chemistry question about orbitals.?

Question

why do the two electrons in the 2p sublevels of carbon occupy different 2p orbitals?

Answer 1

The s and p orbitals are close in energy. Close enough that the carbon can reconfigure itself and form hybridized orbitals by mixing of the s an p orbitals. This results in four - sp3 orbitals - each in a tetrahedral symmetry (this in energy minimum compared to s or p orbitals symmetry).

Answer 2

The electron configuration notation for carbon is 1s2, 2s2, 2p2. Remember that the p sublevel holds three orbitals; the order of filling is such that the first electron will enter the first orbital (or X orbital of the p sublevel) with a clockwise spin, then the 2nd electron will enter the next orbital of the p sublevel (y) and also have a clockwise spin. This is because of Hund's Rule, which states that electrons occupy equal-energy orbitals so that a maximum number of electrons results. The effect here is that a single electron, spinning clockwise, will occupy each orbital of all the orbitals of any sublevel before another electron can be added to any of the other orbitals in that sublevel. When the second electron is finally added to any orbital of any sublevel, it will automatically have a counterclockwise spin. Thus, it would be best to see carbon as 1s2, 2s2, 2px1, 2py1.

Answer 3

P is atomic type 15. So it could be placed interior the three-D era, and can be the 5th element in that era. all of us be conscious of the whole first era orbital notation is 1s2 the whole 2nd era notation is 2s2 2p6 The third era notation could be 3s2 3p3 the entire configuration could be 1s2 2s2 2p6 3s2 3px1 3py1 3pz1 that's prolonged to tutor that the electrons interior the 3p orbitals "load" one to each orbital first somewhat than 2 in a single, one in yet another, and none in a third. via fact the previous noble gas is Neon, this notation could be Ne 3s2 3p3.

Answer 4

Hund's Rule says that a single electron will exist in each degenerate orbital (with each electron having the same spin) until they all have a single electron. Then, they will begin to pair.