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Determine the intermolecular forces for each of the following molecules: Does the molecule contain polar bonds? yes or no total Compound valance electrons N₂ CHA CH₂OH H₂O IF CCIA NHS NF₁ Lewis Structure Molecular Geometry 0: Page 1 of 2 Is the molecule a polar molecule? yes or no Two Requirements: 1. polar bonds 2. lack of symmetry Dominant Intermolecular Force for Molecule
4. A compound's boiling point is the temperature when the kinetic energy of the molecules overcome the attractive force (intermolecular forces) between the molecules. So a higher boiling point corresponds to a stronger intermolecular forces. a. b. Which three molecules in exercise 3 are expected to have the highest boiling points? and what is the dominant intermolecular force for these three molecules? Which molecules in exercise 3 are expected to have the lowest boiling points? and what is the dominant intermolecular force for these three molecules? 5. A compound's vapor pressure is the pressure reached above the liquid in a closed container. At the same temperature, a compound with higher intermolecular forces will have a smaller vapor pressure because the molecules are more attracted to each other in the liquid, so they are less likely to escape the liquid into the gas phase to create a vapor pressure. a. Which three molecules in exercise 3 are expected to have the highest vapor pressures? and what is the dominant intermolecular force for these three molecules? b. Which molecules in exercise 3 are expected to have the lowest vapor pressures? and what is the dominant intermolecular force for these three molecules? b. Circle the molecules below (from exercise 3) which would be expected to be soluble in water: N₂, CH4, CH₂OH, IF, CCla, NHs, NF₁ 6. Polar molecules are stabilized more by each other than with nonpolar molecules, so polar molecules will group around each other and avoid nonpolar molecules. This is why oil and water do not mix. Polar molecules will also stabilize charged particles (ions) whereas nonpolar substances do not stabilize charged particles. This is why salts dissolve in polar solutions. a. Is water a polar or nonpolar compound? (circle correct answer) 7. When a substance boils, what state does it begin in? What state does it end in? 8. What is the difference between melting point and freezing point? For the same substance, do melting points and freezing points occur at different temperatures? vapor prestare 9. Which substance will have the highest boiling point, CBra or CFa? (circle correct answer) 10. Which substance will have the highest vapor pressure, CBr4 or CH₂OH? (circle correct answer) 11. Which would be more soluble in water (H₂O), Br₂ or CH₂OH? (circle correct answer) Liquid