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A comprehensive overview of transition metals, covering their electronic structure, coordination compounds, and key properties. It delves into the crystal field theory, explaining how d-orbital energies split in the electrostatic field of ligands. The document also explores the spectrochemical series, which helps predict the color and magnetic properties of complexes. Additionally, it examines the trends in physical and chemical properties of transition metals, including atomic radii and redox potentials. Enriched with examples and diagrams to illustrate concepts and enhance understanding.
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Trends in Physical Properties Trends in Chemical Properties The Electronic Structure Crystal Field Theory The Spectrochemical Series The Colors of Complexes The Magnetic Properties of Complexes Ligand Field Theory Coordination Compounds Coordination Complexes The Shapes of Complexes Isomers
General Properties of Transition Metals:
Radial distribution functions Core electrons (1s^2 2s^2 2p^6 )
๐๐ ๐
Radial probability of 3d vs. 4s orbitals Nucleus The energy of an empty atomic 3 d orbital is higher than that of an empty 4s orbital
2
2
10
2 # Valence electrons/ max. oxidation state 3/ 3 4/^4
4 s , 3 d
known oxidation states common oxidation states Group 3 4 5 6 7 8 9 10 11 12 Reduction/ Oxidation common = most stable **VO 2
O**^ V
- (3+) - : (^) O : : : : : 4 s , 3 d 5 s , 4 d 6 s , 5 d
General Rule: Ionization takes away electrons from the outermost atomic orbitals. Ti (4 s 2 3 d 2 ) โ Ti 2+ ( 3 d 2 ) ( different from Ca (4s 2 ) ) Hundโs Rule: Electron configurations maximizing the spin are preferred by energy. Fe (4 s 2 3 d 6 ) โ Fe 3+ ( 3 d 5 ) The energy of an occupied atomic 3 d orbital is lower than that of an occupied 4s orbital Element 4 s 3 d 4 p Unpaired Electrons Ti โโ^ โ^ โ^2 Element 4 s 3 d 4 p Unpaired Electrons Fe โโ^ โโ^ โ^ โ^ โ^ โ^5
Some important aspects of transition metal ions:
Standard Reduction Potentials
n+
-
The more negative E o , the stronger tendency of M to give electrons in redox reactions (M gets stronger as a reducing agent).
Fe 2+
โ Cu E o = 0.34 V
2+
2+
The more positive E o, the stronger tendency of Mn+^ to receive electrons in redox reactions (Mn+^ gets stronger as an oxidizing agent)
Reduction Potentials and Transition Metal Reactivity Metals with E **o < 0 are oxidized by H 3 O
upon reacting with acids** Zn ( s ) + 2H 3 O
( aq ) โ Zn 2+ ( aq ) + H 2 ( g ) + 2H 2 O ( l ) Cu 2+
- โ Cu E o = 0.34 V Cu ( s ) + 2H 3 O
( aq ) โ no reaction Zn 2+
Representation of the 3 d orbitals
d - Orbital lobes affect the properties in two ways: Trends in Physical Properties 1 .) Electrons in the lobes are far apart and weakly repealing each other. 2 .) d - Orbitals are poor at shielding because their electron density is low near the nucleus.
Radial probability of 3d vs. 4s orbitals Nucleus
