The document discusses the periodic table and properties of elements. It is divided into blocks based on orbital filling: s, p, d, and f blocks. Transition metals are in the d block and have partially filled d orbitals. They exhibit variable oxidation states, can form colored complexes, and show catalytic activity due to this electronic configuration. Magnetic properties depend on paired or unpaired electrons in the outer shell.

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+