s-orbital = 2e-
(s) orbital can hold 2 electrons, each with opposite spin.
p-orbital = 6e-
(p) orbital can hold 6 electrons in 3 suborbitals, so 2 electrons in each
d-orbital = 10e-
(d) orbital can hold 10 electrons in 5 suborbitals, so 2 electrons in each
f-orbital = 14e-
(f) orbital can hold 14 electrons in 7 suborbitals, so 2 electrons in each
trick question, you would think 1s=2, 2p=6, 3d=10, 4f=14... but each orbit can hold only 2e-
This is true if you mean orbitals and not orbits.
Each orbital can contain a maximum of two electrons, each with opposite spins.
2
2 electrons
There are 5 d orbitals which hold 2 electrons each. Thus, 10 electrons are needed to completely fill them.
There can only be 2 electrons in each single orbital, and they will be on opposite sides of the electron cloud (orbital).
6 electrons in total, 2 in each orbital
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.
8 electrons
2
2 electrons
There can only be 2 electrons in each single orbital, and they will be on opposite sides of the electron cloud (orbital).
There are 5 d orbitals which hold 2 electrons each. Thus, 10 electrons are needed to completely fill them.
2
any time there are as many electrons and protons and they fill each orbital optimally.
6 electrons in total, 2 in each orbital
17
6 electrons in total, 2 in each orbital
There are no unpaired electrons in calcium, all 20 electrons are in pairs, i.e. each pair is configured in one orbital: 2x in 1s orbital 2x in 2s orbital 2x in each of the three 2p orbitals 2x in 3s orbital 2x in each of the three 3p orbitals and 2x in 4s orbital (these two are the valence electrons)
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.