6 electrons can ocupy the 2p, 3p, 4p, and so on.
each p subshell has 3 orbitals, and each orbital can hold up to 2 electrons, so each p subshell can hold up to 6 electrons total.
The p suborbital is the second orbital to be filled in an atom, starting with the second period. Each p suborbital can hold a maximum of six electrons.
the p orbital can hold up to six electrons
6 electron are ther in p-orbital
the p-orbital always contain six eletron
There is technically a 9i orbital, but no atom in the ground state has any electrons in this orbital (in fact, no known element has any electrons in even the 8s orbital, and there are quite a few energy levels between that and 9i). In an excited state ... sure, it could happen.
There can be a maximum of 14 electrons in any "f" orbital. However, the 3f orbital does not exist. f orbitals are only found in quantum energy level 4 and above.
2. The five d orbitals can hold ten in total.
Since they are p orbitals, 6 electrons are occupied in the 3p orbital. there are 3 types of p orbital, px, py and pz
In any one orbital there is only one way to arrange the two electrons and that is with opposite spin. (Paulis exlusion principle) In the 3 different p orbitals you could arrange 2 electrons without spin pairing in the same orbital in 3 ways, The middle two are the same. The same applies to d orbitals
Any orbital is complete when it contains 2 electrons.
Ground state.
Any orbital can hold a maximum of 2 electrons
Yes a single orbital in the 3d level can hold 2 electrons.
When you fill an orbital the electrons must spin in opposite directions. This results in no two electrons having the same quantum number, a result defined as the Pauli Exclusion Principle. You can have 2 electrons in an orbital. Note that 2py 2px and 2pz are three different orbitals.
Two electrons can fit into the first orbital shell of any atom.
There is technically a 9i orbital, but no atom in the ground state has any electrons in this orbital (in fact, no known element has any electrons in even the 8s orbital, and there are quite a few energy levels between that and 9i). In an excited state ... sure, it could happen.
The max. number of electrons that can fill the 3s orbital is 2.
There can be a maximum of 14 electrons in any "f" orbital. However, the 3f orbital does not exist. f orbitals are only found in quantum energy level 4 and above.
The 2p sub-level can hold a maximum of 6 electrons. The 2p sub-level is divided into 2px, 2py and 2pz. Each of those orbitals can hold a maximum of 2 electrons. There are 3 of them and thus 6 total for the 2p sub-level.
2. The five d orbitals can hold ten in total.
Since they are p orbitals, 6 electrons are occupied in the 3p orbital. there are 3 types of p orbital, px, py and pz