💏Intro to Chemistry Unit 19 – Transition Metals & Coordination Compounds

Key Concepts

• Transition metals are elements in the d-block of the periodic table that have partially filled d orbitals in their neutral or ionic states
• Coordination compounds consist of a central metal atom or ion bonded to surrounding molecules or ions called ligands
• Ligands donate electron pairs to the central metal atom to form coordinate covalent bonds
• Crystal field theory explains the bonding, structure, and properties of coordination compounds based on the splitting of d orbitals
• The splitting of d orbitals in coordination compounds leads to the absorption of specific wavelengths of light, resulting in the characteristic colors of transition metal complexes
• Transition metals and their coordination compounds have important applications in various fields (catalysis, pigments, and biological systems)

Transition Metal Properties

• Transition metals exhibit a wide range of oxidation states due to their ability to lose electrons from both the s and d subshells
• They form stable coordination compounds with ligands, resulting in complex geometries (octahedral, tetrahedral, and square planar)
• Transition metals often display paramagnetism, meaning they are attracted to magnetic fields due to the presence of unpaired electrons
• Many transition metals and their compounds are colored due to d-d electronic transitions
  • The specific color depends on the energy gap between the split d orbitals
• Transition metals have high melting and boiling points compared to main group elements due to their strong metallic bonding
• They exhibit good electrical and thermal conductivity, making them useful in various industrial applications (wiring and heat exchangers)
• Transition metals are generally hard and dense, with high tensile strength and ductility

Electron Configuration

• The electron configuration of transition metals involves the filling of the d subshell after the s subshell of the valence shell
• The general electron configuration for transition metals is $[Noble Gas] (n-1)d^x ns^2$, where n is the principal quantum number and x is the number of electrons in the d subshell
  • For example, the electron configuration of iron (Fe) is $[Ar] 3d^6 4s^2$
• Exceptions to the general electron configuration occur when the d subshell is half-filled or completely filled, as these configurations are more stable
  • For example, chromium (Cr) has the electron configuration $[Ar] 3d^5 4s^1$ instead of $[Ar] 3d^4 4s^2$
• The partially filled d subshell contributes to the unique properties of transition metals, such as variable oxidation states and the formation of coordination compounds

Coordination Compounds

• Coordination compounds are composed of a central metal atom or ion surrounded by ligands
• The central metal atom or ion is typically a transition metal, but can also be a main group element or a lanthanide/actinide
• Ligands are molecules or ions that donate electron pairs to the central metal atom, forming coordinate covalent bonds
• The number of ligands bonded to the central metal atom is called the coordination number, which typically ranges from 2 to 9
  • Common coordination numbers include 4 (tetrahedral and square planar) and 6 (octahedral)
• The geometry of a coordination compound depends on the coordination number and the nature of the ligands
• Coordination compounds can be neutral or charged, depending on the charges of the central metal ion and the ligands
  • For example, $[Co(NH_3)_6]Cl_3$ is a cationic complex with a +3 charge on the cobalt ion and three chloride counterions

Ligands and Bonding

• Ligands are classified as monodentate (one donor atom), bidentate (two donor atoms), or polydentate (multiple donor atoms) based on the number of atoms that bond to the central metal
• Common monodentate ligands include water ($H_2O$), ammonia ($NH_3$), and halides ($Cl^-$, $Br^-$, $I^-$)
• Bidentate ligands, such as ethylenediamine ($H_2NCH_2CH_2NH_2$) and acetylacetonate ($CH_3COCHCOCH_3^-$), form chelate rings with the central metal atom
  • Chelate rings enhance the stability of coordination compounds due to the chelate effect
• Polydentate ligands, like EDTA (ethylenediaminetetraacetic acid), can form multiple chelate rings and lead to very stable complexes
• The bonding in coordination compounds involves a combination of electrostatic interactions and covalent bonding between the ligands and the central metal atom
  • The coordinate covalent bond is formed by the donation of an electron pair from the ligand to the metal, creating a shared electron pair

Crystal Field Theory

• Crystal field theory (CFT) describes the bonding, structure, and properties of coordination compounds based on the splitting of d orbitals
• In a coordination compound, the ligands create an electrostatic field that interacts with the d orbitals of the central metal atom
• The d orbitals split into two energy levels: the lower energy $t_{2g}$ orbitals ($d_{xy}$, $d_{xz}$, $d_{yz}$) and the higher energy $e_g$ orbitals ($d_{z^2}$, $d_{x^2-y^2}$)
  • The energy difference between the $t_{2g}$ and $e_g$ orbitals is denoted as $\Delta_o$ (octahedral crystal field splitting energy)
• The magnitude of the crystal field splitting depends on the nature of the ligands and the central metal atom
  • Strong-field ligands (CN-, CO) cause a larger splitting, while weak-field ligands (I-, Br-) result in a smaller splitting
• The electron configuration of the central metal atom in a coordination compound is determined by the relative energies of the $t_{2g}$ and $e_g$ orbitals and the pairing energy
  • High-spin complexes have a smaller $\Delta_o$ and electrons occupy both $t_{2g}$ and $e_g$ orbitals before pairing
  • Low-spin complexes have a larger $\Delta_o$ and electrons pair in the $t_{2g}$ orbitals before occupying the $e_g$ orbitals

Colors and Magnetism

• The colors of transition metal coordination compounds arise from d-d electronic transitions between the split d orbitals
• When light is absorbed, an electron is promoted from a lower energy d orbital to a higher energy d orbital
  • The wavelength of light absorbed corresponds to the energy difference between the two orbitals
• The complementary color to the absorbed wavelength is observed as the color of the complex
  • For example, a complex that absorbs orange light will appear blue
• The intensity of the color depends on the probability of the electronic transition, which is governed by selection rules
• The magnetic properties of coordination compounds are determined by the number of unpaired electrons in the d orbitals
  • High-spin complexes have more unpaired electrons and are paramagnetic, while low-spin complexes have fewer unpaired electrons and may be diamagnetic
• The magnetic moment of a coordination compound can be measured experimentally and compared to the predicted values based on the spin-only formula
  • $\mu = \sqrt{n(n+2)}$ $\mu_B$, where n is the number of unpaired electrons and $\mu_B$ is the Bohr magneton

Applications and Real-World Examples

• Transition metal coordination compounds have numerous applications in various fields, including catalysis, pigments, and biological systems
• In catalysis, coordination compounds are used as homogeneous and heterogeneous catalysts for industrial processes (Wilkinson's catalyst for hydrogenation)
• Pigments based on transition metal coordination compounds are used in paints, inks, and plastics (cobalt blue, chromium oxide green)
• Biological systems employ coordination compounds for essential functions, such as oxygen transport (hemoglobin) and photosynthesis (chlorophyll)
• Transition metal complexes are used in medicine for diagnostic imaging (contrast agents) and therapy (cisplatin for cancer treatment)
• Coordination compounds are also used in analytical chemistry for the detection and quantification of metal ions (complexometric titrations with EDTA)
• Transition metal complexes are employed in the fabrication of advanced materials, such as light-emitting diodes (LEDs) and solar cells (ruthenium-based dye-sensitized solar cells)
• The study of transition metal coordination compounds has led to the development of new technologies and materials, such as superconductors and molecular magnets