diatomic

When the Cv of a diatomic gas goes from 3/2R to 5/2R there is an intermediate part that is complicated.

But if there's a reducing agent around, such as charcoal, coal or fuel oil, you'll get lots of diatomic nitrogen.

Actually I'm not sure hydrogen is worse, because it's normally found in diatomic form.

Those atoms have probably been recently recombined to form the diatomic gas, by plants.

Calculations are mostly done on atoms and diatomic molecules to benchmark the functionals.

Monatomic gas can't store any energy in rotation whereas diatomic and larger molecules can.

Uh chemistry is only predictable from first principles for diatomic molecules, or very simple extended structures like perfect bulk graphene.

Knowing nothing about this, broadly speaking, the enthalpy of formation of the diatomic nitrogen molecule is very high, and you might expect to achieve high energy density.

One of the things that amazes me is that it is still not possible to do an ab initio quantum mechanics calculation of the rotational spectrum of even a diatomic molecule with sufficient accuracy to allow identification from measured spectra.

In a presentsrion by Rich Hickey, one of the answers in the Q&A section afterwards about this was along the lines of "I want to put my kids in college"I too am very interested in diatomic, but I find the no benchmarking clause to be absolutely ridiculous in this environment.

The manufacturing process for ammonium nitrate involves using quite considerable amounts of energy to persuade nitrogen to get itself hitched to hydrogen and oxygen, but it would much rather be free as diatomic nitrogen, and when that happens you get that energy back.