In the following pair of molecules, which would you expect to have a higher boiling point and why? CH3CI or Cl2 O CH3CI, because it is has more atoms and therefore has stronger London dispersion forces. O C2, because it is nonpolar and has stronger London dispersion forces. O CH3CI, because it has dipole-dipole forces. O Cl2 , because it is more massive and has stronger London dispersion forces.

In the following pair of molecules, which would you expect to have a higher boiling point and why? CH3CI or Cl2 O CH3CI, because it is has more atoms and therefore has stronger London dispersion forces. O C2, because it is nonpolar and has stronger London dispersion forces. O CH3CI, because it has dipole-dipole forces. O Cl2 , because it is more massive and has stronger London 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

Consider two molecular compounds: carbon monoxide (CO) and nitrogen (N2). Which statement below is TRUE? O Nitrogen (N2) has the higher boiling point because it has greater dispersion forces. O CO has the higher boiling point because it experiences dipole-dipole forces. O Both CO and N2 must have the same boiling point, since their molar masses are similar. O N2 has the higher boiling point because it experiences dipole-dipole forces.
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.
1. Use the information for the structure of A3Z to answer the following questions. Note: A has 7 valence electrons and Z has 5 valence electrons. The A-Z bond is polar. What is the bond angle? BI U X₂ X² Is the molecule polar? 109 What is the electron pair geometry? What is the molecular shape? What is the hybridization? BIUX, X² | BIU X₂ X² Type the molecular shape BIU X₂ X² Type the hybridization Polar O Non-Polar
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 of the following in the liquid state should have the highest boiling point? H2O C5H12 H2S NaBr
The molecules in a sample of liquid propionitrile, CH3CH2C≡N, are attracted to each other by which intermolecular forces? Select one: a.Dispersion forces and dipole-dipole interaction b.Hydrogen bonding and ionic bonding c.Dispersion forces and hydrogen bonding d.Covalent bonding and dipole-dipole interaction
1: Ã 01 Question 7 Which intermolecular forces are present in a pure sample of the compound below? O dipole-dipole and hydrogen bonding O London-dispersion forces only O hydrogen-bonding, dipole-dipole, and London-dispersion O dipole-dipole and London-dispersion forces Question 8
Polar or London Dispersion Dipole-Dipole Hydrogen Nonpolar Forces Forces Bonding 1.C,Hg 2.CH;OH 3.H;S 4.HF 5.НС
What is the predominant intermolecular force of attraction existing between the molecules shown below? H H. O Hydrogen bonding O Dipole-dipole interaction O London dispersion forces
The two compounds shown below have the same chemical formula. Which compound would you expect to have the highest boiling point? Explain your choice.
Argon is a noble gas and is expected to have a very low boiling point due to its weak intermolecular forces of attraction. Given CO2, HF, HCl, and NH3, which compound has a boiling point that is expected to be near to that of argon? a. HF b. HCl c. NH3 d. CO2
Which of these pure substances has only dispersion forces present between molecules? O H2 O HCI O NH3 o H20