BIOL 112 Lecture Notes - Lecture 2: Sodium Chloride, Magnesium Chloride, Ionic Bonding

• School: McGill University
• Department: Biology
• Course: BIOL 112
• Professor: Frieder Schoeck

Document Summary

When two atoms form a bond, it is now a molecule. Hydrogen can only form one covalent bond, never more than one covalent bond. Carbon can form 4 covalent bonds because it has four electrons in the outer shell and each orbital has only one electron. Nitrogen has 5 electrons in the outermost shell, so it can form 3 covalent bonds. Oxygen has 6 electrons in the outermost shell, so it can form 2 covalent bonds. When a covalent bond is formed, there is a new kind of orbital. Example: the ch covalent bond had a new length, unique size, and angle, with respect to the other covalent bonds. A methane atom always looks like a tetrahedron. The oxygen2 in this example forms a double covalent bond. Ball-and-stick model is good to know something about the structure/shape about the molecule. Space filling model is rarely used, but gives the electron density.