Recently I moved to the north of Norway, so I've seen quite a few auroras. Because the colour is mainly green, I was sure this must be due to electron transitions in $\ce{N2}$ (because the atmosphere is like $75\%$ $\ce{N2}$) Looking into this, however, I found out that the colours of the aurora are mainly due to electron transitions in oxygen gas. Why is it that the electron transitions of oxygen are most prevalent in the colours of the aurora, even though it is far less abundant than nitrogen?

I also read that oxygen gas gives one colour up to $150$ miles altitude(green), and another above $150$ miles (red). Can someone explain the reason for the difference in colour? Does oxygen exist in different oxidation states at different altitudes, leading to different electron configurations => different available electron transitions?


3 Answers 3


There is good information at Glowing Gases - Aurorae

There are many factors that need to be considered.

Once an atom or molecule is excited, it can lose the energy by collision or by emission of light.

The longer the lifetime of the excited state, the higher the altitude is required to make radiation vs. collision the way energy is lost.

The atomic oxygen transition with green light has a lifetime of about 1 second, while the transition for red light is 110 seconds, so a higher altitude is required for the red transition to become significant.

For molecular nitrogen, radiative lifetime is only $4 \times 10^{-8}$ seconds according to Electronically excited molecular nitrogen and molecular oxygen in the high-latitude upper atmosphere Ann. Geophys., 26, 1159–1169, 2008

Also, human eyes are more sensitive to green light than red light.

  • $\begingroup$ This article is very useful, providing a good explaination for the variation of colour from Oxygen with heigth. However, I still remain unsatisfied With the explaination of why Nitrogen does not play a larger role in determining the colour of the aurora. Given that the atmostphere is 78% N2, but only 21% O2, how could this be? The article simply states "[...] nitrogen N2, is exceptionally stable and there are not many nitrogen atoms below 400 km to make aurorae." $\endgroup$
    – Adroit
    Commented Oct 13, 2016 at 16:38
  • $\begingroup$ @Adroit the composition of the atmosphere is much different at high altitude malagabay.files.wordpress.com/2014/07/… $\endgroup$
    – DavePhD
    Commented Oct 13, 2016 at 16:49
  • 1
    $\begingroup$ @Adroit - Nitrogen is really hard to ionize, even with energetic charged particles. Then you've got the non-radiative energy loss mechanisms thrown in. It is not simple. $\endgroup$
    – Jon Custer
    Commented Oct 13, 2016 at 18:56
  • $\begingroup$ @DavePhD When your source says "The transition is O 1S to 1D" about the green emission line from atomic oxygen, does this mean that the transition is from S to D orbitals both in the first Principal energy level(Bohr Shell n=1)? From my knowledge of quantum numbers the first Principal energy level only has one S-orbital. Is this what it means by "The singlet S to singlet D state transition is not allowed by the quantum selection rules for electric and magnetic dipole transitions"? $\endgroup$
    – Adroit
    Commented Oct 14, 2016 at 17:09
  • 1
    $\begingroup$ Yes, a free atom is a centrosymmetric environment. $\endgroup$
    – DavePhD
    Commented Oct 16, 2016 at 14:56

This phenomenon is already explained in this website, but I will paraphrase it.

All images here are from that website.

The atomic oxygen causes the green and the red color, while diatomic nitrogen causes blue and red:

The effect of altitude on the color is not explained.

However, an explanation is found on Wikipedia:

The highest altitudes have fewer particles, hence fewer collisions. In this state, the oxygen emits the lower-energy $630.0 \mathrm{nm}$ (red).

At lower altitudes, there are more collisions, and the nitrogen molecule also helps exciting atomic oxygen, so the higher-energy $557.7 \mathrm{nm}$ emission (green) dominates.

  • $\begingroup$ the cartoon has $\ce{N2}$ transmuting into $\ce{O}$ $\endgroup$
    – DavePhD
    Commented Oct 14, 2016 at 17:08

The anwer lies in understanding forbidden transitions. These are transitions which are "forbidden" by quantum mechanical electric dipole selection rules, have long radiative lifetimes and only occur radiatively if the density falls below some quenching threshold. Above this density the dexcitation takes place collisionally.

So let me advance a plausible explanation. The green northern lights are formed high up ($\geq 100$ km) in the Earth's atmosphere, largely by photons at 557.7 nm emitted from excited oxygen atoms. This is an example of a forbidden transition with a long radiative lifetime (a second or so).

Forbidden lines get "quenched" by collisions if the density is high enough - i.e. the atoms are de-excited by a collision rather than by emitting a "forbidden line" photon. At lower heights in the atmosphere the densities increase and the forbidden emission is quenched, thus we may not expect to see any green light emitted lower down in the atmosphere. This also accounts for the stripes of different colours that are sometime seen, caused by transitions with different radiative lifetimes and different collisional cross-sections that quench at different densities and hence heights.

A quantitative answer to the question would require a detailed model of the atmosphere (since the quenching densities are also temperature dependent), a model for the energy spectrum and flux (as a function of height) of the incident exciting particles as well as the detailed quantum mechanical radiative lifetimes and collisional cross-sections for each of the relevant transitions. I think that the relative abundances of oxygen and nitrogen play a very minor role compared with these factors.


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