# Chemical Forums

## Specialty Chemistry Forums => Nuclear Chemistry and Radiochemistry Forum => Topic started by: awesumsingh on July 16, 2014, 10:51:22 AM

Title: schrodinger wave equation and nuclear chemistry
Post by: awesumsingh on July 16, 2014, 10:51:22 AM
what is the schrodinger wave equation?
electron cloud?
i am really confused with all these and all my book seems to offer me is a set of very complex words and definitions.I am relatively new to atomic structure and related things so a brief answer in  simple words would really be helpful!also a bit on hamiltonian and laplacian operators and other related stuff!
Title: Re: schrodinger wave equation and nuclear chemistry
Post by: Enthalpy on July 16, 2014, 01:21:45 PM
Hi Awesumsingh, welcome here!

Schrödinger's equation tells how electrons (sometimes others) behave. It contains both the wave nature of electrons and the equivalent of d2x/dt2=qE/m.

Variants depend on if one puts importance on relativistic corrections, influences through the magnetic moment... which get included in the hamiltonian H or the mass.

The Hamiltonian pre-existed quantum mechanics. It relates the energy of a particle in some condition with its tendency to let the condition evolve over time. In classical mechanics, it told that a particle accelerates towards a location or condition where it has a smaller energy. QM generalizes it because a wave has a volume, so the electron exists also at locations less favourable - tunnel effect is nothing more.

The Laplacian is just the one used for any wave: acoustic, electromagnetic... and here an electron. Without potential energy, the electron propagates as any free wave does; with a potential, the electron concentrates where the energy is more favourable, and is almost always trapped near a nucleus, on Earth.

Being waves, electrons have no point-like positions. At most, one can compute a probability to find one in a volume around some position - and observed only by measurement means that are more accurate than an atom's size. And since electrons are identical, the experiment can't usually even tell which one was detected. The expression "electron cloud" reminds both.

The radial probability function is a probability to detect an electron in a spherical volume of dR thickness as a function of the distance. It differs from Ψ2 because the spherical volume increases as R2, so for instance the 1s orbital decreases over the distance, but the probability in a thin spherical volume first increases before decreasing.
http://www.chemistry.mcmaster.ca/esam/Chapter_3/section_2.html
And anyway, only s orbitals depend only on the distance and not on the direction, so this "radial probability function" gets less simple for other orbitals.

p, d, f... orbitals depend on the direction and have angular nodes in addition to radial ones. Best meditate the nice drawings there: