IB Chemistry on Properties of Transition Metal and Magnetism

1. PeriodicTable of elements– dividedinto s, p, d, f blocks
p block
• p orbital partially fill
d block
• d orbital partially filled
• transition element
f block
• f orbital partially fill
s block
• s orbital partiallyfill

2. Periodic Table – s, p d, f block elements block elements
• s orbitals partially fill
p block elements
• p orbital partially fill
d block elements
• d orbitals partially fill
• transition elements
1 H 1s1
2 He 1s2
11 Na [Ne] 3s1
12 Mg [Ne] 3s2
5 B [He] 2s2 2p1
6 C [He] 2s2 2p2
7 N [He] 2s2 2p3
8 O [He] 2s2 2p4
9 F [He] 2s2 2p5
10 Ne [He] 2s2 2p6
13 Al [Ne] 3s2 3p1
14 Si [Ne] 3s2 3p2
15 P [Ne] 3s2 3p3
16 S [Ne] 3s2 3p4
17 CI [Ne] 3s2 3p5
18 Ar [Ne] 3s2 3p6
19 K [Ar] 4s1
20 Ca [Ar] 4s2
21 Sc [Ar] 4s2 3d1
22 Ti [Ar] 4s2 3d2
23 V [Ar] 4s2 3d3
24 Cr [Ar] 4s1 3d5
25 Mn [Ar] 4s2 3d5
26 Fe [Ar] 4s2 3d6
27 Co [Ar] 4s2 3d7
28 Ni [Ar] 4s2 3d8
29 Cu [Ar] 4s1 3d10
30 Zn [Ar] 4s2 3d10
n = 2 period 2
3 Li [He] 2s1
4 Be [He] 2s2
Click here video s,p,d,f blocks,Click here video on s,p,d,f notationClick here electron structure
Video on electron configuration
f block elements
• f orbitals partially fill

3. Periodic Table – s, p d, f blocks element
Electron structure
Chromium d block (Period 4)
1s2 2s2 2p6 3s2 3p6 4s1 3d5
[Ar] 4s1 3d5
Electron structure
Germanium p block, Gp 14 (Period 4)
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p2
[Ar] 4s2 3d10 4p2
Electron structure
Lead p block, Gp 14 (Period 6)
1s2 2s2 2p6 3s2 3p6 3d104s2 4p6 5s2 4d10 5p6 6s2 4f14 5d106p2
[Xe] 6s2 4f14 5d10 6p2
Electron structure
Iodine p block, Gp 7 (Period 5)
1s2 2s2 2p6 3s2 3p6 3d104s2 4p6 5s2 4d10 5p5
[Kr] 5s2 4d10 5p5
Electron structure
Cadmium d block (Period 5)
1s2 2s2 2p6 3s2 3p6 3d104s2 4p6 5s2 4d10
[Kr] 5s2 4d10
Electron structure
Mercury d block (Period 6)
1s2 2s2 2p6 3s2 3p6 3d104s2 4p6 5s2 4d10 5p6 6s2 4f14 5d10
[Xe] 6s2 4f14 5d10
Gp 14 -4 valence electron Gp 17 - 7 valence electron
Gp 14 - 4 valence electrond block – d partially filledd block – d partially filled
d block – d partially filled
О
О
О
О
О
О

4. 3d
Nuclear charge increase IE increase slowly
3d elec added to 3d sub level
3d elec – shield the outer 4s elec from nuclear charge
Ionization Energy – Transition metal Why IE increases slowly across ?IE Transition metal
Sc Ti V Cr Mn Fe Co
Period 4
Ni Cu
Shielding nuclear charge by 3d electron
+21 +22 +23 +24 +25 +26 +27 +28 +29
4s
Sc Ti V Cr Mn Fe Co Ni Cu Zn
+21 +22 +23 +24 +25 +26 +27 +28 +29 +30
Nuclear pull
Shielding by 3d electron
Shielding by 3d electron
↓
Balance increase in nuclear charge
↓
Small increase in IE
↓
Easier to lose outer electron
↓
Variable oxidation state

5. Transition Metal (d block )
Across period
Cr - 4s13d5
• half filled more stable
Cu - 4s13d10
• fully filledmore stable
Ca
4s2
K
4s1
Transitionmetal have partially fill 3d orbital
• 3d and 4s electron can be lost easily
• electron fill from 4s first then 3d
• electron lost from 4s first then 3d
• 3d and 4s energy level close together (similar in energy)
Filling electron- 4s level lower, fill first Losing electron- 4s higher, lose first
3d
4s

6. d block element with half/partially fill d orbital / sublevel in one or more of its oxidation states
Partially fill d orbital
Lose electron
↓
Formation ions
Sc3+
4s03d0
Zn 2+
4s03d10
Zn → Zn2+
4s2
3d10 4s0
3d10
fully fill d orbital
Sc → Sc 3+
4s2
3d1 4s0
3d0
empty d orbital
Transition Metal (d block )
NOT
Transition element.
NOT
Transition element.
О
О

7. Transition Metal
Physical properties Chemical properties
Element properties Atomic properties
• High electrical/thermal conductivity
• High melting point
• Malleable
• Ductile
• Ferromagnetic
• Ionization energy
• Atomic size
• Electronegativity
Transition Metal ( d block)
Gp 1 Gp 17
Sc
Ionization energy
↓
IE increase ↑ slowly
↓
Shielding of nuclear
charge by 3d elec
↓
Electrostatic force
attraction ↓
Atomic size
↓
Decrease ↓ slowly
↓
Shielding of outer
electron from
nuclear charge by
3d elec
Electronegativity
↓
EN increase ↑ slowly
Physical Properties
Zn
EN increase ↑
Atomic size decrease ↓
IE increase ↑
• Formation of complexion
• Formation coloured complexes
• Variable oxidation states
• Catalytic activity
Formation complexion Formation coloured complexes
Catalytic activity Variable Oxidation states
molecule adsorp on
surface catalyst
V Cr Mn Fe Co Ni
+2 +2 +2 +2 +2 +2
+3 +3 +3 +3 +3 +3
+4 +4 +4 +4 +4 +4
+5 +5 +5 +5 +5
+6 +6 +6
+7

8. Transition Metal – Variable Oxidation States
+3 +3 +3+3+3 +3
+2 +2 +2 +2 +2
+4 +4
+5
+2
+6 +6
+7
+2
+3
+4
+5
+6
+7
ScCI3 TiCI3 VCI3 CrCI3
MnCI3
FeCI3
CrCI2
MnCI2
FeCI2 CoCI2 NiCI2 CuCI2 ZnCI2
TiCI4
MnCI4V2O5
Cr2O7
2-
+2
(VO2)2+
(MnO4)2-
(MnO4)-
oxides
oxyanion
chlorides
+2 oxidation state more common+3 oxidation state more common
+3
CoCI3
Oxidation state Mn is highest +7
Highest oxidation state exist
↓
Element bond to oxygen
(oxide/oxyanion)
Oxidation state +2 common (Co → Zn)
↓
Harder to lose electron
↓
Nuclear charge (NC ↑) from Co - Zn
Oxidation state +3 common (Sc → Fe)
↓
Easierto lose electron
↓
Nuclear charge (NC ↓) from Sc - Fe
Transition metal – variable oxidation state
↓
4s and 3d orbital close in energy
↓
Easy to lose electron from 4s and 3d level
Ionic bond – more common for lower oxi states
TiCI2 – Ionic bond
Covalent bond – more common for higher oxi states
TiCI4 – Covalent bond
Highest oxidation states – bind to oxygen

9. Transition Metal
Formation coloured complexes Variable Oxidation states
Sc Ti V Cr Mn Fe Co Ni Cu Zn
+1
+2 +2 +2 +2 +2 +2 +2 +2 +2 +2
+3 +3 +3 +3 +3 +3 +3 +3
+4 +4 +4 +4 +4 +4 +4
+5 +5 +5 +5 +5
+6 +6 +6
+7
+3- most common
oxi state
+ 2- most common
oxi state
+ 7- Highest
oxi state
Click here vanadium ion complexes Click here nickel ion complexes
V5+/ VO2
+ - yellow
V4+/ VO2+ - blue
V3+ - green
V2+ - violet
NiCI2 - Yellow
NiSO4 - Green
Ni(NO3)2 - Violet
NiS - Black
Diff oxidation states
Colour formation
Nature of
transition metal
Oxidation
state
Diff ligands Shape
Stereochemistry
Diff ligandDiff metals
MnCI2 - Pink
MnSO4 - Red
MnO2 - Black
MnO4
- - Purple
Cr2O3 - Green
CrO4
2- - Yellow
CrO3 - Red
Cr2O7
2- - Orange
Shape/ Stereochemistry
Tetrahedral Octahedral
BlueYellow

10. TransitionMetal ion
• High charged density metal ion
• Partially fill 3d orbital
• Attract to ligand
• Form dative/co-ordinatebond
(lone pair from ligand)
Ligand
• Neutral/anion species that donate lone pair/non bonding electron pair to metal ion
• Lewis base, lone pair donor – dative bond with metal ion
Ligand
+2
Formation complex ion
TransitionMetal ion
Neutral ligand Anion ligand
H2O
NH3
CO
CI–
CN–
O2-
OH–
SCN–
: CI :
:.
Monodentate Bidentate
Polydentate
C2O4
2- C2H4(NH2)2
Drawingcomplex ion
• Overall charged on complex ion
• Metal ion in center (+ve charged)
• Ligand attach
• Dative bond from ligand
+3
4 water ligand attach
4 dative bond
Coordination number= 4
6 water ligand attach
6 dative bond
Coordination number= 6
Transitionmetal + ligand= Complex Ion

11. Coordination
number
Shape Complex ion
(metal + ligand)
Ligand
(charged)
Metal ion
(Oxidation #)
Overall charge
on complex ion
linear [Cu(CI2)]- CI = -1 +1 - 1
[Ag(NH3)2]+ NH3 = 0 +1 + 1
[Ag(CN)2]- CN = -1 +1 - 1
Square
planar
[Cu(CI)4]2- CI = -1 +2 - 2
[Cu(NH3)4]2+ NH3 = 0 +2 +2
[Co(CI)4]2- CI = -1 +2 - 2
Tetrahedral [Cu(CI)4]2- CI = -1 +2 - 2
[Zn(NH3)4]2+ NH3 = 0 +2 + 2
[Mn(CI)4]2- CI = -1 +2 - 2
Octahedral [ Cu(H2O)6]2+ H2O = 0 +2 + 2
[Fe(OH)3(H2O)3] OH = -1
H2O = 0
+3 o
[Fe(CN)6]3- CN = -1 +3 - 3
[Cr(NH3)4CI2]+ NH3 = 0
CI = -1
+3 + 1
Types of ligand:
• Monodentate– 1 lone pair electrondonor– H2O, F-, CI-, NH3, OH-, SCN- CN-
• Bidentate – 2 lonepair electrondonor–1,2 diaminoethaneH2NCH2CH2NH2, ethanedioate(C2O4)2-
•Polydentate – 6 lone pair electrondonor– EDTA4- (ethylenediaminetetraaceticacid)
Complex ion with diff metal ion, ligand,oxidationstate and overallcharge
Mn+L: :L
Mn+
:L
:L
L:
L:
Mn+
:L
:L
:L
:L
Mn+
:L
:L
:L
:L
:L
:L
Coordination number
– number of ligand
around central ion
2
4
4
6

12. Ligand
• Neutral/anion species that donate lone pair/non bonding electron pair to metal ion
• Lewis base, lone pair donor – dative bond with metal ion
Neutral ligand Anion ligand
H2O
NH3
CO
CI–
CN–
O2-
OH–
SCN–
: CI :
:.
Monodentate
Bidentate Polydentate
C2O4
2- C2H4(NH2)2
Ligand displacement
Co/CN > en > NH3 > SCN- > H2O > C2O4
2- > OH- > F- > CI- > Br- > I-
Spectrochemicalseries
Tetraaqua
copper(II)ion
H2O displace
by CI-
2+
CI- displace
by NH3
Tetrachloro
copper(II)ion
Strongerligand displaceweakerligand
Tetraamine
copper(II)ion
О
О
Stronger
ligand
Stronger
ligand
Chelating agent
EDTA – for removal of Ca2+
• Prevent blood clotting
• Detoxify by removing heavy
metal poisoning

13. 4s
3d
Magnetic properties of transition metals
Paired electron – spin cancel – NO net magnetic effect
Ti V Cr Mn Fe Co
Diamagnetism
↓
Paired electron
↓
No Net magnetic effect
(Repel by magnetic field)
Ni Zn
Spin cancel
Sc
Spinning electron in atom – behave like tiny magnet
Unpaired electron – net spin – Magnetic effect
Spin cancel Net spin
Paramagnetism
↓
Unpaired electron
↓
Net magnetic effect
(Attract by magnetic field)
Material
Diamagnetic Paramagnetic Ferromagnetic
• Iron
• Cobalt
• Nickel
Zn2+ Mn2+
Click here paramagnetism Click here paramagnetism Click here levitation bismuth Click here levitation

14. 4s
3d
Magnetic properties of transition metal
Ti V Cr Mn Fe Co
Diamagnetism
↓
Paired electron
↓
No Net magnetic effect
(Repel by magnetic field)
Zn
Spin cancel Net spin
Sc
pyrolytic graphite
Spin cancel Spin cancel
Paramagnetism
↓
Unpaired electron
↓
Net magnetic effect
(Attract by magnetic field)
DiamagneticParamagnetic
Click here levitation bismuth Click here levitation
Click here paramagnetism measurement
Vs
Bismuth
Click here paramagnetism
Strong diamagnetic materials

15. Pt/Pd surface
Transition Metal – Catalytic Activity
Catalytic Properties of Transition metal
• Variableoxidationstate - lose and gain electroneasily.
• Use 3d and 4s electronsto form weak bond.
• Act as Homogeneousor Heterogenouscatalyst – lower activationenergy
• Homogeneouscatalyst – catalyst and reactant in same phase/state
• Heterogeneouscatalyst – catalyst and reactantin diff phase/state
• Heterogenouscatalyst- Metal surface provideactive site (lowerEa )
• Surfacecatalyst bringmoleculetogether(closecontact) -bond breaking/makingeasier
Transition metal as catalyst with diff oxidationstates
2H2O2 + Fe2+ → 2H2O+O2+Fe3+
H2O2+Fe2+→H2O+ O2 + Fe3+
Fe3+ + I- → Fe2+ + I2
Fe2+ ↔ Fe3+
Rxn slow if only I- is added H2O2 + I- → I2 + H2O + O2
Rxn speed up if Fe2+/Fe3+ added
Fe2+ change to Fe3+ and is changeback to Fe2+ again
recycle
molecule adsorp on
surface catalyst
Pt/Pd surface
Bond break
Bond making
3+
CH2 = CH2 + H2 → CH3 - CH3
Nickel catalyst
Without
catalyst, Ea
CH2= CH2 + H2 CH3 - CH3
Surface of catalyst for adsorption
With catalyst, Ea
adsorption
H2
adsorption
C2H4
bond breaking
making
desorption
C2H6
Fe2+ catalyst
How catalyst work ?
Activation energy

16. • Haber Process – Production ammonia for fertiliser/ agriculture
3H2 + N2 → 2NH3
Uses of transition metal as catalyst in industrial process
Iron , Fe
Vanadium (V) oxide, V2O5
Nickel, Ni
Manganese(IV) oxide, MnO2
Platinum/Palladium,Pt/PdCobalt, Co3+
Iron , Fe2+ ion
Contact Process – Sulphuric acid/batteries
2SO2 + O2 → 2SO3
Hydrogenation Process- Margerine and trans fat
C2H4 + H2 → C2H6
Hydrogen peroxide decomposition – O2 production
2H2O2→ 2H2O + O2
Catalytic converter – Convertion to CO2 and N2
2CO + 2NO → 2CO2 + N2
Biological enzyme
Hemoglobin – transport oxygen
Vitamin B12 – RBC production
NH3
Co3+
O2Fe2+