Ch 101 1st Edition Lecture 16Outline of Last LectureI. Ideal Gas LawA. Boyle’s LasB. Charles’ LawC. Avogadro’s LawD. Gay-Lussac’s LawII. MolarityIII. Finding the Pressure of a Gas in a Manometer.Outline of Current LectureI. Partial PressureII. Intramolecular ForcesIII. Intermolecular ForcesA. Dispersion ForcesB. Dipole DipoleC. Hydrogen Bonding IV. Determining Polarity Current LectureI. 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 equationwould 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 - 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.IV. 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: H2ONonpolar:
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