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

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SUMMARY

The discussion focuses on the combustion reactions of hydrides B2H6, CH4, NH3, and H2S, specifically analyzing which reaction has the lowest energy of activation. It emphasizes the role of intermolecular forces and electronegativity in determining activation energy. The conversation also highlights that hydrogen bonding, particularly the O-H---O bond, is stronger than the N-H---H bond due to oxygen's higher electronegativity. Understanding these concepts is crucial for solving related chemistry problems.

PREREQUISITES
  • Understanding of combustion reactions and activation energy
  • Knowledge of intermolecular forces, specifically hydrogen bonding
  • Familiarity with electronegativity and its effects on molecular interactions
  • Basic concepts of molecular structure and bonding
NEXT STEPS
  • Research the activation energy of combustion reactions for various hydrides
  • Study the principles of hydrogen bonding and its implications in chemistry
  • Explore the concept of electronegativity and its role in determining bond strength
  • Learn about the different types of intermolecular forces and their effects on molecular behavior
USEFUL FOR

Chemistry students, educators, and professionals interested in understanding intermolecular forces, combustion reactions, and the factors influencing activation energy in chemical processes.

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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