Transition Metals

Front 1

Deifne transition metal.

Back 1

Any metal which can form at least 1 stable complex ion and has an incomplete D sub level.

Front 2

Where in the periodic table are transition metals found?

Back 2

The D block.

Front 3

Which of the period 4 elements are transition metals?

Back 3

All of them apart from Sc and Zn (the two bookends).

Front 4

What 2 exeptions are there in transition metals to the rule that the 4s shell fills before the 3d shell?

Back 4

Copper, has 1 electron in 4s and 1 in 3d.

Chromium, has a full 3d and 1 in the 4s.

Front 5

In what order are electrons removed when transition metals form positive ions?

Back 5

The 4s electrons are removed and then the sd electrons are removed.

Front 6

Why are Scandium and Zinc not transition metals?

Back 6

They do not form stable ions with incomplete d sub levels.

Front 7

Name two physical properties of transition metals.

Back 7

High density

High melting and boiling points

Front 8

Name 4 chemical properties of transition metals.

Back 8

Form complex ions

Form coloured ions

Can work as catalysts

Variable oxidation states

Front 9

Why is it that transition metals can show variable oxidation states?

Back 9

4s and 3d are of similar energies and therefore electrons can be gained or lost using similar amounts of energy.

Front 10

What is a complex ion?

Back 10

A metal ion surrounded by co-ordinately bonded ligands.

Front 11

What is a ligand?

Back 11

A molecule, atom or ion that donates a pair of electrons to a central metal ion via a coordinate bond.

Front 12

What is a co-ordinate bond?

Back 12

A covalent bond where both electrons from the shared electron pair come from one atom.

Front 13

What is a monodentate ligand?

Back 13

A monodentate ligand is a ligand which can form one co-ordinate bond.

Front 14

Give 3 examples of monodentate ligands.

Back 14

Ammonia

Water

Cl- ions

Front 15

What is a multidentate ligand?

Back 15

A ligand which can form multiple co-ordinate bonds with a central metal ion.

Front 16

Give one example of a multidentate ligand.

Back 16

EDTA (4-)

ethylenediaminetetra-acetic acid.

Front 17

How many co-ordinate bonds can EDTA (4-) form, and where do they come from?

Back 17

6

4 from lone pairs on oxygen

2 from lone pairs on nitrogen

Front 18

What is a bidentate ligand?

Back 18

A ligand which can form TWO co-ordinate bonds.

Front 19

Give an example of a bidentate ligand and explain its structure.

Back 19

Ethane- 1,2- diamene

2 carbon chain with two NH3 molecules on the ends (NH2 CH2 CH2 NH2)

Lone pairs on the nitrogens

Front 20

How many co-ordinate bonds can the ligand ethane- 1,2- diamine form?

Back 20

2

Front 21

How do we display the overall charge of a complex ion?

Back 21

Outside of a pair of square brackets.

Front 22

How do you work out the oxidation state of the transition metal ion within the complex?

Back 22

Total charge of the complex- charge of all the ligands.

Front 23

What does the co-ordination number of a complex ion show?

Back 23

How many co-ordination bonds are formed around the central ion.

Front 24

What are the 3 most common co-ordination numbers?

Back 24

6, 4 and 2.

Front 25

Which ligands will form a complex ion with co-ordination number 6.

Back 25

EDTA (4-)

Small monodentate ligands such as water, ammonia and chloride ions.

Front 26

Which ligands will form a complex ion with co-ordination number 4.

Back 26

Large monodentates such as chloride ions.

Front 27

Which ligands will form a complex ion with co-ordination number 2.

Back 27

Ethane- 1,2- diamene.

Complexes with Ag

Front 28

What shape do complex ions with co-ordination number 6 form.

Back 28

Octohederal.

Front 29

What name is given to complexes involving a metal ion bound to 6 water ligands.

Back 29

Hexaqua complex.

Front 30

What shapes to complex ions with co-ordination number 4 usually take?

Back 30

Tetrahederal and less commonly square planar.

Front 31

Give one example of a complex ion with coordination number 4, that takes a square planar shape.

Back 31

Cisplatin.

Front 32

What shape do ions with co-ordination number 2 usually take?

Back 32

Linear planar.

Front 33

What metal usually forms complexes with co-ordination number 2, and a linear planar shape.

Back 33

Ag (silver).

Front 34

What is optical isomerism?

Back 34

A type of stereoisomerism

Stereoisomerism= same molecular formula, different arrangement of bonds in space.

Front 35

When are complex ions able to form enantiomers.

Back 35

When they have 3 bidentate ligands in an octohederal shape.

Front 36

Name the 2 types of stereoisomerism which transition metal ion complexes can undergo.

Back 36

Optical

E/Z

Front 37

Describe the structure of Cisplatin.

Back 37

Cisplatin is a Z (cis) isomer. It has a central platinum ion with 2 ammonia ligands and 2 Chloride ion ligands. Square planar shape.

Front 38

What is Cisplatin used for?

Back 38

Cisplatin is used to treat cancer by preventing uncontrolled cell division.

Front 39

What is transplatin?

Back 39

The E (trans) isomer of cisplatin which holds different biological effects.

Front 40

Name 2 downsides of Cisplatin?

Back 40

It also prevents cell reproduction in healthy, normal cells.

Kidney damage.

Front 41

When can octohederal complex ions form cis/trans isomers?

Back 41

4 ligands of 1 type and 2 of another type.

Two odd ligands opposite sides= trans (E)

Two odd ligands same side= cis (Z)

Front 42

In complex ions, what happens which causes the 3d shell of the transition metal to seperate into 2 energy levels?

Back 42

The attatchment of ligands.

Front 43

What property of transition metal ions allows them to form coloured ions?

Back 43

The 3d energy sub level seperates into 2 seperate energy levels from which electrons can jump between.

Front 44

When the 3d sub shell in the transition metal of a complex ion seperates into 2, which energy level do electrons generally occupy?

Back 44

The lower energy level.

Front 45

Where do electrons in a complex ion gain energy from, in order to breach the energy gap between the 2 3d energy levels?

Back 45

Visible light.

Front 46

In terms of complex transition metal ions, what is ΔE?

Back 46

Energy required to breach the gap between the 2 energy levels which are created when the 3d energy level is seperated into 2.

Front 47

What is the equation used to work out ΔE, in terms of transition metal ions?

Back 47

ΔE= hv= hc/λ

Front 48

In the equation 'ΔE= hv= hc/λ'

What do all of the letters represent?

Back 48

ΔE = energy gap

h = plancks constant (Js)

v = freq of light absorbed (Hz)

c = speed of light (ms-1)

λ= Wavelength of light (m)

Front 49

What is plancks constant?

Back 49

6.63 x 10-34 js

Front 50

What happens when light hits a transition metal ion? Why?

Back 50

Some of the frequencies of light are absorbed as electrons jump from one energy level to another, in the 2 energy levels that are created when the 3d sub level is split.

Front 51

What determines which frequences of light are absorbed by a complex transition metal ion?

Back 51

The size of the energy gap (ΔE)

Front 52

What happens to the frequences of light which are not absorbed by the transition metal ion?

Back 52

They are reflected and this is what we see.

Front 53

In a transition metal complex ion, what colour would the ion be if the 3d sub level was full or completely empty?

Back 53

The ion would be colourless or white, as there will be no electrons to jump between the 2 energy levels that are created when the 3d sub level splits. No jumping of electrons= no light absorption.

Front 54

Name 4 factors which affect the size of the energy gap in the 3d subshell of a transition metal ion.

Back 54

Central metal ion

Oxidation state

Ligands

Co-ordination number