First Ionization Energies of Transition Metals The first
- Slides: 33
First Ionization Energies of Transition Metals • The first ionization energy increases gradually from left to right on the periodic table. 5 d 3 d 4 d
Oxidation States of 3 d Transition Metals Element group Sc 3 Ti 4 V 5 Cr 6 Oxidation state Key Mn 7 Fe 8 Co 9 Ni 10 Cu 11 Zn 12 Valance configuration +1 d 4 d 5 d 6 d 7 d 8 d 9 d 10 +2 d 1 d 2 d 3 d 4 d 5 d 6 d 7 d 8 d 9 d 10 +3 d 0 d 1 d 2 d 3 d 4 d 5 d 6 d 7 d 8 +4 d 0 d 1 d 2 d 3 d 4 d 5 d 6 +5 d 0 d 1 d 2 d 3 d 4 +6 d 0 d 1 d 2 +7 d 0 +2 +3 +4 d 0 *Table lists the configuration of the ion corresponding to each observed oxidation state. The most important oxidation states of each element are color screened.
Formation of Coordinate Covalent Bonds • A ligand donates a lone pair of electrons to form a bond to a metal. – Ex. The Ni–N bonds in [Ni(NH 3)6]2+ form by overlap of the lone pair sp 3 orbital on the nitrogen atom with an empty valence orbital on the metal. Donor Metal
2+ Two Ni -Ligand Complexes • Both water and ammonia form six covalent bonds with Ni 2+, resulting in octahedral geometry.
Colors of Two Ni 2+-Ligand Complexes [Ni(H 2 O)6]2+ [Ni(NH 3)6]2+
Coordination Number - Two • Complexes with coordination number two always adopt linear geometry about the metal cation.
Coordination Number – Four Tetrahedral and Square planar
Coordination Number – Six Octahedral
Bidentate Ligands
Heme • Oxygen-carrying component of blood. • Planar structure. • Multi-ring structure of C and N atoms. • Extensive delocalized π system. • Binds one Fe 2+ cation at its center. Iron
Repulsion of Ligand Electrons and Metal Electrons is Greatest with Overlap • dx 2–y 2 points directly toward the ligands. – Overlap results in increased repulsion. • dxy points between the ligands. – Lack of overlap results in less repulsion. y y x x dxy orbital dx 2–y 2 orbital
The Five d Orbitals Interacting with an Octahedral Set of Ligands
The Crystal Field Level Diagram for Octahedral Coordination Complexes • Electron-cation attraction stabilized all five d orbitals. • Electron-electron repulsion destabilizes the five d orbitals by different amounts.
Crystal Field Splitting Energy • Crystal field splitting energy: – The difference in energy between the eg and t 2 g sets. – Symbolized by the Greek letter, Δ. dz 2 dx 2–y 2 Δ dxy eg dxz dyz t 2 g
The Spectrochemical Series • The spectrochemical series lists the common ligands in order of increasing ability to split the energies of the t 2 g and eg subsets of orbitals. • The ranking of ligands is influenced most strongly by the donor atom: – Generally decreases across Row 2 of the periodic table. – Generally decreases down the halogen column. – Molecular orbital theory is best used to explain the trend.
Relationships Among Wavelength, Color, and Crystal Field Splitting Energy (Δ) Wavelength (nm) Color absorbed Complementary color Δ (k. J/mol) >720 Infrared Colorless <165 720 Red Green 166 680 Red-orange Blue-green 176 610 Orange Blue 196 580 Yellow Indigo 206 560 Yellow-green Violet 214 530 Green Purple 226 500 Blue-green Red 239 480 Blue Orange 249 430 Indigo Yellow 279 410 Violet Lemon-yellow 292 <400 Ultraviolet Colorless >299
Colors of Cr 3+ Coordination Complexes • The colors of Cr 3+ coordination complexes depend on the magnitude of the crystal field splitting energy. – Higher Δ, shorter λ. • The spectrochemical series indicates the relative magnitude of Δ.
- Ionization energy transition metals
- Electronegativity trend exceptions
- 6 the periodic table
- Largest atomic radius
- Knockhardy publishing
- Non metals in the periodic table
- Ferrous vs non ferrous
- Metals vs nonmetals vs metalloids
- Natural science grade 7 term 2 notes
- Grade 7 term 2 natural science
- Is sodium a metal or nonmetal
- What are the group 15 elements
- Group with 6 valence electrons
- Transition metals valence electrons
- Elements and their properties
- Electron configuration of transition metal ions
- A linear complex ion with ligands on the x-axis
- Inner transition metals definition
- List of multivalent metals
- Ionic compounds containing transition metals
- Transition metals display great similarities
- Whats atomic radius
- First ionization energy definition ib
- Ib chemistry atomic structure
- Order of increasing first ionization energy
- Ionization energy practice
- Definition of first ionisation energy
- Physics what is energy
- Is bond breaking endothermic
- Ganggalion
- Successive ionisation energies of calcium
- Bonding force and energy
- European renewable energies federation
- Why are average bond enthalpies inexact values