On one energy level, how many electrions are needed to fill the s and p orbitals together?

Question

On one energy level, how many electrions are needed to fill the s and p orbitals together? And also, what is that called??

Answer 1

It takes 2 electrons to fill an s orbital and 6 for a p orbital. Therefore, for both, it takes 8. The s and p orbitals on the same, highest energy level are collectively called the "valence shell".

s and p orbitals can, according to the valence bond theory, "hybridize"- that is, add together to form orbitals resembling both, and bonds between atoms are formed when hybridized orbitals of both atoms overlap.

Answer 2

In any energy level, it takes 2 electrons to fill the s orbital and 6 to fill the p orbital, so it takes 8 to fill them both.

There's no special name for this as far as I know. However, where the highest energy level has both s and p orbitals filled you have the noble gases.

Answer 3

3 forces are in touch, the charm of detrimental electrons to the pricey nucleus. This forces the electrons to rhe LOWEST potential orbitals first. This determines the order in which orbital contraptions fill. for 2 electrons to occupy the same orbital they ought to have opposite spins. this makes them in touch in one yet another like opposite poles of a bar magnet. This, in spite of the undeniable fact that, is the weakest stress. it isn't waiting to conquer the like value repulsion of both electrons at the same time as an empty, same potential orbital is for sale. therefore orbital contraptions fill singly then doubly. apparently, contained in the nucleus, the debris pair up doubly first, earlier yet another orbital is filled. also, the orbital contraptions fill in a diverse order. 1s, 1p, 1d, 2s, 1f, and so on.

Answer 4

it always takes 2 electrons to fill the s orbitals and 6 to fill the p orbitals

Answer 5

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