There are 2 energy levels in a Carbon atom. The first energy level consists of '1s' orbital, and the second energy level consists of the '2s' orbital and the '2p' orbital.
It has a lower energy level. All else being equal, electrons tend to go into the lowest energy orbital with space available.
The s orbital fills before the p orbital because it has lower energy, and is more stable.
If the S orbital has two electrons and the P orbital has six you go on to the D orbital. Electron energy levels follow this format: 1s2 2s2 2p6 3s2 3p6 4s2 4p6 4d10 and so on
The s orbital is lower in energy than the porbital.
Because of the energy levels, sublevels and the probability map
the s orbital is lower in energy than the p orbital
There are 2 energy levels in a Carbon atom. The first energy level consists of '1s' orbital, and the second energy level consists of the '2s' orbital and the '2p' orbital.
It has a lower energy level. All else being equal, electrons tend to go into the lowest energy orbital with space available.
The s orbital fills before the p orbital because it has lower energy, and is more stable.
The shape of a p orbital is like a dumbbell-shaped. P orbital shapes depends on the quantum numbers affiliated with an energy state.
Each electron in an atom is in an orbital (*NOT* an orbit!!) at a specific energy level from the positive nucleus. The energy levels of these orbitals are fixed -- an electron can go from orbital 's' to orbital 'p', but it can't go halfway between these two orbitals. When an electron in an atom goes from a higher orbital to a lower one, then the atom must give off an amount of energy, that is exactly the difference in energy in the two levels. For a hydrogen atom, these orbital levels are fixed by the fact that the angular momentum of an electron in an orbital is quantized -- ie, it comes in exact multiples, but not fractions, of a minimal amount.
Each electron in an atom is in an orbital (*NOT* an orbit!!) at a specific energy level from the positive nucleus. The energy levels of these orbitals are fixed -- an electron can go from orbital 's' to orbital 'p', but it can't go halfway between these two orbitals. When an electron in an atom goes from a higher orbital to a lower one, then the atom must give off an amount of energy, that is exactly the difference in energy in the two levels. For a hydrogen atom, these orbital levels are fixed by the fact that the angular momentum of an electron in an orbital is quantized -- ie, it comes in exact multiples, but not fractions, of a minimal amount.
The quantum number relating to the size and energy of an orbital
Each main energy level (1 to 7) has at least an s-orbital, p-orbitals are possible from the second level onwards (2 to 7) d-orbitals from 4th level f-orbitals from 6th level
If the S orbital has two electrons and the P orbital has six you go on to the D orbital. Electron energy levels follow this format: 1s2 2s2 2p6 3s2 3p6 4s2 4p6 4d10 and so on
2p