CHEM 1A Lecture Notes - Lecture 8: Octet Rule, Lewis Structure, Zirconium

• School: UC-Irvine
• Department: Chemistry
• Course: CHEM 1A
• Professor: Craig Martens

Document Summary

The ability of an atom to attract electrons to itself in a chemical bond. The higher the electronegativity, the greater the ability of an atom to attract electrons towards itself. In a chemical bond, the atom with the highest electronegativity carries the highest electron density in the bond. A bond is polar when the electron density in a covalent bond is unequally distributed. Bond polarity increases when the difference in electronegativity between the atoms is larger. Drawing lewis structures: add up the valence electrons of all the atoms, use a pair of electrons to form a bond between each pair of bound atoms. In general, take the least electronegative atom as the center atom of the skeletal structure: arrange remaining electrons to satisfy the duet rule for h and the octet rule for c, n, o, and f. The electrical charge difference between the valence electrons in an isolated atom and the number of electrons assigned to that atom.