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.
2. The five d orbitals can hold ten in total.
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.
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
Two electrons in the outer shell of radium.
Any orbital is complete when it contains 2 electrons.
Ground state.
Any orbital can hold a maximum of 2 electrons
Two electrons can fit into the first orbital shell of any atom.
An unoccupied orbital is represented by an empty box in orbital notation. It does not have any electrons present in it but is available to accept electrons if needed.
Yes a single orbital in the 3d level can hold 2 electrons.
2. The five d orbitals can hold ten in total.
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.
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.
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.
it depends on which orbital: 1: 2 2: 8 3: 18 4: 32 5: 50 6: 72 7: 98 despite the large capacities, atoms will typically attempt to maintain 8 valence electrons.
In any shell excluding shell1, there is only 1 s orbital and 1 p orbital. Subshells and the Orbitals are same. Orbital g is known as subshell 5. g orbital is present shell 6. But till today no element is discovered with an electron in g orbital.