2 For each pair, decide which substance has the stronger London forces and explain your answer:...
Applications 5.91 Would behave more like an ideal gas at Skor SOK? Explain your reasoning. 592 Would co behave more like an ideal gas at 2 atm or 20 atm? Explain your reasoning. The Liquid State Foundations 5.93 Compare the strength of intermolecular forces in liquids with those in gases. Compare the strength of intermolecular forces in liquids with those in solids. What is the relationship between the temperature of a liquid and the vapor pressure of that liquid? 5.96...
10. (10 pts.) Identify the intermolecular forces present in the following compounds: Compound Intermolecular forces H- N- H H₃C CH₂ ç CC-C1 a. Which compound would you expect to have the higher boiling point? b. Justify your selection. C. Which compound would you expect to have the highest vapor pressure? d. Justify your selection.
just do the circle number only Applications 5.91 Would behave more like an ideal gas at 5 Kor 50 K? Explain your reasoning 5.92 Would CO behave more like an ideal gas at 2 atm or 20 atm? Explain your reasoning. The Liquid State Foundations 5.93 Compare the strength of intermolecular forces in liquids with those in gases 5.94 Compare the strength of intermolecular forces in liquids with those in solids. What is the relationship between the temperature of a...
20)Which compound will have the highest surface tenssonr (Awater B) gasoline C) chloroform, CHCI cooking oil 21) Choosing from the intermolecular forces listed, which is the strongest? ATdispersion forces (London or Van der Wals) B) dipole-dipole forces hydrogen bonding PrX-forces rdelta forces ONF 22hWhich compound has the highest boiling point based on its intermolecular forces? AIOCH CHOH BTCH,CH CI HSH CH,CH,CH 23) In the following heating curve, what state is the water at point D? E) so0C (B Time )...
1.Which attractions are stronger: intermolecular or intramolecular? 2.How many times stronger is a covalent bond compared to a dipole-dipole attraction? 3.What evidence is there that nonpolar molecules attract each other? 4.Which chemical in table 10.1 has the weakest intermolecular forces? Which has the strongest? How can you tell? 5.Suggest some ways that the dipoles in London forces are different from the dipoles in dipole-dipole attractions. 6.A) Which would have a lower boiling point: O2or F2? Explain. B) Which would have a lower boiling...
Full Name Dis Sec. Day/Time Forces Which of the following series of compounds is listed in serms of insreasing intermolecular forces decreasing vapor pressure, increasing boiling point and freezing point NaCl CCl. Ar A) NaCI> CCl. HOA D) HO>NaCI> Ar > CCL 2 Circle the species having the smallest (Gowest) value of the property listed A) Viscous B) Intermolecular Forces C) Vapor Pressure CCL H,0 D) Freezing Point E) Solubility in WaterCH, Cl CH CH CH CH CH,OH 3. Which...
UP Determine what type of intermolecular forces are in the following molecules. a) N2 b) HCN c) CCL d) MgBr2 e) CH CI Dispersion forces only because nonpolar molecules) f) CH3CO2H 5. Which of the following substances would you expect to have a nonzero dipole moment? Explain, and show the direction of each. a) NF3 b) CH3NH2 c) XeF2 d) PCI e) XeFg f) BF;
help please Question 3 (1.5 points) Which of the following pure liquids would have dispersion forces (London forces) as its strongest intermolecular force? CH, CH, Hoc O CH Question 4 (1.5 points) Which of the following molecules has dipole-dipole interactions as it's strongest interaction? (no hydrogen bonding) You may select more than one answer. H₂ C CH 2 CH CH2 CH₂ CH2 CH₂ C H3C H2C CH3 H₂N
rank the molecules in the table from weakest to strongest intermolecular forces and briefly justify the ranking. temperature 310 20 time (s) 40 Fig. 10.1. Sample data for an evaporative cooling process. Before You Come to Lab Based on what you know about the relationship between the structure of a molecule and the strength of its intermolecular forces, rank the molecules in the table below in order from the weakest to the strongest intermolecular forces and briefly justify your ranking...
Which member of each pair has the greater polarizability (forming stronger dispersion forces)? Briefly explain your reasoning. a. CH 2 or butane b. Mg or Mg? c. XeCla or XeF