There is no such level as 2d. In 1st level there is just 1s. In the 2nd level there is 2s and 2p. Only in the 3rd level is there 3s, 3p and 3d. The sublevels of 3d are
3 dxy dyz dxz d(x2-y2) dz2 so 5 sublevels of 3d.
There are three 2p orbitals and each can hold a maximum of two electrons with opposite spins, for a total of 6 electrons. This is true of the p sublevel in any energy level, except for the first energy level, which does not have a p sublevel.
All p sublevels contain three orbitals, including the 4p sublevel.
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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.
Nitrogen has one electron in the 2s orbital and three electrons in the 2p orbitals.
The 2p sublevel can hold a maximum of 6 electrons.
There are three 2p orbitals and each can hold a maximum of two electrons with opposite spins, for a total of 6 electrons. This is true of the p sublevel in any energy level, except for the first energy level, which does not have a p sublevel.
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There are 6 electrons in the 2p sublevel of fluorine. Each of the three p orbitals can hold 2 electrons, giving a total of 6 electrons in the 2p sublevel of an atom.
The electron in the second main energy level and second sublevel is described by the quantum numbers n=2 (main energy level) and l=1 (sublevel), which corresponds to the p orbital. The set of quantum numbers for this electron is 2p.
All p sublevels contain three orbitals, including the 4p sublevel.
6 electrons in 3 orbitals of p-sublevel: px, py and pz
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The 3rd period contains 2 of the 3 orbitals for the third sublevel. It has the s and p orbitals in it.
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.
Nitrogen has one electron in the 2s orbital and three electrons in the 2p orbitals.