CHEM 101 Lecture Notes - Lecture 7: Electrical Polarity, Chemical Polarity, Covalent Bond

• School: Drexel University
• Department: Chemistry
• Course: CHEM 101
• Professor: Monica Ilies

Document Summary

Vsepr theory helps predict geometry using the number of electron pairs. Goal is to maximize the distance between the electron groups. Note: a lone pair of electrons occupies more space than a bonding pair of electrons. Tendency of an atom to attract an electron. Least electronegative element= cs, fr (lower left corner) Ionic bond (the most polar because of transfer of electrons) Nonpolar covalent bond (equal sharing of electrons) Polar covalent bond (unequal sharing of electrons) Polar bonds have dipole moments (a measure of polarity) There are 3 types of dipole moments. Electric: electrical polarity of a system of charges. Molecular: electric dipole moment of a molecule. Cl is more electronegative and will have a stronger pull on the electrons (which results in polarity) Net dipole moment is in an upwards direction (towards the lone pair of electrons in a bent structure) To be a polar molecule it must have. Polarity affects the intermolecular forces of attraction.