lon-dipole interaction Dipole-dipole interaction lon-ion interaction Induced dipole-dipole interaction Decane is liquid while Ethane is gas at room temperature. This can be as the carbon chain increases. explained by stronger O London dispersion force hydrogen bond induced dipole-dipole interaction dipole-dipole interaction

lon-dipole interaction Dipole-dipole interaction lon-ion interaction Induced dipole-dipole interaction Decane is liquid while Ethane is gas at room temperature. This can be as the carbon chain increases. explained by stronger O London dispersion force hydrogen bond induced dipole-dipole interaction dipole-dipole interaction

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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Dipole-dipole interactions typically are not as strong as ion-dipole interactions because a) ion-dipole interactions involve only the partial transfer of charge between atoms. Ob) ion-dipole interactions involve partial charges caused by the equal sharing of electrons by atoms forming a bond. c) ion-dipole interactions always involve water. d) dipole-dipole interactions involve only partial charges caused by an unequal sharing of electrons by atoms forming a bond. dipole-dipole interactions involve the complete transfer of charge between atoms. e)
Which of the following explains the sublimation (solid gas ⟶ change of state) of carbon dioxide observed at room temperature? Group of answer choices Ion-induced dipole forces hold carbon dioxide in the solid state. Dipole-dipole forces hold carbon dioxide in the solid state. Dispersion forces hold carbon dioxide in the solid state. Ion-dipole forces hold carbon dioxide in the solid state. Dipole-induced dipole forces hold carbon dioxide in the solid state.
Which is NOT belong to the group
Decide which intermolecular forces act between the molecules of each compound in the table below. compound nitrogen trichloride carbon dioxide hydrogen chloride CHA methane intermolecular forces (check all that apply) dispersion dipole hydrogen-bonding O 0 □ 0 X
Butter easily melts than potassium nitrate because the type of interaction in butter is while in potassium nitrate it is Induced dipole-dipole interaction, ion-ion interaction O Induced dipole-dipole interaction, dipole-dipole interaction London dispersion force, dipole-dipole interaction London dispersion force, ion-ion interaction Acetone easily evaporates than water. It can be explained by the weaker interaction between acetone molecules than interaction between water molecules." O Dipole-dipole, Hydrogen bond London dispersion forces, lon-ion Dipole-dipole, lon-ion lon-ion, Hydrogen bond Hydrogen fluoride (HF) has higher boiling point than Hydrogen bromide (HBr) because of between HF molecules. * O ion-ion interaction lon-dipole interaction Dipole-dipole interaction Hydrogen bond O O O O O O O O O
Intermolecular force between molecules of a substance involving hydrogen being chemically combined with fluorine: * A. Ion - Dipole Interaction B. London Dispersion Force C. Hydrogen Bond D. Dipole - Dipole Interaction
Identify the intermolecular force between NaSiO3 and water. Group of answer choices Ion-dipole intermolecular force Dipole-dipole intermolecular force Dispersion forces Hydrogen bonding Ion-induced dipole intermolecular force Dipole-induced dipole intermolecular force
Which type of intermolecular interaction is shown below? ion-ion H-bond ion-dipole H dipole-dipole +N H induced dipole/dispersion H |||H
Stronger intermolecular forces will lead to which of the following? Select all that apply. Higher volatility U Higher surface tension O Higher boiling point Higher vapor pressure O Higher viscosity
What two factors causes hydrogen bonds to be so much stronger than typical dipole-dipole bonds?
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