing reaction pathways of lower energy compared to the uncatalyst reaction

40
Q

Why are simple ions and complex ions of transition metals often coloured

A

Because they absorb certain parts of the visible spectrum

41
Q

What happen if red, blue and all the colours are abosrbed by an ion or complex ion from the visible spectrum

A

Red light is absorbed, the colours transmitted are blue green which is seen as cyan or green/blue
Blue light is abosbred, the colours transmitted are red and green which is Ennis as yellow
All he colours absorbed the complex or ion will appear black

42
Q

What does degenerate mean

A

Have the same energy

43
Q

What are d orbitals when the transition metal is not bonded to anything else

A

There are five d orbitals and they are all degenerate

44
Q

When a ligand approaches a d orbitals that are all degenerate what happens in transition metals

A

The lone pair of ligands repels the d orbitals. Th d subshell is split into two distinct sets of orbitals that have a difference in energy between them

45
Q

The size of the energy gap(/\E) between two sets of d orbitals varies with

A

The transition metal ion
The oxidation state of transition metal
The type of ligand

46
Q

What does energy in the visible region of the spectrum cause

A

D electrons transitions between lower energy orbitals and d orbitals of higher energy

47
Q

What determines the colour produced by the compound or complex

A

Different ligands bonded to the central transition metal ion cause different splits in the d orbitals. The size of this split determines it

48
Q

What is given by the spectrochemical series

A

The ability of ligands to cause splitting is given by the spectrochemical series

49
Q

What happens the greater the splitting in d orbitals

A

The more energy is needed to promote an electron from the lower group of d orbitals to the higher ones

50
Q

What happens when the greater the energy of light absorbed

A

The shorter the wavelengths, as the splitting increases the light absorbed shifts away from the red end of the spectrum towards orange yellow and so on

51
Q

Describe concentration of transition metals

A

The higher the concentration of ions the greater the absorbance

52
Q

What does the abosorption of ultraviolet or visible radiation correspond to

A

Outer electrons becoming excited

53
Q

What are complexes containing weak field ligands do

A

More likely to absorb visible region (400-700 nm)

54
Q

What can a colorimetry be used for

A

To determine the concentration of ions

55
Q

When will a compound be colourless

A

If the energy absorbed is in the ultraviolet part of the electromagnetic spectrum, the compound will be colourless so ultraviolet spectroscopy is used

56
Q

When does the d-d interaction tend to occur in the ultraviolet region(200-400)

A

When the ligands surrounding the transition metal ion are strong field ligands

57
Q

What cannot have d-d interactions

A

If the transition metal ion as no d electrons or ions that have a complete d subshell. D-d interactions only occur in transition metals in a compound that as 1-9 d electrons

58
Q

Whats a catalyst

A

Speeds up chemical reactions by providing an alternative reaction pathway of lower activation energy

59
Q

Why can transition metal form a variable number of bonds

A

Because of the availability of unoccupied or partially occupied d orbitals

60
Q

Why can transition metals act as homogeneous catalysts

A

There ability to have a variety of oxidation states enables them to act as catalysts. The transition metal returns to its original oxidation state once catalyst reaction is performed

61
Q

What are d block transition metals

A

Metals with an incomplete d subshell in at least one of their ions

62
Q

What can transition metals have in its compounds

A

Different oxidation numbers

63
Q

Whats the spectrochemical series

A

When ligands are placed in an order of their ability to split d orbitals

64
Q

Describe heterogeneous catalysts

A

Explained in terms of the formation of activated complexes and the absorption of reactive molecules onto active sites. The presence of unpaired d electrons or unfilled d orbitals is though to allow activated complexes to form. This an provide reaction pathways with lower activation energies compared to uncatalsed reactions

Chemistry Unit 1 How To Pass Book (3 decks)

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