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

Transition Metals Flashcards

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
What is the coordination number
The total number of coordinate bonds from the ligand to the enthral metal ion
26
What are ligands referred to
A Lewis bases
27
LEARN HOW TO NAME COMPEXES !!!!!
28
What are d orbitals in transition metals
D orbitals are no longer degenerate
29
Why do the same metal ion with different ligands have different colours
Different ligands produce different field splitting and so complexes of the same metal ion with different ligands will have different colours
30
What are strong field ligands
Ligands that cause a large difference in energy between subshells of d orbitals
31
What are weak field ligands
Cause a small energy difference between subshells of d orbitals
32
What does the energy difference between subshells of d orbitals depend on
The position of the ligands in the spectrochemical series
33
How can colours of transition metal complexes be explained
In terms of d-d interactions. The effects of d-d transitions can be studied using ultraviolet and visible absorption spectroscopy
34
When is light absorbed
When electrons in a lower energy d orbital are promoted to a d orbital of higher energy
35
What does ultraviolet and visible absorption spectroscopy involve
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
What does an ultraviolet/visible spectrometer
Measures the intensity of radiation transmitted through the sample and compares this with the intensity of incident radiation
37
What can transition metals or their compounds act as
Act as catalysts in many chemical reactions
38
What can catalysts be
Homogeneous- in the same state as the reactants Heterogeneous-in different state to the reactants
39
What causes intermediate complexes to form
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
Why are simple ions and complex ions of transition metals often coloured
Because they absorb certain parts of the visible spectrum
41
What happen if red, blue and all the colours are abosrbed by an ion or complex ion from the visible spectrum
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
What does degenerate mean
Have the same energy
43
What are d orbitals when the transition metal is not bonded to anything else
There are five d orbitals and they are all degenerate
44
When a ligand approaches a d orbitals that are all degenerate what happens in transition metals
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
The size of the energy gap(/\E) between two sets of d orbitals varies with
The transition metal ion The oxidation state of transition metal The type of ligand
46
What does energy in the visible region of the spectrum cause
D electrons transitions between lower energy orbitals and d orbitals of higher energy
47
What determines the colour produced by the compound or complex
Different ligands bonded to the central transition metal ion cause different splits in the d orbitals. The size of this split determines it
48
What is given by the spectrochemical series
The ability of ligands to cause splitting is given by the spectrochemical series
49
What happens the greater the splitting in d orbitals
The more energy is needed to promote an electron from the lower group of d orbitals to the higher ones
50
What happens when the greater the energy of light absorbed
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
Describe concentration of transition metals
The higher the concentration of ions the greater the absorbance
52
What does the abosorption of ultraviolet or visible radiation correspond to
Outer electrons becoming excited
53
What are complexes containing weak field ligands do
More likely to absorb visible region (400-700 nm)
54
What can a colorimetry be used for
To determine the concentration of ions
55
When will a compound be colourless
If the energy absorbed is in the ultraviolet part of the electromagnetic spectrum, the compound will be colourless so ultraviolet spectroscopy is used
56
When does the d-d interaction tend to occur in the ultraviolet region(200-400)
When the ligands surrounding the transition metal ion are strong field ligands
57
What cannot have d-d interactions
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
Whats a catalyst
Speeds up chemical reactions by providing an alternative reaction pathway of lower activation energy
59
Why can transition metal form a variable number of bonds
Because of the availability of unoccupied or partially occupied d orbitals
60
Why can transition metals act as homogeneous catalysts
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
What are d block transition metals
Metals with an incomplete d subshell in at least one of their ions
62
What can transition metals have in its compounds
Different oxidation numbers
63
Whats the spectrochemical series
When ligands are placed in an order of their ability to split d orbitals
64
Describe heterogeneous catalysts
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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