CHEM 101 Lecture Notes - Lecture 8: Lattice Energy, Ionic Compound, Ionic Bonding
Document Summary
Lewis developed a method that showed the representation of an atom that shows valence electrons as dots around the symbol of the element. Example: carbon will have 4 dots around octet rule when forming compound atoms tend to gain lose or share electrons until they are surrounded by eight valence electrons ionic bonding. One element readily gives up an electron because it has a low ionization energy another element readily gains an electron because it has a high electron affinity. Start with the metal and nonmetal elements: n a(s) and c l2(g). Make gaseous atoms: n a(g) and c l(g). Energy required to completely remove one mole of a solid ionic compound into its gaseous ions. For example: the nrg required for this: nacl=na+(g) + cl-(g)= change in lattice= This is the same amount of energy released to make the ionic compound trends in lattice energy.
