CHEM 1030 Lecture Notes - Lecture 13: Electric Potential Energy, Ionic Compound, Lattice Energy

• School: Auburn University
• Department: Chemistry
• Course: CHEM 1030
• Professor: Allie Brandriet

Document Summary

Chem 1030 lecture 13 chapter 4. Ionic compounds: coulombic attraction: a way to mathematically relate the attraction. Equation for this mathematical attraction: eel= the electrostatic potential energy; q1 and q2= charge one and charge two respectively; d= distance. Eel= opposite which is a good indicate of the bond being stable. +eel= like charges are more likely to repel: the potential energy well is the most appropriate distance that creates the bond, where it is the most stable. If you continue to push the ions together past this point, the repulsion of the ions begins: example: k+ and cl- 2. 31 x 10-19 j nm (q1 x q2/d) = -7. 24 x 10-19 j/ion pair. Must get rid of the (cid:862)io(cid:374) pair(cid:863) (cid:271)(cid:455) stoi(cid:272)hio(cid:373)etr(cid:455): (-7. 24 x 10-19 j/ion pair) x (6. 0221 x 1023 ion pairs/ 1mol ion pairs) x (1 kj/1000 j) K+ (g) + cl- (g) kcl (s) Hbr (aq) ionizable = hydrobromic: polyatomic ions: both covalent and ionic bonds, example: so4.