Transition Metals

Question 1

Define Transition Metal

Answer 1

Metal atom with partially filled d subshell

Question 2

What transition metals do we cover?
What is an exception that isn’t a transition metal?

Answer 2

Top row Sc-Zn
Zn exception 3d10 subshell for atoms & ions

Question 3

How do transition metals form complexes?

Answer 3

Forms coordinate bond with ligand from e-s from ligand for dative bond

Question 4

Define a Ligand

Answer 4

Particle with lone pair that forms a co-ordinate bond with metals

Question 5

Define a Complex

Answer 5

Metal ion + ligand with a co-ordinate bond

Question 6

Define co-ordination number

Answer 6

Number of co-ordinate bonds in a complex

Question 7

Define a Lewis Base

Answer 7

Lone pair donor

Question 8

Define a Lewis Acid

Answer 8

Lone pair acceptor

Question 9

What shapes do 4 co-ordinate bonds make?

Answer 9

Tetrahedral mostly but sometimes square planar

Question 9

What shape do 6 co-ordinate bonds make?

Answer 9

Octahedral

Question 10

What shape do 2 co-ordinate bonds make

Answer 10

Linear

Question 11

What type of ligand forms 2 co-ordinate bonds?

Answer 11

Bidentate ligands

Question 12

How do transition metals form coloured ions?

Answer 12

They absorb different wavelengths of light

Question 13

What does the colour of the transition metal ion depend on?

Answer 13

1. The metal ion
2. The Type of ligand attached
3. The co-ordination number
4. The oxidation state of the transition metal

Question 14

What happens to transition metal d orbitals when ligands bond?

Answer 14

When ligands bond 5 d orbitals don’t have same energy
e- excited from lower d orbitals to higher d orbitals

Question 15

How do coloured ions form?

Answer 15

Different energy of d orbitals is in the UV/Visible region -> d-d

Question 16

Outline the Planck equation with units

Answer 16

E diff between 2 d-d orbitals (J) = Planck’s constant (6.63x10-34 Jhz-1) X frequency (hz)
E diff = hf