The principal energy level is three, so there are three sublevels: 3s, 3p, and 3d. S,P and D
There are three types of orbitals that involve the third energy level. 3s, 3p, 3d. But when only looking at the third period of the periodic table... The 3s pertains to Na and Mg. 3p pertains to Al, Si, P, S, Cl, and Ar. These tables, as you could say, are called Electron Configurations. Therefore, for Argon, Ar, the electron configuration would be 1s22s22p63s23p6 or in shorter version: [Ne] 3s23p6.
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Ultraviolet Types
7
The principal energy level is three, so there are three sublevels: 3s, 3p, and 3d. S,P and D
In the principal energy level n=4, you would find s, p, d, and f orbitals. These orbitals can hold different numbers of electrons and vary in shape and orientation within that energy level.
An s orbital
In the principal energy level n = 3, there are s, p, and d orbitals. The s sublevel has 1 orbital, the p sublevel has 3 orbitals, and the d sublevel has 5 orbitals. These orbitals can hold up to a total of 18 electrons.
In electron orbitals there are a few different types of orbitals or levels. Refering to the periodic table of elements, the s orbitals are spherical and are seen in the first to columns. The p orbitals are in the last four columns.
Aufbau: 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f In a 3p element, which include Al, Si, P, S, Cl, and Ar, there are 2p and 3p orbitals, of which only the 3p exists in the third energy level. There are three types of p orbital, px, py, and pz. They orient themselves in the x, y and z axes, as is suggested. Therefore, there are three p-orbitals in the third energy level.
Electrons orbit around the nucleus in an atom at different levels. The space between each level is referred to as an orbital.
Electrons orbit around the nucleus in an atom at different levels. The space between each level is referred to as an orbital.
In every atom there are principle energy levels, sub-levels and atomic orbitals. The principle energy levels are often those first taught when studying chemistry. They correspond to how close the electrons are to the nucleus. The first principle energy level is closest to the nucleus and can hold a maximum of two electrons. The second principle energy level is slightly further away from the nucleus and can hold a maximum of eight electrons. The third energy level is even further away and can hold a maximum of ten electrons. Each principle energy level is comprised of different sub-levels: s, p, d and f. The s sub-level can hold a maximum of two electrons; , p a maximum of 6; d, a maximum of 10 and f, a maximum of 14 (although the f sub-level is only present in the lanthanide and actanide series). Sub-levels all have different energies and electrons fill sub-levels in order of lowest energy to highest. The first principle energy level has one sub-level, the 1s sub-level. The second principle energy level has two sub-levels, 2s and 2p. The third principle energy level has three sub-levels, 3s 3p and 3d. (However, the 4s sub-level is filled before the 3d sub-level, which is a different matter which cannot be explained quite so simply.) Now, each sub-level is comprised of atomic orbitals which define the approximate boundaries of the electron orbit. Each orbital can hold up to two electrons, so a s sub-level has one orbital; a p sub-level has three orbitals; a d sub-level has five orbitals and a f sub-level has seven. This explanation is really quite brief as there is so much more information concerned with principle energy levels, sub-levels and atomic orbitals.
The allowed orbital types for the second period of the periodic table (n=2) are s and p orbitals. There are 2s and 2p orbitals in the second energy level, with a total of 4 orbitals available (1 s orbital and 3 p orbitals).
In the 8th energy level, there would be 8 sublevels (s, p, d, and f orbitals) in total. Each sublevel can hold a different number of electrons, with s holding 2, p holding 6, d holding 10, and f holding 14.
There are three different types of energy sources that are available. The three are hydro energy, wind energy, and solar energy.