inorganic chem; transition metals

Question 1

Transition element

Answer 1

It’s a d-block element that can form at least one stable ion with a partially filled d-subshell

Question 2

Exceptions of transition elements & why

Answer 2

Zinc & Scandium
As they don’t form a stable ion with a partially filled sub-shell

Question 3

Which transition elements fill their orbitals differently?

Answer 3

Chromium & copper

Question 4

How are the electrons filled in chromium & copper’s orbitals?

Answer 4

An e- from the 4s orbital moves into the 3d orbital to create a more a stable half full / full 3d sub-shell

Question 5

How do transition metals lose their electrons?

Answer 5

Lose e- from 4s then 3d orbital

Question 6

Transition metals properties

Answer 6

• variable oxidation states
• form coloured ions in solution
• good catalyst

Question 7

Why do transition metals have variable oxidation states?

Answer 7

• As their e- sit in 4s & 3d orbitals which are very close to each other
• so e- are gained & lost using similar amount of energy

Question 8

Transition metals forming coloured ion solutions

Answer 8

Question 9

Complex ion

Answer 9

It’s where a central transition metal ion is surrounded by ligands bonded by dative covalent (coordinate) bonds — ligands have at least 1 lone pair of e- which is used to form coordinate bond with the metal

Question 10

Ligand

Answer 10

It’s an ion, atom or molecule that has at least 1lone pair of e- — they can be monodenate, bidenate or polydenate

Question 11

Monodenate (unidenate) ligand

Answer 11

A ligand with only 1 lone pair of e-

Question 12

Bidenate ligand

Answer 12

A ligand with 2 lone pairs of e-

Question 13

Multidenate ligand

Answer 13

Ligand with more than 1 coordinate bond

Question 14

Example of multidenate ligand

Answer 14

EDTA4-
Forms 6 coordinate binds with central metal ion

Question 15

The shape of the complex ion depends on:

Answer 15

• the size of ligands
• the coordination number

Question 16

Coordination number

Answer 16

No.of coordinate bonds in a complex ion

Question 17

Complexes with a coordination number of 6 form…

Answer 17

…octahedral shapes — bond angle 90˚

Question 18

Complexes with a coordination number of 4 form…

Answer 18

…tetrahedral (109.5˚) & square planar (90˚) shapes

Question 19

Example of a square planar complex

Answer 19

Anti-cancer drug cis-platin

Question 20

Complexes with a coordination number of 2 form…

Answer 20

…linear shapes — bond angle 180˚

Question 21

Example of linear shape complex

Answer 21

Tollen’s reagent

Question 22

Complexes overall charge which is the same as…

Answer 22

…the oxidation state

Question 23

How is the total oxidation state of a metal calculated?

Answer 23

Total oxidation state of metal = total oxidation state - total oxidation state of ligands

Question 24

… is a multidenate ligand that is doing in haemoglobin and it has an … shape

Answer 24

…Haem
…octahedral

Question 25

How does haemoglobin transport oxygen?

Answer 25

- O2 substitutes the water log and in the lungs where O2 conc is high to form oxyhaemoglobin — transported around the body - oxyhaemoglobin gives up O2 to a place where its needed - water takes the place & haemoglobin returns back to the lungs to repeat the process

Question 26

What happens when carbon monoxide is inhaled?

Answer 26

- the water ligand is replaced with a carbon monoxide ligand - carbon monoxide bonds strongly so it’s not readily replaced by O2 or water - this means that O2 cannot be transported — leads to O2 starvation in organs

Question 27

Complex ions such as… show…

Answer 27

…octahedral complexes with 3 bidentate ligands … optical isomerism

Question 28

Complex ions also show … , shown in…

Answer 28

…cis-trans isomerism …octahedral complexes with 4 ligands of the same type & 2 ligands of a different type

Question 29

How are cis-trans isomers identified?

Answer 29

- trans isomer: if the 2 different ligands are opposite each other - cis isomer: if the 2 different ligands are adjacent to each other

Question 30

What complex ion shape also shows cis-trans isomerism?

Answer 30

Square planar complexes — 2 ligands of the same type & 2 ligands of a different type

Question 31

D-orbital splitting

Answer 31

This is where the d-subshell is split into 2 when ligands bond with the central metal ion

Question 32

Process of d-orbital splitting

Answer 32

- e- absorb light, some energy moves from the lowest energy level (ground state) to a higher energy level (excited state) - for this to happen the energy from the light must equal ∆E

Question 33

What is the size ∆E dependent on?

Answer 33

- the central metal ion & its oxidation state - the type of ligand - coordination number

Question 34

How is the energy absorbed by the e- calculated?

Answer 34