Ch 101 1st Edition Lecture 16 Outline of Last Lecture I Ideal Gas Law A Boyle s Las B Charles Law C Avogadro s Law D Gay Lussac s Law II Molarity III Finding the Pressure of a Gas in a Manometer Outline of Current Lecture I Partial Pressure II Intramolecular Forces III Intermolecular Forces A Dispersion Forces B Dipole Dipole C Hydrogen Bonding IV Determining Polarity Current Lecture I Partial Pressure The partial pressure of a gas means the total pressure If you are given the pressure of different gasses and then asked what the partial pressure of the gasses are the equation would be Ppartial P1 P2 P3 etc II Intramolecular Forces Intramolecular forces are between different molecules These forces are covalent ionic and metallic These notes represent a detailed interpretation of the professor s lecture GradeBuddy is best used as a supplement to your own notes not as a substitute III Intermolecular Forces These are the forces within the molecule intermolecular forces are the forces that make up the bonds between the atoms There are four different types of intermolecular bonds dispersion or London dispersion dipole dipole hydrogen bonds and ionic where dispersion is the weakest force and ionic is the strongest A Dispersion Forces Every molecule has dispersion forces This type of bond is technically a dipole dipole bond only it is temporary because the polarity is constantly shifting around the atoms B Dipole Dipole A bond has dipole dipole forces when the bond is polar This type of bond is C Hydrogen Bonding IV Hydrogen bonding needs two things to occur a lone pair and a hydrogen bonded to a nitrogen fluorine or oxygen In order for there to be hydrogen bonds between molecules there must be a lone pair and a hydrogen that can attach to N O or F Determining Polarity A molecule is polar there is an unequal sharing of valence electrons or when it has dipoles that don t have another equivalent dipole to balance out the electrons Also if a molecule has lone pairs they will be polar Polar H2O Nonpolar CH4
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