In electron configuration, why is it counted as 3d instead of 4d? Ex. Cr: 1s2 2s2 2p6 3s2 3p6 4s2 3d4. You would think it would be 1s2 2s2 2p6 3s2 3p6 4s2 4d4.
2006-10-11 12:03:57 · 4 answers · asked by m123 2 in Education & Reference ➔ Homework Help
when the electron is in 4s2 it is full of energy and skips a level of the configuration and then it goes back to the lower level
2006-10-11 12:06:02 · answer #1 · answered by Anonymous · 0⤊ 0⤋
The shapes of the orbitals are not spherical, but different shapes. These shapes are so wild-looking that they actually overlap each other around the atom. Electrons always take the lowest orbital (lowest energy) available, so if the overlapping orbital is lower in energy they will fill that one first. The 4s orbital is lower in energy than the arms of the 3d orbitals which extend beyond the 4s level, so the 4s fills before the 3d.
2006-10-11 19:08:42 · answer #2 · answered by physandchemteach 7 · 0⤊ 0⤋
No.first energy level has only s orbitals. second level, n=2, has s and p. Third level, n=3, has s, p, and d. n=4 has s, p, d, and f. When there are no electrons, all orbitals within the level are equal in energy. When electrons fill in the energy levels change: lowest is 1s then 2s, 2p, 3s, 3p ,4s, 3d,4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p............
I hope thi helps you.
2006-10-11 19:18:49 · answer #3 · answered by Anonymous · 0⤊ 0⤋
it's 3d, because the electrons that belong in the 'd' ring that appear on the 4th row actually below (from experiments) to the 3rd energy level. (n = 3)
2006-10-11 19:06:42 · answer #4 · answered by Jeffrey W 3 · 0⤊ 0⤋