What type of orbital is represented by

It is important to note here that these orbitals, shells etc. As with any theory, these explanations will only stand as truth until someone you maybe?

So here are a couple of pictures of atoms with their shells populated by electrons to help you remember this atomic theory. If you still need more review, the theory was presented in Kotz Chapter 7. So now that we have reminded ourselves about the orbitals and how the electrons fill them, we need to address how these orbitals interact when two or more atoms bond together. Those orbitals are spheres. The higher the value of n, the larger the sphere — that is, the more likely it is that the electron will be found farther from the nucleus.

The spheres are not equally dense throughout; they are more like nested shells. For historical reasons, this is called an s orbital. The s orbital also exists for every other value of n. When n is larger than one, more possibilities open up.

L, the orbital quantum number, can have any value up to n When l equals one, the orbital is called a p orbital. P orbitals look kind of like dumbbells. For each l, m goes from positive to negative l in steps of one.

That means there are three versions of the p orbital: one with the dumbbell up and down, another with the dumbbell left-to-right, and another with the dumbbell at right angles to both of the others.

P orbitals exist for all principal quantum numbers greater than one, although they have additional structure as n gets higher. The other four d orbitals look like four eggs stacked on end in a square pattern. When electrons are placed in a set of orbitals of equal energy, they are spread out as much as possible to give as few paired electrons as possible Hund's rule.

In a ground state configuration, all of the electrons are in as low an energy level as it is possible for them to be. When an electron absorbs energy, it occupies a higher energy orbital, and is said to be in an excited state. The electrons in the outermost shell the ones with the highest value of n are the most energetic, and are the ones which are exposed to other atoms. This shell is known as the valence shell.

The inner, core electrons inner shell do not usually play a role in chemical bonding. Elements with similar properties generally have similar outer shell configurations. The next shell down is now the outermost shell, which is now full — meaning there is very little tendency to gain or lose more electrons.