Select the appropriate options to identify which compound in the following pair has the lower freezing point and identify the strongest intermolecular forces for that compound: Au (gold) or P (phosphorous) 1. Au (gold) 2. P (phosphorous) The strongest 3. ion-dipole forces intermolecular forces of the compound with the lower freezing point are 4. hydrogen-bonding forces 5. dipole-dipole forces has the lower freezing point. 6. ion-induced dipole forces 7. dipole-induced dipole forces 8. dispersion forces

Select the appropriate options to identify which compound in the following pair has the lower freezing point and identify the strongest intermolecular forces for that compound: Au (gold) or P (phosphorous) 1. Au (gold) 2. P (phosphorous) The strongest 3. ion-dipole forces intermolecular forces of the compound with the lower freezing point are 4. hydrogen-bonding forces 5. dipole-dipole forces has the lower freezing point. 6. ion-induced dipole forces 7. dipole-induced dipole forces 8. dispersion forces

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

What intermolecular force is responsible for the fact that ice is less dense than liquid water? hydrogen bonding ionic bonding ion-dipole forces dipole-dipole forces London dispersion forces
Select the appropriate options to identify which compound in the following pair has the lower freezing point and identify the strongest intermolecular forces for that compound: CH3CH₂CH₂OH (n-propanol) or CH3CH₂CH3 (propane) has the lower freezing point. The strongest intermolecular forces of the compound with the lower freezing point are 1. CH3CH₂CH₂OH (n-propanol) 2. CH3CH₂CH3 (propane) 3. ion-dipole forces 4. hydrogen-bonding forces 5. dipole-dipole forces 6. ion-induced dipole forces 7. dipole-induced dipole forces 8. dispersion forces
List the substances BaCl₂, H₂, CO, HF, and Ne in order of increasing normal boiling point. Solution (a) BaCl₂-IONIC substance: strongest intermolecular force. High normal b.p. H₂ - Has ONLY LDF intermolecular forces. Its MM = 2.016 g/mol. CO - Has BOTH LDF and dipole-dipole interactions, thus dipolar forces are more predominant. HF - Has BOTH LDF and H-Bonding. Will have quite a high normal b.p. Ne - Has ONLY LDF available. Its AM = 20.180 g/mol. Thus: BaCl₂ has the highest comparative b.p. since it is ionic. When a substance has LDF only, then it is necessary to compare other factors, principally MM, AM, and/or shape. For these small molecules, mass will suffice. Lowest normal b.p. Highest normal b.p. H₂ < Ne HF < BaCl, IDF only (MM decides) < dipole-dipole < H-bond
Question 42 Why does the vapor pressure of water decrease when we add NaCl to it? A The ion-dipole attractions of the water to the NaCl, since stronger than water'd H-bonding, make water less willing to evaporate. B Only the liquid at the surface evaporates, so when we add the NaCl, some of it will take up some of the surface spots decreasing the amount of water molecules who have the opportunity to evaporate. D) None of these are correct. Since the water is now trying to separate the sodium ions Hom the chloride ions, the water molecules are too busy to evaporate. C The vapor pressure actually increases because water wants to get away from the NaCl and try to be pure again. E 1
Which letter(s) represents a TRUE hydrogen bond between two water molecules? H H H H A H H B H All of these letters represent true hydrogen bonds. O Hydrogen bond C Hydrogen bond B Hydrogen bond A
What is the strongest intermolecular force influencing the boiling point of the following molecule? O van der Waals attractions (aka London dispersion forces) Dipole-Dipole interactions O Hydrogen bonding O lonic interaction zeppnptomima OH
Indicate the type of solid in each example lattice points type of crystal sodium phosphate ammonia, NH3 helium iron diamond While sodium phosphate is a solid, glass is an solic a. jons b. molecules C. atoms d. ionic e. molecular f. atomic g. amorphous h. crystalline
Which statement accurately depicts what happens to water on the molecular level in a tea pot when it begins to boil? The molecules begin to move farther apart increasing their intramolecular forces and they escape the liquid state to enter the solid state The molecules begin to move farther apart decreasing their intermolecular forces and they escape the liquid state to enter the gas state The molecules begin to move closer together overcoming their intermolecular forces which holds them together and they escape the liquid state to enter the gas state
Part A Two liquids, A and B, have vapor pressures at a given temperature of 24 mmHg and 36 mmHg, respectively. We prepare solutions of A and B at a given temperature and measure the total pressures above the solutions. We obtain the following data: Solution Amt A (mol) Amt B (mol) P (mmHg) 1 1 1 30 1 28 3 1 32 4 1 33 Predict the total pressure above a solution of 4 mol A and 2 molB. Express your answer to two significant figures and include the appropriate units. HÀ ? Ptotal Value Units
Which intermolecular force of attraction caused the deviation in the following graph? 120 100 80 60 40 20 -20 -40 -60 -80 H,0 H,S H,Se H,Te A) ion-dipole forces B dipole-dipole hydrogen bond D dispersion forces Boiling Point (°C)
Which of the following molecules has the higher AHvap (the amount of energy needed to change the substance from a liquid to a gas) and why? A They both have the same Hvap, because they have the same type of intermolecular force. AHvap is temperature dependent, so it depends on the temperature. A, because it has stronger intermolecular forces, requiring more energy to overcome the intermolecular forces. B, because it has stronger intermolecular forces, requiring more energy to overcome the intermolecular forces. Not enough information is given.