CHEM 112 Lecture Notes - Lecture 5: Unpaired Electron, Electron Configuration, Lone Pair

• School: Queen's University
• Department: Chemistry
• Course: CHEM 112
• Professor: John Carran

Document Summary

We can write their formulas and determine compositions. We can write, balance and use chemical equations to make stoichiometric and thermochemical calculations. This can be done without considering atomic structure, molecular shapes or other properties of the chemicals being studied. What forces hold: the ions together in the ionic crystal, naci ionic bond the molecules of h2o together in ice hydrogen bond the atoms together within molecules of common gases such as h2 and cl2 - covalent. Interactions that hold ions are referred to as chemical bonds. Lewis electron dot symbols gilbert lewis noted that: Noble gases were inert because of unique electron configuration (filled octet) Atoms combine (bond) to achieve stable electron configurations. Maximum stability results when an atom is isoelectronic (has the same number of electrons) with noble gas. Electrons of prime importance are those found in the valence shell (outer energy level) since these are the electrons which interact when chemical bonds are formed.