Chemistry Unit 5 - Transition Metals

Front 1

Which block are transition metals found in ?

Back 1

The d-Block

Front 2

Definition of transition metal

Back 2

A transition metal is a metal that can form one ore more stable ions with a partially filled d-subshell

Front 3

Which two d-Block elements are not transition metals and why

Back 3

Scandium as it forms a 3+ ion with an empty subshell and Zinc which forms a 2+ ion with a full d-subshell. Both of these are not transition metals by definition (transition metals have partially filled d-subshells)

Front 4

When ions form which electrons are removed first

Back 4

s electrons are removed first, so the 4s subshell will always be removed first

Front 5

What are the physical properties of transition metals

Back 5

They all have a high density, high melting and boiling points and their ionic radii are more or less the same

Front 6

What are the special chemical properties of transition metals

Back 6

They have variable oxidation states, can form complex ions and coloured ions and are good catalysts

Front 7

Colour?

+7 oxidation state MnO4 (Manganese Oxide)

Back 7

Purple

Front 8

Colour?

+6 oxidation state Cr2O7 2- (Chromium oxide)

Back 8

Orange

Front 9

Colour?

+5 Oxidation state VO2 + (Vanadium Oxide)

Back 9

Yellow

Front 10

Colour?

+4 Oxidation state VO 2+ (Vanadium Oxide)

Back 10

Blue

Front 11

Colour?

+3 Oxidation state V 3+ (Vanadium)

Back 11

Green

Front 12

Colour?

+ 3 Oxidation state Cr 3+ (Chromium)

Back 12

Green/Violet

Front 13

Colour?

+3 Oxidation state Fe 3+ (Iron)

Back 13

Yellow

Front 14

Colour?

+2 Oxidation state V 2+ (Vanadium)

Back 14

Violet

Front 15

Colour?

+2 Oxidation state Mn 2+ (Manganese)

Back 15

Pale pink

Front 16

Colour?

+2 Oxidation state Fe 2+ (Iron)

Back 16

Pale green

Front 17

Colour?

+2 Oxidation state Co 2+ (Cobalt)

Back 17

Pink

Front 18

Colour?

+2 Oxidation state Ni 2+

Back 18

Green

Front 19

Colour?

+2 Oxidation state Cu 2+

Back 19

Blue

Front 20

What is a complex

Back 20

A metal ion surrounded by coordinately bonded ligands

Front 21

What is a ligand

Back 21

An atom, ion or molecule that donates a pair of electrons to a central metal ion

Front 22

What is the coordination number

Back 22

The number of coordinate bonds that are formed with the central metal ion

Front 23

What size ligands form 6 coordination number

Back 23

Small Ligands

Front 24

What size ligands form 4 coordination number

Back 24

Large ligands

Front 25

What molecular shape does a 6 coordinate bonds form

Back 25

Octahedral shape

Front 26

What molecular shape does a 4 coordinate bonds form

Back 26

Tetrahedral shape

Front 27

Some silver complexes have 2 coordinate bonds. What molecular shape does that form

Back 27

Linear shape

Front 28

What is the overall charge on the complex ion represented by

Back 28

Total oxidation stae

Front 29

How do you work out oxidation state of the metal

Back 29

oxidation state of metal ion = total oxidation state - the sum of the oxidation states of the ligands

Front 30

What is a unidentate

Back 30

a ligand with one coordinate bond

Front 31

What is a multidentate

Back 31

a ligand with more than two coordinate bonds

Front 32

What is a bidentate

Back 32

a ligand with two coordinate bonds

Front 33

How do transition metals formulate colours

Back 33

Ligands bonded cause the d subshell to split into two different energy levels. Electrons tend to occupy the lower level and need a certain amount of energy to jump to the next level obtained from visible light. The visible light absorbed are specific frequencies, the other frequencies are reflected and is the colour that can be observed

Front 34

What factors affect the amount of energy in the form of visible light needed to jump the energy gap to a higher energy level in the d subshell

Back 34

The metal ion, oxidation state, the ligands and the coordination number of these ligands will affect the energy gap

Front 35

Colour?

[Fe(H20)6]2+

+2 Oxidation state

Back 35

Pale green

Front 36

Colour?

[Fe(H2O)6]2+

+3 Oxidation state

Back 36

Yellow

Front 37

Colour?

[V(H20)6]2+

+2 Oxidation state

Back 37

Violet

Front 38

Colour?

[V(H2O)6]3+

+3 Oxidation state

Back 38

Green

Front 39

Colour?

[Cu(H20)6]2+

6 coordination number

Back 39

blue

Front 40

Colour?

[CuCL4]2-

4 Coordination number

Back 40

Yellow

Front 41

Colour?

[Co(H20)6]2+

+2 Oxidation state

Back 41

Pink

Front 42

Colour?

[Co(NH3)6]2+

+2 Oxidation state

Back 42

Straw coloured

Front 43

Colour?

Cr2O7 2-

+6 Oxidation state

Back 43

Orange

Front 44

Colour?

CrO4 2-

+6 Oxidation state

Back 44

Yellow

Front 45

Colour?

Cr 3+

+3 Oxidation state

Back 45

Green (Violet)

Front 46

Colour?

Cr 2+

+2 Oxidation state

Back 46

Blue

Front 47

Colour?

[Co(H20)6] 2+

+2 Oxidation state

Back 47

Pink solution

Front 48

Colour?

[Co(H20)4(OH)2]

Back 48

Blue precipitate

Front 49

Colour?

[Co(NH3)6] 2+

+2 Oxidation state

Back 49

Straw coloured solution

Front 50

Colour?

[Co(NH3)6] 3+

+3 Oxidation state

Back 50

Dark brown solution