True or false: For molecules with similar molecular weights, the dispersion forces become stronger as the molecules become more polarizable. a. b. For the noble gases, the dispersion forces decrease while the boiling points increase as you doWE the column in the periodic table. c. In terms of the total attractive forces for a given substance, dipole-dipole interactions, when present, are always greater than dispersion forces. d. All other factors being the same, dispersion forces between linear molecules are greater than those between molecules whose shapes are nearly spherical. e. The larger the atom, the more polarizable it is.

True or false: For molecules with similar molecular weights, the dispersion forces become stronger as the molecules become more polarizable. a. b. For the noble gases, the dispersion forces decrease while the boiling points increase as you doWE the column in the periodic table. c. In terms of the total attractive forces for a given substance, dipole-dipole interactions, when present, are always greater than dispersion forces. d. All other factors being the same, dispersion forces between linear molecules are greater than those between molecules whose shapes are nearly spherical. e. The larger the atom, the more polarizable it is.

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...

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Similar questions

1.) A larger dipole will create a stronger intermolecular interaction 2.) If the dipole is sufficiently large, dispersion forces can be neglected 3.) Polar molecules that form dipole-dipole bonds will always have stronger intermolecular networks than non-polar compounds that form dispersion forces only. Which statement or statements, if any, are true?
The high boiling point of water (100 °C) is due to. between water molecules. * van der Waals forces O ion-dipole interaction O dipole-dipole interaction O hydrogen bonding
PLease be detailed in your explination. Write a whole paragraph on it. Also explain using a diagram as well
The boiling point of HF is 19.5 and the boiling point for HCI is -85. Which of the following answers is the best explanation for the difference in these boiling points. The hydrogen bonding between molecules of HF are stronger than the hydrogen bonding forces between molecules of HCI. O The hydrogen bonding between molecules of HF are stronger than the dipole-diopole forces between molecules of HCI. O This is because the F atom in HF has less electrons than the Cl atom in HCI. This is because the dispersion forces between HCI molecules are weaker than the dispersion forces between HF molecules.
What is viscosity? For a liquid, it's viscosity decreases as temperature increases. Explain it in terms of intermolecular force?
Molecular or atomic solids and liquids are bound in their condensed phases by cohesive forces between the atoms or molecules. What is the extent of these cohesive forces in the gas phase?
Give detailed Solution with explanation needed
RANKING: Knowing the effects of intermolecular forces on the boiling points of substances, rank the ones below from weakest to strongest. CO,, Ar, CF,, LICI, SiF, Which of the following will have the highest boiling point? b. Which of the following will have the lowest boiling point? c. Explain your answers in a and b.
1. What is a chemical bond? How is it different from intermolecular forces of attraction?2. How is polarity related to the formation of intermolecular forces of attraction?3. Define the following weak intermolecular forces of attraction:a. Hydrogen bondb. Dipole-dipole interactionc. Ion-dipole interactiond. Electrostatic attractione. Van der Waals interaction4. It is common knowledge that most solids are denser than liquids. Within the context of intermolecular forces, how can you explain the phenomenon when solid ice floats in water?
O London-dispersion forces and hydrogen bonding Question 9 Which intermolecular forces are present in a pure sample of the compound below? NH₂ O hydrogen bonding, dipole-dipole, and London-dispersion forces O dipole-dipole and London-dispersion forces O London-dispersion forces only O London-dispersion and dipole-dipole forces Question 10 Based on your answers to Questions 7, 8, and 9, which ranks these three compounds in order of increasing water solubility?