CHEM 111 Chapter Notes - Chapter 2: Trigonal Planar Molecular Geometry, Trigonal Pyramidal Molecular Geometry, Intermolecular Force

• School: Texas A&M University
• Department: Chemistry
• Course: CHEM 111
• Professor: Daniel P Collins

Document Summary

Drawing lewis structures - steps: count the number of valence electrons. Can also be used to determine geometry/shape. Count each bond (single, double, and triple) and each lone pair as one group of electrons. 3 groups = sp2 = trigonal planar. Remember that any atom with lone pairs adjacent to a sp2 will also be sp2. Total number of electron groups determine bond angles. These all have the same bond angles, but different molecular geometries/shapes. Chemical bonds are formed when electrons are shared between two atoms as their orbitals overlap. The strength of a chemical bond is dependent upon . Shorter distance between atoms = stronger bond. Stronger bonds = higher bond dissociation energies. Breaking a bond is always an endothermic process. Determined by the difference in electronegativity of the atoms. Covalent bonds are formed between atoms with high electronegativity (nonmetals with nonmetals) The electrons in the bond are donated from both atoms.