CHM136H1 Study Guide - Midterm Guide: Valence Bond Theory, Electron Shell, Unpaired Electron

• School: UTSG
• Department: Chemistry
• Course: CHM136H1
• Professor: Andrew( Andy) Dicks

Document Summary

Chapter 1: structure and bonding. Chemistry notes perpendicular directions, px,py, and pz. Describing chemical bonds: two models have been developed to describe covalent bonding, valence bond theory and molecular orbital theory. H2, 436 kj/mol is rleased. Chemistry notes reactant and we say that the h h bond has a bond strength of 436 kj/mol. There is a bond length (optimum distance b/w nuclei that leads to maximum stability) 2p orbitals: three sp2 hybrid orbitals result, and one. Has a planar structure with h c h and h c c bond angles of approx. 120 sp hybrid orbitals and the structure of acetylene. Hybridization of nitrogen, oxygen, phosphorus, and sulphur. Chapter 2: polar covalent bonds; acids and bases. En: o, n, and halogens on the right side of the periodic table attract e- strongly and have higher. Formal charges: formal charges are a formalism and don"t imply the presence of actual ionic charges in a molecule.