the answer is 3
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It is believed to be 6.
Arsenic has three electrons occupying the three 4p orbitals in its valence shell. Hund's first rule tells us that they will each occupy separate orbitals before they start to pair up. So there are three half-filled orbitals in an arsenic atom.
All p sublevels contain three orbitals, including the 4p sublevel.
There are 36 types of orbitals in the sixth shell.
zero - after the 4s orbitals are filled at Calcium, the 3d orbitals start to fill - not until Gallium do the 4p orbitals start to fill.
After the 3d sublevel is filled, additional electrons will occupy the 4p orbitals, for a total of 6 electrons in the 4p sublevel.
Shells: 3 Orbitals: 9
* Ground state electron configuration:[Ar].3d10.4s2.4p6 so...4s and 4p
1s22s22p6
4
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