CHEM101 Lecture Notes - Lecture 14: Covalent Bond, Valence Electron, Chemical Formula

• School: University of Alberta
• Department: Chemistry
• Course: CHEM101
• Professor: Yoram Apelblat

Document Summary

A balance between attraction and repulsion: atoms are far apart a(cid:374)d do(cid:374)"t i(cid:374)flue(cid:374)(cid:272)e each other, nuclei attract ea(cid:272)h other"s e ; repulsions increase as well, minimum energy (balance between attraction and repulsion, repulsions dominate, and energy rises rapidly. Distribution of electron density in h2: electron density is enhanced between the nuclei atoms bond through the sharing of electrons. In order to achieve a full valence level (an octet), atoms in covalent bonds count shared electron pairs (bonding pairs) as belonging entirely to themselves. Figure 9. 13: valence electrons not involved in bonding are called lone pairs. The shared pair is represented as a pair of dots or a line: Properties of covalent bonds: bond order, bond length, bond energy, bond polarity. The number of e pairs being shared by a pair of atoms: single bond one bonding pair (e. g. f2): bond order = 1, double bond two bonding pairs (e. g. o2, triple bond three bonding pairs (e. g. n2)