CHMA10H3 Chapter Notes - Chapter 9: Linus Pauling, Infrared Spectroscopy, Electronegativity

• School: UTSC
• Department: Chemistry
• Course: CHMA10H3
• Professor: Nirusha Thavarajah

Document Summary

Chma10 - chapter 9: chemical bonding i lewis theory. They form because the potential energy between the charged particles decrease when forming atoms. The potential energy of this bond should be less than the potential energy of separate atoms. The following interactions can be used to calculate potential energy: Formed by gilbert n. lewis (1875 1946). The lewis theory uses valance electrons to explain chemical bonding. Lewis structure: is a structure of electrons of an atom by using the lewis theory. It is also known as electron dot structures. The lewis structure helps to predict the properties of molecules, such as shape, size, and molecular stability. Atoms bond with each other to gain a stable electron configuration. The more stable an atom, the less potential energy is used. When atoms transfer or share electrons, an outer shell with 8 electrons is usually obtained. Chemical bonding uses the transfer or sharing of electrons between atoms.