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I came up with this question when I was trying to determine whether H2O2 is polar or not.

H2O2 looks like this when looked parallel to oxygen-oxygen bound:(source: Pubchem) -

Each hydrogen is in one of the three positions available around each oxygen(the two nonbonding electron pairs occupy the other two); even the oxygen-oxygen bound can rotate to set hydrogens in any position relative to each other. Therefore I don't see the problem in following nonpolar structure(pretty neat!)


What concept am I missing while determining molecular geometry?

Is a H2O2 molecule sometimes polar and sometimes nonpolar?

Thanks for your help!


marked as duplicate by bon, Todd Minehardt, M.A.R. ಠ_ಠ, Jan, ringo Sep 2 '16 at 23:50

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  • 1
    $\begingroup$ The answer is not quite easy, you can find the answer of your question there deepblue.lib.umich.edu/bitstream/handle/2027.42/71115/… but I guess it would be better if someone could explain it too you. I have not time right now, but there is difference of energy in comparaison with ethene about the rotation on the single bond. It is an atropisomer en.wikipedia.org/wiki/Atropisomer $\endgroup$ – Hexacoordinate-C Sep 2 '16 at 16:11
  • $\begingroup$ The conformation of hydrogen peroxide (H2O2) is dominated by the lone pairs rather than the hydrogen atoms. Instead of the expected anti conformation in the free state the dihedral angle is 94°. The conformation of hydrogen peroxide is therefore neither eclipsed nor staggered but an intermediate structure. When in the solid state hydrogen bonding will cause the shape and angles to change. $\endgroup$ – Hexacoordinate-C Sep 2 '16 at 16:17
  • $\begingroup$ I suppose you could reason with orbitals/VSEPR that for hydrogen on one oxygen to line up with a lone pair on the other oxygen as a kind of hydrogen bonding, the planar version would require the oxygens to be sp2 hybridized rather than sp3 hybridized, which is unfavored due to electron pair repulsion favoring sp3. $\endgroup$ – user19026 Sep 2 '16 at 16:25
  • $\begingroup$ Maybe useful: chemistry.stackexchange.com/a/69587/40029 $\endgroup$ – Felipe S. S. Schneider Mar 2 '17 at 12:31

As stated in the link provided by @Shadock, hydrogen peroxide, like many more other molecules, is subject to hindered internal rotation. When you rotate the two OH groups with respect to each other around the O-O bond, this requires a certain energy depending on the relative angle. In the eclipsed configuration (OH groups pointing in the same direction), it's easy to see that there must be a maximum in the potentiall due to the Paulli repulsion. In the anti-eclipsed configuration (both OH groups pointing in opposite directions) there is another maximum as you anti align the two dipoles of the groups. In between these maxima, you'll find a minimum and the potential can be expanded as a Fourier series in the relative bond angle


where $V_2$ and $V_4$ are related to the heights of the two barriers. If the barriers were infinitely high, the OH groups would act as a quantum harmonic oscillator in one of the potential minima. On the other hand, if the barrier were very small, the OH groups would rotate freely around each other. In the case of hydrogen peroxide, the eclipsed barrier is so high that the OH groups can hardly go over/through it. The lower barrier is a different story. It is high enough to support a few vibrational levels, but not high enough to prevent the OH groups from tunnelling through the barrier and as a consequence, these energy levels are split in two. (In fact, these two levels are again split by the tunnelling through the higher barrier, but since this is so high the splitting is very small). Mathematically, the Schroedinger equation for this periodic potential is equivalent to the Mathieu equation (or more general Hill's equation).

In the case of H$_2$O$_2$ the tunnelling is so fast, that the molecule vibrates around the lower barrier with a period of ~100 fs. As a consequence, to determine the polarity, you have to average over this motion, resulting in a net polarity.

Note that, if the barrier would be so high that tunnelling would be sufficiently slow, H$_2$O$_2$ would be a chiral molecule!

  • $\begingroup$ I'm sorry but i don't get the second maximum. Why anti aligning the two dipole groups increases potential? $\endgroup$ – Rima Sep 2 '16 at 17:48
  • $\begingroup$ An intuitive example is the alignment of two bar magnets; if you align the poles in the same direction you have an attractive force whereas you'll experience a repulsive force when you anti align them, i.e., put the two north or south poles together. $\endgroup$ – Paul Sep 2 '16 at 20:50

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