CHEM 1A03 Lecture Notes - Lecture 5: Group 3 Element, Formal Charge, Electronegativity

• School: McMaster University
• Department: Chemistry
• Course: CHEM 1A03
• Professor: David Emslie

Document Summary

Lewis structure: by using lewis dot symbols, we can keep track of where electrons come from as they are transferred. Covalent bonds: non-metal + non-metal, sharing of electrons, coordinate covalent bond: when one atom provides a pair of electrons to form a bond (2 electrons), ex. Nh3 + h+ nh4 : ammonia provides 2 electrons to share with hydrogen. Cl2: as the electronegativity increases, the bond becomes more polarized. Electrostatic potential maps: the different colours depict areas of charge density, red=negative charge, blue=positive charge. *not all elements have a valence shell that supports 8 electrons* Rules for drawing: count the total number of valence electrons on all atoms (atomic numbers). Exclude the electrons from the d & f blocks: include the charges by subtracting electrons for positive charges and adding them for negative charges, draw a skeletal structure with contains central and terminal atoms.