key term - 18-electron rule

Definition

The 18-electron rule is a guideline used in organometallic chemistry that suggests stable transition metal complexes tend to have a total of 18 valence electrons. This rule is based on the idea that a full octet around the central metal, combined with contributions from its ligands, leads to enhanced stability in these compounds.

5 Must Know Facts For Your Next Test

1. The 18-electron rule accounts for the contributions from the metal's d-electrons, s-electrons, and the electrons donated by its ligands.
2. Complexes with fewer or more than 18 electrons often display unusual reactivity and may undergo specific reactions to achieve stability.
3. Exceptions to the 18-electron rule can occur with metals in low oxidation states or in cases where backbonding significantly influences stability.
4. Some main group elements can also follow the 18-electron rule, particularly when they form complexes similar to transition metals.
5. The rule is particularly useful for predicting the structures and reactivities of organometallic compounds in synthesis and catalysis.

Review Questions

• How does the 18-electron rule help predict the stability of transition metal complexes?
  • The 18-electron rule helps predict stability by indicating that complexes with a total of 18 valence electrons, including contributions from both the central metal and its ligands, tend to be more stable. When a complex achieves this electron count, it suggests that all available orbitals are fully utilized, resulting in strong bonding interactions. Conversely, complexes that deviate from this count may exhibit higher reactivity or instability due to incomplete electron configurations.
• What are some notable exceptions to the 18-electron rule and what factors contribute to these exceptions?
  • Notable exceptions to the 18-electron rule include certain low oxidation state complexes, like those of chromium or manganese, which may have fewer than 18 electrons yet remain stable. Factors contributing to these exceptions can include strong backbonding interactions with ligands, which can stabilize lower electron counts, and the unique properties of specific metals that allow them to maintain stable configurations even with fewer valence electrons.
• Evaluate how understanding the 18-electron rule can influence synthetic strategies in organometallic chemistry.
  • Understanding the 18-electron rule allows chemists to design organometallic compounds with desired properties by predicting their stability and reactivity. By targeting specific electron counts during synthesis, chemists can tailor complexes for particular catalytic activities or functional applications. Additionally, knowledge of exceptions helps chemists navigate scenarios where traditional predictions may not hold, enabling innovative approaches to creating new compounds and advancing catalytic processes.

Related terms

Coordination Number:

The number of ligand atoms that are bonded to the central metal atom in a complex.

Ligands:

Molecules or ions that donate electron pairs to the central metal atom, forming coordinate covalent bonds.

Backbonding: The process where electron density is transferred from filled metal d-orbitals to empty p-orbitals of ligands, stabilizing the metal-ligand bond.