CH 104 Lecture Notes - Lecture 4: Dinitrogen Tetroxide, Electronegativity, Lewis Structure

• School: University of Alabama
• Department: Chemistry
• Course: CH 104
• Professor: Stephen Woski

Document Summary

Covalent bonding: bonding between two non-metals or a metal and a metalloid involves sharing pairs of electrons, by sharing pairs of electrons, both atoms have octets of valence electrons. Lewis structures: electron dot structures for molecules, they show the location of all valence electrons, bonding pairs of electrons become lines between bonded atoms. Bonding patterns: carbon has 4 unpaired electrons. Can form 4 bonds: oxygen has 2 unpaired electrons. Have 2 lone pairs: hydrogen only needs 1 pair. Drawing a lewis structure steps: arrange atoms with those bonded next to eachother, count valence electrons, place one bond between neighboring atoms, give every atom an octet of electrons using lone pairs. Name first nonmetal by its name and the second using the suffix ide: 2. Add prefixes to show number of atoms of each element. Common prefixes; goes by number of atoms. Electronegativity: the electronegativity increases in the periodic table as it goes up and to the right.