d – Block transition elements (group 3–12)
Uses Compound
• Electronic configuration : (n –1)d1–10 ns1–2
• In production of iron and steels.
Cr=4s13d5 Non-typical transition elements • TiO in pigment industry
Exceptions • MnO2 in dry battery cells.
Cu=4s13d10,Pd=5s04d10 Zn,Cd & Hg
• As catalysts in industry.
• Physical properties: • Ni complexes:polymerization of
alkynes and other organic compounds
Potassium dichromate K2Cr2O7
-High melting and boiling point
Melting point : s-block metals < d-block metals • AgBr in photographic industry.
Preparation :
Sc < Ti < V < Cr > Mn < Fe > Co > Ni > Cu > Zn (3d Series)
4FeCr2O4 + 8Na2CO3 + 7O2→8Na2CrO4 + 2Fe2O3 +8CO2
Zn > Cd > Hg 2Na2CrO4 + 2H+→ Na2Cr2O7 + 2Na+ + H2O
Melting point
Cu > Ag ≤ Au Na2Cr2O7 + 2KCl → K2Cr2O7 + 2NaCl
-High enthalpies of atomization(Highest for V in 3d, series)
Catalysts Properties : Strong oxidising agent
Cr2O72- + 14H+ + 6e–→2Cr3+ + 7H2O
Atomic Radius: Contact process = V2O5
3d series: Sc > Ti > V > Cr > Mn ≥ Fe Co Ni≤ Cu < Zn
Haber process = Fe 2O3+ Al2O3 + K2O
Decomposition of KClO 3 = MnO2 Cr2O72– (Orange)
In a group 3d 4d 5d (Lanthanide contraction)
2–
Ostwald process = Pt/Rh SO2 SO4
Smallest radius – Ni
eg : Ti Zr Hf Zeigler Natta catalyst = TiCl4+(C2H5)3Al H2S S
Largest radius – La O
2– 2–
O
pm
SO3 SO4
Hydrogenation of Alkene = Ni/Pd
9
126°
17
- –
Density: NO2 NO3 O Cr Cr
Wilkinson‛s catalyst=RhCl(PPh3)3 I– I2
16
3p
s-Block < d-Block
O m
Br– Br2
3d series: Sc < Ti < V < Cr < Mn < Fe <Co ≤ Ni< Cu > Zn S2O3
2–
SO42–
In a group C 2H5OH CH3COOH
• Ionisation enthalpy:increases from left to right Sn2+ Sn4+
• Oxidation states : Variable; higher O.S. stable down the group Ln2S3 Fe
2+
Fe
3+
• Trends in E°M2+/M : E° for Mn, Ni and Zn are more negative
Ln2O3
than expected.
+3
• Trends in E°M3+/M: variable Cr (green)
• Chemical reactivity and E° values : Variable Ti2+ , V2+ and Cr2+ are strong
ted
Hea S
s
Burn
reducing agents
+
2– H 2–
CrO4 Cr2O7
2
h
in O
t
–
• Magnetic properties : Diamagnetism and paramagnetism. µ = n(n + 2) BM OH
i
H2 (Orange)
w
(Yellow)
• Formation of coloured ions : due to d – d transitions LnN
• Form a large number of complex compounds
• Forms interstitial compounds : Non - stoichiometric and are neither He ith
ionic nor covalent. wit ated W ids
• Alloy formation : Due to similar atomic sizes.(15% difference in metallic radius) hN ac
Actinoids
Ln • Electronic configuration : [Rn]5f1–14 6d0–1
• Ionic sizes : Gradual decrease along the
Lanthanoids Wit
h Lnx3 • Oxidation states : Most common is +3 .
halo
gens O.S. of +4, +5, +6 and +7.
• Electronic configuration: 4f1–14 5d0–1 6s2 (Gd:4f7 5d1 6s2) C
th • General characteristics :
• Atomic and ionic sizes: Decreases from La to Lu(Eu is the largest)
LnC2 Wi 3 K
7 –Highly reactive metals
• Oxidation states: Most common is +3. 27
–Irregularities in metallic radii,greater tha
Wi
H2
t
Uses Compound
• Electronic configuration : (n –1)d1–10 ns1–2
• In production of iron and steels.
Cr=4s13d5 Non-typical transition elements • TiO in pigment industry
Exceptions • MnO2 in dry battery cells.
Cu=4s13d10,Pd=5s04d10 Zn,Cd & Hg
• As catalysts in industry.
• Physical properties: • Ni complexes:polymerization of
alkynes and other organic compounds
Potassium dichromate K2Cr2O7
-High melting and boiling point
Melting point : s-block metals < d-block metals • AgBr in photographic industry.
Preparation :
Sc < Ti < V < Cr > Mn < Fe > Co > Ni > Cu > Zn (3d Series)
4FeCr2O4 + 8Na2CO3 + 7O2→8Na2CrO4 + 2Fe2O3 +8CO2
Zn > Cd > Hg 2Na2CrO4 + 2H+→ Na2Cr2O7 + 2Na+ + H2O
Melting point
Cu > Ag ≤ Au Na2Cr2O7 + 2KCl → K2Cr2O7 + 2NaCl
-High enthalpies of atomization(Highest for V in 3d, series)
Catalysts Properties : Strong oxidising agent
Cr2O72- + 14H+ + 6e–→2Cr3+ + 7H2O
Atomic Radius: Contact process = V2O5
3d series: Sc > Ti > V > Cr > Mn ≥ Fe Co Ni≤ Cu < Zn
Haber process = Fe 2O3+ Al2O3 + K2O
Decomposition of KClO 3 = MnO2 Cr2O72– (Orange)
In a group 3d 4d 5d (Lanthanide contraction)
2–
Ostwald process = Pt/Rh SO2 SO4
Smallest radius – Ni
eg : Ti Zr Hf Zeigler Natta catalyst = TiCl4+(C2H5)3Al H2S S
Largest radius – La O
2– 2–
O
pm
SO3 SO4
Hydrogenation of Alkene = Ni/Pd
9
126°
17
- –
Density: NO2 NO3 O Cr Cr
Wilkinson‛s catalyst=RhCl(PPh3)3 I– I2
16
3p
s-Block < d-Block
O m
Br– Br2
3d series: Sc < Ti < V < Cr < Mn < Fe <Co ≤ Ni< Cu > Zn S2O3
2–
SO42–
In a group C 2H5OH CH3COOH
• Ionisation enthalpy:increases from left to right Sn2+ Sn4+
• Oxidation states : Variable; higher O.S. stable down the group Ln2S3 Fe
2+
Fe
3+
• Trends in E°M2+/M : E° for Mn, Ni and Zn are more negative
Ln2O3
than expected.
+3
• Trends in E°M3+/M: variable Cr (green)
• Chemical reactivity and E° values : Variable Ti2+ , V2+ and Cr2+ are strong
ted
Hea S
s
Burn
reducing agents
+
2– H 2–
CrO4 Cr2O7
2
h
in O
t
–
• Magnetic properties : Diamagnetism and paramagnetism. µ = n(n + 2) BM OH
i
H2 (Orange)
w
(Yellow)
• Formation of coloured ions : due to d – d transitions LnN
• Form a large number of complex compounds
• Forms interstitial compounds : Non - stoichiometric and are neither He ith
ionic nor covalent. wit ated W ids
• Alloy formation : Due to similar atomic sizes.(15% difference in metallic radius) hN ac
Actinoids
Ln • Electronic configuration : [Rn]5f1–14 6d0–1
• Ionic sizes : Gradual decrease along the
Lanthanoids Wit
h Lnx3 • Oxidation states : Most common is +3 .
halo
gens O.S. of +4, +5, +6 and +7.
• Electronic configuration: 4f1–14 5d0–1 6s2 (Gd:4f7 5d1 6s2) C
th • General characteristics :
• Atomic and ionic sizes: Decreases from La to Lu(Eu is the largest)
LnC2 Wi 3 K
7 –Highly reactive metals
• Oxidation states: Most common is +3. 27
–Irregularities in metallic radii,greater tha
Wi
H2
t
