Nitrogen's intermolecular bonding

  • Thread starter Thread starter sludger13
  • Start date Start date
  • Tags Tags
    Bonding
Click For Summary

Discussion Overview

The discussion revolves around the intermolecular bonding of nitrogen (N2), specifically focusing on the differences between its liquid and solid states, the conditions for freezing, and the nature of intermolecular forces involved. Participants explore theoretical aspects of bonding, phase transitions, and the behavior of similar substances.

Discussion Character

  • Exploratory
  • Technical explanation
  • Conceptual clarification
  • Debate/contested

Main Points Raised

  • One participant questions whether the difference between liquid and solid nitrogen is solely due to the quantity of van der Waals forces.
  • Another participant inquires about the conditions under which nitrogen is ready for freezing, suggesting it relates to the kinetic energy of atoms and the strength of induced dipoles.
  • A participant asks about the nature of repulsive interactions that prevent atomic collapse, specifically in the context of dipole interactions being attractive.
  • Some participants express uncertainty about the behavior of other substances with similar properties to nitrogen, noting that freezing transitions can vary based on the type of bonding present.
  • One participant asserts that no covalent bonds are created during the freezing process.
  • Another participant proposes that some inorganic substances may have covalent bonds in their solid state that disappear as atoms become sufficiently distant.
  • A later reply references the van der Waals equation as a qualitative description of the liquid-gas phase transition for gases like nitrogen, mentioning attractive and repulsive interactions.

Areas of Agreement / Disagreement

Participants express differing views on the nature of bonding during freezing and the role of covalent bonds in various substances. The discussion remains unresolved, with multiple competing perspectives on the behavior of nitrogen and similar substances.

Contextual Notes

Participants highlight limitations in understanding the behavior of substances with different bonding types and the complexity of phase transitions. There is also mention of unresolved assumptions regarding the nature of interactions at different states.

sludger13
Messages
83
Reaction score
0
Hi again, I have a couple of questions:
1) Nitrogen (N2) exists liquid and solid. The molecules bond with van der Waals forces. What's the difference between liquid and solid state? Just quantity of van der Waals forces?

2) When is nitrogen ready for freezing? When atoms have such a heat kinetic energy, that they bring near enough and the induced electric field is strong enough to induce dipoles in another molecules? Or where is the breaking point?

3) Dipole's interaction is attractive. What's the repulsive interactions, in order atoms don't collapse?

4) One more question here (LINK). I hope I'm not so much annoying with that. :shy:
Thanks for every single advice or remark.
 
Chemistry news on Phys.org
Why do you limit your question to nitrogen? The answer would be mostly identical for every other substance that can exist as a gas (by which I mean it doesn't decompose before becoming gaseous, think glucose for example).
 
Of course, I don't understand the behaviour of many other substances with similar properties.
Some substances have obvious freezing transition, as covalent bonds are creating. Glucose doesn't belongs there, with its molecular (or ionic) crystal structure (I don't know, maybe glucose can't even get liquid, due to pyrolysis).
 
There are no covalent bonds created during freezing.
 
I thought maybe some inorganic substances are covalent bonded in solid state (e.g. graphite) and some of those covalent bonds disappear as the atoms are sufficiently distant (the orbitals are no longer overlapping).
 

Similar threads

About Van Der Waals interactions
  • · Replies 2 ·
Replies
2
Views
2K
Van der Waals' Forces and Hydrogen Bonding
  • · Replies 2 ·
Replies
2
Views
2K
How Do Volume Expansions Differ in Liquids and Gases Due to Temperature Change?
  • · Replies 1 ·
Replies
1
Views
2K
Undergrad Covalent Bonds -- Which type of force?
  • · Replies 8 ·
Replies
8
Views
3K
Chemical Bonds - various questions
  • · Replies 3 ·
Replies
3
Views
2K
Effect of intermolecular hydrogen bonding
  • · Replies 3 ·
Replies
3
Views
2K
What type of intermolecular forces are exhibited in BF3?
  • · Replies 8 ·
Replies
8
Views
13K
Implementing “Ab initio” approach in molecular mechanics method
  • · Replies 4 ·
Replies
4
Views
2K
Undergrad Wall material effect on Van der Waals gas?
  • · Replies 23 ·
Replies
23
Views
3K
Van der Waals vs. Hydrogen bonds
  • · Replies 1 ·
Replies
1
Views
3K