Nitrogen's intermolecular bonding

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The discussion revolves around the properties and behavior of nitrogen in its liquid and solid states, focusing on the role of van der Waals forces. The difference between these states is primarily attributed to the quantity and strength of these forces. The conversation explores when nitrogen is ready for freezing, suggesting that it occurs when atomic kinetic energy allows for sufficient proximity to induce dipoles in neighboring molecules, although the exact breaking point is not clearly defined. The topic of dipole interactions is addressed, noting that while they are attractive, there are also repulsive interactions that prevent atomic collapse, primarily due to the Pauli exclusion principle. The discussion briefly touches on the behavior of other substances, emphasizing that many gases exhibit similar properties to nitrogen, with the van der Waals equation effectively describing the liquid-gas phase transition for gases like nitrogen. The conversation highlights the complexities of freezing transitions, particularly in substances with different bonding structures, such as glucose.
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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.
 
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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).
 

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