Solving Intermolecular Bonding Exercises: B2H6, CH4, NH3 & H2S

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Discussion Overview

The discussion focuses on solving exercises related to intermolecular bonding and combustion reactions of various hydrides, specifically B2H6, CH4, NH3, and H2S. Participants explore concepts of activation energy and hydrogen bonding strength, seeking clarification and hints to guide their understanding.

Discussion Character

  • Exploratory
  • Technical explanation
  • Homework-related

Main Points Raised

  • One participant requests help determining which combustion reaction has the lowest energy of activation, suggesting a need to consider intermolecular forces.
  • Another participant emphasizes the importance of thinking about electronegativity when discussing hydrogen bonding strength.
  • A later reply proposes that the O-H---O hydrogen bond is stronger than the N-H---H bond due to oxygen's higher electronegativity, which results in a greater dipole strength.
  • One participant expresses confusion about relating intermolecular forces to activation energy and seeks further clarification.
  • Another participant questions what keeps atoms in molecules from breaking apart and what is necessary to break bonds between atoms.

Areas of Agreement / Disagreement

Participants do not reach a consensus on the relationship between intermolecular forces and activation energy, as well as the strength of hydrogen bonds, indicating that multiple views and uncertainties remain in the discussion.

Contextual Notes

Participants have not fully resolved the connections between intermolecular forces and activation energy, nor have they clarified the assumptions regarding the strength of hydrogen bonds based on electronegativity.

broegger
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Hi. I need help with (part of) this exercise:

c) By considering the differences in bonding determine which of the combustion reactions (in part a) I have written combustion reactions for the following hydrides: B2H6, CH4, NH3 and H2S) must be expected to have the lowest energy of activation.

f) Hydrogen bonding is the strongest intermolecular interaction, and it is of enormous importance in chemistry. Two important hydrogen bondings is O-H---O and N-H---H. Which of these two hydrogen bonds must be expected to be strongest (explain)?

I'm lost again... Any hints?
 
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You know the rules - we need to some some thought process from you first.
 
c) Think intermolecular forces.
f) Think electronegativity.
 
end3r7 said:
c) Think intermolecular forces.
f) Think electronegativity.

c) Still in the dark. Can't relate these things to the activation energy... sorry.

f) Oxygen is more electronegative than nitrogen, so the OH-molecule has a greater dipole strength than the NH-molecule and therefore the hydrogen bond is stronger in the former case (O-H---O). Right?

Thanks for helping.
 
c) What is it that is keeping the atoms in the molecules from just breaking loose? What is needed to break bonds between atoms?
 

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