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I recently learned about orbitals in class, and I am really confused.

I am very confused about what the orbitals look like, what the signs (such as $-2s, ---2p$ etc.) mean and how they work.

What they taught us was how there are little spaces that the electrons can fit through, because they want to get to the center of the atom, and how $2s$ is in the shape of the sphere.

But I am confused how everything is laid out. Is the "sphere" shape inside the shell and around the nucleus, or is it containing the shell. but inside another shell.

They also introduced something about the $x,y,z$ axis and I am just as confused on that too.

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    $\begingroup$ These are not signs, but merely placeholders for electrons. Also, there are really no such things as "inside" or "fit"; basically, every orbital is everywhere, and they simply go through each other, much like ghosts. All in all, orbitals are much less real than everyday things. $\endgroup$ – Ivan Neretin Oct 6 '16 at 21:10
  • $\begingroup$ The basic idea is orbitals are region around the nucleus where we can find electrons with largest probability. I usually visualize a orbitals similar(not same) to a physcial address (eg:BBC Broadcasting House, Portland Place, LONDON, W1A 1AA). Just like we can find BBC broadcasting house with high probability(99.999...9%) on that address, orbitals are space where we can find electons $\endgroup$ – Eka Oct 6 '16 at 23:08
  • $\begingroup$ Oh... very different than how I imagined it... $\endgroup$ – Frank Oct 6 '16 at 23:10
  • $\begingroup$ @Frank, you've received some excellent answers below, they give a good picture of the idea of orbitals (especially when combined). I just want to offer a few words that may help tie it all together: the graphic representations of the orbitals can be thought of as inflated balloons. The electrons that fill them can be anywhere within the balloon (perhaps they are constantly appearing and disappearing at different locations), but at any time most of the volume of the balloons is empty of electrons - the majority of an atom's volume is nothing, but it serves as potential location of electrons. $\endgroup$ – Don_S Nov 27 '16 at 6:10
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First thing you need to understand is that orbitals are not actual physical things that exist. Simply put, an orbital is a function that describes the probability of finding the electron with certain energy at certain distance from the nucleus. The shapes of the orbitals are just the boundaries of space where you can find the electron 90% of the time.

Electrons behave both as particles and waves. Their wave behavior is described by what is called a wave function. It has two components - radial and angular. The radial component depends on the distance from the nucleus while the angular depends on the direction. It is the angular component that shapes the orbitals. Just as it is, the wave function does not have any physical meaning, but it's square is proportional to the probability of finding the electron in a particular region of space around the nucleus.

The x, y and z axis simply refer to the Cartesian coordinate system and can describe points in 3D space. Imagine three lines where each of them is perpendicular to the other two. It doesn't matter which one you name x, y or z, this is all arbitrary.

The electrons around the nucleus are not really ordered. The terms shell, sub-shell, orbital are just a way of describing different energy levels and probabilities of finding electrons around the nucleus.

There are four quantum numbers that describe electrons in atoms - principal, azimuthal, magnetic and spin.

The principal quantum number (n) can take integer values from 1 to infinity. It describes the different energy levels with increasing distance from the nucleus. As n gets bigger, orbitals within that "shell" also increase in size.

The azimuthal quantum number (l) can take values from 0 to n-1. It describes the type of orbital the electron resides in. It is also call angular momentum quantum number and as I've said above, the angular wave function is responsible for the shape of the orbitals. Makes sense? For each value of l, there is a different type of orbital - 0=s, 1=p, 2=d, 4=f, 5=g (not really seen occupied in the ground state of any element), and these can go on alphabetically.

The magnetic quantum number (ml) describes the direction of the orbital in space with respect to the three Cartesian axis - x, y and z. It can take values from -l to +l. For s orbital, ml can only be 0 and so there is only one s orbital that can exist for a particular principal quantum number. For p orbitals, ml can be -1, 0 and +1 and so there are three p orbitals that can exist - each along different axis - px, py and pz. The axis labeling get more complicated for d and f orbitals.

The spin quantum number (ms) can either be +1/2 or -1/2 and simply describes the direction an electron spins around its axis.

For n=1, l can only be 0 and so there is only an s orbital in that level, referred to as 1s. For n=2, l=0,1 and there can be s and p-types orbitals. For n=3, l=0,1,2 and so you can have s, p and d orbitals in the third shell.

When you're filling up shells with electrons, you go from the lowest energy level to the highest and this can easily be determined by summing up n+l which would give you the relative energies of orbitals. When n+l is the same for two orbitals, the one with the lower n fills up first. One orbital can house 2 electrons which must have opposite spins. There can never be two electrons with the same four quantum numbers in a system (Pauli exclusion principle).

Sorry if I went into too much detail but if you don't understand anything please comment so that I can clarify.

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  • $\begingroup$ how we choose our x y z components ? in what reference frame ? $\endgroup$ – ado sar May 13 at 17:31
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The hard part of quantum mechanics is that you can't know how everything is laid out. Elections fit into some distribution about the nucleus defined by the mathematical functions that are the orbitals. You can't practically know where they are per se, just where they are likely to be.

The traditional orbits you learn about are a gross oversimplification.

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What is an orbital?

According to the Oxford Dictionary of English [1], orbital is defined as

Each of the actual or potential patterns of electron density which may be formed in an atom or molecule by one or more electrons, and can be represented as a wave function.

Wikipedia [2] says:

In quantum mechanics, an atomic orbital is a mathematical function that describes the wave-like behavior of either one electron or a pair of electrons in an atom.

If you go to Wikibooks [3], you will get that:

Each shell is subdivided into subshells, which are made up of orbitals, each of which has electrons with different angular momentum. Each orbital in a shell has a characteristic shape, and is named by a letter. They are: s, p, d, and f. (…) Within any particular shell, the energy of the orbitals depend on the angular momentum of orbitals s, p, d, and f in order of lowest to highest energy. No two orbitals have the same energy level.

(…)

enter image description here

Wikipedia [2] shows these graphical representations:

The shapes of the first five atomic orbitals are: $1s$, $2s$, $2p_x$, $2p_y$, and $2p_z$. The two colors show the phase or sign of the wave function in each region. These are graphs of $ψ(x, y, z)$ functions which depend on the coordinates of one electron. (…)

References

[1] Oxford Dictionary of English, 3rd ed.; Stevenson, A, Ed.; Oxford University Press: Oxford, U.K., 2010.
[2] Atomic orbital. Wikipedia, The Free Encyclopedia. [Online]; Posted October 29, 2016. https://en.wikipedia.org/w/index.php?title=Atomic_orbital&oldid=746850729 (accessed Oct 29, 2016).
[3] General Chemistry/Shells and Orbitals. Wikibooks, The Free Textbook Project. [Online]; 7 November 7, 2016. https://en.wikibooks.org/w/index.php?title=General_Chemistry/Shells_and_Orbitals&oldid=3143833 (accessed Nov 7, 2016).

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The form of the orbitals in an atom is determined by the charges and the masses of the electrons and the nucleus. The orbitals determine regions of space where an electron is most likely to be found if we make a measurement of the position of the electron. However make no mistake. The electrons in an atomic orbital can have a well-determined energy, a well-determined total angular momentum and a well-determined projection of the angular momentum on an arbitrarily chosen z-axis. It can also have a spin quantum number. But it cannot have a well-determined position. The electron in an atomic orbital has lost its particle property and has become wave-like. Its charge and mass is smeared out over the orbital and replaced by a density function given by the absolute square of the orbital mathematical function. This density function can be used to calculate the exact Coulomb potential energy of the atom. This Coulomb energy also determines the total kinetic energy (and hence the total energy) of the atom by the virial theorem.

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