Transition metals

Question 1

What are d block transition metals

Answer 1

The d-block transition metals are metals with an incomplete d subshell in at least one of their ions.

Question 2

The filling of d orbitals follows what principal

Answer 2

The filling of the d orbitals follows the aufbau principle, with the exception of chromium and copper atoms.

Question 3

Why do chromium and copper atoms not follow the aufbau principal

Answer 3

These exceptions are due to the special stability associated with the d subshell being half- filled or completely filled.

Question 4

What happens to electrons when atoms from the first row of transition elements form ions

Answer 4

When atoms from the first row of the transition elements form ions, it is the 4s electrons that are lost first rather than the 3d electrons.

Question 5

When is a element said to be in a particular oxidation state

Answer 5

An element is said to be in a particular oxidation state when it has a specific oxidation number.

Question 6

How many states can a transition metal have in its compounds

Answer 6

A transition metal can have different oxidation states in its compounds.

Question 7

What colours are compounds of the same transition metal in different oxidation states

Answer 7

Compounds of the same transition metal in different oxidation states may have different colours.

Question 8

Oxidation

Answer 8

Oxidation can be defined as an increase in oxidation number.

Question 9

Reduction

Answer 9

Reduction can be considered as a decrease in oxidation number.

Question 10

What can be used to determine whether ox or red has occurred in transition metals

Answer 10

Changes in oxidation number of transition metal ions can be used to determine whether oxidation or reduction has occurred.

Question 11

What is the difference in compounds containing Hugh oxidation states compared to low oxidation states

Answer 11

Compounds containing metals in high oxidation states are often oxidising agents, whereas compounds with metals in low oxidation states are often reducing agents.

Question 12

What are ligands

Answer 12

Ligands may be negative ions or molecules with non-bonding pairs of electrons that they donate to the central metal atom or ion, forming dative covalent bonds.

Question 13

Ligands can be classified as:

Answer 13

monodentate, bidentate, up to hexadentate.

Question 14

How can you deduce the ligand classification

Answer 14

It is possible to deduce the ligand classification from a formula or structure of the ligand or complex.

Question 15

What is the coordination number

Answer 15

The total number of bonds from the ligands to the central transition metal is known as the coordination number.

Question 16

What happens to d orbitals in a complex of a transition metal

Answer 16

In a complex of a transition metal, the d orbitals are no longer degenerate.

Question 17

When does splitting of d orbitals to higher and lower energies occur

Answer 17

Splitting of d orbitals to higher and lower energies occurs when the electrons present in approaching ligands cause the electrons in the orbitals lying along the axes to be repelled.

Question 18

What are strong field ligands

Answer 18

Ligands that cause a large difference in energy between subsets of d orbitals are strong field ligands.

Question 19

What are weak field ligands

Answer 19

Weak field ligands cause a small energy difference.

Question 20

What is the spectrochemical series

Answer 20

Ligands can be placed in an order of their ability to split d orbitals. This is called the spectrochemical series.

Question 21

When is light absorbed

Answer 21

Light is absorbed when electrons in a lower energy d orbital are promoted to a d orbital of higher energy.

Question 22

What happens if light of one colour is absorbed

Answer 22

If light of one colour is absorbed, then the complementary colour will be observed.

Question 23

When do electrons transition to higher energy levels

Answer 23

Electrons transition to higher energy levels when energy corresponding to the ultraviolet or visible regions of the electromagnetic spectrum is absorbed.

Question 24

When do electrons transition to higher energy levels

Answer 24

Electrons transition to higher energy levels when energy corresponding to the ultraviolet or visible regions of the electromagnetic spectrum is absorbed.

Question 25

When do electrons transition to higher energy levels

Answer 25

Electrons transition to higher energy levels when energy corresponding to the ultraviolet or visible regions of the electromagnetic spectrum is absorbed.

Question 26

What else can transition metals act as

Answer 26

Transition metals and their compounds can act as catalysts.

Question 27

What is the state of heterogenous catalysts

Answer 27

Heterogeneous catalysts are in a different state to the reactants.

Question 28

What state are homogenous catalysts in

Answer 28

Homogeneous catalysts are in the same state as the reactants.

Question 29

Homogenous catalysts

Answer 29

Homogeneous catalysis can be explained in terms of changing oxidation states with the formation of intermediate complexes.