How many different "p" orbitals are possible in an energy level?

Answer 1

In the Heisenberg Model you still have elements of the Bohr Model. That is there are still the quantised energy levels 1, 2, 3, 4, and so on.

However in the Heisenberg Model the energy levels or orbitals are split further into s, p and d orbitals. The p orbitals are split into three orbitals called px, py, and pz. The d orbital is split into dz2, dx2-y2, dxy, dxz, dyz. Again these sub orbitals have an order of in which electrons will enter them.


Not all electrons inhabit s orbitals (in fact, very few electrons live in s orbitals). At the first energy level, the only orbital available to electrons is the 1s orbital, but at the second level, as well as a 2s orbital, there are also orbitals called 2p orbitals.

A p orbital is rather like 2 identical balloons tied together at the nucleus. The diagram on the right is a cross-section through that 3-dimensional region of space. Once again, the orbital shows where there is a 95% chance of finding a particular electron.


Unlike an s orbital, a p orbital points in a particular direction - the one drawn points up and down the page.

At any one energy level it is possible to have three absolutely equivalent p orbitals pointing mutually at right angles to each other. These are arbitrarily given the symbols px, py and pz. This is simply for convenience - what you might think of as the x, y or z direction changes constantly as the atom tumbles in space.

The p orbitals at the second energy level are called 2px, 2py and 2pz. There are similar orbitals at subsequent levels - 3px, 3py, 3pz, 4px, 4py, 4pz and so on.

All levels except for the first level have p orbitals. At the higher levels the lobes get more elongated, with the most likely place to find the electron more distant from the nucleus.

Answer 2

3

Answer 3

a million. Orbitals may be idea-about because the actual route the electron follows around the nucleus. at the same time as potential aspect are the quantity of potential (in J or eV or the different potential contraptions) those particular orbitals own. the present idea says that each and every orbital corresponds to a diverse quantity of potential, thereby the orbital energies are at diverse ranges, and not in any respect a continuum. as an example orbital a million would own 5J, and orbital 2 may be at 10J, there isn't any longer some thing in between; if an electron own 7.5J of potential, it wouls nevertheless in effortless words exist at orbital a million, no longer some intermediate orbit. 2 & 3. Electrons closest to the nucleus have an decrease quantity of potential because they're more beneficial in touch in the pricey nucleus, which limit their freedom in a experience. while electrons extra away have more beneficial "freedom", and they'd go away the atomic nucleus (i.e develop into ionized) a lot more beneficial actual. in case you actual learn this in additional beneficial intensity, you'll study that each and every one bonded electrons actual own a detrimental potential. In a hydrogen atom, the first discreet potential aspect (n=a million) has -13.6eV, and the better potential ranges are merely a lot less detrimental. in case you supply the electron it is in that first potential aspect 13.6eV of potential, then it may now own 0eV of potential, and would destroy out the pull of the nucleus. the same idea is used for gravitational potential potential.

Answer 4

3. For a p level, L = 1. The possible values of m(L) are -L to +L, so m(L) can be -1, 0, or 1, where each m(L) value corresponds to one orbital.

Answer 5

There are 3 different p orbitals (x, y, z)