The 2s and2p orbitals are on the same energy because for higher elements more protons in the nucleus and hence electrons go closer to the nucleus and as the distance decreases the magnitude of energy increases.
They are the designation for the orbitals present. s and p orbitals in the 2nd energy level.
1s, 2s, and 2p
You can tell the difference between 2s sub-shell and 2p sub-shell by checking their energy levels whereby a 2p orbital has a higher energy level compared to a 2s orbital.
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.
All orbitals imaginable are about every atom regardless of what it is. In its ground state He has cause to only employ the 1s orbital; however, when its electrons are excited they can jump up and down through all possible energy levels producing emissions that are characteristic of its particular spectrum.
They are the designation for the orbitals present. s and p orbitals in the 2nd energy level.
4 (apex lol)
2. the 2s ordital and 2p
1s, 2s, and 2p
2s, 2p. 2s contains 1 orbital, the 2p sublevel contains 3 orbitals 2px 2py, 2pz where the suffix is the direction the orbital lies in, 2px lies on the x axis.
The 1s, 2s, 2p and 3s
You can tell the difference between 2s sub-shell and 2p sub-shell by checking their energy levels whereby a 2p orbital has a higher energy level compared to a 2s orbital.
No
Nitrogen has 5 valence electrons. Valence electrons are the electrons that are found in the outer most shell of an atom, and are consequently the electrons that move from atom to atom in the formation of compounds. The reason for this is a result of the electron configuration. A nitrogen atom has 3 orbitals; the 1s orbital, the 2s orbital, and the 2p orbital. In this case, the 2s and 2p orbitals are the valence orbitals, as they have the electrons with the most energy. With 7 protons, a neutral nitrogen atom has 7 electrons. The s orbitals can only hold 2 electrons, and the p orbitals can hold up to 6 electrons. The 1s orbital is filled first, leaving five electrons, then the 2s orbital is filled, leaving 3 electrons, and then these remaining electrons fill the 2p orbital halfway. There are a total of 5 electrons in the 2s and 2p orbitals, and since these orbitals have the most energy, there are 5 valence electrons.
You can tell the difference between a 2s sub-shell and 2p sub-shell from their energy levels, because a 2p sub-shell is a higher energy level than a 2s sub-shell.
8 electrons can be accommodated in the 2nd shell (aka 2nd energy level). 2 in the 2s orbital and 6 in the 2p orbitals.
There are 9 occupied orbitals in a phosphorus atom's ground state: one 1s orbital, one 2s orbital, three 2p orbitals, one 3s orbital, and three 3p orbitals.