Trigonal planar

Definition

Trigonal planar is a molecular geometry that describes a central atom bonded to three other atoms, with all bonds lying in a single plane and the bond angles measuring approximately 120 degrees. This arrangement results from the hybridization of orbitals, which leads to specific molecular shapes that minimize repulsion between electron pairs around the central atom.

5 Must Know Facts For Your Next Test

1. In trigonal planar geometry, the central atom typically has three bonding pairs and no lone pairs of electrons, such as in the case of BF3 or C2H4.
2. The ideal bond angle in a trigonal planar arrangement is 120 degrees, which minimizes electron pair repulsion according to VSEPR theory.
3. Hybridization involved in creating a trigonal planar shape typically involves the mixing of one s orbital and two p orbitals, forming three sp2 hybrid orbitals.
4. Molecules with trigonal planar geometry are flat and symmetrical, which can influence their reactivity and interaction with other molecules.
5. Trigonal planar structures are often found in molecules that have double bonds, as seen in alkenes, where one of the bonds results from a p orbital overlap.

Review Questions

• How does VSEPR theory explain the trigonal planar geometry of certain molecules?
  • VSEPR theory posits that electron pairs around a central atom will arrange themselves to minimize repulsion. In a trigonal planar configuration, the central atom is bonded to three atoms with no lone pairs present. This results in a flat structure where the three bond angles are approximately 120 degrees, effectively reducing electron pair repulsion and maintaining stability.
• Discuss the role of hybridization in achieving a trigonal planar molecular geometry and how it relates to covalent bonding.
  • Hybridization plays a crucial role in forming a trigonal planar geometry by allowing atomic orbitals to mix and create new hybrid orbitals. Specifically, one s orbital combines with two p orbitals to form three equivalent sp2 hybrid orbitals that lie in a single plane. These sp2 hybrid orbitals then overlap with the atomic orbitals of other atoms to create covalent bonds, resulting in the characteristic 120-degree angles of the trigonal planar shape.
• Evaluate how molecular structures like trigonal planar influence chemical reactivity and properties in organic compounds.
  • Molecular structures such as trigonal planar significantly impact chemical reactivity and properties due to their geometric arrangement and bond angles. The flat, symmetrical nature of trigonal planar molecules allows for efficient overlap of p orbitals during reactions, especially in alkenes with double bonds. This can lead to increased reactivity as these compounds participate in electrophilic addition reactions. Furthermore, the spatial arrangement affects intermolecular interactions, boiling points, and solubility, influencing how these compounds behave chemically.

Related terms

Hybridization: A concept in chemistry where atomic orbitals mix to form new hybrid orbitals, allowing for more effective bonding and specific molecular shapes.

VSEPR Theory: Valence Shell Electron Pair Repulsion theory explains the geometry of molecules based on the repulsion between electron pairs surrounding a central atom.

Covalent Bonding: A type of chemical bond where atoms share pairs of electrons to achieve stable electron configurations.