transition metals

Question 1

why do transition metals have high boiling points

Answer 1

both 4s and 3d electrons delocalised
stronger metallic bond

Question 2

define transition metal

Answer 2

an element that has one or more stable ions with incompletely filled d orbitals

Question 3

what is a d block element

Answer 3

have their highest energy, last valence electron in a d orbital

Question 4

electron configuration of copper

Answer 4

[Ar] 3d10 4s1

Question 5

electron configuration of chromium

Answer 5

[Ar] 3d5 4s1

Question 6

which electrons are lost first

Answer 6

4s

Question 7

how can the maximum oxidation number of a transition metal be calculated

Answer 7

adding the number of unpaired 3d electrons to the total number of 4s electrons

Question 8

what is a characteristic property of transition metals

Answer 8

ability to form ions with various oxidation states

Question 9

what is a ligand

Answer 9

a species dative covalently bonded to a central metal ion

Question 10

what is a coordination number

Answer 10

number of coordinate bonds from ligands to central metal ion

Question 11

order of how to name a ligand

Answer 11

1 number of ligands
2 name of ligand
3 central metal ion
4 oxidation number of metal ion

Question 12

one ligand

Answer 12

mono-

Question 13

two ligands

Answer 13

di-

Question 14

three ligands

Answer 14

tri-

Question 15

four ligands

Answer 15

tetra-

Question 16

five ligands

Answer 16

penta-

Question 17

six ligands

Answer 17

hexa-

Question 18

CN- ligand name

Answer 18

cyano

Question 19

OH- ligand name

Answer 19

hydroxo

Question 20

H2O ligand name

Answer 20

aqua

Question 21

NH3 ligand name

Answer 21

ammine

Question 22

CO ligand name

Answer 22

carbonyl

Question 23

what do complexes with a net negative charge’s metal ions end in (name)

Answer 23

-ate

Question 24

copper overall negative charge name

Answer 24

cuprate

Question 25

ion overall negative charge name

Answer 25

ferrate

Question 26

name [Cr(Cl)2(H2O)4]+

Answer 26

di chloro tetra aqua chromium (III) ion

Question 27

why do complex ions form coloured compounds

Answer 27

- ligand binding causes d orbitals to split - light of certain wavelengths absorbed - promotes e- to a higher energy orbital - difference in energy levels determines the frequency absorbed and hence the colour observed - remaining wavelengths of light are transmitted - seen as colour in the visible region

Question 28

what does the extent of the d orbital splitting (and hence the colour of the complex) depend on (3)

Answer 28

- nature of the ligand - oxidation state of transition metal ion - co-ordination number

Question 29

colour of V2+

Answer 29

violet

Question 30

colour of V3+

Answer 30

green

Question 31

colour of V4+

Answer 31

blue

Question 32

colour of V5+

Answer 32

yellow

Question 33

why does a solution of Zn2+ have no colour

Answer 33

[Ar] 3d10 full d sub shell no unpaired d orbital e- movement of e- between d orbitals not possible

Question 34

what is deprotonation

Answer 34

reaction in which the base removes a proton from the water molecules

Question 35

what is a ligand exchange reaction

Answer 35

where a stronger ligand replaces a weaker one

Question 36

mono dentate ligand

Answer 36

forms one co-ordinate bond eg CN-

Question 37

polydentate ligand

Answer 37

can form several co-ordinate bonds eg EDTA 4-

Question 38

bidentate ligand

Answer 38

forms two co-ordinate bonds eg ethandioate

Question 39

iron (II) solution

Answer 39

pale green [Fe(H20)6]2+

Question 40

iron (II) solution + sodium hydroxide

Answer 40

green precipitate formed insoluble with excess red/brown on standing

Question 41

iron (II) solution + sodium hydroxide equation

Answer 41

[Fe(H2O)6]2+(aq) + 2OH- (aq) --> [Fe(OH)2(H2O)4] (s) + 2H2O (l)

Question 42

iron (II) solution + ammonia

Answer 42

green precipitate formed insoluble with excess red/brown on standing

Question 43

iron (II) solution + ammonia equation

Answer 43

[Fe(H2O)6]2+ (aq) + 2NH3 (aq) --> [Fe(OH)2(H2O)4] (s) + 2NH4+ (aq)

Question 44

iron (II) solution + aqueous sodium carbonate produces..

Answer 44

[Fe(OH)2(H2O)4] (s) green precipitate

Question 45

iron (III) solution

Answer 45

yellow/brown [Fe(H2O)6]3+

Question 46

iron (III) solution + sodium hydroxide

Answer 46

red/brown precipitate insoluble with excess

Question 47

iron (III) solution + sodium hydroxide equation

Answer 47

[Fe(H2O)6]3+ (aq) + 3OH- (aq) --> [Fe(OH)3(H2O)3](s) + 3H2O(l)

Question 48

iron (III) solution + ammonia

Answer 48

red/brown precipitate insoluble with excess

Question 49

iron (III) solution + ammonia equation

Answer 49

[Fe(H2O)6]3+ (aq) + 3NH3 (aq) --> [Fe(OH)3(H2O)3] (s) + 3NH4+ (aq)

Question 50

iron (III) solution + aqueous sodium carbonate produces...

Answer 50

[Fe(OH)3(H2O)3] (s) red/brown precipitate

Question 51

chromium (III) solution

Answer 51

green [Cr(H2O)6]3+

Question 52

chromium (III) solution + sodium hydroxide

Answer 52

green precipitate soluble with excess - dark green solution

Question 53

chromium (III) solution + sodium hydroxide equation

Answer 53

[Cr(H2O)6]3+ (aq) + 3OH (aq) --> [Cr(H2O)3(OH)3] (s) + 3H2O (l) with excess --> [Cr(OH)6]3- (aq)

Question 54

chromium (III) solution + ammonia equation

Answer 54

[Cr(H2O)6]3+ (aq) + 3NH3 (aq) --> [Cr(H2O)3(OH)3] (s) + 3NH4+ (aq) with excess --> [Cr(NH3)6]3+ (aq)

Question 54

chromium (III) solution + ammonia

Answer 54

green precipitate soluble with excess - purple solution

Question 55

cobalt (II) solution

Answer 55

pink [Co(H2O)6]2+

Question 56

cobalt (II) solution + sodium hydroxide

Answer 56

blue precipitate insoluble with excess turns pink on standing

Question 57

cobalt (II) solution + sodium hydroxide equation

Answer 57

[Co(H2O)6]2+ (aq) + 2OH- (aq) --> [Co(H2O)4(OH)2] (s) + 2H2O (l)

Question 58

cobalt (II) solution + ammonia

Answer 58

blue precipitate soluble with excess - brown solution darkens on standing

Question 59

cobalt (II) solution + ammonia equation

Answer 59

[Co(H2O)6]2+ (aq) + 2NH3 (aq) --> [Co(H2O)4(OH)2] (s) + 2NH4+ (aq) with excess --> [Co(NH3)6]2+ (aq)

Question 60

copper (II) solution

Answer 60

blue [Cu(H2O)6]2+

Question 61

copper (II) solution + sodium hydroxide

Answer 61

pale blue precipitate insoluble with excess

Question 62

copper (II) solution + sodium hydroxide equation

Answer 62

[Cu(H2O)6]2+ (aq) + 2OH- (aq) --> [Cu(H2O)4(OH)2] (s) + 2H2O (l)

Question 63

copper (II) solution + ammonia

Answer 63

pale blue precipitate soluble with excess - deep blue solution

Question 64

copper (II) solution + ammonia equation

Answer 64

[Cu(H2O)6]2+ (aq) + 2NH3 (aq) --> [Cu(H2O)4(OH)2] (s) + 2NH4+ (aq) with excess --> [Cu(H2O)2(NH3)4]2+ (aq)

Question 65

what kind of reaction is metal ion solution with NaOH

Answer 65

deprotonation

Question 66

what kind of reaction is metal ion solution with excess NaOH

Answer 66

deprotonation

Question 67

what kind of reaction is metal ion solution with NH3

Answer 67

deprotonation

Question 68

what kind of reaction is metal ion solution with excess NH3

Answer 68

ligand exchange